Geometry, indicate the molecular shape, determine hybridization, and determine if polar/nonpolar,

geometry, indicate the molecular shape, determine hybridization, and determine if polar/nonpolar,

A. NH₄⁺
B. H₂NF₂⁺
C. HCO₃^–
D. CO₃^2-
E. NO₃^–
F. NO₂^–
G. SO₄^2-
H. SO₃^2-
I. SO₃
J. SO₂
K. PO₄^3-
L. PO₃^3-

For the following polyatomic ions and compounds with varying numbers of oxygens, draw the correct Lewis structure, indicate electron pair geometry, indicate the molecular shape, determine hybridization, and determine if polar/nonpolar,

The Correct Answer and Explanation is:

A. NH₄⁺ (Ammonium)

Lewis Structure: N single bonded to four H, one positive charge.
Electron Pair Geometry: Tetrahedral
Molecular Shape: Tetrahedral
Hybridization: sp³
Polarity: Nonpolar

B. H₂NF₂⁺

Lewis Structure: N central, bonded to 2 H and 2 F, one positive charge.
Electron Pair Geometry: Tetrahedral
Molecular Shape: Bent (due to lone pair on N)
Hybridization: sp³
Polarity: Polar

C. HCO₃⁻ (Bicarbonate)

Lewis Structure: Central C bonded to OH and two O atoms (one with a double bond), one negative charge.
Electron Pair Geometry: Trigonal planar
Molecular Shape: Trigonal planar
Hybridization: sp²
Polarity: Polar

D. CO₃²⁻ (Carbonate)

Lewis Structure: C central, bonded to three O atoms, resonance structure, two negative charges.
Electron Pair Geometry: Trigonal planar
Molecular Shape: Trigonal planar
Hybridization: sp²
Polarity: Nonpolar

E. NO₃⁻ (Nitrate)

Lewis Structure: N central, bonded to 3 O atoms, one with double bond, resonance, one negative charge.
Electron Pair Geometry: Trigonal planar
Molecular Shape: Trigonal planar
Hybridization: sp²
Polarity: Nonpolar

F. NO₂⁻ (Nitrite)

Lewis Structure: N bonded to 2 O atoms, one lone pair, one negative charge.
Electron Pair Geometry: Trigonal planar
Molecular Shape: Bent
Hybridization: sp²
Polarity: Polar

G. SO₄²⁻ (Sulfate)

Lewis Structure: S central, four O atoms (two with double bonds), two negative charges.
Electron Pair Geometry: Tetrahedral
Molecular Shape: Tetrahedral
Hybridization: sp³
Polarity: Nonpolar

H. SO₃²⁻ (Sulfite)

Lewis Structure: S central, three O atoms, one lone pair on S, two negative charges.
Electron Pair Geometry: Tetrahedral
Molecular Shape: Trigonal pyramidal
Hybridization: sp³
Polarity: Polar

I. SO₃ (Sulfur Trioxide)

Lewis Structure: S central, three double-bonded O atoms (resonance).
Electron Pair Geometry: Trigonal planar
Molecular Shape: Trigonal planar
Hybridization: sp²
Polarity: Nonpolar

J. SO₂ (Sulfur Dioxide)

Lewis Structure: S central, two double bonds to O, one lone pair on S.
Electron Pair Geometry: Trigonal planar
Molecular Shape: Bent
Hybridization: sp²
Polarity: Polar

K. PO₄³⁻ (Phosphate)

Lewis Structure: P central, four O atoms, three with single bonds, one with double, three negative charges.
Electron Pair Geometry: Tetrahedral
Molecular Shape: Tetrahedral
Hybridization: sp³
Polarity: Nonpolar

L. PO₃³⁻ (Phosphite)

Lewis Structure: P central, three O atoms, one lone pair, three negative charges.
Electron Pair Geometry: Tetrahedral
Molecular Shape: Trigonal pyramidal
Hybridization: sp³
Polarity: Polar

Explanation

Understanding molecular structure involves analyzing electron configurations and geometry. Lewis structures show how atoms and electrons are arranged. Molecular geometry is determined by the number of bonding and lone pairs using VSEPR theory. Hybridization explains orbital overlap forming specific molecular shapes.

For example, NH₄⁺ is tetrahedral and nonpolar because its symmetric geometry cancels out dipoles. In contrast, H₂NF₂⁺ has a bent shape due to lone pairs on nitrogen, making it polar. Carbonate (CO₃²⁻) and nitrate (NO₃⁻) are resonance-stabilized and trigonal planar, resulting in nonpolarity due to symmetry.

Ions like SO₄²⁻ and PO₄³⁻ exhibit tetrahedral geometry due to four regions of electron density. However, when lone pairs exist, as in SO₃²⁻ or PO₃³⁻, the shape becomes trigonal pyramidal and results in a polar molecule. The lone pair contributes to molecular asymmetry.

Sulfur compounds like SO₂ and SO₃ differ in shape and polarity due to the number of oxygen atoms and lone pairs on sulfur. SO₂ is bent and polar, while SO₃ is trigonal planar and nonpolar.

Hybridization reflects the number of bonding domains: sp³ for tetrahedral shapes (e.g., NH₄⁺, SO₄²⁻), and sp² for trigonal planar (e.g., NO₃⁻). Polar molecules have unequal charge distributions, typically from lone pairs or asymmetric shapes, affecting their physical and chemical properties, including solubility and reactivity.

This understanding is essential in predicting molecular behavior in reactions, bonding strength, and interactions in biological and industrial processes.