Oxidation Numbers and Transition Metals

The video tutorial explains how to determine oxidation numbers for transition metals in compounds. It covers general rules for finding oxidation numbers, including the importance of knowing the charges of elements and polyatomic ions. The tutorial provides examples with iron, copper, and manganese, demonstrating how to set up equations to solve for unknown oxidation numbers. It emphasizes the need to understand polyatomic ions and offers additional resources for further learning.

What characteristic of transition metals makes it necessary to consider their bonding when determining oxidation numbers?

• They have variable charges.

• They have fixed charges.

• They do not form compounds.

• They are always neutral.

In a neutral compound, what should the sum of all oxidation numbers equal?

• Zero.

• The charge of the most electronegative element.

• The number of atoms in the compound.

• The atomic number of the central atom.

What is the usual oxidation number for chlorine in compounds?

• -1

• 0

• +1

• +2

When dealing with polyatomic ions, what must the sum of the oxidation numbers equal?

• Zero.

• The charge of the ion.

• The atomic mass of the ion.

• The number of atoms in the ion.

In the compound Cu2O, what is the oxidation number of copper?

• 0

• +1

• +2

• -1

What is the oxidation number of manganese in the permanganate ion?

• +6

• +4

• +7

• +2

In the permanganate ion, what is the oxidation number of each oxygen atom?

• +1

• 0

• -2

• -1

For the compound with chromium, what is the oxidation number of each chromium atom?

• +3

• +6

• +4

• +2

What is the charge on the ion in the final example involving chromium?

• -2

• +1

• -1

• 0

What is the general rule for the sum of oxidation numbers in an ion?

• It equals the number of electrons.

• It equals zero.

• It equals the charge of the ion.

• It equals the atomic number of the central atom.