CHAPTER 2 Flashcards
1
Q
Atom comes from the Greek word ___ meaning “unable to cut.” I
A
Atomos
2
Q
The building blocks that comprise all forms of matter.
A
Atoms
3
Q
These are named for people, places, and things.
A
Elements
4
Q
Carbon (C) comes from the Latin word carbo, meaning
A
coal or charcoal
5
Q
This was named for the planet Neptune
A
neptunium (Np)
6
Q
Einsteinium (Es) was named for this scientist
A
Albert Einstein
7
Q
Californium (Cf) was named for the state of
A
California
8
Q
This is a pure substance that cannot be broken down into simpler substances by a chemical reaction
A
Element
9
Q
This is formed in small amounts during the combustion of fossil fuels like gasoline and is a toxic component of the smoggy air in many large cities.
A
Carbon monoxide (CO)
10
Q
How many elements are currently known?
A
118
11
Q
Of the118 elements currently known, how many are naturally occurring?
A
90
12
Q
Of the 118 elements that are currently known, the remaining 28 have been___.
A
prepared by scientists in the laboratory
13
Q
This is identified by a one- or two-letter symbol.
A
Element
14
Q
While most element symbols are derived from the first one or two letters of the element name, ____ elements have symbols derived from Latin or German origins.
A
11
15
Q
German/Latin-derived symbols
A
Antimony - Sb (stibium)
Copper - Cu (cuprum)
Gold - Au (aurum)
Iron - Fe (ferrum)
Lead - Pb (plumbum)
Mercury - Hg (hydrargyrum)
Potassium - K (kalium)
Silver - Ag (argentum)
Sodium - Na (natrium)
Tin - Sn (stannum)
Tungsten - W (wolfram)
16
Q
Elements could be arranged in a schematic way called the___.
A
periodic table
17
Q
The position of an element in the periodic table tells us much about its____.
A
Chemical properties
18
Q
These are shiny substances that conduct heat and electricity.
A
Metals
19
Q
These are ductile, meaning they can be drawn into wires, and malleable, meaning they can be hammered into shapes.
A
Metals
20
Q
These have properties intermediate between metals and nonmetals.
A
Metalloids
21
Q
These are poor conductors of heat and electricity.
A
Nonmetals
22
Q
The elements in the periodic table are divided into three categories:
A
metals
nonmetals
metalloids
23
Q
The solid line that begins with ___ and angles in steps down to ____ marks the three regions corresponding to these groups.
A
boron (B)
astatine (At)
24
Q
All metals are located to the ___ of the line.
A
left
25
All nonmetals except ___ are located to the right.
hydrogen
26
Metalloids are located along the ___.
steps
27
These are shiny materials that are good conductors of heat and electricity.
Metals
28
All metals are solids at room temperature except for ___, which is a liquid.
mercury
29
These do not have a shiny appearance, and they are generally poor conductors of heat and electricity.
Nonmetals
30
Nonmetals like ___ and ____ are solids at room temperature; ___ is a liquid; and ____ are gases.
Solids at room temp:
(1) sulfur
(2) carbon
Liquid
(1) bromine
Gases
nonmetals like nitrogen and oxygen and nine other elements are gases
31
These have properties intermediate between metals and nonmetals. Only seven elements are categorized as these:
Metalloids
(1) boron (B)
(2) silicon (Si)
(3) germanium (Ge)
(4) arsenic (As)
(5) antimony (Sb)
(6) tellurium (Te)
(7) astatine (At)
32
Does living organisms selectively take up elements from their surroundings?
Yes
33
These comprise 96% of the mass of the human body,
Four nonmetals oxygen, carbon, hydrogen, and nitrogen
34
Four nonmetals oxygen, carbon, hydrogen, and nitrogen comprise _____ of the mass of the human body.
96%
35
These are called the building-block elements (4)
(1) oxygen
(2) carbon
(3) hydrogen
(4) nitrogen
36
Hydrogen and oxygen are the elements that form ___, the most prevalent substance in the body.
water
37
The four main types of biological molecules:
(1) proteins
(2) carbohydrates
(3) lipids
(4) nucleic acids
38
These are found in the four main types of biological molecules: (3)
Carbon, hydrogen, and oxygen
39
These (from the four main types of biological molecules) contain the element nitrogen.
