Chemistry Exam

Front 1

quantitative observation

Back 1

involves numbers

Front 2

qualitative observation

Back 2

involves descriptions

Front 3

celsius to kelvin

Back 3

k=c+273

Front 4

celsius to fahrenheit

Back 4

f=1.8c+32

Front 5

density

Back 5

density=mass/volume

Front 6

accuracy

Back 6

how close a measured value is to an accepted or true value

Front 7

precision

Back 7

how close a series of measurements are to one another

Front 8

percent error

Back 8

accepted value-experimental
percent error---------------------
accepted value

Front 9

gases

Back 9

indefinite shape indefinite volume

Front 10

liquids

Back 10

definite volume indefinite shape

Front 11

solids

Back 11

definite shape definite volume

Front 12

physical properties

Back 12

describe the appearance of matter

state, color, volume, odor, taste, hardness, density, solubility, melting/boiling point.

Front 13

extensive properties

Back 13

dependent upon the amount of substance present

mass, length and volume

Front 14

intensive properties

Back 14

independent of the amount of substance present.

density, color, temperature, hardness, melting point, boiling point, pressure, and molecular weight

Front 15

physical changes

Back 15

the form but not the identity of matter changes

bend, crumple, split, crush, boil, freeze, condense, vaporize, or melt
**if after the substance undergoes the change and can still be identified as the original substance it is a physical change**

Front 16

solid--> liquid

Back 16

melting

Front 17

gas--> liquid

Back 17

condensing

Front 18

solid-->gas

Back 18

sublimation

Front 19

liquid--> solid

Back 19

freezing

Front 20

gas--> solid

Back 20

reverse sublimation

Front 21

liquid--> gas

Back 21

evaporation

Front 22

chemical property

Back 22

the ability of a substance to combine with or change into one or more other substances. describes how matter behaves when it changes into another kind of matter

Front 23

chemical change

Back 23

process that involves one or more substances changing into new substances. also called chemical reaction

explode, rust, cook, oxidize, corrode, tarnish, ferment, burn, or rot.

Front 24

element

Back 24

pure substance that cannot be broken down into other substances by chemical means

Front 25

compound

Back 25

when two or more elements combine in a fixed composition by weight. can be broken down into simpler substances by chemical means

Front 26

law of definite proportions

Back 26

regardless of amount, a compound is always composed of the same elements in the same proportion by mass.

Front 27

percent by mass

Back 27

mass of element
% by mass=--------------- x 100
mass of compound

Front 28

mixture

Back 28

something that has variable composition and is made of a number of pure substances and each pure substance retains its individual properties

wood, wine, coffee, air

Front 29

pure substance

Back 29

always has the same composition like
elements and compounds

purified water

Front 30

homogeneous mixture

Back 30

the same throughout.

salt water

Front 31

solid--> liquid

Back 31

melting

Front 32

gas--> liquid

Back 32

condensing

Front 33

solid-->gas

Back 33

sublimation

Front 34

liquid--> solid

Back 34

freezing

Front 35

gas--> solid

Back 35

reverse sublimation

Front 36

liquid--> gas

Back 36

evaporation

Front 37

chemical property

Back 37

the ability of a substance to combine with or change into one or more other substances. describes how matter behaves when it changes into another kind of matter

Front 38

chemical change

Back 38

process that involves one or more substances changing into new substances. also called chemical reaction

explode, rust, cook, oxidize, corrode, tarnish, ferment, burn, or rot.

Front 39

element

Back 39

pure substance that cannot be broken down into other substances by chemical means

Front 40

compound

Back 40

when two or more elements combine in a fixed composition by weight. can be broken down into simpler substances by chemical means

Front 41

law of definite proportions

Back 41

regardless of amount, a compound is always composed of the same elements in the same proportion by mass.

