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chemistry a molecular approach

Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions

Describe the Mond process.
Which metals are found in carbaloy steel?
Which metals are found in Monel steel?
After 2.0 * 104 kg of an ore that contains 0.051% ilmenite is mined, the percent yield from extracting and refining the metals from the mineral is 87% for the iron and 63% for the titanium.Calculate the mass of iron and titanium produced from the ore.
Calculate the mass of aluminum metal that is needed to produce Cr metal from 5.00 * 102 g of chromite. Calculate how many grams of Cr metal are produced from 5.00 * 102 g of chromite.
How many lattice atoms surround a tetrahedral hole and an octahedral hole in a closest-packed structure? Describe which hole site is larger and explain why.
Explain why the crystal structure and atomic size of the two elements are important factors in a two-component phase diagram.
Why is MnO2 added to silica glass?
Co, Fe, and Ni are ferromagnetic. What is the difference between ferromagnetic and paramagnetic?
Is the chromate ion or dichromate ion more stable in an acidic solution? Which ion has a higher Cr : O ratio? Which ion has a higher oxidation state for Cr?
The first ionization energies of iron, cobalt, nickel, and the first three platinum metals are all about the same, but the first ionization energies of osmium, iridium, and platinum are substantially greater. Suggest an explanation for this observation.
Although both the group IA and IB metals have a half-filled s subshell, the IB metals have markedly higher first ionization energies, densities, and melting points, and markedly lower second and third ionization energies than the corresponding IA metals. Explain these observations.
Iron powder is placed into a tall cylinder-shaped die and pressed from the top and bottom to make a cylinder-shaped pressed part with a height of 5.62 cm and a radius of 4.00 cm. The density of the iron powder before it was pressed was 2.41 g/mL.The density of a pressed iron part is 6.85 g/mL. The
When a part is made by pressing together powdered metal, no metal is wasted. In contrast, metal is typically scrapped after a metal part is cut from a solid metal plate. If a circular part with a diameter of 10.0 cm is made from an original shape of a square with a side length of 10.0 cm, calculate
Find the equilibrium constant at 298 K for the reaction.The Kf for [Cu(CN)2]- = 1.0 * 1024 and the rest of the data needed are in Appendix II. [Ag(CN)₂] (aq) + Cu(s) [Cu(CN)₂] (aq) + Ag(s)
Hydrogen can be in both the octahedral and tetrahedral holes for lanthanum. Determine the percentage of the holes that are filled if the formula is LaH2.76.
Find the equilibrium constant at 298 K for the reaction.The Kf for [Cu(NH3)2]+ = 6.3 * 1010 and the rest of the data needed are in Appendix II. 2 [Cu(NH3)2](aq) = [Cu(NH3)4]²+ (aq) + Cu(s)
Tin exists in two allotropic forms. Gray tin has a diamond structure, and white tin has a close-packed structure. Predict which allotrope is (a) Denser, (b) A conductor of electricity. Predict the valence electronic configuration of tin in each allotrope.
Propose a chemical procedure to extract cobalt from the mineral cobaltite, CoAsS. What are some of the hazards of such a procedure?
Why are metals such as Ni and Co economical to mine and use in industrial processes, even though they have a very low natural abundance in Earth’s crust?
Explain why metals such as Au and Ag are found in their elemental states in nature, but metals like Na and Ca are always found in compounds in nature.
What allows some pairs of metals to form alloys that have the same structure at any composition, while other pairs of metals form alloys with structures that depend on the relative composition of the two metals?
Assign each element in the first row of the transition metals, scandium through zinc, to a group member. Have each group member look up on the Internet or in a reputable chemistry reference book the electrical resistivity for his or her element(s).Agree on the units and temperature. As a group,
Would you expect an alloy of iron and vanadium to be substitutional or interstitial? Explain your choice. Create a phase diagram for the binary alloy of iron and vanadium based on the tabulated data provided. % V 0 20 40 60 80 100 Melting Point 1530 1480 1470 1560 1720 1900
Create a table comparing and contrasting pyrometallurgy, hydrometallurgy, and electrometallurgy. Include a definition, an application or two, and any relevant notes for each type of metallurgy. Once your table is complete, pass it around your group asking each group member to read one cell from
Assign each group member a different interstitial alloy from Table 25.3. Each group member should look up a few interesting facts for his or her alloy, including how it is used. Present findings, along with a description of each alloy’s structure, to the group. TABLE 25.3 Formulas of Several
Alloys of tin and lead are common solders. A solder is a metal alloy that melts at a relatively low temperature and connects two or more metal pieces. The technique of soldering is commonly used by plumbers to fuse copper water pipes and by electricians to affix electrical components to printed
Write the ground state electron configuration for Zr.
What is the electron configuration of the Cu+ ion? a) [Ar]4s²3dº c) [Ar]4s¹3d⁹ b) [Ar]4s²3d8 d) [Ar] 4sº3d10
Which element has the larger atomic radius, Fe or W?(a) Fe(b) W
When a transition metal atom forms an ion, which electrons are lost first?
Write the ground state electron configuration for Co3+.
