The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals. Concept Introduction: The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is 1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy. Figure 1 The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy. Principal Quantum Number (n) The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell ( level ). The total number of orbitals for a given n value is n 2 . As the value of ‘n’ increases, the energy of the electron also increases. To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen. Find the value of ‘n’

Question

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Answer 1

Question

Chapter 7, Problem 7.67QP

(a)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen.

Find the value of ‘n’

(b)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 2p, 3p orbitals of hydrogen

Find the value of ‘n’

(c)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3d_xy, 3d_yz orbitals of hydrogen

Find the value of ‘n’

(d)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3s, 3d orbitals of hydrogen

Find the value of ‘n’

(e)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 4f, 5s orbitals of hydrogen

Find the value of ‘n’

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Г C-RSA CHROMATOPAC CH=1 DATA 1: @CHRM1.C00 ATTEN=10 SPEED= 10.0 0.0 b.092 0.797 1.088 1.813 C-RSA CHROMATOPAC CH=1 Report No. =13 ** CALCULATION REPORT ** DATA=1: @CHRM1.000 11/03/05 08:09:52 CH PKNO TIME 1 2 0.797 3 1.088 4 1.813 AREA 1508566 4625442 2180060 HEIGHT 207739 701206 V 287554 V MK IDNO CONC NAME 18.1447 55.6339 26.2213 TOTAL 8314067 1196500 100 C-R8A CHROMATOPAC CH=1 DATA 1: @CHRM1.C00 ATTEN=10 SPEED= 10.0 0. 0 087 337. 0.841 1.150 C-R8A CHROMATOPAC CH=1 Report No. =14 DATA=1: @CHRM1.000 11/03/05 08:12:40 ** CALCULATION REPORT ** CH PKNO TIME AREA 1 3 0.841 1099933 41.15 4039778 HEIGHT MK IDNO 170372 649997¯¯¯ CONC NAME 21.4007 78.5993 TOTAL 5139711 820369 100 3 C-R8A CHROMATOPAC CH=1 DATA 1: @CHRM1.C00 ATTEN=10 SPEED= 10.0 0.100 0:652 5.856 3 1.165 C-RSA CHROMATOPAC CH-1 Report No. =15 DATA=1: @CHRM1.000 11/03/05 08:15:26 ** CALCULATION REPORT ** CH PKNO TIME AREA HEIGHT MK IDNO CONC NAME 1 3 3 0.856 4 1.165 TOTAL 1253386 4838738 175481 708024 V 20.5739 79.4261 6092124…

Draw the product of the reaction shown below. Ignore small byproducts that would evaporate please.

Relative Abundance 20- Problems 501 (b) The infrared spectrum has a medium-intensity peak at about 1650 cm. There is also a C-H out-of-plane bending peak near 880 cm. 100- 80- 56 41 69 M(84) LL 15 20 25 30 35 55 60 65 70 75 80 85 90 m/z

Answer 2

Question

Chapter 7, Problem 7.67QP

(a)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen.

Find the value of ‘n’

(b)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 2p, 3p orbitals of hydrogen

Find the value of ‘n’

(c)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3d_xy, 3d_yz orbitals of hydrogen

Find the value of ‘n’

(d)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3s, 3d orbitals of hydrogen

Find the value of ‘n’

(e)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 4f, 5s orbitals of hydrogen

Find the value of ‘n’

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 7, Problem 7.67QP

(a)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen.

Find the value of ‘n’

(b)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 2p, 3p orbitals of hydrogen

Find the value of ‘n’

(c)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3d_xy, 3d_yz orbitals of hydrogen

Find the value of ‘n’

(d)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3s, 3d orbitals of hydrogen

Find the value of ‘n’

(e)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 4f, 5s orbitals of hydrogen

Find the value of ‘n’

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 7, Problem 7.67QP

(a)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen.

