Question

Using molecular models, construct the following molecules/polyatomic ions, and write their Lewis formulas. Record the following information for each in your laboratory notebook. a) Molecule or ion (Formula and IUPAC name) b) Lewis structure c) Draw any resonance structures if applicable d) # of bonding regions (double and triple bonds count as a single region) e) # of nonbonding pairs f) Hybridization of the central atom g) VSEPR designation h) Molecular geometry of the molecule/polyatomic ion, i) Polarity of the molecule/ion j) 3-D sketch Your table in your notebook should be neat and organized to include all of the following information for each of the 16 molecules/ions: Molecule Lewis Structure or (include any Data Sketch of the 3-D Polyatomic resonance lon structures) Bonding regions # of bonding regions # of non-bonding pairs Hybridization VSEPR formula Molecular geometry Polar or nonpolar 1. CFCI 2. HS 3. NO 4. HNO3

Answer 1

1. CH₃Cl :  

# Bonding regions : 4

# Non- Bonding pairs : 0 (on Cl but not part of central atom)

Hyybridization : sp3

VSEPR Formula : AX₄

Molecular geometry : Tetrahedral

Polarity : Polar ( mainly by -C-Cl bond)

2. H₂S :  

# Bonding regions : 2

# Non- Bonding pairs : 2

Hyybridization : sp3

VSEPR Formula : AX₂E₂

Molecular geometry : Bent

Polarity : Polar

14 :7 : D: H 2. 3. N:N: : 6 T NIN:::0 @NニNニ0の 6:: N:8:H

3. N₂O :  

# Bonding regions : 2

# Non- Bonding pairs : 0 (we count central atom N)

Hyybridization : sp

VSEPR Formula : AX₂

Molecular geometry : Linear

Polarity : Polar (N , O E.N. difference)

4. HNO₃ :  

# Bonding regions : 3

# Non- Bonding pairs : 0

Hyybridization : sp2

VSEPR Formula : AX₃

Molecular geometry : Trigonal planar

Polarity : Polar