Please help me with this chemistry problem?

Question

Here is the question. If anyone knows the answer please tell me because I need the answers by tomorrow. Thanks!

Use the details of modern atomic theory to explain the following:
a. For the alkali metals, the ionic radius increases as atomic number increases.
b. The radius of the chlorine atom is smaller than the radius of the chloride ion.
c. The first ionization energy of aluminum is lower than the first ionization energy of magnesium.
d. For magnesium, the difference between the first and second ionization energies is much less than the difference between the second and third ionization energies.

Answer 1

a) here, you're basically going down a column of the periodic table. the electrons are thus filling up higher energy levels, which causes the atomic radii to increase.
b) the chloride ion has one more electron than the chlorine atom, so the increased force of repulsion among the electrons causes the atom to expand.
c) magnesium has a full 3s subshell, so it's relatively difficult to remove an electron. aluminum has one lone electron in its 3p subshell, so removing it would lead to a relatively stable configuration (magnesium's configuration), and removing an electron is easier.
d) after removing 2 electrons from magnesium, you'll have reached a noble gas configuration, so the 3rd ionization energy of magnesium is SUPER-HIGH, resulting in a greater difference.

Answer 2

I'm going to give you the answer you probably don't want to hear. I'm sure all of these things are discussed in your textbook in the section describing periodic properties. So, open your text book and read about those properties. That way, you'll actually KNOW the information and will have actually LEARNED something.

Answer 3

If you just read your book you would know the answers.

This is the easy stuff.

If you don't read and learn yourself you will not pass the course as you haven't even gotten to the hard stuff yet.