Chapter 4: Atoms and Elements Flashcards
1
Q
____ are pure substances
from which all other
things are built.
A
Elements
2
Q
__ cannot be broken
down into simpler
substances
A
Elements
3
Q
Uranium comes from
A
the planet Uranus
4
Q
Titanium comes from
A
titans (myth)
5
Q
Chlorine comes from
A
Chloros: “ greenish yellow”
6
Q
Iodine comes from
A
Ioeides : “ violet”
7
Q
Magnesium comes from
A
Magnesia, a mineral
8
Q
Californium comes from
A
California
9
Q
Curium comes from
A
Marie and Pierre Curie
10
Q
Copernicium comes from
A
Nicolaus Copernicus
11
Q
___ represent the names of the
elements
A
chemical symbols
12
Q
____ consist of one to two letters
and start with a capital letter
A
Chemical symbols
13
Q
Iodine
A
I
14
Q
Iron
A
Fe
15
Q
Magnesium
A
Mg
16
Q
Zinc
A
Zn
17
Q
Nitrogen
A
N
18
Q
Phosphorus
A
P
19
Q
Aluminum
A
Al
20
Q
Manganese
A
Mn
21
Q
Hydrogen
A
H
22
Q
Potassium
A
K
23
Q
___ is a silvery, shiny element that is a liquid at room temperature.
A
Mercury (Hg)
24
Q
Mercury can enter the body by
A
- contact with the skin
- ingestion of water
- food contaminated with mercury
25
Once mercury has entered the body, it destroys proteins and disrupts cell function. Long-term exposure can:
1. damage the brain and kidneys.
2. cause mental retardation.
3. decrease physical development
26
Mercury contamination comes from
* industrial wastes.
* fish and seafood.
* batteries.
* compact fluorescent bulbs
27
The periodic table
organizes 118 elements into groups
with similar properties and places them in
order of increasing atomic mass
28
The periodic table
organizes ____ into groups
with similar properties
and places them in
order of increasing
atomic mass.
118
elements
29
In the periodic table, elements are arranged according to_____.
properties.
30
In the periodic table, ___ contain elements with similar properties in vertical columns
groups
31
In the periodic table, ___ are horizontal rows of elements, counted from top to bottom of the table
periods
32
Group 1A (1), the alkali
metals, includes the
following:
* lithium (Li)
* sodium (Na)
* potassium (K)
* rubidium (Rb)
* cesium (Cs)
33
______ the alkaline earth metals, are shiny but not as reactive as Group 1A metals
Group 2A (2) elements
34
Group 2A (2) elements, the alkaline
earth metals include the following:
* beryllium (Be)
* magnesium (Mg)
* calcium (Ca)
* strontium (Sr)
* barium (Ba)
* radium (Ra)
35
____ gives the red color in fireworks.
Strontium
36
Group 7A (17) is the ____
Halogen
37
Group 7A (17), the
halogens, includes the
following:
* fluorine (F)
* chlorine (Cl)
* bromine (Br)
* iodine (I)
38
In periodic table, metals are located to the
left
39
In periodic table, Nonmetals are located to the
right
40
In periodic table, Metalloids are located along the
heavy zigzag line on the nonmetals part
41
Metals, except for hydrogen,
1. are shiny and ductile, and conduct
heat and electricity
2. are solids
42
A metal that is liquid
Mercury (Hg)
43
Nonmetals are
* are dull, brittle, and poor
conductors but often good
insulators.
* have low densities and melting
points
44
Metalloids
* 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
45
exhibit properties of metals and nonmetals
Metalloids
46
____ are better conductors than nonmetals but not as
good as metals.
Metalloids
47
_____ are dull, brittle, and poor
conductors but often good
insulators.
nonmetals
48
___ have low densities and melting
points
Nonmetals
49
_____ are shiny and ductile, and conduct
heat and electricity
Metals
50
____ are used as semiconductors and insulators,
because they can be modified to function as
conductors or insulators
Metalloids
51
Of all the elements,
_____ are essential for the well-being and survival of the
human body.
20
52
The 4 elements make up 96% of our body mass.
oxygen, carbon, hydrogen, and nitrogen
53
Most of our _____ is found as water, which makes up 55 to 60% of our body mass
hydrogen and oxygen
54
Hydrogen and oxygen makes up ____ of our body mass
55 to 60%
55
What are the Macrominerals
Ca, P, K, Cl, S, Na, and Mg
56
The macrominerals are involved in
* 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
____ is the smallest
particle of an element that
retains the characteristics
of that element.
Atom
58
Aluminum foil contains
atoms of __
aluminum
59
Based on _____, atoms are tiny particles of matter.
Dalton’s atomic theory.
60
According to ____ of an element are similar to each other and different
from those of other elements.
Dalton’s atomic theory
61
Atoms of two or more different elements combine to form ____
compounds
62
____ are rearranged to form new combinations in a
chemical reaction.
Atoms
63
____ are never created or destroyed during a chemical
reaction.
