Question

1. The following successive ionization energies are for a particular metal:

IE₁ = 578 kJ mol^-1

IE₂ = 1820 kJ mol^-1

IE₃ = 2750 kJ mol^-1

IE₄ = 11600 kJ mol^-1

Based on these ionization energies, what charge ion would you expect to be the most stable? Briefly explain.

1. Write shorthand electronic configurations for the atoms/ions below:
   1. Na
   2. V³⁺
   3. S^2-

2. Which statement is true of an endothermic reactions? Briefly explain your choice.
   1. Weak bonds break and strong bonds form
   2. Strong bonds break and weak bonds form
   3. The bonds that break and those that form are of approximately the same strength

3. The difference in electronegativity between two atoms bonded together determines if the bond is non polar covalent (∆EN between 0-0.4), polar covalent (∆EN between 0.4-2.0) or ionic (∆EN greater than 2). Using Figure 9.12 in your textbook, classify these bonds as non polar covalent, polar covalent or ionic.
   1. Sr-F
   2. C-S
   3. N-O

Answer 1

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