Deck 11: Atomic Theory: The Quantum Model of the Atom

Question 1

Which of the following is/are the major flaw(s)of the Bohr model of the hydrogen atom?
i.Hydrogen is the only atom that fits the model
ii.Circular orbits violate the Law of Conservation of Energy
iii.It explains atomic line spectra in terms of electron energies
iv.It introduced the idea of quantized electron energy levels in an atom

A)ii only
B)i and ii
C)i and iii
D)iii and iv
E)i, ii, and iii

Answer 1

i and ii

Question 2

Which of the following statements is/are incorrect?
i.The Bohr model successfully predicts energies in the ultraviolet portion of the hydrogen spectrum
ii.The Bohr model successfully predicts energies in the infrared portions of the sodium spectrum
iii.The Bohr model associates electron energy with the radius at which an electron orbits the nucleus
iv.The Bohr model does not explain the failure of an electron to lose energy as it travels a circular path around a nucleus

A)i only
B)ii only
C)iii only
D)iv only
E)iii and iv

Answer 2

ii only

Question 3

The Bohr model of the atom assumes that which of the following quantities for the electron in a hydrogen atom is/are quantized?
i.Speed
ii.Direction of spin axis
iii.Energy
iv.Radius of its orbit

A)iii only
B)i and iii
C)iii and iv
D)i, iii, and iv
E)i, ii, and iii

Answer 3

iii and iv

Question 4

Which of the following statements is/are incorrect?
i.For each value of n the number of sublevels is also n
ii.There is an s sublevel for every value of n
iii.Some principal energy levels have no f sublevels
iv.There is no d sublevel when n = 3

A)i only
B)ii only
C)iii only
D)iv only
E)ii and iv

Question 5

The order of increasing principal energy levels in an atom is related to which of the following sequences?

A)1-2-3-4
B)1-3-5-7
C)4-3-2-1
D)s-p-d-f
E)f-d-p-s

Question 6

Complete the statement with the best choice: In hydrogen,the ground state:

A)has the lowest energy
B)has the most energy
C)is known as the first excited state
D)is the only energy level that is not quantized
E)is one of the energy levels that is not quantized

Question 7

Which of the following statements is true?

A)The dark bands in a rainbow are examples of line spectra
B)The light from neon signs is used as a source for producing continuous spectra
C)The light from standard light bulbs is used as a source for producing line spectra
D)A continuous spectrum consists of an uninterrupted distribution of colored light
E)A continuous spectrum results when light from a heated elemental substance passes through a prism

Question 8

Complete the statement with the best choice: Excited states for the hydrogen atom are states in which:

A)electrons are found after they have released energy
B)electrons are more stable than in the ground state
C)the electron has more energy than in the ground state
D)electrons orbit in opposite directions as in the ground state
E)electrons orbit closer to the nucleus than in the ground state

Question 9

Which of the following statements is/are correct?
i.Wavelength is the distance between identical parts of a wave
ii.Frequency is the number of complete waves passing a point in a given period of time
iii.The speed of light is equal to the product of the wavelength and frequency of an electromagnetic wave

A)i only
B)iii only
C)i and ii
D)ii and iii
E)i, ii, and iii

Question 10

Which of the following statements about atomic spectra is/are correct?
i.The discrete line spectrum of elements is evidence that electron energies are quantized
ii.Lines in the spectrum are discrete because electron energies are restricted to certain values
iii.Energy is emitted from atoms as electrons move from higher energy levels to lower energy levels
iv.Electron transitions of differing energies produce different wavelengths of light.

A)i and ii
B)i and iii
C)ii and iv
D)i, iii, and iv
E)All are correct statements.

Question 11

In the third principal energy level,what is the order of energies of the sublevels,from lowest to highest?

A)1s < 2s < 3s
B)3d < 3p < 3s
C)3p < 3s < 3d
D)3p < 3d < 3s
E)3s < 3p < 3d

Question 12

Which of the following statements about atomic spectra is incorrect?

A)An atom must absorb energy before it can emit a spectral line
B)Only atoms in the ground state can radiate energy
C)An electron dropping between two specific energy levels always emits the identical spectral line
D)No two elements have identical atomic spectra
E)All of the statements above are correct (choosing this statement indicates that it is correct)

Question 13

Which of the following statements correctly describes the relationship between principal energy levels of an electron and the principal quantum number?

