Reference no: EM132732285
Ionic and Covalent Bonding
1. Contrast the physical characteristics of ionic compounds, covalent compounds and metallic compounds.
2. What information can you use to predict whether a bond between two atoms is covalent or ionic?
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:
(a) Cl2CO
(b) MnO
(c) NCl3
(d) CoBr2
(e) K2S
(f) CO
(g) CaF2
(h) HI
4. Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond.
5. From its position in the periodic table, determine which atom in each pair is more electronegative:
(a) Br or Cl
(b) N or O
(c) S or O
6. Which atoms can bond to sulfur so as to produce a positive partial charge on the sulfur atom?
7. Which is the most polar bond?
(a) C-C
(b) C-H
(c) N-H
(d) O-H
(e) Se-H
8. Identify the more polar bond in each of the following pairs of bonds:
(a) HF or HCl
(b) NO or CO
(c) SH or OH
9. What is the energy change in kJ/mole when LiF is formed from elemental lithium and fluorine? Is this process endothermic or exothermic? Does this process require or release energy? The lattice energy of LiF is -1036 kJ/mole, the ionization energy of Li(g) is 520 kJ/mole and the electron affinity of F(g) is -328 kJ/mole.