Basics

Question 1

Liquid

Answer 1

State or phase of matter. Particles have more KE than in solid state. Particles can move (flow)past each other, and are not held in a regular arrangement, but cannot move freely because they are held by weak intermolecular attractions (attractive forces), resulting in cohesion. Particles are still close together–>liquids have a definite volume, but an indefinite shape that can change to fit/conform to the container. They cannot withstand any shear without deforming. Force is spread evenly throughout, so an object placed in a liquid will displace the liquid’s particles. They basically cannot be compressed (particles close together–cant be easily compressed and keep same volume; compression requires so much force and even when it occurs is so minimal that it’s not useful to think of them as being compressible). Liquids are relatively dense-lots of particles in a small volume.

Question 2

Gas

Answer 2

State or phase of matter where particles have enough KE to overcome intermolecular forces that hold solid and liquids together. Particles in a gas have very weak forces of attraction between them, which essentially means they are far apart and can move freely past each other–lots of space in between particles. Fast movement (high KE) in all directions. They do not have a definite shape or volume; unconfined will expand indefinitely, and confined will expand to fill any container. They can be easily compressed into a smaller volume because of the weak attractive forces that mean there is lots of space between them; compression results in increased pressure exerted by more frequent collisions btwn particles and increased temperature (KE). Increasing the temperature of a gas without changing the volume of the container will also increase the pressure exerted by more frequent collisions. Because particles are spread out in a large volume (or per volume unit there are fewer particles), gases have very low densities.

Question 3

Solid

Answer 3

A state of matter. Particles are held tightly together by strong forces of attraction. Solids cannot flow; they have a definite shape and volume (do not conform to shape of container)-the particles cannot be easily compressed to a smaller volume. Low kinetic energy. Particles have a fixed position–movement of particles (atoms can vibrate) does not change their position/arrangement. Can withstand shear without deforming. Brittle–if enough force is applied, will break/shatter. Generally solids are thought of as the densest state of matter, because the ratio of particles to volume is smallest (lots of particles in small volume)

Question 4

Vapor pressure

Answer 4

Inverse relationship to IMF. The stronger the IMF, the lower the vapor pressure. Vapor pressure is a measure of the likelihood of a molecule of a liquid to turn into a gas (to have enough KE to overcome IMF). Direct relationship to temp-increase in temperature also means increase in vapor pressure. Direct relationship to boiling point and melting point-increase in vapor pressure means increase in boiling point or melting point.

Question 5

Joules (unit)

Answer 5

(Kg • m^2)/(s^2)

Question 6

Dichromate

Answer 6

Cr2O7 (2-)

Question 7

Chromate

Answer 7

CrO4 (2-)

Question 8

Atomic radius

Answer 8

Distance between the 2 nuclei of a diatomic molecule of an element. Indicates atomic size. Generally, larger atoms are more polarizable.

Question 9

Atomic radius

Answer 9

Distance between the 2 nuclei of a diatomic molecule of an element. Indicates atomic size. Generally, larger atoms are more polarizable.

Question 10

Name of the element whose symbol is P

Answer 10

Phosphorus

Note the spelling!