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ANALYTICAL CHEMISTRY > Chapter 4: Atoms and Elements > Flashcards

Chapter 4: Atoms and Elements Flashcards

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1
Q

____ are pure substances
from which all other
things are built.

A

Elements

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2
Q

__ cannot be broken
down into simpler
substances

A

Elements

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3
Q

Uranium comes from

A

the planet Uranus

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4
Q

Titanium comes from

A

titans (myth)

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5
Q

Chlorine comes from

A

Chloros: “ greenish yellow”

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6
Q

Iodine comes from

A

Ioeides : “ violet”

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7
Q

Magnesium comes from

A

Magnesia, a mineral

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8
Q

Californium comes from

A

California

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9
Q

Curium comes from

A

Marie and Pierre Curie

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10
Q

Copernicium comes from

A

Nicolaus Copernicus

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11
Q

___ represent the names of the
elements

A

chemical symbols

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12
Q

____ consist of one to two letters
and start with a capital letter

A

Chemical symbols

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13
Q

Iodine

A

I

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14
Q

Iron

A

Fe

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15
Q

Magnesium

A

Mg

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16
Q

Zinc

A

Zn

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17
Q

Nitrogen

A

N

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18
Q

Phosphorus

A

P

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19
Q

Aluminum

A

Al

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20
Q

Manganese

A

Mn

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21
Q

Hydrogen

A

H

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22
Q

Potassium

A

K

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23
Q

___ is a silvery, shiny element that is a liquid at room temperature.

A

Mercury (Hg)

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24
Q

Mercury can enter the body by

A
  1. contact with the skin
  2. ingestion of water
  3. food contaminated with mercury
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25
Q

Once mercury has entered the body, it destroys proteins and disrupts cell function. Long-term exposure can:

A
  1. damage the brain and kidneys.
  2. cause mental retardation.
  3. decrease physical development
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26
Q

Mercury contamination comes from

A
  • industrial wastes.
  • fish and seafood.
  • batteries.
  • compact fluorescent bulbs
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27
Q

The periodic table

A

organizes 118 elements into groups
with similar properties and places them in
order of increasing atomic mass

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28
Q

The periodic table
organizes ____ into groups
with similar properties
and places them in
order of increasing
atomic mass.

A

118
elements

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29
Q

In the periodic table, elements are arranged according to_____.

A

properties.

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30
Q

In the periodic table, ___ contain elements with similar properties in vertical columns

A

groups

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31
Q

In the periodic table, ___ are horizontal rows of elements, counted from top to bottom of the table

A

periods

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32
Q

Group 1A (1), the alkali
metals, includes the
following:

A
  • lithium (Li)
  • sodium (Na)
  • potassium (K)
  • rubidium (Rb)
  • cesium (Cs)
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33
Q

______ the alkaline earth metals, are shiny but not as reactive as Group 1A metals

A

Group 2A (2) elements

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34
Q

Group 2A (2) elements, the alkaline
earth metals include the following:

A
  • beryllium (Be)
  • magnesium (Mg)
  • calcium (Ca)
  • strontium (Sr)
  • barium (Ba)
  • radium (Ra)
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35
Q

____ gives the red color in fireworks.

A

Strontium

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36
Q

Group 7A (17) is the ____

A

Halogen

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37
Q

Group 7A (17), the
halogens, includes the
following:

A
  • fluorine (F)
  • chlorine (Cl)
  • bromine (Br)
  • iodine (I)
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38
Q

In periodic table, metals are located to the

A

left

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39
Q

In periodic table, Nonmetals are located to the

A

right

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40
Q

In periodic table, Metalloids are located along the

A

heavy zigzag line on the nonmetals part

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41
Q

Metals, except for hydrogen,

A
  1. are shiny and ductile, and conduct
    heat and electricity
  2. are solids
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42
Q

A metal that is liquid

A

Mercury (Hg)

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43
Q

Nonmetals are

A
  • are dull, brittle, and poor
    conductors but often good
    insulators.
  • have low densities and melting
    points
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44
Q

Metalloids

A
  • exhibit properties of metals and nonmetals.
  • are better conductors than nonmetals but not as
    good as metals.
  • are used as semiconductors and insulators,
    because they can be modified to function as
    conductors or insulators
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45
Q

exhibit properties of metals and nonmetals

A

Metalloids

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46
Q

____ are better conductors than nonmetals but not as
good as metals.

A

Metalloids

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47
Q

_____ are dull, brittle, and poor
conductors but often good
insulators.

A

nonmetals

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48
Q

___ have low densities and melting
points

A

Nonmetals

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49
Q

_____ are shiny and ductile, and conduct
heat and electricity

A

Metals

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50
Q

____ are used as semiconductors and insulators,
because they can be modified to function as
conductors or insulators

A

Metalloids

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51
Q

Of all the elements,
_____ are essential for the well-being and survival of the
human body.

