New Semester Started Get 50% OFF Study Help! --h --m --s Claim Now

Question Answers

Textbooks

Find textbooks, questions and answers

Oops, something went wrong!

Change your search query and then try again

Result Not Found

Books FREE
Study Help
Tutors
AI Study Planner NEW
Sell Books

Search
Sign In
Register

study help
sciences
chemical principles

Chemical Principles The Quest For Insight 7th Edition Peter Atkins, Loretta Jones, Leroy Laverman - Solutions

Suppose you are developing a radiation detector to be used on a spacecraft and decide to use a thin layer of metallic potassium to detect certain ranges of electromagnetic radiation. You need to make some estimates of the physical properties involved. The speed of an electron emitted from the
From the following list of observations, select the one that best supports the idea that particles have wave properties. Explain your reasoning.(a) Scattering of a particles by gold foil.(b) Electron diffraction.(c) Cathode rays.(d) The photoelectric effect.
Which ion of each of the following pairs has the larger radius:(a) Ga3+, In3+;(b) P3– , S2–;(c) Pb2+, Pb4+?
(a) Write an expression for the total coulombic potential energy for a beryllium atom.(b) If Z denotes the number of electrons present in an atom, write a general expression to represent the total number of terms that will be present in the total coulombic potential energy expression.
Which of the following statements about the electromagnetic spectrum is true? Explain your reasoning.(a) X-rays travel faster than infrared radiation because they have higher energy.(b) The wavelength of visible radiation decreases as its color changes from blue to green.(c) The frequency of
Refer to Exercise 1C.3. If one side of the box is twice that of the other, the energy levels are given by (n12 / L12 + n22 / L22) * h2/8 m.Can any of these levels have identical energies? If so, find the values of the quantum numbers n1 and n2 for the lowest levels having identical
In one trial on Millikan’s oil drop experiment, each droplet observed by technicians contained an even number of electrons. If the technicians were unaware of this limitation, how would it affect their report of the charge of an electron?
Now suppose you were de Broglie and you had just devised your formula. A friend points out that the world obviously isn’t wavelike. Maybe you should check whether your formula has worrying consequences for everyday objects. Calculate the wavelength of a particle of mass 1 g traveling at 1
The γ-ray photons emitted by the nuclear decay of a technetium- 99 atom used in radiopharmaceuticals have an energy of 140.511 keV. Calculate the wavelength of these γ-rays.
Which member of each pair has the smaller first ionization energy:(a) Ca or Mg;(b) Mg or Na;(c) Al or Na?
Which of the following statements are true for many-electron atoms? If false, explain why.(a) The effective nuclear charge Zeffe is independent of the number of electrons present in an atom.(b) Electrons in an s-orbital are more effective than those in other orbitals at shielding other electrons
Arrange the following types of photons of electromagnetic radiation in order of increasing energy: γ -rays, visible light, ultraviolet radiation, microwaves, x-rays.
(a) Use the Living Graphs on the Web site for this book to plot the particle-in-a-box wavefunction for n = 2 and L = 1 m. (b) How many nodes does the wavefunction have? Where do these nodes occur? (c) Repeat parts (a) and (b) for n = 3. (d) What general conclusion can you draw about the relation
Wavefunctions corresponding to states of different energy of a particle in a box are mutually “orthogonal” in the sense that, if the two wavefunctions are multiplied together and then integrated over the length of the box, the outcome is zero.(a) Confirm that the wavefunctions for n = 1 and n
Some lasers work by exciting atoms of one element and letting these excited atoms collide with atoms of another element and transfer their excitation energy to those atoms. The transfer is most efficient when the separation of energy levels matches in the two species. Given the information in
For each of the following ground-state atoms, predict the type of orbital (1s, 2p, 3d, 4f, etc.) from which an electron will be removed to form the 1 1 ion:(a) Zn;(b) Cl;(c) Al;(d) Cu.
Below is pictured the reaction between an atom of magnesium and an atom of oxygen. Identify each element and the ions formed and explain your reasoning. A B C D
