The Periodic Table

Fluorine ($F$)

Chlorine ($Cl$)

Oxygen ($O$)

Nitrogen ($N$)

Group 1

Group 14

Group 17

Group 18

Atomic radius decreases down the group, making it harder to lose the valence electron.

Effective nuclear charge increases significantly, pulling the valence electron closer.

The outer electron is further from the nucleus and more shielded, so it is less strongly attracted.

Shielding effect decreases down the group, allowing the nucleus to hold the outer electron tighter.

$-1$

$+2$

$+1$

$+3$

Oxygen ($O_2$)

Hydrogen ($H_2$)

Chlorine ($Cl_2$)

Carbon dioxide ($CO_2$)

Reactivity decreases because the atoms get smaller.

Reactivity remains constant because they all have one valence electron.

Reactivity increases because the outer electron is further from the nucleus.

Reactivity decreases because the nuclear charge increases.

Reactivity increases and the color becomes lighter.

Reactivity increases and the color becomes darker.

Reactivity decreases and the color becomes lighter.

Reactivity decreases and the color becomes darker.

The number of protons increases, pulling electrons closer.

The number of electron shells increases, increasing the distance from the nucleus.

The electronegativity increases, making the atom smaller.

The atoms lose electrons more easily as you go down the group.

They exist as monatomic atoms in their natural state.

They are diatomic molecules held together by covalent bonds.

They are diatomic molecules held together by ionic bonds.

They form giant covalent lattice structures like diamond.

They are always colorless liquids.

They form white precipitates with all acids.

They are often brightly colored.

They are all gaseous at room temperature.

Calcium ($Ca$)

Iron ($Fe$)

Sodium ($Na$)

Barium ($Ba$)

They act as efficient solvents.

They increase the yield by shifting equilibrium.

They act as catalysts to increase the rate of reaction.

They prevent the corrosion of the reaction vessels.

Argon

Krypton

Neon

Xenon

The boiling points increase.

The boiling points decrease.

The boiling points remain constant.

The boiling points decrease then increase.

Helium is more abundant and cheaper than hydrogen.

Helium has a lower density and is highly flammable.

Helium has a higher density but is more reactive.

Helium has a low density and is chemically inert (non-flammable).