Question 1

An electron in the n = 6 level emits a photon with a wavelength of 410.2 nm.To what energy level does the electron move?

Accepted Answer

The energy difference between two levels in the hydrogen atom is given by the formula derived from the Rydberg equation: $\Delta E = E_f - E_i = R_H \left( \frac{1}{n_f^2} - \frac{1}{n_i^2} \right)$, where $R_H$ is the Rydberg constant, $n_i$ is the initial energy level, and $n_f$ is the final energy level. The wavelength of the emitted photon is related to the energy difference by the equation $E = \frac{hc}{\lambda}$, where $h$ is Planck's constant, $c$ is the speed of light, and $\lambda$ is the wavelength. Given the wavelength, we can calculate the energy of the emitted photon and then use the Rydberg formula to find the final energy level. The given wavelength corresponds to a transition to the $n = 2$ level for a photon emitted in the Balmer series of the hydrogen spectrum.

Question 2

According to the Rydberg equation,the longest wavelength (in nm)in the series of H-atom lines with N₁ = 3 is

Accepted Answer

The longest wavelength corresponds to the smallest energy transition, which is from n=4 to n=3 in the Paschen series. Using the Rydberg formula, this transition gives approximately 1875 nm.

Question 3

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s.What is his wavelength at this speed if his mass is 84.5 kg?

Accepted Answer

The answer of A sprinter must average 24.0 mi/h to...

Question 4

Green light has a wavelength of 5200 Å.Calculate the energy of one photon of green light.

Accepted Answer

The answer of Green light has a wavelength of 5200...

Question 5

Consider the following adjectives used to describe types of spectrum:
Continuous line atomic emission absorption
How many of them are appropriate to describe the spectrum of radiation given off by a black body?

Accepted Answer

The spectrum of radiation given off by a black body is a continuous spectrum and can also have absorption lines superimposed on it. Therefore, the appropriate adjectives to describe the black body spectrum are continuous and absorption. Line and atomic emission are not appropriate as they describe spectra produced by specific atoms or molecules, not a black body.

Question 6

The Bohr theory of the hydrogen atom predicts the energy difference (in J)between the n = 3 and the n = 5 state to be

Accepted Answer

According to the Bohr theory, the energy difference between two states can be calculated using the following equation:
ΔE = Rh [(1/n1^2) - (1/n2^2)]
where Rh is the Rydberg constant for hydrogen, n1 and n2 are the initial and final energy levels, respectively.
Plugging in the values, we get:
ΔE = Rh [(1/3^2) - (1/5^2)]
ΔE = (2.18 x 10^-18 J) [(1/9) - (1/25)]
ΔE = (2.18 x 10^-18 J) [0.1111]
ΔE = 2.42 x 10^-19 J
Therefore, choice D (1.55 x 10^-19 J) is the closest match.

Question 7

Infrared radiation from the sun has a wavelength of 6200 nm.Calculate the energy of one photon of that radiation.

Accepted Answer

The energy of a photon is calculated using the formula E = hc/λ, where h is Planck's constant (6.626 x 10^-34 J·s), c is the speed of light (3 x 10^8 m/s), and λ is the wavelength in meters (6200 nm = 6.2 x 10^-6 m). This calculation results in an energy value between 10^-20 and 10^-19 J.

Question 8

The de Broglie equation predicts that the wavelength (in m)of a proton moving at 1000.m/s is

Accepted Answer

The answer of The de Broglie equation predicts that the...

Question 9

According to the Rydberg equation,the line with the shortest wavelength in the emission spectrum of atomic hydrogen is predicted to lie at a wavelength (in nm)of

Accepted Answer

The answer of According to the Rydberg equation,the line with...

Question 10

For potassium metal,the work function $\phi$ (the minimum energy needed to eject an electron from the metal surface)is 3.68 $\times$ 10^-19 J.Which is the longest wavelength of the following which could excite photoelectrons?

