Exam 1

Front 1

Chemistry

Back 1

the study of composition, structure, properties, and reactions of matter

Front 2

Matter

Back 2

anything that occupies space and mass, which can be classified by state and by composition

Front 3

Chemical

Back 3

substance that has the same composition and property wherever it is found

Front 4

Scientific Method

Back 4

a general approach that scientists use to solve problems

Four parts: observations, hypothesis, experiment, theory

Front 5

Observations

Back 5

what a scientist sees

Qualitative

Quantitative

Front 6

Hypothesis

Back 6

proposed explanation of an observation

Front 7

Experiment

Back 7

procedural steps to test hypothesis

Front 8

Theory

Back 8

prediction of behavior based on experiment

underlying cause

Front 9

Mass

Back 9

kilogram

kg

Front 10

Length

Back 10

meter

m

Front 11

Time

Back 11

second

s

Front 12

Temperature

Back 12

Kelvin

K

Front 13

Amount of substance

Back 13

mole

mol

Front 14

mega-

Back 14

10^6

M

Front 15

kilo-

Back 15

10^3

k

Front 16

hecto-

Back 16

10^2

h

Front 17

deca-

Back 17

10^1

da

Front 18

deci-

Back 18

10^-1

d

Front 19

centi-

Back 19

10^-2

c

Front 20

milli-

Back 20

10^-3

m

Front 21

micro-

Back 21

10^-6

µ

Front 22

nano-

Back 22

10^-9

n

Front 23

Precision

Back 23

depends on the number of times you get the same results

Front 24

Accuracy

Back 24

depends on the degree of closeness to the actual value

Front 25

Percent error

Back 25

determines how well you performed your experiment compared to a perfect experiment

percent error = 100% * [(experimentally determined - calculated value) / calculated value]

Front 26

Density

Back 26

describes how much an object weighs compared to its size

d = mass/volume

conversion factor and formula

Front 27

Matter

Back 27

anything that occupies space and mas, which can be classifies by composition and by state

Front 28

Composition of Matter

Back 28

pure substance or mixture

Front 29

Pure substance

Back 29

a substance containing only one type of atom or molecule

can be element or compound

Front 30

Mixture

Back 30

a substance composed of two or more different types of atoms or molecules that can be combined in variable proportions

heterogeneous (visible parts) or homogeneous (non visible parts)

Front 31

Decanting

Back 31

separates a liquid and a solid via carefully pouring off the liquid leaving the solid behind

Front 32

Filtration

Back 32

separates a solid and a liquid via pouring the mixture through a filter, which the liquid passes through but not the solid

Front 33

Distillation

Back 33

separates a miscible (mixes equally in all proportions) liquid by boiling off the one with the lower boiling point

Front 34

Solid

Back 34

fixed shape and volume

noncompressible

Front 35

Liquid

Back 35

variable shape

fixed volume

noncompressible

Front 36

Gas

Back 36

variable shape and volume

compressible

Front 37

Physical properties

Back 37

describe the APPEARANCE of the type of matter

extensive and intensive

Front 38

Extensive property

Back 38

depends on the amount of substance present

Ex: mass and volume

can change

extra

Front 39

Intensive property

Back 39

does not depend on the amount of substance present

Ex: density and boiling point

doesn't change

Front 40

Chemical property

Back 40

one that substance diplays only by changing its composition via a chemical change

Ex: flammability of gasoline

Front 41

Energy

Back 41

the capacity to do work

Joule (J)

Front 42

Kinetic energy

Back 42

energy of motion

Ex: running

Front 43

Potential energy

Back 43

the amount of energy that results from an objects position

Front 44

Heat of a substance (q)

Back 44

can either be absorbed (q) or released (-q)