Which type of isomerism is NOT considered structural isomerism?(a) Coordination isomerism(b) Linkage isomerism(c) Geometric isomerism
Which metal has the highest first ionization energy?a) Ti b) Mn c) Ru d) Au
Explain why transition metals exhibit multiple oxidation states instead of a single oxidation state (like most of the main-group metals).
Name the following compound:[Cr(H2O)5Cl]Cl2.
Two ligands, A and B, form complexes with a particular metal ion. When the metal ion complexes with ligand A, the resulting solution is red. When the metal ion complexes with ligand B, the resulting solution is yellow. Which of the two ligands produces the larger Δ?(a) Ligand A (b) Ligand B
What is the formula of hexaaquamanganese(II) sulfate? a) [Mn(OH)6]SO4 c) [Mn(H₂O)612SO4 b) [Mn(H₂O)6]SO4 d) [Mn₂(H₂O),]SO4
Name the following compound:K3[Fe(CN)6].
Explain why atomic radii of elements in the third row of the transition metals are no larger than those of elements in the second row.
Draw the structures and label the type of all the isomers of [Co(en)2Cl2]+.
Which complex ion can exhibit cis-trans isomerism?Assume that M is the metal ion, A and B are ligands, and the geometry is octahedral. a) [MA6]²+ c) [MA4B₂]²+ 2+ b) [MA,B]²+ d) [MA3B3]2+
Gold is the most electronegative transition metal. Explain.
Pick the optical isomer of the complex ion represented here: en -+-₁ Ru --+-- Hi.. Len ity. en 2+
Draw the structures and label the type of all the isomers of [Ni(CN)2Cl2]2¯.
Determine whether the cis or trans isomers in Example 26.5 are optically active (demonstrate optical isomerism). EXAMPLE 26.5 Identifying and Drawing Geometric Isomers Draw the structures and label the type of all the isomers of [Co(en)₂Cl₂]*.
Briefly define each term.a. Coordination numberb. Ligandc. Bidentate and polydentated. Complex ione. Chelating agent
According to valence bond theory, what is the hybridization of the central metal ion in an octahedral complex ion? a) sp b) sp³ c) dsp² d) d²sp³
Using the Lewis acid–base definition, how would you categorize a ligand? How would you categorize a transition metal ion?
Estimate the crystal field splitting energy (in kJ/mol) for a complex ion that is red in solution. a) 228 kJ/mol c) 2.84 x 10-¹9 kJ/mol b) 171 kJ/mol d) 3.79 x 10-¹⁹ kJ/mol
The complex ion [Cu(NH3)6]2+ is blue in aqueous solution. Estimate the crystal field splitting energy (in kJ/mol) for this ion.
Explain the differences between each pair of isomer types.a. Structural isomer and stereoisomerb. Linkage isomer and coordination isomerc. Geometric isomer and optical isomer
How many unpaired electrons are there in the complex ion [CoF6]3¯?
Use crystal field theory to determine the number of unpaired electrons in the complex ion [Fe(CN)6]4 ¯.a) 0 b) 2 c) 3 d) 4
Which complex ion geometry has the potential to exhibit cis–trans isomerism: linear, tetrahedral, square planar, octahedral?
Which complex ion is diamagnetic? a) [Cr(H₂O)4Cl₂]+ c) [Co(NH,)]3+ 2+ b) [Fe(H₂O)]²+ d) [CoCl6]³-
How many unpaired electrons are there in the complex ion [Co(NH3)5NO2]2+?
How can you tell whether a complex ion is optically active?
Explain the differences between weak-field and strong-field metal complexes.
Explain why compounds of Sc3+ are colorless, but compounds of Ti3+ are colored.
Explain why compounds of Zn2+ are colorless, but compounds of Cu2+ are often blue or green.
Explain the differences between high-spin and low-spin metal complexes.
Why are almost all tetrahedral complexes high-spin?
Write the ground state electron configuration for each atom and ion pair. a. Ni, Ni²+ b. Mn, Mn4+ c. Y, Y+ d. Ta, Ta²+
Many transition metal compounds are colored. How does crystal field theory account for this?
