Chemistry Exam Review

Front 1

scientific method

Back 1

question, research, hypothesis, experiment, analyze results/conclusion, report results

Front 2

bunsen burner rules

Back 2

tie back hair, light match before turning on gas valve, stand to the side while lighting

Front 3

glassware rules

Back 3

do not use cracked/chipped glass, make sure glassware is safe to heat, do not heat graduated cylinders, clean glassware before and after you use it, never use bare hands to pick up broken glass

Front 4

SI units

Back 4

mass-gram, length- meter, time-second, temperature- Kelvin, amount of substance- mole

Front 5

metric conversion chart

Back 5

Mega Kilo Hecto Deca Meter(gram/liter) deci centi milli micro nano pico

Front 6

1 liter=
l liter=
l mL=

Back 6

10 cubic centimeters
1 cubic decimeter
1 cubic centimeter

Front 7

Precision

Back 7

consistency, limited by smallest value on measurement scale

Front 8

Accuracy

Back 8

extent to which a group of data agrees with accepted value

Front 9

Sig Fig rules

Back 9

1. all non-zero digits are significant
2. everything after decimal is significant
3. everything in between sig figs is significant
4. if there is a sig fig and a decimal, everything before decimal is significant
5. if there are zeroes and sigfigs after decimal, and non zero before decimal, all are significant
6. defined unit=infinite number of sig figs

Front 10

rules for multiplying/dividing sig figs

Back 10

take last answer and round it to the smallest number of sig figs in problem

Front 11

rules for adding/subtracting sig figs

Back 11

final answer must have least number of decimal places in problem

Front 12

scientific notation

Back 12

when power gets smaller, number gets bigger; when power gets bigger, number gets smaller

Front 13

adding and subtracting= scientific notation

Back 13

both terms have to have the same power

Front 14

multiplying scientific notation

Back 14

multiply numbers first, then add the powers!

Front 15

dimensional analysis

Back 15

horizontal line= division; vertical line= multiplication

Front 16

density

Back 16

d=m/v
*remember the triangle*

Front 17

intensive property
extensive property

Back 17

-does not depend on amt. of substance
-depends on amt. of substance

Front 18

physical property
physical change

Back 18

-can be observed without changing composition
-alters a substance without changing composition

Front 19

chemical property
chemical change

Back 19

-ability of substance to combine with or change into one or more substances
-one or more substances change into new substances

Front 20

evidence of chemical change

Back 20

bubbling(release of gas); color change; change in odor; release of heat

Front 21

solid

Back 21

does not flow, does not compress, expands slighty when heated, very closely packed, definite volume

Front 22

liquid

Back 22

flows, does not compress, expands when heated, lass closely packed, constant volume

Front 23

gas

Back 23

flows, compressible, free, rapid movement, far apart molecules, conforms to shape of container

Front 24

Law of Conservation of Mass

Back 24

mass is neither created or destroyed during a chamical reaction , it is rearranged

Front 25

Law of Definite Proportions

Back 25

a compound is always made of the same elements in the same proportions by mass

Front 26

Law of Multiple Proportions

Back 26

different compounds can be made by using the same elements in different proportions

Front 27

Democritus

Back 27

matter is made up of solid, indivisible atoms

Front 28

Aristotle

Back 28

rejected Democritus's thoery

Front 29

John Dalton

Back 29

Modern Atomic Theory- matter is made up of indivisible atoms, all atoms of a given element are identical, different atoms combine into whole number ratios to make compounds

Front 30

William Crooke

Back 30

found cathode ray when noticed a flas of light in a tube mode made by rays striking a light producing coating(stream of negatively charged particles)

Front 31

J.J. Thomson

Back 31

"plum pudding model"; found electrons by testing to determine ration of charge to mass with cathode rays, mass of charged particle=much less than lightest known hydrogen atom

Front 32

Ernest Rutherford

Back 32

found nucleus, and later... protons!; tested to see if gold foil atoms would deflect positively charged alpha particles=were major and minor deflections

Front 33

James Chadwick

Back 33

discovered neutrons

Front 34

atomic number-
mass number-

Back 34

-number of protons
-protons+neutrons

Front 35

isotopes-

Back 35

-when the number of protons in an atom of an element is the same, but there are different number of neutrons

Front 36

isotopes with more neutrons have a...

