Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781259631757
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 8, Problem 8.21P

(a)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the outermost electron in Rb 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.

Chemistry: The Molecular Nature of Matter and Change, Chapter 8, Problem 8.21P , 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 8.21P

The possible quantum numbers for the outermost electron in Rb atom are n=5, l=0, ml=0 and ms=+12 or ms=12.

Explanation of Solution

The atomic number of rubidium is 37 and its electronic configuration is [Kr]5s1.

Its outermost electron enters in the 5s orbital so the value of its principal quantum number (n) is 5. The value for azimuthal quantum number (l) for the s orbital is 0. The value of the magnetic quantum number (ml) for the 5s electron is 0. The value of the spin quantum number (ms) for the 5s electron can be +12 or 12.

Conclusion

The possible quantum numbers for the outermost electron in Rb atom are n=5, 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 S ion becomes an S2 ion is to be determined.

Concept introduction:

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.

Chemistry: The Molecular Nature of Matter and Change, Chapter 8, Problem 8.21P , 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 8.21P

The possible quantum numbers for the electron gained when an S ion becomes an S2 ion are n=3, l=1, ml=1 , 0, or +1, and ms=+12 or ms=12.

Explanation of Solution

The atomic number of sulfur is 16 so its electronic configuration is [Ne]3s23p4. It gains one electron to become S whose electronic configuration is [Ne]3s23p5. It further gains one more electron to become S2 whose electronic configuration is [Ne]3s23p6.

The ion formation occurs as:

S([Ne]3s23p4)+eS([Ne]3s23p5)S([Ne]3s23p5)+eS2([Ne]3s23p6)

Its outermost electron enters in the 3p orbital so the value of its principal quantum number (n) is 3. 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 electron added to the 3p orbital is the second electron thus by convention its ms value should be 12 but the possible value of the spin quantum number (ms) for the 3p electron can be +12 or 12.

Conclusion

The possible quantum numbers for the electron gained when an S ion becomes an S2 ion are n=3, l=1, ml=1 , 0, or +1, and ms=+12 or ms=12.

(c)

Interpretation Introduction

Interpretation:

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

Concept introduction:

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.

Chemistry: The Molecular Nature of Matter and Change, Chapter 8, Problem 8.21P , 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 8.21P

The possible quantum numbers for the electron lost when gained when an Ag atom ionizes are n=5, l=0, ml=0 and ms=+12 or ms=12.

Explanation of Solution

The atomic number of silver is 47 so its electronic configuration is [Kr]5s14d10. Electron is lost always from the highest energy level. It loses one electron from 5s orbital to become Ag+ whose electronic configuration is [Kr]4d10.

The ion formation occurs as:

Ag([Kr]5s14d10)eAg+([Kr]4d10)

The electron is lost from the 5s orbital so the value of its principal quantum number (n) is 5. The value of azimuthal quantum number (l) for the s orbital is 0. The value of the magnetic quantum number (ml) for the 5s electron is 0. The value of the spin quantum number (ms) for the 5s electron can be +12 or 12.

Conclusion

The possible quantum numbers for the electron lost when gained when an Ag atom ionizes are n=5, l=0, ml=0 and ms=+12 or ms=12.

(d)

Interpretation Introduction

Interpretation:

The full set of possible quantum numbers for the electron gained when an F ion is formed from F atom is to be determined.

Concept introduction:

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.

Chemistry: The Molecular Nature of Matter and Change, Chapter 8, Problem 8.21P , 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 8.21P

The quantum numbers for the electron gained when an F ion is formed from F atom are n=2, l=1, ml=1 , 0, or +1 and ms=+12 or ms=12.

Explanation of Solution

The atomic number of fluorine is 9 so its electronic configuration is 1s22s22p5. It gains one electron to form F ion whose electronic configuration is 1s22s22p6.

The ion formation occurs as:

F(1s22s22p5)+eF(1s22s22p6)

The electron is added to 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 value of the spin quantum number (ms) for the 2p electron can be +12 or 12.

Conclusion

The quantum numbers for the electron gained when an F ion is formed from F atom are n=2, l=1, ml=1 , 0, or +1 and ms=+12 or ms=12.

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Chapter 8 Solutions

Chemistry: The Molecular Nature of Matter and Change

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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