Question

Consider the group 1A elements sodium (period 3), potassium (period 4), and rubidium (period 5). What would you predict about the ionization energies of these elements?

Answer 1

Ionzation energy describes the amount of energy needed to remove a valence electron.

Group 1 electrons have only 1 electron in their valence, and are very willing to give up that electron to reach a higher stability; as opposed to gaining 7 more.

As opposed to a group 7 halogen which has 7 valence electrons and it eager to attain one more electron to fill its octet, as opposed to removing 7.

Because group 1 elements only have 1 valence electron, the ionization energy needed to remove an electron is relatively low; especially when compared to a group 8 noble gas which has a fully stable octet in its valence.

Does that make sense?

Answer 2

Ionization energies increase from left to right and down to up

Answer 3

So groups 1 to 5 would increase ionization energy

Answer 4

As we go down the group, the ionisation energy increases because it is the ability of an atom to give away its electrons. As the atom size increases down the group, the influence of nuclear charge over the outermost electrons or the valence electrons decreases. Hence it can give away its electrons easily. Therefore, Ionisation energy increases as we go down the group from top to bottom in a periodic table.

Answer 5

Na, K, Rb are all group one elements and belong to same group.so, the ionisation energy of Rb>K>Na