Electron Configuration of Potassium Ion (K+)

The video tutorial explains how to write the electron configuration for a potassium ion (K+). It begins by detailing the electron configuration for neutral potassium, using the periodic table to distribute 19 electrons across various orbitals. The tutorial then transitions to the potassium ion, explaining that it loses one electron to form K+, resulting in a stable electron configuration similar to argon. The video emphasizes the stability of a full outer electron shell and concludes with a brief summary of the process.

What is the first step in writing the electron configuration for the potassium ion (K+)?

• Identify the element's position in the periodic table.

• Count the number of neutrons.

• Directly write the configuration for K+.

• Write the electron configuration for neutral potassium.

Why are elements on the periodic table considered neutral?

• They have a full outer shell.

• They have no charge.

• They have an equal number of protons and electrons.

• They have an equal number of protons and neutrons.

What is the atomic number of potassium?

• 21

• 18

• 19

• 20

How many electrons does a neutral potassium atom have?

• 18

• 21

• 20

• 19

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

• 2s

• 2p

• 1s

• 3s

How many electrons can the 2p orbital hold?

• 6

• 4

• 8

• 2

What is the electron configuration for neutral potassium?

• 1s2 2s2 2p6 3s2 3p6

• 1s2 2s2 2p6 3s2 3p6 4s2

• 1s2 2s2 2p6 3s2 3p6 4s1

• 1s2 2s2 2p6 3s2 3p6 4p1

What happens to the electron configuration when potassium forms a K+ ion?

• It gains an electron.

• It loses an electron.

• It gains a proton.

• It loses a proton.

What is the electron configuration for the potassium ion (K+)?

• 1s2 2s2 2p6 3s2 3p6

• 1s2 2s2 2p6 3s2 3p6 4s2

• 1s2 2s2 2p6 3s2 3p6 4s1

• 1s2 2s2 2p6 3s2 3p5

Why is the electron configuration of K+ considered stable?

• It has fewer electrons than protons.

• It has an equal number of protons and electrons.

• It has a full outer shell.

• It has more electrons than protons.