MCGRAW: CHEMISTRY THE MOLECULAR NATURE
MCGRAW: CHEMISTRY THE MOLECULAR NATURE
8th Edition
ISBN: 9781264330430
Author: VALUE EDITION
Publisher: MCG
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Chapter 8, Problem 8.22P

(a)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the outermost electron in Li atom is to be determined.

Concept introduction:

The electrons in the outermost occupied shell that determine the chemical properties of the elements are called the outermost electrons.

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

MCGRAW: CHEMISTRY THE MOLECULAR NATURE, Chapter 8, Problem 8.22P , additional homework tip  1

3. The magnetic quantum number and it is represented by ml. It tells about the orbitals present in the subshell. The value of ml ranges from l to l including 0.

4. The spin quantum number and it is represented by ms. It tells about the spin of the electron and its value can either be +12 or 12.

(a)

Expert Solution
Check Mark

Answer to Problem 8.22P

The quantum numbers for the outermost electron in Li atom are n=2, l=0, ml=0 and ms=+12 or ms=12.

Explanation of Solution

The atomic number of lithium is 3 and its electronic configuration is 1s22s1

Its outermost electron enters in the 2s orbital so the value of its principal quantum number (n) is 2. The value for azimuthal quantum number (l) for the s orbital is 0.

The value of the magnetic quantum number (ml) for a given value of l extends from l to +l. Therefore, the value of the magnetic quantum number (ml) for l=0 is 0.

The possible value of the spin quantum number (ms) for the 2s electron is +12,12 but by convention its value is taken as positive.

Conclusion

The quantum numbers for the outermost electron in Li atom are n=2, l=0, ml=0 and ms=+12 or ms=12.

(b)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the electron gained when an Br ion becomes an Br ion is to be determined.

Concept introduction:

The electrons in the outermost occupied shell that determine the chemical properties of the elements are called the outermost electrons.

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

MCGRAW: CHEMISTRY THE MOLECULAR NATURE, Chapter 8, Problem 8.22P , additional homework tip  2

3. The magnetic quantum number and it is represented by ml. It tells about the orbitals present in the subshell. The value of ml ranges from l to l including 0.

4. The spin quantum number and it is represented by ms. It tells about the spin of the electron and its value can either be +12 or 12.

(b)

Expert Solution
Check Mark

Answer to Problem 8.22P

The quantum numbers for the electron gained when an Br ion becomes an Br ion are n=4, l=1, ml=1,0,+1 and ms=+12,12.

Explanation of Solution

The atomic number of bromine is 35 so its electronic configuration is [Ar]3d104s24p5. It gains one electron to become Br whose electronic configuration is [Ar]3d104s24p6. The ion formation occurs as:

Br([Ar]3d104s24p5)+eBr([Ar]3d104s24p6)

Its outermost electron enters in the 4p orbital so the value of its principal quantum number (n) is 4. The value of azimuthal quantum number (l) for the p orbital is 1.

The value of the magnetic quantum number (ml) for a given value of l extends from l to +l. Therefore the possible value of magnetic quantum number (ml) for l=1 are +1, 0, or 1.

The possible value of the spin quantum number (ms) for the 4p electron is +12,12 but by convention its value is taken as negative.

Conclusion

The quantum numbers for the electron gained when an Br ion becomes an Br ion are n=4, l=1, ml=1,0,+1 and ms=+12,12.

(c)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the electron lost when a Cs atom ionizes is to be determined.

Concept introduction:

The electrons in the outermost occupied shell that determine the chemical properties of the elements are called the outermost electrons.

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

MCGRAW: CHEMISTRY THE MOLECULAR NATURE, Chapter 8, Problem 8.22P , additional homework tip  3

3. The magnetic quantum number and it is represented by ml. It tells about the orbitals present in the subshell. The value of ml ranges from l to l including 0.

4. The spin quantum number and it is represented by ms. It tells about the spin of the electron and its value can either be +12 or 12.

