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Unit 2 Practice Questions Atomic Theory. Questions 1-4 refer to the following: Proton Neutron Electron Isotope Ion Neutral charge; 1 amu Positive charge Negligible weight Negative charge; pairs with opposite spin. Questions 1-4 refer to the following: Atom Ion Neutron Proton - PowerPoint PPT Presentation
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1
Unit 2 Practice QuestionsI. Atomic Theory
Questions 1-4 refer to the following:
(A) Proton(B) Neutron(C) Electron(D) Isotope(E) Ion
1. Neutral charge; 1 amu2. Positive charge3. Negligible weight4. Negative charge; pairs with opposite spin
2
Questions 1-4 refer to the following:
(A) Atom(B) Ion(C) Neutron(D) Proton(E) electron
1. The smallest representative particle of helium2. Loss or gain creates positively or negatively
charged ion, respectively3. Particle responsible for positive nuclear charge4. Isotopes of uranium always differ in their number
of this particle5. Their number in the nucleus determines an
element’s atomic number
3
I
The periodic table does not report mass numbers
II
A mass number can be assigned to one isotope of an element but not to an element in general
Addition of an electron to an atom creates a positively charged ion
Every electron carries a negative charge
BECAUSE
BECAUSE
4
I
Ca is a neutral atom
II
It has the same number of protons and electrons
An element (X) with an atomic number of 16 has 14 electrons in X-2
Two protons bind the two outermost electrons
BECAUSE
BECAUSE
5
I
Two isotopes of the same element have the same mass number
II
Isotopes have the same number of protons
An atom of 12C contains 12 protons
The identity of an element is determined by the number of protons in the nuclei of its atoms
BECAUSE
BECAUSE
6
I
The atomic number of a neutral atom that has a mass of 39 and has 19 electrons is 19
II
The number of protons in a a neutral atom is equal to the number of electrons
A large number of alpha particles were deflected in the Rutherford experiment
Alpha particles that came close to the nucleus of the gold atoms were deflected
BECAUSE
BECAUSE
7
I
The isotope Cl-37 has 17 protons, 17 neutrons, and 17 electrons
II
The atomic mass of chlorine is 35.43 amu
BECAUSE
8
Which of the following is not a conclusion Rutherford made from his experiment with alpha particles being shot at a thin sheet of gold foil?
(A) An atom has a very small, compact nucleus(B) An atom is mainly empty space(C) An atom’s mass is concentrated in the nucleus(D) An atom has a very dense nucleus(E) An atom has a negatively charged nucleus
9
Which of the following statements is false regarding sub-atomic particles?
(A) The proton has a positive one charge(B) The neutron has no charge(C) The electrons are found in regions of the atom
called orbitals(D) The electrons have a greater mass than the
protons(E) Protons and neutrons are the nucleons of the
atom
10
The two main regions of an atom are the
(A) Principal energy levels and energy sublevels(B) Nucleus and kernel(C) Nucleus and energy levels(D) Planetary electrons and energy levels
11
An atom of beryllium consists of 4 protons, 5 neutrons and 4 electrons. The mass number of this atom is
(A) 13(B) 9(C) 8(D) 5
12
A mysterious element has the following relative abundances: X-34 15%, X-35 20%, X-36 65%Which of the following is true?
(A) The atomic mass of the element is closer to 34.1(B) The atomic mass of the element is closer to 34.9(C) The atomic mass of this element cannot be
determined without knowing exactly what X is(D) A mass spectrophotometer would not be
helpful in determining the percentages of the isotopes
(E) The atomic mass of this element is approximately 35.5
13
Atoms of 235U and 238U differ in structure by three
(A) Electrons(B) Isotopes(C) Neutrons(D) protons
14
Which of the following pairs of compounds can be used to illustrate the Law of Multiple Proportions?
(A) NO and NO2
(B) CH4 and CO2
(C) ZnO2 and ZnCl2
(D) NH3 and NH4Cl(E) H2O and HCl
15
Two different sodium atoms or ions may differ in all of the following ways EXCEPT
(A) The number of electrons outside their nuclei(B) The overall charge they carry(C) Their mass numbers(D) The number of neutrons in their nuclei(E) The number of protons in their nuclei
16
Which of the following isotopes has the greatest number of neutrons?