Neon lights glow with orange light and they also emit radiation of wavelength 865 nm. Calculate the energy change resulting from the emission of 1.00 mol of photons at this wavelength.
Which member of each pair is likely to have the smaller second ionization energy:(a) Ca or Mg;(b) Mg or Na;(c) Al or Na?
For the electrons on a carbon atom in the ground state, decide which of the following statements are true. If false, explain why.(a) Zeffe for an electron in a 1s-orbital is the same as Zeffe for an electron in a 2s-orbital.(b) Zeffe for an electron in a 2s-orbital is the same as Zeffe for an
Arrange the following types of photons of electromagnetic radiation in order of increasing frequency: visible light, radio waves, ultraviolet radiation, infrared radiation.
Verify the conclusion in part (d) of Exercise 1C.5 by plotting the wavefunction for n = 4 and determining the number of nodes.Exercise 1C.5 part (d)(d) What general conclusion can you draw about the relation between n and the number of nodes present in a wavefunction?
Wavefunctions are “normalized” to 1. This term means that the total probability of finding an electron in the system is 1. Verify this statement for a particle-in-the-box wavefunction.
Determine whether each of the following electron configurations represents the ground state or an excited state of the atom given. (a) C (c) Be 1s 2s 1s 2s 2p 2p (b) N 1s 2s (d) ON N 1s 2s 2p 2p
Sodium vapor lamps, used for public lighting, emit yellow light of wavelength 589 nm. How much energy is emitted by(a) An excited sodium atom when it generates a photon;(b) 5.00 mg of sodium atoms emitting light at this wavelength;(c) 1.00 mol of sodium atoms emitting light at this wavelength?
Place each of the following sets of elements in order of decreasing ionization energy. Explain your choices.(a) Selenium, oxygen, tellurium;(b) gold, tantalum, osmium;(c) lead, barium, cesium.
The wavefunction for a particle in a one- dimensional box is given in Eq. 2. Confirm that the probability of finding the particle in the left half of the box is 1/2 regardless of the value of n. 1/2 n(x) = (*) - (²) * sin(x) n = 1, 2, ... (2)
(a) The frequency of violet light is 7.1 * 1014 Hz. What is the wavelength (in nanometers) of violet light?(b) When an electron beam strikes a block of copper, x-rays with a frequency of 2.0 * 1018 Hz are emitted. What is the wavelength (in picometers) of these x-rays?
The intensity of a transition between the states n and n′ of a particle in a box is proportional to the square of the integral μnn′ where(a) Can there be a transition between states with quantum numbers 3 and 1?(b) Consider the transition between states with quantum numbers 2 and 1. Does
(a) Generally, the first ionization energies of elements in the same period increase upon going to higher atomic number. Why?(b) Examine the data for the p-block elements given in Fig. 1F.9. Note any exceptions to the rule given in part (a). How are these exceptions explained? Ionization energy,
When an electron beam strikes a block of copper, x-rays with a frequency of 1.2 * 1017 Hz are emitted. How much energy is emitted at this wavelength by(a) An excited copper atom when it generates an x-ray photon;(b) 2.00 mol of excited copper atoms;(c) 2.00 g of copper atoms?
Each of the following valence-shell configurations is possible for a neutral atom of a certain element. What is the element and which configuration represents the ground state? (a) N 4s (c) 4s 4p 4p (b) N 4s (d) 4s 4p 4p
The wavefunction for a particle in a one- dimensional box is given in Eq. 2. Does the probability of finding the particle in the left-hand one-third of the box depend on n ? If so, find the probability. 1/2 n(x) = (*) - (²) * sin(x) n = 1, 2, ... (2)
(a) Radio waves for the FM station “Rock 99 at 99.3 on the FM dial” are generated at 99.3 MHz. What is the wavelength of this station?(b) Radioastronomers use 1420.-MHz waves to look at interstellar clouds of hydrogen atoms. What is the wavelength of this radiation?
The first and second ionization energies of phosphorus, sulfur, and chlorine atoms are listed in the following table. Explain why the first ionization energies of phosphorus and sulfur are nearly the same, whereas the second ionization energy of sulfur is much greater than that of phosphorus.
