Group 13 and Period 4 Trends

Group 13 and Period 4 Trends

Group 13 Elements

Ionic Radii Trend

Reactivity Trends

Group 13 Reactivity-Reactivity decreases as going down in the group. Why? The general trend down Group 13 is from non-metallic to metallic character. Boron is a nonmetal and is covalent in reactivity. The other elements are more metallic, much larger, and exhibit a ionic bonding structure.

Group 13 and Period 4

As you go down a group, the ionic radius increases because the number of electrons and filled electron shells increases, but the number of valence electrons remains the same. The outermost electrons in a group are exposed to the same effective nuclear charge, but electrons are found farther from the nucleus as the number of filled energy shells increases.

As you move across a period, the ionic radius decreases because the radius decreases, because the electrons are more tightly bound. More protons are being added to each element across a period. The more protons there are, the more of a nuclear charge you will get. Also, more valence electrons are added one at a time to the outer energy shell. Electrons within a shell cannot shield each other from the attraction to protons.

B-Boron

Al-Aluminum

Ga-Gallium

In-Indium

Tl-Thallium

Period 4 Reactivity-As you move from left to right, the reactivity decreases. Why? The # of valence electrons increases from left to right, and the more valence electrons there are the less reactive they will be. The elements with the least amount of valence electrons will react more violently because they do not require a lot of enegery to release their extra electron.

Lewis Dot structures

Atomic Radii Trends

Ionization Trends

Period 4 Lewis dot structures

Group 13 Lewis Dot Structures for all

Group 13

Period 4

Period 4 Elements

The general trend for the ionization energy of atoms in group 13 is generally sporadic and does not follow much of a trend, however, generally the ionization energy decreases as you move down a group.

Group 13 and Period 4

As you move from top to bottom, the atomic radii increases.

As you move down in groups there is an extra electron orbital for each group moved down so the radii also increases. As you move from left to right on a period the atomic radii decreases because from left to right across the periodic table you are adding one more proton every time, which increases the nuclear charge of the atom. An increased nuclear charge means the nucleus attracts the electrons more to it hence the size of the atom decreases as it "tightens".

Potassium

Calcium

Germanium

Arsenic

Selenium

Bromine

Krypton

The general trend for period 4's 1st ionization energy is that it increases as you move from left to right across the period. It becomes harder to remove one electron because when there are more protons in the nucleus, the attraction between the positivly charged proton and negativly charged electron become greater, this making it harder to remove the electron.

3 Valence Electrons

per element in group

13

K-Potassium

Ca-Calcium

Ge-Germanium

As-Arsenic

Se-Seleniun

Br-Bromine

Kr-Krypton

Electronegativity Trends

Period 14

Group 13

There really is no trend for the electronegativity for Group 13 as all the atoms have the same number of valence electrons and no trend is prevalent. though, for most other groups, electronegativity decreases as you move down a group.

In period 4 the trend for electronegativity is as you move from left to right, it increases. this is because atoms with less electrons are obligated to give away there electrons, while ones with more electrons that are cloase to filling there rings will want an extra electron.