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4.E: Exercises

General, Organic, and Biochemistry with Problems, Case Studies, and Activities · LibreTexts

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    Multiple Choice Questions

    1. Which of the following is an ionic compound?
      1. PCl5
      2. BaS
      3. NO2
      4. XeF4
    2. Which of the following shows the correct Lewis dot structure for CaO? 
      Illustration
    3. How many valence electrons are present in phosphate?
      1. 5
      2. 8
      3. 26
      4. 32
    4. Which of the following shows the correct Lewis dot structure for CF4? 
      Illustration
    5. What is the formal charge on bromide?
      1. −1
      2. 0
      3. 7
      4. 8
    6. Which molecule requires octet expansion?
      1. CO2
      2. NH3
      3. CBr4
      4. SF6
    7. Which central atom is sp2 hybridized?
      1. BF3
      2. CH4
      3. NH3
      4. H2O
    8. What is the hybridization of carbon in CH2O?
      1. sp
      2. sp2
      3. sp3
      4. sp4
    9. Which molecule is polar?
      1. CO2
      2. SO2
      3. CH4
      4. PCl5
    10. Which molecule is nonpolar?
      1. SF6
      2. NH3
      3. CS2
      4. H2O

    Easy

    1. From their positions on the periodic table, order the atoms in terms of increasing electronegativity: F, Li, N
    2. From their positions on the periodic table, order the atoms in terms of increasing electronegativity: Cl, Br, Rb
    3. Predict which of the following compounds are ionic and which are covalent based on the location of their constituent atoms in the periodic table:
      1. MnO
      2. NCl3
      3. CoBr2
      4. K2S
      5. CO
    4. Predict which of the following compounds are ionic and which are covalent based on the location of their constituent atoms in the periodic table:
      1. CaF2
      2. HI
      3. CaO
      4. IBr
      5. CO2
    5. Write the Lewis dot symbol for each of the following ions:
      1. As3−
      2. I−
      3. Be2+
    6. Write the Lewis dot symbol for each of the following ions:
      1. O2−
      2. Ga3+
      3. Li+
    7. Write the Lewis dot symbols of the ions in each of the following ionic compounds:
      1. MgS
      2. Al2O3
      3. GaCl3
    8. Write the Lewis dot symbols of the ions in each of the following ionic compounds:
      1. K2O
      2. Li3N
      3. KF
    9. Write the Lewis dot structure for the following molecules:
      1. CCl4
      2. CO2
      3. O2
    10. Write the Lewis dot structure for the following molecules:
      1. N2
      2. H2O
      3. NH3
    11. What is the hybridization of the carbon atom in CH4?
    12. What is the hybridization of the carbon atom in CO2?
    13. Determine whether each of the following molecules is polar. Note: you should draw a Lewis dot structure of each molecule to determine your answer.
      1. CH2Cl2
      2. XeF4
      3. PCl3
    14. Determine whether each of the following molecules is polar.
      1. SiF4
      2. SCl2
      3. HCN