Atoms
64
Atoms contain the following
subatomic particles:
Protons, electron, and neutrons
65
____ that have a positive
(+) charge
Protons
66
___ that have a negative
(–) charge
electron
67
neutron
___ that have no charge
(neutral)
68
From _____ experiment, cathode rays contain negatively charged particles
J.J. Thomson's
69
Thomson proposed a _____ in which protons and electrons were randomly distributed in a
positively charged cloud, like plums in a pudding
"plum-pudding” model of the atom
70
Thomson's plum-pudding model shows that the atoms such as _____
protons and electrons were randomly distributed in a
positively charged cloud
71
In Rutherford’s gold foil experiment, positively charged
particles
* were aimed at atoms of gold.
* mostly went straight through the atoms.
* were deflected only occasionally.
72
Rutherford’s experiment concluded that there must be a ____, ____, ____ nucleus in the atom that deflects
positive particles that come close
small,
dense, positively charged
73
An atom consists of
a ____, located in the center of the atom, that
contains ____ and ___ and represents most of
the mass of an atom.
neutrons, protons, and electrons
74
____ occupy a large, empty space around the
nucleus
electrons
75
76
chemists use a very small unit of mass called
atomic
mass unit (amu)
77
1 amu = ____ in biology
1 Dalton (Da)
78
____ have such a small mass that they are not
included in the mass of an atom.
Electrons
79
All atoms of an element
have the same number of ___ and ___
protons and atomic number
80
___ is a whole number specific for each element and is the same for all atoms of an element.
Atomic number
81
Atomic number =
number of protons
82
For neutral atoms, the net charge is ___. Therefore, the number of protons is equal to the ____
0, number of electrons
83
__ represents the number of particles in the nucleus
Mass number
84
Mass number is equal to
number of protons + the number of neutrons
85
Mass number
* is always a whole number.
* does not appear in the periodic table.
86
Number of neutrons =
mass number - atomic number
87
Mass numbers are given for specific ___ only
isotopes
88
* 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
Isotopes
89
____ with three
naturally occurring
isotopes, has an atomic
mass of 24.31 amu
Magnesium
90
Magnesium have ___ naturally occurring
isotopes
three
91
Carbon consist of 3 isotopes:
12C, 13C, and 14C
92
____ is the
* weighted average of all
naturally occurring
isotopes of that element
Atomic Mass
93
____ is the number on the periodic
table below the chemical
symbol
Atomic Mass
94
___ Electromagnetic radiation
Electromagnetic radiation
95
The distance between the peaks of waves is called ___
Wavelength
96
High-energy radiation has ___ wavelength
shorter
97
Low-energy radiation has ____ wavelengths
longer
98
When light from a heated element passes through a
prism, it separates into distinct lines of color separated
by dark areas called an ____
Atomic spectrum
99
In an atomic spectrum, light from a heated element separates into ___
Distinct lines
100
In an atom, each electron has a specific energy, known as its
____
energy level
101
increases in energy as the value of n increases and
electrons are ____ from the nucleus
farther away
102
Electrons can have only specific energy value
quantized
103
Electrons with the same energy are grouped in the
same ___
energy level
104
_____ with the same
energy are grouped in the same energy level.
Electrons
105
106
Energy levels are assigned
values ___
principal
quantum numbers (n), (n = 1, n = 2, …)
107
Electrons move to a ____ level
when they absorb
energy
higher energy
108
The energy emitted or
absorbed is equal to
the differences
between the two
energy levels
109
It is the arrangement of electrons that determines the
physical and chemical properties of an element
Sublevels
110
Each energy level consists of one or more ___
sublevels
111
The number of sublevels in an energy level is ___ to the
principal quantum number n of that energy level.
equal
112
The sublevels are identified as
s,p,d,and f
113
Orbitals are a three dimensional volume in
which electrons have the
highest probability of being found.
s orbitals
114
The s orbitals are shown as ___
sphere
115
Each ____ has two lobes, like a balloon tied
in the middle, and can hold a maximum of two
electrons.
p orbital
116
p orbitals can hold a maximum of ___
2 electrons
117
118
The three p orbitals are
arranged ___ to
each other along the x, y, and z axes around the
nucleus.
perpendicular
119
Orbital that has a __- shape
dumbell
120
Four of the five ____ consist of four lobes that are aligned
along or between
different axes.
d
orbitals
121
The Pauli exclusion principle states that
* 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
electrons in the same orbital ___ each other
repel
123
Each orbital can hold a maximum of ___ with opposite spins
two electrons
124
Each s sublevel has ____ and can hold a maximum
of ____
one orbital, two electrons.
125
Each ____has three orbitals and can hold a
maximum of ___
p sublevel , six electrons.
126
Each ____ has five orbitals and can hold a maximum
of 10 electrons
d sublevel, 10 electrons
127
Each ____ can has 7 orbitals and can hold a
maximum of 14 electrons
f sublevel, 14 electrons
128
_____ is used to indicate the placement of electrons in an atom
Electronic configuration
129
If the charge of an element is +, the electronic configuration should be ____ than original charge
lesser
130
If the charge of an element is -, the electronic configuration should be ____ than original charge
greater
131
f block holds a __
14 electrons
132
d block holds a __
10 electrons
133
p block holds a __
6 electrons
134
s block holds a __
2 electrons
135
