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Chemistry 1 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

the smallest identifiable unit of an element

A

atom

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2
Q

the matter that reacts

A

reactants

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3
Q

the matter that forms

A

product

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4
Q

The theory that all matter is composed of
atoms originated from several observations
and laws.

A

atomic theory

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5
Q

In a chemical reaction, matter is neither
created nor destroyed.

A

law of conservation of mass

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6
Q

law of conservation of mass

A

In a chemical reaction, matter is neither
created nor destroyed.

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7
Q

All samples of a given compound, regardless of
their source or how they were prepared, have the
same proportions of their constituent elements.

A

Law of definite proportions

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8
Q

When two elements (call them A and B) form
two different compounds, the mass of element
B that combine with 1 g of element A can be
expressed as a ratio of small whole numbers.

A

Law of multiple proportions

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9
Q

partially evacuated glass
tube called a

A

cathode ray tube

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10
Q

a beam of particles

A

cathode rays

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11
Q

negatively charged electrode

A

cathode

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12
Q

positively charged electrode

A

anode

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13
Q

a fundamental property of some of the particles that compose atoms and results in attractive and repulsive forces between hose particles

A

electrical charge

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14
Q

attractive and repulsive forces

A

electrostatic forces

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15
Q

the area around a charged particle

A

electric field

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16
Q

fundamental charge

A

–1.6 × 10–19

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17
Q

proposed that the negatively
charged electrons were small particles held
uniformlywithin a positively charged
sphere.

A

J.J. Thomson

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18
Q

directed
positively charged particles at an ultra thin
sheet of gold foil.

A

Ernest Rutherford

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19
Q

what did oil drop experiment do

A

deduce that the charge of a single electron

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20
Q

what did oil drop experiment do

A

deduce that the charge of a single electron Z

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21
Q

the emission of small energetic particles from the core of certain unstable atoms

A

radioactivity

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22
Q

a small core called a

A

nucleus

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23
Q

positively charged particles

A

protons

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24
Q

neutral particles within the nucleus

A

neutrons

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25
Q

the mass of a proton

A

1.67493 x 10 to the negative 27th power kg`

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26
Q

the mass of a neutron

A

1.67493 x 10 to the negative 27th power kg`

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27
Q

the mass of an electron

A

9.1 x 10 to the negative 31st power kg

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28
Q

unit to express the mass

A

atomic mass units (amu)

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29
Q

the most important number to identify an atom is

A

the number of protons

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30
Q

The number of protons in an atom’s nucleus is its

A

atomic number

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31
Q

what is the symbol fo 4th atomic number

A

Z

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32
Q

He

A

Helium

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33
Q

Helium

A

He

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34
Q

H

A

Hydrogen

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35
Q

Hydrogen

A

H

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36
Q

Li

A

Lithium

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37
Q

Lithium

A

Li

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38
Q

Be

A

Beryllium

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39
Q

Beryllium

A

Be

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40
Q

B

A

Boron

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41
Q

Boron

A

B

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42
Q

C

A

carbon

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43
Q

Carbon

A

C

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44
Q

N

A

Nitrogen

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45
Q

Nitrogen

A

N

46
Q

O

A

Oxygen

47
Q

Fluorine

A

F

48
Q

Neon

A

Ne

49
Q

Sodium

A

Na

50
Q

Magnesium

A

Mg

51
Q

Aluminum

A

Al

52
Q

Silicon

A

Si

53
Q

Phosphorus

A

P

54
Q

Sulfer

A

S

55
Q

Chlorine

A

Cl

56
Q

Argon

A

Ar

57
Q

potassium

A

K

58
Q

Calcium

A

Ca

59
Q

is either a one- or
two-letter abbreviation listed directly below
its atomic number on the periodic table.

A

chemical symbol

60
Q

toms with the same number of protons
but a different number of neutrons are
called

A

isotopes

61
Q

The relative amount of each isotope in a
naturally occurring sample of a given
element is roughly constant.

