Download - Unit 2 Practice Questions Atomic Theory

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

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(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

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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

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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

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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

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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

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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

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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

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II. Nuclear


(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

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(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

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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

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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

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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

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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

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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

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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

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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

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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

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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

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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

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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?

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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

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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

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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

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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

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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


(A) K(B) As(C) Be(D) Se(E) Ir

1. Metalloid2. Nonmetal3. Group 1A metal4. Is an alkaline earth metal

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(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

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(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

Download - Unit 2 Practice Questions Atomic Theory

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