Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 22, Problem 83GQ
Cerium, as noted in Applying Chemical Principles: 22.3 The Rare Earths, is a relatively abundant lanthanide element that has some important uses. Cerium(IV) oxide. CeO2, is widely used as a polishing agent for glass. Cerium(III) sulfide, Ce2S3, is becoming more widely used as a red pigment to replace cadmium pigments, which are environmentally less desirable.
(a) Give the electron configurations (using the noble gas notation) for Ce, Ce3+, and Ce4+.
(b) Is either Ce3+ or Ce4+ paramagnetic? If so, how many unpaired electrons does each have?
(c) The solid state structure for CeO2 is shown below. Describe the unit cell of the compound. How is this structure related to the formula?
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Chapter 22 Solutions
Chemistry & Chemical Reactivity
Ch. 22.4 - (a) What is the formula of a complex ion composed...Ch. 22.4 - (a) Determine the metals oxidation number and...Ch. 22.4 - Name the following coordination compounds. (a)...Ch. 22.5 - What types of isomers are possible for the...Ch. 22.6 - Prob. 22.5CYUCh. 22.7 - Prob. 22.6CYUCh. 22.7 - Prob. 1.1ACPCh. 22.7 - Copper has a face-centered cubic unit cell. If...Ch. 22.7 - Prob. 1.3ACPCh. 22.7 - If a patient is given 10.0 mg of cisplatin, what...
Ch. 22.7 - Prob. 2.2ACPCh. 22.7 - How are the d electrons of Pt distributed in a...Ch. 22.7 - What are the electron configurations for Nd and...Ch. 22.7 - Prob. 3.2ACPCh. 22.7 - Prob. 3.3ACPCh. 22.7 - Prob. 3.4ACPCh. 22 - Identify, based on the position in the periodic...Ch. 22 - Prob. 2PSCh. 22 - Prob. 3PSCh. 22 - Prob. 4PSCh. 22 - Prob. 5PSCh. 22 - Iron is the most abundant transition element in...Ch. 22 - Prob. 7PSCh. 22 - Prob. 8PSCh. 22 - Prob. 9PSCh. 22 - Prob. 10PSCh. 22 - Identify a cation of a first series transition...Ch. 22 - Match up the isoelectronic ions on the following...Ch. 22 - The lanthanide contraction is given as an...Ch. 22 - Prob. 14PSCh. 22 - Prob. 15PSCh. 22 - Prob. 16PSCh. 22 - Prob. 17PSCh. 22 - Prob. 18PSCh. 22 - Which of the following ligands is expected to be...Ch. 22 - One of the following nitrogen compounds or ions is...Ch. 22 - Prob. 21PSCh. 22 - Prob. 22PSCh. 22 - Prob. 23PSCh. 22 - Prob. 24PSCh. 22 - Prob. 25PSCh. 22 - Prob. 26PSCh. 22 - Prob. 27PSCh. 22 - Prob. 28PSCh. 22 - Prob. 29PSCh. 22 - Prob. 30PSCh. 22 - Give the name or formula for each ion or compound,...Ch. 22 - Prob. 32PSCh. 22 - Prob. 33PSCh. 22 - Prob. 34PSCh. 22 - Prob. 35PSCh. 22 - Prob. 36PSCh. 22 - Prob. 37PSCh. 22 - Prob. 38PSCh. 22 - Prob. 39PSCh. 22 - Prob. 40PSCh. 22 - Prob. 41PSCh. 22 - Prob. 42PSCh. 22 - Prob. 43PSCh. 22 - Prob. 44PSCh. 22 - Prob. 45PSCh. 22 - Prob. 46PSCh. 22 - Prob. 47PSCh. 22 - Prob. 48PSCh. 22 - Prob. 49PSCh. 22 - Prob. 50PSCh. 22 - In water, the titanium(III) ion, [Ti(H2O)6]3+, has...Ch. 22 - Prob. 52PSCh. 22 - Prob. 53GQCh. 22 - Prob. 54GQCh. 22 - How many unpaired electrons are expected for...Ch. 22 - Prob. 56GQCh. 22 - Which of the following complex ions is (are)...Ch. 22 - Prob. 58GQCh. 22 - How many geometric isomers are possible for the...Ch. 22 - For a tetrahedral complex of a metal in the first...Ch. 22 - Prob. 61GQCh. 22 - Prob. 62GQCh. 22 - Prob. 63GQCh. 22 - A platinum-containing compound, known as Magnuss...Ch. 22 - Prob. 65GQCh. 22 - Prob. 66GQCh. 22 - Prob. 67GQCh. 22 - How many geometric isomers of the complex ion...Ch. 22 - Prob. 69GQCh. 22 - Prob. 70GQCh. 22 - Prob. 71GQCh. 22 - The square-planar complex Pt(en)Cl2 has chloride...Ch. 22 - The complex [Mn(H2O)6]2+ has five unpaired...Ch. 22 - Experiments show that K4[Cr(CN)6] is paramagnetic...Ch. 22 - Give a systematic name or the formula for the...Ch. 22 - When CrCI3 dissolves in water, three different...Ch. 22 - Prob. 77GQCh. 22 - The glycinate ion, H2NCH2CO2, formed by...Ch. 22 - Prob. 79GQCh. 22 - Nickel and palladium both form complexes of the...Ch. 22 - The transition metals form a class of compounds...Ch. 22 - Cerium, as noted in Applying Chemical Principles:...Ch. 22 - Prob. 84GQCh. 22 - Two different coordination compounds containing...Ch. 22 - Prob. 89SCQCh. 22 - Prob. 90SCQ