Millikan measured the charge of the electron in electrostatic units, esu. The data that he collected included the following series of charges found on oil drops: 9.60 * 10-10 esu, 1.92 * 10-9 esu, 2.40 * 10-9 esu, 2.88 * 10-9 esu, and 4.80 * 10-9 esu. (a) From this series, find the likely charge
A lamp rated at 32 W (1 W = 1 J·s–1) emits violet light of wavelength 420 nm. How many photons of violet light can the lamp generate in 2.0 s? How many moles of photons are emitted in that time interval?
Of the following sets of four quantum numbers {n , l, ml, ms}, identify the ones that are forbidden for an electron in an atom and explain why they are invalid: (a) {4, 2, −1, +}; (b) {5,0,−1, +¹}; (c) {4, 4, − 1, +¹}.
A college student recently had a busy day. Each of the student’s activities on that day (reading, getting a dental x-ray, making popcorn in a microwave oven, and acquiring a suntan) involved radiation from a different part of the electromagnetic spectrum. Complete the following table and match
The first and second ionization energies of phosphorus, sulfur, and chlorine atoms are listed in the table in Exercise 1F.9.Explain why the first ionization energy of chlorine is much greater than that of sulfur, whereas their second ionization energies are nearly the same.Exercise 1F.9The first
An electron in a hydrogen atom is excited to a 2px-orbital. What is the probability that the electron will be found in the region of space for which the wavefunction has a positive sign?
Of the following sets of four quantum numbers { n, l, ml, ms}, identify the ones that are forbidden for an electron in an atom and explain why they are invalid: (a) {2, 2, − 1, +¹}; (b) {6, 6, 0, +½}; (c) {5, 4, +5, +1}.
A lamp rated at 40. W (1 W = 1 J·s–1) emits blue light of wavelength 470 nm. How many photons of blue light can the lamp generate in 2.0 s? How many moles of photons are emitted in that time interval?
A college student encountered a variety of types of electromagnetic radiation when going to a restaurant for lunch (watching a red traffic light change, listening to the car radio, being struck by a stray γ -ray from outer space while entering the restaurant, and taking food from a serving table
In the f-block there are numerous exceptions to the regular order of orbital occupation predicted by the building-up principle.Suggest why so many exceptions are noted for these elements.
Which element of each of the following pairs has the higher electron affinity:(a) Tellurium or iodine;(b) Beryllium or magnesium;(c) Oxygen or sulfur;(d) Gallium or indium?
The star Antares emits light with maximum intensity at 850 nm. What is the temperature at the surface of Antares?
In the spectrum of atomic hydrogen, several lines are generally classified together as belonging to a series (for example, Balmer series or Lyman series, as shown in Fig. 1A.10). What is common to the lines within a series that makes grouping them together logical?
Write the ground-state electron configuration for each of the following atoms:(a) Sodium;(b) Silicon;(c) Chlorine;(d) Rubidium.
Photoelectron spectroscopy can be used to determine the energies of atomic orbitals by measuring the energies required to remove electrons from them. The following peaks were observed in the photoelectron spectra for two elements.Identify the elements, write their electron configurations, and
Which element of each of the following pairs has the higher electron affinity:(a) Germanium or selenium;(b) Boron or carbon;(c) Phosphorus or arsenic?
The very hot star Spica has a surface temperature of 23 kK (2.3 * 104 K). At what wavelength does Spica emit the maximum intensity of light?
The following peaks were observed in the photoelectron spectra for two elements (see Exercise 1.11). Identify the elements, write their electron configurations, and explain your reasoning:Exercise 1.11Photoelectron spectroscopy can be used to determine the energies of atomic orbitals by measuring
Write the ground-state electron configuration for each of the following atoms:(a) Titanium;(b) Chromium;(c) Europium;(d) Krypton.
(a) What is the inert-pair effect?(b) Why is the inert-pair effect observed only for heavy elements?
(a) Use the Rydberg formula for atomic hydrogen to calculate the wavelength of radiation generated by the transition from n = 2 to n = 1. (b) What is the name given to the spectroscopic series to which this transition belongs?(c) Use Table 1A.1 to determine the region of the spectrum in which
