Periodic Trends in Atomic Properties

The video tutorial explains the trends and exceptions in ionization energy, electron affinity, and atomic radius across the periodic table. It highlights how ionization energy generally increases across a period but has exceptions like oxygen. Electron affinity trends are discussed with nitrogen as an exception. The atomic radius is explained to decrease across a period due to increased nuclear attraction, while it increases down a group due to added energy levels.

What happens to ionization energy as you move across period 2 of the periodic table?

• It fluctuates randomly.

• It increases.

• It decreases.

• It remains constant.

Why is it easier to remove an electron from oxygen compared to nitrogen?

• Oxygen has a double occupancy in its 2p orbital.

• Oxygen is a noble gas.

• Oxygen has a lower atomic number.

• Oxygen has a full outer shell.

What is electron affinity?

• The energy released when an atom loses a neutron.

• The energy required to add a proton.

• The energy released when an atom gains an electron.

• The energy required to remove an electron.

Why does nitrogen have a lower electron affinity than expected?

• It has a half-filled 2p orbital.

• It prefers to lose electrons.

• It has a full outer shell.

• It is a noble gas.

Which group in the periodic table is known for bucking the trend in ionization energy?

• Group 14

• Group 15

• Group 16

• Group 17

Which group in the periodic table is known for bucking the trend in electron affinity?

• Group 14

• Group 15

• Group 17

• Group 16

What happens to the atomic radius as you move across a period?

• It increases.

• It fluctuates randomly.

• It decreases.

• It remains constant.

Why does the atomic radius decrease across a period?

• The number of protons decreases.

• The number of energy levels increases.

• The attractive force on electrons increases.

• The atomic mass decreases.

What is the trend in atomic radius as you move down a group?

• It increases.

• It remains constant.

• It decreases.

• It fluctuates randomly.

Why does the atomic radius increase as you move down a group?

• The atomic mass decreases.

• The number of energy levels increases.

• The number of protons decreases.

• The attractive force on electrons increases.