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CHEM111 > Science and Measurement > Flashcards

Science and Measurement Flashcards

1
Q

What is chemistry

A

the study of matter and energy

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2
Q

matter

A

anything that has mass and occupies space

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3
Q

elements

A

the simplest form of matter that has distinct physical and chemical properties and cannot be broken down chemically into simpler, stable substances; building blocks for everything

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4
Q

atom

A

the smallest amount of an element that still has the characteristics of that element

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5
Q

chemical bonds

A

An attraction between atoms of different elements; can be broken and re-formed

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6
Q

compound

A

a chemical combination of elements that has its own set of properties and a definite composition

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7
Q

The two types of pure substances:

A

elements and compounds

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8
Q

mixture

A

two or more pure substances physically combined; no definite composition and can be heterogeneous or homogeneous

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9
Q

Homogeneous mixtures

A

also called solutions

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10
Q

Which phases can solutions be found in?

A

gas, solid, aqueous

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11
Q

Element examples

A

Hydrogen, sodium

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12
Q

Compound examples

A

water (H2O), Table salt (NaCl)

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13
Q

Heterogeneous mixture examples

A

oil and water mixture, chicken noodle soup

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14
Q

homogeneous mixture examples

A

brass, vodka

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15
Q

properties

A

characteristics by which something can be identified

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16
Q

Physical Properties

A

describe or identify a substance w/o changing its chemical composition

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17
Q

Physical Properties Examples

A

color, melting point, conductivity

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18
Q

Chemical properties

A

characteristic chemical reactions a substance undergoes

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19
Q

Extensive Properties

A

depend on the amount of a substance present

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20
Q

Extensive properties examples

A

mass, volume

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21
Q

Intensive properties

A

properties that are the same regardless of sample size

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22
Q

Intensive properties Examples

A

density, color, melting point

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23
Q

Physical Change

A

Chemical composition is not altered; Iron and sulfur can be mixed but remain iron and sulfur. They can be separated based on their different solubilities (another physical property).

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24
Q

Reactant

A

starting material in a chemical change (reaction)

25
Q

product

A

resulting material in a chemical change (reaction)

26
Q

Chemical changes

A

alter the chemical structure of a substance by breaking and/or forming chemical bonds

27
Q

Mass

A

how much matter an object has; directly proportional to weight

28
Q

Energy

A

capacity to do work

29
Q

Law of Conservation of Energy

A

Energy cannot be created or destroyed but can be converted from one form to another

30
Q

Scientific Method

A

A process that combines observation, hypothesis, and experimentation

31
Q

Hypotheses

A

the initial explanation for some observed fact(s), based on observation/evidence; are to be revised and tested through experimentation

32
Q

Theories

A

explain and predict many different observations that are linked by the same underlying phenomena; generally widely accepted as valid explanations of phenomena

33
Q

Scientific Laws

A

observations that are always true; statements of a phenomenon w/o explanation

34
Q

Law of Conservation of Mass

A

in any chemical reaction or physical change, the total mass present after the change is equal to the total mass present before the change; discovered by Lavoisier; does not apply to nuclear reactions

35
Q

Base Units (fundamental units)

A

units defined by a particular physical measurement

36
Q

SI unit of length

A

meter, m

37
Q

SI unit of mass

A

Kilogram, kg

38
Q

SI unit of time

A

second, s

39
Q

SI unit of temperature

A

Kelvin, K

40
Q

SI unit for Amount of a Substance

A

Mole, mol

41
Q

Tera-

A

10^12

42
Q

Giga-

A

10^9

43
Q

Mega-

A

10^6

44
Q

Kilo-

A

10^3

45
Q

Deci-

A

10^-1

46
Q

Centi-

A

10^-2

47
Q

Milli-

A

10^-3

48
Q

Micro-

A

10^-6

49
Q

Nano-

A

10^-9

50
Q

Pico-

A

10^-12

51
Q

Qualitatitve

A

the identity or form of a substance present

52
Q

quantitative

A

the amount of a substance present

53
Q

accuracy

A

the closeness of the average of a set of measurements to the true value

54
Q

precision

A

the closeness of all of a set of measured values to one another

55
Q

significant digit

A

every digit that reflects the precision of the measurement, including the estimated digit at the end

56
Q

Density

A

the measure of how much mass something has relative to its volume; m/v

57
Q

Three temperature scales

A

Fahrenheit, Celsius, Kelvin

58
Q

Conversion from Fahrenheit to Celsius

A

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

59
Q

Celsius to Kelvin

A

K= C+273.15

CHEM111 (5 decks)

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