Chem 2 Exam 1

Front 1

Matter

attractive forces are so strong atoms, molecules, or ions are held together in specific arrangement

Back 1

solid

Front 2

Matter

attractive forces are strong enough to pull the particles close together but still allowing them considerable freedom to move about

Back 2

Liquid

Front 3

Matter

attractive forces among the particles are very weak, far apart from each other and have almost no influence on one another

Back 3

gas

Front 4

The transformation of a substance from one state to another. Every change of state is reversible and is characterized by a free-energy change.

Back 4

Phase change or change of state

Front 5

The temperature at which solid and liquid are in equilibrium.

Back 5

Melting point (mp)

Front 6

The temperature at which liquid and gas are in equilibrium.

Back 6

Boiling point (bp)

Front 7

A process in which a solid changes directly to a gas without going through the liquid state.

Back 7

Sublimation

Front 8

A process in which a gas changes directly to a solid without going through the liquid state.

Back 8

Diposition

Front 9

depends primarily on the strength of the attractions between solute and solvent particles relative to the strengths of the attractions within the pure substances.

Back 9

solubility

Front 10

The clustering of solvent molecules around a dissolved solute molecule or ion.

Back 10

Solvation

Front 11

Some ionic compounds attract water strongly enough to hold on to water molecules even when crystalline.

Back 11

Solid hydrate

ex: CuSO4.5H2O for every unit of copper sulfate, there are 5 water molecules present

Front 12

The forces that act between molecules and hold molecules close to one another.

Back 12

Intermolecular Forces

Front 13

3 major types of intermolecular forces are

Back 13

dipole-dipole

London dispersion

hydrogen bonding

Front 14

Molecule containing polar covalent bond may have a net molecular polarity. In such cases, the positive and negative ends of different molecules are attracted to each other

Back 14

Dipole-dipole

Front 15

The short-lived attractive force due to constant motion of electrons within molecules.

Back 15

London dispersion Force

Front 16

an attractive interaction between an unshared electron pair on an electronegative O, N, and F and a positively polarized hydrogen atom bonded to another O, N, or F.

Back 16

Hydrogen bonds

Front 17

Molecules are in constant motion in the ________ state. If a molecule is happened to be near the surface of a liquid, and if it has enough energy, it can break free of the liquid and escape into the gas state, called __________.

Back 17

liquid

vaporIn an open container, the gaseous molecule will wander away from the liquid, and the process will continue until all the molecules escape from the container.

Front 18

In an open container, the gaseous molecule will wander away from the liquid, and the process will continue until all the molecules escape from the container.

Back 18

evaporation

Front 19

If the liquid is in a closed container, the gaseous molecule can’t escape. The random motion of molecule occasionally will bring them back into the liquid. After the concentration of molecule in the gas state has increased sufficiently, the number of molecules reentering the liquid becomes equal to the number of molecules escaping the liquid.

Back 19

Dynamic equillibrium

Front 20

In a closed container at equilibrium, the gas molecules make their own contribution to the total pressure of the gas above the liquid according to the Dalton’s law.

Back 20

Vapor pressure of the liquid

Front 21

normal boiling point occurs at

Back 21

760 mm Hg

Front 22

water covers ___ % of earths surface

water accounts for ___% of mass of adult

Back 22

71

66

Front 23

water has the highest _______ _____ of any liquid. It absorbs a large quantity of heat while changing the temperature slightly

Back 23

specific heat

Front 24

Water has unusually _______________ – it carries away large amount of heat when it evaporates.

Back 24

heat of vaporization

Front 25

One whose particles – whether atoms, ions, or molecules- have an ordered arrangement extending over a long range.

Back 25

Crystalline solid

Front 26

Cystalline solids

1. Na+Cl- whose constituent particles are ions.

2. diamond or quartz where molecules are held together by covalent bonds.

3. sucrose or ice whose constituent particles are molecules held together by the intermolecular forces.

4.such as silver or iron – three dimensional array of metal ions immersed in electrons that are free to move about.

