CHEM 212:STUDENT SOLUTION MANUAL
CHEM 212:STUDENT SOLUTION MANUAL
8th Edition
ISBN: 9781260304473
Author: SILBERBERG
Publisher: MCGRAW-HILL CUSTOM PUBLISHING
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Chapter 10, Problem 10.63P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of PF5 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(a)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of PF5 is trigonal bipyramidal.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  1

Explanation of Solution

The total number of valence electrons of PF5 is calculated as,

  Total valence electrons(TVE)=[[(Total number of P atom)(Valence electrons of P)]+[(Total number of F atom)(Valence electrons of F)]]        (2)

Substitute 1 for the total number of P the atom, 5 for valence electrons of P, 7 for the total valence electrons of F, and 5 for the value of the total number of F atom in equation (1).

  Total valence electrons(TVE)=[(1)(5)+(5)(7)]=40.

PF5 has 40 valence electrons. 10 electrons are used to form 5 single bonds with the five fluorine atoms and the remaining 30 electrons are placed on the five fluorine atoms as 3 lone pairs on each.

Thus, the Lewis structure of PF5 is drawn as follows,

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  2

According to the Lewis structure of PF5, there are five electron groups around the central atom P with no lone pair. This gives a trigonal bipyramidal electron-group arrangement (AX5) and gives trigonal bipyramidal molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in PF5 is AX5 and has a trigonal bipyramidal shape.

(b)

Interpretation Introduction

Interpretation:

The molecular shape of CCl4 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(b)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of CCl4 is tetrahedral.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  3

Explanation of Solution

The total number of valence electrons of CCl4 is calculated as,

  Total valence electrons(TVE)=[[(Total number of C atom)(Valence electrons of C)]+[(Total number of Cl atom)(Valence electrons of Cl)]]        (2)

Substitute 1 for the total number of C the atom, 4 for valence electrons of C, 7 for the total valence electrons of Cl, 4 for the total number of Cl the atom in equation (2).

  Total valence electrons(TVE)=[(1)(4)+(4)(7)]=32.

The Lewis structure of CCl4 is,

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  4

According to the Lewis structure of CCl4, four electron groups are present around the central atom C with no lone pair. This gives a tetrahedral electron-group arrangement (AX4) and gives tetrahedral molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in CCl4 is AX4 and has a tetrahedral shape.

(c)

Interpretation Introduction

Interpretation:

The molecular shape of H3O+ is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(c)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of H3O+ is trigonal pyramidal.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  5

Explanation of Solution

The total number of valence electrons of H3O+ is calculated as,

  Total valence electrons(TVE)=[[(Total number of O atom)(Valence electrons of O)]+[(Total number of H atom)(Valence electrons of H)](positive charge)]        (3)

Substitute 1 for the total number of O the atom, 6 for valence electrons of O, 1 for the total valence electrons of H, 3 for the total number of H atom, and 1 for the positive charge in equation (3).

  Total valence electrons(TVE)=[(1)(6)+(3)(1)1]=8.

The total number of valence electrons in H3O+ is 8. The Lewis structure of H3O+ is given as,

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  6

According to the Lewis structure of H3O+, four electron groups are present around the central atom C as three bond pair and one lone pair. This gives a tetrahedral electron-group arrangement (AX3E) and gives trigonal pyramidal H3O+ molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in H3O+ is AX3E and has a trigonal pyramidal shape.

(d)

Interpretation Introduction

Interpretation:

The molecular shape of ICl3 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(d)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of ICl3 is T-shaped.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  7

Explanation of Solution

The total number of valence electrons of ICl3 is calculated as,

  Total valence electrons(TVE)=[[(Total number of I atom)(Valence electrons of I)]+[(Total number of Cl atom)(Valence electrons of Cl)]]        (4)

Substitute 1 for the total number of I atom, 7 for valence electrons of I, 7 for the total valence electrons of Cl, and 3 for the total number of Cl atom in equation (4).

  Total valence electrons(TVE)=[(1)(7)+(3)(7)]=28.

With I as central atom, first three bond pairs are placed between each I-Cl bond then the remaining are placed as the lone pairs. Lewis structure of ICl3 is,

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  8

According to the Lewis structure of ICl3, there are 5 electron groups around the central atom I of which three are bond pairs and 2 are lone pairs. This gives it an electron-group arrangement of the type AX3E2, molecular shape assigned would be T-shaped according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in ICl3 is AX3E2 and has a T-shape.