The temperature of molten iron can be estimated by using Wien’s law. If the melting point of iron is 1540°C, what will be the wavelength (in nanometers) corresponding to maximum intensity when a piece of iron melts? In what region of the electromagnetic spectrum is this light?
Write the ground-state electron configuration for each of the following atoms:(a) Silver;(b) Beryllium;(c) Antimony;(d) Gallium;(e) Tungsten;(f) Iodine.
Ionization energies usually increase on going from left to right across the periodic table. The ionization energy for oxygen, however, is lower than that of either nitrogen or fluorine. Explain this anomaly.
Identify which of the following elements experience the inert-pair effect and write the formulas for the ions that they form:(a) Sb;(b) As;(c) Tl;(d) Ba.
An astronomer discovers a new red star that emits light with maximum intensity at 632 nm. What is the temperature at the surface of the star?
(a) Use the Rydberg formula for atomic hydrogen to calculate the wavelength for the transition from n = 3 to n = 1. (b) What is the name given to the spectroscopic series to which this transition belongs?(c) Use Table 1A.1 to determine the region of the spectrum in which the transition takes
Write the ground-state electron configuration for each of the following atoms:(a) Germanium;(b) Cesium;(c) Iridium;(d) Tellurium;(e) Thallium;(f) Plutonium.
Thallium is the heaviest stable member of Group 13. Aluminum is also a member of that group, and its chemical properties are dominated by the 13 oxidation state. Thallium, however, is found most usually in the 11 oxidation state. Examine this difference by plotting the first, second, and third
The German physicist Lothar Meyer observed a periodicity in the physical properties of the elements at about the same time that Mendeleev was working on their chemical properties. Some of Meyer’s observations can be reproduced by examining the molar volume for the solid element as a function of
(a) What is a diagonal relationship?(b) How does it arise?(c) Give two examples to illustrate the concept.
Use Appendix 2D to find the values for the atomic radii of germanium and antimony, as well as the ionic radii for Ge2+ and Sb3+. What do these values suggest about the chemical properties of these two ions?Appendix 2D Element actinium (Greek aktis, ray) aluminum (from alum, salts of the form KAI
The velocity of an electron that is emitted from a metallic surface by a photon is 3.6 * 103 km·s–1.(a) What is the wavelength of the ejected electron?(b) No electrons are emitted from the surface of the metal until the frequency of the radiation reaches 2.50 * 1016 Hz. How much energy is
Which elements are predicted to have the following ground-state electron configurations of their atoms:(a) [Kr]4d10 5s2 5p4;(b) [Ar]3d3 4s2;(c) [He]2s2 2p2;(d) [Rn]7s2 6d2?
In the ultraviolet spectrum of atomic hydrogen, a line is observed at 102.6 nm. Determine the values of n for the initial and final energy levels of the electron during the emission of energy that leads to this spectral line.
What are the principal and orbital angular momentum quantum numbers for each of the following orbitals:(a) 3s;(b) 4p;(c) 5d;(d) 6f?
The work function for chromium metal is 4.37 eV. What wavelength of radiation must be used to eject electrons with a velocity of 1.5 * 103 km·s–1?
Which elements are predicted to have the following ground-state electron configurations of their atoms:(a) [Ar]3d10 4s2 4p1;(b) [Ne]3s1;(c) [Kr]5s2;(d) [Xe]4f7 6s2?
A violet line is observed at 434 nm in the spectrum of atomic hydrogen. Determine the values of n for the beginning and ending energy levels of the electron during the emission of energy that leads to this spectral line.
In the spectroscopic technique known as photoelectron spectroscopy (PES), ultraviolet radiation is directed at an atom or a molecule. Electrons are ejected from the valence shell, and their kinetic energies are measured. Because the energy of the incoming ultraviolet photon is known and the kinetic
For each orbital listed in Exercise 1D.15, give the possible values of the magnetic quantum number.Exercise 1D.15What are the principal and orbital angular momentum quantum numbers for each of the following orbitals:(a) 6p;(b) 3d;(c) 2p;(d) 5f?
Which of the following pairs of elements exhibit a diagonal relationship:(a) Li and Mg;(b) Ca and Al;(c) F and S?
Who has the shorter wavelength when running at the same speed: a person weighing 60 kg or a person weighing 80 kg? Explain your reasoning.
