Chemistry chapter 8

CHEM 1210 – General Chemistry I: Chapter 08 – Basic Concepts of Chemical Bonding Study Notes

Lattice Energy Predictions

1. Predicting Lattice Energy Orderings

   • Without referencing Table 8.2, determine the ordering of lattice energy for the following ionic compounds. Choices:

     • (a) NaCl > MgO > CsI > ScN

     • (b) ScN > MgO > NaCl > CsI

     • (c) NaCl > CsI > ScN > CaO

     • (d) MgO > NaCl > ScN > CsI

     • (e) ScN > CsI > NaCl > MgO

Compounds Formation

2. Binary Compounds

   • Given the Lewis symbols for nitrogen (N) and fluorine (F) from Table 8.1, predict the formula of the stable binary compound formed when nitrogen reacts with fluorine.

   • Lewis Structure: [Draw the correct Lewis structure here]

Electron Pair Analysis

3. Shared vs. Unshared Electron Pairs

   • Identify which molecule has the same number of shared electron pairs and unshared electron pairs. Options:

     • (a) HCl

     • (b) H2S

     • (c) PF3

     • (d) CCl2F2

     • (e) Br2

Electronegativity Facts

4. Electronegativity Statements

   • Identify the false statement about electronegativity among the following:

     • (a) Electronegativity is the ability of an atom in a molecule to attract electron density toward itself.

     • (b) Electronegativity is the same as electron affinity.

     • (c) The numerical values for electronegativity have no units.

     • (d) Fluorine is the most electronegative element.

     • (e) Cesium is the least electronegative element.

Bond Polarity

5. Most Polar Bond Determination

   • Which bond is most polar? Choices include:

     • (a) H-F

     • (b) H-I

     • (c) Se-F

     • (d) N-P

     • (e) Ga-Cl

Dipole Moment Calculations

6. Dipole Moment of HF

   • Calculate the dipole moment for HF with a bond length of 0.917 Å, assuming it behaves as a completely ionic bond. Options:

     • (a) 0.917 D

     • (b) 1.91 D

     • (c) 2.75 D

     • (d) 4.39 D

     • (e) 7.37 D

7. Chlorine Monofluoride (ClF) Dipole Moment Analysis

   • Given a dipole moment of ClF(g) at 0.88 D and a bond length of 1.63 Å:

     • (a) Determine which atom carries the expected partial negative charge.

     • (b) What is the charge on that atom in units of elementary charge (e)?

Lewis Structures

8. Lewis Structure for HCN

   • Draw the Lewis structure for HCN. [Include Lewis structure here].

9. Lewis Structure for C2H3N

   • For the molecule with the formula C2H3N, where N is connected to only one other atom, draw the appropriate Lewis structure. Identify the number of double bonds in the structures. Choices:

     • (a) 0

     • (b) 1

     • (c) 2

     • (d) 3

     • (e) 4

10. Lewis Structure for BrO3- Ion

    • Draw the Lewis structure for the BrO3- ion. [Include structure here].

11. Nonbonding Electron Pairs in Peroxide Ion (O2^2-)

    • How many nonbonding electron pairs are there in the Lewis structure of the peroxide ion (O2^2-)? Choose from:

      • (a) 7

      • (b) 6

      • (c) 5

      • (d) 4

      • (e) 3

Formal Charge in Molecules

12. Formal Charge Minimization in POCl3

    • Determine how many bonds phosphorus makes to other atoms in phosphorus oxychloride (POCl3) to minimize formal charge. Choices include:

      • (a) 3

      • (b) 4

      • (c) 5

      • (d) 6

      • (e) 7

Lone Pairs in Molecules

13. Lone Pairs on Central Sulfur Atom

    • Identify in which of the following molecules or ions the central sulfur atom has only one lone pair of electrons:

      • (a) SF4

      • (b) SF6

      • (c) SOF4

      • (d) SF2

      • (e) SO4^2-

14. Maximum Octet Electrons

    • From the following list, identify which atom is never found with more than an octet of valence electrons:

      • S

      • C

      • P

      • Br

      • I

15. Lewis Structure for XeF2

    • Draw the Lewis structure for xenon difluoride (XeF2). [Include Lewis structure here].