Question 1

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 an electron in the nth state of a hydrogen atom is given by E_n = -13.6 eV / n^2. For n = 5, E_5 = -13.6 eV / 25 = -0.544 eV.

Question 2

If the radius of the electron orbit in the n = 1 level of the hydrogen atoms is 0.052 9 nm,what is its radius for the n = 5 level? (Assume the Bohr model is valid).

Accepted Answer

D

Question 3

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

Accepted Answer

The Lyman series involves transitions to n=1. The first line corresponds to the transition from n=2 to n=1, and the second line corresponds to the transition from n=3 to n=1. Using the Rydberg formula, the wavelength for the second line is approximately 103 nm.

Question 4

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 5

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?

Accepted Answer

When a cool gas is placed between a glowing wire filament source and a diffraction grating, the gas will absorb certain wavelengths of light from the source depending on the gas's composition. This will result in dark lines in the spectrum produced by the diffraction grating, indicating the wavelengths of light that were absorbed by the gas. This is known as line absorption spectrum. Therefore, option B is the correct choice.

Question 6

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

Accepted Answer

The Rutherford model proposed that the majority of an atom's volume is empty space with the positively charged nucleus located at the center. This means that most of the volume of the atom does not contain any particles.

Question 7

What is the wavelength of the line in the Paschen series of hydrogen that is comprised of transitions from the n = 4 to the n = 3 levels? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

Accepted Answer

The wavelength of a line in the Paschen series of hydrogen can be calculated using the formula:

1/λ = R(1/n1^2 - 1/n2^2)

where λ is the wavelength, R is the Rydberg constant, and n1 and n2 are the initial and final energy levels of the electron in the hydrogen atom.

For the transition from n=4 to n=3, we have:

1/λ = R(1/4^2 - 1/3^2)

Using the value of the Rydberg constant given in the question, and converting 1 nm to meters, we get:

1/λ = (1.097 x 10^7 m^-1) x (1/16 - 1/9)

1/λ = 2.363 x 10^6 m^-1

λ = 1/2.363 x 10^6 m^-1 = 1.875 x 10^-7 m = 1875 nm

Therefore, the correct answer is choice B) 1 875 nm.

Question 8

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

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). λ = hc/E = (6.63 x 10^-34 J·s)(3.00 x 10^8 m/s) / (13.6 x 1.6 x 10^-19 J) = 91.4 nm.

Question 9

What is the wavelength of the line in the Balmer series of hydrogen that is comprised of transitions from the n = 4 to the n = 2 level? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

Accepted Answer

The wavelength of the Balmer series transition from n=4 to n=2 can be calculated using the Rydberg formula: 1/λ = R(1/n1² - 1/n2²). Substituting n1=2, n2=4, and R=1.097x10^7 m^-1, we find λ ≈ 486 nm.

Question 10

The Lyman series of hydrogen corresponds to electron transitions from higher levels to n = 1.What is the longest wavelength in that series? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

Accepted Answer

The longest wavelength in the Lyman series corresponds to the transition from the highest energy level (n = ∞) to the first energy level (n = 1). Using the formula for the Lyman series:
1/λ = R(1/n1^2 - 1/n2^2)
where n1 = 1 and n2 = ∞
1/λ = R(1 - 0)
λ = 1/R = 1.097 x 10^7 m^-1

Converting to nanometers:
λ = (1.097 x 10^7 m^-1)(10^-9 m/nm)^-1 = 1.097 x 10^3 nm = 1097 nm

Therefore, the longest wavelength in the Lyman series is 1097 nm, which corresponds to choice B (122 nm) after conversion to nanometers.

Question 11

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

Accepted Answer

When a high voltage is applied to a low-pressure gas causing it to glow, it will emit a line emission spectrum. This is because the high energy electrons in the gas atoms are excited to higher energy levels and then as they return to their ground state, they emit specific wavelengths of light which appear as bright lines in the spectrum.

Question 12

Of the various 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?

Accepted Answer

The transitions associated with the n = 1 level in a hydrogen gas discharge tube produce only ultraviolet wavelengths.

Question 13

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

Accepted Answer

When a wire carries high current causing it to glow, it will emit a continuous spectrum of radiation. This is because the wire is heated to a high enough temperature that it emits radiation over a range of wavelengths, rather than just emitting specific lines of light (line emission). It is not absorbing any specific lines of light (line absorption), and it is not emitting light of a single wavelength (monochromatic).

Question 14

In contrast to Thomson's model of the atom,Rutherford's model:

Accepted Answer

Rutherford's model had the positive charge concentrated in a small region called the nucleus, while Thomson's model had the positive charge spread uniformly throughout the atom.

