Single Replacement Reactions Concepts

The video tutorial explains how to determine if a single replacement reaction will occur by using the activity series of metals and the periodic table for halogens. It provides examples of reactions involving lithium, magnesium, iron, and halogens, demonstrating how to predict whether a reaction will take place. The tutorial concludes with the importance of balancing chemical equations after predicting reactions.

What is the primary tool used to predict if a single replacement reaction will occur?

• Molecular Weight

• Activity Series

• Chemical Formula

• Periodic Table

In a single replacement reaction, if the lone metal is higher in the activity series than the metal in the compound, what will happen?

• No reaction will occur

• The metals will form an alloy

• The compound will decompose

• The lone metal will replace the metal in the compound

Which metal can replace hydrogen in a single replacement reaction?

• Gold

• Magnesium

• Silver

• Copper

When iron replaces copper in a reaction, what compound is formed?

• Copper Chloride

• Iron Sulfate

• Iron Nitrate

• Copper Oxide

Which halogen is more reactive and can replace iodine in a compound?

• Fluorine

• Astatine

• Chlorine

• Bromine

What happens if bromine tries to replace fluorine in a compound?

• Bromine will replace fluorine

• A new compound will form

• No reaction will occur

• Fluorine will form a diatomic molecule

What should you write if a single replacement reaction does not occur?

• NR

• No Reaction

• X

• None

What is the next step after predicting a reaction will occur?

• Balance the chemical equation

• Measure the reactants

• Write the chemical formula

• Heat the mixture

Which of the following is NOT a factor in predicting single replacement reactions?

• Activity Series

• Position in the Periodic Table

• Color of the metal

• Reactivity of halogens

Why is it important to balance chemical equations after predicting a reaction?

• To change the products formed

• To ensure the reaction is safe

• To comply with the law of conservation of mass

• To make the reaction faster