For each of the following ground-state atoms, predict the type of orbital (1s, 2p, 3d, 4f, etc.) from which an electron will be removed to form the + 1 ion:(a) Ge;(b) Mn;(c) Ba;(d) Au.
The energy levels of hydrogenlike one-electron ions of atomic number Z differ from those of hydrogen by a factor of Z2.Predict the wavelength of the transition from n = 2 to n = 1 in He+.
Apparent anomalies in the filling of electron orbitals in atoms occur in chromium and copper. In these elements an electron expected to occupy an s-orbital occupies a d-orbital instead.(a) Explain why these anomalies occur.(b) Similar anomalies are known to occur in seven other elements of the
For each orbital listed in Exercise 1D.16, give the possible values of the magnetic quantum number.Exercise 1D.16What are the principal and orbital angular momentum quantum numbers for each of the following orbitals:(a) 3s;(b) 4p;(c) 5d;(d) 6f?
Which of the following pairs of elements do not exhibit a diagonal relationship:(a) Be and Al;(b) As and Sn;(c) Ga and Sn?
(a) Calculate the wavelength of a hydrogen atom traveling at 10. m· s–1.(b) What would cause the wavelength of the atom to decrease, accelerating the atom to higher speeds or slowing it down? Explain your reasoning.
The electron in a hydrogen atom is excited to a 4d-orbital. Calculate the energy of the photon released if the electron were then to move to each of the following orbitals:(a) 1s;(b) 2p;(c) 2s;(d) 4s.(e) If the outermost electron in a potassium atom were excited to a 4d-orbital and then fell
How many orbitals are present in the(a) 4p-subshell;(b) 3d-subshell;(c) 1s-subshell;(d) 4f-subshell of an atom?
Why are s-block metals typically more reactive than p-block metals?
Protons and neutrons have nearly the same mass. How different are their wavelengths? Calculate the wavelength of each particle when traveling at 2.75 * 105 m· s–1 in a particle accelerator and report the difference as a percentage of the wavelength of the neutron.
Predict the number of valence electrons present in each of the following atoms (include the outermost d-electrons):(a) N;(b) Ag;(c) Nb;(d) W.
The following properties are observed for an unknown element. Identify the element from its properties.(a) The neutral atom has two unpaired electrons with l = 2. (b) The previous noble gas in the periodic table is krypton.
How many orbitals are present in a subshell with l =(a) 0;(b) 1;(c) 2;(d) 3?
Which of the following elements are transition metals:(a) Radium;(b) Radon;(c) Hafnium;(d) Niobium;(e) Cadmium?
What is the wavelength of an electron when the distance it travels in 1 s is equal to its wavelength?
Predict the number of valence electrons present in each of the following atoms (include the outermost d-electrons):(a) N;(b) Ag;(c) Nb;(d) W.
The electron affinity of thulium has been measured by a technique called laser photodetachment electron spectroscopy. In this technique a gaseous beam of the anions of an element is bombarded with photons from a laser. The photons eject electrons from some of the anions and the energies of the
Write the subshell notation (3d, for instance) and the number of orbitals having the following quantum numbers:(a) n = 5, l = 2;(b) n = 1, l = 0;(c) n = 6, l = 3;(d) n = 2, l = 1.
Identify the following elements as metals, nonmetals, or metalloids:(a) Lead;(b) Sulfur;(c) Zinc;(d) Silicon;(e) Antimony;(f) Cadmium.
A baseball must weigh between 5.00 and 5.25 ounces (1 ounce = 28.3 g). What is the wavelength of a 5.15-ounce baseball thrown at 92 mph?
How many unpaired electrons are predicted for the ground-state configuration of each of the following atoms:(a) Bi;(b) Si;(c) Ta;(d) Ni?
Francium is thought to be the most reactive of the alkali metals. Because it is radioactive and available in only very small amounts, it is difficult to study. However, its properties can be predicted based on its location in Group 1 of the periodic table.Estimate the following properties of

Showing 2400 - 2500 of 3011

First
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31

Step by Step Answers

Services

Sitemap
Fun
Definitions
Become Tutor
Used Textbooks
Study Help Categories
Recent Questions
Expert Questions
Campus Wear
Sell Your Books

Company Info

Security
Copyrights
Privacy Policy
Terms & Conditions
SolutionInn Fee
Scholarship
Online Quiz
Give Feedback, Get Rewards

Get In Touch

About Us
Contact Us
Career
Jobs
FAQ
Student Discount
Campus Ambassador

Secure Payment

Download Our App

© 2026 SolutionInn. All Rights Reserved