Accepted Answer

The longest wavelength that could excite photoelectrons is the one with the lowest energy, as it must be greater than or equal to the work function of potassium. Using the equation E = hc/λ, where E is the energy of a photon, h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon, we can solve for the energy of each wavelength option:

A) E = hc/λ = (6.626 x 10^-34 J s)(3.00 x 10^8 m/s)/(550 x 10^-9 m) = 3.62 x 10^-19 J 
B) E = hc/λ = (6.626 x 10^-34 J s)(3.00 x 10^8 m/s)/(500 x 10^-9 m) = 4.21 x 10^-19 J 
C) E = hc/λ = (6.626 x 10^-34 J s)(3.00 x 10^8 m/s)/(450 x 10^-9 m) = 4.65 x 10^-19 J 
D) E = hc/λ = (6.626 x 10^-34 J s)(3.00 x 10^8 m/s)/(400 x 10^-9 m) = 5.24 x 10^-19 J 
E) E = hc/λ = (6.626 x 10^-34 J s)(3.00 x 10^8 m/s)/(350 x 10^-9 m) = 6.03 x 10^-19 J

Option B has the lowest energy, which is greater than the work function of potassium, so it is the best choice.

Question 11

According to the Bohr theory of the hydrogen atom,the minimum energy (in J)needed to ionize a hydrogen atom from the n = 2 state is

Accepted Answer

According to the Bohr theory, the energy needed to ionize a hydrogen atom from the n = 2 state is given by:

E = (-13.6 eV) [(1/2^2) - (1/n^2)]

where n is the final state of the hydrogen atom after ionization.

For ionization from the n = 2 state, the final state is n = infinity, so we have:

E = (-13.6 eV) [(1/2^2) - (1/∞^2)] = 10.2 eV

To convert this to joules, we use the conversion factor 1 eV = 1.602 x 10^-19 J:

E = (10.2 eV) (1.602 x 10^-19 J/eV) = 1.64 x 10^-18 J

Therefore, the answer is choice C.

Question 12

A photon has an energy of 5.53 $\times$ 10^-17 J.What is its frequency in s^-1?

Accepted Answer

The answer of A photon has an energy of 5.53...

Question 13

The size of an atomic orbital is associated with

Accepted Answer

The size of an atomic orbital is associated with the principal quantum number (n), which determines the average distance of the electron from the nucleus. As n increases, the size of the orbital increases as well.

Question 14

The orientation in space of an atomic orbital is associated with

Accepted Answer

The answer of The orientation in space of an atomic...

Question 15

Consider the following adjectives used to describe types of spectrum:
Continuous line atomic emission absorption
How many of them are appropriate to describe the spectrum of radiation absorbed by a sample of mercury vapor?

Accepted Answer

The answer of Consider the following adjectives used to describe...

Question 16

Platinum,which is widely used as a catalyst,has a work function $\phi$ (the minimum energy needed to eject an electron from the metal surface)of 9.05 $\times$ 10^-19 J.What is the longest wavelength of light which will cause electrons to be emitted?

Accepted Answer

The answer of Platinum,which is widely used as a catalyst,has...

Question 17

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n₁ = 2 to n₂ = 4.(R = 1.096776 $\times$ 10⁷ m^-1)

Accepted Answer

The answer of Use the Rydberg equation to calculate the...

Question 18

Line spectra from all regions of the electromagnetic spectrum,including the Paschen series of infrared lines for hydrogen,are used by astronomers to identify elements present in the atmospheres of stars.Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 3.(R = 1.096776 $\times$ 10⁷ m^-1)

Accepted Answer

The answer of Line spectra from all regions of the...

Question 19

The shape of an atomic orbital is associated with

Accepted Answer

The shape of an atomic orbital is primarily determined by the angular momentum quantum number (l). The other quantum numbers (n, mS, and s) determine other properties of the orbital, but not its shape.

Question 20

If the energy of a photon is 1.32 $\times$ 10^-18 J,what is its wavelength in nm?

Accepted Answer

The answer of If the energy of a photon is...

Quiz 7: Quantum Theory and Atomic Structure

An electron in the n = 6 level emits a photon with a wavelength of 410.2 nm.To what energy level does the electron move?

According to the Rydberg equation,the longest wavelength (in nm) in the series of H-atom lines with N₁ = 3 is

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s.What is his wavelength at this speed if his mass is 84.5 kg?

Green light has a wavelength of 5200 Å.Calculate the energy of one photon of green light.

Consider the following adjectives used to describe types of spectrum: Continuous line atomic emission absorption How many of them are appropriate to describe the spectrum of radiation given off by a black body?

