Sodium Electron Configuration Concepts

The video tutorial explains how to write the electron configuration and atomic orbital diagram for sodium. It begins by identifying sodium on the periodic table and determining its atomic number and electron count. The tutorial then guides viewers through writing the electron configuration using the periodic table, detailing each step and energy level. Following this, the video transitions to constructing the atomic orbital diagram, illustrating how electrons are placed in energy levels around the nucleus. The tutorial concludes with a visual representation of the atomic orbital diagram for sodium.

What is the first step in writing the atomic orbital diagram for sodium?

• Identify the number of neutrons

• Write the electron configuration

• Determine the atomic mass

• Find the melting point

How many electrons does sodium have?

• 13

• 12

• 11

• 10

Which of the following is the correct electron configuration for sodium?

• 1s2 2s2 2p6 3s1

• 1s2 2s2 2p5 3s2

• 1s2 2s2 2p6 3p1

• 1s2 2p6 3s2

What is the significance of the 3s1 in sodium's electron configuration?

• It represents a pair of electrons

• It shows the presence of a lone electron in the 3s orbital

• It signifies an empty orbital

• It indicates a full shell

In the atomic orbital diagram, how are electrons represented?

• As numbers

• As arrows

• As lines

• As dots

What is the purpose of spreading out electrons in the 2p orbital before pairing them?

• To balance the nucleus

• To fill the 3s orbital first

• To maximize energy

• To minimize energy

How is the atomic orbital diagram for sodium sometimes represented?

• Vertically

• Horizontally

• Diagonally

• In a circular pattern

What does the atomic orbital diagram visually represent?

• The number of protons

• The chemical reactivity

• The arrangement of electrons around the nucleus

• The atomic mass

Which energy level is filled after 2p6 in sodium's electron configuration?

• 3p

• 1s

• 2s

• 3s

What is the atomic number of sodium?

• 10

• 11

• 12

• 13