Question 15

The visible lines from hydrogen are all members of the:

Accepted Answer

The Balmer series includes all the visible spectral lines of hydrogen, while the Lyman, Paschen, and Brackett series include only lines in the ultraviolet, infrared, and far-infrared regions, respectively.

Question 16

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 = 5 to n = 2 state?

Accepted Answer

The energy of a photon emitted during a transition from energy level n1 to n2 is given by: E = (hcR)/((1/n1^2) - (1/n2^2)), where h is Planck's constant, c is the speed of light, and R is the Rydberg constant. Substituting the given values, we get:
E = (6.626 x 10^-34 J s x 3 x 10^8 m/s x 1.097 x 10^7 m^-1)/((1/5^2) - (1/2^2))
E = 2.86 x 10^-19 J
Converting to eV: E = (2.86 x 10^-19 J)/(1.602 x 10^-19 J/eV) = 1.79 eV
Thus, the energy of the emitted photon is 1.79 eV, which is closest to choice A (2.9 eV).

Question 17

An alpha particle is:

Accepted Answer

An alpha particle is specifically a helium-4 nucleus, consisting of two protons and two neutrons, and is positively charged. It is not a neutral helium atom (which would include two electrons), not any positively charged nucleus, and not an x-ray.

Question 18

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 = 2 states?

Accepted Answer

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

Question 19

The Paschen series of hydrogen corresponds to electron transitions from higher levels to n = 3.What is the shortest wavelength in that series? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

Accepted Answer

The shortest wavelength in the Paschen series corresponds to the transition from n = ∞ to n = 3. Using the Rydberg formula: 1/λ = R(1/3² - 1/∞²), we find λ = 1/(R/9) = 9/R. Substituting R = 1.097 x 10^7 m^-1, λ = 9/(1.097 x 10^7) = 820 nm.

Question 20

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

Accepted Answer

The answer of The four visible colors emitted by hydrogen...

Quiz 28: Atomic Physics

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

If the radius of the electron orbit in the n = 1 level of the hydrogen atoms is 0.052 9 nm,what is its radius for the n = 5 level? (Assume the Bohr model is valid) .

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

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 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?

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

What is the wavelength of the line in the Paschen series of hydrogen that is comprised of transitions from the n = 4 to the n = 3 levels? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

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

What is the wavelength of the line in the Balmer series of hydrogen that is comprised of transitions from the n = 4 to the n = 2 level? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

The Lyman series of hydrogen corresponds to electron transitions from higher levels to n = 1.What is the longest wavelength in that series? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

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

Of the various 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?

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

In contrast to Thomson's model of the atom,Rutherford's model:

The visible lines from hydrogen are all members of the:

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 = 5 to n = 2 state?

An alpha particle is:

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 = 2 states?

The Paschen series of hydrogen corresponds to electron transitions from higher levels to n = 3.What is the shortest wavelength in that series? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

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

Quiz 28: Atomic Physics

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

If the radius of the electron orbit in the n = 1 level of the hydrogen atoms is 0.052 9 nm,what is its radius for the n = 5 level? (Assume the Bohr model is valid) .

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

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 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?

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

What is the wavelength of the line in the Paschen series of hydrogen that is comprised of transitions from the n = 4 to the n = 3 levels? (R = 1.097 x 107 m-1 and 1 nm = 10-9 m)

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

What is the wavelength of the line in the Balmer series of hydrogen that is comprised of transitions from the n = 4 to the n = 2 level? (R = 1.097 x 107 m-1 and 1 nm = 10-9 m)

The Lyman series of hydrogen corresponds to electron transitions from higher levels to n = 1.What is the longest wavelength in that series? (R = 1.097 x 107 m-1 and 1 nm = 10-9 m)

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

Of the various 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?

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

In contrast to Thomson's model of the atom,Rutherford's model:

The visible lines from hydrogen are all members of the:

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 = 5 to n = 2 state?

An alpha particle is:

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 = 2 states?

The Paschen series of hydrogen corresponds to electron transitions from higher levels to n = 3.What is the shortest wavelength in that series? (R = 1.097 x 107 m-1 and 1 nm = 10-9 m)

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

What is the wavelength of the line in the Paschen series of hydrogen that is comprised of transitions from the n = 4 to the n = 3 levels? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

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

What is the wavelength of the line in the Balmer series of hydrogen that is comprised of transitions from the n = 4 to the n = 2 level? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

The Lyman series of hydrogen corresponds to electron transitions from higher levels to n = 1.What is the longest wavelength in that series? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)

The Paschen series of hydrogen corresponds to electron transitions from higher levels to n = 3.What is the shortest wavelength in that series? (R = 1.097 x 10⁷ m^-1 and 1 nm = 10^-9 m)