Exam Flashcards
(193 cards)
1
Q
Electromagnetic radiation is a kind of
A
Energy
2
Q
that behaves like a(n)
A
Wave
3
Q
is one type of electromagnetic radiation. Other examples include X rays, radio waves, and microwaves. All waves can be characterized by their wavelength, amplitude, frequency,
A
Speed
4
Q
The shortest distance between equivalent points on a continuous wave is called a(n)
A
wavelength
5
Q
The height of a wave from the origin to a crest or from the origin to a trough is the
A
amplitude
6
Q
is the number of waves that pass a given point in one second
A
Frequency
7
Q
Wavelength is measured in
A
Meters
8
Q
That has the symbol?
A
M
9
Q
We measure frequency in
A
Hertz
10
Q
That has the symbol
A
Hz
11
Q
A(n) is the minimum amount of energy that can be lost or gained by an atom.
A
quantum
12
Q
The is the phenomenon in which electrons are emitted from a metal’s surface when light of a certain frequency shines on it.
A
photoelectric effect
13
Q
When an atom emits light, photons having certain specific energies are being emitted.
A
True
14
Q
A flame test cannot be used to identify the presence of certain elements in a compound.
A
False
15
Q
The fact that only certain colors appear in an element’s atomic emission spectrum indicates that only certain frequencies of light are emitted
A
True
16
Q
Atomic emission spectra can be explained by the particle model of light.
A
False
17
Q
The neon atoms in a neon sign emit their characteristic color of light as they release energy
A
True
18
Q
Like the visible spectrum, an atomic emission spectrum is a continuous range of colors.
A
False
19
Q
When an atom emits light, photons having certain specific energies are being emitted.
A
True
20
Q
Each element does not have a unique atomic emission spectrum.
A
False
21
Q
There are three main classifications of elements.
A
True
22
Q
There are three main classifications of elements.
A
True
23
Q
Group 7A elements are highly reactive nonmetals known as noble gases.
A
False
24
Q
Group 4A elements are the alkaline earth metals.
A
False
25
Alkaline earth metals do not react with oxygen.
False
26
Alkali and alkaline earth metals are not reactive.
False
27
The metal lithium has a diagonal relationship with the metal aluminum.
False
28
An alloy is a compound of two or more metals.
True
29
Alkali metals are shiny gray solids soft enough to be cut by a knife.
True
30
The order of reactivity of the alkaline earth metals, from least to most reactive, is beryllium, magnesium, calcium, strontium, and barium.
True
31
Sodium and potassium are the most abundant alkali metals.
True
32
Sodium and potassium are the most abundant alkali metals.
True
33
Barium chloride can be used as a substitute for sodium chloride.
False
34
Alkaline earth metals form ions with a 2+ charge.
True
35
The ending -ide is used to designate an anion.
True
36
The ending -ide is used to designate an anion.
True
37
Elements in group 1A lose their one valence electron, forming an ion with a 1- charge
False
38
```
The electron structure of a zinc ion (
Z
n
2
+
Zn
2+
) is an example of a pseudo-noble gas formation.
```
True
39
A positively charged ion is called an anion.
False
40
The lowest allowable energy state of an atom is called its
Ground states
41
Bohr’s model of the atom predicted the
Frequencies
42
According to Bohr’s atomic model, the smaller an electron’s orbit, the
Lower
43
According to Bohr’s atomic model, the larger an electron’s orbit, the
Higher
44
Bohr proposed that when energy is added to a hydrogen atom, its
Electron
45
According to Bohr’s atomic model, the hydrogen atom emits a photon corresponding to the difference between the
Energy levels
46
Bohr’s atomic model failed to explain the blank of elements other than hydrogen.
Atomic emission spectrum
47
Atomic orbitals blank have an exactly defined size
Do not
48
Each orbital may contain at most electrons.
Two
49
The maximum number of blank related to each principal energy level equals
Electron
50
Principal energy level 2 consists of
2s and 2p
51
Strontium - period:
Valence electron:
Block:
Period: 5
Block: s
Valence electron: 2
52
Potassium
Period: 6
Block: d
Valence electron: 2
53
Osmium -
Period: 6
Block:d
Valence electron: 2
54
According to Planck’s theory, for a given frequency, ν ν , matter can emit or absorb energy only in
whole-number multiples of hν
55
Which equation would you use to calculate the energy of a photon?
E photon=hν E photon
=hν
56
The modern model of the atom that treats electrons as waves
quantum mechanical model of the atom
57
Originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom
Schrödinger wave equation
58
States that it is impossible to know both the velocity and the position of a particle at the same time
Heisenberg uncertainty principle
59
A three-dimensional region around the nucleus representing the probability of finding an electron
atomic orbital
60
The arrangement of electrons in an atom is called the atom’s
electron configuration
61
Electrons in an atom tend to assume the arrangement that gives the atom the
Lowest
62
This arrangement of electrons is the most arrangement and is called the atom’s ground-state.