Proteins and nucleic acids
40
The major minerals or macronutrients, are also present in the body in much smaller amounts. How much percentage by mass?
0.1-2%
41
How many elements are major minerals or macronutrients?
Seven elements:
Sodium
Potassium
Chlorine
Magnesium
Sulfur
Calcium
Phosphorus
42
These take up 0.1-2% by mass
Major minerals or macronutrients
43
These are present in body fluids. (3)
(1) Sodium
(2) potassium
(3) chlorine
44
These occur in proteins (macronutrient) (2).
Magnesium and sulfur
45
These are present in teeth and bones.
Calcium and phosphorus
46
This is also contained in all nucleic acids, such as the DNA that transfers genetic information from one generation to another.
Phosphorus
47
At least _____ of each macronutrient is needed in the daily diet.
100 mg
48
These other elements occur in very small amounts in the body, but are essential to good health. These are:
trace elements or micronutrients
49
These are required in the daily diet in small quantities.
trace elements or micronutrients
50
These are required in the daily diet in small quantities— usually less than ___
15 mg
51
Each trace element has a specialized function that is important for ___.
proper cellular function
52
This trace element is needed for hemoglobin and myoglobin
Iron
53
This is the protein that carries oxygen in red blood cells.
Hemoglobin
54
This is the protein that stores oxygen in muscle.
myoglobin
55
This is needed for the proper functioning of many enzymes in the liver and kidneys.
Zinc
56
This is needed for proper thyroid function.
iodine
57
Although most of the trace elements are metals, nonmetals like ___ and ___ are micronutrients as well.
fluorine and selenium
58
Trace Elements (14)
Arsenic(As)
Boron (B)
Chromium (Cr)
Cobalt(Co)
Copper(Cu)
Fluorine (F)
lodine (I)
Iron (Fe)
Manganese (Mn) Molybdenum(Mo)
Nickel (Ni)
Selenium (Se)
Silicon(Si)
Zinc (Zn)
59
This contains all four building-block elements
Muscle tissue
60
This is a pure substance formed by chemically combining two or more elements together.
Compound
61
These are used to write chemical formulas for compounds.
Element symbols
62
This uses element symbols to show the identity of the elements forming a compound and subscripts to show the ratio of atoms contained in the compound.
chemical formula
63
All ____ is composed of the same basic building blocks called atoms.
matter
64
A __, symbolized by p, has a positive (+) charge.
proton
65
An ___, symbolized by e, has a negative (-) charge.
electron
66
A ___, symbolized by n , has no charge.
Neutron
67
These have approximately the same, exceedingly small mass.
Protons and neutrons
68
The mass of an electron is much less _____ the mass of a proton.
1/1,836
69
The ____ are not evenly distributed in the volume of an atom
Subatomic particles
70
This is a dense core that contains the protons and neutrons
Nucleus
71
Most of the mass of an atom resides in the ___
Nucleus
72
This is composed of electrons that move rapidly in the almost-empty space surrounding the nucleus. It comprises most of the volume of an atom.
Electron cloud
73
The diameter of an atom
10^-10 m
74
The diameter of a nucleus
10^-15 m
75
What is the charge of a proton?
+1
76
What is the charge of an electron?
-1
77
What is the charge of a neutron?
0
78
What is the mass(g) of a proton?
1.6726x10^-27
79
What is the mass(g) of a neutron?
1.6749x10^-27
80
What is the mass(g) of an electron?
9.1093x10^-31
81
What is the mass(amu) of a proton?
1
82
What is the mass(amu) of an electron?
Negligible
83
What is the mass(amu) of a neutron?
1
84
These charges repel
Positive and negative
85
These charges attract
Opposite
86
chemists use a standard mass unit, the ___, which defines the mass of individual atoms relative to a standard mass.
atomic mass unit
87
This is the number of protons in the nucleus of an atom.