Back 36

larger mass

Front 37

atomic mass

Back 37

weighted average of mass numbers of all isotopes

Front 38

Aufbau principle

Back 38

each electron occupies lowest energy level available

Front 39

Pauli Exclusion Principle

Back 39

maximum of two electrons with opposite spin in one orbital

Front 40

Hund's Rule

Back 40

single electrons with the same spin must occupy each equal energy orbital before electrons with opposite spins occupy the same orbital

Front 41

electromagnetic spectrum

Back 41

radio, microwaves, infrared, visible light (ROGYBV), ultraviolet, x-ray, gamma

Front 42

electromagnetic spectrum diagram (left to right)

Back 42

frequency increases, energy increases, wavelength decreases

Front 43

when atoms are in an excited state....

Back 43

electrons move to higher energy levels and absorb energy

Front 44

when atoms reture to ground state.....

Back 44

electrons return to normal energy levels and release energy in different colors (atomic emission spectrum)

Front 45

atomic emission spectrum diagram (left to right)

Back 45

frequency decreases, energy decreases, wavelength increases

Front 46

Newlands

Back 46

every eighth element repeats physical and chemical properties: octave rule

Front 47

Meyer

Back 47

demonstrated connection between atomic mass and elemental properties

Front 48

Mendeleev

Back 48

first periodic table by atomic mass; left spaces where he thought undiscovered elements should go

Front 49

Mosley

Back 49

arranged periodic table by atomic number; periodic law

Front 50

energy...

Back 50

increases in the order of filling orbitals

Front 51

as you go across a period

Back 51

atomic radius decreases, ionic radius decreases (1a-4a, 5a-8a), electronegativity and ionization potential energy increases

Front 52

as you go down a group

Back 52

atomic radius increases, ionic radius increases, electronegativity and IPE decreases

Front 53

chemical bond

Back 53

force that holds two atoms together

Front 54

atoms form ions to....

Back 54

resemble noble gasses (octet rule)

Front 55

cation-
anion-

Back 55

-electrons are lost (+charge)
-electrons are gained(-charge)

Front 56

ionic bond

Back 56

metal and a nonmetal; form when cation and anion close to eachother attract, forming a tightly packed geometric crystal lattice

Front 57

lattice energy...

Back 57

is needed to break the force of attraction between oppositely charged ions arranged in a crystal lattice

Front 58

physical properties of ionic solids...

Back 58

are related to strength of ionic bonds and presence of ions

Front 59

ionic compound is an...

Back 59

electrolyte(conducts electricity as a liquid or acqueous solution)

Front 60

convalent bond

Back 60

formed when atoms share electrons; 2 nonmetals

Front 61

1st covalent bond-
2nd covalent bond-

Back 61

sigma
pi

Front 62

bond length depends on...

Back 62

size of bonded atoms and number of electron pairs they share

Front 63

naming covalent molecules

Back 63

use prefixes to show amount of each element

Front 64

all acids need a

Back 64

H atom

Front 65

naming binary acids...

Back 65

always has "hydro" in front; replaces last part of element with "ic"

Front 66

naming oxyacids...

Back 66

no hydro in front!; polyatomic with H atom; ends in ite/ate, replaces with ous/ic

Front 67

naming ionic compounds...

Back 67

cation first, then anion; 1st element=normal name, second ends in -ide; put oxidation #'s of transition metals in parentheses; polyatomic always stays the same!

Front 68

diatomics...

Back 68

BIG SEVEN! cannot exist on their own...always paired with same element

Front 69

all polar bonds are....

Back 69

dipoles; asymmetrical; any central atom with a lone pair is polar

Front 70

resonance structure-

Back 70

can change the position of double bonds

Front 71

5 types of chemical reactions

Back 71

synthesis, decomposition, combustion, single replacement, double replacement

Front 72

endothermic

Back 72

energy is absorbed

Front 73

exothermic

Back 73

energy is released

Front 74

STUDY POLYATOMIC...

Back 74

AND MOLECULAR SHAPES CHART!