Principles of Chemistry I - Exam 3

Arrange from shortest to longest

A) Single bonds, double bonds, triple bonds B) Triple bonds, double bonds, single bonds C) None of the above

Bond strength is __________ proportional to the number of bonding electrons between two atoms.

A) Directly B) Indirectly C) Not D) All of the above

A measure of the decrease in the energy of a system if bonding electrons are localized in the vicinity of a given type of atom.

A measure of the probability of finding the electrons in a bond localized in the vicinity of that atom.

Symbol for electronegativity

A very reactive atom with one unpaired electron.

E Pair Geometry: 2 electron domains

A) Linear B) Trigonal Planar C) Tetrahedral D) Trigonal pyramidal

E Pair Geometry: 3 electron domains

A) Linear B) Trigonal Planar C) Tetrahedral D) Trigonal pyramidal

E Pair Geometry: 4 electron domains

A) Linear B) Trigonal Planar C) Tetrahedral D) Trigonal bipyramidal

E Pair Geometry: 5 electron domains

A) Linear B) Trigonal Planar C) Tetrahedral D) Trigonal bipyramidal

Bond angle: bent (one lone pair)

A) 109.5 B) >120 C) 120 D) 180 E) <109.5

Bond angle: bent (two lone pairs)

A) 109.5 B) >120 C) 120 D) 180 E) <109.5

Bond angle: trigonal planar

A) 109.5 B) >120 C) 120 D) 180 E) <109.5

Bond angle: tetrahedral

A) 109.5 B) >120 C) 120 D) 180 E) <109.5

Bond angle: linear

A) 109.5 B) >120 C) 120 D) 180 E) <109.5

Ketone

Aldehyde

Carboxyl

Alkoxy

Amine

Phenyl

Hydroxyl

Vibrations that absorb IR radiation

Vibrations that do not absorb IR radiation

What things affect how a molecule interacts with other particles?

The strength of IMFs depends on....

A measure of how easily an electron cloud is distorted or shifted by an electric field.

More electrons and a larger radius means a molecule is (more/less) easily polarizable

A molecule has a large surface area and more e-. Which is true?

A) Lower polarizability B) Lower vapor pressure C) High BP D) Low BP

Which intramolecular forces are present in this molecule?

CH4

A) London Dispersion B) Dipole-Dipole C) Hydrogen bonds

Which intermolecular forces are present in this molecule?

HCl and HCl

A) London Dispersion B) Dipole-Dipole C) Hydrogen bonds

Strongest?

A) London Dispersion B) Dipole-Dipole C) Dipole-induced dipole D) Ion-dipole E) Ion-induced dipole

Weakest?

A) London Dispersion B) Dipole-Dipole C) Dipole-induced dipole D) Ion-dipole E) Ion-induced dipole

Ion with a NP molecule

A) London Dispersion B) Dipole-Dipole C) Dipole-induced dipole D) Ion-dipole E) Ion-induced dipole

NP Molecule with a Polar Molecule

A) London Dispersion B) Dipole-Dipole C) Dipole-induced dipole D) Ion-dipole E) Ion-induced dipole

Same as instant dipole-induced dipole

A) London Dispersion B) Dipole-Dipole C) Dipole-induced dipole D) Ion-dipole E) Ion-induced dipole

More "branches" (more circular of a structure) means (higher/lower) IMFs.

Lower IMFs mean lower...

A) Melting Points B) Boiling Points C) Vaporization Energy D) Viscosities E) All of the above

Lower IMFs mean higher...

A) Melting Points B) Boiling Points C) Vaporization Energy D) Viscosities E) Volatilities

2 polar molecules

A) London Dispersion B) Dipole-Dipole C) Dipole-induced dipole D) Ion-dipole E) Ion-induced dipole

Ion & a polar molecule

A) London Dispersion B) Dipole-Dipole C) Dipole-induced dipole D) Ion-dipole E) Ion-induced dipole

A substance wants to be in the state with the ___________ energy and the __________ # of configurations

A) Highest, highest B) Highest, lowest C) Lowest, highest D) Lowest, lowest

To determine if two substances mix, pick the state with the....

A) Highest energy B) Highest # configs C) Lowest energy D) Lowest # configs