Back 26

1. Ionic

2. Colvalent

3. Molecular

4. Metallic

Front 27

One whose constituent particles are randomly scattered and has no long range structure.

Back 27

Amorphous solid

Front 28

The quantity of heat required to completely melt a substance once it has reached its melting point.

Back 28

Heat of Fusion

Front 29

The quantity of heat required to completely vaporize a substance once it has reached its boiling point.

Back 29

Heat of vaporization

Front 30

Law: Volume of a fixed amount of gas is inversely proportional to its pressure.

Back 30

Boyle's Law

Front 31

Law: Volume of a fixed amount of gas is directly proportional to its Kelvin temperature.

Back 31

Charles Law

Front 32

Law: The pressure of a fixed amount of gas at constant volume is directly proportional to its Kelvin temperature.

Back 32

Gay-Lussac's Law

Front 33

Law: Equal volume of gases at the same temperature and pressure contain the same number of moles.

Back 33

Avogadro's Law

Front 34

Law: Boyle’s law, Charles’ law, and Gay-Lussac’s law together is known as ...

Back 34

Combined gas law

Front 35

Law: Relates the effects of temperature, pressure, volume, and molar amount.

Back 35

Ideal gas law

Front 36

At 0oC and 1 atm pressure, Standard temperature and pressure (STP), 1 mole of any gas occupies a volume of _____ liters

Back 36

22.4

Front 37

The amount of pressure exerted by an individual gas in a mixture.

Back 37

Partial Pressure

Front 38

A nonuniform mixture that has regions of different composition

Back 38

Heterogeneous mixture

Front 39

A uniform mixture that has the same composition throughout.

Back 39

Homogeneous mixture

Front 40

A homogeneous mixture that contains particles the size of a typical ion or small molecule.

Back 40

Solution

Front 41

A homogeneous mixture that contains particles in the range of 2-500 nm diameter.

Back 41

Colloid

Front 42

A substance dissolved in a liquid.

Back 42

Solute

Front 43

The liquid in which another substance is dissolved.

Back 43

Solvent

Front 44

Having the ability to pull water molecules from the surrounding atmosphere. Some ionic compounds attract water so strongly that they pull water from humid air to become hydrated, such as CaCl2.

Back 44

hygroscopic

Front 45

Law: The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas over the liquid if the temperature is constant.

-Pressure has virtually no effect on the solubility of a solid in a liquid or a liquid in a liquid.

Back 45

Henry's law

Front 46

the number of moles of solute dissolved per liter of solution’.

Back 46

Molarity

Front 47

Weight/Volume Percent Concentration [(w/v)%]

Back 47

Mathematically, (w/v)% concentration is found by taking the number of grams of solute per milliliters of solution and multiplying by 100.

Front 48

Lowering concentration by adding additional solvent. the amount of solute remains constant only the volume is increased by adding more solvent.

Back 48

Dilution

Front 49

A substance that produces ions and therefore conducts electricity when dissolved in water.Ionic compounds in aqueous solution can conduct electricity

Back 49

Electrolyte

Front 50

A substance that ionizes completely when dissolved in water, such as NaCl.

Back 50

Strong electrolyte

Front 51

A substance that is partly ionized in water, such as CH3COOH.

Back 51

Weak electrolyte

Front 52

A substance that does not produce ions when dissolved in water, such as sucrose.

Back 52

Nonelectrolyte

Front 53

The properties of a solution that depends on the concentration of a dissolved solute but not on its chemical identity is known as

Back 53

colligative properties

Front 54

The passage of solvent through a semipermeable membrane separating two solutions of different concentrations.

Back 54

osmosis

Front 55

The amount of external pressure applied to the more concentrated solution to halt the passage of solvent molecules across a semipermeable membrane.

Back 55

osmotic pressure

Front 56

red blood cells in

1. hypotonic solution....

2. hypertonic solution....

Back 56

1. swollen bc water gain

2. shriveled bc water loss

Front 57

similar to osmosis, except the pores are larger than those in osmotic membrane.

Back 57

dialysis