(e)

Interpretation Introduction

Interpretation:

The molecular shape of BeH2 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(e)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of BeH2 is linear.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  9

Explanation of Solution

The total number of valence electrons of BeH2 is calculated as,

  Total valence electrons(TVE)=[[(Total number of  Be atom)(Valence electrons of Be )]+[(Total number of H atom)(Valence electrons of H )]]        (5)

Substitute 1 for the total number of Be atom, 2 for valence electrons of Be, 1 for the total valence electrons of H, and 2 for the total number of H atom in equation (5).

  Total valence electrons(TVE)=[(1)(2)+(2)(1)]=4.

With Be as central atom, first two bond pairs are placed between each Be-H bond then the remaining are placed as the lone pairs. Lewis structure of BeH2 is depicted as,

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  10

According to the Lewis structure of BeH2, there are two electron groups around the central atom Be and no lone pairs around Be. This gives a linear arrangement of the type AX2, thus molecular shape assigned would be linear according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in BeH2 is AX2 and has a linear shape.

(f)

Interpretation Introduction

Interpretation:

The molecular shape of PH2 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(f)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of PH2 is bent.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  11

Explanation of Solution

The total number of valence electrons of PH2 is calculated as,

  Total valence electrons(TVE)=[[(Total number of P atom)(Valence electrons of P)]+[(Total number of H atom)(Valence electrons of H  )]+(negative charge)]        (6)

Substitute 1 for the total number of P atom, 5 for valence electrons of P, 1 for the total valence electrons of H, 2 for the total number of H atom, and  1 for the negative charge in equation (6).

  Total valence electrons(TVE)=[(1)(5)+(2)(1)+1]=8.

The Lewis structure of PH2 is,

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  12

According to the Lewis structure of molecular shape of PH2 would be T-shaped according to VSEPR. There are 4 electron groups around the central atom P of which two are lone pairs and two bond pairs. This gives AX2E2 type arrangement, a bent V-shaped molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in PH2 is AX2E2 and has a bent shape.

(g)

Interpretation Introduction

Interpretation:

The molecular shape of GeBr4 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(g)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of GeBr4 is tetrahedral.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  13

Explanation of Solution

The total number of valence electrons of GeBr4 is calculated as,

  Total valence electrons(TVE)=[[(Total number of Ge atom)(Valence electrons of Ge)]+[(Total number of Br atom)(Valence electrons of Br)]]        (7)

Substitute 1 for the total number of Ge the atom, 4 for valence electrons of Ge, 7 for the total valence electrons of Br, 4 for the total number of Br the atom, in equation (7).

  Total valence electrons(TVE)=[(1)(4)+(4)(7)]=32.

The total number of valence electrons in GeBr4 is 32. The Lewis structure of GeBr4 is,

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  14

According to the Lewis structure of GeBr4, four electron groups are present around the central atom Ge with no lone pair. This gives a tetrahedral electron-group arrangement (AX4) and gives tetrahedral molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in GeBr4 is AX4 and has a tetrahedral shape.

(h)

Interpretation Introduction

Interpretation:

The molecular shape of CH3 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(h)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of CH3 is trigonal pyramidal.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  15

Explanation of Solution

The total number of valence electrons of CH3 is calculated as,

  Total valence electrons(TVE)=[[(Total number of C atom)(Valence electrons of C)]+[(Total number of H atom)(Valence electrons of H)]+(negative charge)]        (8)

Substitute 1 for the total number of C atom, 4 for valence electrons of C, 1 for the total valence electrons of H, 3 for the total number of H atom, and 1 for the negative charge in equation (8).

  Total valence electrons(TVE)=[(1)(4)+(3)(1)+1]=8.

The total number of valence electrons in CH3 is 8. These eight electrons are placed such that three electrons form bonding pair and the last resides on carbon as shown below:

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  16

According to the Lewis structure of CH3, four electron groups are present around the central atom C as three bond pairs and one lone pair. This gives a tetrahedral electron-group arrangement (AX3E) and the electrons will best occupy the position as in a trigonal pyramidal shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in CH3 is AX3E and has a trigonal pyramidal shape.

(i)

Interpretation Introduction

Interpretation:

The molecular shape of BCl3 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(i)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of BCl3 is trigonal planar.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  17

Explanation of Solution

The total number of valence electrons of BCl3 is calculated as,

  Total valence electrons(TVE)=[[(Total number of B atom)(Valence electrons of B)]+[(Total number of Cl atom)(Valence electrons of Cl  )]]        (9)

Substitute 1 for the total number of B atom, 3 for valence electrons of B, 7 for the total valence electrons of Cl, and 3 for the total number of Cl atom in equation (9).

