Atomic Structure and Effective Nuclear Charge

The video tutorial explains how atomic size varies in the periodic table. It describes that atomic size decreases across a period due to increased nuclear charge, which pulls electrons closer to the nucleus. Conversely, atomic size increases down a group because additional electron shells outweigh the increase in nuclear charge, leading to a larger atomic radius. The tutorial also highlights the concept of effective nuclear charge and its impact on atomic size.

What is the primary reason for the decrease in atomic size across a period?

• Decrease in electron shells

• Increase in nuclear charge

• Increase in electron shells

• Decrease in nuclear charge

Why does atomic size increase as you move down a group?

• Decrease in nuclear charge

• Decrease in electron shells

• Increase in nuclear charge

• Addition of extra electron shells

What effect does the addition of electron shells have on atomic size down a group?

• It has no effect on atomic size

• It decreases atomic size

• It stabilizes atomic size

• It increases atomic size

Which factor outweighs the increase in nuclear charge down a group?

• Increase in atomic mass

• Decrease in electron shells

• Decrease in atomic mass

• Increase in electron shells

How does the effective nuclear charge affect atomic radius across a period?

• It has no effect on atomic radius

• It increases the atomic radius

• It stabilizes the atomic radius

• It decreases the atomic radius

What happens to the outermost electron as the effective nuclear charge increases across a period?

• It moves to a higher energy level

• It remains unaffected

• It becomes more attached to the nucleus

• It becomes less attached to the nucleus

What is the effect of having more electrons in the same number of shells across a period?

• It has no effect on the effective nuclear charge

• It increases the effective nuclear charge

• It decreases the effective nuclear charge

• It stabilizes the effective nuclear charge