Chemistry

Front 1

Atomic # 1

Back 1

H-hydrogen

Front 2

Atomic # 2

Back 2

He-helium

Front 3

Atomic # 3

Back 3

Li-lithium

Front 4

Atomic # 4

Back 4

Be-beryllium

Front 5

Atomic # 5

Back 5

B-boron

Front 6

Atomic # 6

Back 6

C-carbon

Front 7

Atomic # 7

Back 7

N-nitrogen

Front 8

Atomic # 8

Back 8

O-oxygen

Front 9

Atomic # 9

Back 9

F-fluorine

Front 10

Atomic # 10

Back 10

Ne-neon

Front 11

Atomic # 11

Back 11

Na-sodium

Front 12

Atomic # 12

Back 12

Mg-magnesium

Front 13

Atomic # 13

Back 13

Al-aluminum

Front 14

Atomic # 14

Back 14

Si-silicon

Front 15

Atomic # 15

Back 15

P-phosphorous

Front 16

Atomic # 16

Back 16

S-sulfur

Front 17

Atomic # 17

Back 17

Cl-chlorine

Front 18

Atomic # 18

Back 18

Ar-argon

Front 19

Atomic # 19

Back 19

K-potassium

Front 20

Atomic # 20

Back 20

Ca-calcium

Front 21

Atomic # 24

Back 21

Cr-chromium

Front 22

Atomic # 25

Back 22

Mn-manganese

Front 23

Atomic # 26

Back 23

Fe-iron

Front 24

Atomic # 27

Back 24

Co-cobalt

Front 25

Atomic # 28

Back 25

Ni-nickel

Front 26

Atomic # 29

Back 26

Cu-copper

Front 27

Atomic # 30

Back 27

Zn-zinc

Front 28

Atomic # 34

Back 28

Se-selenium

Front 29

Atomic # 35

Back 29

Br-bromine

Front 30

Atomic # 36

Back 30

Kr-krypton

Front 31

Atomic # 46

Back 31

Pd-palladium

Front 32

Atomic # 47

Back 32

Ag-silver

Front 33

Atomic # 53

Back 33

I-iodine

Front 34

Atomic # 54

Back 34

Xe-xenon

Front 35

Atomic # 78

Back 35

Pt-platinum

Front 36

Atomic # 79

Back 36

Au-gold

Front 37

Atomic # 80

Back 37

Hg-mercury

Front 38

*f to*c

Back 38

*C=5/9(*f-32)

Front 39

*c to *f

Back 39

*f= 9/5*c+32

Front 40

*k

Back 40

*c+273.15

Front 41

*c

Back 41

*k-273.15

Front 42

what are the rules of exponents

Back 42

add exponents when multiplying

subtract exponents when dividing

Front 43

Scientific notation to #

Back 43

a positive exponent means decimal moves to right

a negative exponent means decimal moves to the left

Front 44

# to scientific notation

Back 44

move to the left = positive exponent

move to the right= negative exponent

Front 45

what are isotopes?

Back 45

atoms of same element with same atomic # but different Mass # (diff number of neutrons)

Front 46

atomic number

Back 46

is equal to the number of protons

Front 47

mass number

Back 47

is the sum of protons and neutrons

Front 48

What are ions

Back 48

elements where # of protons is NOT equal to # of electrons

Front 49

what is a cation

Back 49

ion with a positive charge

Front 50

what is an anion

Back 50

ion with a negative charge

Front 51

give ion of Nitrate

Back 51

NO₃⁻

Front 52

Give ion of carbonate

Back 52

CO₃⁻²

Front 53

give ion of chlorate

Back 53

ClO₃⁻

Front 54

give ion of sulfate

Back 54

SO₄⁻²

Front 55

give ion of phosphate

Back 55

PO₄⁻³

Front 56

ion of ammonium

Back 56

NH₄⁺

Front 57

ion of hydroxide

Back 57

OH⁻

Front 58

ion for hydrogen carbonate

Back 58

HCO₃⁻

Front 59

ion for hydrogen sulfate

Back 59

HSO₄⁻

Front 60

ion for hydrogen phosphate

Back 60

HPO₄⁻²

Front 61

rules for naming polyatomic ions

Back 61

taking an oxygen away from an -ite ion makes it a hypo- ion
(NO⁻)= hyponitrite

taking an oxygen away from an -ate ion makes it an -ite ion
(NO₂⁻)=nitrite

Any -ate ion is the most common form
(NO₃⁻)=nitrate

adding an oxygen to common form is a per- ion
(NO₄⁻)=pernitrate

Front 62

rules for naming type I binary ionic compounds

Back 62

1-cation is always named 1st and anion 2nd

2- monoatomic cation keeps its name

3-monoatomic anion is named by adding -ide to root of element

ex: NaCl= sodium chloride

Front 63

rules for naming type II binary ionic compounds

Back 63

1- metal + nonmental+ -ide
2- in simplest form

Transition metals: have no set charge (except Zn⁺² & Ag⁺), so charge in indicated with toman numerals

ex: Fe₂O₃= iron(III) oxide
ex2: Iron(II) oxide=Fe₂O₂=simplified to FeO

polyatomic ions are compounds with 2 or more elements
ex: Li₂SO₄= lithium sulfate

Front 64

common type II cations

Back 64

Fe- Iron (II) and Iron (III)

Cu- Copper (I) and copper (II)

Co- Cobalt (II) and Cobalt (III)

Sn- Tin(IV) and Tin (II)

Pb- Lead(IV) and Lead (II)

