Oxidation States in Diborane

The video tutorial explains how to determine the oxidation numbers for each element in diborane (B2H6). It begins by noting that B2H6 is a neutral compound, meaning the sum of oxidation numbers is zero. The tutorial discusses hydrogen's typical oxidation state of +1 when bonded to non-metals, but highlights that when bonded to boron, a metalloid, hydrogen's oxidation state is -1 due to its higher electronegativity. The video then calculates the oxidation numbers, showing that hydrogen is -1 and boron is +3, ensuring the sum is zero. The tutorial concludes with a summary of these findings.

What is the total sum of oxidation numbers in a neutral compound like diborane?

• It is always zero.

• It is always positive.

• It varies depending on the compound.

• It is always negative.

What is the typical oxidation state of hydrogen when bonded to non-metals?

• 0

• +2

• -1

• +1

Why is hydrogen assigned a negative oxidation state when bonded to boron?

• Because hydrogen is more electronegative.

• Because boron is a metal.

• Because boron is more electronegative.

• Because they have equal electronegativity.

What is the oxidation number of hydrogen in diborane (B2H6)?

• 0

• -1

• +1

• +2

How many hydrogen atoms are present in diborane (B2H6)?

• 8

• 2

• 4

• 6

What is the oxidation number of boron in diborane (B2H6)?

• +2

• +3

• +1

• 0

How does the oxidation number of boron ensure the neutrality of diborane?

• By being negative.

• By being zero.

• By being positive.

• By being equal to hydrogen's oxidation number.

What is the total oxidation number contributed by hydrogen atoms in diborane?

• -3

• -6

• +6

• 0

What is the sum of the oxidation numbers of boron atoms in diborane?

• 0

• +6

• +3

• -6