Ch.7 - Quantum MechanicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

What happens when light strikes the surface of a metal? The Photoelectric Effect can help to explain that. 

Examining the Photoelectric Effect

Concept #1: Understanding the Photoelectric Effect

The Photoelectric Effect was theorized by Albert Einstein to help explain what would happen to the electrons on the surface of a metal when a photon (light particle) with enough energy struck. 

Concept #2: Illustrating what happens when a photon strikes the surface of a metal.

Additional Problems
In an experiment of the photoelectric effect, an incident beam of ultraviolet radiation shined on a piece of metal and produced electrons with zero kinetic energy. Which of the following radiation would be most likely to produce electrons with some kinetic energy? A. radio wave B. microwave C. green light D. infrared E. gamma ray
It takes 261 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect? A) 233 B) 165 C) 552 D) 458 E) 725
The figure below shows Ek plotted as a function of v for photoelectric emission from two metals, A and B. Which of the following statements for the two metals is correct? A. Both metals will produce the approximately equal currents under identical conditions. B. The threshold frequencies suggest that metal A is an alkali metal. C. The threshold frequency is the same for both metals. D. The threshold frequency of A is greater than that of B. E. The threshold frequency of A is less than that of B.
The ionization energy of sodium is 496 kJ/mol. In an experiment similar Hertz's experiment to which Einstein famously discovered the photoelectric effect, which statement below is true about the wavelength of radiation that could cause sodium to be ionized upon irradiation? A. If sodium is irradiated with radiation with a wavelength greater than 496 nm, sodium can become ionized B. If sodium is irradiated with radiation with a wavelength greater than 241 nm, sodium can become ionized C. If sodium is irradiated with radiation with a wavelength lower than 496 nm, sodium can become ionized D. If sodium is irradiated with radiation with a wavelength lower than 241 nm, sodium can become ionized E. Since radiation is not a particle, no form of it may cause an electron to be ejected from sodium
Consider two different light sources produce photons of light with wavelengths of 225 nm and 650 nm. If these photons are shined onto zinc metal, which has a work function of 350 kJ/mol, which statement is true? (Hint: The work function corresponds to the least amount of energy required to cause an electron to be ejected from a substance). a. Only the 225 nm photon can cause an electron to be ejected from zinc. b. Only the 650 nm photon can cause an electron to be ejected from zinc c. Neither photon can cause an electron to be ejected from zinc d. Both 225 and 650 nm photons can cause an electron to be ejected from zinc e. None of the above
The work function for chromium metal is 4.37 eV. What wavelength of radiation must be used to eject electrons with a velocity of 2500 km/s?
The photoelectric effect provided evidence for the (wave, particle)-like behavior of light. The phenomenon of diffraction provided evidence for the (wave, particle)-like bahavior of light.  1. wave, wave 2. wave, particle 3. particle, wave 4. particle, particle
Magnesium metal is used in a photoelectric effect experiment.  The work function for Mg (i.e. the energy required to remove an electron) is 3.68 eV.  What is the longest wavelength of light, in nm, that can remove an electron from the Mg.   (1 eV = 1.602 x 10 -19 J; h = 6.63 x 10 -34 J•sec; c = 3.00x10 8 m/sec).  
You may want to reference (Page 305) Section 7.2 while completing this problem.Light from three different lasers (A, B, and C), each with a different wavelength, was shined onto the same metal surface. Laser A produced no photoelectrons. Lasers B and C both produced photoelectrons, but the photoelectrons produced by laser B had a greater velocity than those produced by laser C. Arrange the lasers in order of increasing wavelength.
Titanium metal requires a photon with a minimum energy of  6.94 10 - 19 to emit electrons. You may want to reference (Pages 217 - 218) Section 6.2 while completing this problem.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  6.94 10 - 19 to emit electrons. You may want to reference (Pages 217 - 218) Section 6.2 while completing this problem.Is it possible to eject electrons from titanium metal using visible light?
You may want to reference (Pages 299 - 308) Section 7.2 while completing this problem.The energy required to dislodge electrons from sodium metal via the photoelectric effect is 275 kJ/mol . What wavelength (in nm) of light has sufficient energy per photon to dislodge an electron from the surface of sodium?
The photoelectric effect. If the frequency of the incoming light is increased, will the energy of the ejected electrons increase, decrease, or stay the same?