A)Energy levels have no relationship to principal quantum number
B)In general, energy levels increase in the principal quantum number order s < p < d < f
C)In general, energy levels decrease as principal quantum number orbital occupancy increases
D)In general, energies decrease as the principal quantum number increases
E)In general, energies increase as the principal quantum number increases

Question 14

Which of the following is the letter representation of the electron orbital below?

A)s
B)p_z
C)p_x
D)d_xz
E)d_z2

Question 15

Identify the best description of an s orbital:

A)Spherical
B)Two pair of lobes
C)One pair of lobes and a collar
D)One pair of lobes oriented on the x-axis
E)Three pair of lobes oriented on the x-, y-, and z-axes

Question 16

Which of the following defines a correct relationship for electromagnetic radiation?

A)
B)
C)
D)
E)

Question 17

Which of the following statements is false?

A)Line spectra can be produced by holding a glass prism next to an incandescent light bulb.
B)Each element has a unique line spectrum.
C)The separate lines of color in a line spectrum are known as discrete lines.
D)The light emitted from a heated element forms a line spectrum when passed through a prism.
E)Line spectra can be produced by holding a glass prism next to a gas discharge tube.

Question 18

The Bohr model of the hydrogen atom gives specific information about all of the following except i.Electron paths
ii.Orbital shapes
iii.Atomic radius
iv.Electron energies
v.Restrictions on the electron population of an orbital

A)i only
B)ii only
C)iii only
D)iv only
E)ii and v

Question 19

Which of the following statements is/are correct?
i.Principal energy levels are identified by the letters s,p,d,and f
ii.Principal energy levels appear in both the quantum mechanical model of the atom and the Bohr model of the atom
iii.In general,n = 1 is at lower energy than n = 2,and n = 2 is lower than n = 3,and so on
iv.The principal energy level is related to electron spin

A)i only
B)iv only
C)i and ii
D)ii and iii
E)iii and iv

Question 20

Which of the following statements is/are correct?
i.Visible light is a very small part of the entire electromagnetic spectrum.
ii.Low frequency electromagnetic radiation has a short wavelength
iii.Electromagnetic radiation travels at a finite speed

A)i only
B)ii only
C)iii only
D)i and ii
E)i and iii

Question 21

Which of the following pairs of atomic numbers belong to elements whose atoms have the highest occupied energy level electron configuration of the form ns²np²?

A)23 and 26
B)4 and 20
C)30 and 80
D)6 and 82
E)22 and 72

Question 22

The maximum number of electrons that can be held in the 5p sublevel is:

A)2
B)3
C)4
D)5
E)6

Question 23

Which of the following elements has the Lewis symbol below,where Sy represents the elemental symbol?

A)Na
B)Mg
C)Al
D)Si
E)P

Question 24

Which of the following lists electron sublevels in order of increasing energy?

A)4p < 4d < 5s < 5p < 6s
B)4p < 5s < 4d < 5p < 6s
C)6s < 5p < 5s < 4d < 4p
D)6s < 5p < 4d < 5s < 4p
E)4p = 4d < 5s = 5p < 6s

Question 25

Consider the following periodic table. Which section represents elements whose electron configuration for the highest occupied energy level is ns²np⁵?

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

Question 26

List the atomic numbers of all atoms that are smaller than atoms of fluorine.

A)10 and greater
B)8 and less
C)1, 2, 10
D)1, 2
E)None is smaller than fluorine.

Question 27

Which of the following lists electron sublevels in order of increasing energy?

A)4p < 3d < 4s < 3p < 3s
B)4p < 4s < 3d < 3p < 3s
C)3s < 3p < 4s < 3d < 4p
D)3s < 3p < 3d < 4s < 4p
E)3s < 4s < 3p < 4p < 3d

Question 28

What is the ground state electron configuration of iron?

A)[Ar] 3d⁸
B)[Ar] 4s²3d⁶
C)[Ne] 3d¹⁰4s²
D)[Ar] 4s¹3d⁸
E)none of the above is correct

Question 29

In a given energy level,which of the following types of orbitals will have the lowest energy?

A)
B)
C)
D)

Question 30

Which of the following pairs of atomic numbers belong to elements whose atoms have the highest occupied energy level electron configuration of the form ns²np⁴?

A)16 and 52
B)40 and 72
C)24 and 42
D)9 and 17
E)14 and 32

Question 31

How many orbitals are in the 5d sublevel?

A)1
B)3
C)5
D)7
E)9

Question 32

Which of the following elements has the Lewis symbol below,where Sy represents the elemental symbol?

