Chem Test 3

Front 1

solute

Back 1

a component of a solution present in lesser amount than the solvent

Front 2

solubility

Back 2

the maximum amount of a solute that will dissolve in a solvent under a given set of conditions

Front 3

colloidal dispersion

Back 3

a homogeneous mixture that contains dispersed particles intermediate in size between those of a true solution and those of a heterogeneous mixture

Front 4

osmosis

Back 4

the passage of solvent through a semipermeable membrane separating a dilute solution (or pure solvent) from a more concentrated solution

Front 5

chemical reduction

Back 5

the gain of electrons in a reaction

Front 6

catalyst

Back 6

a substance that increases a reaction rate without being consumed in the reaction

Front 7

equilibrium constant

Back 7

a numerical value characterizing the ratio of products to reactants when forward and reverse reactions are happening at the same rate

Front 8

amphiprotic

Back 8

describes a substance that can function as either an acid or a base

Front 9

salt

Back 9

an ionic compound that can be formed in an acid-base neutralization reaction

Front 10

base (Bronsted-Lowry)

Back 10

a substance that can accept a proton (H+) from an acid

Front 11

conjugate acid

Back 11

a chemical species formed when a base accepts a proton

Front 12

buffer

Back 12

a mixture that, in aqueous solution, resists changes in pH even if small amounts of acid or base are added

Front 13

strong acid vs. weak acid

Back 13

A strong acid ionizes almost completely in aqueous solution; that is, it transfers all (or nearly all) possible hydrogen ions to water to form hydronium ion. A weak acid ionizes only slightly in aqueous solutions; that is, it transfers only a small percentage of hydrogen ions to water.

Front 14

hypotonic vs. hypertonic

Back 14

A hypotonic solution has an osmotic pressure lower than that found in cells, while a hypertonic solution has an osmotic pressure higher than that found in cells.

Front 15

catalyst vs. reactant

Back 15

A catalyst is not consumed in a chemical reaction, while reactants are.

Front 16

First factor that effects a chemical reaction

Back 16

The physical nature of the reactant(s): the more finely divided the reactant particles are the more quickly they tend to react, so that gaseous reactants (separated down to the molecular level) tend to react faster than liquids or solids.

Front 17

2nd factor that effects a chemical reaction

Back 17

Concentrations of reactants: the more concentrated (or the higher the pressure for gaseous reactants) the faster the reactions.

Front 18

3rd factor that effects a chemical reaction

Back 18

Temperature: generally the higher the temperature the faster the reactions.

Front 19

4th factor that effects a chemical reaction

Back 19

Catalysis: a catalyst provides for a lower activation energy, so it accelerates reactions.

Front 20

combination reaction

Back 20

a chemical reaction in which a single product is produced from 2 (or more) reactants

X+Y------> XY

Front 21

decomposition reaction

Back 21

a chemical reaction in which a single reactant is converted into tow (or more) simpler substances (elements or compounds)

XY ---------> X+Y

Front 22

displacement reactions

Back 22

a chemical reaction in which an atom or molecule displaces an atom or group of atoms from a compound

X + YZ ------> Y + XZ

Front 23

exchange reactions

Back 23

a chemical reaction in which 2 substances exchange parts with one another and form 2 different substances

AX + BY--------> AY + BX

Front 24

combustion reactions

Back 24

a chemical reaction between a substance and oxygen (usually air) that proceeds with the evolution of heat and light (usually a flame)

Front 25

saturated solution

Back 25

is a chemical solution containing the maximum concentration of a solute dissolved in the solvent.

Front 26

colligative property

Back 26

a physical property of a solution that depends only on the number (concentration) of solute particles (molecules or ions) present in a given quantity of solvent and not on their chemical identities

Front 27

give 2 examples of a colligative property

Back 27

freezing point depression, osmotic pressure

Front 28

Mole

Back 28

- a number equal to 6.02 X 1023 objects

Front 29

reactant

Back 29

- a starting material that undergoes a change in a chemical reaction

Front 30

Kinetic energy

Back 30

- the capacity of an object to do work because of its motion

Front 31

sublimation

Back 31

direct conversion from the solid state to the gaseous state

Front 32

volatile

Back 32

- having a high vapor pressure

Front 33

trianglar plainer

Back 33

- a molecular shape that is flat and triangular, resulting from 3 VSEPR electron groups

Front 34

Binary compound

Back 34

- a pure substance made up of exactly two elements

Front 35

theoretical yield

Back 35

- the maximum number of grams of product obtainable from given amounts of reactants

Front 36

polar covalent bond

Back 36

- an unequal sharing of electrons between two atoms

Front 37

vapor pressure

Back 37

- the force exerted by a gas produced by evaporation of molecules from a liquid state

