More review Flashcards
(173 cards)
1
Q
Which of the following trends in the periodic table should be expected as the atomic number of the halogens increases from fluorine (F) to iodine (I)?
A
B. Electronegativity decreases.
2
Q
Which is an example of an element?
A
B. lead
3
Q
Which Lewis dot structure represents an element that should be placed in column VIIA (17) of the periodic table?
A
C.
4
Q
Why are elements of the alkali metal family highly reactive?
A
A. Alkali metals are easily ionized.
5
Q
What is the best way to determine if an object is made of pure silver?
A
C. determine the density of the object and compare the known density of pure silver.
6
Q
Isotopes of an atom could be detected based on which characteristic?
A
C. nuclear mass.
7
Q
How many protons are in an atom of bromine?
A
D. 35.
8
Q
What is the mass number of an atom with 29 protons, 29 electrons, and 35 neutrons?
A
D. 93.
9
Q
Why are cations smaller than the atoms from which they are formed?
A
B. The metallic atom loses electrons, resulting in loss of an entire energy level.
10
Q
What is the formula for a compound formed from sodium (Na) and oxygen (O)?
A
C. Na2O.
11
Q
What can be concluded about a substance that dissolves well in water but not in benzene?
A
C. The substance is polar.
12
Q
Which Lewis dot structure represents the compound methane (CH4)?
A
A.
13
Q
Which property of water most likely causes large rocks to break apart?
A
A. Water expands when it freezes.
14
Q
What does the data indicate about how temperature affects states of matter?
A
B. temperature physically changes matter.
15
Q
What best explains the high melting point of salt?
A
D. the strong electrostatic attraction between Na+ and Cl-.
16
Q
What does water change to as it boils?
A
A. Gas.
17
Q
What best describes the reason for the increase in pressure when a gas is heated in a closed container?
A
C. The average kinetic energy of the gas molecules increases.
18
Q
Which of the following does not increase as a gas is heated?
A
D. the average distance between the gas molecules.
19
Q
What best describes the nitrogen gas in box A if it has twice the average speed of the molecules in box B?
A
C. The nitrogen gas in box A has a greater temperature than the nitrogen gas in box B.
20
Q
What property describes KCl(s) after the water in KCl(aq) is completely evaporated?
A
C. The melting point of the KCl(s) is unchanged.
21
Q
Which two particle diagrams represent two different phases of the same compound?
A
B. A and C.
22
Q
A substance is classified as either an element or a?
A
A. compound.
23
Q
Tetrachloromethane, CCl4, is classified as a?
A
A. compound because the atoms of the elements are combined in a fixed proportion.
24
Q
Which sample of matter cannot be broken down by a chemical change?
A
A. antimony.
25
Which substance cannot be decomposed by a chemical change?
D. Cu.
26
What is the percent error for a student's measured value of water in a hydrate if the accepted value is 36.0% and the student measured 37.8%?
B. 4.8%.
27
What is the percent error in a student's result if the molecular mass for O2(g) is 32.0 and the student measured it to be 28.0?
C. 12.5%.
28
What is the percent error if a student determined the percent by mass of water in a hydrated salt to be 17.3% and the accepted value is 14.8%?
B. 5.92%.
29
Which kelvin temperature is equal to 56 °C?
A. 329 K.
30
Compared to the Celsius temperature of a sample, the Kelvin temperature will always be?
A. 273 ° greater.
31
As elements in Period 3 are considered from left to right, what happens?
C. increase in number of protons.
32
How do the relative electronegativity and covalent radius of elements Li to F compare?
C. The relative electronegativity increases, and the covalent radius decreases.
33
As elements in Group IA are considered in order of increasing atomic number, what happens to the atomic radius?
D. increases due to an increase in the number of principal energy levels.
34
What happens as elements in Period 2 are considered from lithium to fluorine?
B. increase in electronegativity.
35
Which Period 4 element has the most metallic properties?
D. Sc.
36
Which element has chemical properties most similar to calcium?
C. Mg.
37
Which symbol represents an alkaline earth element?
B. Mg.
38
In which group would a nonmetallic element belong if it tends to gain two electrons?
C. 16.
39
Which group contains a metalloid?
