Question 1: Indicate the hybridization for the designated atoms.
Question 2: Identify the polar covalent compounds from the list:
a. TeH2
b. BCl3
c. NCl3
d. CH3CH3
e. Si(CH3)2F2
f. CO2
Question 3: Determine the types of intermolecular forces present between a PCl3 and HCl molecule.
Question 4: Which solution is the weakest electrolytic solution?
a. HCl
b. MgCl2
c. LiBr
d. FeCl3
e. K2O
f. HF
Question 5: Identify which of the following does NOT contain acidic protons:
a. CH3COOH
b. NH3
c. HBr
d. H3PO4
e. HNO3
Question 6: Count the number of sigma (σ) and pi (π) bonds in the molecule:
a. 8 σ and 6 π
b. 3 σ and 5 π
c. 6 σ and 4 π
d. 8 σ and 2 π
e. 6 σ and 2 π
Chapter 15 Topics:
15.1 Molecular Structure and Functional Groups
15.2 Organic Molecules and Isomers (Chirality skipped)
15.4 Functional Groups
Including Alkanes, Alkenes, and Alkynes
Understanding Aromaticity
Carbon (C): always has 4 bonds
Nitrogen (N): typically has 3 bonds (4 indicates a cation, e.g. NH4+)
Oxygen (O): typically has 2 bonds
Halogens (F, Br, Cl, I): typically have 1 bond
Organic Chemistry: study of carbon compounds, primarily those containing hydrogen.
Carbon readily bonds with itself and heteroatoms (common ones: H, N, O, F, P, S, Cl, Br, I).
Carbon compounds: Millions exist, with ~15,000 new compounds added daily to the chemical registry.
Electron Configuration: [He]2s22p2
Valence Electrons: 4
Tendency to Form Ions: Not favorable (doesn’t form C4+ or C4- ions).
Bonding Nature: Forms 4 covalent bonds (σ and π), adhering to the octet rule.
Electronegativity (EN): 2.5 (between Li EN = 1.0 and F EN = 4.0).
Forms 4 bonds via hybridization.
Small size allows for strong, short carbon-carbon bonds, facilitating π-bonding.
Catenation: carbon's ability to bond to itself, results in stable molecular constructs compared to silicon.
Atomic sizes:
Carbon: 77 pm
Silicon: 118 pm
Bond strength comparisons: C-C (347 kJ/mol) vs Si-Si (226 kJ/mol)
C’s small size leads to better orbital overlap and stability of molecules.
Carbon Skeleton: Variation in structures leads to numerous compounds.
Structures can be linear, branched, or cyclic.
Rule of 4 Bonds: Hydrogen count based on carbon's valency.
C single-bonded to one atom has 3 H atoms, 2 bonded has 2 H, 3 bonded has 1 H, and 4 bonded means no H.
Each C in double bonds treated as if bonded to two other atoms.
Hydrocarbons: Compounds of carbon and hydrogen (e.g. methane, ethane, benzene).
Bonding Behavior: Rotation in single bonds, fixed in double bonds.
Definition: Alkanes contain only single bonds (saturated hydrocarbons).
General Formula: CnH2n+2
Alkane Examples: Butane, Pentane, etc.
Naming Convention: Root name + prefix + suffix.
Example Roots: meth- (1), eth- (2), prop- (3), but- (4), pent- (5).
Structure: CnH2n; rings insensitive to saturation.
Stability: 5 & 6 member rings are more stable than 3 or 4.
Isomer Types: Same molecular formula but different arrangements.
Properties: Depend on specific structural orientations and functional groups.
Alkenes: Include double bonds (general formula CnH2n).
Alkynes: Include triple bonds (general formula CnH2n-2).
Functional Groups: Specific atomic combinations that influence chemical reactivity and properties.
Alcohols: Contain -OH; named with suffix -ol.
Haloalkanes: Contain halogen bonded to carbon.
Amines: Derivatives of ammonia (NH3) with weak base characteristics.
Carbonyl Group: Found in aldehydes, ketones, carboxylic acids, and other functional groups; highly polar.
Example Compounds: Methanal and Ethanal with diverse chemical uses.
Various examples, descriptions, and their chemical behavior in relation to other molecules.