(A) 35Cl(B) 31P(C) 40Ar(D) 41Ca(E) 14C
17
Which is inconsistent with the concept of an isotope?
(A) Same atomic number(B) Different number of neutrons(C) Same mass number(D) Same name of the element(E) Same number of protons
18
Two isotopes of the same element will always differ in
(A) Mass number but never in atomic number(B) Atomic number but never in mass number(C) Charge outside but never inside their nuclei(D) Nuclear charge but never in overall charge(E) The number of electrons outside their nuclei
but never in the number of neutrons inside their nuclei
19
What is the number of protons and neutrons in an atom with mass number 89 and atomic number 39?
(A) 50 protons and 50 neutrons(B) 50 protons and 39 neutrons(C) 39 protons and 89 neutrons(D) 39 protons and 50 neutrons(E) 39 protons and 39 neutrons
20
Twenty-five percent of element X exists as 210X and seventy-five percent of it exists as 214X. What is the atomic weight of element X in amu?
(A) 85(B) 211(C) 212(D) 213(E) 214
21
Which of the following combinations represents an element with a net charge of +1 with a mass number of 75?
(A) 35 neutrons, 35 protons, 34 electrons(B) 40 neutrons, 40 protons, 39 electrons(C) 40 neutrons, 35 protons, 34 electrons(D) 37 neutrons, 38 protons, 39 electrons(E) 40 neutrons, 35 protons, 35 electrons
22
Of the following statements about the number of subatomic particles in an ion of 32
16S-2, which are true?
I. 16 protonsII. 14 neutronsIII. 18 electrons
(A) II only(B) III only(C) I and II only(D) I and III only(E) I, II and III
23
Isotopes of an element are related because which of the following are the same in these isotopes?
I. Atomic massII. Atomic numberIII. Arrangement of orbital electrons
(A) I only(B) II only(C) I and II only(D) II and III only(E) I, II and III
24
For the radioactive element 99Tc, what is the correct number of protons and neutrons?
(A) 43 protons and 56 neutrons(B) 43 protons and 99 neutrons(C) 56 protons and 43 neutrons(D) 56 protons and 99 neutrons(E) Cannot be determined
25
II. Nuclear
Questions 1-4 refer to the following:
(A) Alpha particle(B) Beta particle(C) Gamma radiation(D) Neutron(E) Positron
1. Has a negative charge2. Has no mass and no charge3. Has the greatest positive charge4. Is very similar to an electron
26
Questions 1-3 refer to the following:
(A) Alpha decay(B) Beta decay(C) Positron emission(D) Gamma decay(E) Electron capture
1. Often accompanies other radioactive processes2. Causes an atom to reduce its atomic number by 2
and its mass number by 43. Occurs when a neutron is converted into a proton in
a nucleus
27
I
12C is an isotope of 14C
II
The nuclei of both atoms have the same number of neutrons
Alpha particles are the heaviest type of radiation decay
Alpha emission particles consist of 2 protons and 2 neutrons
BECAUSE
BECAUSE
28
I
Nuclear fusion on the sun converts hydrogen to helium with a release of energy
II
Some mass is converted to energy in a solar fusion
The “bullet” usually used to initiate the fusion of 235U is a neutron
Capture of the neutron by the 235U nucleus causes an unstable condition that leads to its disintegration
BECAUSE
BECAUSE
29
I
Radioactive elements can emit alpha particles, beta particles, and gamma rays
II
Radioactive elements have extremely stable nuclei
If a radioactive sample with a half-life of 40 years decays for 80 years, 25% of the sample will remain
One half of 100% is 50%, and one half of 50% is 25%
BECAUSE
BECAUSE
30
In the artificial transmutation 94Be + X 6
3Li + 4
2He, the particle represented by the letter X is a(n)
(A) Beta particle(B) Positron(C) Deuteron(D) Proton(E) Alpha particle
31
146C 14
7N + X
What is X?(A) 4
2He(B) 0
+1e(C) 0
-1e(D) 1
1H(E) 12
6C
This reaction is an example of(A) Alpha decay(B) Beta decay(C) Fusion(D) Gamma decay(E) Positron emission
32
22686Rn 218
84Po + 42He
The radioactive decay shown above is an example of(A) Positron emission(B) Gamma ray emission(C) Alpha decay(D) Beta decay(E) Ionization
33
13153I 131
54Xe + 0-1e
The radioactive decay shown above is an example of(A) Positron emission(B) Gamma ray emission(C) Alpha decay(D) Beta decay(E) Ionization
34
Which equation is an example of an artificial transmutation?
