Questions: Answer Bank

Answer Bank
Transcript text: Answer Bank
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Solution

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Solution Steps

Step 1: Determine the formal charge of Boron

The formal charge of an atom in a molecule is calculated as follows:

Formal charge = (Valence electrons) - (Non-bonding electrons) - (Bonding electrons)/2

Boron (B) has 3 valence electrons. In BH4, boron is bonded to four hydrogen atoms, meaning it has 8 bonding electrons (4 bonds * 2 electrons/bond) and 0 non-bonding electrons. Formal charge of B = 3 - 0 - 8/2 = 3 - 4 = -1

Step 2: Determine the formal charge of Hydrogen

Hydrogen (H) has 1 valence electron. In BH4, each hydrogen is bonded to the central boron atom, sharing 2 electrons in the bond. Each H has 0 non-bonding electrons. Formal charge of H = 1 - 0 - 2/2 = 1 - 1 = 0

Step 3: Determine the overall charge

The overall charge of the BH4 ion is the sum of the formal charges of all the atoms. Overall charge = (Formal charge of B) + 4 * (Formal charge of H) Overall charge = -1 + 4 * 0 = -1

Final Answer

\( \boxed{-1} \)

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