Find the value of ‘n’

(b)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 2p, 3p orbitals of hydrogen

Find the value of ‘n’

(c)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3d_xy, 3d_yz orbitals of hydrogen

Find the value of ‘n’

(d)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3s, 3d orbitals of hydrogen

Find the value of ‘n’

(e)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 4f, 5s orbitals of hydrogen

Find the value of ‘n’

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Answer 5

Chapter 7, Problem 7.67QP

(a)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen.

Find the value of ‘n’

(b)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 2p, 3p orbitals of hydrogen

Find the value of ‘n’

(c)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3d_xy, 3d_yz orbitals of hydrogen

Find the value of ‘n’

(d)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3s, 3d orbitals of hydrogen

Find the value of ‘n’

(e)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 4f, 5s orbitals of hydrogen

Find the value of ‘n’

Answer 6

Chapter 7, Problem 7.67QP

(a)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen.

Find the value of ‘n’

Answer 7

Chapter 7, Problem 7.67QP

(a)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 1s, 2s orbitals of hydrogen.

Find the value of ‘n’

Answer 8

(b)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 2p, 3p orbitals of hydrogen

Find the value of ‘n’

Answer 9

(b)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 2p, 3p orbitals of hydrogen

Find the value of ‘n’

Answer 10

(c)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3d_xy, 3d_yz orbitals of hydrogen

Find the value of ‘n’

Answer 11

(c)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3d_xy, 3d_yz orbitals of hydrogen

Find the value of ‘n’

Answer 12

(d)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3s, 3d orbitals of hydrogen

Find the value of ‘n’

Answer 13

(d)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 3s, 3d orbitals of hydrogen

Find the value of ‘n’

Answer 14

(e)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 4f, 5s orbitals of hydrogen

Find the value of ‘n’

Answer 15

(e)

Interpretation Introduction

Interpretation:

The orbital which is higher in energy should be identified in the given pairs of hydrogen orbitals.

Concept Introduction:

The energies of orbitals in the hydrogen atom depend on the value of the principal quantum number (n). When n increases, energy also increases. For this reason, orbitals in the same shell have the same energy in spite of their subshell. The increasing order of energy of hydrogen orbitals is

1s < 2s = 2p < 3s = 3p = 3d < 4s = 4p = 4d = 4f

In the case of one 2s and three 2p orbitals in the second shell, they have the same energy. In the third shell, all nine orbitals (one 3s, three 3p and five 3d) have the same energy. All sixteen orbitals (one 4s, three 4p, five 4d and seven 4f) in the fourth shell have the same energy.

Figure 1

The energy levels of the different orbitals in hydrogen atom are easily explained by considering the given diagram. Here, each box represents one orbital. Orbitals with the same principal quantum number (n) have the same energy.

Principal Quantum Number (n)

The principal quantum number (n) assigns the size of the orbital and specifies the energy of an electron. If the value of n is larger, then the average distance of an electron in the orbital from the nucleus will be greater. Therefore the size of the orbital is large. The principal quantum numbers have the integral values of 1, 2, 3 and so forth and it corresponds to the quantum number in Bohr’s model of the hydrogen atom. If all orbitals have the same value of ‘n’, they are said to be in the same shell (level). The total number of orbitals for a given n value is n². As the value of ‘n’ increases, the energy of the electron also increases.

To find: Identify the orbital which is higher in energy in the given pair 4f, 5s orbitals of hydrogen

Find the value of ‘n’

Answer 16

Expert Solution & Answer

Answer 17

Expert Solution & Answer

Answer 18

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Answer 19

Ch. 7.1 - Review of Concepts What of the waves shown here...Ch. 7.1 - Prob. 1PE Ch. 7.1 - Prob. 2RC Ch. 7.2 - Prob. 1PE Ch. 7.2 - Prob. 2PE Ch. 7.2 - Prob. 1RC Ch. 7.3 - Prob. 1PE Ch. 7.3 - Prob. 1RC Ch. 7.4 - Prob. 1PE Ch. 7.4 - Prob. 1RC

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