C. 15.
40
What describes the elements in Period 3?
D. All elements have valence electrons in the same principal energy level.
41
Which element in Period 3 exists as diatomic molecules at STP?
A. chlorine.
42
What is the basis for the arrangement of elements in Period 4?
B. atomic number.
43
Which period contains more metallic elements than nonmetallic elements?
D. Period 4.
44
Which atom in the ground state has a stable electron configuration?
C. neon.
45
Which element has the greatest number of valence electrons in the ground state?
D. fluorine.
46
What do arsenic and silicon have in common?
D. are metalloids.
47
Which element exhibits both metallic and nonmetallic properties?
D. tellurium.
48
The element sulfur is classified as a?
C. nonmetal.
49
Which elements are both classified as metalloids?
A. Ge and As.
50
Which metal will undergo the greatest degree of corrosion if left unprotected?
D. iron.
51
Which element is malleable and a good conductor of electricity at STP?
D. silver.
52
Low ionization energies are most characteristic of atoms that are?
A. metals.
53
Which element would have properties characteristic of both a metal and a nonmetal?
C. Si.
54
Which element is most likely a nonmetal based on the properties in the table?
D. D.
55
Which nonmetallic element is a liquid at STP?
B. bromine.
56
Which element is a nonmetal and solid at STP?
D. sulfur.
57
Which atom has the greatest ability to attract electrons in a bond with an H atom?
D. chlorine.
58
What is the most likely electronegativity value for a metallic element?
A. 1.3.
59
If the electronegativity difference in NaX is 3.1, what is the element represented by X?
A. F.
60
Which atom has the weakest attraction for electrons in a bond with an H atom?
D. S atom.
61
Which group on the Periodic Table has the element with the highest electronegativity?
C. Group 17.
62
Which group has the highest electronegativity?
C. Group 17
63
What ions are dissolved in a 500-gram sample of bottled water?
Ca 2+, Mg 2+, Na +, SO 2-4, HCO 3-
64
How does the radius of a Mg 2+ ion compare to the radius of a Mg atom?
The Mg 2+ ion is smaller than the Mg atom.
65
How does the size of an aluminum atom change when it becomes an ion with a charge of +3?
A. It becomes smaller by losing 3 electrons.
66
When an atom loses one or more electrons, what does it become?
A. positive ion with a radius smaller than the radius of this atom
67
What is the atomic radius of Period 3 elements?
Atomic numbers and corresponding atomic radii are: 11 - 160 pm, 12 - 140 pm, 13 - 124 pm, 14 - 114 pm, 15 - 109 pm, 16 - 104 pm, 17 - 100 pm, 18 - 101 pm.
68
How does the size of a barium ion compare to the size of a barium atom?
C. The ion is larger because it has fewer electrons.
69
Which element in Group 1 has the greatest tendency to lose an electron?
A. cesium
70
Which element in Period 3 has the least tendency to lose an electron?
A. argon
71
From which of these atoms in the ground state can a valence electron be removed using the least amount of energy?
D. chlorine
72
Which element has an atom with the electron configuration 2-8-8-2?
B. Ni
73
What is the electron configuration of a sulfur atom in the ground state?
D. 2-8-6
74
What is the total number of valence electrons in an atom of electron configuration X (2-8-8-2)?
The total number of valence electrons is 2.
75
Which Lewis electron-dot diagram is correct for a S 2- ion?
A.
76
Which electron dot symbol represents an atom of chlorine in the ground state?
A.
77
Draw a Lewis electron-dot diagram for a fluoride ion.
The diagram shows 8 electrons around F.
78
What is the correct Lewis electron-dot structure for the compound magnesium fluoride?
A.
79
Draw a Lewis electron-dot diagram for a molecule of phosphorus trichloride, PCl3.
The diagram shows P with 5 electrons and 3 Cl atoms each with 7.
80
What is the maximum number of electrons that can occupy the second principal energy level?
B. 8
81
A substance conducts electricity in the liquid phase but not in the solid phase. This substance can be classified as?
B. ionic
82
Identify the two types of bonds in the compound sodium stearate.
Ionic and covalent bonds.
83
The bonds present in silicon carbide (SiC) are?
