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Chem110 > Ch1-2 > Flashcards

Ch1-2 Flashcards

1
Q

experiment

A

observation of natural phenomena carried out in a controlled manner

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2
Q

law

A

observations in nature that are repeated and give the same result

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3
Q

mass

A

the quantity of matter in a material

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4
Q

weight

A

the force of gravity exerted on an object

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5
Q

matter

A

whatever occupies space and can be perceived by our senses

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6
Q

law of conservation of mass

A

Lavoisier stated that total mass remains constant during a chemical reaction

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7
Q

fixed shape/fixed volume/neither

1) solid
2) liquid
3) gas

A

1) fixed shape, fixed volume
2) no fixed shape, fixed volume
3) no fixed shape, no fixed volume

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8
Q

1) physical change
vs
2) chemical change

A

1) change in the form of matter but not in its chemical identity
2) change in which one or more kinds of matter are transformed into a new kind of matter

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9
Q

distillation

A

process of separating an easily vaporized liquid from another substance (water from sodium chloride)

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10
Q

1) physical property
vs
2) chemical property

A

1) characteristic that can be observed without changing chemical identity
(color)
2) a characteristic involving its chemical change
(chemical property of iron = rust)

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11
Q

mixtures are separated by a ____ property

A

physical

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12
Q

elements in a compound are separated by a ____ property

A

chemical

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13
Q

1) substance
vs
2) element

A

1) kind of matter that cannot be separated into other matter by physical processes (EX: sodium chloride only separated by chemical)
2) a substance that cannot be decomposed by any chemical processes into simpler substances
(EX: arsenic, mercury, etc)

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14
Q

1) compound
vs
2) mixture

A

1) a substance composed of two or more elements chemically combined; can be separated
(water = hydrogen + oxygen)

2) the combination of two or more substances in which substances retain their distinct properties
(dissolving salt in water, can be distilled)

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15
Q

1) law of definite proportions
vs
2) law of multiple proportions

A

1) a pure compound always contains constant proportions of the elements by mass
2) when two elements form more than one compound, the masses of one element have a fixed ratio for the mass of the other element
(ex: CO 2:1 mass, CO2 2:1 mass)

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16
Q

a solution is also known as

A

a homogeneous mixture

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17
Q

602200 in scientific notation

A

6.022 x 10^5

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18
Q

.000166 in scientific notation

A

1.66 x 10^-4

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19
Q

precision vs accuracy

A

precision = closeness of a set of values to one another

accuracy = closeness of a single measurement to correct value

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20
Q

350 + 93,000,000 in sig figs

A

93,000,000 because since 100,000 is next biggest column and 350 doesn’t fit there, it is not added on

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21
Q

measured number vs exact number

A

1) measured = number which is observed and recorded in an experiment
2) recorded= number that arises when you count items (9 coins)

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22
Q

prefixes

A 
kilo (10^3)
hecto (10^2)
deca (10^1)
UNIT
deci (10^-1)
centi (10^-2)
milli (10^-3)
micro (10^-6)
nano (10^-9)
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23
Q

1 mL =

A

1 m^3

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24
Q

atomic theory

A

an explanation of the structure of matter

25
Q

4 main points of dalton’s atomic theory

A

1) elements are composed of extremely small particles called atoms
2) atoms of a given element are identical, having the same size, mass, and chemical properties
3) compounds are composed of atoms of more than one element (equal ratio)
4) a reaction only involves the separation, combination or rearrangement of atoms

26
Q

atom-

A

an extremely small particle of matter

27
Q

chemical reaction-

A

the rearrangement of atoms present in the reactants

28
Q

nucleus-

A

the atom’s central core, positively charged

29
Q

what did each person discover?

1) chadwick
2) rutherford
3) thomson
4) dalton

A

1) neutrons
2) nucleus
3) electrons
4) atom

30
Q

atomic number

A

number of protons

31
Q

mass number

A

total number of protons and neutrons

32
Q

isotopes

A

atoms whose nuclei have same atomic number but different mass numbers (neutron numbers)

33
Q

how does dalton use the laws of chemical composition in his atomic theory?

A

1) elements are composed of the same atom = law of definite proportions
2) a reaction only involves the separation, combination or rearrangement of atoms = law of conservation of mass

34
Q

what points in john dalton’s atomic theory are still considered valid as he presented them?

A

atoms are the smallest particles

35
Q

describe ONE discovery that changed the view of the atom and how it changed the atomic view

A

not all elements are identical = isotopes

36
Q

fractional abundance

A

the fraction of the total number of atoms that is composed of an isotope

37
Q

an atom that is most abundant is ____

A

the closest to its average atomic mass

38
Q

period vs group

A

period = horizontal

group = vertical

39
Q

metal vs nonmetal vs metalloid

A

1) metal = solids at room temp
2) nonmetal = gases/solids at room temp
3) metalloid = has both metallic and nonmetallic properties

40
Q

1) molecular formula
vs
2) structural formula

A

1) gives the exact number of different atoms of an element in a molecule (H2O)
2) shows how the atoms are bonded together in a molecule (H-O-H)

41
Q

molecule-

A

definite group of atoms chemically bonded together by attractive forces

42
Q

polymers
vs
monomers

A

large polymers are made of smaller monomers

43
Q

ion

A

an electrically charged particle obtained from an atom or chemically bonded group of atoms by adding or removing atoms

44
Q

anion vs cation

A

1) anion- negatively charged ion, when an atom gains an electron
2) cation- positively charged ion, when an atom loses an electron

45
Q

monatomic ion
vs
polyatomic ion

A

1) single atom ion (H+)

2) ions made up of more than one atom (NO2-)

46
Q

ionic compounds
vs
molecular compounds

A

1) between two metals (transfer electrons)

2) between two or more nonmetals (share electrons)

47
Q

differentiate between an isotope’s atomic mass and an element’s average atomic mass (atomic weight)

A

1) atomic mass is total number of protons and neutrons

2) average atomic mass is the sum of all of the isotopes masses and their fractional abundance’s

48
Q

organic compounds

A

molecular substances that contain carbon combined with other elements (H, O, N)

49
Q

hydrocarbons

A

compounds containing only hydrogen carbon (CH4 methane)

50
Q

functional group

A

a reactive portion of a molecule that undergoes predictable reactions

51
Q

chemical nomenclature

A

the systemic naming of chemical compounds

52
Q

inorganic compounds

A

compounds composed of elements other than carbon

53
Q

chemical equation

A

the symbolic representation of a chemical reaction in terms of chemical formulas

54
Q

pure water is an example of a

A

compound

55
Q

since the sample of salt and water tastes the same from the top and bottom of the container it is an example of a

A

homogenous mixture

56
Q

it is cold when it is 32 degrees outside

A

false

57
Q

a measurement is a number

A

false

58
Q

the formula of the ionic compound formed by (Na, Group IA) and oxygen (O, Group VIA) is

A

Na2O

Chem110 (1 decks)

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