7.E: Chemical Bonds (Exercises)

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Exercises (Lewis Electron Dot Diagrams)

Explain why the first two dots in a Lewis electron dot diagram are drawn on the same side of the atomic symbol.
Is it necessary for the first dot around an atomic symbol to go on a particular side of the atomic symbol
What column of the periodic table has Lewis electron dot diagrams with two electrons?
What column of the periodic table has Lewis electron dot diagrams that have six electrons in them?
Draw the Lewis electron dot diagram for each element.
1. strontium
2. silicon
Draw the Lewis electron dot diagram for each element.
1. krypton
2. sulfur
Draw the Lewis electron dot diagram for each element.
1. titanium
2. phosphorus
Draw the Lewis electron dot diagram for each element.
1. bromine
2. gallium
Draw the Lewis electron dot diagram for each ion.
1. Mg²⁺
2. S²⁻
Draw the Lewis electron dot diagram for each ion.
1. In⁺
2. Br⁻
Draw the Lewis electron dot diagram for each ion.
1. Fe²⁺
2. N³⁻
Draw the Lewis electron dot diagram for each ion.
1. H⁺
2. H⁻

Answers

1. The first two electrons in a valence shell are s electrons, which are paired.

3. The second column of the periodic table

5. a.

7. a.

9. a. Mg2+

11. a. Fe2+

Exercises (Electron Transfer - Ionic Bonds)

Comment on the possible formation of the K²⁺ ion. Why is its formation unlikely?
Comment on the possible formation of the Cl²⁻ ion. Why is its formation unlikely?
How many electrons does a Ba atom have to lose to have a complete octet in its valence shell?
How many electrons does a Pb atom have to lose to have a complete octet in its valence shell?
How many electrons does an Se atom have to gain to have a complete octet in its valence shell?
How many electrons does an N atom have to gain to have a complete octet in its valence shell?
With arrows, illustrate the transfer of electrons to form potassium chloride from K atoms and Cl atoms.
With arrows, illustrate the transfer of electrons to form magnesium sulfide from Mg atoms and S atoms.
With arrows, illustrate the transfer of electrons to form scandium fluoride from Sc atoms and F atoms.
With arrows, illustrate the transfer of electrons to form rubidium phosphide from Rb atoms and P atoms.
Which ionic compound has the higher lattice energy—KI or MgO? Why?
Which ionic compound has the higher lattice energy—KI or LiF? Why?

Which ionic compound has the higher lattice energy—BaS or MgO? Why?

Answers

1. The K²⁺ ion is unlikely to form because the K⁺ ion already satisfies the octet rule and is rather stable.

3. two

5. two

11. MgO because the ions have a higher magnitude charge

13. MgO because the ions are smaller

Exercises (Covalent Bonds)

How many electrons will be in the valence shell of H atoms when it makes a covalent bond?
How many electrons will be in the valence shell of non-H atoms when they make covalent bonds?
What is the Lewis electron dot diagram of I₂? Circle the electrons around each atom to verify that each valence shell is filled.
What is the Lewis electron dot diagram of H₂S? Circle the electrons around each atom to verify that each valence shell is filled.
What is the Lewis electron dot diagram of NCl₃? Circle the electrons around each atom to verify that each valence shell is filled.
What is the Lewis electron dot diagram of SiF₄? Circle the electrons around each atom to verify that each valence shell is filled.
Draw the Lewis electron dot diagram for each substance.
1. SF₂
2. BH₄⁻
Draw the Lewis electron dot diagram for each substance.
1. PI₃
2. OH⁻
Draw the Lewis electron dot diagram for each substance.
1. GeH₄
2. ClF
Draw the Lewis electron dot diagram for each substance.
1. AsF₃
2. NH₄⁺
Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed.
1. SiO₂
2. C₂H₄ (assume two central atoms)
Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed.
1. CN⁻
2. C₂Cl₂ (assume two central atoms)
Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed.
1. CS₂
2. NH₂CONH₂ (assume that the N and C atoms are the central atoms)
Draw the Lewis electron dot diagram for each substance. Double or triple bonds may be needed.
1. POCl
2. HCOOH (assume that the C atom and one O atom are the central atoms)

Answers

1. two

7a.

7b.

9a.

9b.

11a.

11b.

13a.

13b.

