Deck 29: Nuclear Physics: Part A

Question 1

In an analysis relating Bohr's theory to the de Broglie wavelength of electrons,when an electron moves from the n = 1 level to the n = 3 level,the circumference for its orbit becomes 9 times greater.This occurs because:

A) the wavelength of the electron becomes nine times as long.
B) there are triple as many wavelengths,and each wavelength is triple in length.
C) there are nine times as many wavelengths in the new orbit.
D) the electron is moving nine times as fast.

Answer 1

there are triple as many wavelengths,and each wavelength is triple in length.

Question 2

Characteristic K x-rays are the result of:

A) inner electron transitions.
B) outer electron transitions.
C) nuclear electron states.
D) buckytubes.

Answer 2

inner electron transitions.

Question 3

In the n = 5 shell,how many distinct values of
Are possible?

A) 5
B) 15
C) 10
D) The correct value is not given.

Answer 3

The correct value is not given.

Question 4

In the Bohr model of the atom,the orbits where electrons move slowest:

A) have the least radius.
B) have the highest energy.
C) have the least angular momentum.
D) have the lowest energy.

Question 5

Which of the following transitions in hydrogen from an initial state (n_i)to a final state (n_f)results in the least energy emitted?

A) n_i = 3,n_f = 95
B) n_i = 80,n_f = 2
C) n_i = 2,n_f = 1
D) n_i = 1,n_f = 3

Question 6

The ionization energy of the hydrogen atom is 13.6 eV.What is the energy of the n = 5 state?

A) -0.544 eV
B) 0.378 eV
C) 0.544 eV
D) -0.378 eV

Question 7

The four visible colors emitted by hydrogen atoms are produced by electrons:

A) that start in the ground state.
B) that end up in the ground state.
C) that end up in the level with n = 2.
D) that start in the level with n = 2.

Question 8

Of the various wavelengths emitted from a hydrogen gas discharge tube,those associated with transitions from higher levels down to the n = 2 level produce which of the following?

A) visible
B) infrared
C) ultraviolet
D) a mixture of visible and ultraviolet

Question 9

The ionization energy of the hydrogen atom is 13.6 eV.What is the wavelength of a photon having this much energy? (h = 6.63 × 10−³⁴ J⋅s,c = 3.00 × 10⁸ m/s,1 eV = 1.6 × 10−¹⁹ J,and 1 nm = 10−⁹ m)

A) 91.4 nm
B) 360 nm
C) 136 nm
D) 273 nm

Question 10

The ionization energy of the hydrogen atom is 13.6 eV.What is the energy of a photon emitted corresponding to a transition from the n = 6 to n = 2 state?

A) 7.9 eV
B) 2.9 eV
C) 3.0 eV
D) 4.0 eV

Question 11

When an electron moves from the n = 1 to the n = 3 orbit:

A) the radius doubles and the angular momentum increases by a factor of 9.
B) the radius increases by a factor of 9,and the angular momentum triples.
C) both the radius and the angular momentum increase by a factor of 9.
D) both the radius and the angular momentum triple.

Question 12

In the hydrogen atom the potential energy is negative,but the absolute value of the potential energy:

A) is half the kinetic energy of the electron.
B) is equal to n² times the kinetic energy of the electron.
C) is equal to the kinetic energy of the electron.
D) is twice the kinetic energy of the electron.

Question 13

What is the wavelength of the line in the hydrogen spectrum that is comprised of transitions from the n = 5 to the n = 3 levels?

A) 1880 nm
B) 1290 nm
C) 2250 nm
D) 1920 nm

Question 14

When a hydrogen atom absorbs a photon that raises it to the n = 4 state,what is the least number of photons that can be emitted by that atom as it returns to the ground state?

A) 4
B) 3
C) 5
D) The correct value is not given.

Question 15

The ionization energy for the hydrogen atom is 13.6 eV.What is the energy of a photon that is emitted as a hydrogen atom makes a transition between the n = 4 and n = 3 states?

A) 3.40 eV
B) 0.66 eV
C) 6.80 eV
D) 2.55 eV

Question 16

When a hydrogen atom absorbs a photon that raises it to the n = 5 state,how many different energies are possible for the photon(s)that may be emitted as the atom eventually returns to the ground state?

A) 5
B) 3
C) 4
D) The correct value is not given.

Question 17

If the radius of the electron orbit in the n = 1 level of the hydrogen atoms is 0.0529 nm,what is its radius for the n = 4 level? (Assume the Bohr model is valid).

A) 1.32 nm
B) 0.265 nm
C) 0.106 nm
D) 0.846 nm

Question 18

If a hydrogen atom,originally in its ground state of energy -13.6 eV,absorbs a photon of energy 22.0 eV,what is the resulting kinetic energy of the electron if the proton has negligible kinetic energy?

A) Such a photon cannot be absorbed in this case.
B) 8.4 eV
C) 2.4 eV
D) 16.0 eV

Question 19

The Paschen series of hydrogen corresponds to electron transitions from higher levels to n = 3.What is the longest wavelength in that series? (h = 6.63 × 10−³⁴ J⋅s.The ground state of hydrogen is at -13.6 eV. )

A) 822 nm
B) 365 nm
C) 1880 nm
D) 1094 nm

Question 20

The Lyman series of hydrogen corresponds to electron transitions from higher levels to n = 1.What is the longest wavelength in that series? (h = 6.63 × 10−³⁴ J⋅s.The ground state of hydrogen is at -13.6 eV. )

A) 91.4 nm
B) 273 nm
C) 456 nm
D) 122 nm

Question 21

The quantum mechanical model of the hydrogen atom requires that if the principal quantum number = 3,there will be permitted how many orbital magnetic quantum numbers?

