Deck 2: The Structure of the Atom and the Periodic Table

Question 1

What is Rutherford's important contribution to our knowledge of atomic structure?

A)Atoms contain a small,dense,positively charged nucleus,surrounded largely by empty space.
B)The atom cannot be created,divided,destroyed,or converted to any other type of atom.
C)Electrons in an atom have the magnetic property of spin.
D)Electrons are confined to certain specific regions of space outside the nucleus.
E)Electrons follow circular paths around the nucleus of an atom.

Answer 1

Atoms contain a small,dense,positively charged nucleus,surrounded largely by empty space.

Question 2

The identity of an atom is determined by which of the following?

A)the number of electrons it contains
B)its mass number
C)the number of isotopes it has
D)the number of protons it contains
E)the number of protons and neutrons it contains

Answer 2

the number of protons it contains

Question 3

Which period contains the element sodium?

A)one
B)two
C)three
D)five
E)eleven

Answer 3

three

Question 4

Which statement concerning atoms is FALSE?

A)The atomic number of an atom is the number of protons it contains.
B)The mass number of an atom is the sum of the number of protons,neutrons,and electrons it contains.
C)The nucleus of an atom contains its protons and neutrons,and is positively charged.
D)The nucleus of an atom is the heaviest part of the atom.
E)Electrons reside outside the nucleus in what is called the electron cloud.

Question 5

Who stated that the elements,when arranged according to their atomic masses,showed a distinct periodicity of their properties?

A)Dmitri Mendeleev
B)Niels Bohr
C)J.J Thomson
D)Ernest Rutherford
E)John Dalton

Question 6

When is an atom in its ground state?

A)when the electrons of the atom are in the lowest possible energy levels
B)when an atom loses all of its electrons to form a noble gas
C)when the electrons of the atom are in the highest possible energy levels
D)when an electron is promoted to a higher energy level,farther from the nucleus
E)when the electrons of an atom spontaneously emit energy in the form of a photon

Question 7

What are the three primary particles found in an atom?

A)neutron,positron,and electron
B)electron,neutron,and proton
C)electron,proton,and nucleon
D)positron,electron,and nucleon
E)proton,electron,and neutrino

Question 8

Which statement about the modern periodic table is FALSE?

A)Elements are arranged in order of increasing atomic number.
B)A period is a horizontal row of elements.
C)A group is a vertical column of elements.
D)A stepwise line separates the metals from the nonmetals; metals are to the left of the line,nonmetals are to the right of the line.
E)Elements in the same period share similar chemical and physical properties.

Question 9

In modern atomic theory,Bohr's orbits are replaced by atomic orbitals.What is an atomic orbital?

A)a circular path around the nucleus travelled by an electron
B)a dense,positively charged region of space at the center of an atom
C)a region of space within an atom where there is a high probability of finding an electron
D)the outermost principle energy level in an atom
E)the lowest energy arrangement of electrons in an atom

Question 10

The ion K⁺ is formed by which process?

A)loss of an electron by K
B)gain of a proton by K
C)loss of a proton by K
D)gain of an electron by K
E)None of these are correct.

Question 11

What was J.J.Thomson's important discovery about cathode rays in 1897?

A)Cathode rays were indestructible.
B)Cathode rays were heavier than anode rays.
C)Cathode rays consisted of a stream of electrons.
D)Cathode rays were produced by all radioactive atoms.
E)Cathode rays were able to initiate radioactive decay of an atom.

Question 12

When a neutral atom gains one or more electrons,what type of particle is formed?

A)an anion
B)an isotope
C)a proton
D)a positron
E)a cation

Question 13

What is the value of the mass number in the isotope 131
53 I?

A)53
B)78
C)126.9
D)131
E)184

Question 14

Which describes the basic concept of Bohr's theory of the atom?

A)Atoms contain a small,dense positively charged region called the nucleus.
B)The energy of an electron in an atom is quantized; it has only certain allowable values.
C)Light is made up of particles called photons.
D)Electrons have the magnetic property of spin.
E)Radioactive atoms spontaneously decay and release large amounts of energy from the nucleus.

Question 15

Which statement explains why isotopes have different mass numbers?

A)Isotopes differ in the number of protons each contains.
B)Isotopes differ in the number of electrons each contains.
C)Isotopes differ in the number of neutrons each contains.
D)Isotopes differ in the number of protons and neutrons each contains.
E)Isotopes differ in the number of protons and electrons each contains.

Question 16

Tungsten is a metal containing 74 protons,and is used widely in the electronics industry.What is the chemical symbol for tungsten?

A)T
B)Tg
C)Tn
D)W
E)As

Question 17

The modern periodic law states that the physical and chemical properties of the elements are periodic functions of what property?

A)electrons
B)atomic weight
C)neutrons
D)atomic number
E)mass number

Question 18

What term is used to describe atoms of the same element that have different masses?

