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chemistry > Chem eoc > Flashcards

Chem eoc Flashcards

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1
Q

The two types of substances

A

element and compound

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2
Q

classify Cl2 as either a substance or mixture, and what type

A

A substance: element

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3
Q

classify H2O as either a substance or mixture, and what type

A

A substance: compound

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4
Q

The two types of mixtures

A

homogeneous and heterogeneous

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5
Q

classify Sugar water (C2H12O6+H2O) as either a substance or mixture, and what type

A

homogeneous mixture

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6
Q

classify Cookie dough ice cream as either a substance or mixture, and what type

A

heterogeneous mixture

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7
Q

color property=chemical or physical?

A

physical property

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8
Q

density property=chemical or physical?

A

physicalf

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9
Q

flammability property =chemical or physical?

A

chemical

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10
Q

solubility property=chemical or physical?

A

physical

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11
Q

reaction property (reacts w/..)=chemical or physical?

A

chemical

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12
Q

sour taste property=chemical or physical?

A

physical

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13
Q

melting point property==chemical or physical?

A

physical

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14
Q

luster property=chemical or physical?

A

physical

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15
Q

odor property=chemical or physical?

A

physical

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16
Q

rusting property=chemical or physical?

A

chemical

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17
Q

king henry drank bubbly dark chocolate milk
king henry danced badly during christmas morning

A

ya

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18
Q

Atlantic rule

A

if the 0 is AFTER the decimal point, it should be accounted for in sig. figs

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19
Q

Pacific rule

A

if the 0 is PREVIOUS (before) the decimal point, it should NOT BE ACCOUNTED FOR

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20
Q

how many sig digs. in 8040

A

3

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21
Q

how many sig digs in 0.020

A

2

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22
Q

how many sig digs in 6,051.00

A

6

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23
Q

calculate the percent error given
experimental value: 1.24 g
accepted value: 1.30g

A

(1.30g-1.24g)/1.30g
times 100
=4.62%

IMPORTANT: bigger value goes first always

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24
Q

how to calculate density? d=

A

d=m/v

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25
Q

how to calculate mass? m=

A

m=dv

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26
Q

how to calculate volume? v=

A

v=m/d

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27
Q

what goes on top in the triangle

A

m

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28
Q

plum pudding model guy

A

Jj thomson

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29
Q

cathode ray guy

A

jj thomson

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30
Q

charge and mass of electron guy

A

robert millikan

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31
Q

oil drop experiment guy

A

robert millikan

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32
Q

first atomic theory guy from experiment

A

dalton

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33
Q

electron clouds guy

A

niels bohr

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34
Q

uncertainty principle guy

A

heisenberg

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35
Q

top number in atomic structure is what?

A

the mass number

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36
Q

bottom number in atomic structure is what?

A

the atomic number

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37
Q

isotope name example

A

element-number (Cs-133)

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38
Q

what does the 133 in Cs-133 stand for?

A

the mass number

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39
Q

How to calculate average atomic mass

A

(mass number)(percent abundance)+(mass number2)(percent abundance2) etc

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40
Q

group name for 1a elements

A

alkali metals

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41
Q

group name for 2a elements

A

alkali earth metals

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42
Q

group name for 7a elements

A

halogens

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43
Q

group name for 8a elements

A

noble gases

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44
Q

group name for 3-12 elements (or 3d elements in the electron configuration)

A

transition metals

45
Q

highest electronegativity

A

Fluorine

46
Q

highest ionization energy

A

Helium

47
Q

highest atomic radius

A

Francium

48
Q

Negative ion=

A

gains electrons

49
Q

Positive ion=

A

loses electrons

50
Q

ammonium polyatomic formula

A

NH4+

51
Q

acetate polyatomic formula

A

C2H3O2-

52
Q

hydroxide polyatomic formula

A

OH-

53
Q

phosphate polyatomic ion formula

A

PO43-

54
Q

sulfate polyatomic ion formula

A

SO42-

55
Q

Carbonate polyatomic ion formula

A

CO3^2

56
Q

Nitrate polyatomic ion formula

A

NO3-

57
Q

Cation=

A

Pawsitively charged

58
Q

Anion

A

negatively charged

59
Q

covalent bonds=

A

nonmetal+nonmetal

60
Q

ionic bonds=

A

metal+nonmetal

61
Q

If the polyatomic ion ends in ate then you change the acid formula ending to…

A

ic acid

62
Q

if the polyatomic ion ends in ite then you change the acid formula ending to…

A

ous acid

63
Q

if the polyatomic ion ends in ide then you change the acid formula prefix and ending to…