q = m*SH(c)∆t

Front 45

Protein

Back 45

17 kJ/g 4 kcal/g

Front 46

Carbohydrate

Back 46

17 kJ/g 4 kcal/g

Front 47

Fat

Back 47

38 kJ/g 9 kcal/g

Front 48

Si

Back 48

silicon

Front 49

Sc

Back 49

scandium

Front 50

V

Back 50

vanadium

Front 51

Cr

Back 51

chromium

Front 52

Mn

Back 52

manganese

Front 53

Co

Back 53

colbalt

Front 54

Zr

Back 54

zirconium

Front 55

Mo

Back 55

molybdenum

Front 56

Pd

Back 56

Palladium

Front 57

Ag

Back 57

silver

Front 58

Sn

Back 58

tin

Front 59

I

Back 59

iodine

Front 60

Xe

Back 60

xenon

Front 61

Cs

Back 61

Cesium

Front 62

Ba

Back 62

barium

Front 63

La

Back 63

lanthanum

Front 64

Ga

Back 64

gallium

Front 65

Ge

Back 65

germanium

Front 66

As

Back 66

arsenic

Front 67

Se

Back 67

selenium

Front 68

Br

Back 68

bromine

Front 69

Kr

Back 69

krypton

Front 70

Rb

Back 70

rubidium

Front 71

Sr

Back 71

strontium

Front 72

Zr

Back 72

zirconium

Front 73

Pd

Back 73

palladium

Front 74

Cs

Back 74

cesium

Front 75

La

Back 75

lanthanum

Front 76

W

Back 76

tungsten

Front 77

Pt

Back 77

plantinum

Front 78

Hg

Back 78

mercury

Front 79

Pb

Back 79

lead

Front 80

Bi

Back 80

bismuth

Front 81

At

Back 81

astatine

Front 82

Rn

Back 82

radon

Front 83

Fr

Back 83

francium

Front 84

Ac

Back 84

actinium

Front 85

U

Back 85

uranium

Front 86

elements

Back 86

the fundamental building blocks of matter

116 of them

arranged in periodic table

Front 87

Periodic law

Back 87

Dmitri Mendeleev

when elements are arranged in order of increasing mass; certain sets of properties recur periodically

Front 88

Periods

Back 88

rows of the periodic table

Front 89

Groups

Back 89

columns with special names because of similarity of the chemical properties within

Front 90

Metals

Back 90

comprise most of elements

usually lose e- when involved in chemical reactions

make good electrical and thermal conductors

Front 91

Nonmetals

Back 91

located near the top right of the periodic table

usually gain electrons from metals and share electrons with nonmetals in reaction

Front 92

Metalloids (semi-metals or semi-conductors)

Back 92

both metal and nonmetal propeties

can be found in region of table between metals and nonmetal

B, Si, Ge, As, Sb, Te

Front 93

Group 1A- Li, Na, K, Rb, Cs, Fr

Back 93

Alkali metals

solid at room temp

react violently with water

Front 94

Group 2A- Be, Mg, Ca, Sr, Ba, Ra

Back 94

Alkaline Earth Metals

Solid at room temperature

React vigorously with oxygen

Front 95

Group 7A- F, Cl, Br, I, At

Back 95

Halogens

Mostly gas at room temp

Forms salts when bonded to a metal

Front 96

Group 8A- He, Ne, Ar, Kr, Xe, Rn

Back 96

Noble gases

Gases at room temp

Monatomic gases

Front 97

Groups A

Back 97

Representative elements

Front 98

1B-8B

Back 98

Transition metals

mostly solid at room temp

can form complex ions

Front 99

Diatomics

Back 99

Have (H2) No (N2) Fear (F2) Of (O2) Ice (I2) Cold (Cl2) Beer (Br2)

Front 100

Dalton's Atomic Theory of Matter

Back 100

Law of Conservation of Mass

Law of Definite Proportions

Law of Multiple Proportions

1. All matter is made of atoms. Atoms are indivible and indestructable

2. All atoms of a given element are indentical both in mass and in chemical properties

3. Atoms combine in simple, fixed whole number ratios to form compounds

4. Atoms are not created or destroyed in a chemical reaction

Front 101

J.J. Thompson

Back 101

Cathode ray tube

discovered electron

Front 102

Robert Millikan

Back 102

oil drop experiment

charge of electron

Front 103

Francis W. Aston

Back 103

Masses of isotopes

spectrograph

Front 104

Ernest Rutherford

Back 104

Proton and nucleus

gold foil experiment

Front 105

James Chadwick

Back 105

neutrons

Front 106

Atomic number

Back 106

proton number

Front 107

Mass number

Back 107

protons + neutrons

Front 108

Isotope

Back 108

variation of an element that has the same number of protons and electrons, but has a different number of neutrons

Front 109

Relative abundance

Back 109

percentage of an isotope that exists in nature

sum of all = 100%

Front 110

Avg atomic mass=

Back 110

(1st isotope mass)(Rel. Abundance) +......

Front 111

What does n describe?

Back 111

level or shell 1, 2, 3, 4, etc.

indicates the relative distance of the orbital from the nucleus

the higher the number, the greater the distance of the electrons from the nucleus

Front 112

Subshell

Back 112

where you can find electrons with the identical energy

indicates the shape

identified as s < p < d < f (energy wise)

Max number of possible subshells in each level = n

Front 113

1s obital

Back 113

spherical shape

Front 114

3p orbitals

Back 114

dumbbell shape

Front 115

5d orbitals

Back 115

double dumbbell and double dumbbell with a taurus shape

Front 116

Pauli exclusion principle

Back 116

an atomic orbital can hold a maximum of 2 electrons

Front 117

Total number of orbitals in a shell =

Back 117

n^2

Front 118

Total number of electrons in a shell =

Back 118

2 * n^2

Front 119

Orbital Diagram

Back 119

shows how electrons are arranged in orbitals in order of increasing energy

Front 120

Aufbau priciple

Back 120

to build up

Front 121

Hund's rule

Back 121

fill in each orbital with 1 electron first and then go back and fill in the rest

Front 122

Electron configuration for Cr

Back 122

[Ar] 3d^5 4s^1

Front 123

Electron configuration for Cu

Back 123

[Ar] 3d^10 4s^1