Periodic Trends

What trend in atomic radius do you see as you go down a group/family on the periodic table?

It increases.

What causes this trend?

Adding more energy.

What trend in atomic radius do you see as you go across a period/row on the periodic table?

It decreases.

What causes this trend?

More protons, more pull.

Define ionization energy.

The amount of energy required to remove an electron from an atom.

Is it easier to form a positive ion with an element that has a high ionization energy or an element that has a low ionization energy?

An element with low ionization energy because the less energy, the less work.

Explain why it is hard to remove an inner shell electrons than a valence electron from an atom.

It takes more energy to remove and inner than an outer

Explain why sodium forms a 1+ ion (Na+) but magnesium forms a 2+ ion (Mg 2+).

Na- one valence electron

Mg- two valence electrons

What trend in ionization energy do you see as you go down a group/family on the periodic table?

It decreases.

What causes this trend?

Electrons further away from nucleus.

What trend in ionization energy do you see as you go across a period/row on the periodic table?

It increases.

What causes this trend?

Atoms want to have a full valence shell.

Define electronegativity.

How bad an atom wants to gain an electron

How does the ionic radius of a nonmetal compare with its atomic radius?

Ionic radius is greater because it gains electrons but the atomic radius is smaller.

What trend in electronegativity do you see as you go down the group/family on the periodic table?

It decreases.

What causes this trend?

The further away the electrons from the nucleus, the less attraction there is

What trend in electronegativity do you see as you go across a period/row on the periodic table?

It increases.

What causes this trend?

Atoms are closer to filling their valence shell.