Front 65

rules for naming type III binary covalent compounds

Back 65

1- NO simplification

2- between 2 or more NON-metals

3- use PREFIXES and keep -IDE suffic

ex: CF₄= tretraoxide

ex2: N₂O₅= dinitrogen pentoxide

Front 66

prefixes

Back 66

1-mono 6-hexa
2-di 7-hepta
3-tri 8-octa
4-tetra 9-nona
5-penta 10-deca

Front 67

naming binary acids

Back 67

1- only 2 different atoms

2- one atom is ALWAYS a hydrogen

3- other atom is a NON-metal

4- binary acid name ALWAYS begin with hydro- prefix and ends w/ -ic acid

ex: HCl= Hydrochloric acid

Front 68

Naming Polyatomic acids (oxy-acids)

Back 68

1) -ate ion produces -ic acid
ex:HNO₃→ nitrate ion=nitric acid

2)-per_ate ion produces a per_ic acid
ex:HNO₄→pernitrate=pernitic acid

3) -ite ion produces -ous acid
ex:HNO₂→nitrite=nitrous acid

4) hypo__ite ion produces hypo__ous acid
ex:HNO→hyponitrite=hyponitrous acid

Front 69

give ion of polyatomic mercury (I)

Back 69

Hg₂⁺²

Front 70

Give ion of Ammonium

Back 70

NH₄⁺

Front 71

Give ion of hydroxide

Back 71

OH⁻

Front 72

Give ion of Thiocyanate

Back 72

NCS⁻ or SCN⁻

Front 73

Give ion of acetate

Back 73

C₂H₃O₂

Front 74

Give ion of permanganate

Back 74

MnO₄⁻

Front 75

Give ion of dichromate

Back 75

Cr₂O₇²⁻

Front 76

Give ion of Chromate

Back 76

CrO₄²⁻

Front 77

Give ion of Peroxide

Back 77

O₂²⁻

Front 78

Give ion of Oxalate

Back 78

C₂O₄²⁻

Front 79

Give ion of Thiosulfate

Back 79

S₂O₃²⁻

Front 80

List acids that do not contain Oxygen

Back 80

HF- Hydrofluoric acid
HCL- Hydrochloric acid
HBr- Hydrobromic acid
HI- Hydroiodic acid
HCN- Hydrocyanic acid
H₂S- Hydrosulfuric acid

Front 81

What is chemistry

Back 81

Study of change of one substance into another

Front 82

list steps of scientific method

Back 82

1-observe
2-form hypothesis
3-experiment hypothesis
4-theory (confirmation or validation with or against hypothesis)

Front 83

what's principal of falsifiability

Back 83

for something to be called a science it must be challengable

Front 84

what is a pure substance

Back 84

form of matter unable to be separated by physical technique

Front 85

what is a mixture

Back 85

combination of 2 or more substances, which each substance retains its identity

Front 86

what is a heterogeneous mix

Back 86

mix where properties in part of mixture are different than properties in another part of mixture.
Ex-sand water where bottom of contain is mostly sand while upper container is mostly water

Front 87

what is a homogeneous mix

Back 87

a mix where everything is the same throughout mixture
ex-sugar water

Front 88

what is another name for homogeneous mix

Back 88

solution

Front 89

what is physical change

Back 89

change in physical property which doesn't produce a new chemical substance
ex-phase change-water to iceq

Front 90

what is chemical change

Back 90

change which results in one or more different/new substances

Front 91

what is precision

Back 91

when you get the same answer repeatedly

Front 92

what is accuracy

Back 92

when you get the right answer over and over

Front 93

what is law of conservation of mass

Back 93

matter is neither created nor destroyed in a chemical reaction

Front 94

what is law of definite proportion

Back 94

a given compound always contains the exact same proportion of elements by mass

Front 95

what are groups on a periodic table

Back 95

vertical columns on periodic table

Front 96

what are periods on a periodic table

Back 96

horizontal columns on a periodic table

Front 97

describe Alkali metals

Back 97

-group 1A period 2-7
-in pure form it's very reactive with water

Front 98

describe alkaline earth metals

Back 98

-group 2A
-isn't as reactive with water

Front 99

describe noble gases

Back 99

- group 8A
- tend not to react with anything

Front 100

describe halogens

Back 100

- group 7A
-highly reactive and very corrosive in elemental form

Front 101

list and describe the 3 groups elements are broken into broadly

Back 101

metals: solid, conduct electricity, ductile (turn into wire), and malleable (can turn into a flat sheet), form alloys (what life is made of)

nonmetals: don't conduct electricity, not ductile, not malleable, no alloys

semimetals/ metalloids: some properties of metals and chemical properties of nonmetals

Front 102

define molecule

Back 102

smallest identifiable unit which a pure substance can be divided and still retain the composition and chemical properties of that substance

Front 103

ammonium vs ammonia

Back 103

Ammonium-NH₄⁺

ammonia-NH₃

Front 104

To calculate avg atomic mass

Back 104

Take % abundance and divide by 100, then multiply by atomic mass unit (amu) of every isotope and add them up to get avg atomic mass which tells you the element

Front 105

to calculate limiting reactant

Back 105

-calculate moles of reactants

-determine mole ration between reactants in balanced equation

- how does actual mole ratio compare required ratio, if actual is smaller than the compound/element in numerator is limiting

Front 106

from percent to empirical and molecular formula

Back 106

-covert % to grams and grams to moles

- compound/element producing smallest # of moles is dividing into all #'s=giving ratios determining empirical formula

-* if given molar mass of compound, divide provided molar mass by molar mass produced by empirical formula and multiply moles of compound by that produced #

Front 107

calculating % yeild

Back 107

-convert grams to moles

- determine required and actual mole ratio, if actual is smaller then numerator is limiting

- use limiting mole to determine product mole and convert to mass if asked

-use provided product mass/ actual yeild and divide by mass produced by limiting mole, then multiply by 100 giving % yeild