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fall semester 2024-25 LSSU > chem week 1 > Flashcards

chem week 1 Flashcards

(70 cards)

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1
Q

scientific theory

A

concise, extensively tested explanation of widely observed natural phenomena

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2
Q

scientific law

A

concise + generally applicable statement of a fundamental scientific principle (math, how)

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3
Q

atoms

A

smallest particle of an element, cannot be chemically or mechanically divided into smaller pieces

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4
Q

element

A

a pure substance that cannot be separated into simpler substances

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5
Q

compound

A

pure substance, 2 or more elements chemically bonded in fixed proportion

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6
Q

law of constant composition

A

compound always has the same elemental composition by mass, no matter its source ie: PURE WATER

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7
Q

law of multiple proportions

A

when 2 masses of one element react with a given mass of another to form two compounds, the two masses of the first element have a ratio of two small whole numbers ex: 15g O campared to 10g O has a ratio 3:2

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8
Q

chemical formulas

A

notation that uses the symbols of the elements to represent the elemental composition of a pure substance ie) SO2 SO3

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9
Q

matter

A

anything with mass, occupies space

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10
Q

pure substance

A

matter with constant composition, cannot be broken down into simpler matter by any PHYSICAL process

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11
Q

physical process or change

A

transformation of a sample of matter such as physical state change that does not alter chemical identity of any substance in sample
ie) state change

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12
Q

intensive properties

A

property that is independent of the amount of substance ie)density

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13
Q

extensive property

A

varies with amount of substance ie) mass

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14
Q

physical property

A

observed with out changing substance into another ie)density (state changes)

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15
Q

density

A

ratio of mass of an object to its volume d=m/v

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16
Q

chemical property

A

observed only by reacting substance with smt else (identity changes)

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17
Q

chemical bond

A

force holds two atoms/ions in a molecule/compound

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18
Q

molecule

A

collection of chemically bonded atoms, usually neutral

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19
Q

ion

A

particle consisting of one or more atoms, has net pos/neg charge

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20
Q

mixtures

A

two or more pure substances, homogenous or heterogenous

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21
Q

homogenous mixture

A

components distributed uniformly, composition and appearance uniform, appears even

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22
Q

heterogenous mixture

A

not distributed uniformly, contains regions of different composition

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23
Q

distillation

A

process using evaporation. or condensation to separate mixtures with different volatilities (water, gas)

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24
Q

filtration

A

process separating solid particles from liquid or gas (coffee, dust)

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25
chromatography
process separating a mixture of substances according to different affinities (forensics)
26
energy
capacity to do work
27
work
exertion of a force through a distance w = f x d
28
potential energy
energy stored in object because of its position or composition
29
kinetic energy
energy of object in motion because of mass and speed KE = 1/2 mu^2
30
heat
transfer of energy between objects that occur because of differences in temp
31
law of conservation of energy
cannot be created nor destroyed, but can change forms
32
molecular formula
chem formula that indicated how many atoms of each element are in one mol of pure substance C6H12O6
33
structural formula
representation of molecule that uses short lines between symbols of elements to show chem bonds between atoms CH3-C-CH3
34
ionic compounds
consists of a characteristic ratio of pos ions and neg ions ie) NaCl
35
empirical formula
chem formula in which subscripts represent the simplest whole number ratio of the atoms/ions in compound *ionic compounds always empirical
36
SI units
set of base and derived units used worldwide to express distances and quantities of matter and energy
37
T(K)=
T(C) + 273.15
38
T(C)=
(5/9) (T(F) -32)
39
precision
the extent to which repeated measurements of the same variable agree (HOW REPEATABLE)
40
accuracy
how close to true value (HOW CORRECT)
41
if this much sulfur added to this much oxygen to make SO2, then this much sulfur and HOW MUCH OXYGEN to make SO3??
- find moles of known - stoichiometry to find moles of unknown - MM to find g of unknown
42
melting
solid --> liquid
43
deposition
gas --> solid
44
sublimation
solid --> gas
45
vaporization
liquid --> gas
46
condensation
gas --> liquid
47
freezing
liquid --> solid
48
lifting BRICK
increases pot energy, pos!
49
ICE CUBE in hand
thermal energy goes into system, pos!
50
AIR BALLOON
not enough info: temp, pressure, etc
51
kilo
10^3
52
centi
10^-2
53
nano
10^-9
54
milli
10^-3
55
micro
10^-6
56
pico
10^-12
57
low of multiple proportions example
15g O + 10g S 10g O + 10g S 15/10 = 3/2
58
can distillation remove soil particles from water? (solid from liquid)
Yes, but it would require much more energy
59
properties used to distinguish things
- physical - chemical - density - conductivity - element/compound/mixture
60
between particles of gas?
empty space
61
what kind of property? density
physical
62
what kind of property? reacts with oxygen
chemical
63
what kind of property? boiling point
physical
64
what kind of property? conductivity
physical
65
mean
average calculated by summing all values in a series and dividing sum by number of values
66
standard deviation
a measure of the amount of variation in a set of related values
67
confidence interval
range of values that has a specified probability of containing the true value of a measurement
68
solid
definite volume and shape
69
liquid
definite volume but not shape
70
gas
neither definite volume nor shape

fall semester 2024-25 LSSU (10 decks)

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