Oxidation Numbers in Compounds

The video tutorial covers the concept of oxidation numbers, starting with the rules for assigning oxidation numbers to pure elements, such as sodium and oxygen. It explains the role of electronegativity in binary and ionic compounds, highlighting the positions of cations and anions. The tutorial discusses fluorine's consistent oxidation number due to its high electronegativity and explores periodic trends. It also covers the oxidation numbers of oxygen, including exceptions like peroxides, and hydrogen, depending on its bonding partners. The video concludes with the algebraic sum of oxidation numbers in compounds and polyatomic ions.

What is the oxidation number of an atom in its pure elemental form?

• 0

• +2

• -1

• +1

In a binary compound, which element is assigned a negative oxidation number?

• The element with a larger atomic radius

• The more electronegative element

• The element with a smaller atomic radius

• The less electronegative element

What is the oxidation number of fluorine in all its compounds?

• +2

• -1

• 0

• +1

What is the typical oxidation number of oxygen in most compounds?

• -2

• 0

• -1

• +1

In which type of compound does oxygen have an oxidation number of -1?

• Sulfides

• Fluorides

• Peroxides

• Oxides

What is the oxidation number of oxygen in compounds with fluorine?

• -2

• -1

• +2

• 0

What is the oxidation number of hydrogen when it is bonded to a metal?

• +2

• -1

• +1

• 0

What is the algebraic sum of oxidation numbers in a neutral compound?

• 0

• -1

• +2

• +1

Which of the following is true for the oxidation number of hydrogen in compounds with nonmetals?

• It is +1

• It is 0

• It varies

• It is -1

What is the oxidation number of a monatomic ion?

• Always -1

• Always +1

• Always zero

• Equal to the charge of the ion