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Final Flashcards

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1
Q

Define purpose of an experiment

A

A 2-3 sentence summary of what you want to find out by conducting the experiment or the question that the experiment will answer

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2
Q

Independent Variable

A

What you change

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3
Q

Dependent Variable

A

What you measure, depends on what you change

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4
Q

Controlled Variable

A

Constant, what stays the same

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5
Q

Conclusion of an experiment

A

Summarize how your results support or contradict your original hypothesis

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6
Q

Density formula

A

D=m/v

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7
Q

Metric system acronyms

A 
King kilo
Henry hecta
Died deka
By base (m, l, g)
Drinking deci
Chocolate centi
Milk milli
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8
Q

Convert from celsius to kelvin

A

C+273

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9
Q

Convert from celsius to fahrenheit

A

(9/5)(C)+32=F

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10
Q

Convert Fahrenheit to celsius

A

(5/9)(F-32)=C

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11
Q

Accuracy

A

how close a measurement is to its standard or known value

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12
Q

Precision

A

how close two or more measurements are to each other, regardless whether those measurements are accurate or not

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13
Q

X axis is independent or dependent variable

A

independent variable

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14
Q

Y axis is independent or dependent variable

A

dependent variable

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15
Q

Sig fig rules

A
  • All digits 1-9 are significant.
  • Zeros between 1-9 are significant. Ex: 5007
  • Trailing zeros: counted for if decimal
  • Zeros only to place decimal point are NOT significant Ex: 0.00025
  • Zeros following a decimal sig fig are significant Ex: .470000
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16
Q

Chemical properties

A

properties that can be observed only when substances interact with one another
(Did you make something new?)

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17
Q

Examples of chemical properties

A

rust
explosion
oxidation reduction

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18
Q

Evidence of a chm rxn

A 
change of color
formation of ppt 
odor
change in temp
combustion
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19
Q

Physical properties

A

properties that can be observed or measured without changing the composition of matter

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20
Q

Examples of physical properties

A 
texture
mass
volume
length
width
height
taste
odor
malleability
flexibility
viscosity 
hardness
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21
Q

Examples of physical changes

A 
melting
cut wood
phase changes
break glass
color
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22
Q

Physical change

A

a change that effects only physical properties

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23
Q

Chemical change

A

a change that produces one or more substances

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24
Q

Element

A

cannot be further broken down by ordinary chemical means

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25
Q

Compound

A

combined chemically/ two or more elements chemically combined

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26
Q

Mixture

A

combined physically

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27
Q

Heterogeneous mixture

A

not the same throughout

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28
Q

Homogeneous mixture

A

same throughout

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29
Q

What are physical means to separate a mixture?

A
  • evaporation
  • chromatography
  • distillation
  • decantation
  • filtration
  • centrifuge
  • chemical separation
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30
Q

% error formula

A

theo - exp/ (theo)

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31
Q

Law of Conservation of Mass

A

mass cannot be created nor destroyed

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32
Q

proton charge, location, amu

A

+, nucleus, 1

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33
Q

neutron charge, location, amu

A

neutral, nucleus, 1

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34
Q

electron charge, location, amu

A

-, electron cloud, very small

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35
Q

parts of an atom?

A

proton, neutron, electron

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36
Q

STUDY SCIENTISTS

A

okay

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37
Q

STUDY DIATOMICS

A

okay

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38
Q

what is the mass number equal to

A

protons + neutrons

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39
Q

isotopes

A

have same number of electrons, just different # of neutrons/ two of same element w/ diff number of neutrons