(A) 238U 4He + 234Th(B) 27Al + 4He 30P + 1
0n(C) 14C 14N + 0
-1e(D) 226Ra 4He + 222Rn(E) 99
43Tc 9943Tc + g
35
Which nuclear equation below demonstrates beta decay?
(A) 238U X + 234Th(B) 1H + X 3H(C) 14N + X 17O + 1H(D) 234Pa X + 234U(E) None of the above demonstrates beta decay
36
Element 10220X is formed as a result of 3 alpha and 2
beta decays. Which of the following is the parent element?
(A) 9016A
(B) 11424Z
(C) 11428Q
(D) 128J + 90
12L
37
Radioactive emanations can be detected by using
(A) A person’s DNA(B) A block of lead(C) A Geiger counter(D) An x-ray machine(E) Graphite and heavy water
38
Sodium-24, a radioactive isotope used medically in blood studies, decays by beta decay and has a half-life of 15.0 hours. What is the product of the radioactive decay of sodium-24?
(A) F-20(B) Ne-24(C) Ne-23(D) Na-23(E) Mg-24
39
After 62.0 hours, 1.0 gram remained unchanged from a sample of potassium-42 (half life is 12.4 hours). What was the mas of potassium-42 in the original sample?
(A) 64 grams(B) 32 grams(C) 16 grams(D) 8 grams (E) 4 grams
40
The emission of a beta particle results in a new element with the atomic number
(A) Increased by 1(B) Increased by 2(C) Decreased by 1(D) Decreased by 2
41
The energy released by the detonation of an atomic bomb is NOT related to
(A) Fission of the atom’s nucleus(B) Fusion of the atom’s nucleus(C) A chain reaction(D) The release of many neutrons(E) The uncontrolled speed of many neutrons
42
As a nucleus of a particular isotope disintegrates, another nuclide is formed. This change in the nucleus to form a new nuclide is called
(A) Binding energy(B) Transmutation(C) Stability(D) Generation(E) Synthesis
43
Which element has no known stable isotope?
(A) Carbon(B) Silver(C) Radon(D) Phosphorus(E) Lead
44
Which pair below would not be deflected or attracted by the charged plates in an electric field?
(A) An alpha particle and a neutron(B) A beta particle and a positron(C) A quark and a deuteron(D) A proton and gamma radiation(E) Gamma radiation and a neutron
45
In 6.20 hours, a 50.0 gram sample of silver-112 decays to 12.5 grams. What is the half-life of silver-112?
(A) 1.60 hours(B) 3.10 hours(C) 6.20 hours(D) 12.4 hours(E) 18.6 hours
46
A physicist starts out with 320 grams of a radioactive element Z and after 20 minutes he has only 20 grams left. What is the half-life of element Z?
(A) 2 minutes(B) 3 minutes(C) 4 minutes(D) 5 minutes(E) 10 minutes
47
Which of the following is closest in mass to a proton?
(A) Alpha particle(B) Positron(C) Neutron(D) Electron
48
The daughter nucleus formed when 18F undergoes positron emission is
(A) 14N(B) 16O(C) 18O(D) 19F(E) 20Ne
49
In 12.4 hours, a 100 gram sample of an element decays so that its mass is 25 grams. What is the approximate half-life of this radioactive substance?
