Understanding the Shielding Effect

What is the shielding effect in an atom?

• The attraction between the nucleus and the outermost electrons.

• The repulsion between electrons in different energy levels.

• The reduction in effective nuclear charge on the electron cloud, due to a difference in the attraction forces of electrons in different shells.

• The increase in atomic size due to additional electron shells.

How does the shielding effect influence the atomic size of an element?

• It decreases the atomic size by increasing the effective nuclear charge.

• It has no impact on the atomic size.

• It increases the atomic size by reducing the effective nuclear charge.

• It decreases the atomic size by reducing the number of electron shells.

Which of the following statements best describes the role of the shielding effect in ionisation energy?

• The shielding effect increases ionisation energy by increasing the effective nuclear charge.

• The shielding effect decreases ionisation energy by reducing the effective nuclear charge.

• The shielding effect has no impact on ionisation energy.

• The shielding effect increases ionisation energy by decreasing the atomic size.

Which of the following factors contributes to a stronger shielding effect?

• A higher number of protons in the nucleus.

• A higher number of electron shells.

• A higher number of neutrons in the nucleus.

• A higher number of electrons in the outermost shell.

In which of the following elements would you expect the shielding effect to be the greatest?

• Hydrogen (H)

• Helium (He)

• Sodium (Na)

• Neon (Ne)

What is the meaning of amphoteric?

• capable of reacting chemically either as an acid or as a base

• capable of acting as a base with Halogens

• capable of acting as an acid with Halogens

• capable of acting as a Noble Gas

Electronegativity is .....

• a measure of an atom's ability to attract electrons in a chemical bond.
• a measure of an atom's size in a molecule.
• a measure of an atom's temperature in a reaction.
• a measure of an atom's mass in a chemical reaction.

Electronegativity trends across the periodic table can be described as:

• Electronegativity increases across a period and decreases down a group.
• Electronegativity increases down a group and decreases across a period.
• Electronegativity remains constant across a period and down a group.
• Electronegativity decreases across a period and increases down a group.

How does electronegativity affect bonding?

• Electronegativity affects bonding by determining the type of bond (covalent, polar covalent, or ionic) based on the difference in electronegativity between the atoms.
• Electronegativity determines the color of the bond.
• Electronegativity only influences the size of atoms.
• Electronegativity has no effect on bonding.

Using Aufbaus principle, what is the electronic configuration of Vanadium?

• [Ar] 4s² 3d³
• [Ar] 4s¹ 3d⁵
• [Ar] 4s² 3d⁴
• [Ar] 4s² 3d²