  Total valence electrons(TVE)=[(1)(3)+(3)(7)]=24.

These 24 electrons are placed such that three of these form bonding pairs and the remaining ones reside as lone pairs as shown below:

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  18

According to the Lewis structure of BCl3, there are three electron groups around the central atom B. This gives a trigonal planar arrangement of the type AX3, a trigonal planar molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in BCl3 is AX3 and has a trigonal planar shape.

(j)

Interpretation Introduction

Interpretation:

The molecular shape of BrF4+ is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(j)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of BrF4+ is seesaw.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  19

Explanation of Solution

The total number of valence electrons of BrF4+ is calculated as,

  Total valence electrons(TVE)=[[(Total number of Br atom)(Valence electrons of Br )]+[(Total number of F atom)(Valence electrons of F )](positive charge)]        (10)

Substitute 1 for the total number of Br atom, 7 for valence electrons of Br, 7 for the total valence electrons of F, 4 for the total number of F atom, and 1 for the positive charge in equation (10).

  Total valence electrons(TVE)=[(1)(7)+(4)(7)1]=34.

The Lewis structure for BrF4+ is represented as follows:

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  20

According to the Lewis structure of BrF4+, there are 5 electron groups around the central atom of which one is lone pair and three are bond pairs. This gives an arrangement of type AX4E , and seesaw molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in BrF4+ is AX4E and has a seesaw shape.

(k)

Interpretation Introduction

Interpretation:

The molecular shape of XeO3 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(k)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of XeO3 is trigonal pyramidal.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  21

Explanation of Solution

The total number of valence electrons of XeO3 is calculated as,

  Total valence electrons(TVE)=[[(Total number of Xe atom)(Valence electrons of Xe)]+[(Total number of O atom)(Valence electrons of O)]]        (11)

Substitute 1 for the total number of Xe the atom, 8 for valence electrons of Xe, 6 for the total valence electrons of O, 3 for the total number of O the atom in equation (11).

  Total valence electrons(TVE)=[(1)(8)+(3)(6)]=26.

The total number of valence electrons in XeO3 is 26. The Lewis structure of XeO3 is thus drawn as:

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  22

According to the Lewis structure of XeO3, 4 electron groups are present as three bond pairs and 1 lone pair. This gives a tetrahedral electron-group arrangement (AX3E) and gives trigonal pyramidal molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in XeO3 is AX3E and has a trigonal pyramidal shape.

(l)

Interpretation Introduction

Interpretation:

The molecular shape of TeF4 is to be determined.

Concept introduction:

The steps to draw the Lewis structure of the given molecule are as follows:

Step 1: Choose the least electronegative central metal atom and place the atoms relative to each other.

Step 2: Determine the total number of valence electron.

Step 3: Place a single electron pair between each atom and subtract 2 electrons corresponding to each of these bonds from the total number of valence electrons.

Step 4: Distribute the remaining electrons in pairs around each atom as non bonding electrons such that each atom gets a complete share of eight electrons.

(l)

Expert Solution
Check Mark

Answer to Problem 10.63P

The molecular shape of TeF4 is seesaw.

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  23

Explanation of Solution

The total number of valence electrons of TeF4 is calculated as,

  Total valence electrons(TVE)=[[(Total number of Te atom)(Valence electrons of Te )]+[(Total number of F atom)(Valence electrons of F )]]        (12)

Substitute 1 for the total number of Te atom, 6 for valence electrons of Te, 7 for the total valence electrons of F, and 4 for the total number of F atom in equation (12).

  Total valence electrons(TVE)=[(1)(6)+(4)(7)]=34.

Analogous to GeBr4 Lewis structure for TeF4 may be drawn as follows:

CHEM 212:STUDENT SOLUTION MANUAL, Chapter 10, Problem 10.63P , additional homework tip  24

According to the Lewis structure of TeF4, there are 5 electron groups of which 4 are bond pairs and 1 is lone pair. This gives an arrangement of type AX4E , a seesaw molecular shape according to VSEPR.

Conclusion

The electron-group arrangement around the central atom in TeF4 is AX4E and has a seesaw shape.

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Chapter 10 Solutions

CHEM 212:STUDENT SOLUTION MANUAL

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Publisher:WILEY
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY