Understanding Oxygen and Electron Configuration

The video tutorial explains how to write the electron configuration for the oxide ion (O2-). It begins by detailing the electron configuration for neutral oxygen, emphasizing that elements on the periodic table are neutral, meaning their atomic number equals the number of protons and electrons. The tutorial then guides viewers through writing the electron configuration for oxygen using orbitals, resulting in 1s2 2s2 2p4. To find the configuration for the oxide ion, two electrons are added, resulting in 1s2 2s2 2p6, a stable configuration with a full valence shell. This stability is why oxygen gains electrons to form ionic bonds.

What does it mean for an element to be neutral on the periodic table?

• It has more electrons than protons.

• It has an equal number of protons and electrons.

• It has no electrons.

• It has more protons than electrons.

How many electrons does a neutral oxygen atom have?

• 12

• 10

• 8

• 6

Which orbital is filled first when writing the electron configuration for oxygen?

• 1s

• 3s

• 2s

• 2p

What is the electron configuration for a neutral oxygen atom?

• 2s2 2p4

• 1s2 2s2 2p4

• 1s2 2s2 2p6

• 1s2 2p4

How many additional electrons does the oxide ion (O2-) have compared to neutral oxygen?

• 2

• 3

• 4

• 1

What is the electron configuration for the oxide ion (O2-)?

• 1s2 2s2 2p4

• 1s2 2s2 2p6

• 1s2 2p6

• 2s2 2p6

Why is the electron configuration of the oxide ion considered stable?

• It has no electrons.

• It has more protons than electrons.

• It has an equal number of protons and electrons.

• It has a full outer shell of electrons.

How many valence electrons does the oxide ion have?

• 12

• 10

• 8

• 6

What happens to oxygen when it forms ionic bonds?

• It gains one electron.

• It loses one electron.

• It gains two electrons.

• It loses two electrons.

What is the significance of a full valence shell in the oxide ion?

• It makes the ion stable.

• It makes the ion highly reactive.

• It makes the ion neutral.

• It makes the ion unstable.