Ion Formation and Reactivity Concepts

This video tutorial from KET Labs explains how to predict ion formation using the periodic table and valence electrons. It covers examples of sodium, magnesium, oxygen, and fluorine, illustrating how atoms gain or lose electrons to form ions. The tutorial also discusses the role of the periodic table in predicting ion charges and highlights the stability of noble gases due to their full valence shells.

What is the primary factor that determines how an atom will form an ion?

• The atomic mass of the element

• The number of valence electrons

• The number of neutrons in the nucleus

• The number of protons in the nucleus

Why is sodium considered highly reactive?

• It has a full outer shell of electrons

• It easily loses its single valence electron

• It is a noble gas

• It has a high atomic mass

What happens to sodium when it forms an ion?

• It gains two electrons

• It gains one electron

• It loses one electron

• It loses two electrons

How many electrons does magnesium lose to form an ion?

• None

• Three

• Two

• One

What is the charge of a magnesium ion after it loses electrons?

• 2-

• 1-

• 2+

• 1+

How does oxygen achieve a full valence shell?

• By losing one electron

• By gaining two electrons

• By losing two electrons

• By gaining one electron

What is the charge of an oxygen ion after it gains electrons?

• 2-

• 2+

• 1+

• 1-

What is the primary goal of atoms when forming ions?

• To become a noble gas

• To decrease atomic number

• To achieve a full valence shell

• To increase atomic mass

Why do noble gases not form ions?

• They are highly reactive

• They have no valence electrons

• They have a high atomic mass

• They have a full valence shell

How can the periodic table help predict ion formation?

• By indicating the number of valence electrons

• By displaying the element's color

• By showing the atomic mass

• By listing the atomic number