Front 42

percent by mass

Back 42

mass of element
% by mass=--------------- x 100
mass of compound

Front 43

mixture

Back 43

something that has variable composition and is made of a number of pure substances and each pure substance retains its individual properties

wood, wine, coffee, air

Front 44

pure substance

Back 44

always has the same composition like
elements and compounds

purified water

Front 45

homogeneous mixture

Back 45

the same throughout. also called a solution

salt water, cough syrup, lemonade, air, brass (made of copper and zinc)

Front 46

heterogeneous mixture

Back 46

contains regions that have different properties from those of other regions

sand water

Front 47

filtration

Back 47

used to separate an insoluble solid from a liquid

pour mixture onto a mesh or filter paper which allows the liquid to pass through and leaves the solid behind

Front 48

distillation

Back 48

used to separate either a liquid from a soluble solid or two liquids with different boiling points

Front 49

distillation of liquid from soluble solid

Back 49

mixture is heated to boiling state so liquid will evaporate and rise into the condenser where it returns back to liquid state leaving the solid behind

Front 50

distillation of two liquids

Back 50

mixture is heated to one of the liquid's boiling points so that liquid evaporates leaving the liquid with the higher boiling point behind.

Front 51

energy

Back 51

the ability to do work or produce heat
measured in joules (J) or calories

**1 calorie= 4.184 J**

Front 52

potential energy

Back 52

energy due to composition or position of an object
also known as death from physics las year

Front 53

kinetic energy

Back 53

the energy of motion
or potential energy's partner in crime

Front 54

law of conservation of energy

Back 54

in any chemical reaction or physical process, energy can be converted from one for to another but it is neither created nor destroyed

Front 55

calorie

Back 55

amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius

Front 56

specific heat capacity

Back 56

the amount of energy required to change the temperature of one gram of that substance by one degree Celsius

Energy (heat) required= SHC x mass x change in temp. ºC
or
Q = s x m x change in temp ºC
unit: J/gºC

Front 57

exothermic process

Back 57

when heat is transferred from the system to the surroundings

freezing, wood that is burning

Front 58

endothermic process

Back 58

when heat is transferred to the system from the surroundings

melting,

Front 59

Dalton's Atomic Theory

Back 59

1. All matter is composed of tiny particles called atoms
2. All atoms of a given element are identical
3. The atoms of a specific element are different to those of any other element
4. atoms of different elements combine to form compounds. compounds have a fixed composition known as the law of definite proportion
5. atoms cannot be created, divided in small particles, or destroyed. in a chemical reaction they are simply rearranged to form new compounds.

Front 60

JJ Thompson

Back 60

discovered the electron and it's mass using negative cathode rays

Front 61

heterogeneous mixture

Back 61

contains regions that have different properties from those of other regions

sand water

Front 62

filtration

Back 62

used to separate an insoluble solid from a liquid

pour mixture onto a mesh or filter paper which allows the liquid to pass through and leaves the solid behind

Front 63

distillation

Back 63

used to separate either a liquid from a soluble solid or two liquids with different boiling points

Front 64

distillation of liquid from soluble solid

Back 64

mixture is heated to boiling state so liquid will evaporate and rise into the condenser where it returns back to liquid state leaving the solid behind

Front 65

distillation of two liquids

Back 65

mixture is heated to one of the liquid's boiling points so that liquid evaporates leaving the liquid with the higher boiling point behind.

Front 66

energy

Back 66

the ability to do work or produce heat
measured in joules (J) or calories

**1 calorie= 4.184 J**

Front 67

potential energy

Back 67

energy due to composition or position of an object
also known as death from physics las year

Front 68

kinetic energy

Back 68

the energy of motion
or potential energy's partner in crime

Front 69

law of conservation of energy

Back 69

in any chemical reaction or physical process, energy can be converted from one for to another but it is neither created nor destroyed

Front 70

calorie

Back 70

amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius

Front 71

specific heat capacity

Back 71

the amount of energy required to change the temperature of one gram of that substance by one degree Celsius

Energy (heat) required= SHC x mass x change in temp. ºC
or
Q = s x m x change in temp ºC
unit: J/gºC

Front 72

exothermic process

Back 72

when heat is transferred from the system to the surroundings

freezing, wood that is burning

Front 73

endothermic process

Back 73

when heat is transferred to the system from the surroundings

melting,

Front 74

Dalton's Atomic Theory

Back 74

1. All matter is composed of tiny particles called atoms
2. All atoms of a given element are identical
3. The atoms of a specific element are different to those of any other element
4. atoms of different elements combine to form compounds. compounds have a fixed composition known as the law of definite proportion
5. atoms cannot be created, divided in small particles, or destroyed. in a chemical reaction they are simply rearranged to form new compounds.