If electrons are ejected from a given metal when irradiated with a 11-W red laser pointer, what will happen when the same metal is irradiated with a 5-W green laser pointer?
We shine light of three different wavelengths—325 nm, 455 nm, and 632 nm —on a metal surface. We record the following observations for each wavelength, labeled A, B, and C: Observation A: No photoelectrons were observed.Observation B: Photoelectrons with a kinetic energy of 155 kJ/mol were observedObservation C: Photoelectrons with a kinetic energy of 51 kJ/mol were observedWhich observation corresponds to which wavelength of light?
Describe the photoelectric effect.
How did the photoelectric effect lead Einstein to propose that light is quantized?
Determine the longest wavelength of light required to remove an electron from an atom of a metal, if the binding energy for an electron in that metal is 309 kJ/mol.a. 147 nmb. 68.0 nmc. 113 nmd. 885 nme. 387nm
Determine the shortest frequency of light required to remove an electron from a sample of a metal, if the binding (threshold) energy of the metal is 3.14x103 kJ/mol. a. 7.87x1015 Hzb. 4.74x1015 Hzc. 2.11x1015 Hzd. 1.27x1015 Hze. 6.19x1015 Hz 
R = 2.18x10-18 J;  h = 6.626x10-34 J•sec or 6.626x10-34 kg•m2 sec-1;  c = 3.00 x 10 8 m•sec-1; 1eV= 1.602x10-19 J a.) What is the energy of a photon with a wavelength of 335 nm?    b.) If a metal that has a work function of 2.80 eV, what wavelength of light is required to generate electrons with a kinetic energy of 1.02 eV?      c.) If a reaction is exothermic, does it mean that ΔE for the reaction is negative? Explain.   
The first ionization energy of carbon is 1.81 aJ. Assuming an ionization efficiency of 22.35%, how many photons of the lowest possible frequency are required to ionize a sample of carbon that contains 5.32 x 1018 atoms?a) 2.38 x 1019 photonsb) 4.20 x 10-20 photonsc) 2.73 x 1015 photonsd) 9.11 x 106 photons 
Determine the longest wavelength of light required to remove an electron from a sample of potassium metal, if the binding energy for an electron in K is 1.76 × 103 kJ/mol.A) 113 nmB) 885 nmC) 68.0 nmD) 147 nmE) 387 nm 
What is a quantum of light called?a) the wavelengthb) the frequencyc) the amplituded) a photon
Assuming an ionization efficiency of 18.0%, how many photons are needed to ionize 1.00 x 1016 atoms?
Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (a) What is the minimum energy needed to eject an electron?
Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (b)What wavelength of radiation will provide a photon of this energy?
Molybdenum metal must absorb radiation with a minimum frequency of 1.09 x 10 15 s-1 before it can eject an electron from its surface via the photoelectric effect. (c) If molybdenum is irradiated with light of wavelength of 120 nm, what is the maximum possible kinetic energy of the emitted electrons?
Sodium metal requires a photon with a minimum energy of 4.41 x 10 -19 J to emit electrons. (c) If sodium is irradiated with light of 439 nm, what is the maximum possible kinetic energy of the emitted electrons?
The work function (ϕ) of a metal is the minimum energy needed to remove an electron from its surface. Is it easier to remove an electron from a gaseous silver atom or from the surface of solid silver (ϕ = 7.59×10−19 J; IE = 731 kJ/mol)?
The work function (ϕ) of a metal is the minimum energy needed to remove an electron from its surface. Explain the results in terms of the electron-sea model of metallic bonding.
The photoelectric effect is illustrated in a plot of the kinetic energies of electrons ejected from the surface of potassium metal or silver metal at different frequencies of incident light.Why don’t the lines begin at the origin?
The photoelectric effect is illustrated in a plot of the kinetic energies of electrons ejected from the surface of potassium metal or silver metal at different frequencies of incident light.Why don’t the lines begin at the same point?
The photoelectric effect is illustrated in a plot of the kinetic energies of electrons ejected from the surface of potassium metal or silver metal at different frequencies of incident light.From which metal will light of shorter wavelength eject an electron?
The photoelectric effect is illustrated in a plot of the kinetic energies of electrons ejected from the surface of potassium metal or silver metal at different frequencies of incident light.Why are the slopes equal?
You may want to reference (Pages 296 - 324)Chapter 7 while completing this problem.The energy required to ionize sodium is 496 kJ/mol. What minimum frequency of light is required to ionize sodium?
In his explanation of the threshold frequency in the photoelectric effect, Einstein reasoned that the absorbed photon must have a minimum energy to dislodge an electron from the metal surface. This energy is called the work function (ϕ) of the metal. What is the longest wavelength of radiation (in nm) that could cause the photoelectric effect in calcium, ϕ = 4.60 x 10−19 J?
