The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn. Concept Introduction: The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is n s 1 − 2 , that of p block elements is n s 2 n p 1 − 6 , that of d block elements is ( n − 1 ) d 1 − 10 n s 0 − 2 and that of f block elements is ( n − 2 ) f 1 − 14 ( n − 1 ) d 0 − 10 n s 2 . Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

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Answer 1

Question

Chapter 7, Problem 7.74QE

(a)

Interpretation Introduction

Interpretation:

The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

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MISSED THIS? Read Section 19.9 (Pages 878-881); Watch IWE 19.10 Consider the following reaction: CH3OH(g) CO(g) + 2H2(g) (Note that AG,CH3OH(g) = -162.3 kJ/mol and AG,co(g)=-137.2 kJ/mol.) Part A Calculate AG for this reaction at 25 °C under the following conditions: PCH₂OH Pco PH2 0.815 atm = 0.140 atm 0.170 atm Express your answer in kilojoules to three significant figures. Ο ΑΣΦ AG = -150 Submit Previous Answers Request Answer □? kJ × Incorrect; Try Again; 2 attempts remaining Calculate the free energy change under nonstandard conditions (AGrxn) by using the following relationship: AGrxn = AGrxn + RTInQ, AGxn+RTInQ, where AGxn is the standard free energy change, R is the ideal gas constant, T is the temperature in kelvins, a is the reaction quotient. Provide Feedback Next >

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Answer 2

Question

Chapter 7, Problem 7.74QE

(a)

Interpretation Introduction

Interpretation:

The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 3

Question

Chapter 7, Problem 7.74QE

(a)

Interpretation Introduction

Interpretation:

The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 4

Question

Chapter 7, Problem 7.74QE

(a)

Interpretation Introduction

Interpretation:

The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

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Answer 5

Chapter 7, Problem 7.74QE

(a)

Interpretation Introduction

Interpretation:

The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

(b)

Interpretation Introduction

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

Answer 6

Chapter 7, Problem 7.74QE

(a)

Interpretation Introduction

Interpretation:

The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

Answer 7

Chapter 7, Problem 7.74QE

(a)

Interpretation Introduction

Interpretation:

The orbital diagrams for elements with atomic number 1, 3, 5, and 9 has to be drawn.

Concept Introduction:

The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. 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 called core electrons. The general outer electronic configuration of s block elements is ns1−2, that of p block elements is ns2np1−6, that of d block elements is (n−1)d1−10ns0−2 and that of f block elements is (n−2)f1−14(n−1)d0−10ns2.

Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that 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 that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 7 - Prob. 7.1QE Ch. 7 - Prob. 7.2QE Ch. 7 - Prob. 7.3QE Ch. 7 - Prob. 7.4QE Ch. 7 - Prob. 7.5QE Ch. 7 - Prob. 7.6QE Ch. 7 - Prob. 7.7QE Ch. 7 - Prob. 7.8QE Ch. 7 - Prob. 7.9QE Ch. 7 - Prob. 7.10QE

Solution Summary: The author defines the electronic configuration as the distribution of electrons in various atomic orbitals of the atom.

Videos

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).

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Chapter 7 Solutions

Solution Summary: The author defines the electronic configuration as the distribution of electrons in various atomic orbitals of the atom.

Videos

Interpretation: The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined. Concept Introduction: Refer to part (a).

Interpretation: The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined. Concept Introduction: Refer to part (a).

Want to see the full answer?

Chapter 7 Solutions

Interpretation:

The electron configuration with completely filled subshells for the element with an atomic number less than 10 has to be determined.

Concept Introduction:

Refer to part (a).

Interpretation:

The orbital diagram for electronic configuration of elements with an atomic number 6 and 8 has to be determined.

Concept Introduction:

Refer to part (a).