Ionization Energy - Chemistry LibreTexts

Questions

1) By looking at following electronic configuration of elements, can you predict which element has the lowest first ionization energy?

1. 1s2 2s2 2p6
2. 1s2 2s2 2p4
3. 1s2 2s2 2p6 3s2
4. 1s2 2s2 2p6 3s1
5. 1s2 2s2 2p5.

2) The ionization energy of \(Na^{+3}\) ion is one of the following (7)

1. More than first ionization only
2. More than second ionization only
3. Sum of first and second ionization energies
4. Sum of first, second, and third ionization energies

3) Ionization energies and electron affinities are

1. Dependent upon each other,
2. Similar trend of increasing/decreasing along the periods and within the group of periodic table,
3. Inversely related with each other,
4. Indirectly related with each other

4) Ionization energy is the ability to capture an electron:

1. False,
2. True

5) The second ionization energy of Mg is greater than second ionization energy of Al:

1. False,
2. True

6) Which group would generally have the lowest first ionization energy?

1. Transition Metals
2. Alkali Metals
3. Noble Gases
4. Alkaline Earth Metals
5. Halogens

7) Sulfur has a first ionization energy of 999.6 kJ/mol. Rubidium has a first ionization energy of 403 kJ/mol. What bond do they form when chemically combined?

1. Covalent
2. Polar Covalent
3. Ionic

8) Ionization energy, when supplied to an atom, results in a(n)

1. Anion and a proton
2. Cation and a proton
3. Cation and an Electron
4. Anion and an electron

9) Low first ionization energy is considered a property of

1. Metals
2. Nonmetals

10) Gallium has a first ionization energy of 578.8 kJ/mol, and calcium has a first ionization energy of 589.8 kJ/mol . According to periodic trends, one would assume that calcium, being to the left of gallium, would have the lower ionization energy. Explain, in terms of orbitals, why these numbers make sense.