Front 75

JJ Thompson

Back 75

discovered the electron using negative cathode rays

Front 76

heterogeneous mixture

Back 76

contains regions that have different properties from those of other regions

sand water

Front 77

filtration

Back 77

used to separate an insoluble solid from a liquid

pour mixture onto a mesh or filter paper which allows the liquid to pass through and leaves the solid behind

Front 78

distillation

Back 78

used to separate either a liquid from a soluble solid or two liquids with different boiling points

Front 79

distillation of liquid from soluble solid

Back 79

mixture is heated to boiling state so liquid will evaporate and rise into the condenser where it returns back to liquid state leaving the solid behind

Front 80

distillation of two liquids

Back 80

mixture is heated to one of the liquid's boiling points so that liquid evaporates leaving the liquid with the higher boiling point behind.

Front 81

energy

Back 81

the ability to do work or produce heat
measured in joules (J) or calories

**1 calorie= 4.184 J**

Front 82

potential energy

Back 82

energy due to composition or position of an object
also known as death from physics las year

Front 83

kinetic energy

Back 83

the energy of motion
or potential energy's partner in crime

Front 84

law of conservation of energy

Back 84

in any chemical reaction or physical process, energy can be converted from one for to another but it is neither created nor destroyed

Front 85

calorie

Back 85

amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius

Front 86

specific heat capacity

Back 86

the amount of energy required to change the temperature of one gram of that substance by one degree Celsius

Energy (heat) required= SHC x mass x change in temp. ºC
or
Q = s x m x change in temp ºC
unit: J/gºC

Front 87

exothermic process

Back 87

when heat is transferred from the system to the surroundings

freezing, wood that is burning

Front 88

endothermic process

Back 88

when heat is transferred to the system from the surroundings

melting,

Front 89

Dalton's Atomic Theory

Back 89

1. All matter is composed of tiny particles called atoms
2. All atoms of a given element are identical
3. The atoms of a specific element are different to those of any other element
4. atoms of different elements combine to form compounds. compounds have a fixed composition known as the law of definite proportion
5. atoms cannot be created, divided in small particles, or destroyed. in a chemical reaction they are simply rearranged to form new compounds.

Front 90

JJ Thompson

Back 90

discovered the electron using negative cathode rays
also constructed plum pudding model

Front 91

Robert Millikan

Back 91

determined exact mass and charge or the electron

Front 92

Ernest Rutherford

Back 92

designed experiment involving directing alpha (+) particles towards a thin metal foil. surrounding the foil was a detector coated with a substance that produced tiny flashes wherever it was hit by an alpha particle. he discovered that some particles were deflected at angles and some straight back and some passed through concluding that atoms had a small positively charged center called a nucleus containing protons

Front 93

James Chadwick

Back 93

discovered the nucleus also contained neutral particle called the neutron with the same mass as a proton

Front 94

atomic number

Back 94

the number of protons in the nucleus of the atom
also tells us the number of electrons

Front 95

mass number

Back 95

number of protons + neutrons

Front 96

Isotope

Back 96

an atom with the same number of protons and electrons but different number of neutrons

Front 97

metals

Back 97

good conductors of heat and electricity, usually shiny in appearance, and most are solid at room temp.

Front 98

Diatomic molecules

Back 98

molecules mad up of 2 atoms of the same element
***HOFBrINCl***

Front 99

ion

Back 99

an atom that has lost or gained an electron

Front 100

cations

Back 100

atoms that have lost electrons and are positively charged

Front 101

anions

Back 101

atoms that have gained an electron and are negatively charged

Front 102

ionic compounds

Back 102

compounds that contain a metal and a nonmetal

Front 103

molecular compounds

Back 103

compounds that contain two nonmetals

Front 104

type II binary compound prefixes

Back 104

mono...1
di...2
tri...3
tetra...4
penta...5
hexa...6
hepta...7
octa...8

Front 105

acid

Back 105

a compound that produces hydrogen ions when dissolved in water

Front 106

aqueous solutions

Back 106

a substance dissolved in water.

Front 107

strong electrolyte

Back 107

when a large number of ions are present in a solution, the solution will be an excellent conductor of electricity.
any aqueous ionic compound

Front 108

weak electrolyte

Back 108

does not conduct electricity well
molecular compound

Front 109

Precipitation Reactions

Back 109

formation of a solid
double displacement reaction
***memorize solubility rules***

Front 110

spectator ions

Back 110

ions that do not participate in the reaction.

