Draw the Lewis structure of (CH3)2CHCH2CHO

Draw the Lewis structure of (CH3)2CHCH2CHO

Draw the Lewis structure of [CH3CH(OH2)CH2CH3]+

Draw the Lewis structure of CH3CH(CN)CH3

Draw the Lewis structure of [(CH3)2O(CH3)]+

fe3n2 oxidation number

The Correct Answer and Explanation is:

Sure! Let’s go through each part of your question in two sections:

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1. Lewis Structures

A. (CH₃)₂CHCH₂CHO

This is isovaleraldehyde, a five-carbon aldehyde. Its structure is:

        H   H   O
        |   |  ||
CH₃ — C — C — C — H
     |   |   |
    CH₃ H   H

Breakdown:

• Two CH₃ (methyl) groups attached to a CH (central carbon).
• That CH connects to a CH₂.
• CH₂ connects to a CHO (aldehyde).

Lewis structure:

• Each C makes 4 bonds.
• O in the aldehyde has a double bond with C and 2 lone pairs.
• H makes 1 bond.

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B. [CH₃CH(OH₂)CH₂CH₃]⁺

This is a protonated alcohol, specifically a protonated form of butanol.

Structure:

CH₃–CH(OH₂⁺)–CH₂–CH₃

Notes:

• OH₂⁺ means the oxygen has 3 bonds (to H, H, and carbon) and one lone pair.
• The molecule has an overall +1 charge centered on the oxygen.

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C. CH₃CH(CN)CH₃

This is 2-methylpropanenitrile.

Structure:

    CN
     |
CH₃–CH–CH₃

• CN is a nitrile group with a triple bond between carbon and nitrogen.
• N has a lone pair.
• Central carbon is bonded to two CH₃ groups and the CN group.

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D. [(CH₃)₂O(CH₃)]⁺

This is a trimethyloxonium ion, also written as (CH₃)₃O⁺.

Structure:

      +
     O
   / | \
CH₃ CH₃ CH₃

• O has three single bonds and no lone pairs, carrying a +1 charge.

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2. Fe₃N₂ – Oxidation Number Explanation

To find the oxidation number of iron (Fe) in Fe₃N₂ (iron(II) nitride), follow these steps:

Step-by-step:

1. Let the oxidation number of Fe be x.
2. Nitrogen (N) in nitrides almost always has an oxidation number of –3.
3. There are 2 nitrogen atoms: 2 × (–3) = –6
4. There are 3 Fe atoms: 3x

Set up the equation:

3x + (–6) = 0
=> 3x = +6
=> x = +2

✅ Answer: Iron (Fe) has an oxidation number of +2 in Fe₃N₂.

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Explanation (300+ words):

Oxidation numbers are used to determine how electrons are transferred or shared in compounds. In ionic compounds like Fe₃N₂, we assume that atoms exist as ions with integer oxidation states. Iron (Fe) and nitrogen (N) are both elements that can form multiple oxidation states, but in this case, we are dealing with a nitride compound.

Nitrogen is more electronegative than iron and typically forms a –3 oxidation state when bonded to metals, as seen in compounds like Li₃N and Mg₃N₂. This is because nitrogen needs three electrons to complete its octet and becomes N³⁻.

The formula Fe₃N₂ contains:

• 3 iron (Fe) atoms.
• 2 nitrogen (N) atoms.

If each nitrogen atom has a –3 oxidation state (N³⁻), the total negative charge from nitrogen is:

2 × (–3) = –6

To balance this charge in a neutral compound, the total positive charge from the iron atoms must be:

+6

Since there are 3 iron atoms, we divide:

+6 / 3 = +2

This tells us that each Fe atom has an oxidation number of +2. Thus, Fe₃N₂ is made up of three Fe²⁺ cations and two N³⁻ anions. This compound is therefore called iron(II) nitride, where the Roman numeral II reflects the +2 oxidation state of iron.

Understanding oxidation numbers is essential in predicting reactivity, identifying redox reactions, and naming compounds systematically.