Shielding and Effective Nuclear Charge

Shielding electrons causes the force of attraction to the nucleus to 

• increase

• decrease

The effective nuclear charge is _____ the actual nuclear charge

• equal to

• less than

• greater than

Tags

NGSS.HS-PS1-8

Choose the answer choice that best describes why cations are smaller than the parent atoms.

• cations lose electron(s) resulting in more protons than electrons. Zeff increases

• cations gain electron(s) resulting in more electrons than protons. Zeff decreases

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

As you move down a family on the periodic table, the increase in atomic radius can be explained by the ___.

• increase in number of shielding electrons

• increase in effective nuclear charge

• decrease in number of shielding electrons

• decrease in effective nuclear charge

What is the effective nuclear charge of a valence electron in the Al⁺ cation?

• 2

• 3

• 12

• 13

What is the effect of shielding on the effective nuclear charge experienced by outer electrons?

• Increases the effective nuclear charge

• Decreases the effective nuclear charge

• Has no effect on the effective nuclear charge

• Doubles the effective nuclear charge

Which of the following best explains why the effective nuclear charge is less than the actual nuclear charge?

• Presence of inner-shell electrons

• Absence of inner-shell electrons

• Increase in atomic radius

• Decrease in atomic radius

How does the effective nuclear charge change as you move across a period in the periodic table?

• Increases

• Decreases

• Remains constant

• First increases, then decreases

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which factor contributes to the shielding effect in an atom?

• Valence electrons

• Core electrons

• Protons

• Neutrons

What happens to the effective nuclear charge when an electron is added to the outer shell of an atom?

• Increases

• Decreases

• Remains the same

• Doubles

Tags

NGSS.HS-PS1-1