Front 38

Boiling point

Back 38

- the temperature at which the vapor pressure above a liquid is equal to external air pressure

Front 39

barometer

Back 39

- a device used to measure atmospheric pressure

Front 40

electronegativity

Back 40

- the attraction of an atom for electrons

Front 41

Matter

Back 41

- anything that has mass and occupies space

Front 42

physical change

Back 42

- any process that results in no new substance being formed

Front 43

density

Back 43

- the ratio of an object’s mass to its volume

Front 44

atomic number

Back 44

- the sum total of protons in a nucleus

Front 45

halogen

Back 45

- an element found in Group VIIA on the periodic table

Front 46

isotope

Back 46

- a form of an element whose atoms differ from those of other forms of that element in the number of neutrons in the nucleus

Front 47

ion

Back 47

- an atom (or group of atoms) that bears an electrical charge

Front 48

formula unit

Back 48

- the smallest whole-number ratio of ions needed for net charge neutrality in an ionic compound

Front 49

binary compound

Back 49

- a pure substance made up of exactly two elements

Front 50

element

Back 50

- a pure substance that cannot be broken down to simpler substances by chemical means

Front 51

heterogeneous vs. homogeneous

Back 51

”Heterogeneous” means that two or more visibly different phases are present; while “homogeneous” means that only one phase, with uniform properties throughout, is present.

Front 52

compound vs. homogeneous mixture

Back 52

A compound can be broken down to simpler substances only by chemical means, while a homogeneous mixture can be separated into its components by physical means.

Front 53

mass number vs. atomic mass

Back 53

Mass number is the integer number of nucleons present in an atom, while atomic mass is the weighted average of the mass of all naturally occurring isotopes of an element.

Front 54

metal vs. nonmetal

Back 54

A metal is a substance that is shiny (or lustrous), a good conductor of heat and electricity, malleable, and ductile. A nonmetal is a substance that is dull (not lustrous), usually a poor conductor of heat and electricity, and generally brittle (if solid) rather than malleable.

Front 55

group vs. period (on periodic tables)

Back 55

Groups are vertical columns, periods are horizontal rows.

Front 56

shell vs. orbital

Back 56

A shell is a level (region of space) about a nucleus where electrons of approximately the same energy are found, while an orbital is a specifically shaped volume of space within a shell.

Front 57

mass number

Back 57

the total number of protons and neutrons in a necleus

Front 58

alkali metal

Back 58

a general name for any element in group 1A of the periodic table except for Hydrogen

Front 59

forumla unit

Back 59

the smallest whole-number repeating ratio of ions present in an ionic compound that results in charge neutrality

Front 60

based on the kinetic molecular theory, the two states of matter in which the particles can readily move around each other are _______and ______

Back 60

solid and liquid

Front 61

the maximum number of grams of produce that can be obtained from specified amounts of the starting materials is called the ______yield

Back 61

theoretical

Front 62

according to the VSEPR rules, a ______shape is characteristic of molecules like O3

Back 62

bent (or trigonal planer)

Front 63

the force exerted by particles that have escaped from the surface of a liquid to enter the gaseous state is called the_________pressure

Back 63

vapor

Front 64

an equal sharing of elections between two atoms that are bonded together is called a__________covalent bond

Back 64

non polar

Front 65

how many elections are being shared in a double covalent bond?

Back 65

four

Front 66

what is the name given to the substances to the left of a reaction arrow in a chemical equation?

Back 66

reactants

Front 67

if vapor molecules are returning to the liquid state as fast as molecules escape from the liquid to become vapor, what is the name of this state?

Back 67

equilibrium

Front 68

the intermolecular force holding molecules like HF to each other has what name?

Back 68

hydrogen bonding

Front 69

what will happen if salt is added to pure water?

Back 69

it increases the boiling point relative to pure water

Front 70

if the activation energy of a reaction is high, what must be true about the reaction

Back 70

the reaction rate will be low

Front 71

solubilities of most substances increase with increasing temperature, with what important exceptions?

Back 71

all gases

Front 72

a buffer solution is made by mixing nitrous acid with sodium nitrate in water. what will be the pH of this solution

Back 72

can not be determined

Front 73

which of the following is true about a hypotonic solution

Back 73

is has a low osmotic pressure

Front 74

isoelectronic

Back 74

having the same number of electrons

Front 75

percent by mass

Back 75

percent by mass = total mass of solute/mass of solution x 100

Front 76

percent by volume

Back 76

percent by volume = volume of solute/volume of solution x 100

Front 77

mass volume percent

Back 77

mass-volume percent = mass of solute (g)/ volume of solution (mL) x 100