The atomic number (Z)
88
The periodic table is arranged in order of ____ beginning at the upper left-hand corner.
increasing atomic number
89
the ____ tells us both the number of protons in the nucleus and the number of electrons in the electron cloud of a neutral atom.
atomic number
90
The ____, symbolized by A, is the sum of the number of protons and neutrons.
mass number
91
The number of uncharged particles.
number of neutrons
92
Two atoms of the same element always have the same number of protons, but the number of ___ can vary.
neutrons
93
Most elements in nature exist as a mixture of ___.
isotopes
94
A/An ____is also written using the element symbol with the atomic number as a subscript and the mass numberas a superscript, both to the left.
isotope symbol
95
About 1% of hydrogen atoms have one proton and one neutron, giving them a mass number of two. This isotope is called ____, and it is often symbolized as __.
deuterium (D)
96
An even smaller number of hydrogen atoms contain one proton and two neutrons, giving them a mass number of three. This isotope is called ____, symbolized as __.
tritium (T)
97
The ___ gives the mass number
superscript
98
This gives the atomic number
subscript
99
The ____ = mass number (A) - atomic number (Z)
number of neutrons + protons
100
the average mass, called the ____(or atomic mass),
atomic weight
101
The ___ is the weighted average of the mass of the naturally occurring isotopes of a particular element reported in atomic mass units.
atomic weight
102
The mass of any isotope is very close to the:
mass number of the isotope.
103
Generally the ____ of isotopes are identical.
chemical properties
104
This have both diagnostic and therapeutic uses in medicine.
Radioactive isotopes
105
Higher doses of ___ can also be used to treat thyroid disease.
iodine-131
106
Most prominent was Russian chemist ___, whose arrangement in 1869 of the 60 known elements into groups having similar properties became the precursor of the modern periodic table
Dmitri Mendeleev
107
The periodic table is arranged into ___ and ____. The particular row and column tell us much about the properties of an element.
seven horizontal rows
18 vertical columns
108
A row in the periodic table is called a ____.
period
109
Elements in the same row are similar in ___.
size
110
A column in the periodic table is called a ___.
group
111
Elements in the same group have similar ____.
electronic and chemical properties
112
The ___ in the periodic table are numbered 1-7.
rows
113
The first period has just:
Two elements:
Hydrogen and Helium
114
The second and third rows have:
eight elements each
115
the fourth and fifth rows have:
18 elements.
116
Two rows of ___ elements appear at the bottom of the periodic table.
14
117
Each column in the periodic table is assigned a ___.
group number
118
Elements are divided into three categories:
Main group elements- 1A-8A
Transition elements- 1B-8B
Inner transition metals
119
Elements that comprise a particular group have similar __.
chemical properties
120
Hydrogen is located in Group 1A, is it an alkali metal?
No
121
What is the group 1A (group 1) called and what are the elements in this group (6)
alkali metals
lithium (Li)
sodium (Na)
potassium (K)
rubidium (Rb)
cesium (Cs)
francium (Fr)
122
What is this?
•They are soft and shiny and have low melting points.
• They are good conductors of heat and electricity.
• T h e yreactreadily with water to form basic solutions.
Alkali metals
123
The ___, located ni group 2A (group 2), include ____. (6)
alkaline earth elements
beryllium (Be)
magnesium (Mg)
calcium (Ca),
strontium (Sr)
barium (Ba)
radium (Ra).
124
These are also shiny solids but less reactive than the alkali metals.
Alkaline earth metals
125
The group 3a elements are:
boron (B)
aluminum (Al)
gallium (Ga)
indium (In)
thallium (Tl)
126
The group 4a elements are: (6)
Carbon (C)
Silicon (Si)
Germanium (Ge)
Tin (Sn)
Lead (Pb)
Flerovium (Fl)
127
The group 5a elements are:
nitrogen (N)
phosphorus (P)
arsenic (As)
antimony (Sb)
bismuth (Bi)
128
The group 6a elements are:
oxygen (O)
sulfur (S)
selenium (Se)
tellurium (Te)
polonium (Po)
129
The group 7a is called?? And what is the elements under this?
Halogens
fluorine (F)
chlorine (CI)
bromine (Br)
iodine (I)
astatine (At)
130
These are very reactive and combine with many other elements to form compounds.
Halogens
131
The ___, located in group 8A (group 18), include___.
noble gases
helium (He)
neon (Ne)
argon (Ar)
krypton (Kr)
xenon (Xe)
radon (Rn)
132
Unlike other elements, the noble gases are especially ___ as atoms, so they rarely combine with other elements to form compounds.
stable
133
The chemical properties of an element are determined by the number of __ in an atom.
electrons
134
These do not move freely in space; rather, it is confined to a specific region, giving it a particular energy.
