Topic 7: Periodic Trends, Video D: Ionization Energy Part 2

Question 1

As you move across a period atoms get smaller and ionization energy increases or decreases?

Answer 1

Increases.

Question 2

The closer and electron is to the nucleus the more difficult or easy it is to remove them?

Answer 2

Difficult.

Question 3

Why is the ionization energy for Al smaller than for Mg?

Answer 3

The Aluminum configuration puts an electron in the 3p orbital. The 3p orbitap is typically slightly higher in energy than the 3s and so it is easier to remove a 3p electron than a 3s electron. The electrons in the 3 p orbitals are said to be shielded by the 3 s electrons.

Question 4

Shielded electrons are more or less strongly attracted to the nucleus?

Answer 4

Less strongly attracted and more easily removed.

Question 5

Why is the ionization energy smaller for S than it is for P?

Answer 5

The 4th p electron in S is spin paired. The orbital is thus at a higher energy than phosphorus. The 4th p electron in S is easier to remove Electron electron repulsions are higher than those in P.

Question 6

In general ionization energy increases or decreases as you move up and across the periodic table.

Answer 6

Increases.

Question 7

What is the first exception to ionization energy increasing as size decreases as you move up and across the periodic table?

Answer 7

The electron electron repulsions in the fourth p electron as you go from group 15 to group 16 makes these electrons easier to remove. The 4th p electron is spin paired.

Question 8

What is the second exception to ionization energy increasing as size decreases as you move up and across the periodic table?

Answer 8

The shielding of the p electrons in group 13 by their s electrons make the first p electrons easier to remove.