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Chemistry 1515 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

states that different samples of a given compound always contain the same elements in the same mass ratio

A

law of definite proportions

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2
Q

states that if two elements can combine to form more than one compound with each other, the masses of the one element that combine with a fixed mass of the other element are in ratios of small whole numbers

A

law of multiple proportions

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3
Q

-discovered the ratio of the electric charge to the mass of an individual electron using the cathode ray tube

A

J.J. Thomson

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4
Q

determined the charge on an electron

A

milikan

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5
Q
  • noticed that cathode rays caused glass and metal to emit another type of ray
  • he named the rays “X rays” because of their mysterious nature
  • caused fluoresence
  • were not defined by a magnet
A

wilhelm roentgen

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6
Q

accidentally discovered that uranium darkened photographic film

A

antonine becquerel

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7
Q
  • suggested name “radioactivity”
  • rays were highly energetic and not deflected by a magnet
  • however, rays arose spontaneously unlike the rays discovered by roentgen
A

marie curie

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8
Q

describes a substance that spontaneously emits radiation

A

radioactive

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9
Q

positively charged particles

A

alpha (a)

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10
Q

electrons

A

beta (B)

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11
Q

no charge and are unaffected by external electric or magnetic fields

A

gamma (y)

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12
Q

number of protons in the nucleus of each atom of an element

A

atomic number (Z)

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13
Q

total num,ber of neutrons and protons present in the nucleus

A

mass number (A)

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14
Q
  • all atoms are not identical (as proposed by Dalton)

- same atomic number (Z) but different mass numbers (A)

A

isotopes

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15
Q

horizontal rows

A

periods

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16
Q
  • vertical columns

- elements in the same family have similar chemical and physical properties

A

families

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17
Q

good conductors of heat and electricity (majority of elements on the table, located to the left of the stair step)

A

metals

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18
Q

nonconductors (located in upper right-hand corner)

A

nonmetals

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19
Q

in between metals and nonmetals (those that lie along the separation line)

A

metalloids

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20
Q

is the mass of the atom in atomic mass units (amu)

A

atomic number

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21
Q

is defined as a mass exactly equal to one-twelth the mass of one carbon- 12 atom

A

atomic mass unit

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22
Q

combination of at least two atoms in a specific arrangement held together by chemical bonds

A

molecule

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23
Q

2 of the same atoms

A

homonuclear- diatomic molecules

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24
Q

2 different atoms

A

heteronuclear- diatomic molecules

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25
Q
  • contain more than 2 atoms
  • most molecules
  • may contain more than one element
  • ex: ozone, o3; white phosphorus, p4; water, h2o, and methane CH4
A

polyatomic molecules

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26
Q

shows exact number of atoms of each element in a molecule

A

molecules

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27
Q

one of the two or more distinct forms of an element

-ex: oxygen, ozone, diamond and graphite

A

allotrope

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28
Q

shows the general arrangement of atoms within the molecule

H-O-H

A

structural formula

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29
Q

mono

A

1

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30
Q

di

A

2

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31
Q

tri

A

3

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32
Q

tetra

A

4

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33
Q

penta

A

5

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34
Q

hexa

A

6

35
Q

hepta

A

7

36
Q

octa

A

8

37
Q

nona

A

9

38
Q

deca

A

10

39
Q

a substance that produces hydrogen ions (H+) when dissolved in water

A

acid

40
Q

contain carbon and hydrogen (sometimes with oxygen, nitrogen, sulfur and the halogens)

A

organic compounds

41
Q

contain only carbon and hydrogen

A

hydrocarbons

42
Q

simplest examples of hydrocarbons

A

alkanes

43
Q

determines chemical properties

A

functional group

44
Q

reveal the elements present and in what whole-number ratio they are combined

A

empirical formula

45
Q

an atom or group of atoms that has a net positive or negative charge

A

ion

46
Q

one atom with a positive or negative charge

A

monatomic ion

47
Q

ion with a net positive charge due to the loss of one or more electrons

A

cation

48
Q

ion with a net negative charge due to the gain of one or more electrons

A

anion

49
Q

ions that are a combination of two or more atoms

A

polyatomic ions

50
Q
  • 5thh century B.C.
  • greek
  • “atomos”
  • which is to say “indivisible”
  • no substantial visual model
  • determine properties
A

Democritus

51
Q
  • english..1808
  • billard ball model
  • solid sphere
  • determined composition
  • workable atomic theory
  • revived greek thoughts
A

Dalton

52
Q
  • early 1900’s
  • discovered e’s
  • plum-pudding model
  • but blueberry muffin model is better
A

JJ Thomson

53
Q
  • 1910
  • gold foil experiment
  • nuclear model
  • what a surprise
A

Rutherford

54
Q
  • 1913
  • planetary model
  • energy levels
  • defined orbits
  • not bad for the time
A

Bohr

55
Q
  • many contributors
  • schroedinger a key player
  • probability model with electron cloud
  • 1920’s
A

Quantum-Mechanical

56
Q

ammonium

A

NH4+

57
Q

hydronium

A

H3O+

58
Q

Mercury(I)

A

Hg2+2

59
Q

azide

A

N3-

60
Q

carbonate

A

CO3-2

61
Q

Chlorate

A

ClO3-

62
Q

chlorite

A

ClO2-

63
Q

chromate

A

Cr2O7-2

64
Q

cyanide

A

CN-

65
Q

dichromate

A

Cr2O7-2

66
Q

dihydrogen phosphate

A

H2PO4-

67
Q

bicarbonate

A

HCO3-

68
Q

hydrogen phosphate

A

HPO4-2

69
Q

bisulfate

A

HSO4-

70
Q

hydroxide

A

OH-

71
Q

hypochlorite

A

ClO-

72
Q

nitrate

A

NO3-

73
Q

nitrite

A

NO2-

74
Q

oxalate

A

C2O4-2

75
Q

perchlorate

A

ClO4-

76
Q

permanganate

A

MnO4-

77
Q

peroxide

A

O2-2

78
Q

phosphate

A

PO4-3

79
Q

phosphite

A

PO3-3

80
Q

sulfate

A

SO4-2

81
Q

sulfite

A

SO3-2

82
Q

thiocyanate

A

SCN-

83
Q

compounds that have a specific number of water molecules within their solid structure

A

hydrates

Chemistry 1515 (8 decks)

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