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Chem eoc Flashcards

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
how to calculate mass? m=
m=dv
26
how to calculate volume? v=
v=m/d
27
what goes on top in the triangle
m
28
plum pudding model guy
Jj thomson
29
cathode ray guy
jj thomson
30
charge and mass of electron guy
robert millikan
31
oil drop experiment guy
robert millikan
32
first atomic theory guy from experiment
dalton
33
electron clouds guy
niels bohr
34
uncertainty principle guy
heisenberg
35
top number in atomic structure is what?
the mass number
36
bottom number in atomic structure is what?
the atomic number
37
isotope name example
element-number (Cs-133)
38
what does the 133 in Cs-133 stand for?
the mass number
39
How to calculate average atomic mass
(mass number)(percent abundance)+(mass number2)(percent abundance2) etc
40
group name for 1a elements
alkali metals
41
group name for 2a elements
alkali earth metals
42
group name for 7a elements
halogens
43
group name for 8a elements
noble gases
44
group name for 3-12 elements (or 3d elements in the electron configuration)
transition metals
45
highest electronegativity
Fluorine
46
highest ionization energy
Helium
47
highest atomic radius
Francium
48
Negative ion=
gains electrons
49
Positive ion=
loses electrons
50
ammonium polyatomic formula
NH4+
51
acetate polyatomic formula
C2H3O2-
52
hydroxide polyatomic formula
OH-
53
phosphate polyatomic ion formula
PO43-
54
sulfate polyatomic ion formula
SO42-
55
Carbonate polyatomic ion formula
CO3^2
56
Nitrate polyatomic ion formula
NO3-
57
Cation=
Pawsitively charged
58
Anion
negatively charged
59
covalent bonds=
nonmetal+nonmetal
60
ionic bonds=
metal+nonmetal
61
If the polyatomic ion ends in ate then you change the acid formula ending to...
ic acid
62
if the polyatomic ion ends in ite then you change the acid formula ending to...
ous acid
63
if the polyatomic ion ends in ide then you change the acid formula prefix and ending to...
hydro....ic
64
H2SO4- formula acid name
Sulfuric acid
65
one more than -ate polyatomic=
add per prefix (ex: ClO4- is perchlorate)
66
one less than -ate polyatomic=
add -ite (ex: ClO2- is chlorite)
67
two less than -ate polyatomic=
add hypo and -ite (ex: ClO- is hypochlorite)
68
remove oxygen from -ate polyatomic
add -ide (Cl- is chloride)
69
H2SO3 acid name
sulfurous acid
70
H2S acid name
hydrosulfuric acid
71
HClO4 acid name
perchloric acid
72
HCLO acid name
hypochlorous acid
73
HCl acid name
hydrochloric acid
74
HNO3
Nitric acid
75
HNO2 acid name
Nitrous acid
76
Standard number for particles
6.022*10^23 particles
77
how to find percentage composition
divide mass of element by total mass of compound for each element, then multiply by 100.
78
how to find empirical formula of a compound, given percentage compositions
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
Molecular formula given empirical formula compound and molecular weight.
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
temperature increase shift
shifts to the side that doesn't state the heat energy.
81
if one element is removed, shifts to what side?
shifts to the side where the element is removed.
82
if one element is added, shifts to what side?
shifts to the opposite side of the elemtn added.
83
if pressure decreases, shifts to what side?
the side with less moles
84
reducing agent in a redox reaction does what with electrons:
gains electrons
85
oxidizing agent in a redox reaction does what with electrons:
loses electrons
86
strength of solid Intermolecular forces
are strong
87
strength of gas intermolecular forces
are weak
88
ideal gas law equation
PV=nRT
89
boyle's law
P1V1=P2V2
90
endothermic reactions do what wtih energy
gain energy
91
exothermic reactions do what with energy
release energy
92
where is the activation energy located in potential energy curves?
the arrow on the side from the activated complex to the dotted line signifying the reactants
93
STP of gas' volume
22.41 L
94
STP of temperature
273.15 K or 0 degrees Celsius
95
STP of pressure
1 atm
96
Charle's law
V1T2=V2T1
97
Gay lussac's law
P1T2=P2T1
98
Combined gas law
P1V1T2=P2V2T1
99
Molarity formula=
moles/volume(L)
100
Molarity by dilution formula
M1V1=M2V2
101
in what direction do excited electrons move in the Bohr Model
to a higher ring.
102
elements in the same group have...
similar properties
103
C of water
4.184 J/g*C
104
formula to find energy from a wavelength
E=hc/wavelength
105
h in wavelength/energy formulas=
6.626*10^-34 J*g
106
Relationship between frequency and wavelength
inverse: high frequency=short wavelength
107
example of a high frequency form of energy
gamma rays
108
example of a long wavelength form of energy
Radio waves

chemistry (5 decks)

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