A) 5
B) 8
C) 4
D) 7

Question 22

How many possible substates are available in a hydrogen atom where the principal quantum number is 2?

A) 18
B) 8
C) 36
D) 9

Question 23

The quantum mechanical model of the hydrogen atom requires that if the principal quantum number is 5,there will be how many different permitted orbital quantum number(s)?

A) two
B) five
C) one
D) four

Question 24

What is the next energy level that fills after the 4d energy level is full?

A) 5p
B) 4s
C) 6s
D) 4f

Question 25

The ground state electronic configuration for magnesium is 1s²2s²2p⁶3s².Which of the following would most likely result in an element being chemically similar to magnesium?

A) the valence subshell having 2 electrons
B) the valence electron being an s² electron
C) the valence electron being a p² electron
D) the valence electron having principal quantum number 3

Question 26

If the principal quantum number for hydrogen is 4,which one of the following is not a permitted orbital magnetic quantum number for that atom?

A) −2
B) 0
C) 3
D) 5

Question 27

For the n = 5 shell,what are the lowest values possible for
And
Respectively?

A) -5,-5
B) −4,-4
C) 0,-4
D) 0,0

Question 28

The ground state configuration for an element is 1s²2s²2p⁶3s²3p¹.What is the atomic number of the element?

A) 11
B) 9
C) 24
D) 13

Question 29

For n = 6,what are the maximum orbital quantum number and the maximum orbital magnetic quantum number?

A) 7,6
B) 5,4
C) 6,5
D) 5,5

Question 30

The quantum mechanical model of the hydrogen atom requires that if the principal quantum number = 6,there will be how many permitted orbital quantum numbers?

A) 3
B) 16
C) 6
D) 5

Question 31

The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number of the hydrogen atom is 3,there will be how many permitted orbital magnetic quantum numbers?

A) three
B) nine
C) four
D) seven

Question 32

How many electrons are in chlorine's (atomic number 17)next to outer shell (n = 2)?

A) 18
B) 4
C) 2
D) 8

Question 33

Magnesium has atomic number 12.In its ground state,how many electrons are in its n = 3 shell?

A) 2
B) 8
C) 16
D) 10

Question 34

The quantum mechanical model of the hydrogen atom requires that if the orbital magnetic quantum number is 4,there will be how many permitted spin magnetic quantum numbers?

A) four
B) seven
C) three
D) two

Question 35

The ground state electronic configuration for silicon is 1s²2s²2p⁶3s²3p².Which of the following elements would be expected to be chemically similar to silicon?

A) boron with configuration 1s²2s²2p¹
B) lithium with configuration 1s²2s¹
C) carbon with configuration 1s²2s²2p²
D) sodium with configuration 1s²2s²2p⁶3s¹

Question 36

What is the maximum number of electrons that can occupy a 3d subshell?

A) 5
B) 14
C) 10
D) 18

Question 37

The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number = 5,there will be how many permitted orbital magnetic quantum numbers allowed?

A) 7
B) 15
C) 5
D) 11

Question 38

For n = 5,how many allowed values are possible for the orbital quantum number and the orbital magnetic quantum number?

A) 5,11
B) 6,12
C) 5,9
D) 4,9

Question 39

The ground state electronic configuration for sodium is 1s²2s²2p⁶3s¹.What is the orbital quantum number of the last (3s¹)electron?

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

Question 40

The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number = 4,there are permitted how many possible substates?

A) 22
B) 18
C) 8
D) 32

Question 41

A ruby laser delivers a 2.28-J pulse in approximately 50 nanoseconds.The wavelength of the light is 694.4 nm.At least how many atoms within the ruby rod had to be excited to allow this high-energy laser pulse? (h = 6.63 × 10−³⁴ J⋅s,c = 3.00 × 10⁸ m/s,1 eV = 1.6 × 10−¹⁹ J,and 1 nm = 10−⁹ m)

A) 3 × 10¹⁹
B) 4 × 10¹⁸
C) 8 × 10¹⁸
D) 6 × 10²⁰

Question 42

The wavelength of a coherent laser is 628 nm.What energy difference exists between the upper excited state involved and the lower unexcited ground state? (h = 6.63 × 10−³⁴ J⋅s,c = 3.00 × 10⁸ m/s,1 eV = 1.60 × 10−¹⁹ J,and 1 nm = 10−⁹ m)

A) 1.86 eV
B) 1.81 eV
C) 1.75 eV
D) 1.98 eV

Question 43

The red light from a HeNe laboratory laser results from a transition in Ne.Determine the energy difference between the states if the wavelength of the light given off is 634 nm.(h = 6.63 × 10−³⁴ J⋅s,c = 3.00 × 10⁸ m/s,1 eV = 1.60 × 10−¹⁹ J,and 1 nm = 10−⁹ m)

A) 2.22 eV
B) 1.43 eV
C) 1.96 eV
D) 2.04 eV