A

hydro….ic

64
Q

H2SO4- formula acid name

A

Sulfuric acid

65
Q

one more than -ate polyatomic=

A

add per prefix (ex: ClO4- is perchlorate)

66
Q

one less than -ate polyatomic=

A

add -ite (ex: ClO2- is chlorite)

67
Q

two less than -ate polyatomic=

A

add hypo and -ite (ex: ClO- is hypochlorite)

68
Q

remove oxygen from -ate polyatomic

A

add -ide (Cl- is chloride)

69
Q

H2SO3 acid name

A

sulfurous acid

70
Q

H2S acid name

A

hydrosulfuric acid

71
Q

HClO4 acid name

A

perchloric acid

72
Q

HCLO acid name

A

hypochlorous acid

73
Q

HCl acid name

A

hydrochloric acid

74
Q

HNO3

A

Nitric acid

75
Q

HNO2 acid name

A

Nitrous acid

76
Q

Standard number for particles

A

6.022*10^23 particles

77
Q

how to find percentage composition

A

divide mass of element by total mass of compound for each element, then multiply by 100.

78
Q

how to find empirical formula of a compound, given percentage compositions

A

turn the percent into grams, then solve for moles. then divide by smallest number of moles for whole number. if the number is not close to a whole number (ex:2.5) then multiply by a whole number for each to have all numbers be whole. Then those numbers will signify how many of each element is in the compound

79
Q

Molecular formula given empirical formula compound and molecular weight.

A

divide the molecular weight by the mass of the empirical formula compound. then multiply that whole number by the subscript numbers indicating how much of each element there is in a compound given.
ex: CHO *2= C2H2O2

80
Q

temperature increase shift

A

shifts to the side that doesn’t state the heat energy.

81
Q

if one element is removed, shifts to what side?

A

shifts to the side where the element is removed.

82
Q

if one element is added, shifts to what side?

A

shifts to the opposite side of the elemtn added.

83
Q

if pressure decreases, shifts to what side?

A

the side with less moles

84
Q

reducing agent in a redox reaction does what with electrons:

A

gains electrons

85
Q

oxidizing agent in a redox reaction does what with electrons:

A

loses electrons

86
Q

strength of solid Intermolecular forces

A

are strong

87
Q

strength of gas intermolecular forces

A

are weak

88
Q

ideal gas law equation

A

PV=nRT

89
Q

boyle’s law

A

P1V1=P2V2

90
Q

endothermic reactions do what wtih energy

A

gain energy

91
Q

exothermic reactions do what with energy

A

release energy

92
Q

where is the activation energy located in potential energy curves?

A

the arrow on the side from the activated complex to the dotted line signifying the reactants

93
Q

STP of gas’ volume

A

22.41 L

94
Q

STP of temperature

A

273.15 K or 0 degrees Celsius

95
Q

STP of pressure

A

1 atm

96
Q

Charle’s law

A

V1T2=V2T1

97
Q

Gay lussac’s law

A

P1T2=P2T1

98
Q

Combined gas law

A

P1V1T2=P2V2T1

99
Q

Molarity formula=

A

moles/volume(L)

100
Q

Molarity by dilution formula

A

M1V1=M2V2

101
Q

in what direction do excited electrons move in the Bohr Model

A

to a higher ring.

102
Q

elements in the same group have…

A

similar properties

103
Q

C of water

A

4.184 J/g*C

104
Q

formula to find energy from a wavelength

A

E=hc/wavelength

105
Q

h in wavelength/energy formulas=

A

6.62610^-34 Jg

106
Q

Relationship between frequency and wavelength

A

inverse:
high frequency=short wavelength

107
Q

example of a high frequency form of energy

A

gamma rays

108
Q

example of a long wavelength form of energy

A

Radio waves

chemistry (5 decks)

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