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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1. Answer the questions about the following reaction: (a) Draw in the arrows that can be used make this reaction occur and draw in the product of substitution in this reaction. Be sure to include any relevant stereochemistry in the product structure. + SK F Br + (b) In which solvent would this reaction proceed the fastest (Circle one) Methanol Acetone (c) Imagine that you are working for a chemical company and it was your job to perform a similar reaction to the one above, with the exception of the S atom in this reaction being replaced by an O atom. During the reaction, you observe the formation of three separate molecules instead of the single molecule obtained above. What is the likeliest other products that are formed? Draw them in the box provided.

3. For the reactions below, draw the arrows corresponding to the transformations and draw in the boxes the reactants or products as indicated. Note: Part A should have arrows drawn going from the reactants to the middle structure and the arrows on the middle structure that would yield the final structure. For part B, you will need to draw in the reactant before being able to draw the arrows corresponding to product formation. A. B. Rearrangement ΘΗ

2. Draw the arrows required to make the following reactions occur. Please ensure your arrows point from exactly where you want to exactly where you want. If it is unclear from where arrows start or where they end, only partial credit will be given. Note: You may need to draw in lone pairs before drawing the arrows. A. B. H-Br 人 C Θ CI H Cl Θ + Br O

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).

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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).