(c)

Expert Solution
Check Mark

Answer to Problem 8.22P

The quantum numbers for the electron lost when gained when a Cs atom ionizes are.

n=6, l=0, ml=0 and ms=+12,12.

Explanation of Solution

The atomic number of cesium is 55 so its electronic configuration is [Xe]6s1. It loses one electron to become Cs+ whose electronic configuration is that of xenon.

The ion formation occurs as:

Cs([Xe]6s1)Cs+([Xe])+e

The electron is lost from the 6s orbital so the value of its principal quantum number (n) is 6. The value of azimuthal quantum number (l) for the s orbital is 0. The value of the magnetic quantum number (ml) for the 6s electron is 0. The possible values of the spin quantum number (ms) for the 6s electron are +12,12 but by convention its value is taken as positive.

Conclusion

The quantum numbers for the electron lost when gained when a Cs atom ionizes are.

n=6, l=0, ml=0 and ms=+12,12.

(d)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the highest energy electron in the ground state of B atom is to be determined.

Concept introduction:

The electrons in the outermost occupied shell that determine the chemical properties of the elements are called the outermost electrons.

The quantum numbers provide complete information about the electron. There are four quantum numbers as follows:

1. The principal quantum number and it is represented by n. It tells about the shell to which the electron belongs.

2. The azimuthal quantum number and it is represented by l. It tells about the subshell of the electrons.

MCGRAW: CHEMISTRY THE MOLECULAR NATURE, Chapter 8, Problem 8.22P , additional homework tip  4

3. The magnetic quantum number and it is represented by ml. It tells about the orbitals present in the subshell. The value of ml ranges from l to l including 0.

4. The spin quantum number and it is represented by ms. It tells about the spin of the electron and its value can either be +12 or 12.

(d)

Expert Solution
Check Mark

Answer to Problem 8.22P

The quantum numbers for the highest energy electron in the ground state of B atom are n=2, l=1, ml=1,0,+1 and ms=+12,12.

Explanation of Solution

The atomic number of boron is 5 so its electronic configuration is [He]2s22p1. Its highest energy electron lies in 2p orbital.

The electron is present in the 2p orbital so the value of its principal quantum number (n) is 2. The value of azimuthal quantum number (l) for the p orbital is 1.

The value of the magnetic quantum number (ml) for a given value of l extends from l to +l. Therefore the possible value of magnetic quantum number (ml) for l=1 are +1, 0, or 1.

The possible values of the spin quantum number (ms) for the 2p electron is +12,12 but by convention its value is taken as positive.

Conclusion

The quantum numbers for the highest energy electron in the ground state of B atom are n=2, l=1, ml=1,0,+1 and ms=+12,12.