Stable and electron configuration
63
states that each electron occupies the lowest energy orbital available.
Aufbau principle
64
The Pauli exclusion is
principle
65
states that a maximum of two electrons may occupy a single atomic orbital, but only if the electrons have opposite
spins
66
states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins occupy the same orbitals.
Hund’s rule
67
Give the ground state electron configurations for the following elements. Use the following format:principle quantum number, sublevel, number of valence electrons, repeat. You do not have to use the ^ for the exponent
Carbon: 1s^2 2s^2 2p^2 1s^2 2s^2 2p^2
68
Chromium
1s^ 2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^4
69
The s-block contains groups
1A and 2A
70
How many d-block elements are there? (number)
40
71
There are blank f-block elements. (number)
28
72
The table below was developed by John Newlands and is based on a relationship called the law of
octaves
73
According to this law, the properties of the elements repeated every
Eight element
74
Thus, for example, element two and element
Nine
75
have similar properties. The law of octaves did not work for all the known elements and was not generally
Accepted
76
The first periodic table is mostly credited to
Dmitri Mendeleev
77
In his table, the elements were arranged according to increasing
Atomic mass
78
One important result of this table was that the existence and properties of undiscovered
Element
79
could be predicted. The elements in the modern periodic table are arranged according to increasing
Atomic number
80
as a result of the work of
Henry Moseley
81
This arrangement is based on number of
Protons
82
in the nucleus of an atom of the element. The modern form of the periodic table results in the
periodic law
83
which states that when elements are arranged according to increasing atomic number, there is a periodic repetition of their chemical and physical
Properties
84
Indicate the trend across a period and down a group for ionic radii, using increase or decrease
Decrease and increase
85
Indicate the trend across a period and down a group for electronegativity using increase or decrease.
Increase and decrease
86
The general trend in the radius of an atom moving down a group is partially accounted for by the
shielding of the outer electrons by inner electrons
87
arsenic (As)
nitrogen (N)
88
bromine (Br)
iodine (I)
89
gallium (Ga)
boron (B)
90
iridium (Ir)
cobalt (Co)
91
nickel (Ni)
platinum (Pt)
92
osmium (Os)
iron (Fe)
93
sodium (Na)
cesium (Cs)
94
tungsten (W)
chromium (Cr)
95
zirconium (Zr)
hafnium (Hf)
96
Elements that are shiny and conduct electricity
metals
97
Group B elements
transition elements
98
A row on the periodic table
Period
99
Group A elements
representative elements
100
A column on the periodic table
Group
101
Atomic radii cannot be measured directly because the electron cloud surrounding the nucleus does not have a clearly defined
outer edge
102
A(n) ion is an atom, or bonded group of atoms, that has a
positive/ negative
103
The block portion of the periodic table span two groups because it can hold a max of two electrons
S
104
The group blank are virtually unreactive because they have a full valence level
8A
105
The p-block contains elements in groups
3A through 8A
106
An atom becomes negatively charged by
Gaining electron
107
Choose the most reactive element
K
108
Choose the most reactive element
Fr
109
Plants and animals get the nitrogen they need
from nitrogen-fixing bacteria.
110
The release of phosphate ions from fertilizers or detergents into bodies of water may lead to depletion of dissolved oxygen because
phosphate ions serve as nutrients for algae.
111
The best conductor of electricity
Silver
112
Used in electrical wiring
Copper
113
Are classified as “strategic” metals
tungsten,chromium,cobalt,platinum, manganese
114
Found in molecules that help the body digest proteins and eliminate carbon dioxide
Zinc,
115
Involved in cell respiration
manganese,copper
116
Found in the center of a hemoglobin molecule
Iron,
117
Provides a protective coating to resist rusting
Zinc
118
Needed for the development of red blood cells
Cobalt
119
The main element in steel
Iron
120
Choose two ways that hydrogen is produced in a lab.
using electricity to separate water into its parts
metal reacts with an acid
121
treating bipolar disorders
lithium
122
fertilizers
potassium
123
chalk
calcium
124
X rays
barium
125
nonsparking tools
beryllium
126
fireworks
strontium
127
baking soda
Sodium
128
Choose the most reactive element
F
129
The major industrial use for nitrogen is to make
ammonia
130
Ozone is
an allotrope of oxygen
131
Write the ground state electron configurations for titanium (Ti), vanadium (V), chromium (Cr), and manganese (Mn)
?
132
Ti
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2
133
V
1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3
134
Transition metals are elements whose final electron enters a blank sub level and inner transition metals are elements whose final electron enters an blank sub level.
d and f
135
is the most abundant element in the Earth's crust
Oxygen
136
Some of the uses for phosphorous are in cleaning products and
fertilizers
137
The second most abundant element in Earth’s crust is
silicon
138
The branch of chemistry that studies most
Carbon
139
Boron nitride and aluminum oxide are both
abrasives
140
is found in California in the form of borax.