The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the n = 3 and the n = 5 state to be

Infrared radiation from the sun has a wavelength of 6200 nm.Calculate the energy of one photon of that radiation.

The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000.m/s is

According to the Rydberg equation,the line with the shortest wavelength in the emission spectrum of atomic hydrogen is predicted to lie at a wavelength (in nm) of

For potassium metal,the work function $\phi$ (the minimum energy needed to eject an electron from the metal surface) is 3.68 $\times$ 10^-19 J.Which is the longest wavelength of the following which could excite photoelectrons?

According to the Bohr theory of the hydrogen atom,the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state is

A photon has an energy of 5.53 $\times$ 10^-17 J.What is its frequency in s^-1?

The size of an atomic orbital is associated with

The orientation in space of an atomic orbital is associated with

Consider the following adjectives used to describe types of spectrum: Continuous line atomic emission absorption How many of them are appropriate to describe the spectrum of radiation absorbed by a sample of mercury vapor?

Platinum,which is widely used as a catalyst,has a work function $\phi$ (the minimum energy needed to eject an electron from the metal surface) of 9.05 $\times$ 10^-19 J.What is the longest wavelength of light which will cause electrons to be emitted?

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n₁ = 2 to n₂ = 4.(R = 1.096776 $\times$ 10⁷ m^-1)

The shape of an atomic orbital is associated with

If the energy of a photon is 1.32 $\times$ 10^-18 J,what is its wavelength in nm?

Quiz 7: Quantum Theory and Atomic Structure

An electron in the n = 6 level emits a photon with a wavelength of 410.2 nm.To what energy level does the electron move?

According to the Rydberg equation,the longest wavelength (in nm) in the series of H-atom lines with N1 = 3 is

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s.What is his wavelength at this speed if his mass is 84.5 kg?

Green light has a wavelength of 5200 Å.Calculate the energy of one photon of green light.

Consider the following adjectives used to describe types of spectrum: Continuous line atomic emission absorption How many of them are appropriate to describe the spectrum of radiation given off by a black body?

The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the n = 3 and the n = 5 state to be

Infrared radiation from the sun has a wavelength of 6200 nm.Calculate the energy of one photon of that radiation.

The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000.m/s is

According to the Rydberg equation,the line with the shortest wavelength in the emission spectrum of atomic hydrogen is predicted to lie at a wavelength (in nm) of

For potassium metal,the work function ϕ\phiϕ (the minimum energy needed to eject an electron from the metal surface) is 3.68 ×\times× 10-19 J.Which is the longest wavelength of the following which could excite photoelectrons?

According to the Bohr theory of the hydrogen atom,the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state is

A photon has an energy of 5.53 ×\times× 10-17 J.What is its frequency in s-1?

The size of an atomic orbital is associated with

The orientation in space of an atomic orbital is associated with

Consider the following adjectives used to describe types of spectrum: Continuous line atomic emission absorption How many of them are appropriate to describe the spectrum of radiation absorbed by a sample of mercury vapor?

Platinum,which is widely used as a catalyst,has a work function ϕ\phiϕ (the minimum energy needed to eject an electron from the metal surface) of 9.05 ×\times× 10-19 J.What is the longest wavelength of light which will cause electrons to be emitted?

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n1 = 2 to n2 = 4.(R = 1.096776 ×\times× 107 m-1)

The shape of an atomic orbital is associated with

If the energy of a photon is 1.32 ×\times× 10-18 J,what is its wavelength in nm?

According to the Rydberg equation,the longest wavelength (in nm) in the series of H-atom lines with N₁ = 3 is

For potassium metal,the work function $\phi$ (the minimum energy needed to eject an electron from the metal surface) is 3.68 $\times$ 10^-19 J.Which is the longest wavelength of the following which could excite photoelectrons?

A photon has an energy of 5.53 $\times$ 10^-17 J.What is its frequency in s^-1?

Platinum,which is widely used as a catalyst,has a work function $\phi$ (the minimum energy needed to eject an electron from the metal surface) of 9.05 $\times$ 10^-19 J.What is the longest wavelength of light which will cause electrons to be emitted?

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n₁ = 2 to n₂ = 4.(R = 1.096776 $\times$ 10⁷ m^-1)

If the energy of a photon is 1.32 $\times$ 10^-18 J,what is its wavelength in nm?