A

20

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52
Q

The 4 elements make up 96% of our body mass.

A

oxygen, carbon, hydrogen, and nitrogen

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53
Q

Most of our _____ is found as water, which makes up 55 to 60% of our body mass

A

hydrogen and oxygen

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54
Q

Hydrogen and oxygen makes up ____ of our body mass

A

55 to 60%

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55
Q

What are the Macrominerals

A

Ca, P, K, Cl, S, Na, and Mg

56
Q

The macrominerals are involved in

A
  • the formation of bones and teeth.
  • maintenance of heart and blood vessels, muscle
    contraction, nerve impulses, and acid–base balance of body fluids.
  • regulation of cellular metabolism
57
Q

____ is the smallest
particle of an element that
retains the characteristics
of that element.

A

Atom

58
Q

Aluminum foil contains
atoms of __

A

aluminum

59
Q

Based on _____, atoms are tiny particles of matter.

A

Dalton’s atomic theory.

60
Q

According to ____ of an element are similar to each other and different
from those of other elements.

A

Dalton’s atomic theory

61
Q

Atoms of two or more different elements combine to form ____

A

compounds

62
Q

____ are rearranged to form new combinations in a
chemical reaction.

A

Atoms

63
Q

____ are never created or destroyed during a chemical
reaction.

A

Atoms

64
Q

Atoms contain the following
subatomic particles:

A

Protons, electron, and neutrons

65
Q

____ that have a positive
(+) charge

A

Protons

66
Q

___ that have a negative
(–) charge

A

electron

67
Q

neutron

A

___ that have no charge
(neutral)

68
Q

From _____ experiment, cathode rays contain negatively charged particles

A

J.J. Thomson’s

69
Q

Thomson proposed a _____ in which protons and electrons were randomly distributed in a
positively charged cloud, like plums in a pudding

A

“plum-pudding” model of the atom

70
Q

Thomson’s plum-pudding model shows that the atoms such as _____

A

protons and electrons were randomly distributed in a
positively charged cloud

71
Q

In Rutherford’s gold foil experiment, positively charged
particles

A
  • were aimed at atoms of gold.
  • mostly went straight through the atoms.
  • were deflected only occasionally.
72
Q

Rutherford’s experiment concluded that there must be a ____, ____, ____ nucleus in the atom that deflects
positive particles that come close

A

small,
dense, positively charged

73
Q

An atom consists of
a ____, located in the center of the atom, that
contains ____ and ___ and represents most of
the mass of an atom.

A

neutrons, protons, and electrons

74
Q

____ occupy a large, empty space around the
nucleus

A

electrons

75
Q
A
76
Q

chemists use a very small unit of mass called

A

atomic
mass unit (amu)

77
Q

1 amu = ____ in biology

A

1 Dalton (Da)

78
Q

____ have such a small mass that they are not
included in the mass of an atom.

A

Electrons

79
Q

All atoms of an element
have the same number of ___ and ___

A

protons and atomic number

80
Q

___ is a whole number specific for each element and is the same for all atoms of an element.

A

Atomic number

81
Q

Atomic number =

A

number of protons

82
Q

For neutral atoms, the net charge is ___. Therefore, the number of protons is equal to the ____

A

0, number of electrons

83
Q

__ represents the number of particles in the nucleus

A

Mass number

84
Q

Mass number is equal to

A

number of protons + the number of neutrons

85
Q

Mass number

A
  • is always a whole number.
  • does not appear in the periodic table.
86
Q

Number of neutrons =

A

mass number - atomic number

87
Q

Mass numbers are given for specific ___ only

A

isotopes

88
Q
  • are atoms of the same element.
  • have different mass numbers.
  • have the same number of protons but different numbers
    of neutrons.
  • can be distinguished by their atomic symbols
A

Isotopes

89
Q

____ with three
naturally occurring
isotopes, has an atomic
mass of 24.31 amu

A

Magnesium

90
Q

Magnesium have ___ naturally occurring
isotopes

A

three

91
Q

Carbon consist of 3 isotopes:

A

12C, 13C, and 14C

92
Q

____ is the
* weighted average of all
naturally occurring
isotopes of that element

A

Atomic Mass

93
Q

____ is the number on the periodic
table below the chemical
symbol

A

Atomic Mass

94
Q

___ Electromagnetic radiation

A

Electromagnetic radiation

95
Q

The distance between the peaks of waves is called ___

A

Wavelength

96
Q

High-energy radiation has ___ wavelength

A

shorter

97
Q

Low-energy radiation has ____ wavelengths

A

longer

98
Q

When light from a heated element passes through a
prism, it separates into distinct lines of color separated
by dark areas called an ____

A

Atomic spectrum

99
Q

In an atomic spectrum, light from a heated element separates into ___

A

Distinct lines

100
Q

In an atom, each electron has a specific energy, known as its
____

A

energy level

101
Q

increases in energy as the value of n increases and
electrons are ____ from the nucleus

A

farther away

102
Q

Electrons can have only specific energy value

A

quantized

103
Q

Electrons with the same energy are grouped in the
same ___

A

energy level

104
Q

_____ with the same
energy are grouped in the same energy level.

A

Electrons

105
Q
A
106
Q

Energy levels are assigned
values ___

A

principal
quantum numbers (n), (n = 1, n = 2, …)

107
Q

Electrons move to a ____ level
when they absorb
energy

A

higher energy

108
Q

The energy emitted or
absorbed is equal to

A

the differences
between the two
energy levels

109
Q

It is the arrangement of electrons that determines the
physical and chemical properties of an element

A

Sublevels

110
Q

Each energy level consists of one or more ___

A

sublevels

111
Q

The number of sublevels in an energy level is ___ to the
principal quantum number n of that energy level.

A

equal

112
Q

The sublevels are identified as

A

s,p,d,and f

113
Q

Orbitals are a three dimensional volume in
which electrons have the
highest probability of being found.

A

s orbitals

114
Q

The s orbitals are shown as ___

A

sphere

115
Q

Each ____ has two lobes, like a balloon tied
in the middle, and can hold a maximum of two
electrons.

A

p orbital

116
Q

p orbitals can hold a maximum of ___

A

2 electrons

117
Q
A
118
Q

The three p orbitals are
arranged ___ to
each other along the x, y, and z axes around the
nucleus.

A

perpendicular

119
Q

Orbital that has a __- shape

A

dumbell

120
Q

Four of the five ____ consist of four lobes that are aligned
along or between
different axes.

A

d
orbitals

121
Q

The Pauli exclusion principle states that

A
  • each orbital can hold a maximum of two electrons.
  • electrons in the same orbital repel each other.
  • electrons in the same orbital must have their magnetic spins
    cancel (they must spin in opposite directions).
122
Q

electrons in the same orbital ___ each other

A

repel

123
Q

Each orbital can hold a maximum of ___ with opposite spins

A

two electrons

124
Q

Each s sublevel has ____ and can hold a maximum
of ____

A

one orbital, two electrons.

125
Q

Each ____has three orbitals and can hold a
maximum of ___

A

p sublevel , six electrons.

126
Q

Each ____ has five orbitals and can hold a maximum
of 10 electrons

A

d sublevel, 10 electrons

127
Q

Each ____ can has 7 orbitals and can hold a
maximum of 14 electrons

A

f sublevel, 14 electrons

128
Q

_____ is used to indicate the placement of electrons in an atom

A

Electronic configuration

129
Q

If the charge of an element is +, the electronic configuration should be ____ than original charge

A

lesser

130
Q

If the charge of an element is -, the electronic configuration should be ____ than original charge

A

greater

131
Q

f block holds a __

A

14 electrons

132
Q

d block holds a __

A

10 electrons

133
Q

p block holds a __

A

6 electrons

134
Q

s block holds a __

A

2 electrons

135
Q
A

ANALYTICAL CHEMISTRY (5 decks)

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