Write the ground state electron configuration for each atom and ion pair. 2+ a. Zr, Zr2 b. Co, Co²+ c. Tc, Tc³+ d. Os, Os4+
Which first-row transition metal(s) has the following highest possible oxidation state? a. +3 b. +7 c. +4
Determine the highest possible oxidation state for each element.a. V b. Re c. Pd
Determine the oxidation state and coordination number of the metal ion in each complex ion. a. [Cr(H₂O)6]³+ C. [Cu(CN)4]²- b. [Co(NH3)3C13]¯¯ d. [Ag(NH3)2]*
Determine the oxidation state and coordination number of the metal ion in each complex ion. a. [Co(NH3) 5Br]2+ [Co(ox)3]4- C. b. [Fe(CN)6] d. [PdC14]²-
Name each complex ion or coordination compound. [Cr(H₂O)6]3+ C. [Fe(NH3)5Br]SO4 a. b. [Cu(CN)4]²- d. [Co(H₂O)4(NH3)(OH)]Cl₂
Name each complex ion or coordination compound. a. [Cu(en)2]²+ C. Na[Cr(H₂O)2(ox)2] b. [Mn(CO)3(NO2)3]²+ d. [Co(en)3] [Fe(CN)6]
Write the formula for each complex ion or coordination compound.a. Hexaamminechromium(III)b. Potassium hexacyanoferrate(III)c. Ethylenediaminedithiocyanatocopper(II)d. Tetraaquaplatinum(II) hexachloroplatinate(IV)
Write the formula for each complex ion or coordination compound.a. Hexaaquanickel(II) chlorideb. Pentacarbonylchloromanganese(I)c. Ammonium diaquatetrabromovanadate(III)d. Tris(ethylenediamine)cobalt(III) trioxalatoferrate(III)
Write the formula and the name of each complex ion.a. A complex ion with Co3+ as the central ion and three NH3 molecules and three CN¯ ions as ligands b. A complex ion with Cr3+ as the central ion and a coordination number of 6 with ethylenediamine ligands
Write the formula and the name of each complex ion or coordination compound.a. A complex ion with four water molecules and two ONO¯ ions connected to an Fe(III) ion b. A coordination compound made of two complex ions: one a complex of V(III) with two ethylenediamine molecules and two Cl¯ ions as
Draw two linkage isomers of [Mn(NH3)5(NO2)]2+.
Draw two linkage isomers of [PtCl3(SCN)]2¯.
Write the formulas and names for the coordination isomers of [Fe(H2O)6]Cl2.
Which complexes exhibit geometric isomerism? a. [Cr(NH3)5(OH)]²+ C. [Cr(H₂O) (NH3)3Cl₂] e. [Pt(H₂O)₂(CN)₂] b. [Cr(en)₂Cl₂]+ d. [Pt(NH3)C13]
Write the formulas and names for the coordination isomers of [Co(en)3][Cr(ox)3].
Which complexes exhibit geometric isomerism? a. C. [Co(H₂O)2(0x)2] [Co(H,O)2(NH3)2(ox)]* e. [Ni(CO)₂Cl₂] b. [Co(en)3]³+ d. [Ni(NH3)2(en)]2+
If W, X, Y, and Z are different monodentate ligands, how many geometric isomers are there for each ion? a. square planar [NiWXYZ]²+ b. tetrahedral [ZnWXYZ]2+
How many geometric isomers are there for each species? a. [Fe(CO) 3C13] b. [Mn(CO)₂Cl₂Br₂]+
Draw the structures and label the type for all the isomers of each ion. a. [Cr(CO) 3 (NH3)3]³+ b. [Pd(CO)₂(H₂O)CI]+
Draw the structures and label the type for all the isomers of each species. a. [Fe(CO)4Cl₂]+ b. [Pt(en)Cl₂]
Determine if either isomer of [Cr(NH3)2(ox)2]¯ is optically active.
Draw the octahedral crystal field splitting diagram for each metal ion. a. Zn²+ c. V/3+ b. Fe³+ (high- and low-spin) d. Co2+ (high-spin)
Determine if either isomer of [Fe(CO)3Cl3] is optically active.
Draw the octahedral crystal field splitting diagram for each metal ion. a. Cr³+ b. Cu²+ 3+ C. Mn³+ (high- and low-spin) d. Fe2+ (low-spin)
The [CrCl6]3 ¯ ion has a maximum in its absorption spectrum at 735 nm. Calculate the crystal field splitting energy (in kJ/mol) for this ion.
The absorption spectrum of the complex ion [Rh(NH3)6]3+ has maximum absorbance at 295 nm. Calculate the crystal field splitting energy (in kJ/mol) for this ion.
Three complex ions of cobalt(III), [Co(CN)6]3¯, [Co(NH3)6]3+, and [CoF6]3¯, absorb light at wavelengths of (in no particular order) 290 nm, 440 nm, and 770 nm. Match each complex ion to the appropriate wavelength absorbed. What color would you expect each solution to be?
Three bottles of aqueous solutions are discovered in an abandoned lab. The solutions are green, yellow, and purple. It is known that three complex ions of chromium(III) were commonly used in that lab: [Cr(H2O)6]3+, [Cr(NH3)6]3+, and [Cr(H2O)4Cl2]+. Determine the likely identity of each of the
The [Mn(NH3)6]2+ ion is paramagnetic with five unpaired electrons. The NH3 ligand is usually a strong-field ligand. Is NH3 acting as a strong-field ligand in this case?
How many unpaired electrons would you expect for each complex ion? a. [RhCl6]³- b. [Co(OH)6] c. cis-[Fe(en)₂(NO2)2]*
The complex [Fe(H2O)6]2+ is paramagnetic. Is the H2O ligand inducing a strong or weak field?
How many unpaired electrons would you expect for each complex ion? a. [Cr(CN)6]4 b. [MnF6]4- C. [Ru(en)3]²+
How many unpaired electrons would you expect for the complex ion [CoCl4]2- if it is a tetrahedral shape?
The complex ion [PdCl4]2¯ is known to be diamagnetic. Use this information to determine if it is a tetrahedral or square planar structure.

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