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40
Q

atomic number

A

of protons/ identifies number on periodic table

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41
Q

of neutrons

A

mass # - atomic number

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42
Q

of electrons

A

equal to protons if the atom is a neutral atom

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43
Q

of protons

A

atomic number

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44
Q

ion

A

when theres a charge + or -

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45
Q

mass number then atomic number when you write the symbol

A

okay

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46
Q

alkali metals

A

1A

47
Q

alkaline-earth

A

2A

48
Q

transition metals

A

3-12

49
Q

halogens

A

7 valence electrons

50
Q

noble gases

A

full shell, furthest to the right

51
Q

lathanide

A

top bottom, 4f

52
Q

actinide

A

lower bottom, 5f

53
Q

super 7

A

H2, N2, O2, F2, Cl2, Br2, I2

54
Q

increasing ionization energy

A

to the right and up

55
Q

increasing atomic radius

A

to the left and down

56
Q

increasing Ionic radius

A

to the left and down

57
Q

increasing electron affinity

A

down: no trend
across: increases

58
Q

increasing metallic characteristic

A

to the left and down

59
Q

increasing electronegativity

A

to the right and up

60
Q

order for quantum numbers

A

n, l, ml, ms

61
Q

for quantum numbers, n is the

A

coefficient

62
Q

for quantum numbers, l is the

A

s p d f

0 1 2 3

63
Q

for quantum numbers, ml is the

A

-1, 0, +1

64
Q

for quantum numbers, ms is the

A

up arrow +1/2

down arrow -1/2

65
Q

electromagnetic spectrum

A 
Radio (red)
Microwave
Infrared
Visible
Ultraviolet
X-ray
Gamma ray ( higher frequency, smallest wavelengths) (purple)
66
Q

photon

A

a tiny packet of energy

67
Q

ground state of atoms

A

the lowest possible energy state of an atom, closest to the nucleus and most stable

68
Q

excited state

A

atoms get zapped with energy

69
Q

when the electron jumps back to the ground state, photons are ______

A

emitted

70
Q

An electron transitioning from a 4s orbital to the ground state gives off yellow light. What color of light might be emitted by an electron transitioning from a 5s orbital to the ground state in the same atom?

A

green, blue or purple

71
Q

difference between ionic and covalent

A

ionic metals

covalent nonmetals

72
Q

identify compounds as ionic or molecular

A

molecular non metal plus non metal

ionic ALL metals according to nick

73
Q

metal gives ______ to nonmetal in ionic bonding

A

electron

74
Q

how are electrons transferred in covalent bonding

A

they are shared

75
Q

ternary is

A

polyatomic ions

76
Q

ionic naming

A

change ending to ide

77
Q

what do transition metals need when naming

A

roman numerals

78
Q

molecular naming

A

prefixes

79
Q

HF

A

hydro _____ ic acid

80
Q

acronym for polyatomic acids

A

i ate a dic

ite ous

81
Q

hydrates

A

name normal then add prefix to hydrate

82
Q

example of hydrate

A

MnSO4 - 4H2O

Manganese (ll) Sulfate Tetrahydrate

83
Q

What are the types of reactions in equations

A

synthesis, double replacement, single replacement, decomposition

84
Q

what is the type of reaction when carbon dioxide and water is formed

A

combustion

85
Q

When is resonance formed when drawing compounds

A

when the double bond can go with multiple elements

86
Q

what is the VSEPR theory

A

model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms

87
Q

what are the hybridizations of molecular orbitals

A 
sp1
sp2
sp3
sp3d
sp3d2
88
Q

polar

A

not symmetrical

89
Q

nonpolar

A

symmetrical

90
Q

exceptions to the octet rule

A

odd # of valence e’ ex: NO
incomplete (mostly B or Be) ex: BF3
Expanded: PCl5

91
Q

polar dissolves

A

polar

92
Q

non polar dissolves

A

non polar

93
Q

for solids as temperature increases solubility…

A

increases bitch

94
Q

for gases as temperature increases solubility…

A

decreases slut

95
Q

for gases as pressure increases solubility…

A

increases

96
Q

for solids as pressure increases solubility…

A

stays the same

97
Q

suspension

A

a temporary mixture; the particles will eventually settle

98
Q

colloid

A

a mixture that scatters light and particles don’t settle out

99
Q

solution

A

a mixture that is homogeneous at the molecular level

100
Q

emulsion

A

mixture of two or more liquids that are normally immiscible

101
Q

electrolytes

A

a compound that conducts an electric current (aqueous sol.)

102
Q

non-electrolytes

A

dissolve in solution/doesn’t dissociate or conduct elect.

103
Q

molarity formula

A

moles of solute/liters of solvent

104
Q

molality

A

moles of solute/kg of solvent

105
Q

What is the formula for dilutions

A

M1V1 = M2V2

106
Q

What is the name for the “i value”

A

Vant hoff factor

107
Q

How do you find the i value

A

You see how many ions the substance will disociate into

108
Q

What is the formula for FP depression

A

K x m x i

K is the constant from the chart, m is for molality, and i is the vant hoff factor

109
Q

What is the formula for BP elevation

A

K x m x i

K is the constant from the chart, m is for molality, and i is the vant hoff factor

110
Q

chromatography

A

ink permeates up

111
Q

intensive property

A

do not depend on the amount of matter

112
Q

extensive property

A

do depend on the amount of matter

113
Q

% yield

A

actual/theoretical

114
Q

What is a real gas

A

Hip lot

High pressure
Low temperature

Chemistry (10 decks)

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