Front 111

acid-base reactions

Back 111

formation of water
double displacement reaction
acid+base-->salt+water

Front 112

strong acids

Back 112

HCl, HBr, HI, HClO4, HNO3, H2SO4
**all numbers are subscript**

Front 113

strong bases

Back 113

group 1 and Ca, Sr, Ba with hydroxide

Front 114

Oxidation Reduction (REDOX) reactions

Back 114

transfer of electrons
element losing electrons become oxidized, element gaining electrons becomes reduced, element being oxidized is reducing agent, element being reduced is oxidizing agent

Front 115

single displacement reaction

Back 115

reactions that form gases
where only a single type of ion has been exchanged between positive ions

Front 116

combustion

Back 116

reactions where oxygen is used to burn fuels to produce energy. products are always CO2 and H2O
C & H +O2--> CO2 + H2O

Front 117

synthesis

Back 117

when two elements combine to form a compound

Front 118

decomposition

Back 118

a reaction where a compound is broken down into simpler substances. opposite of synthesis.

Front 119

Atomic Mass Unit

Back 119

amu
unit for mass of atoms.
**unit of mass of element on periodic table**

Front 120

average atomic mass

Back 120

(m # of 1st x % abundance)+(m # of 2nd...)/100

when writing % abundance keep number in % form. so for 75% use the number 75 rather than .75

Front 121

mole

Back 121

the number equal to the number of atoms in 1g of an element.
6.02x10^23

Front 122

molar mass

Back 122

g of substance/ 1 mole of substance

Front 123

percent composition

Back 123

tot. m of element in 1 mole of compound
--------------------------------
total mass of 1 mole of the compound

Front 124

empirical formula

Back 124

simplest whole number ratio of the atoms of each element in that compound.

Front 125

molecular formula

Back 125

tells us exactly how many atoms of each element are present in the compound rather than just the simplest whole number ratio like in the empirical formula
molar mass of molecular formula
n=--------------------------
molar mass of empirical formula

**molar mass of molecular formula is always given

Front 126

stiochiometry

Back 126

the study of quantitative relationships between amounts of reactants used and the products formed y a chemical reaction

Front 127

percent yield

Back 127

actual yield of product
% Yield=----------------------
theoretical yield of product

Front 128

Electromagnetic radiation

Back 128

one of the ways light travels through space.

Front 129

speed of light

Back 129

c=3x10^8
c=wavelength x frequency

wavelength and frequency are inversely related

Front 130

Electromagnetic spectrum

Back 130

ROYGBIV
red has large wavelength and small frequency
violet has small wavelength and large frequency

Front 131

quantum concept

Back 131

Max Planck concluded that matter can gain or lose energy only in small specific amounts called quanta

Front 132

quantum

Back 132

minimum amount of energy that can be gained or lost by an atom
Equantum = hv
h=6.62x10^-34 Js (joule seconds)
E= energy
v= frequency

Front 133

atomic emission spectra

Back 133

the set of frequencies of the electromagnetic waves emitted by atoms of an element
each element emits a color unique to that element

Front 134

Bohr model of the atom

Back 134

all atoms have a ground state (lowest allowable energy) and an excited state (highest allowable energy)

Front 135

quantum mechanical model of the atom

Back 135

each orbital can be thought of as a fuzzy cloud where an electron may be found
it may not be possible to pin point the exact position of the electron at any one time, but it is possible to say that the electron will be within a certain area called an orbital

Front 136

major difference between the Bohr model and wave mechanical model of the atom

Back 136

in the bohr model, the energy of the electron is described in terms of a definite orbit or pathway. in the wave mechanical model the energy is described in terms of the probability of locating the electron in a region of space outside the nucleus. energy levels are thought of as clouds of electrical charge surrounding the nucleus.... POOP!!!! hahaah : )

Front 137

aufbau principle

Back 137

electrons enter orbitals of lowest energy first

Front 138

pauli exclusion principle

Back 138

2 electrons per orbital with opposite "spins" represented by up and down arrows

Front 139

hund's rule

Back 139

fill orbitals of a given energy one at a time before pairing electrons up.

Front 140

valence electrons

Back 140

the electrons in the outermost principle energy level of an atom.

Front 141

core electrons

Back 141

electrons not involved in bonding

Front 142

CHEMISTRY

Back 142

DEATH!!!!

Front 143

cameron

Back 143

most amazing person ever for making all these flashcards and being wiling to share with everyone!!!