    Medium

    1. Explain how a nonpolar covalent bond, a polar covalent bond, and an ionic bond differ from one another.
    2. Which bond is more polar: N−O or N−F? Explain your reasoning.
    3. Order the following bonds from least to most polar: Si-O, N-O, P-O.
    4. Order the following bonds from least to most polar: C-Cl, C-Br, C-I.
    5. Draw a Lewis dot structure for each of the following species.
      1. COCl2
      2. PO33−
      3. I3–
    6. Draw a Lewis dot structure for each of the following species.
      1. CN−
      2. XeF4
      3. NH4+
    7. A Lewis dot structure for NO2− is shown below. What is the formal charge on N in this structure? What is the formal charge on each oxygen atom? What is the sum of the formal charges on all atoms in this structure? 
      Illustration
    8. A Lewis dot structure for CO32− is shown below. What is the formal charge on C in this structure? What is the formal charge on each oxygen atom? What is the sum of the formal charges on all atoms in this structure? 
      Illustration
    9. Draw a Lewis dot structure for each of the following molecules or ions. In all cases, you should draw the best Lewis dot structure allowing for octet expansion (when feasible) and following the rules of formal charges. Include resonance structures when relevant. Finally, state the VSEPR structure for each molecule or ion.
      1. PClO3
      2. ClO2−
      3. SO3
    10. Draw a Lewis dot structure for each of the following molecules or ions. In all cases, you should draw the best Lewis dot structure allowing for octet expansion (when feasible) and following the rules of formal charges. Include resonance structures when relevant. Finally, state the VSEPR structure for each molecule or ion.
      1. PO43−
      2. SOCl2
      3. ClO3–
    11. An incomplete Lewis dot structure of the molecule dimethyl fumarate, a medication used to treat multiple sclerosis, is shown below. Complete the Lewis dot structure by adding lone pairs and multiple bonds when needed. In addition, state the electron and local geometries around the atoms labeled C1, C2, C3, and O1. 
      Illustration
    12. An incomplete Lewis dot structure of the molecule Vitamin A is shown below. Complete the Lewis dot structure by adding lone pairs and multiple bonds when needed. In addition, state the electron and local geometries around the atoms labeled C1, C2, and O1. Note: In addition to the bonds shown, CH2 indicates that the C atom is bonded to two H atoms and CH3 indicates three bonds to H atoms. 
      Illustration
    13. The Lewis dot structure for the DNA base adenine is shown below. State the hybridization of N1, N2, and C1. In addition, state the number of π (pi) bonds present in this molecule. 
      Illustration
    14. The Lewis dot structure for the amino acid histidine is shown below. State the hybridization of N1, N2, C1, C2, and O1. In addition, state the number of π (pi) bonds present in this molecule. 
      Illustration
    15. Draw a Lewis dot structure for each of the following molecules, allowing for octet expansion (when feasible) and following the rules of formal charges. State the VSEPR structure for each molecule and state whether the molecule is polar or nonpolar.
      1. COCl2
      2. IF5
      3. RnCl2
    16. Draw a Lewis dot structure for each of the following molecules, allowing for octet expansion (when feasible) and following the rules of formal charges. State the VSEPR structure for each molecule and state whether the molecule is polar or nonpolar.
      1. SO2Cl2
      2. BF3
      3. ClF3

    Challenge

    1. Draw all possible Lewis dot structures for an ion containing one atom each of O, C, and N, with an overall charge of -1. You should have a total of nine Lewis dot structures. Assign formal charges to all atoms in each structure. Based on your formal charge analysis, which structure is the best structure? Explain your choice.
    2. An incomplete Lewis dot structure of the antihistamine diphenhydramine is shown below. Add lone pairs and multiple bonds as needed to complete this structure. In addition, state the electron and local geometries for the atoms labeled C1, C2, C3, O1, and N1. In addition, state the hybridization for each of these numbered atoms. 
      Illustration

    Health-Related

    1. Iodine (I2) is a disinfectant. It is the active ingredient in topical disinfectants like Betadine. What is the Lewis structure of I2? Is it polar?
    2. Chlorine (Cl2) is a disinfectant and bleaching agent that is used to treat water for drinking. What is the Lewis structure of Cl2? Is it polar?
    3. Dinitrogen monoxide, or nitrous oxide, is a linear molecule that has been used as an inhaled anesthetic. What is the Lewis structure of N2O? Is it polar?
    4. Chloroform, CHCl3, is a small molecule with carbon as the central atom. It was used as an anesthetic in the 1800s but was abandoned due to toxicity and fatalities. What is the Lewis structure of chloroform? Is it polar?
    5. Bicarbonate is an important ion in blood. What is the Lewis structure of bicarbonate? Show formal charges and include any resonance structures.
    6. The nitrate anion is found in water and food and is present in our bodies in low amounts. What is the Lewis structure of nitrate? Show formal charges and include any resonance structures.

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