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:

Accepted Answer

B

Question 2

Characteristic K x-rays are the result of:

Accepted Answer

Characteristic K x-rays are the result of inner electron transitions, specifically when an outer shell electron fills a vacancy in the K-shell and emits an x-ray photon.

Question 3

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

Accepted Answer

D

Question 4

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

Accepted Answer

The answer of In the Bohr model of the atom,the...

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?

Accepted Answer

The answer of Which of the following transitions in hydrogen...

Question 6

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

Accepted Answer

The energy of the n = 5 state is given by:E = -13.6 eV / n^2 = -13.6 eV / 5^2 = -0.544 eV

Question 7

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

Accepted Answer

The four visible colors emitted by hydrogen atoms are produced when electrons transition from higher energy levels to the n=2 energy level. Therefore, the electrons end up in the level with n=2. Options A and D are incorrect because they imply that the electrons start in the ground state or level n=2, which is not the case for the visible colors emitted by hydrogen atoms. Option B is incorrect because it implies that the electrons end up in the ground state, which is not possible for the visible colors emitted by hydrogen atoms since the ground state does not produce any visible light.

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?

Accepted Answer

The answer of Of the various wavelengths emitted from a...

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)

Accepted Answer

The energy of a photon is given by the equation:
E = hc/λ
where E is the energy of the photon, h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon.
To find the wavelength of a photon with 13.6 eV of energy, we need to convert this energy to joules:
13.6 eV x (1.6 x 10^-19 J/eV) = 2.176 x 10^-18 J
Now we can use the equation above to solve for λ:
2.176 x 10^-18 J = (6.63 x 10^-34 J s)(3.00 x 10^8 m/s)/λ
λ = (6.63 x 10^-34 J s)(3.00 x 10^8 m/s)/(2.176 x 10^-18 J)
λ = 91.4 nm

Therefore, the answer is A.

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?

Accepted Answer

The answer of The ionization energy of the hydrogen atom...

Question 11

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

Accepted Answer

According to Bohr's model, the radius of the electron orbit is proportional to n^2, so as the electron moves from n=1 to n=3, the radius of the orbit increases by a factor of (3^2)/(1^2) = 9. The angular momentum of the electron is given by L = n(ħ/2π), so as n increases from 1 to 3, the angular momentum triples (L3/L1 = 3(3/2)/1/2 = 9). Therefore, choice B is the correct option.

Question 12

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

Accepted Answer

In a hydrogen atom, the potential energy (PE) is negative and twice the magnitude of the kinetic energy (KE), but opposite in sign. Therefore, the absolute value of the potential energy is twice the kinetic energy.

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?

Accepted Answer

To determine the wavelength of a hydrogen line, we use the formula:

1/λ = R(1/n1^2 - 1/n2^2)

where λ is the wavelength, R is the Rydberg constant (1.0974 x 10^7 m^-1), and n1 and n2 are the initial and final energy levels, respectively. Plugging in n1 = 5 and n2 = 3, we get:

1/λ = R(1/5^2 - 1/3^2) = 1.0974 x 10^7 m^-1 (1/25 - 1/9) = 1.0974 x 10^7 m^-1 (4/225) = 0.0000486 m^-1

Taking the reciprocal of this value gives us the wavelength:

λ = 1/0.0000486 m^-1 = 20,491 nm

Therefore, the correct answer is B, which is the closest option to 20,491 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?

Accepted Answer

The answer of When a hydrogen atom absorbs a photon...

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?

Accepted Answer

The energy difference between levels n=4 and n=3 in a hydrogen atom is calculated using the formula: E = 13.6 eV * (1/n1^2 - 1/n2^2). For n1=3 and n2=4, E = 13.6 * (1/3^2 - 1/4^2) = 0.66 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?

Accepted Answer

The answer of When a hydrogen atom absorbs a photon...

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).

Accepted Answer

The radius of electron in the nth level of hydrogen atom can be calculated using the following formula:

r = (n²h²ε₀)/(πme²)

where 
r = radius of orbit
n = principal quantum number
h = Planck's constant
ε₀ = permittivity of free space
me = mass of electron
e = elementary charge

For n = 1, r = 0.0529 nm

For n = 4, we need to calculate the radius using the above formula:

r = (4²h²ε₀)/(πme²) = (16h²ε₀)/(πme²)

Substituting the values of h, ε₀, and me, we get:

r = (16 x 6.626 x 10^-34 J s x (8.854 x 10^-12 F/m) ) / (π x (9.109 x 10^-31 kg) x (1.602 x 10^-19 C)^2)

r = 8.46 x 10^-11 m = 0.846 nm

Therefore, the radius of electron orbit in the n = 4 level of hydrogen atom is 0.846 nm, which is closest to option 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?

Accepted Answer

The energy required to ionize the hydrogen atom from the ground state is 13.6 eV. If a photon of 22.0 eV is absorbed, the excess energy after ionization is 22.0 eV - 13.6 eV = 8.4 eV, which becomes the kinetic energy of the electron.

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. )

Accepted Answer

The longest wavelength in the Paschen series corresponds to the transition from infinity (or very high energy level) to n = 3. Using the formula:
1/λ = R(1/3^2 - 1/n^2), where R is the Rydberg constant (1.097 x 10^7 m^-1)
we can calculate the longest wavelength:
1/λ = R(1/9 - 1/infinity) = R/9
λ = 9R = 9 x 1.097 x 10^7 m^-1 = 9.87 x 10^7 nm
Converting to meters, we get:
λ = 9.87 x 10^-2 m = 98.7 nm
This is closest to choice C: 1880 nm, which is approximately 18 times longer than the actual answer. Therefore, choice C is the best choice.

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. )

Accepted Answer

The longest wavelength in the Lyman series corresponds to the transition from n=2 to n=1. Using the Rydberg formula for hydrogen, the wavelength is approximately 122 nm.

Quiz 29: Nuclear Physics: Part A

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:

Characteristic K x-rays are the result of:

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

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

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?

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

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

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?

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)

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?

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

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

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?

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?

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?

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?

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) .

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?

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. )

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. )

Quiz 29: Nuclear Physics: Part A

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:

Characteristic K x-rays are the result of:

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

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

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

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

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

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?

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)

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?

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

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

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?

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?

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?

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?

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) .

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?

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. )

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. )

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?

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)

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. )

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. )