Exploring Atomic Structure

What is the electron configuration of oxygen?

• 1s² 2s² 2p⁴

• 1s² 2s¹ 2p⁴

• 1s² 2s² 2p³

• 1s² 2s² 2p⁶

How many electrons can the s orbital hold?

• 3

• 1

• 8

• 2

What is the shape of the p orbital?

• Cylindrical shape

• Dumbbell shape

• Spherical shape

• Flat shape

Describe the trend in atomic radius across a period.

• The atomic radius remains constant across a period.

• The atomic radius fluctuates randomly across a period.

• The atomic radius decreases across a period.

• The atomic radius increases across a period.

What is the electron configuration for a sodium ion (Na+)?

• 1s² 2s² 2p⁵

• 1s² 2s² 2p⁶

• 1s² 2s² 2p⁶ 3s¹

• 1s² 2s² 2p⁶ 3p⁶

Which element has the highest electronegativity?

• Carbon

• Nitrogen

• Fluorine

• Oxygen

Explain the concept of hybridization in atomic orbitals.

• Hybridization refers to the separation of atomic orbitals.

• Hybridization is the process of ionization in atoms.

• Hybridization involves the loss of electrons from atomic orbitals.

• Hybridization is the mixing of atomic orbitals to create new hybrid orbitals for bonding.

What is the maximum number of electrons in the d orbital?

• 8

• 12

• 10

• 6

How does ionization energy change down a group?

• Ionization energy increases down a group.

• Ionization energy remains constant down a group.

• Ionization energy fluctuates randomly down a group.

• Ionization energy decreases down a group.

What is the electron configuration of a chlorine atom?

• 1s² 2s² 2p⁶ 3s² 3p³

• 1s² 2s² 2p⁶ 3s² 3p⁵

• 1s² 2s² 2p⁶ 3s² 3p⁶

• 1s² 2s² 2p⁶ 3s² 3p⁴