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5.E: Covalent Bonding and Simple Molecular Compounds (Exercises)-

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    5.1 Covalent Bonds

    PROBLEM 5-1 How is a covalent bond formed between two atoms?

    PROBLEM 5-2 How does covalent bonding allow atoms in group 6A to satisfy the octet rule?

    PROBLEM 5-3 Identify whether each compound(s) is/are ionic.

    1. NaI
    2. Au2CO3
    3. N2O
    4. SiO2
    Answer

    Only answers (a) and (b) are ionic compounds. Both formulas begin with a metal (atom from the left side of the periodic table) ion.

    PROBLEM 5-4 Identify whether each compound(s) is/are covalent.

    1. SiH3
    2. C6H5Cl
    3. KC2H3O2
    4. Ca(OH)2
    Answer

    Only answers (a) and (b) are covalent compounds. Both formulas begin with nonmetals and/or metalloids (atoms from the right side of the table)

    PROBLEM 5-5 Predict the number of covalent bonds formed by each nonmetal atom.

    Atom N Cl C O Br H
    # Covalent Bonds            

    5.2: Drawing Lewis Structures

    PROBLEM 5-6 Draw the Lewis diagram for the covalent bond in:

    1. The H2 molecule.
    2. Draw the Lewis diagram for the covalent bond in the Br2 molecule.
    3. Draw the Lewis diagram for the covalent bond in the HCl molecule.
    4. Why do hydrogen atoms not follow the octet rule when they form covalent bonds?

    PROBLEM 5-7 Draw the Lewis diagram for the covalent bonding in

    1. H2S. How many bonding electrons and non-bonding electrons are in the molecule?
    2. CF4. How many bonding electrons and non-bonding electrons are in the molecule?
    3. PCl3. How many bonding electrons and non-bonding electrons are in the molecule?

    PROBLEM 5-8 Each molecule contains double bonds. Draw the Lewis diagram for each. The first element is the central atom.

    1. CS2
    2. C2F4
    3. COCl2

    PROBLEM 5-9 Each molecule contains multiple bonds. Draw the Lewis diagram for each. Assume that the first element is the central atom, unless otherwise noted.

    1. N2
    2. CO
    3. HCN (The carbon atom is the central atom.)
    4. POCl (The phosphorus atom is the central atom.)

    5.3 Naming Covalent Compounds

    PROBLEM 5-10 Write the formula for each covalent compound.

    1. iodine trichloride
    2. disulfur dibromide
    3. arsenic trioxide
    4. xenon hexafluoride
    5. chlorine trifluoride
    6. phosphorus pentachloride
    7. sulfur dioxide
    8. nitrogen dioxide
    9. dioxygen difluoride
    10. dinitrogen pentoxide
    11. sulfur hexafluoride
    12. nitrogen monoxide

    PROBLEM 5-11 Write the name for each covalent compound.

    1. SiF4
    2. NO2
    3. CS2
    4. P2O5
    5. CO
    6. S2O3
    7. BF3
    8. GeS2

    5.8 Unequal Sharing- Polar Covalent Bonds

    PROBLEM 5-21 What is the name for the distance between two atoms in a covalent bond?

    PROBLEM 5-22 What does the electronegativity of an atom indicate?

    PROBLEM 5-23 Using the Figure from section 5.8, determine which atom in each pair has the higher electronegativity.

    1. H or C
    2. O or Br
    3. Na or Rb
    4. I or Cl

    PROBLEM 5-24 Using the Figure from section 5.8, determine which atom in each pair has the lower electronegativity.

    1. Mg or O
    2. S or F
    3. Al or Ga
    4. O or I

    PROBLEM 5-25 Will the electrons be shared equally or unequally across each covalent bond? If unequally, to which atom are the electrons more strongly drawn?

    1. a C–O bond
    2. an F–F bond
    3. an S–N bond
    4. An I–Cl bond

    PROBLEM 5-26 Will the electrons be shared equally or unequally across each covalent bond? If unequally, to which atom are the electrons more strongly drawn?

    • a C–C bond
    • a S–Cl bond
    • an O–H bond
    • an H–H bond

    PROBLEM 5-27 Arrange the following bonds from least polar to most polar: H-F, H-N, H-O, H-C

    PROBLEM 5-28 Arrange the following bonds from least polar to most polar: C-F, C-N, C-O, C-C

    Solution of Selected Problems

    PROBLEM 5-6

    a-clipboard_e008252218a6269ce674e8598c8c45b76.png clipboard_ed6c566be2219377b4bf3581daeb219ee.png b- clipboard_eb9c59adf9c59c3611dcb4bb36e74bda0.png clipboard_ebf435e2bb1d4ab33089847b44b24e3aa.png c-clipboard_eac8aed392cf4840684480fe3699e09ca.png clipboard_e2bc812a0ebd7b413e350365152efc394.png

    d-Hydrogen atoms follow the duet rule (not the octet rule). This is because it has only one shell and this shell can only hold 2 electrons.

    PROBLEM 5-7

    a-9.jpg bonding electrons: 4; nonbonding electrons: 4
    b-11.jpgbonding electrons: 8; nonbonding electrons: 24

    c- clipboard_e17030c2141b989f269868f6ced872ece.png bonding electrons: 6; nonbonding electrons: 20

    PROBLEM 5-8

    a.1a.jpgb.1b.jpgc.1c.jpg

    PROBLEM 5-9

    a. clipboard_e5140e3be566dc8ae53fa713d1a23a3dc.png b. clipboard_e7a3ed60e086664fba0796c9e1688da22.png c. clipboard_ece7acc6e4dee2fc87065c548827ea90a.png d. clipboard_e077dd4a07a9a36e76b80ea93c2ba82d6.png

    PROBLEM 5-10

    a. ICl3 b. S2Br2 c. AsO3 d. XeF6 e. ClF3 f. PCl5 g. SO2 h. NO2 i. O2F2 j. N2O5 k. SF6 l. NO

    PROBLEM 5-11

    1. silicon tetrafluoride
    2. nitrogen dioxide
    3. carbon disulfide
    4. diphosphorus pentoxide
    5. carbon monoxide
    6. disulfur trioxide
    7. boron trifluoride
    8. germanium disulfide

    5.8 Unequal Sharing- Polar Covalent Bonds

    PROBLEM 5-21 Electronegativity is a qualitative measure of how much an atom attracts electrons in a covalent bond.

    PROBLEM 5-22 nonpolar; polar; ionic

    PROBLEM 5-23

    1. C
    2. O
    3. Na
    4. Cl

    PROBLEM 5-24

    1. Mg
    2. S
    3. Al
    4. I

    PROBLEM 5-25

    1. unequally toward the O
    2. equally
    3. unequally toward the N
    4. unequally toward the Cl

    PROBLEM 5-26

    • equally
    • unequally toward the Cl
    • unequally toward the O
    • equally

    PROBLEM 5-27 The electronegativity difference increases from 0.4; 0.9; 1.4; 1.9. Hence, the least to most polar: H-C, H-N, H-O, H-F

    PROBLEM 5-28 The electronegativity difference increases from 0; 0.5; 1.0; 1.5. Hence, the least to most polar: C-C, C-N, C-O, C-F

    This page titled 5.E: Covalent Bonding and Simple Molecular Compounds (Exercises)- was last modified on Thu, 31 Jul 2025 00:06:37 GMT and is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Sol Parajon Puenzo (Cañada College) .