The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified. Figure 1 Concept Introduction: Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals. Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s , p , d a n d f . The lowest energy orbital is l s . The energy order of the orbital for the first three periods is as follows, l s , 2 s , 2 p , 3 s , a n d 3 p . The orbital which is closer to the nucleus has lower energy; therefore the 2 s is lower in energy than 3 s . Accordingly 2 s is lower in energy than 2 p a n d 4 s is lower in energy than 3 d . In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin. The subshell ordering by Aufbau principle is given below, l s , 2 s , 2 p , 3 s , 3 p , 4 s , 3 d , 4 p , 5 s , 4 d , 5 p , 6 s , 4 f , 5 d , 6 p , 7 s , 5 f , 6 d , 7 p , 8 s , ... Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired. If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital. If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

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Answer 1

Question

Chapter 1, Problem 1E.8E

(a)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 1

Concept Introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f.    The lowest energy orbital is ls.

The energy order of the orbital for the first three periods is as follows,

    ls, 2s, 2p, 3s, and 3p.

The orbital which is closer to the nucleus has lower energy; therefore the 2s is lower in energy than 3s.   Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    ls, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired.

If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital.

If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

(b)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

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Experiment 1 Data Table 1: Conservation of Mass - Initial Mass Data Table 1 Data Table 2 Data Table 3 Data Table 4 Panel 1 Photo 1 Data Table 5 Reaction Mass of test tube and 5.0% HC₂H₂O2 (g) # (A) (B) Mass of NaHCO, (g) Mass of balloon and NaHCO, (g) (C) 0.10 1 0829 14.38g 0.20 2 0.929 14.29g 0.35 1.00g 3 14.25g 0.50 1.14g 14.29 Experiment 1 Data Table 2: Moles of HC2H3O2 Reaction Volume of Mass of Moles of HC₂H₂O₂ 5.0% Vinegar (g) (ML) 5.0 0.25 0042 mol 2 5.0 0.25 0042 mol 3 5.0 0.25 0042 mol 5.0 0.25 0042 mol Experiment 1 Data Table 3: Moles of NaHCO3 Reaction Mass of NaHCO (g) 10g 20g 35g 50g Experiment 1 Data Table 4: Theoretical Yield of CO₂ Reaction # 1 2 3 Experiment 1 Total mass before reaction (g) (D=A+C) 15.29 15.21g 15.25g 15.349 Exercise 1 Data Table 1 Data Table 2 Data Table 3 Data Table 4 Panel 1 Photo 1 Data Table 5 Exercise 1- Data Table 1 Data Table 2 DataTable 3 Data Table 4 Panel 1 Photo 1 Data Table 5 Exercise 1- Moles of NaHCO 0012 mol 0025 mol 0044 mol 0062 mol…

The chemical reaction you investigated is a two-step reaction. What type of reaction occurs in each step? How did you determine your answer?

What is the relationship between the limiting reactant and theoretical yield of CO2?

Answer 2

Question

Chapter 1, Problem 1E.8E

(a)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 1

Concept Introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f.    The lowest energy orbital is ls.

The energy order of the orbital for the first three periods is as follows,

    ls, 2s, 2p, 3s, and 3p.

The orbital which is closer to the nucleus has lower energy; therefore the 2s is lower in energy than 3s.   Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    ls, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired.

If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital.

If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

(b)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

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Answer 3

Question

Chapter 1, Problem 1E.8E

(a)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 1

Concept Introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f.    The lowest energy orbital is ls.

The energy order of the orbital for the first three periods is as follows,

    ls, 2s, 2p, 3s, and 3p.

The orbital which is closer to the nucleus has lower energy; therefore the 2s is lower in energy than 3s.   Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    ls, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired.

If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital.

If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

(b)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

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Answer 4

Question

Chapter 1, Problem 1E.8E

(a)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 1

Concept Introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f.    The lowest energy orbital is ls.

The energy order of the orbital for the first three periods is as follows,

    ls, 2s, 2p, 3s, and 3p.

The orbital which is closer to the nucleus has lower energy; therefore the 2s is lower in energy than 3s.   Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    ls, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired.

If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital.

If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

(b)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

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Answer 5

Chapter 1, Problem 1E.8E

(a)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 1

Concept Introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f.    The lowest energy orbital is ls.

The energy order of the orbital for the first three periods is as follows,

    ls, 2s, 2p, 3s, and 3p.

The orbital which is closer to the nucleus has lower energy; therefore the 2s is lower in energy than 3s.   Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    ls, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired.

If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital.

If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

(b)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

(d)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

Answer 6

Chapter 1, Problem 1E.8E

(a)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 1

Concept Introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f.    The lowest energy orbital is ls.

The energy order of the orbital for the first three periods is as follows,

    ls, 2s, 2p, 3s, and 3p.

The orbital which is closer to the nucleus has lower energy; therefore the 2s is lower in energy than 3s.   Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    ls, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired.

If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital.

If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

Answer 7

Chapter 1, Problem 1E.8E

(a)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 1

Concept Introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is s, p, d and f.    The lowest energy orbital is ls.

The energy order of the orbital for the first three periods is as follows,

    ls, 2s, 2p, 3s, and 3p.

The orbital which is closer to the nucleus has lower energy; therefore the 2s is lower in energy than 3s.   Accordingly 2s is lower in energy than 2p and 4s is lower in energy than 3d.

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    ls, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s, ...

Electrons are filled in each orbital one after another in the increasing order of energy. While filling the orbitals, more than two electrons can be placed in an orbital. And also, the spin of the two electron in the same orbital must be paired.

If there are more than one orbitals in a subshell are available for filling the electron, then electrons with parallel spin goes to different subshell rather than pairing two electrons in one orbital.

If an atom having electrons in energy states higher than predicted by the above rules then it is said to be in an excited state.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

Answer 12

(d)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

Answer 13

(d)

Interpretation Introduction

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 1 - Prob. 1A.1AST Ch. 1 - Prob. 1A.1BST Ch. 1 - Prob. 1A.2AST Ch. 1 - Prob. 1A.2BST Ch. 1 - Prob. 1A.1E Ch. 1 - Prob. 1A.3E Ch. 1 - Prob. 1A.4E Ch. 1 - Prob. 1A.5E Ch. 1 - Prob. 1A.6E Ch. 1 - Prob. 1A.7E

Videos

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).

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Chapter 1 Solutions

Videos

Interpretation: The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified. Figure 2 Concept Introduction: Refer to part (a).

Interpretation: The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified. Figure 3 Concept Introduction: Refer to part (a).

Interpretation: The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified. Figure 4 Concept Introduction: Refer to part (a).

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Chapter 1 Solutions

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 2

Concept Introduction:

Refer to part (a).

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 3

Concept Introduction:

Refer to part (a).

Interpretation:

The element having the given configuration has to be identified. Also whether the configuration represent ground state or not has to be identified.

Figure 4

Concept Introduction:

Refer to part (a).