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Chapter 8 Solutions

MCGRAW: CHEMISTRY THE MOLECULAR NATURE

Ch. 8.4 - Prob. 8.6AFPCh. 8.4 - Prob. 8.6BFPCh. 8.4 - Prob. 8.7AFPCh. 8.4 - Prob. 8.7BFPCh. 8.4 - Prob. 8.8AFPCh. 8.4 - Prob. 8.8BFPCh. 8 - Prob. 8.1PCh. 8 - Prob. 8.2PCh. 8 - Prob. 8.3PCh. 8 - To test Döbereiner’s idea (Problem 8.3),...Ch. 8 - Summarize the rules for the allowable values of...Ch. 8 - Prob. 8.6PCh. 8 - State the exclusion principle. What does it imply...Ch. 8 - What is the key distinction between sublevel...Ch. 8 - Prob. 8.9PCh. 8 - Prob. 8.10PCh. 8 - Prob. 8.11PCh. 8 - How many electrons in an atom can have each of the...Ch. 8 - Prob. 8.13PCh. 8 - How many electrons in an atom can have each of the...Ch. 8 - Prob. 8.15PCh. 8 - State Hund’s rule in your own words, and show its...Ch. 8 - Prob. 8.17PCh. 8 - For main-group elements, are outer electron...Ch. 8 - Prob. 8.19PCh. 8 - Prob. 8.20PCh. 8 - Prob. 8.21PCh. 8 - Prob. 8.22PCh. 8 - Write the full ground-state electron configuration...Ch. 8 - Prob. 8.24PCh. 8 - Prob. 8.25PCh. 8 - Prob. 8.26PCh. 8 - Prob. 8.27PCh. 8 - Draw a partial (valence-level) orbital diagram,...Ch. 8 - Prob. 8.29PCh. 8 - Draw a partial (valence-level) orbital diagram,...Ch. 8 - Draw the partial (valence-level) orbital diagram,...Ch. 8 - Prob. 8.32PCh. 8 - Prob. 8.33PCh. 8 - Prob. 8.34PCh. 8 - Prob. 8.35PCh. 8 - Prob. 8.36PCh. 8 - How many inner, outer, and valence electrons are...Ch. 8 - How many inner, outer, and valence electrons are...Ch. 8 - Prob. 8.39PCh. 8 - Prob. 8.40PCh. 8 - Prob. 8.41PCh. 8 - Prob. 8.42PCh. 8 - Prob. 8.43PCh. 8 - Prob. 8.44PCh. 8 - If the exact outer limit of an isolated atom...Ch. 8 - Given the following partial (valence-level)...Ch. 8 - In what region of the periodic table will you find...Ch. 8 - Why do successive IEs of a given element always...Ch. 8 - Prob. 8.49PCh. 8 - Prob. 8.50PCh. 8 - Prob. 8.51PCh. 8 - Prob. 8.52PCh. 8 - Prob. 8.53PCh. 8 - Prob. 8.54PCh. 8 - Prob. 8.55PCh. 8 - Prob. 8.56PCh. 8 - Prob. 8.57PCh. 8 - Prob. 8.58PCh. 8 - Prob. 8.59PCh. 8 - Prob. 8.60PCh. 8 - Prob. 8.61PCh. 8 - Prob. 8.62PCh. 8 - Prob. 8.63PCh. 8 - Prob. 8.64PCh. 8 - Prob. 8.65PCh. 8 - What is a pseudo-noble gas configuration? Give an...Ch. 8 - How are measurements of paramagnetism used to...Ch. 8 - Prob. 8.68PCh. 8 - Prob. 8.69PCh. 8 - Prob. 8.70PCh. 8 - Prob. 8.71PCh. 8 - Prob. 8.72PCh. 8 - Prob. 8.73PCh. 8 - Prob. 8.74PCh. 8 - Prob. 8.75PCh. 8 - Prob. 8.76PCh. 8 - Prob. 8.77PCh. 8 - Prob. 8.78PCh. 8 - Prob. 8.79PCh. 8 - Prob. 8.80PCh. 8 - Which of these atoms are paramagnetic in their...Ch. 8 - Prob. 8.82PCh. 8 - Prob. 8.83PCh. 8 - Write the condensed ground-state electron...Ch. 8 - Prob. 8.85PCh. 8 - Prob. 8.86PCh. 8 - Rank the ions in each set in order of increasing...Ch. 8 - Prob. 8.88PCh. 8 - Prob. 8.89PCh. 8 - Prob. 8.90PCh. 8 - Prob. 8.91PCh. 8 - A fundamental relationship of electrostatics...Ch. 8 - Prob. 8.93PCh. 8 - Prob. 8.94PCh. 8 - Prob. 8.95PCh. 8 - Prob. 8.96PCh. 8 - Prob. 8.97PCh. 8 - Prob. 8.98PCh. 8 - Use Figure 8.16, to find: (a) the longest...Ch. 8 - Prob. 8.100PCh. 8 - Prob. 8.101PCh. 8 - Prob. 8.102P
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