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Chemistry 121 > Chapter Two: Atoms, Molecules, and Ions > Flashcards

Chapter Two: Atoms, Molecules, and Ions Flashcards

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1
Q

What is Dalton’s Atomic Theory? (4)

A
  1. Each element is composed of atoms
  2. All atoms of an element are identical, different atom = different element
  3. Atoms of one element can’t be changed into a different atom, not created nor destroyed
  4. Compounds are formed when atoms of more than one element combine
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2
Q

mono

A

1

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3
Q

di

A

2

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4
Q

tri

A

3

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5
Q

tetra

A

4

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6
Q

penta

A

5

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7
Q

hexa

A

6

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8
Q

hepta

A

7

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9
Q

octa

A

8

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10
Q

nona

A

9

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11
Q

deca

A

10

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12
Q

Law of Constant Composition:

A

in a given compound, the relative numbers and kinds of atoms are constant

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13
Q

Law of Conservation of Mass:

A

the total mass of materials present after a chemical reaction is the same as the total mass present before the chemical reaction

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14
Q

Law of Multiple Proportions:

A

If two elements, A and B, combine to form more than one compound, then the masses of B that combine with a given mass of A are in the ratio of small whole numbers

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15
Q

Who discovered Cathode Rays and created the Plum Pudding model?

A

J.J. Thompson

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16
Q

What are cathode rays?

A

Streams of electrons
produced when a high voltage is applied to electrodes in an evacuated tube

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17
Q

What was the plum pudding model?

A

Negative electrons in a positive spread

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18
Q

What did Henri Becquerel, Marie Curie, and Rutherford discover?

A

Radioactivity through uranium

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19
Q

What did Rutherford find through his extensive research of radioactivity?

A

Alpha, Beta, and Gamma rays

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20
Q

What did Rutherford discover through his alpha-scattering experiment (gold foil experiment)?

A

Nucleus

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21
Q

What is the alpha radiation?

A

positive charges

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22
Q

What is the beta radiation?

A

High-speed electrons

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23
Q

What is the Gamma radiation?

A

high-energy electromagnetic radiation

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24
Q

What is mass number?

A

The number of protons plus neutrons

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25
Q

What is the atomic number

A

The number of protons

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26
Q

Isotope:

A

atoms of the same element containing different numbers of neutrons and therefore having different masses

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27
Q

Angstrom:

A

A common non-SI unit of length that is used to measure atomic dimensions

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28
Q

How do you find the ionic charge of a transition metal?

A

By looking at the ionic charge of what it is bonded to, must make the compound neutral

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29
Q

ate changes to…

A

ic

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30
Q

ous changes to…

A

ite

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31
Q

ide of an acid changes to….

A

ic

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32
Q

when changing ide to ic in a acid what prefix must be added?

A

hydro

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33
Q

ate of an acid changes to…

A

ic

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34
Q

ite of an acid changes to…

A

ous

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35
Q

What is Group 1A considered?

A

Alkali Metals

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36
Q

What is Group 2A considered?

A

Alkaline Earth Metals

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37
Q

What is Group 6A considered?

A

Chalcogens

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38
Q

What is Group 7A considered?

A

Halogens

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39
Q

What is Group 8A considered?

A

Noble Gases

40
Q

What are the 7 Diatomic Elements

A

Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine

41
Q

Molecular compounds are composed of….

A

only nonmetals

42
Q

Ionic compounds contain….

A

metals and nonmetals

43
Q

Monatomic anions are formed by _____________ with the exception of noble gases

A

nonmetals

44
Q

Monatomic cations are formed by _____________

A

metals

45
Q

this formula gives the lowest whole-number ration of atoms of each element in a compound

A

empirical formula

46
Q

this formula gives the exact number of atoms of each element in a compound

A

molecular formula

47
Q

What is the charge of those in 1A?

A

+

48
Q

What is the charge of those in 2A

A

2+

49
Q

What is the charge of those in 3A?

A

3+

50
Q

What is the charge of those in 7A?

A

-

51
Q

What is the charge of those in 6A?

A

2-

52
Q

What is the charge of those in 5A?

A

3-

53
Q

What type of compound typically has a metal combined with a nonmetal?

A

Ionic compound

54
Q

What portion of the ionic compound is almost always positive?

A

metal

55
Q

Ag+

A

Silver

56
Q

Fe2+

A

iron (II)

57
Q

Cu+

A

Copper (I)

58
Q

Sn2+

A

tin (II)

59
Q

Pb2+

A

Lead (II)

60
Q

Zn2+

A

Zinc

61
Q

Fe3+

A

Iron (III)

62
Q

Cu2+

A

Copper (II)

63
Q

Sn4+

A

Tin (IV)

64
Q

Pb4+

A

Lead (IV)

65
Q

What are the two rules for naming ionic compounds?

A
  1. if the cation can have more than one possible charge, write the charge as a roman numeral
  2. if the anion is an element, change its ending to -die
66
Q
A

Carbonate

67
Q
A

Nitrate

68
Q
A

Nitrite

69
Q
A

Phosphate

70
Q
A

Phosphite

71
Q
A

Sulfate

72
Q
A

Sulfite

73
Q
A

Perchlorate

74
Q
A

Chlorate

75
Q
A

Chlorite

76
Q
A

hypochlorite

77
Q
A

perbromate

78
Q
A

Bromate

79
Q
A

Bromite

80
Q
A

hypobromite

81
Q
A

periodate

82
Q
A

Iodate

83
Q
A

Iodite

84
Q
A

hypoiodite

85
Q
A

Hydrogen Phosphate

86
Q
A

Dihydrogen phosphate

87
Q
A

Phosphoric acid

88
Q

If the anion in the acid is, after a hydrogen, an oxyanion that ends in -ate, change the ending to…

A

-ic acid

89
Q

If the anion in the acid (that is after a Hydrogen) ends in -ide, change the ending to _______ and add the prefix ___________

A
  • ic acid
  • hydro
90
Q
A

Hydroxide

91
Q
A

Acetate

92
Q
A

Acetate

93
Q
A

Cyanide

94
Q
A

peroxide

95
Q
A

Ammonium

96
Q

What are the three rules in naming a molecular compound?

A
  1. The atom farther to left, or down, on PT is listed first
  2. A prefix is used to denote the number of atoms in each element
  3. The ending on the right element is changed to -ide
97
Q

What are the two rules for Organic compound formulas?

A
  1. List all elements in their alphabetical order after C and H
  2. Do not reduce the formulas

Chemistry 121 (9 decks)

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