A

natural abundance

62
Q

this has
allowed accurate measurements that reveal
small but significant variations in the natural
abundance of isotopes for many elements.

A

mass spectrometry

63
Q

The sum of the number of neutrons and
protons in an atom is its

A

mass number

64
Q

symbol for chemical symbol

A

X

65
Q

Symbol for mass number

A

A

66
Q

Atoms can lose or gain electrons and
become charged particles

A

ions

67
Q

Atoms can lose or gain electrons and
become charged particles

A

ions

68
Q

positively charges ions

A

cations

69
Q

Negatively charged ions

A

anions

70
Q

what is the law of periodic law

A

When the elements are arranged in order of
increasing atomic mass, certain sets of
properties recur periodically.

71
Q

When the elements are arranged in order of
increasing atomic mass, certain sets of
properties recur periodically.

A

periodic law

72
Q

Columns are
referred to as

A

groups

73
Q

Rows are called

A

periods

74
Q

predicted the existence
(and even the properties) of yet
undiscovered elements.

A

Mendeleev’s table

75
Q

how are the elements listed in modern table

A

increasing in atomic number

76
Q

where does metal reside on table

A

lower left side and middle

77
Q

where do nonmetal lie

A

in the upper right side of the periodic table

78
Q

how many nonmetals are there

A

17

79
Q

where do metalloids lie

A

zigzag
diagonal line that divides metals and
nonmetals.

80
Q

intermediate (and highly temperature-
dependent) electrical conductivity.

A

semiconductors

81
Q

whose properties
tend to be largely predictablebased on their
position in the periodic table.

A

main-group elements

82
Q

whose properties tend to be less predictable
based simply on their position in the
periodic table.

A

transition elements or transition metals

83
Q

how Many groups are there

A

18

84
Q

how many periods are there

A

7

85
Q

the most unreacted elements

A

noble gases (8A)

86
Q

the reactive metals

A

alkali metals (1A)

87
Q

elements within a column are considered

A

families

88
Q

They are fairly reactive

A

alkaline earth metals (2A)

89
Q

are very reactive
nonmetals.

A

halogens (7A)

90
Q

always found in nature as a salt

A

halogens

91
Q

tend to lose electrons,
forming a cation with the same number of
electrons as the nearest noble gas.

A

main group metals

92
Q

tend to gain electrons forming an anion with the same number of electrons as the nearest noble gas

A

main group nonmetals

93
Q

elements in the same what have similar properties

A

group

94
Q

have a tendency to lose one electron and
form 1+ ions.

A

alkali metals (group 1A)

95
Q

tend
to lose two electrons and form 2+ ions.

A

alkaline earth metals (group 2A) `

96
Q

tend to gain one
electron and form 1– ions.

A

halogens (group 7A)

97
Q

tend to gain two electrons and form 2–
ions

A

oxygen family nonmetals (group 6A)

98
Q

what are main-group elements that form
cations

A

metals

99
Q

what are the main-group elements that form
anions (nonmetals) with predictable
charge equal to

A

the group number minus eight

100
Q

average mass of the
isotopes that compose that element,
weighted according to the natural
abundance of each isotope.

A

atomic mass

101
Q

where is the atomic mass shown

A

directly beneath the element’s symbol in
the periodic table.

102
Q

a
technique that separates particles according
to their mass.

A

mass spectrometry

103
Q

The masses of atoms and the percent abundances of isotopes of elements are measured using what

A

mass spectrometry

104
Q

what does the position of each peak indicate

A

the mass of the isotopes

105
Q

what dies the intensity (height of the peak) indicate

A

relative abundance of that isotope

106
Q

where does chemical process happen?

A

between particles

107
Q

is the amount (g)
per mole

A

molar mass

108
Q

the amount of material containing 6.02214 x 10 to the 23rd particle

A

mole

109
Q

the number of moles of a substance

A

the amount of a substance

110
Q

the mass of one mole of an atom of an element is

A

molar mass

111
Q

An element’s molar mass in grams per
mole is numerically equal what

A

atomic mass units (amu)

Chemistry 1 (14 decks)

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