Videos
In this chapter, we have learned about the
suppose it is hypothesized that it requires more energy to remove an electron from a metal that has atoms with one or more half-filled shells than from those that do not.
- Design a series of experiments involving the photoelectric effect that would test the hypothesis.
- What experimental apparatus would be needed to test the hypothesis? Its not necessary that you name actual equipment but rather that you imagine how the apparatus would work-think in terms of the types of measurements that would be needed, and what capability you would need in your apparatus.
- Describe the type of data you would collect and how you would analyze the data to see whether the hypothesis were correct.
- Could your experiments be extended to test the hypothesis for other parts of the periodic table, such as the lanthanide or actinide elements?
Interpretation: The experiments, apparatus and the type of data to test the given hypothesis is to be determined.
(a) A series of experiment involving the photoelectric effect that would test the hypothesis needs to be designed.
(b) The experimental apparatus required to test the given hypothesis should be determined.
(c)The type of data required to conclude whether the given hypothesis is correct or not should be determined.
(d) If the given hypothesis can be tested on lanthanides or actinides or not should be identified.
Concept Introduction: The light falls on the surface of the metal and results in the ejection of electron form its surface. This process is known as the photoelectric effect.
Answer to Problem 1DE
Solution: (a) When the light incident on the metal plate having one or more half-filled orbital; one does not observe the collection of electrons on the collector plate. But as the energy increases the electrons started collecting on the collector plate. This proves the given hypothesis.
(b) The experimental apparatus to study the photoelectric effect consists of the metal plate, collector plate, battery and voltmeter.
(c) The plot of stopping potential as a function of frequency is used to conclude that the given hypothesis is correct.
(d) The given hypothesis is not applicable on lanthanides and actinides because of the presence of d and f orbitals.
(a)
Explanation of Solution
The hypothesis says that that it requires more energy to remove an electron from the metal that has one or more half filled shells.
The ejection of electrons from the metal surface is tested by using the photoelectric effect by considering the apparatus consists of the metal plate on which the light is incident and the collector plate on which the electrons get collected. These two plates are connected to the electric circuit consists of battery, photodiode with amplifier and the voltmeter with reverse voltage.
When the light incident on the metal plate having one or more half filled orbital; one does not observed the collection of electrons on the collector plate. But as the energy increases the electrons starting collecting on the collector plate. This proves the given hypothesis.
(b)
Explanation:
The apparatus to study the photoelectric effect has the following parts,
- A photodiode with an amplifier.
- A digital voltmeter with reverse voltage.
- Batteries to operate amplifier and to provide reverse voltage.
- A monochromatic light source.
- The incident light beam intensity must adjust using a neutral filter.
The apparatus for testing the given hypothesis is shown below:
Figure 1
(c)
Explanation:
The data of frequency and wave length of different light source is collected and it is used in the apparatus of photoelectric effect. The different percentage transmission values as the function of intensity will be observed. The plot of stopping potential as a function of frequency will be observed from this data which conclude whether the hypothesis is correct or not.
(d)
Explanation:
The given hypothesis says that more energy is required to eject the electron form a metal having half filled orbitals as compared to those who have not. But the orbital of lanthanides and actinides are diffused in nature and they are larger in size. Therefore, they can easily accept and eject electrons by using lower energy radiation. Therefore, the given hypothesis cannot be tested on the lanthanides and actinides.
- The ejection of electrons is tested by using the apparatus consists of metal plate and collector plate.
- The experimental apparatus to study the photoelectric effect consists of the metal plate, collector plate, battery and voltmeter.
- The plot of stopping potential as a function of frequency is used to conclude that the given hypothesis is correct.
- The given hypothesis is not applicable on lanthanides and actinides because of the presence of d and f orbitals.
Want to see more full solutions like this?
Chapter 6 Solutions
EP CHEMISTRY:CENTRAL SCI.-MOD.MASTERING
Additional Science Textbook Solutions
Chemistry
Principles of Chemistry: A Molecular Approach (3rd Edition)
Chemistry: A Molecular Approach
Chemistry: Structure and Properties (2nd Edition)
Introductory Chemistry (5th Edition) (Standalone Book)
Chemistry & Chemical Reactivity
- Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff, using the spectroscope they invented in 1859. The name came from the Latin caesius ("sky blue") because of the prominent blue line observed for this element at 455.5 nm. Calculate the frequency and energy of a photon of this light.arrow_forwardA metallic element reacts vigorously with water, evolving hydrogen gas. An excited atom of this element has its outer electron in the 3p orbital. When this electron drops to its ground state in the 3s orbital, light is emitted of wavelength 589 nm What is the identity of the element? Explain how you arrived at your answer. What is the color of the emitted light?arrow_forwardWhich of the following sets of quantum numbers correctly represents a 4p orbital? (a) n = 4, = 0, m = 1 (b) n = 4, = 1, m = 0 (c) n = 4, = 2, m = 1 (d) n = 4, = 1, m =2arrow_forward
- It requires 799 kJ of energy to break one mole of carbon-oxygen double bonds in carbon dioxide. What wavelength of light does this correspond to per bond? Is there any transition in the hydrogen atom that has at least this quantity of energy to one photon?arrow_forward• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.arrow_forwardWhat type of electron orbital (i.e., s, p, d, or f) is designated by an electron with quantum numbers (a) n=1,l=0,m l =0(b) n=3,l=2,m l =1? (c) n=4,l=3,m l =3arrow_forward
- Heated lithium atoms emit photons of light with an energy of 2.9611019 J. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the emitted light?arrow_forward6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.arrow_forwardWhat is the maximum number of electrons that can occupy a f subshell (l = 3)?arrow_forward
- According to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.arrow_forwardAlthough no currently known elements contain electrons in g orbitals in the ground state, it is possible that these elements will be found or that electrons in excited states of known elements could being orbitals. For g orbitals, the value of l is 4. What is the lowest value of n for which g orbitals could exist? What are tile possible values of ml? How many electrons could a set of g orbitals hold?arrow_forward6.71 Several excited states of the neon atom are important in the operation of a helium-neon laser. In these excited states, one electron of the neon atom is promoted from the 2p level to a higher energy orbital. An excited neon atom with a 1s22s22p55s1 electron configuration can emit a photon with a wavelength of 3391 nm as it makes a transition to a lower energy state with a 1s22s22p54p1 electron configuration. Other transitions are also possible. If an excited neon atom with a 1s22s22p53p1 electron configuration makes a transition to a lower energy state with a 1s22s22p53p1 electron configuration, it emits a photon with a wavelength of 632.8 nm. Find the wavelength of the photon that would be emitted in a transition from the 1s22s22p54p1 electron configuration to the 1s22s22p53p1 electron configuration. (It should help if you start by drawing an energy-level diagram.)arrow_forward
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning