Oxidation States and Compounds

The video tutorial explains how to determine the oxidation numbers for each element in the compound NaBrO4, known as sodium perbromate. It begins by stating that the compound is neutral, meaning the oxidation numbers must sum to zero. Sodium, being in group 1, has a +1 oxidation state. Bromine, typically -1, is unknown here due to its bond with oxygen. Oxygen is almost always -2. Using these rules, an equation is set up to solve for bromine's oxidation number, which is found to be +7. The tutorial concludes with a recap of the process.

What is the oxidation number of sodium in NaBrO4?

• +2

• 0

• -1

• +1

In which group is bromine found on the periodic table?

• Group 1

• Group 17

• Group 18

• Group 2

What is the usual oxidation state of oxygen in compounds?

• +2

• -1

• -2

• 0

How many oxygen atoms are present in NaBrO4?

• 2

• 3

• 4

• 5

What is the total oxidation number contributed by the oxygen atoms in NaBrO4?

• -8

• -10

• -6

• -4

What is the oxidation number of bromine in NaBrO4?

• +7

• +6

• +5

• +8

Why does the oxidation number of bromine in NaBrO4 differ from its usual state?

• Because it is in a charged compound

• Because it is in a neutral compound

• Because it is bonded to sodium

• Because it is bonded to oxygen

What is the sum of all oxidation numbers in a neutral compound like NaBrO4?

• 0

• +1

• +2

• -1