Periodicity Worksheet (Page 3 of 4) in pdf

Periodicity Worksheet Page 3

2 pts EC per page

4. Along with the increased distance of the outer electrons from the nucleus, the

of the inner electrons causes ionization energy to decrease going down a column of the periodic table.

5. A low ionization energy is characteristic of

6. Ionization energies tend to

across periods of the periodic table.

7. An element with a high ionization energy is classified as a(n)

8. The attraction an atom has for electrons shared in a bond is called

9. The distance from the nucleus to the outermost electron is known as

10. The

do not have measured electronegativites since they do not

commonly form compounds.

11. The electron arrangement with a complete outermost s and p sublevel is known as

E. Trend Chart: Draw in the trends in the following on the periodic table:

Ionization energy

electronegativity

atomic radius

shielding effect

F. Atomic Radius

1. Circle the atom in each pair with the larger atomic radius.

a) Li, K

b) Ca, Ni

c) Ga, B

d) O, C

e) Cl, Br

f) Be, Ba

g) Si, S

h) Fe, Au

2. Chlorine selenium, and bromine are located near each other on the periodic table. Which of these

elements is the smallest atom and which has the highest ionization energy?

3. Which of the following atoms is smallest: nitrogen, phosphorus, or arsenic? Which of these atoms has the

greatest electronegativity?

4. Which of the following is the largest: a potassium atom, a potassium ion, or a rubidium atom?

5. Which of the following is the smallest: a lithium atom, a lithium ion, or a sodium atom?

6. In terms of electron configuration and shielding, why is the atomic radius of sodium smaller than that of

potassium?

7. In terms of electron configurations and shielding, why do atoms get smaller as you move across a period?

p−

Periodicity Worksheet Page 3