Redox Reactions and Metal Reactivity

The video tutorial by Mr. Donnie covers redox reactions, focusing on metal activity and spontaneity. It explains how metals react based on their position in the reactivity series, using examples like magnesium and copper. The tutorial also explores reactions with acids and predicts reaction outcomes based on metal activity. It concludes with a discussion on non-reactive metals that resist corrosion in acids.

What is the primary process occurring in a redox reaction?

• Atoms are gaining protons.

• Electrons are being transferred.

• Neutrons are being exchanged.

• Atoms are losing protons.

Which metal is more reactive according to the activity series?

• Gold

• Potassium

• Copper

• Platinum

In a reaction between magnesium and copper ions, what happens to magnesium?

• It remains unchanged.

• It gains electrons.

• It forms a compound with copper.

• It loses electrons.

What is the role of the activity series in predicting reactions?

• It determines the color change in reactions.

• It predicts the temperature change in reactions.

• It helps predict which metal will be oxidized.

• It shows the pH level of the reaction.

What happens to the charge of copper when it gains electrons?

• It becomes more positive.

• It becomes neutral.

• It becomes more negative.

• It remains unchanged.

What is the charge of magnesium after it loses two electrons?

• +1

• +2

• 0

• -2

Why does magnesium react with acids?

• Because it is less reactive than hydrogen.

• Because it is more reactive than hydrogen.

• Because it is neutral.

• Because it is a noble gas.

Which metal will not react with acids due to its low reactivity?

• Zinc

• Gold

• Magnesium

• Iron

Which of the following metals is least likely to corrode in an acid bath?

• Zinc

• Iron

• Copper

• Sodium

Why are metals like gold used for currency?

• They are less active than hydrogen.

• They are lightweight.

• They are highly reactive.

• They are abundant.