A)Li
B)Mg
C)Ga
D)Sn
E)Bi

Question 33

Identify the statement among the following that combines a correct cause with a correct effect of that cause.

A)Sulfur atoms are smaller than phosphorus atoms because sulfur has a smaller atomic number
B)The radius of calcium atoms is greater than the radius of magnesium atoms because ground state electrons occupy a higher energy level in calcium than in magnesium
C)Atomic size increases from left to right in a row of the periodic table because density increases in the same direction
D)The relative sizes of silicon atoms and aluminum atoms are not predictable on the basis of nuclear charge and highest occupied energy level because one factor predicts silicon atoms to be larger, and the other factor predicts aluminum atoms to be larger
E)More than one of the above statements combines a correct cause with a correct effect of that cause

Question 34

What is the ground state electron configuration of potassium?

A)[Ar] 3d¹
B)1s²2s²2p⁶3s²3p⁶3d¹
C)[Ar] 4s¹
D)1s²2s²2p⁶2d¹⁰3s¹
E)None of the above is correct

Question 35

Atomic size varies with position in the periodic table primarily because of what influence(s)?
i.Highest occupied principal energy level
ii.Increasing number of electrons with increasing atomic number
iii.Nuclear charge

A)i only
B)ii only
C)iii only
D)i and iii
E)i, ii, and iii

Question 36

Which of the following is the correct Lewis symbol for the given element?

A)K :
B)Kr :
C)B :
D)Be :
E)O :

Question 37

How many orbitals are in the 3p sublevel?

A)1
B)3
C)5
D)7
E)9

Question 38

The maximum number of electrons that can be held in the 4f sublevel is:

A)2
B)6
C)7
D)10
E)14

Question 39

What is the ground state electron configuration of carbon?

A)2s²2p⁴
B)1s²2s²2p⁶3s²
C)1s²1p²2s²
D)1s²2s²2p²
E)none of the above are correct

Question 40

At any instant an electron orbital may be in which occupancy state?
i.Unoccupied
ii.Occupied by one electron
iii.Occupied by two electrons
iv.Occupied by 2,6,10,or 14 electrons

A)iv only
B)i or iv
C)ii or iv
D)i, ii, or iii
E)i, ii, or iv

Question 41

Which general electron configuration is responsible for the family properties of noble gases?

A)ns¹
B)ns²
C)ns²np⁴
D)ns²np⁵
E)ns²np⁶

Question 42

Consider the following periodic table. Which numbered section represents the most metallic elements?

A)1
B)2
C)3
D)4
E)5

Question 43

How many of the following elements belong to the chemical family known as the alkaline earths? sodium,magnesium,chlorine,neon,calcium,bromine,argon,fluorine,helium,hydrogen

A)1
B)2
C)3
D)4
E)5

Question 44

Which of the following is not a property of metals?

A)Tend to gain electrons to form anions
B)1, 2, or 3 valence electrons
C)Low ionization energies
D)High electrical conductivity
E)Malleable and ductile

Question 45

Which of the following provides the best explanation for the many chemical similarities between sodium and potassium?

A)Both have atomic masses between 20 and 40 u
B)Both have an ns¹ electron configuration for their highest occupied energy level
C)Both are main group elements
D)Both are solids at room temperature and pressure
E)The atomic numbers of the two elements differ by less than ten

Question 46

What do elements in a family or group of main-group elements have in common?

A)All have the same number of valence electrons
B)All are in the same period
C)All have eight valence electrons
D)All have the same atomic number
E)All are gases

Question 47

Which of the following is the best definition of first ionization energy?

A)The energy required to remove one electron from a neutral gaseous atom of an element
B)The energy barrier that must be overcome to start a chemical reaction
C)The energy required to raise an electron in the ground state into the first excited state
D)The energy defined by mv²
E)The energy needed to reduce a species in the aqueous phase to its minimum (first) reduction potential

Question 48

Consider the following periodic table. In what numbered section would the elements used in semiconductors be found?

A)1
B)2
C)3
D)4
E)5

Question 49

Which of the following correctly lists the elements sodium,silicon,and chlorine in order of decreasing first ionization energy?

A)Cl > Si > Na
B)Na > Cl > Si
C)Na > Si > Cl
D)Cl > Na > Si
E)Si > Na > Cl

Question 50

Which of the following correctly lists the elements helium,neon,and argon in order of increasing first ionization energy?

A)He < Ne < Ar
B)He < Ar < Ne
C)Ar < Ne < He
D)Ar < He < Ne
E)Ne < Ar < He