Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 6, Problem 63E
Thallium was used as a poison in the Agatha Christie mystery story “The Pale Horse.” Thallium has two possible cationic forms, +1 and +3. The +1 compounds are the more stable. Write the electron structure of the +1 cation of thallium.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Thallium was used as a poison in the Agatha Christie mystery story “The Pale Horse.” Thallium has two possible cationic forms, +1 and +3. The +1 compounds are the more stable. Write the electron structure of the +1cation of thallium.
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.
Ionization is the process of removing an electron from an atom. For an atom, X, the first and second ionizations are described by
the following equations.
First ionization: X(g)
X+(g) + e-
Second ionization: X+(g) -
X2+(g) + e-
Consider the ionization of the period 2 elements.
Which element has the highest second ionization energy?
Which element has the lowest second ionization energy?
nitrogen (N)
nitrogen (N)
fluorine (F)
carbon (C)
lithium (Li)
O boron (B)
oxygen (O)
beryllium (Be)
beryllium (Be)
oxygen (O)
boron (B)
fluorine (F)
O carbon (C)
lithium (Li)
neon (Ne)
neon (Ne)
O O O O
O O O O
Chapter 6 Solutions
Chemistry by OpenStax (2015-05-04)
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. An object is subject to two forces that do not point in opposite directions. Is it possible to choose their ...
College Physics: A Strategic Approach (3rd Edition)
Endospore formation is called (a) _____. It is initiated by (b) _____. Formation of a new cell from an endospor...
Microbiology: An Introduction
Microphylls are found in which plant group? (A) lycophytes (B) liverworts (C) ferns (D) hornworts
Campbell Biology (11th Edition)
Your bore cells, muscle cells, and skin cells look different because a. different kinds of genes are present in...
Campbell Essential Biology (7th Edition)
What percentage of Earths land surface do glaciers presently cover? ____________
Applications and Investigations in Earth Science (9th Edition)
1. Why is the quantum-mechanical model of the atom important for understanding chemistry?
Chemistry: Structure and Properties (2nd 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_forwardFluoride ion, F, has no unpaired electrons. Vanadium forms four binary fluoridesVF2, VF3, VF4, and VF5. Assume that all four are ionic compounds. (a) Which fluoride is diamagnetic? (b) Which fluoride has the greatest attraction to a magnetic field? (c) Which fluoride has two unpaired electrons per vanadium?arrow_forwardConsider the eight most abundant elements in the human body, as outlined in Exercise 156. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?arrow_forward
- Palladium, 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_forwardBoth the electron affinity and the ionization energy of chlorine are higher than the corresponding quantities for sulfur. Explain why in terms of the electronic structure of the atoms.arrow_forwardThe electron configuration of a chlorine atomis [Ne]3 s 2 3 p 5 . When it gains an electron and becomesan ion, its electron configuration changes to [Ne]3 s 2 3 p 6 ,or [Ar], the electron configuration for argon. Has thechlorine atom changed to an argon atom? Explain.arrow_forward
- Arrange the following ions in order of decreasing ionization energy: Sr2+, Se2-, Rb+, Br 1A 7A 8A H 2A I Metals Each element has a name and a ЗА 4А 5A 6А Н Не IMetalloids symbol. Notice that only the first letter of an element's symbol is capitalized - cobalt is Co, not CO. Chemists have arranged the elements in a table that depicts the symbols for the elements along with other information. This is called the periodic table. LI Be INonmetals BCNOF Ne Na Mg 38 4B 5B 6B 7B 8B ¬ 1B 2B Al Si P S CI Ar K Ca Sc TI v Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg TI Pb Bi Po At Rn Fr Ra Ac RE Db Lanthanides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Actinides Th Pa U Np Pu Am Cm Bk cf Es Fm Md No Lr Decreasing ionization energy Drag and drop your selection from the following list to complete the answer: Br Sr2+ Se2- Rb+ Submit Answer Try Another Version 1 item attempt remainingarrow_forwardA ceramic plate has a shiny rim. The ceramic plate is mostly composed of silicon and oxygen atoms. The shiny rim is mostly silver. When the plate is heated in a microwave oven, sparks are observed. Compare the ionization energy values of silver to those of the silicon and oxygen atoms. Explain what is happening in the oven. Why are microwaveable containers usually non-metallic? Why are most pots and pans metallic?arrow_forwardA group of students at College of the Canyons conducted an experiment. Two reactors contained different reagents. Reactor 1: sodium metal + argon gas Reactor 2: sodium metal + chlorine gas When the reactor was heated, reactor 1 did not show a chemical reaction between the sodium metal and argon gas. However, reactor 2 showed a vigorous reaction between sodium metal and chlorine gas to form sodium chloride at the same reaction condition. A) Write the electron configurations (noble-gas core notation) each for argon and chlorine atom. Ar: ____________________ Cl: _____________________ B) Explain the difference in the reactivity of the gases with sodium metal. Hint: Use the electron configurations in A).arrow_forward
- Atoms of Group 1 elements have the lowest first ionization energy of all the elements on the periodic table but subsequently have the largest increase between the first and second ionization energy that any other elements have. Explain why this is the case, based on the electronic structure of the atoms/ions.arrow_forwardPlease solve all questions, including the subparts. What trend in first ionization energy occurs as you go up a group on the periodic table? Explain why this occurs. What trend in atomic radius occurs as you go up a group on the periodic table? Explain why this occurs. Arrange the following in order of increasing electronegativity: Br, F, I, Cl Write four quantum numbers to describe the highest energy electron in the magnesium atom. Be sure to include the four symbols and four correct numbers. Arrange the following in order of increasing first ionization energy: Br, F, I, Clarrow_forwardWhat is the key distinction between sublevel energies in one-electron species, such as the H atom, and those in many- electron species, such as the C atom? What factors lead to this distinction? Would you expect the pattern of sublevel energies in Be3+ to be more like that in H or that in C? Explainarrow_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: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher: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: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Periodic Properties of Elements | Chemistry | IIT-JEE | NEET | CBSE | Misostudy; Author: Misostudy;https://www.youtube.com/watch?v=L26rRWz4_AI;License: Standard YouTube License, CC-BY
Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius - TUTOR HOTLINE; Author: Melissa Maribel;https://www.youtube.com/watch?v=0h8q1GIQ-H4;License: Standard YouTube License, CC-BY