Atomic Trends
Arrange in order of increasing atomic size: Rb, K, Cs
K < Rb < Cs
What kind of configuration does Na+ have
Is Ca2+ bigger or smaller than Ca
Smaller
How many core, outer, and valence electrons does As have?
28 core
5 outer
5 valence
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
Arrange in order of increasing IE1: Sr, Ca, Br
Ba < Sr < Ca
What kind of configuration does Sn2+ have?
Inert Pair Configuration
Is N3- bigger or smaller than N
Bigger
How many core, outer, and valence electrons does Zr have?
36 core
2 outer
4 valence
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.
Which would you expect to have higher magnetic character: P or Ba
Ba
What kind of configuration does Ag+ have
Pseudo Noble Gas Configuration
Is N3- bigger or smaller than Al3+
Bigger
How many core, outer, and valence electrons does Mg have?
10 core
2 outer
2 valence
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.
Arrange in order of increasing IE1: N, B, Ne
B < N < Ne
What kind of configuration does O2- have
noble gas configuration
Is Se2-, Cl-, or O2- biggest
Se2-
How many core, outer, and valence electrons does Ba have?
54 core
2 outer
2 valence
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.
Based on their positions in the periodic table, predict which has the largest electron affinity: Mg, Ba, B, O, Te.
O
What kind of configuration does Zn2+ have
Pseudo Noble Gas Configuration
Is P3-, S2-, or Cl- smallest
Cl-
How many core, outer, and valence electrons does Bi have?
78 core
5 outer
5 valence
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.