Cations, Anions, and Ionic Stability

The video tutorial explains the differences between atoms and ions, focusing on how elements like sodium, magnesium, Florine, and sulfur achieve stability through electron gain or loss. It covers the concept of valence electrons and the formation of cations and anions, highlighting the naming conventions for non-metal ions. The tutorial provides examples to illustrate the transformation from neutral atoms to charged ions.

What is a characteristic of alkaline metals regarding their valence electrons?

• They have a full valence shell.

• They have one valence electron.

• They have no valence electrons.

• They have two valence electrons.

What is the most energetically favorable action for sodium to achieve stability?

• Gain one electron

• Lose one electron

• Gain seven electrons

• Lose seven electrons

How many electrons does magnesium lose to become stable?

• Four

• Three

• Two

• One

What happens to fluorine when it gains an electron?

• It becomes positively charged.

• It becomes a cation.

• It becomes negatively charged.

• It loses its charge.

What is the charge of sulfur after gaining two electrons?

• Plus two

• Minus two

• Plus one

• Minus one

What is the main difference between a sodium atom and a sodium ion?

• The sodium ion has more electrons.

• The sodium ion has a positive charge.

• The sodium atom has more protons.

• The sodium atom has a negative charge.

What happens to magnesium when it loses two electrons?

• It remains neutral.

• It becomes a magnesium ion.

• It gains a negative charge.

• It becomes a magnesium atom.

What is a cation?

• An ion with no charge

• An ion with a negative sign

• A positively charged ion

• A negatively charged ion

How can you remember that cations are positively charged?

• The letter 'C' looks like a plus sign.

• The letter 'A' in cation stands for 'add'.

• The letter 'T' in cation looks like a plus sign.

• The letter 'I' in cation stands for 'increase'.

What is the naming convention for non-metal ions?

• They end with 'ous'.

• They end with 'ide'.

• They end with 'ate'.

• They end with 'ium'.