A. covalent
84
Identify the type of bonding in solid potassium.
Metallic bonding.
85
Identify the type of bonding in a fullerene molecule.
Covalent bonding.
86
Which formula represents a salt?
B. KCl
87
When ionic bonds are formed, metallic atoms tend to?
B. lose electrons and become positive ions.
88
Which substance contains a bond with the greatest ionic character?
A. KCl
89
Write the chemical formula for one compound in the equation that contains both ionic bonds and covalent bonds.
NaHCO3
90
Which molecule can form a coordinate covalent bond?
A. H: .. .. N:H
91
Metallic bonding occurs between atoms of?
B. copper
92
Metallic bonding occurs between metal atoms that have?
C. vacant valence orbitals and low ionization energies.
93
Which substance contains a polar covalent bond?
C. NH3
94
Which type of bond forms when electrons are equally shared between two atoms?
B. a nonpolar covalent bond
95
In a nonpolar covalent bond, electrons are?
C. shared equally by two atoms.
96
The least polar bond is found in a molecule of?
A. HI
97
Which molecule contains a nonpolar covalent bond?
B. F2
98
Which type of substance can conduct electricity in the liquid phase but not in the solid phase?
A. ionic compound
99
The high electrical conductivity of metals is primarily due to?
C. mobile electrons.
100
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
D. metallic, because the valence electrons are mobile.
101
A solid sample of a compound and a liquid sample of the same compound are each tested for electrical conductivity. Which test conclusion indicates that the compound is ionic?
D. The solid is a poor conductor, and the liquid is a good conductor.
102
Explain, in terms of particles in the atoms of an element, why statement C of Dalton's atomic theory is false.
Atoms of the same element can have different masses due to isotopes.
103
State one aspect of the modern model of the atom that agrees with a conclusion made by Thomson.
Atoms contain negatively charged particles (electrons).
104
Which conclusion is based on the 'gold foil experiment' and the resulting model of the atom?
A. An atom is mainly empty space, and the nucleus has a positive charge.
105
According to the wave-mechanical model, an orbital is defined as the most probable location of?
D. an electron.
106
Explain, in terms of particles, why statement A of Dalton's atomic theory is no longer accepted.
Atoms can be divided into smaller particles (protons, neutrons, electrons).
107
Which particles are found in the nucleus of an atom?
D. protons and neutrons.
108
What is the most probable location of an electron?
A. an orbital.
109
Which particles are found in the nucleus of an argon atom?
C. protons and neutrons.
110
Which statement explains why a xenon atom is electrically neutral?
D. The atom has the same number of protons and electrons.
111
Subatomic particles can usually pass undetected through an atom because the volume of an atom is composed of?
B. largely empty space.
112
The atomic number of any atom is equal to the number of?
B. protons in the atom, only.
113
In a sample of pure copper, all atoms have atomic numbers which are?
A. the same and the atoms have the same number of electrons.
114
A sample composed only of atoms having the same atomic number is classified as?
C. an element.
115
All atoms of uranium have the same?
B. atomic number.
116
The mass of one carbon atom is approximately equal to the total mass of?
C. 12 nucleons.
117
What is the mass number of an atom that contains 19 protons, 19 electrons, and 20 neutrons?
C. 39.
118
What is the mass number of an atom which contains 28 protons, 28 electrons, and 34 neutrons?
C. 62.
119
Which two particles have opposite charges?
B. an electron and a proton.
120
Which particles may be gained, lost, or shared by an atom when it forms a chemical bond?
B. electrons.
121
What is the charge and mass of a proton?
A. charge of +1 and mass of 1 amu.
122
The mass of a proton is approximately equal to the mass of?
B. a neutron.
123
An atom in the ground state has two electrons in its first shell and six electrons in its second shell. What is the total number of protons in the nucleus of this atom?
C. 8.
124
What is the total number of neutrons in the nucleus of a neutral atom that has 19 electrons and a mass number of 39?
B. 20.
125
A neutron has a charge of?
A. +1.
126
What is the total number of protons in an atom with 2 electrons in its first shell and 6 electrons in its second shell?
8
127
What is the total number of neutrons in a neutral atom that has 19 electrons and a mass number of 39?
20
128
What charge does a neutron have?
