The number of orbital present in one set g-orbital should be determined. Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows: 1 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 Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

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Answer 1

Question

Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

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Answer 2

Question

Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

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Answer 3

Question

Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

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Answer 4

Question

Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

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Answer 5

Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

Answer 6

Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

Answer 7

Chapter 2, Problem 2.47P

(a)

Interpretation Introduction

Interpretation: The number of orbital present in one set g-orbital should be determined.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

Answer 8

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

Answer 9

(b)

Interpretation Introduction

Interpretation: The angular nodes of g-orbital should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

Answer 10

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

Answer 11

(c)

Interpretation Introduction

Interpretation: The relation between principal quantum number and radial nodes should be explained.

Concept introduction: The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are termed as core electrons. Electrons are filled within orbitals by following three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states, electrons are filled in the orbitals from lower to higher energy level as follows:

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s

Hund’s rule states, initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states, spin of two different electrons in one orbital is always different.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 2.1 - Determine the energy of the transition from nh=3...Ch. 2.2 - Describe the angular nodal surfaces for a dz2...Ch. 2.2 - Prob. 2.3E Ch. 2.2 - A third possible state for the p4 configuration...Ch. 2.2 - A nitrogen atom, with three 2p electrons, could...Ch. 2.2 - Calculate the effective nuclear charge on a 5s,...Ch. 2.2 - Calculate the effective nuclear charge on a 7s,...Ch. 2.3 - Explain why all three graphs in Figure 2.14 have...Ch. 2 - Determine the de Brogue wavelength of a. an...Ch. 2 - Using the equation E=RH(1221nh2) determine the...

Solution Summary: The author explains that the number of orbital present in one set g-orbital should be determined.

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