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

chem week 1 Flashcards

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
Q

chromatography

A

process separating a mixture of substances according to different affinities (forensics)

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26
Q

energy

A

capacity to do work

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27
Q

work

A

exertion of a force through a distance w = f x d

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28
Q

potential energy

A

energy stored in object because of its position or composition

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29
Q

kinetic energy

A

energy of object in motion because of mass and speed

KE = 1/2 mu^2

30
Q

heat

A

transfer of energy between objects that occur because of differences in temp

31
Q

law of conservation of energy

A

cannot be created nor destroyed, but can change forms

32
Q

molecular formula

A

chem formula that indicated how many atoms of each element are in one mol of pure substance C6H12O6

33
Q

structural formula

A

representation of molecule that uses short lines between symbols of elements to show chem bonds between atoms CH3-C-CH3

34
Q

ionic compounds

A

consists of a characteristic ratio of pos ions and neg ions ie) NaCl

35
Q

empirical formula

A

chem formula in which subscripts represent the simplest whole number ratio of the atoms/ions in compound

*ionic compounds always empirical

36
Q

SI units

A

set of base and derived units used worldwide to express distances and quantities of matter and energy

37
Q

T(K)=

A

T(C) + 273.15

38
Q

T(C)=

A

(5/9) (T(F) -32)

39
Q

precision

A

the extent to which repeated measurements of the same variable agree (HOW REPEATABLE)

40
Q

accuracy

A

how close to true value (HOW CORRECT)

41
Q

if this much sulfur added to this much oxygen to make SO2, then this much sulfur and HOW MUCH OXYGEN to make SO3??

A
  • find moles of known
  • stoichiometry to find moles of unknown
  • MM to find g of unknown
42
Q

melting

A

solid –> liquid

43
Q

deposition

A

gas –> solid

44
Q

sublimation

A

solid –> gas

45
Q

vaporization

A

liquid –> gas

46
Q

condensation

A

gas –> liquid

47
Q

freezing

A

liquid –> solid

48
Q

lifting BRICK

A

increases pot energy, pos!

49
Q

ICE CUBE in hand

A

thermal energy goes into system, pos!

50
Q

AIR BALLOON

A

not enough info: temp, pressure, etc

51
Q

kilo

A

10^3

52
Q

centi

A

10^-2

53
Q

nano

A

10^-9

54
Q

milli

A

10^-3

55
Q

micro

A

10^-6

56
Q

pico

A

10^-12

57
Q

low of multiple proportions example

A

15g O + 10g S
10g O + 10g S

15/10 = 3/2

58
Q

can distillation remove soil particles from water? (solid from liquid)

A

Yes, but it would require much more energy

59
Q

properties used to distinguish things

A
  • physical
  • chemical
  • density
  • conductivity
  • element/compound/mixture
60
Q

between particles of gas?

A

empty space

61
Q

what kind of property? density

A

physical

62
Q

what kind of property? reacts with oxygen

A

chemical

63
Q

what kind of property? boiling point

A

physical

64
Q

what kind of property? conductivity

A

physical

65
Q

mean

A

average calculated by summing all values in a series and dividing sum by number of values

66
Q

standard deviation

A

a measure of the amount of variation in a set of related values

67
Q

confidence interval

A

range of values that has a specified probability of containing the true value of a measurement

68
Q

solid

A

definite volume and shape

69
Q

liquid

A

definite volume but not shape

70
Q

gas

A

neither definite volume nor shape

fall semester 2024-25 LSSU (8 decks)

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