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When light of frequency 4.90 x 10¹⁵ s^-1shineson the surface of a metal, electrons are ejected with amaximumkinetic energy of 1.96 x 10^-19 J.
*Calculate the wavelength of this light.

**Find the binding energy of electrons to the metal.

***What is the longest wavelength of light that will ejectelectronsfrom this metal?

When light of frequency equal to 2.11 X 10^15 s^-1 shines on the surface of gold metal, the kinetic energy of ejected electrons is found to be 5.83 X 10^19J. What is the work function of gold?

When light of frequency 1.30x 1015 s-1 shines on the surface of cesium metal, electrons are ejected with a maximum kinetic energy of 5.2x 10-19 J.Calculate the wavelength of this light in nm.

When light of frequency 4.96×10¹⁵ s^-1 shines on the surface of a metal, electrons are ejected with a maximum kinetic energy of 3.88×10^-19 J.

a) Calculate the wavelength of this light.

b) Find the binding energy of electrons to the metal.

c) What is the longest wavelength of light that will eject electrons from this metal?

when light of frequency equal to 2.11 x 10^-15 s-1 shines on the surface of gold metal, the kinetic energy of ejected electrons is found to be 5.83 x 10^-19 J. What is the work function of gold?

when a metal was exposed to light at a frequency of 4.61 x 10^15s^-1, electrons were emitted with kinetic energy of 5.90 x 10^-19J. What is the maximum number of electrons that could be ejectedfrom this metal by a burst of light with a total energy of 4.85 x10^-7 J

When a metal was exposed to light at a frequency of...3.72x10^15 s-1, electrons were emitted with a kinect energy of6.00x10^-19 J.

What is the maximum number of electrons that could be ejectedfrom this metal by a burst of light (at some other frequency) witha total energy of 3.47x10^-7 J?

What is the maximum number of electrons that can be freed by aburst of light of 405 nm whose total energy is 1.00μJ?

When a metal was exposed to light at a frequency of 4.15

When a metal was exposed to light at a frequnecy of 3.16 x 10^15s^-1, electrons were emitted with a kinetic energy of

3.10 x 10^-19 J. What is the maximum number of electrons thatcould be ejected from this metal by a busrt of light (at some otherfrequency) with a total energy of 4.90 x 10^-7 J?

What is the maximum number of electrons that can be freed by a burst of light whose total energy is 2mJ

The work function of potassium is 3.68*10^-19 J. a) What is theminimum frequency of light needed to efect electrons from themetal? b) calculate the kinetic energy of the ejected electronswhen light of frequency equal to 8.62*10^14 s^-1 is used forirradiation.

when a metal was exposed to light at a frequency of 4.49 x 10^15 s^-1, electrons were emitted with a kinetic energy of 4.80 x 10^-19 J. What is the maximum number of electrons that could be ejected from this metal by a burst of light with a total energy of 8.86 x 10^-7 J?

Give the values for n , l , and m l for each orbital in the 2p subshell,

Enter your answer as sets of values of n , l , and m l for different orbitals separated by commas. Separate values within each set by semicolons. Enter your answers in order of increasing n , then in order of increasing l , and then in order of increasing m l . Example: "1;0;-1,1;1;-1,1;2;1" (n;l;ml,n;l;ml,n;l;ml).

Give the values for n , l , and ml for each orbital in the 5d subshell.

Enter your answer as sets of values of n , l , and ml for different orbitals separated by commas. Separate values within each set by semicolons. Enter your answers in order of increasing n , then in order of increasing l , and then in order of increasing ml . Example: "1;0;-1,1;1;-1,1;2;1" (n;l;ml,n;l;ml,n;l;ml).

Problem 6.55

Part A

For n=4, what are the possible values of l?

Enter your answers in ascending order separated by a commas.

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Part B

For l=2, what are the possible values of ml?

Enter your answers in ascending order separated by a commas.

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Correct

Part C

If ml is 2, what are the possible values for l (for all atoms in their ground states that are known to exist)?

Enter your answers in ascending order separated by a commas.

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Problem 6.58

Part A

Give the values for n, l, and ml for each orbital in the 2p subshell,

Enter your answer as sets of values of n, l, and ml for different orbitals separated by commas. Separate values within each set by semicolons. Enter your answers in order of increasing n, then in order of increasing l, and then in order of increasing ml. Example: "1;0;-1,1;1;-1,1;2;1" (n;l;ml,n;l;ml,n;l;ml).

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Part B

Give the values for n, l, and ml for each orbital in the 5d subshell.

Enter your answer as sets of values of n, l, and ml for different orbitals separated by commas. Separate values within each set by semicolons. Enter your answers in order of increasing n, then in order of increasing l, and then in order of increasing ml. Example: "1;0;-1,1;1;-1,1;2;1" (n;l;ml,n;l;ml,n;l;ml).

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Your answer does not have the correct number of comma-separated terms.

