Question

periodic trends practice problems: ionization energy

1. define ionization energy.
2. rank the following elements by increasing ionization energy (period 5): indium, antimony, tin, iodine.
3. rank the following elements by increasing ionization energy (period 4): nickel, manganese, bromine, potassium
4. rank the following elements by increasing ionization energy (group 4a): lead, carbon, germanium, tin
5. rank the following elements by decreasing ionization energy (group 2a): calcium, magnesium, strontium, barium.
6. rank the following elements by decreasing ionization energy (period 6a): gold, bismuth, osmium, cesium
7. describe the trend for ionization energy as you move from top to bottom within a group on the periodic table. why is this the case?

name:
period:

1. describe the trend for ionization energy as you move from left to right within a period on the periodic table. why is this the case?

a chlorine

Explanation:

1. Ionization energy is the energy required to remove an electron from a gaseous atom or ion.
2. In period 5, the order of increasing ionization energy is indium < tin < antimony < iodine as ionization energy generally increases across a period.
3. In period 4, the order is potassium < manganese < nickel < bromine as the trend across a period is an increase in ionization energy with some exceptions due to electron - configuration.
4. In group 4A, the order of increasing ionization energy is lead < tin < germanium < carbon as ionization energy decreases down a group.
5. In group 2A, the order of decreasing ionization energy is barium > strontium > calcium > magnesium as ionization energy decreases down a group.
6. In period 6A, the order of decreasing ionization energy is cesium > bismuth > osmium > gold as metals have lower ionization energies than non - metals in the same period.
7. As you move from top to bottom within a group on the periodic table, ionization energy decreases. This is because the outermost electrons are farther from the nucleus and are shielded by more inner electrons, making them easier to remove.
8. As you move from left to right within a period on the periodic table, ionization energy generally increases. This is because the nuclear charge increases while the shielding effect remains relatively constant, resulting in a stronger attraction for the outermost electrons.

Answer:

1. The energy required to remove an electron from a gaseous atom or ion.
2. Indium, tin, antimony, iodine.
3. Potassium, manganese, nickel, bromine.
4. Lead, tin, germanium, carbon.
5. Barium, strontium, calcium, magnesium.
6. Cesium, bismuth, osmium, gold.
7. Ionization energy decreases. Outermost electrons are farther and more shielded.
8. Ionization energy increases. Nuclear charge increases with constant shielding.