(A) 1.6 hours(B) 3.1 hours(C) 6.2 hours(D) 24.8 hours(E) 49.6 hours
50
Which of the following transmutations demonstrates beta decay?
I. Bi-212 Po-212II. Pb-212 Bi-212III. Ra-228 Ac-228
(A) I only(B) II only(C) II and III only(D) I and II only(E) I , II, and III
51
Which of the following forms of radioactive decay have no electrical charge?
I. Alpha decayII. Beta decayIII. Gamma decay
(A) II only(B) III only(C) I and II only(D) I and III only(E) II and III only
52
Which of the following are uses for radiation and radioactivity that are of benefit to us?
I. nuclear wasteII. radioisotopesIII. Excess exposure
(A) I only(B) II only(C) III only(D) I and II only(E) I and III only
53
A patient undergoing treatment for thyroid cancer receives a dose of radioactive iodine, which has a half-life of 8.05 days. If the original dose contained 12 mg of iodine-131, what mass of iodine-131 remains after 16.1 days?
54
III. Electrons
Questions 1-4 refer to the following:(A) 1s(B) 2s(C) 3s(D) 3p(E) 3d
1. Contains up to 10 electrons2. Contains one pair of electrons in the ground state
of lithium3. Is exactly half filled in the ground state of
phosphorus4. Contains a filled orbital in the ground state of
helium
55
I
Two electrons in the 2s subshell must have opposite spins
II
The Pauli exclusion principle states that no two electrons in the same atom can have identical quantum numbers
Gas-phase elements absorb or emit only specific wavelengths of visible light when excited by an electric current
The energy levels that electrons can occupy in gas-phase atoms and molecules are continuous
BECAUSE
BECAUSE
56
I
The 4s orbital fills before the 3d orbitals
II
Subshells fill in the order from lower to higher energy
The ground state electron configuration of Cu is [Ar]4s13d10
Completely filled and half-filled d orbitals bestow special electronic stabilization
BECAUSE
BECAUSE
57
I
An element that has the electron configuration 1s22s22p63s23p64s23d3 is a transition element
II
The transition elements from scandium to zinc are filling the 3d orbitals
BECAUSE
58
In a hydrogen atom, when an electron jumps from an excited energy state to a more stable energy state,
(A) Electromagnetic radiation is emitted by the atom
(B) Electromagnetic radiation is absorbed by the atom
(C) The atom becomes a positively charged ion(D) The atom becomes a negatively charged ion(E) The atom undergoes nuclear decay
59
Which principal energy level has exactly four sublevels?
(A) 1(B) 2(C) 3(D) 4(E) 5
60
Which metal is not correctly paired with its color when put into a flame?
(A) Lithium-red(B) Potassium-lilac(C) Sodium-yellow(D) Copper-orange(E) Magnesium-white
61
All of the following statements are consistent with Bohr’s model of the atom EXCEPT
(A) An electron may assume an infinite number of velocities
(B) An atom is most stable when its electron configuration is that of the ground state
(C) The electron shell numbers represent the principal energy levels
(D) Electrons in orbitals closest to the nucleus have the lowest energy
(E) They are all consistent
62
The maximum number of electrons in a shell with the principal quantum number equal to 4 is
(A) 2(B) 10(C) 16(D) 32
63
If the principal quantum number of a shell is equal to 2, what types of orbitals will be present?
(A) s(B) s and p(C) s, p, and d(D) s, p, d and f
64
An element with an atomic number of 26 has how many electrons in the 3d sublevel?
(A) 0(B) 2(C) 6(D) 8(E) 10
65
Which of the following orbitals has the lowest energy?
(A) 2p(B) 3s(C) 3d(D) 4s(E) 3p
66
How many valence electrons are in an atom with the configuration 1s22s22p63s23p2?