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- Please help me, using knowledge of ionization energy and atomic radii, to predict the reactivity of metals within the same group. Think about what would make a metal reactive. Examples can be added if you want to clarify meaning.arrow_forward(a) Account for formation of the following series of oxidesin terms of the electron configurations of the elementsand the discussion of ionic K2O, CaO, Sc2O3, TiO2, V2O5, CrO3. (b) Name these oxides.(c) Consider the metal oxides whose enthalpies of formation(in kJ mol -1) are listed here. Calculate the enthalpy changes in the following general reactionfor each case:MnOm(s) + H2(g)----->nM(s) + mH2O(g)(You will need to write the balanced equation for each caseand then compute ΔH°.) (d) Based on the data given, estimatea value of ΔHf° for Sc2O3(s).arrow_forward14. Does the reaction of a main – group metal oxide in water produce an acidic solution or a basic solution? Write a balanced equation for the reaction of a Group 2A oxide with water.arrow_forward
- Potassium and Sulfide ions are isoelectronic. Explain the term isoelectronic with reference to these ions.arrow_forwardWhat are the identidication tests used for the group III and IV elements? Give comprehensive explanation each.arrow_forwardHydrogen is an unusual element because it behaves in someways like the alkali metal elements and in other ways likenonmetals. Its properties can be explained in part by its electronconfiguration and by the values for its ionization energyand electron affinity. (a) Explain why the electron affinity ofhydrogen is much closer to the values for the alkali elementsthan for the halogens. (b) Is the following statement true?“Hydrogen has the smallest bonding atomic radius of anyelement that forms chemical compounds.” If not, correct it.If it is, explain in terms of electron configurations. (c) Explainwhy the ionization energy of hydrogen is closer to the valuesfor the halogens than for the alkali metals. (d) The hydrideion is H-. Write out the process corresponding to the firstionization energy of the hydride ion. (e) How does the processin part (d) compare to the process for the electron affinityof a neutral hydrogen atom?arrow_forward
- Describe the trend in acid – base behaviour of the Period 3 oxides based on the above reactions, moving from left to right across the Period. Describe the nature of oxides in period 3?arrow_forwardWhich of the species NP, NP+ and NP2− would be paramagnetic? Briefly explain why (one sentence).arrow_forwardElemental C has one of the highest atomization energies on the periodic table at 717 kJ/mol. Explain why C is so much harder to atomize than the other main group elements.arrow_forward
- Write the condensed ground-state electron configurations of these transition metal ions, and indicate which are paramagnetic. (Type your answer using the format [Ar] 4s2 3d10 4p1 for [Ar] 4s23d104p1.) (a) Mo3+ O paramagnetic O diamagnetic (b) Hf2+ O paramagnetic O diamagnetic (c) Mn2+ O paramagnetic O diamagnetic (d) v3+ O paramagnetic O diamagneticarrow_forward(a) What is the trend in first ionization energies as one proceedsdown the group 7A elements? Explain how this trendrelates to the variation in atomic radii. (b) What is the trendin first ionization energies as one moves across the fourthperiod from K to Kr? How does this trend compare with thetrend in atomic radii?arrow_forwardWhat is the valence electron configu.ration for Group SA (lS) elements?Metallic character increases when going down a group. Give some examples illustrating how Bi and Sbhave metallic characteristics not associated with N, P,and As. Elemental nitrogen exists as N2 whereas in the gas phase the elements phosphorus, arsenic, and antimony consist of P4' As4, and Sb4 molecules, respectively.Give a possible reason for" this difference between N2 and the other Group SA (lS) elements. White phosphorus is much more reactive than black or red phosphorus. Explain.arrow_forward
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