A)radioactive
B)constituents
C)isotopes
D)telomers
E)isomers

Question 19

Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements?

A)Bohr and Rutherford
B)Plank and Rutherford
C)Maxwell and Dalton
D)Thomson and Crookes
E)Mendeleev and Meyer

Question 20

What is always true for a neutral atom?

A)There is an equal number of protons and neutrons.
B)There is an equal number of protons and electrons.
C)There is an equal number of protons,neutrons,and electrons.
D)The number of protons and neutrons is an even number.
E)The number of protons,neutrons,and electrons is an even number.

Question 21

What are the columns of elements on the periodic table called?

A)groups
B)shells
C)periods
D)metals
E)rows

Question 22

In nature,the element neon exists as three different isotopes: Ne-20,Ne-21,and Ne-22.Which isotope would be the most abundant in a sample of neon?

A)Ne-20
B)Ne-21
C)Ne-22
D)All isotopes would be equally abundant.
E)It is impossible to determine.

Question 23

Atoms with the biggest radii occur in the ________ region of the periodic table.

A)bottom left
B)top right
C)bottom right
D)top left
E)middle

Question 24

Hydrogen can form two different ions: a hydrogen ion (H⁺),and a hydride ion (H⁻).Which statement concerning these ions is FALSE?

A)The H⁺ ion is a cation formed by the loss of one electron; this ion has no valence electrons.
B)The H⁻ ion is an anion formed by the gain of one electron; this ion has a full n=1 energy level.
C)The hydrogen ion and the hydride ion are isotopes.
D)The hydrogen ion and the hydride ion have the same number of protons.
E)The hydrogen ion and the hydride ion have different sizes.

Question 25

What is FALSE about the three orbitals in the 2p sublevel?

A)The orbitals have the same dumbbell-like shape.
B)The orbitals have similar,but different energies.
C)The orbitals are the same distance away from the nucleus.
D)The orbitals are each oriented in a different direction.
E)Each orbital can hold two electrons with opposite spins.

Question 26

Which best explains why an Al³⁺ ion is smaller than an Al atom?

A)In forming the Al³⁺ ion,the Al atom loses the electrons in its outermost energy level,causing a decrease in the atomic radius.
B)In forming the Al³⁺ ion,the Al atom gains three protons and the resulting net positive charge keeps the electrons more strongly attracted to the nucleus,reducing the radius.
C)The Al³⁺ ion contains more electrons than the Al atom,which results in a greater attraction for the nucleus and a smaller atomic radius.
D)In forming the Al³⁺ ion,the Al atom adds electrons into a higher energy level,causing a decrease in the atomic radius.
E)There are more protons in an Al³⁺ ion than there are in an Al atom.

Question 27

The element carbon forms the basis of study in Organic Chemistry.Which statement about the element carbon is FALSE?

A)Carbon is a period 2 element.
B)Carbon is a group 4 element.
C)Carbon is a nonmetal.
D)Carbon atoms have six valence electrons.
E)Carbon atoms have six protons.

Question 28

The ground state electron configuration of a sulfur atom is shown below.What is the ground state electron configuration of the ion S²⁻?

A)1s²2s²2p⁶3s⁰3p⁴
B)1s²2s²2p⁶3s²3p⁶
C)1s²2s²2p⁶3s²3p²
D)1s²2s²2p⁶
E)1s²2s²2p⁶3s³3p⁵

Question 29

Which element is a halogen in period 4?

A)bromine
B)silicon
C)iodine
D)krypton
E)potassium

Question 30

What is the general name given to the elements of Group IA (1)?

A)halogens
B)alkali metals
C)alkaline earth metals
D)noble gases
E)metalloids

Question 31

The Aufbau Principle specifies which of the following?

A)Each atomic orbital has a maximum capacity of two electrons.
B)Two electrons in the same orbital must have opposite spins.
C)Two electrons in the same orbital must be spin paired.
D)Electrons will occupy the lowest energy orbitals that are available.
E)Electrons will half-fill orbitals of equal energy,before any become completely filled.

Question 32

Which statement concerning the elements fluorine,chlorine,bromine,and iodine is FALSE?

A)They are all halogens.
B)They all have the same electron configuration.
C)They are all nonmetals.
D)They are all representative elements.
E)They all have the same number of valence electrons.

Question 33

Which ion is NOT isoelectronic (i.e.has the same electron configuration)with Ar? The electron configuration of Ar is shown. $\begin{array} { |l | l| } \hline \mathrm { S } & 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 4 }\\\hline \end{array}$

A)Cl^?
B)K⁺
C)Br^?
D)Ca²⁺
E)S^2?

Question 34

Which statement correctly describes the basis for the octet rule? $\begin{array} { | l | l | } \hline \text { Ar } & 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } \\\hline\end{array}$

A)Atoms strive to attain eight protons in their nucleus to attain the stability of the nearest noble gas.
B)Atoms have a tendency to form eight bonds with other atoms to attain the stability of a noble gas.
C)Atoms will lose,gain,or share eight electrons to become a noble gas.
D)Atoms are most stable with eight electrons in their outermost shell and the electron configuration of a noble gas.
E)Atoms are most stable when the number of protons they contain is identical to the noble gas closest to them in the periodic table.

Question 35

What term is used for the elements straddling the "staircase" boundary between the metals and nonmetals?

A)transition elements
B)metalloids
C)cations
D)lanthanides
E)noble gases

Question 36

How many valence electrons are present in a chloride ion,Cl^??

A)5
B)7
C)8
D)17
E)18

Question 37

What does the mass number minus the atomic number represent?

A)number of protons
B)number of electrons
C)number of neutrons
D)number of protons - number of neutrons
E)number of neutrons - number of protons

Question 38

What requirement must be met in order for two electrons to coexist in the same orbital?

A)The electrons must have different energies.
B)The electrons must have the same spin.
C)The electrons must have opposite charges.
D)The electrons must be in different principle energy levels.
E)The electrons must have opposite spins.

Question 39

What are valence electrons?

A)the electrons located in the nucleus of an atom
B)the interior electrons,located closest to the nucleus
C)the outermost electrons in an atom
D)the electrons with the lowest energy in an atom
E)the total number of electrons in an atom

Question 40

The ground state electron configuration of chlorine is shown.Which statement concerning an atom of chlorine is FALSE? $\begin{array} { | l | l | } \hline \mathrm { Cl } & 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 5 } \\\hline\end{array}$

A)A chlorine atom has 17 total electrons.
B)The outermost energy level in a chlorine atom is n=3.
C)A chlorine atom has 5 valence electrons.
D)A chlorine atom needs one electron to obtain an octet in its outermost energy level.
E)A chlorine atom has 17 protons.

Question 41

What ion carries two negative charges and is isoelectronic with K⁺?

A)O^2-
B)S^2-
C)F^2-
D)Cl^2-
E)Ar^2-

Question 42

In Mendeleev's table of the elements,the elements were arranged according to

A)atomic number.
B)mass number.
C)atomic mass.
D)neutron number.
E)density.

Question 43

What is a horizontal row of elements on the periodic table called?

A)group
B)period
C)family
D)representative elements
E)transition elements

Question 44

Americium-241 is an isotope used in smoke detectors.What is the composition of a neutral atom of Americium-241?

A)241 protons,95 neutrons,241 electrons
B)241 protons,95 neutrons,146 electrons
C)95 protons,146 neutrons,95 electrons
D)95 protons,146 neutrons,51 electrons
E)95 protons,241 neutrons,95 electrons

Question 45

What Group IA (1)ion has the electronic arrangement shown 1s²2s²2p⁶

A)lithium ion
B)sodium ion
C)potassium ion
D)magnesium ion
E)calcium ion

Question 46

How many neutrons are present in an atom of the isotope 7
3 Li?

A)3
B)4
C)7
D)10
E)None of the choices are correct.

Question 47

In a neutral atom,what number equals the number of electrons?

A)atomic number
B)mass number
C)mass number minus the atomic number
D)atomic number and mass number minus the atomic number are correct.
E)None of the choices are correct.

Question 48

The modern periodic table is arranged according to what property?

A)atomic number
B)mass number
C)atomic mass
D)neutron number
E)density

Question 49

How many orbitals are in an s sublevel? How many in a p sublevel?

A)s: 1,p: 2
B)s: 2,p: 3
C)s: 1,p: 3
D)s: 2,p: 6
E)s: 3,p: 3

Question 50

In Rutherford's experiment,which led to the discovery of the atomic nucleus,what type of particle or ray was fired at the gold foil target?

A)alpha
B)beta
C)gamma
D)neutrons
E)cathode rays

Question 51

Which of the following accounts for the fact that chlorine has an atomic mass of 35.45 amu rather than a whole number?

A)isotopes
B)electrons
C)protons
D)radioactivity
E)isomers

Question 52

Where are the alkaline earth metals located on the periodic table?

A)IA (1)
B)IIA (2)
C)IIIA (3)
D)VIIA (17)
E)VIIIA (18)

Question 53

Which isotope of hydrogen has two neutrons?

A)hydrogen-1
B)hydrogen-2
C)hydrogen-3
D)deuterium
E)H-₂

Question 54

How many electrons are present in an atom of silicon?

A)14
B)16
C)18
D)24
E)26

Question 55

Microwaves,light,and X-rays are all forms of

A)electricity.
B)high energy electrons.
C)electron repulsion.
D)electromagnetic radiation.
E)radioactivity.

