Ions, light, periodic trends

Question 1

Define atomic radius and explain its trends on the periodic table.

Answer 1

Atomic radius defines the size of an atom. Size increases as you go down a group due to additional energy levels, and decreases left to right across a period due to the greater effective nuclear charge.

Question 2

Define electronegativity and its trends on the periodic table.

Answer 2

Electronegativity is a measure of how strongly atoms attract bonding electrons to themselves. Electronegativity decrease as you go down a group due to the additional energy levels and increased shielding affect. It increases as you go left to right across a period due to the greater effective nuclear charge and a decrease in the distance between the nucleus and outer electrons

Question 3

Define ionization energy and its trends on the periodic table.

Answer 3

Ionization energy is the amount of energy that it takes to remove an electron from a gaseous atom or ion.

Question 4

Define effective nuclear charge and explain its trends on the periodic table.

Answer 4

Effective nuclear charge is the amount of positive energy experienced by the electrons within an atom. Effective nuclear charge decreases as you go down a group, as the shielding effect counteracts the number of protons in the nucleus. The effective nuclear charge increases as you go from left to right across a period, as there are additional protons added to the nucleus, but no additional energy levels.