Periodicity Worksheet (Page 2 of 4) in pdf

Periodicity Worksheet Page 2

2 pts EC per page

3. Explain the difference in first ionization energy between lithium and beryllium.

4. The first and second ionization energies of magnesium are both relatively low, but the third ionization

energy requirement jumps to five times the previous level. Explain. (Hint: What is the most likely ion for

magnesium to become when it is ionized?)

5. Compare the first ionization energies for the noble gases.

6. Compare the first ionization energies for a noble gas with that of a halogen in the same period. Support

your comparison with an orbital filling diagram.

7. Where would the largest jump in ionization energies be for oxygen? (Hint: with the loss of how many

electrons?)

8. How can you tell from a list of ionization energies for an element where a core (non-valence) electron has

been removed?

C. Electronegativity and Electron Affinity

1. Arrange the following elements in order of increasing electronegativity.

a. gallium, aluminum, indium

b. calcium, selenium, arsenic

c. oxygen, fluroine, sulfur

d. phosphorus, oxygen, germanium

2. Will the electronegativity of barium be larger or smaller than that of strontium? Explain.

3. Compare the electronegativity of tellurium to that of antimony. Explain your reasoning.

D. Definitions (not all terms are used and some are used more than once)

 atomic radius

 increase

 noble gases

 decrease

 ionization energy

 nonmetals

 electronegativity

 metals

 semimetal

 first ionization energy

 noble gas configuration

 shielding effect

is the energy required to remove an electron from an atom.

2. The energy needed to remove the most loosely held electron from a neutral atom is called

3. When they have a(n)

, ions have a stable, filled outer electron level.

p−

Periodicity Worksheet Page 2