Exercises (Other Aspects of Covalent Bonds)

Give an example of a nonpolar covalent bond. How do you know it is nonpolar?
Give an example of a polar covalent bond. How do you know it is polar?
How do you know which side of a polar bond has the partial negative charge? Identify the negatively charged side of each polar bond.
1. H–Cl
2. H–S
How do you know which side of a polar bond has the partial positive charge? Identify the positively charged side of each polar bond.
1. H–Cl
2. N-F
Label the bond between the given atoms as nonpolar covalent, slightly polar covalent, definitely polar covalent, or likely ionic.
1. H and C
2. C and F
3. K and F
Label the bond between the given atoms as nonpolar covalent, slightly polar covalent, definitely polar covalent, or likely ionic.
1. S and Cl
2. P and O
3. Cs and O
Which covalent bond is stronger—a C–C bond or a C–H bond?
Which covalent bond is stronger—an O–O double bond or an N–N double bond?
Estimate the enthalpy change for this reaction: N₂ + 3H₂ → 2NH₃.Start by drawing the Lewis electron dot diagrams for each substance.
Estimate the enthalpy change for this reaction. Start by drawing the Lewis electron dot diagrams for each substance: HN=NH + 2H₂ → 2NH₃
Estimate the enthalpy change for this reaction. Start by drawing the Lewis electron dot diagrams for each substance: CH₄ + 2O₂ → CO₂ + 2H₂O
Estimate the enthalpy change for this reaction. Start by drawing the Lewis electron dot diagrams for each substance: 4NH₃ + 3O₂ → 2N₂ + 6H₂O

Answers

1; H–H; it is nonpolar because the two atoms have the same electronegativities (answers will vary).

3a. Cl side

3b. S side

5a. slightly polar covalent

5b. definitely polar covalent

5c. likely ionic

7. C–H bond

9. −80 kJ

11. −798 kJ

Exercises (Violations of the Octet Rule)

Why can an odd-electron molecule not satisfy the octet rule?
Why can an atom in the second row of the periodic table not form expanded valence shell molecules?
Draw an acceptable Lewis electron dot diagram for these molecules that violate the octet rule.
1. NO₂
2. XeF₄
Draw an acceptable Lewis electron dot diagram for these molecules that violate the octet rule.
1. BCl₃
2. ClO₂
Draw an acceptable Lewis electron dot diagram for these molecules that violate the octet rule.
1. POF₃
2. ClF₃
Draw an acceptable Lewis electron dot diagram for these molecules that violate the octet rule.
1. SF₄
2. BeH₂

Answers

1. There is no way all electrons can be paired if there are an odd number of them.

3 a.

3b.

5a.

5b.

Exercises (Molecular Shapes)

What is the basic premise behind VSEPR?
What is the difference between the electron group geometry and the molecular geometry?
Identify the electron group geometry and the molecular geometry of each molecule.
1. H₂S
2. POCl₃
Identify the electron group geometry and the molecular geometry of each molecule.
1. CS₂
2. H₂S
Identify the electron group geometry and the molecular geometry of each molecule.
1. HCN
2. CCl₄
Identify the electron group geometry and the molecular geometry of each molecule.
1. BI₃
2. PH₃
What is the geometry of each species?
1. CN⁻
2. PO₄³⁻
What is the geometry of each species?
1. PO₃³⁻
2. NO₃⁻
What is the geometry of each species?
1. COF₂
2. C₂Cl₂ (both C atoms are central atoms and are bonded to each other)
What is the geometry of each species?
1. CO₃²⁻
2. N₂H₄ (both N atoms are central atoms and are bonded to each other)

Answers

1. Electron pairs repel each other.

3. a. electron group geometry: tetrahedral; molecular geometry: bent
b. electron group geometry: tetrahedral; molecular geometry: tetrahedral

5. a. electron group geometry: linear; molecular geometry: linear
b. electron group geometry: tetrahedral; molecular geometry: tetrahedral

7. a. linear
b. tetrahedral

9. a. trigonal planar
b. linear and linear about each central atom

Additional Exercises

Explain why iron and copper have the same Lewis electron dot diagram when they have different numbers of electrons.
Name two ions with the same Lewis electron dot diagram as the Cl⁻ ion.
Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the highest lattice energy?
Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the lowest lattice energy?
P₂ is not a stable form of phosphorus, but if it were, what would be its likely Lewis electron dot diagram?
Se₂ is not a stable form of selenium, but if it were, what would be its likely Lewis electron dot diagram?
What are the Lewis electron dot diagrams of SO₂, SO₃, and SO₄²⁻?
What are the Lewis electron dot diagrams of PO₃³⁻ and PO₄³⁻?
Which bond do you expect to be more polar—an O–H bond or an N–H bond?
Which bond do you expect to be more polar—an O–F bond or an S–O bond?
Use bond energies to estimate the energy change of this reaction.
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
Use bond energies to estimate the energy change of this reaction.
N₂H₄ + O₂ → N₂ + 2H₂O
Ethylene (C₂H₄) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.
Hydrogen peroxide (H₂O₂) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.

Answers

1. Iron has d electrons that typically are not shown on Lewis electron dot diagrams.

3. LiF

5. It would be like N₂:

9. an O–H bond

11. −2,000 kJ

13. trigonal planar about both central C atoms

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Exercises (Lewis Electron Dot Diagrams)

Exercises (Electron Transfer - Ionic Bonds)

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Exercises (Covalent Bonds)

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Exercises (Other Aspects of Covalent Bonds)

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Exercises (Violations of the Octet Rule)

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Exercises (Molecular Shapes)

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Additional Exercises

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