0
129
Which particle has two neutrons?
4 2 He
130
In which pair of atoms do both nuclei contain the same number of neutrons?
40 19 K and 40 17 Cl
131
What is the number of electrons in an atom that has 3 protons and 4 neutrons?
3
132
Compared to the charge of a proton, the charge of an electron has?
the same magnitude and the opposite sign
133
The mass of an electron is approximately 1/1836 times the mass of which particle?
1 1 H
134
What is the total number of electrons in a Mg 2+ ion?
10
135
When a lithium atom forms an Li + ion, the lithium atom?
loses an electron
136
What is the net charge of an ion that has 11 protons, 10 electrons, and 12 neutrons?
1+
137
If the nucleus of an atom is represented as 24 11 X, the atom is?
Mg
138
What is the total number of electrons in an atom of Cu-65?
29
139
How many different elements are represented by the nuclei in the table?
4
140
What is the neutron to proton ratio for an atom of 58 Fe?
1
141
Which two nuclides are isotopes of the same element?
14 6 C and 14 7 N
142
Write an isotopic notation of the heavier isotope of the element boron.
B-11
143
Explain, in terms of protons and neutrons, why I-127 and I-131 are different isotopes of iodine.
They have different numbers of neutrons.
144
The atomic mass of an element is the weighted average of the?
atomic masses of the naturally occurring isotopes of that element
145
Calculate the atomic mass of boron given the isotopes.
10.81
146
Compare the relative abundances of the naturally occurring isotopes of nitrogen.
N-14 is more abundant than N-15.
147
What is the total number of atoms in 1 mole of calcium?
6.02 x 10^23
148
State evidence that indicates the sample undergoes only physical changes during heating.
The substance changes from solid to gas without a chemical reaction.
149
Given the reaction: 4NH3(g) + 5O2(g) ! 4NO(g) + 6H2O(g), how many liters of O2(g) would be required to produce 40 liters of NO(g)?
50
150
At STP, which gas sample has a volume of 11.2 liters?
1.00 mole of CO2
151
If 28.0 grams of a gas occupies 22.4 liters at STP, the gas could be?
CO2
152
Determine the total number of moles of CO2 added to the tank before it is used for paintball.
7.7 moles
153
What is the volume occupied by 11.0 grams of a gas at STP if the molecular mass of the gas is 44.0?
22.4 L
154
At constant pressure, if 50 mL of a gas at 20 °C is heated to 30 °C, the new volume is equal to?
50 x 303/293
155
What volume will the gas have at a pressure of 150 torr and a temperature of 200 K?
200 mL
156
Determine the volume of the helium gas when the pressure is increased to 1.50 atm.
100 mL
157
When the pressure exerted on a confined gas at constant temperature is doubled, the volume of the gas is?
halved
158
As a given volume of gas is compressed, the number of molecules?
remains the same
159
As the piston moves downward, the number of molecules of air in the cylinder?
remains the same
160
What is the answer to question 80?
covalent bonds and ionic bonds, polar and nonpolar, single and double
161
What is the answer to question 82?
metallic bonding
162
What is the answer to question 83?
nonpolar covalent
163
What is the answer to question 87?
NaHCO3 or NH4Cl
164
Why do atoms of different isotopes of an element have different masses?
Atoms of different isotopes of an element have different masses because they have different numbers of neutrons.
165
What is true about the charge of an atom?
An atom has equal amounts of negative and positive charge. An atom has an equal number of protons and electrons. All atoms contain electrons. Electrons are negatively charged.
166
What exists as smaller parts of atoms?
Smaller parts of atoms exist, such as protons, neutrons, and electrons.
167
What is the charge and particle type for an electron?
Particle: electron
Charge of particle: 1
Charge of particle: negative
168
What is the atomic number of copper?
29
169
What is the neutron-proton ratio for an isotope?
32:26
170
Which nitrogen isotope is more abundant?
Nitrogen-14 is more abundant than nitrogen-15.
171
What is an example of a chemical change?
Example answer: No new substance is formed.
172
What is the acceptable range for the answer to question 150?
7.73 mol or any value from 7.7 mol to 8 mol, inclusive.
173
What is the answer to question 154?
100 mL
