Name ____________________________________________________ Period ____

1.2.4a Ionization Energy Quiz 1

1.  Define ionization energy.

2.  Which electron is the first to be removed from any atom?

1. an s electron
2. a p electron
3. a valence electron
4. an electron from the first principal energy level

3.  The presence of inner-shell electrons cause the outermost electrons of an atom to be less attracted to the nucleus.  This is called electron _____.

1. reduction
2. shielding
3. dampening
4. canceling

4.  Ionization energy generally _____ from left to right across a period of the periodic table.

1. increases
2. decreases
3. stays the same
4. increases and decreases randomly

5.  Ionization energy generally _____ from top to bottom down a group of the periodic table.

1. increases
2. decreases
3. stays the same
4. increases and decreases randomly

6.  Compared to the ionization energy of a lithium atom, the ionization energy of a beryllium atom is larger.  This is primarily a result of the beryllium atom having:

1. more principal energy levels
2. greater electron-electron repulsion
3. more energy sublevels
4. greater nuclear charge

7.  Compared to the ionization energy of a magnesium atom, the ionization energy of a calcium atom is smaller.  This is primarily because the calcium atom:

1. has a greater nuclear charge than the magnesium atom
2. has fewer valence electrons than the magnesium atom
3. is larger than the magnesium atom
4. has more electron shielding than the magnesium atom

8.  Arrange the following elements in order of increasing ionization energy: S, O, Te, Se

9.  Arrange the following elements in order of decreasing ionization energy: Mg, Cl, Na, P

The following information on multiple ionizations is to be used for question 10.

Atoms can undergo multiple ionizations as they lose more electrons.  The energy required to lose additional electrons always increases.  The 2nd ionization energy (IE2) is always larger than the first ionization energy (IE1).  Likewise, IE3 is always greater than IE2.  Once all of the valence electrons have been removed, it is extremely difficult to remove any more electrons and the next ionization energy is way, way larger.

10.  A certain element’s first five ionization energies are listed below (in kJ/mol).

        IE1 = 578            IE2 = 1820        IE3 = 2750               IE4 = 11,600              IE5 = 14,800

Which is the most likely identity of this element?

1. sodium
2. magnesium
3. aluminum
4. silicon