Calculate the wavelength of the photon emitted when an electron makes a transition from n=5 to n=3. You can make use of the following constants: h=6.626×10−34 J⋠s c=2.998×108 m/s 1 m=109 nm

Calculate the wavelength of the photon emitted when an electron makes a transition from n=4 to n=3. You can make use of the following constants:

h=6.626×10−34 J⋠s

c=2.998×108 m/s

Part A

Give the values for n, l, and ml for each orbital in the 2p subshell,

Enter your answer as sets of values of n, l, and ml for different orbitals separated by commas. Separate values within each set by semicolons. Enter your answers in order of increasing n, then in order of increasing l, and then in order of increasing ml. Example: "1;0;-1,1;1;-1,1;2;1" (n;l;ml,n;l;ml,n;l;ml).

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Part B

Give the values for n, l, and ml for each orbital in the 5d subshell.

Enter your answer as sets of values of n, l, and ml for different orbitals separated by commas. Separate values within each set by semicolons. Enter your answers in order of increasing n, then in order of increasing l, and then in order of increasing ml. Example: "1;0;-1,1;1;-1,1;2;1" (n;l;ml,n;l;ml,n;l;ml).

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1 m=109 nm

Express your answer to four significant figures and include the appropriate units.

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Part C

Calculate the wavelength of the photon emitted when an electron makes a transition from n=4 to n=3. You can make use of the following constants:

h=6.626×10−34 J⋠s

c=2.998×108 m/s

1 m=109 nm

Express your answer to four significant figures and include the appropriate units.

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Calculate the wavelength of the photon emitted when an electron makes a transition from n=7 to n=3. You can make use of the following constants:

h=6.626×10−34 J⋠s

c=2.998×108 m/s

1 m=109 nm

Express your answer to four significant figures and include the appropriate units.

What is the maximum number of electrons that can be freed by aburst of light of 405 nm whose total energy is 1.00μJ?? Given theminimum evergy of 4.41*10^-19 and a maximum kinetic energy4.95*10^-20.

Titanium metal requires a photon with a minimum energy of 6.94×10−19J to emit electrons.

If titanium is irradiated with light of 233 nm, what is the maximum possible kinetic energy of the emitted electrons?

Titanium metal requires a photon with a minimum energy of 6 .9 4 * 1 0 - 1 9 J to emit electrons. ( a ) What is the minimum frequency of light necessary to emit electrons from titanium via the photoelectric effect? ( b ) What is the wavelength of this light? ( c ) Is it possible to eject electrons from titanium metal using visible light? ( d ) If titanium is irradiated with light of wavelength 233 nm, what is the maximum possible kinetic energy of the emitted electrons? ( d ) What is the maxi - mum number of electrons that can be freed by a burst of light whose total energy is 2 . 0 0 m J ?

It requires a photon with a minimum energy of 4.41 ✕ 10-19 J to emit electrons from sodium metal. c) If sodium is irradiated with light of 389 nm, what is the maximum possible kinetic energy of the emitted electrons?(answer in J) (d) What is the maximum number of electrons that can be freed by a burst of light (λ = 389 nm) whose total energy is 1.20 µJ? (answer in electrons)

It requires a photon with a minimum energy of 4.41 ? 10^-19 J to emit electrons from sodium metal

a)What is the minimum frequency of light necessary to emitelectrons from sodium via the photoelectric effect? I got6.66x10^14 as this answer

I don't understand parts b-d

b)What is the wavelength of this light?
c) If sodium is irradiated with light of 432 nm, what is themaximum possible kinetic energy of the emitted electrons?

d)What is the maximum number of electrons that can be freed by aburst of light (?= 432 nm) whose total energy is 1.29

Part C

Calculate the wavelength of the photon emitted when an electron makes a transition from n=7 to n=3. You can make use of the following constants:

h=6.626×10−34 J⋠s

c=2.998×108 m/s

1 m=109 nm

Express your answer to four significant figures and include the appropriate units.

please help me on my last chem problem first correct answer getsall of the points

s you have discovered, different compositions of semiconductors emit different colors of light with different photon energies.

The energy of each photon (E_photon) emitted from an LED is equal in energy to the band gap (E_g). Recall that the photon energy can be calculated from wavelength:

E_g= E_photon
E_photon = hc/ λ

Where the variables h and c are constants:

Planck ’s Constant, h = 6.626 x 10^-34 J⋠s
Speed of Light, c = 3.0 x 10⁸ m/s

Conversion Factors:

1 m = 1 x 10⁹ nm

Part C - Looking at the equations given above, what is the relationship between band gap energy and the wavelength of light emitted from a semiconductor?

The absolute value of ∆E (J) for an atom is equal to Ephoton, the energy of one photon of light emitted for a transition. If Ephoton is 1.63 x 10-18 J, calculate the wavelength of light, in nanometers. (h = 6.626 x 10-34 J sec ; c = 2.998 x 108 m/s; 1 m = 109 nm).

A. 1.22 x 10-43 nm
B. 122 nm
C. 1.22 x 10-7 nm
D. 1.22 x 10-34 nm