In his explanation of the threshold frequency in the photoelectric effect, Einstein reasoned that the absorbed photon must have a minimum energy to dislodge an electron from the metal surface. This energy is called the work function (ϕ) of the metal. What is the longest wavelength of radiation (in nm) that could cause the photoelectric effect in titanium, ϕ = 6.94 x 10−19 J?
In his explanation of the threshold frequency in the photoelectric effect, Einstein reasoned that the absorbed photon must have a minimum energy to dislodge an electron from the metal surface. This energy is called the work function (ϕ) of the metal. What is the longest wavelength of radiation (in nm) that could cause the photoelectric effect in sodium, ϕ = 4.41 x 10−19 J?
A metal with a threshold frequency of 1.43×1015 s-1 emits an electron with a velocity of 6.96×105 m/s when radiation of 1.76×1015 s-1 strikes the metal. Calculate the mass of the electron.
What is the threshold frequency for sodium metal if a photon with frequency 6.66 × 1014 s−1 ejects an electron with 7.74 × 10 −20 J kinetic energy? Will the photoelectric effect be observed if sodium is exposed to orange light?
In order to comply with the requirement that energy be conserved, Einstein showed in the photoelectric effect that the energy of a photon (hν) absorbed by a metal is the sum of the work function (ϕ), which is the minimum energy needed to dislodge an electron from the metal’s surface, and the kinetic energy (Ek) of the electron: hν = ϕ + E k. When light of wavelength 358.1 nm falls on the surface of potassium metal, the speed (u) of the dislodged electron is 6.40 x 105 m/s. What is Ek (1/2mu2) of the dislodged electron?
In order to comply with the requirement that energy be conserved, Einstein showed in the photoelectric effect that the energy of a photon (hν) absorbed by a metal is the sum of the work function (ϕ), which is the minimum energy needed to dislodge an electron from the metal’s surface, and the kinetic energy (Ek) of the electron: hν = ϕ + E k. When light of wavelength 358.1 nm falls on the surface of potassium metal, the speed (u) of the dislodged electron is 6.40 x 105 m/s. What is ϕ (in J) of potassium?
The work function of an element is the energy required to remove an electron from the surface of the solid element. The work function for lithium is 279.7 kJ/mol (that is, it takes 279.7 kJ of energy to remove 1 mole of electrons from 1 mole of Li atoms on the surface of Li metal; 1 mol Li 5 6.022 x 1023 atoms Li). What is the maximum wavelength of light that can remove an electron from an atom on the surface of lithium metal?
It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium metal. (1 mol electrons = 6.022 x 1023 electrons.) How much energy does it take to remove a single electron from an atom on the surface of solid rubidium? What is the maximum wavelength of light capable of doing this?
It takes 7.21 x 10 -19 J of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?
Many calculators use photocells as their energy source. Find the maximum wavelength needed to remove an electron from silver (ϕ = 7.59 x 10−19 J). Is silver a good choice for a photocell that uses visible light?
You may want to reference (Pages 296 - 324) Chapter 7 while completing this problem.An X-ray photon with a wavelength of 0.965 nm strikes a surface. The emitted electron has a kinetic energy of 965 eV. What is the binding energy of the electron in kJ/mol? [Note that KE = mv2/2 large{frac{_1}{^2}mv^2} and 1 electron volt (eV) = 1.602 x 10 - 19 J]
Ionization involves completely removing an electron from an atom. How much energy is required to ionize a hydrogen atom in its ground (or lowest energy) state?
Ionization involves completely removing an electron from an atom. What wavelength of light contains enough energy in a single photon to ionize a hydrogen atom?
The binding energy of electrons in a metal is 191 kJ/mol. Find the threshold frequency of the metal.
It takes 476 kJ to remove 1 mole of electrons from the atoms at the surface of a solid metal. How much energy (in kJ) does it take to remove a single electron from an atom at the surface of this solid metal?
Find the velocity of an electron emitted by a metal whose threshold frequency is 2.25×1014 s-1 when it is exposed to visible light of wavelength 5.00×10−7 m.
The light emitted from one of the following electronic transitions (n = 4 → n = 3 or n = 3 → n = 2) in the hydrogen atom caused the photoelectric effect in a particular metal while light from the other transition did not. Which transition was able to cause the photoelectric effect?
The light emitted from one of the following electronic transitions (n = 4 → n = 3 or n = 3 → n = 2) in the hydrogen atom caused the photoelectric effect in a particular metal while light from the other transition did not. Why?