(A) 6(B) 5(C) 4(D) 3(E) 2
67
The electron configuration 1s22s22p63s23p64s23d7 represents an atom of the element
(A) Br(B) Co(C) Cd(D) Ga(E) Mg
68
The lowest principal quantum number that an electron can have is
(A) 0(B) 1(C) 2(D) 3
69
The sublevel that has only one orbital is identified by the letter
(A) s(B) p(C) d(D) f
70
The sublevel that can be occupied by a maximum of 10 electrons is identified by the letter
(A) s(B) p(C) d(D) f
71
An orbital may never be occupied by
(A) 1 electron(B) 2 electrons(C) 3 electrons(D) 0 electrons
72
A neutral species whose electron configuration is 1s22s22p63s23p64s23d104p65s24d105p6 is
(A) Highly reactive(B) A positively charged ion(C) A noble gas(D) A transition metal(E) A lanthanide element
73
In going from1s22s22p63s23p64s1 to 1s22s22p63s23p54s2 ,
an electron would
(A) Absorb energy(B) Emit energy(C) Relax to the ground state(D) Bind to another atom(E) Undergo no change in energy
74
Which of the following atoms does 1s22s22p63s23p63d2 represent?
(A) An excited state Ca atom(B) A ground state Ca atom(C) An excited state Sc atom(D) An excited state K atom(E) None of the above
75
Which electron configuration shows that of an excited atom?
(A) 1s22s22p63s1
(B) 1s22s22p63s23p63d1
(C) 1s22s22p4
(D) 1s22s22p63s23p64s2
(E) 1s22s22p63s23p3
76
Which of the following correctly represents an excited state of scandium?
(A) 1s22s22p63s23p64s23d1
(B) 1s22s32p53s23p64s23d1
(C) 1s22s22p63s23p64s13d2
(D) 1s22s22p63s23p64s23d2
(E) 1s22s22p63s23p64s03d1
77
The electron configuration for an atom of the element Tc is
(A) 1s22s22p63s23p64s23d104p55s25p6
(B) 1s22s22p63s23p64s23d104p35s24d5
(C) 1s22s22p63s23p64s23d104p3
(D) 1s22s22p63s23p63d15
(E) 1s22s22p63s23p64s23d104p65s24d5
78
IV. Periodic Table
Questions 1-3 refer to the following:(A) F(B) Li(C) Fe(D) He(E) Si
1. Shows both the properties of metals and non-metals
2. Has the greatest ionization energy3. Has the greatest electronegativity
79
Questions 1-4 refer to the following:
(A) K(B) As(C) Be(D) Se(E) Ir
1. Metalloid2. Nonmetal3. Group 1A metal4. Is an alkaline earth metal
80
Questions 1-4 refer to the following:
(A) Alkali metal(B) Alkaline earth metal(C) Transition metal(D) Halogen(E) Noble gas
1. Reacts most vigorously with water2. Is chemically inert3. Has the highest first ionization energy in its period4. Contains elements in the solid, liquid and gas
phases at STP
81
Questions 1-3 refer to the following:
(A) Ionization energy(B) Electronegativity(C) Atomic radius(D) Atomic number(E) Mass number
1. Is the measure of the pull of the nucleus of an atom on the electrons of other atoms bonded to it
2. Is the energy required to remove an electron from an atom
3. Is equal to the number of protons in an atom
82
I
K is considered to be a metal
II
When K becomes an ion its atomic radius increases
As you go from left to right across the periodic table the elements tend to become more metallic in character
As you go from left to right across the periodic table the elements tend to lose electrons
BECAUSE
BECAUSE
83
I
Elemental fluorine is more reactive than elemental neon
II
Neon has a larger atomic weight than fluorine
Isotopes of a particular element have nearly identical chemical behavior
They have identical electron configurations
BECAUSE
BECAUSE
84
I
The element with an electron configuration of [He]2s1 has a larger atomic radius than fluorine
II
The element with an electron configuration of [He]2s1 has a greater nuclear charge than fluorine
Atomic radii increase down a group
The higher the atomic number within a group, the smaller the atom
BECAUSE
BECAUSE
85
Which of the following substances are liquids at room temperature?
I. HgII. Br2
III. Si
(A) I only(B) II only(C) I and II only(D) II and III only(E) I , II, and III
86
According to placement in the periodic table, which statements regarding the first ionization energies of certain elements should be true?
