Chapter 5

Question 1

Ideal Gas

Answer 1

Model of the way that gas particles (molecules or atoms) behave at the atomic/molecular level.

Question 2

Kinetic Molecular Theory

Answer 2

1) Gases are made up of tiny atoms/molecules that are in constant, random motion. Particles are moving linearly.
2) The Distance of separation among these atoms/molecules is very large. Gas is mostly empty space.
3) All atoms/molecules behave independently.
4) Atoms/molecules collide with each other and container without losing energy
5) The average kinetic energy of the atoms/molecules increases/decreases in proportion to absolute temperature.

Question 3

When do gases behave more ideally?

Answer 3

when there is low pressure and high temperatures

Question 4

Boyle’s law calculates what?

Answer 4

volume resulting from a pressure change, or vise versa

Question 5

Charle’s law:

Answer 5

Volume of a gas varies with absolute temperature if pressure and number of mole of gas are constant (think hot air balloon)

Question 6

Avogadro’s Law

Answer 6

relationship between the volume and # of the mol of a gas at constant temperature and pressure

Question 7

Molar volume

Answer 7

volume occupied by 1 mol of any gas

Question 8

STP?

Answer 8

standard temperature and pressure

Question 9

What is the molar volume of any gas?

Answer 9

22.4L

Question 10

Density equation?

Answer 10

d = mass/volume

Question 11

Dalton’s law

Answer 11

Partial pressure, Pt = p1 + p2 + p3 + etc….

Question 12

Viscosity

Answer 12

a liquids measure of its resistance to flow

Question 13

Molecules with complex structures and polar molecules, have lower or higher viscosity?

Answer 13

tend to have higher viscosity than less structurally complex, less polar liquids

Question 14

Does viscosity decrease or increase with temperature?

Answer 14

generally decreases with increasing temperature

Question 15

Surface tension

Answer 15

measure of attractive forces exerted among molecules at the surface of the liquid

Question 16

Does surface tension increase or decrease with an increase in temperature or a decrease in the polarity?

Answer 16

decreases with increase temp or decreased polarity

Question 17

Surfactant?

Answer 17

substance that can be added to a liquid to decrease surface tension

Question 18

Example of surfactant?

Answer 18

Soap, Detergents

Question 19

dynamic equilibrium

Answer 19

when the rate of evaporation and condensation become equal

Question 20

vapor pressure of a liquid

Answer 20

defined as the pressure exerted by the vapor at equilibrium

Question 21

normal boiling point

Answer 21

temperature at which the vapor pressure of the liquid is equal to 1 atm

Question 22

Large intermolecular attractive forces have higher or lower boiling points?

Answer 22

higher boiling points than non polar liquids

Question 23

Does gasoline have higher or lower attractive forces

Answer 23

lower, making it easier to burn

Question 24

attractive forces between polar molecules, dipole-dipole interactions do what with vapor pressure and b.p.

Answer 24

decrease vapor pressure and increase boiling point

Question 25

London forces

Answer 25

temporary dipoles which can interact with other temporary dipoles, just as permanent dipoles interact in polar molecules

Question 26

Van Der Waals Forces?

Answer 26

collective name for london forces and dipole-diopole

Question 27

Hydrogen atom needs to bond to what highly electronegative atom to be a ‘Hydrogen Bond’?

Answer 27

Nitrogen, Oxygen, or Fluorine

Question 28

polar solid or nonpolar solid, which one has higher melting point?

Answer 28

polar solid

Question 29

crystalline solid

Answer 29

regular repeating structure

Question 30

amorphous solid

Answer 30

no organized structure

Question 31

what kind of solid is glass and concrete?

Answer 31

amorphous, same as plastic

Question 32

ionic solid?

Answer 32

crystalline solid:
composed of positive and negative ions. 
electrostatic forces hold the crystal together
High melting points
hard n brittle
ex. sodium chloride

Question 33

Covalent solid

Answer 33

crystalline solid:
atoms held together by covalent bonds. 
-very high melting points
-extremely hard
-insoluble in most solvents

Question 34

Molecular solid

Answer 34

crystalline solid:
molecules held together by intermolecular attractive forces (London forces, dipole-dipole, hydrogen bonding)
-usually soft and have low melting points
-frequently volatile and poor electrical conductors
ex: ice

Question 35

Metallic Solid

Answer 35

crystalline solid:

• held together by metallic bonds
• high electron density surround the positive metal nuclei
• High conductivity
• easily shaped

Question 36

sublimation

Answer 36

process in which some molecules in sold state convert directly to gaseous state