Boron
141
Hydrogen acts like a blank by gaining an electron and acts like a blank by losing an electron
Nonmetal and metal
142
Elements in group 1A have blank valence electron and elements in group blank have 2 valence electrons
One and 2A
143
Groups 1A-8A elements are called the blank because they have a wide range of chemical and physical properties.
Representative and Element
144
The most chemically active of all the elements is
fluorine
145
A transition metal can form an ion with a charge of 3+ or higher by losing blank valence electrons plus unpaired d electrons.
2
146
block elements contain metals, metalloids , nonmetals, and noble gases
p
147
Elements in the same group don't have the same properties because they don't have the same number of blank electrons and more energy levels.
nonvalence
148
Elements in the same group have the same number of blank electrons.
valence
149
Some blank used in the home contain americium.
smoke, detectors
150
The actinides are blank and decay in the form of particles or rays of energy.
Radioactive
151
Welders’ goggles contain neodymium and praseodymium because these elements absorb high energy . Aluminum is the most abundant blank in Earth’s crust
Radiation,metal
152
Graphite and diamond are examples of blank because they are different forms of the same element in the blank of matter.
allotropes,state
153
Carbonates, cyanides, carbides, sulfides, and oxides of carbon are classified as inorganic compounds. Geologists call these substances.
Minerals
154
Computer chips made of blank are less efficient than gallium chips
silicon
155
is used as an energy source by certain bacteria living near ocean vents.
Hydrogen, sulfide
156
Blank is used in solar panels because it can convert light into electricity.
Selenium
157
Some of the uses for blank are in bleaches, disinfectants, and plastics.
chlorine
158
Differences in properties among the blank elements can be explained by the ability of d electrons that move into the valence level.
transition
159
Elements with atomic numbers above blank are called transuranic elements.
92
160
Because some of its compounds emit red light when excited by electrons, blank is often used in TV screens.
yttrium
161
Because there is little difference in the properties of the blank they are usually found mixed together in nature.
lanthanides
162
Transition metals can be separated by blank electricity or by using solutions.
heat
163
The force that holds two atoms together is called a(n) blank.
chemical bond
164
Such an attachment may form by the attraction of the positively charged blank of one atom for the negatively charged blank
nucleus, electron
165
of another atom, or by the attraction of charged atoms, which are called blank.
ions
166
The attractions may also involve blank electrons, which are the electrons in the outermost.
Valence,energy level
167
The noble blank are a family of elements that have very little tendency to react.
gases
168
Most of these elements have a set of eight outermost electrons, which is called a stable.
octet
169
An ionic bond is
a force that holds together atoms that are oppositely charged
170
The overall charge of a formula unit for an ionic compound
Is always zero
171
Ionic bonds generally occur between
a metal and a nonmetal
172
A three-dimensional arrangement of particles in an ionic solid is called a(n)
crystal lattice
173
What is the relationship between lattice energy and the strength of the attractive force holding ions in place
The more negative the lattice energy is, the greater the force
174
In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, which of the following is correct?
The nonmetallic atom gains electrons from the metallic atom
175
Ionic compounds usually do not have a blank melting point.
high
176
They have a blank boiling point.
high
177
As far as their hardness goes, they are blank.
Hard
178
As far as their brittleness, they are .
Brittle
179
The formula unit of an ionic compound shows the
simplest ratio of the ions.
180
Salts are examples of
ionic compounds,
181
In a crystal lattice of an ionic compound,
ions are surrounded by ions of the opposite charge
182
The formation of a stable ionic compound from ions
is always exothermic.
183
Electrical conductivity in the liquid state
Good
184
Electrical conductivity in the solid state
Poor
185
Electrical conductivity when dissolved in water
Good
186
A one-atom ion is called a(n) blank ion. The charge of such an ion is equal to the atom’s blank. ,
Monatomic, oxidation number
187
which is the number of blank transferred to or from the atom to form the ion. In ionic compounds, the sum of the charges of all the ions equals blank.
electrons, zero
188
Ions made up of more than one atom are called blank ions.
polyatomic
189
If such an ion is negatively charged and includes one or more oxygen atoms, it is called a(n) blank.
oxyanion
190
If two such ions can be formed that contain different numbers of oxygen atoms, the name for the ion with more oxygen atoms ends with the suffix blank . The name for the ion with fewer oxygen atoms ends with.
-ate, -ite
191
In the chemical formula for any ionic compound, the chemical symbol for the blank is written first, followed by the chemical symbol for the blank.
anion,cation
192
A(n) blank is a small number used to represent the number of ions of a given element in a chemical formula.
subscript
193
Such numbers are written to the blank of the symbol for the element.
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