Chemistry I Chapter 9

Ace your homework & exams now with Quizwiz!

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


Related study sets

Econ Module 2.5, 2.6, 2.7, & 2.8

View Set

PSY 212: Exam 2 Activity Questions

View Set

Texas Law of Contracts - Chapter 4

View Set

Chapter 10 Data Quality and Integration

View Set

Hinkle Ch 26: Assessment and Management of Vascular and Peripheral Circulation Disorders

View Set