Bromine and Tin Compounds

This video tutorial explains how to determine the oxidation number of tin in tin(IV) bromide (SnBr4). It begins by introducing the concept of oxidation numbers and the neutrality of compounds. The video then discusses tin as a transition metal and bromine's typical oxidation state. It proceeds to calculate the oxidation numbers, showing that bromine has a -1 oxidation state, and with four bromine atoms, the total is -4. Therefore, tin must have a +4 oxidation state to balance the compound to zero. The video concludes by summarizing the findings.

What is the overall charge of the compound SnBr4?

• Depends on the environment

• Neutral

• Negative

• Positive

Which group on the periodic table does bromine belong to?

• Group 12

• Group 3

• Group 17

• Group 1

What is the oxidation number of a single bromine atom in SnBr4?

• -1

• -2

• 0

• +1

How many bromine atoms are present in SnBr4?

• 2

• 3

• 4

• 5

What must be the oxidation number of tin in SnBr4 to balance the compound?

• +2

• +3

• +4

• +5

Why is SnBr4 named tin(IV) bromide?

• Because tin is in group 4

• Because the compound has four bromine atoms

• Because bromine has an oxidation number of +4

• Because tin has an oxidation number of +4