Ap Chemistry Pearson Test Prep Topic One

Front 1

Matter

Back 1

classified as pure substances or mixtures

Front 2

Pure substances

Back 2

either elements or compounds

Front 3

element

Back 3

substance all of whose atoms contain the same number of protons

Front 4

compound

Back 4

relatively stable combination of two or more chemically bonded elements in a specific ration

Front 5

mixtures

Back 5

consist of two or more substances

Front 6

physical properties

Back 6

can be measured without changing the identity or composition of the substance

Front 7

chemical properties

Back 7

describe the way a substance changes to form other substances.

Front 8

intensive properties

Back 8

do not depend on the amount of substance in a sample, examples are temperature, density, and boiling point

Front 9

extensive properties

Back 9

depend on the quantity of the sample, examples are energy content, mass, and volume

Front 10

physical change

Back 10

changes the appearance of a substance but does not change its composition

Front 11

chemical change

Back 11

transforms a substance into a different substance or substances

Front 12

filtration

Back 12

separates a solid from a liquid

Front 13

distillation

Back 13

separates substances based on their differences in boiling points

Front 14

chromatography

Back 14

a technique that separates substances based on their differences in intermolecular forces and their abilities to dissolve in various solvents

Front 15

SI units

Back 15

mass- grams
length- meter
time- seconde
temperature - kelvin
amount of substance - Mole
Electric current Ampere - A
Luminous intensity- Candela - cd

Front 16

Unit Prefixes from highest to lowest

Back 16

Giga, G, 10^9
Mega, M, 10^6
Kilo, k, 10^3
Deci, d, 10^-1
Centi, c, 10^-2
Milli, m, 10^-3
Micro, (mew), 10^-6
Nano, n, 10^-9
Pico, p, 10^-12
Femto, f, 10^-15

Front 17

Kelvin to celsius equation

Back 17

K=C+273

Front 18

cm^3 to mL

Back 18

cm^3 = 1 mL

Front 19

When Zeros are significant

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1)Those btwn nonzero digits are significant
2)those at the beginning are never significant
3) those at the end are significant only when the number contains a decimal point

Front 20

sig figs for multiplication

Back 20

number of sig figs determined by measure with fewest sig figs

Front 21

sig figs for addition

Back 21

fewest number of decimal places

Front 22

John Dalton

Back 22

proposed that matter is composed of tinyh paritcles called atoms. They combined to form compounds and exist as a number of different elements.

Front 23

J.J. Thomson

Back 23

Showed that cathode rays are streams of negative particles. Discovered the electrona and measured its charge to mass ration. All atoms contain electrons.

Front 24

Robert Millikan

Back 24

measured the charge of an electrona and calculated its mass.

Front 25

Henri Becquerel

Back 25

Discovered Radioactivity

Front 26

Ernest Rutherford

Back 26

characterized radioactivity as three types of radiation, alpha, beta, and gamma rays. He discovered the atomic nucleus and the proton and showed that atoms were mostly empty space.

Front 27

James Chadwick

Back 27

discovered the neutron

Front 28

atomic number

Back 28

number of protons, defined the atom

Front 29

mass number

Back 29

number of protons and neutrons in the nucleus

Front 30

Isotopes

Back 30

atoms of identical atomic numbers but different mass numbers

Front 31

atomic mass unit

Back 31

one amu equals 1.66054 X 10^-24g a carbon-12 (mass number) has 12 amus

Front 32

Atomic mass

Back 32

the wieghted average mass of allthe isotopes of an element

Front 33

Group 1A

Back 33

alkali metals

Front 34

Group 2A

Back 34

alkaline earth metals

Front 35

group 7A

Back 35

halogens

Front 36

group 8A

Back 36

noble gases

Front 37

Diatomic Elements

Back 37

H,O,N,F,Cl,Br,I

Front 38

compounds vs. molecules

Back 38

comounds consist of two or more different elements

Front 39

molecular compounds

Back 39

usually contain only nonmetals

Front 40

Ions

Back 40

charged particles comprised of single atoms or aggregates of atoms,either cation and an anion

Front 41

Ionic compounds

Back 41

composed of ions usually containing both metals and nonmetals

Front 42

Naming monatomic cations

Back 42

have the same name as the metal, potassium ion K+, cobalt (II) ion Co2+

Front 43

Transition metals

Back 43

B group elements

Front 44

non-transition metals

Back 44

A group metals

Front 45

transition metals that only form a single type of charge

Back 45

scandium ion,Sc3+
silver ion, Ag+
zinc ion, Zn2+
cadmium ion, Cd2+
-all the others have 2 or more and must be written with roman numerals

Front 46

non-transition metals that form more than 1 type of charge

Back 46

tin(II) ion, tin (IV) ion,Sn
lead(II) ion, lead (IV) ion,Pb
-all the others have only one type and are written without roman numerals

Front 47

naming monatomic anions

Back 47

replace the end of the element name with ide

Front 48

monatomic anions group 1A

Back 48

hydride

Front 49

monatomic anions group 5A

Back 49

nitride

Front 50

monatomic anions group 6A

Back 50

Oxide, sulfide, selenide (Se2-), telluride (Te2-)

Front 51

monatomic anions group 7A

Back 51

fluoride, chloride, bromide, iodide

Front 52

diatomic anions also ending in ide

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hydroxide (OH-), cyanide (CN-), peroxide (2O2-)

Front 53

naming polyatomic cations

Back 53

end in ium

Front 54

polyatomic cations you should know

Back 54

ammonium NH4(+), methylammonium, CH3NH3(+)
dimethylammonium (CH3)2(NH2)(+)

Front 55

(no per or hypo) Polyatomic Oxyanions with -1 charge

Back 55

phosphate PO4(3-)

Front 56

(no per or hypo) Polyatomic Oxyanions with -2 charge

Back 56

hydrogen phosphate HPO4(2-)
sulfate SO4(2-)
carbonate CO3 (2-)

Front 57

(no per or hyp) polyatomic oxyanions with -1 charge

Back 57

dihydrogen phosphate H2PO4(-)
hydrogen sulfate HSO4(-)
hydrogen carbonate HCO3(-)
nitrate NO3(-)
acetate CH3COO(-)

Front 58

naming polyatomic oxyanions

Back 58

end either in ate or ite, ate denotes the most common oxuanion, ite refers to an oxyanion having the some charge but one fewer oxygen

Front 59

prefixes of halogen oxyanions

Back 59

hypochlorate ClO(-)
chlorite ClO2 (-)
chlorate ClO3 (-)
perchlorate (ClO4)(-)

Front 60

naming ionic compounds

Back 60

consist of the cation name followed by the anion name, magnesium bromide MgBr2, calcium phosphate Ca2(PO4)2
Iron(III)oxide Fe2O3

Front 61

naming acids

Back 61

binary acids contain monatomic ions and oxyacids contain oxyanions (study list on page 15)

Front 62

naming binary molecular compounds

Back 62

1. Name the first element (the one that is least electronegative)
2. name the second giving it an ide ending
3.use prefixes (mono,di,tri, tetra, penta, hexa, hepta, octa, nona, deca) for each elements except if the first element is only one atom