Module 4

Atomic Trends

100

Arrange in order of increasing atomic size: Rb, K, Cs

K < Rb < Cs

200

Arrange in order of increasing IE1: Sr, Ca, Br

Ba < Sr < Ca

300

Which would you expect to have higher magnetic character: P or Ba

Ba

400

Arrange in order of increasing IE1: N, B, Ne

B < N < Ne

500

Based on their positions in the periodic table, predict which has the largest electron affinity: Mg, Ba, B, O, Te.

O

Noble Gas Configurations, Pseudonoble Gas Configurations, and Inert Pair Configurations

100

What kind of configuration does Na⁺ have

noble gas configuration

200

What kind of configuration does Sn²⁺ have?

Inert Pair Configuration

300

What kind of configuration does Ag⁺ have

Pseudo Noble Gas Configuration

400

What kind of configuration does O^2- have

noble gas configuration

500

What kind of configuration does Zn²⁺ have

Pseudo Noble Gas Configuration

Ion Size

100

Is Ca²⁺ bigger or smaller than Ca

Smaller

200

Is N^3- bigger or smaller than N

Bigger

300

Is N^3- bigger or smaller than Al³⁺

Bigger

400

Is Se^2-, Cl^-, or O^2- biggest

Se^2-

500

Is P^3-, S^2-, or Cl^- smallest

Cl^-

Core, Outer, Valence Electrons

100

How many core, outer, and valence electrons does As have?

28 core

5 outer

5 valence

200

How many core, outer, and valence electrons does Zr have?

36 core

2 outer

4 valence

300

How many core, outer, and valence electrons does Mg have?

10 core

2 outer

2 valence

400

How many core, outer, and valence electrons does Ba have?

54 core

2 outer

2 valence

500

How many core, outer, and valence electrons does Bi have?

78 core

5 outer

5 valence

Atomic Trends Explained

100

How does atomic size trend and why

The largest elements are in the bottom left corner. These are the elements with the most electron shells in each group and the smallest atomic number in each period. This means the Zeff is very low

200

What is the IE trend and why does it exist?

Ionization energy is highest in the top right corner of the periodic table. This is where it would be most expensive (cost the most energy) to remove an electron because the Zeff is very high. The number of protons increases and radius shrinks. There's stronger attraction between the electrons and the nucleus, so it's more difficult to remove an electron. The elements with high IE prefer to form anions and those with a low IE prefer to be cations.

300

What is the EA trend and why does it exist?

Electron affinity measures the energy change when an electron is added. It's highest in the top right. High electron affinities are always big negative numbers, because we're talking about the magnitude. High negative numbers means that an atom will release a lot of energy when it becomes an anion, so it's a favorable process. Elements with high electron affinities love gaining electrons and become anions. The noble gases are excluded from this trend.

400

Why are there successive IE and what do they mean? What's the trend between each IE

Successive IEs relate to the cost of each electron removed. IE₁ is the cost of the first electron, IE₂ is the second, and so on. Each successive IE is higher than the previous because it's harder to remove each electron.

500

If an atom has high IE, will you expect a high or low magnitude EA and why? Would this relate to elements that like to form cations or anions?

If something has a high IE, it means that it's expensive to remove an electron. It would rather gain an electron instead. Elements that have high magnitude EA release a lot of energy when they gain an electron, so it happens readily. Therefore, anions will have both a high IE and a high EA.