I. Li has a higher value than NaII. K has a higher value than CsIII. Na has a higher value than Al
(A) I only(B) III only(C) I and II only(D) II and III only(E) I , II, and III
87
The modern periodic table is arranged based upon atomic
(A) Isotopes(B) Number(C) Density(D) Radius(E) Mass
88
Which of the following elements has the lowest electronegativity?
(A) Cesium(B) Strontium(C) Calcium(D) Barium(E) Potassium
89
Where are the highest ionization energies found in the periodic table?
(A) Upper left corner(B) Lower left corner(C) Upper right corner(D) Lower right corner(E) Middle of transition elements
90
The most active nonmetal has
(A) A high electronegativity(B) A low electronegativity(C) A medium electronegativity(D) Large atomic radii(E) A deliquescent property
91
Which of the following metals is most reactive?
(A) Na(B) Mg(C) Cu(D) Au(E) Cl
92
Which of the following is NOT true regarding nickel, Ni?
(A) It is malleable(B) It is ductile(C) It is lustrous(D) It is an insulator(E) It forms colored compounds
93
Which of the following represents an ordering of the period 4 elements by increasing atomic size?
(A) K, Kr, Ca, Br(B) K, Ca, Br, Kr(C) Kr, Br, Ca, K(D) Ca, K, Br, Kr(E) Br, Kr, Ca, K
94
An element has the following properties: shiny, brittle, poor electrical conductivity, and high melting point. This element can be best classified as a
(A) Alkali metal(B) Halogen(C) Metalloid(D) Transition metal(E) Noble gas
95
The order of the elements in the periodic table is based on
(A) The number of neutrons(B) The radius of the atom(C) The atomic number(D) The atomic weight(E) The number of oxidation states
96
The elements within each column of the periodic table
(A) Have similar valence electron configurations(B) Have similar atomic radii(C) Have the same principal quantum number(D) Will react to form stable elements(E) Have no similar chemical properties
97
Which element has the greatest electronegativity?
(A) Chlorine(B) Oxygen(C) Sulfur(D) Phosphorus(E) Fluorine
98
Which of these elements is the most electronegative?
(A) S(B) Cl(C) Na(D) Mg(E) P
99
The elements that display the greatest nonmetallic character are located toward which corner of the periodic table?
(A) Upper left(B) Dead center(C) Lower right(D) Lower left(E) Upper right
100
Which group contains elements in the solid, liquid and gas phases at 298K and 1 atm?
(A) 1(B) 2(C) 16(D) 17(E) 18
101
An element that has a high first ionization energy and is chemically inactive would most likely be
(A) A noble gas(B) A transition element(C) An alkali metal(D) A halogen(E) An alkaline earth metal
102
As the elements of period 2 are considered from left to right, there is generally a decrease in
(A) Ionization energy(B) Electronegativity(C) Metallic character(D) Nonmetallic character(E) None of the above
103
Which of the following has the greatest affinity for electrons?
(A) Na(B) Cl(C) Br(D) K(E) C
104
All members of Group 1A have similar reactivity because
(A) They have the same number of protons(B) They have the same number of electrons(C) They have similar outer-shell electron
configurations(D) They have valence electrons with the same
quantum numbers(E) They have the same number of neutrons
105
Arrange the following elements in order of decreasing nonmetallic character:
Ge,Sn,Pb,Si
(A) Pb, Sn, Ge, Si(B) Ge, Sn, Pb, Si(C) Si, Ge, Sn, Pb(D) They all have equal nonmetallic character since
they are all in the same column of the periodic table
(E) None of the above
106
Which of the following is NOT a property of Group IA elements?
(A) Low ionization energies(B) Low electronegativities(C) High melting points(D) Metallic bonding(E) Electrical conductivity
107
Which of the following elements would have the largest atomic radius?
(A) Cl(B) F(C) Li(D) Ne(E) Na
108
Which of the following elements would have the lowest first ionization energy?
(A) Fluorine(B) Oxygen(C) Nitrogen(D) Carbon(E) Boron