Chemistry I Chapter 9
Determine the intermolecular forces taking place in the molecule: CH₄
Dipole-Dipole Forces 2.55-2.20 = .35
Determine the intermolecular forces taking place in the molecule: PCl₃
Dipole-Dipole Forces 3.16-2.19 = .97
Determine the intermolecular forces taking place in the molecule: NCl₃
Dispersion Forces 3.16-3.04 = .12
Formula for hydrochloric acid
HCl
Formula for chlorous acid
HClO₂
Identify the type of bond and determine the ion charge or pole of each atom. O and S
Polar Covalent, O negative pole, S positive pole 3.44-2.58 = .86
Determine the polarity of the molecule: PCl₃
Polar Molecule 3.16-2.19 = .97 Trigonal pyramidal Satisfies the 2 conditions of a polar molecule
Determine the polarity of the molecule: H₂O
Polar Molecule 3.44-2.20 = 1.24 Bent Satisfies the 2 conditions of a polar molecule
Unequal sharing of electrons.
Polar molecule
Formula for sulfur heptachloride
SCl₇
H₃As
hydroarsenic acid
The strongest type of intermolecular bond.
hydrogen bond
HClO
hypochlorous acid
The suffix of the ion of an oxyacid with the name hydro-suffix-ic acid.
ide
The weak attraction between molecules.
intermolecular forces
The distance between two bonding nuclei at the position of maximum attraction.
bond length
H₂CO₃
carbonic acid
ClBr
chlorine monobromide
The chemical bond that results from the sharing of valence electrons.
covalent bond
The weakest type of intermolecular bond
dispersion force
P₆S₈
hexaphosphorus octasulfide
Another name for a single covalent bond.
sigma bond
The common name for SiI₄ is tetraidosilane. Name this molecule using the scientific method.
silicon tetraiodide.
SI₅
sulfur pentaiodide
N₄Cl
tetranitrogen monochloride
Formula for dichlorine mononitride
Cl₂N
The number of pi bonds in a double covalent bond.
1
The number of covalent bonds formed between chlorine atoms.
1, Cl-Cl share 1 pair of electrons.
The number of pi bonds in a triple covalent bond.
2
Molecular shape of H₂O
Bent, 2 pairs of unbonded pairs of electrons.
Formula for tribromine nonachloride
Br₃Cl₉
Which compound has at least one pi bond? CO₂ CCl₄ AsI₃ or SF₂
CO₂ Its structure is O=C=O, which has 2 double bonds.
Determine the intermolecular forces taking place in the molecule: H₂O
Hydrogen bonds H-O bond
Formula for dichromic acid
H₂Cr₂O₇
Formula for hydrotelluric acid
H₂Te
Identify the type of bond and determine the ion charge or pole of each atom. Na and Cl
Ionic, Na⁺ and Cl⁻ 3.16-.93 = 2.23 ionic
Molecular shape of CS₂
Linear, no unbonded pairs of electrons
Determine the polarity of the molecule: NCl₃
Non-Polar Molecule 3.16-3.04 = .12 Must be over .30
Determine the polarity of the molecule: CO₂
Non-Polar Molecule linear molecule
Determine the polarity of the molecule: CH₄
Non-polar Molecule Tetrahedral is not a condition of being polar.
Identify the type of bond and determine the ion charge or pole of each atom. S and Se
Nonpolar covalent. 2.58-2.55 = .03
Molecular shape of CCl₄
Tetrahedral.
Molecular shape of NO₃⁻
Trigonal planar, no unbonded pairs of electrons.
Molecular shape of NH₃
Trigonal pyramidal, 1 pair of unbonded electrons.
The model that is based on an arrangement that minimizes the repulsion of shared and unshared pairs of electrons around the central atom.
VSEPR Model
HC₂H₃O₂
acetic acid
The suffix of the ion of an oxyacid with the name suffix-ic acid.
ate
