Question 1

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

Accepted Answer

The formula for calculating the wavelength of a photon emitted during a transition between energy levels in hydrogen is:
λ = hc/ΔE
where h is Planck's constant, c is the speed of light, and ΔE is the change in energy between the two levels.

For this transition, ΔE = E5 - E3, where E5 is the energy of the n=5 level and E3 is the energy of the n=3 level. Using the formula for energy levels in hydrogen:
En = -13.6/n^2 (in electron volts)

E5 = -13.6/5^2 = -0.544 eV
E3 = -13.6/3^2 = -1.511 eV

ΔE = (-0.544) - (-1.511) = 0.967 eV

Converting this energy to joules:
1 eV = 1.602 x 10^-19 J
0.967 eV = 1.55 x 10^-19 J

Now we can plug this into the formula for wavelength:

λ = hc/ΔE = (6.626 x 10^-34 J s)(3.00 x 10^8 m/s)/(1.55 x 10^-19 J) = 1.28 x 10^-6 m = 1280 nm

Therefore, the answer is B, 1290 nm (rounded to the nearest 10 nm).

Question 2

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

Accepted Answer

A

Question 3

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.

Accepted Answer

The four visible colors emitted by hydrogen atoms are produced by electrons that end up in the level with n = 2. When an electron transitions from a higher energy level to n = 2, it releases energy in the form of visible light. This results in the emission of four specific colors, known as the Balmer series: red, blue-green, blue-violet, and violet.

Question 4

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^-³⁴J.s. The ground state of hydrogen is at -13.6 eV.) A) 822 nm B) 365 nm C) 1880 nm D) 1094 nm

Accepted Answer

The longest wavelength in the Paschen series corresponds to the transition from n=4 to n=3. Using the Rydberg formula for hydrogen, the wavelength is calculated to be approximately 1875 nm, which is closest to 1880 nm.

Question 5

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

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 6

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.

Accepted Answer

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

Question 7

The Lyman series of hydrogen is made up of those transitions made from higher levels to n = 1. If the first line (n = 2 to n = 1) in this series has a wavelength of 122 nm, what is the wavelength of the third line (n = 4 to n = 1)?
A) 364 nm
B) 97.6 nm
C) 103 nm
D) 486 nm

Accepted Answer

The wavelength of the third line (n = 4 to n = 1) can be calculated using the Rydberg formula. The wavelength is shorter than the first line, and 97.6 nm is the correct value.

Question 8

Of the wavelengths emitted from a hydrogen gas discharge tube, those that are associated with transitions from higher levels down to the n = 1 level produce which of the following?
A) infrared
B) visible
C) ultraviolet
D) mixture of infrared and visible

Accepted Answer

Transitions from higher energy levels to the n = 1 level in hydrogen produce ultraviolet radiation, known as the Lyman series.

Question 9

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 ^- ³⁴J.s. The ground state of hydrogen is at -13.6 eV.) A) 91.4 nm B) 273 nm C) 456 nm D) 122 nm

Accepted Answer

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

Question 10

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"

Accepted Answer

The energy of the photon is greater than the energy difference between the ground state and the first excited state of the hydrogen atom. Therefore, the photon cannot be absorbed in this case.

Question 11

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

Accepted Answer

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

Question 12

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

Accepted Answer

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

Question 13

When a high voltage is applied to a low-pressure gas causing it to glow, it will emit which type of spectrum?
A) line emission
B) line absorption
C) continuous
D) monochromatic

Accepted Answer

When a low-pressure gas is excited by a high voltage, it will emit a line emission spectrum consisting of a few bright, distinct lines at specific wavelengths characteristic of the gas molecules or atoms. This is due to the excited gas atoms or molecules emitting photons of specific energies as they return to their ground state.

Question 14

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 ^- ³⁴J.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

Accepted Answer

The energy of the photon is 13.6 eV, which is equivalent to 13.6 x 1.6 x 10^-19 J. Using the formula E = hc/λ, where h is Planck's constant and c is the speed of light, we can solve for λ (wavelength). Substituting the values, λ = (6.63 x 10^-34 J·s x 3.00 x 10^8 m/s) / (13.6 x 1.6 x 10^-19 J) = 91.4 nm.

Question 15

In contrast to the plum-pudding model of the atom, Rutherford's model:
A) was first to explain atoms emitting discrete frequencies.
B) had the positive charge concentrated in a small region.
C) eliminated radiation from accelerating charges.
D) had the positive charge spread uniformly through the atom.

Accepted Answer

Rutherford's model proposed that the positive charge of the atom is concentrated in a small, dense nucleus, unlike the plum-pudding model which suggested that positive charge was spread uniformly throughout the atom.

Question 16

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

Accepted Answer

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

Question 17

When a cool gas is placed between a glowing wire filament source and a diffraction grating, the resultant spectrum from the grating is which one of the following?
A) line emission
B) continuous
C) line absorption
D) monochromatic

Accepted Answer

The cool gas absorbs specific wavelengths of light from the continuous spectrum of the glowing wire filament, resulting in a line absorption spectrum.

Question 18

When a wire carries high current causing it to glow, it will emit which type of spectrum?
A) line absorption
B) monochromatic
C) continuous
D) line emission

Accepted Answer

A wire carrying high current and glowing emits a continuous spectrum due to the wide range of energies and wavelengths produced by the thermal motion of charged particles.

Question 19

An alpha particle is:
A) any positively charged nucleus.
B) an X-ray.
C) a neutral helium atom.
D) None of these choices.

Accepted Answer

An alpha particle is specifically a helium nucleus consisting of 2 protons and 2 neutrons, not any positively charged nucleus, an X-ray, or a neutral helium atom.

Question 20

According to the Rutherford model of the atom, most of the volume of an atom:
A) is empty space.
B) was occupied by the nucleus.
C) excluded electrons.
D) contained positive charges.

Accepted Answer

The Rutherford model proposed that atoms consist mostly of empty space, with a small, dense, positively charged nucleus at the center, and electrons orbiting around it.

Quiz 29: Atomic Theory

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?

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:

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^-³⁴J.s. The ground state of hydrogen is at -13.6 eV.)

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) .

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

The Lyman series of hydrogen is made up of those transitions made from higher levels to n = 1. If the first line (n = 2 to n = 1) in this series has a wavelength of 122 nm, what is the wavelength of the third line (n = 4 to n = 1) ?

Of the wavelengths emitted from a hydrogen gas discharge tube, those that are associated with transitions from higher levels down to the n = 1 level produce which of the following?

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 ^- ³⁴J.s. The ground state of hydrogen is at -13.6 eV.)

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 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?

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?

When a high voltage is applied to a low-pressure gas causing it to glow, it will emit which type of spectrum?

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 ^- ³⁴J.s, c = 3.00 10⁸ m/s, 1 eV = 1.6 10 ^- ¹⁹ J, and 1 nm = 10 ^- ⁹ m)

In contrast to the plum-pudding model of the atom, Rutherford's model:

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 cool gas is placed between a glowing wire filament source and a diffraction grating, the resultant spectrum from the grating is which one of the following?

When a wire carries high current causing it to glow, it will emit which type of spectrum?

An alpha particle is:

According to the Rutherford model of the atom, most of the volume of an atom: