CHEMISTRY
2nd Edition
ISBN: 9781593995782
Author: OpenStax
Publisher: XANEDU PUBLISHING
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 6, Problem 82E
Of the five elements Al, Cl, I, Na, Rb, which has the most exothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? Hint: note the process depicted does not correspond to
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Which of the following reactions represents an electron gain energy that would be positive (i.e. endothermic).
S(g) → S+(g) + e-
Cl(g) → Cl+(g) + e-
Kr(g) + e- → Kr-(g)
S(g) + e- → S-(g)
Kr(g) → Kr+(g)+ e-
Cl(g) + e- →Cl-(g)
(ii) Draw the Born-Haber cycle and use the data below for the formation of calcium chloride, to
calculate the electron affinity of chlorine:
Ca(s)
→ Ca(g)
AHat = +190 kJ/mol
Ca(g)
> Caz*(g) + 2e¨ AH¡ɛ = +1730 kJ/mol
Cl2{g)
2C1(g)
AHat = +121 kJ/mol
Caz (g) + 2Cl(g)
> CaCl2(s)
AHLE = -2184 kJ/mol
Ca(s) + Cl2(g) –> CaCl2(s) AH; = -795 kJ/mol
Of the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? E(g) ⟶ E+(g) + e−
Chapter 6 Solutions
CHEMISTRY
Ch. 6 - The light produced by a red neon sign is due to...Ch. 6 - An FM radio station found at 103.1 on the FM dial...Ch. 6 - FM-95, an FM radio station, broadcasts at a...Ch. 6 - A bright violet line occurs at 435.8 nm in the...Ch. 6 - Light with a wavelength of 614.5 nm looks orange....Ch. 6 - Heated lithium atoms emit photons of light with an...Ch. 6 - A photon of light produced by a surgical laser has...Ch. 6 - When rubidium ions are heated to a high...Ch. 6 - The emission spectrum of cesium contains two lines...Ch. 6 - Photons of infrared radiation are responsible for...
Ch. 6 - One of the radiographic devices used in a...Ch. 6 - The eyes of certain reptiles pass a single visual...Ch. 6 - RGB color television and computer displays use...Ch. 6 - Answer the following questions about a Blu-ray...Ch. 6 - What is the threshold frequency for sodium metal...Ch. 6 - Why is the electron in a Bohr hydrogen atom bound...Ch. 6 - What does it mean to say that the energy of the...Ch. 6 - Using the Bohr model, determine the energy, in...Ch. 6 - The electron volt (eV) is a convenient unit of...Ch. 6 - Using the Bohr model, determine the lowest...Ch. 6 - Using the Bohr model, determine the lowest...Ch. 6 - Using the Bohr model, determine the energy of an...Ch. 6 - Using the Bohr model, determine the energy of an...Ch. 6 - How far from the nucleus in angstroms (1 angstrom...Ch. 6 - What is the radius, in angstroms, of the orbital...Ch. 6 - Using the Bohr model, determine the energy in...Ch. 6 - Using the Bohr model, determine the energy in...Ch. 6 - Consider a large number of hydrogen atoms with...Ch. 6 - How are the Bohr model and the Rutherford model of...Ch. 6 - The spectra of hydrogen and of calcium are shown...Ch. 6 - How are the Bohr model and the quantum mechanical...Ch. 6 - What are the allowed values for each of the four...Ch. 6 - Describe the properties of an electron associated...Ch. 6 - Answer the following questions: (a) Without using...Ch. 6 - Identify the subshell in which electrons with the...Ch. 6 - Which of the subshells described in the previous...Ch. 6 - Identify the subshell in which electrons with the...Ch. 6 - Which of the subshells described in the previous...Ch. 6 - Sketch the boundary surface of a dx2y2 and a py...Ch. 6 - Sketch the px and dxz orbitals. Be sure to show...Ch. 6 - Consider the orbitals shown here in outline. (a)...Ch. 6 - State the Heisenberg uncertainty principle....Ch. 6 - How many electrons could be held in the second...Ch. 6 - Which of the following equations describe...Ch. 6 - Write a set of quantum numbers for each of the...Ch. 6 - Read the labels of several commercial products and...Ch. 6 - Read the labels of several commercial products and...Ch. 6 - Using complete subshell notation (not...Ch. 6 - Using complete subshell notation ( 1s22s22p6, and...Ch. 6 - Is 1s22s22p6 the symbol for a macroscopic property...Ch. 6 - What additional information do we need to answer...Ch. 6 - Draw the orbital diagram for the valence shell of...Ch. 6 - Use an orbital diagram to describe the electron...Ch. 6 - Using complete subshell notation ( 1s22s22p6, and...Ch. 6 - Which atom has the electron configuration...Ch. 6 - Which atom has the electron configuration...Ch. 6 - Which ion with a +1 charge has the electron...Ch. 6 - Which of the following atoms contains only three...Ch. 6 - Which of the following has two unpaired electrons?...Ch. 6 - Which atom would be expected to have a half-filled...Ch. 6 - Which atom would be expected to have a half-filled...Ch. 6 - In one area of Australia, the cattle did not...Ch. 6 - Thallium was used as a poison in the Agatha...Ch. 6 - Write the electron configurations for the...Ch. 6 - Cobalt60 and iodine131 are radioactive isotopes...Ch. 6 - Write a set of quantum numbers for each of the...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Atoms of which group in the periodic table have a...Ch. 6 - Atoms of which group in the periodic table have a...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - Based on their positions in the periodic table,...Ch. 6 - List the following ions in order of increasing...Ch. 6 - Which atom and/or ion is (are) isoelectronic with...Ch. 6 - Which of the following atoms and ions is (are)...Ch. 6 - Compare both the numbers of protons and electrons...Ch. 6 - Of the five elements Al, Cl, I, Na, Rb, which has...Ch. 6 - Of the five elements Sn, Si, Sb, O, Te, which has...Ch. 6 - The ionic radii of the ions S2, Cl, and K+ are...Ch. 6 - Which main group atom would be expected to have...Ch. 6 - Explain why Al is a member of group 13 rather than...
Additional Science Textbook Solutions
Find more solutions based on key concepts
1. a. Can a vector have nonzero magnitude if a component is zero? If no, why not? If yes, give an example.
b. C...
College Physics: A Strategic Approach (3rd Edition)
1. Why is the quantum-mechanical model of the atom important for understanding chemistry?
Chemistry: Structure and Properties (2nd Edition)
Match the following examples of mutagens. Column A Column B ___a. A mutagen that is incorporated into DNA in pl...
Microbiology: An Introduction
Q1. Which change is likely to increase the rate of reaction in a reaction mixture?
a. decreasing the temperatur...
Introductory Chemistry (6th Edition)
A wild-type fruit fly (heterozygous for gray body color and led eyes) is mated Willi a black fruit fly wltli pu...
Campbell Biology (11th Edition)
4. What five specific threats to biodiversity are described in this chapter? Provide an example of each.
Biology: Life on Earth (11th Edition)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- In one area of Australia, the cattle did not thrive despite the presence of suitable forage. An investigation showed the cause to be the absence of sufficient cobalt in the soil. Cobalt forms cations in two oxidation states, Co2 and Co3+. Write the electron structure of the two cations.arrow_forwardWhat is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forwardPalladium, with an electron configuration of [Kr] 4d10, is an exception to the aufbau principle. Write the electron configuration of the 2+ cation of palladium. Does the fact that palladium is an exception influence the electron configuration of Pd2+?arrow_forward
- (a) Rank elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization energy, and (iii) reactivity. (b) Explain why atomic size decreases from left to right, but increases from top to bottom; (c) Explain why ionization energy increases from left to right, but decreases from top to bottom; (d) Explain why the reactivity of alkali metals (Group-1) increases from top to bottom, where as the reactivity of halogen (Group-17) decreases from top to bottom.arrow_forwardThe following equations represent the chemical process to determine electron affinity of atoms. Identify the process expected to be the most exothermic (that releases the most energy). (A) F(g) + e– --> F– (g); (B) Cl(g) + e– --> Cl–(g); (C) Br(g) + e– --> Br–(g) ; (D) I(g) + e– --> I–(g);arrow_forwardIn the hydrogen atom, the electron is in its lowest energy state, n=1. The maximum electron energy that a hydrogen atom can have is 0 kJ/mole, at which point the electron would essentially be removed from the atom and it would become a H+ ion. How much energy does it take to ionize one hydrogen atom in kilojoules per mole and in Joules per atom? (Hint: calculate ΔE where εfinal is zero and εinitial is –1312.04 kJ/mol.)arrow_forward
- Quesion 10- (Please showall of your work so I can understand going forward) You may need to use a special periodic table to answer the question, it is attached in the images below. You will also need to look at the images to see the figure for the dot sturcture. a) Draw the electron dot structure for Fa. c) Would nitrogen have a larger or smaller ionization energy compared to Fa? (Please explain your answer)arrow_forward1.) Which element would have the lowest ionization energy? S, Ge, Al, Ca, Rb 2.) Which equation below illustrates the second ionization energy for sodium A) Na (g) + 2e– → Na–2 (g) B) Na (g) → Na+2 (g) + 2e– C) Na+ (g) →Na+2(g) + e– D) Na+2 (g) + 2e– → Na (g) E) Na (g) → Na+ (g) + e– F) Na (g) + e– → Na– (g)arrow_forwardWhat is the kinetic energy of the emitted electrons when cesium is exposed to UV rays of frequency 1.90×1015Hz? Express your answer in joules to three significant figures. It is not 9.17×10−19 J or 12.589 x 10-19 J By using the following formula, you can calculate the kinetic energy of the emitted electron: KE=E−ϕ=hν−hν0 where h=6.63×10−34 J⋅s is Planck's constant, ν=1.90×1015Hz is the given frequency, and ν0=9.39×1014 Hz is your answer from Part A. The threshold frequency ν0 of cesium is 9.39×1014 Hzarrow_forward
- 1.) Which element would have the least favorable favorable (least negative) electron affinity? S, Si, Al, Cl 2.) Which equation below illustrates the first electron affinity for gallium?arrow_forwardUse the following data and the Born-Haber cycle to calculate the first ionization energy (ΔH IE1) of K(g) K(s) → K(g) 89 kJ mol-1 Cl(g) + e– → Cl–(g) -349 kJ mol-1 K(s) + ½ Cl2(g) → KCl(s) -437 kJ mol-1 K(g) → K+(g) + e– ΔH IE1 Cl2(g) → 2Cl(g) 244 kJ mol-1 K+(g) + Cl–(g) → KCl(s) -717 kJ mol-1 Use the bond energies listed in the table below to estimate the standard enthalpy of the reaction: CCl3CHCl2(g) + 2HF(g) → CCl3CHF2(g) + 2HCl(g) C – H 412 kJ mol-1 C – C 348 kJ mol-1 C – Cl 338 kJ mol-1 H – Cl 431 kJ mol-1 C – F 484 kJ mol-1 H – F 565 kJ mol-1arrow_forwardWhich equation below depicts the reaction from which the first ionization energy would be determined? Ca(s) + e- → Ca-(g) O Ca(s) → Ca+(g) + e- none of these O Ca(g) → Ca+(g) + e- Ca(g) → Ca2+ + e-arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Lanthanoids and its Position in Periodic Table - D and F Block Elements - Chemistry Class 12; Author: Ekeeda;https://www.youtube.com/watch?v=ZM04kRxm6tY;License: Standard YouTube License, CC-BY