Alkali Metals and Atomic Structure

The video tutorial introduces chemical families, focusing on the periodic table's groupings and the characteristics of alkali metals. It explains how elements are classified into groups and periods based on valence electrons and energy levels. The tutorial covers the four main chemical families: alkali metals, alkaline earth metals, halogens, and noble gases. It delves into the electron configuration of alkali metals and discusses trends in atomic and ionic radii, emphasizing the increase in occupied energy levels down the group.

What determines the classification of elements into groups in the periodic table?

• Number of protons

• Number of neutrons

• Number of valence electrons

• Atomic mass

Which of the following is NOT a member of the alkali metals?

• Calcium

• Sodium

• Potassium

• Lithium

What is the electron configuration of sodium?

• 2, 8, 2

• 2, 8, 8

• 2, 8, 1

• 2, 8, 7

Why are alkali metals considered monovalent?

• They have one electron in their outermost energy level.

• They have two electrons in their outermost energy level.

• They have a full outer shell.

• They gain one electron to become stable.

What happens to the number of occupied energy levels as you move down the group of alkali metals?

• It remains the same

• It increases

• It fluctuates

• It decreases

What is the atomic radius?

• The distance between the nucleus and the innermost energy level

• The distance between two electrons

• The distance between the center of the nucleus and the outermost energy level

• The distance between two nuclei

How does the atomic radius of alkali metals change down the group?

• It first increases then decreases

• It increases

• It remains constant

• It decreases

Why is the atomic radius of an alkali metal larger than its ionic radius?

• Because the atom has more protons

• Because the ion loses an electron

• Because the ion gains an electron

• Because the atom has fewer neutrons

What is the electron configuration of a sodium ion?

• 2, 8

• 2, 7

• 2, 8, 1

• 2, 8, 2

What is the main reason for the difference in size between sodium atoms and sodium ions?

• Sodium ions have more protons

• Sodium ions have fewer occupied energy levels

• Sodium atoms have fewer electrons

• Sodium atoms have more neutrons