Electrons
135
These occupy discrete energy levels.
Electrons
136
The energy of electrons is ___; that is, the energy is restricted to specific values.
quantized
137
The electrons that surround a nucleus are confined to regions called the ___.
principal energy levels or shells
138
Electrons closer to the nucleus are held ___ tightly and are ___ in energy.
more ; lower
139
Electrons farther from the nucleus are held ___ tightly and are ___ in energy.
less ; higher
140
The number of electrons that can occupy a given shell is determined by the ___.
value of n.
141
The ___ a shell is from the nucleus, the larger its volume becomes, and the more electrons it can hold.
farther
142
Thus, the first shell can hold only:
Two electrons
143
the second shell holds:
eight electrons
144
the third shell holds how many electrons
18
145
The maximum number of electrons is given by the formula: ____ where n=the shell number.
2n^2
146
Shells are divided into subshells, identified by the letters:
s, p, d, and f
147
The subshells consist of ___.
orbitals
148
The two electrons in an orbital must have ___ spins.
opposite
149
A/An ____ is a region of space where the probability of finding an electron is high.
orbital
150
Each orbital can hold __ electrons.
two
151
Orbital in the first shell:
S orbital
152
Orbital in the second shell
1 s and 3 p orbitals
153
Orbital in the third shell
1 s, 3 p, 5 d orbitals
154
Orbital in the fourth shell
1 s, 3 p, 5 d, 7 f orbital
155
Shapes of the orbital: s orbital
Sphere
156
Shapes of the orbital: p orbital
Dumbell
157
Shapes of the orbital: d orbital
Cloverleaf
158
Shapes of the orbital: f orbital
Complex
159
It is lower in energy than other orbitals in the same shell because electrons are kept closer to the positively charged nucleus.
S orbital
160
A ___ is higher in energy than an s orbital in the same shell because its electron density is farther from the nucleus.
p orbital
161
The lowest-energy arrangement of electrons is called the ___.
ground state
162
Rules to Determine the Ground-State Electronic Configuration of an Atom
Rule [1]
Electrons are placed inthe lowest-energy orbitals beginning with the 1s orbital.
Rule [2]
Each orbital holds a maximumof two electrons
Rule [3]
When orbitals are equal in energy, one electron is added to each orbital until the orbitals are half filled, before any orbital is completely filled.
163
Period 1
1s
164
Period 2 (1-2a)
2s
165
Period 2 (3a-8a)
2p
166
Transition metals
d
167
Inner transition metals
f
168
Group 1-2a
S orbitals
169
Group 3a-8a
P orbitals
170
The chemical properties of an element depend on the most loosely held electrons that is, the outermost shell, called the ____.
valence shell
171
The ___ tells the number of the valence shell.
period number
172
The electrons in the outermost shell are called the ____.
valence electrons
173
The group number of a main group element is?
the number of valence electrons
174
The chemical properties of a group are similar because these elements contain:
The same electronic configuration of valence electrons
175
The number of valence electrons around an atom is often represented by an ____.
electron-dot symbol
176
Many properties of atoms exhibit ___; that is, they change in a regular way across a row or down a column of the periodic table.
periodic trends
177
The size of an atom is measured by its ____ that is, the distance from the nucleus to the outer edge of the valence shell.
atomic radius
178
The size of atoms ____ down a column of the periodic table, as the valence electrons are farther from the nucleus.
increases
179
The size of atoms ____ across arow of the periodic table as the number of protons in the nucleus increases. An increasing number of ____ pulls the electrons closer to the nucleus, so the atom gets smaller.
decreases
protons
180
Because a negatively charged electron is attracted to a positively charged nucleus, energy is required to ___.
remove an electron from a neutral atom
181
Removing an electron from a neutral atom forms a ___.
cation
182
This is the energy needed to remove an electron from a neutral atom.
ionization energy
183
Ionization energies ____ down a column of the periodic table as the valence electrons get farther from the positively charged nucleus.
decrease
184
Ionization energies generally ___ across a row of the periodic table as the number of protons in thenucleus increases.
increase
185