Question 56

The total mass of the protons in any neutral atom is about ________ times the total mass of electrons in the atom.

A)0.0005
B)0.3
C)1
D)2
E)2000

Question 57

Who discovered the existence of the atomic nucleus?

A)Crookes
B)Thomson
C)Geiger
D)Rutherford
E)Bohr

Question 58

Who discovered that cathode rays consist of a stream of negative particles,electrons?

A)Crookes
B)Thomson
C)Geiger
D)Rutherford
E)Bohr

Question 59

What kind(s)of particles can be found outside the nucleus of an atom?

A)protons
B)neutrons
C)electrons
D)protons and electrons
E)protons and neutrons

Question 60

Given that helium has an isotope 4
2 He,how many electrons does an atom of this helium isotope contain?

A)1
B)2
C)4
D)6
E)0

Question 61

Which of the following elements is a metalloid?

A)C
B)Ge
C)Pb
D)N
E)P

Question 62

Electron affinity is

A)the energy required to remove an electron from an isolated atom.
B)the force between two electrons in the same orbital.
C)the force between two ions of opposite charge.
D)the energy released when an isolated atom gains an electron.
E)the attraction of an atom for an electron in a chemical bond.

Question 63

What can be said about the possibility of the existence of the hydrogen isotope represented by the symbol shown below? $\begin{array} { l } 2 \\2\end{array}$ H

A)This isotope of hydrogen is not possible because it has no electrons.
B)This isotope of hydrogen is not possible because atoms of hydrogen have one proton.
C)This isotope of hydrogen is possible; it simply contains no protons and is an ion.
D)This isotope of hydrogen is possible; it simply contains no neutrons.
E)This isotope of hydrogen is possible; it simply has two neutrons.

Question 64

Which of the following elements is most likely to form a 2+ ion?

A)Li
B)K
C)Al
D)N
E)Ca

Question 65

Where are the halogens located on the periodic table?

A)representative elements
B)transition metals
C)Group VIIA (17)
D)Group IIA (2)
E)Group IIIA (3)

Question 66

Which one of the following elements has the highest electron affinity?

A)Li
B)K
C)Kr
D)O
E)Cl

Question 67

What is the ground state electronic configuration of the sodium ion,Na⁺?

A)1s²2s²2p⁵
B)1s²2s²2p⁶
C)1s²2s²2p⁶3s¹
D)1s²2s²2p⁶3s²
E)1s²2s²2p⁶3s²3p⁶4s¹

Question 68

How many valence electrons are in an atom of carbon?

A)8
B)6
C)4
D)1
E)0

Question 69

Which of the following ions does not follow the octet rule?

A)Na⁺
B)Ca²⁺
C)(Al³⁺)
D)(_N3-)
E)(_Cl2-)

Question 70

Which of the following statements relating to Bohr's model of the hydrogen atom is FALSE?

A)The lowest energy orbit has quantum number n = 1.
B)The highest energy orbits are farthest from the nucleus.
C)In a transition from the n = 3 to the n = 1 level,light is emitted.
D)Energy differences between energy levels can be calculated from the wavelengths of the light absorbed or emitted.
E)The Bohr model consists of energy levels that are evenly spaced,like the rungs of a ladder.

Question 71

What is the ground state electron configuration of sulfur,whose atomic number is 16?

A)1s²1p⁶2s²2p⁶
B)1s²2s²2p⁶2d⁶
C)1s²2s²2p⁶3s²3p⁴
D)1s²2s²2p⁶3s²3d⁴
E)1s²2s²2p⁶3s²2d⁴

Question 72

What is the lowest energy sublevel of a principal level?

A)d
B)e
C)f
D)s
E)p

Question 73

Which of the following elements has the lowest ionization energy?

A)Li
B)B
C)O
D)F
E)Ne

Question 74

Which of the following correctly gives the electron capacity of a principal energy level in terms of the number n?

A)n
B)2n
C)2n + 2
D)n²
E)2n²

Question 75

How many orbitals are there in the second principal energy level?

A)2
B)3
C)1
D)0
E)4

Question 76

How many sublevels are there in the third principal energy level?

A)3
B)2
C)1
D)0
E)4

Question 77

Which one of the following electron configurations is appropriate for a ground state atom?

A)1s¹2s¹
B)1s²2s¹
C)1s²2s²2p⁸
D)1s²2s²2p⁴3s¹
E)1s²2s²2p⁶3d¹

Question 78

Which of the following atoms has the biggest size (radius)?

A)Na
B)Al
C)Cl
D)Rb
E)I

Question 79

Which of the following elements has the highest ionization energy?

A)Li
B)B
C)O
D)F
E)He

Question 80

What are the elements in the A-groups often called?

A)transition elements
B)lanthanides
C)metals
D)non-metals
E)representative elements