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Questions and Answers of Chemical Principles

You are given samples of propanal, 2-propanone, and ethanoic acid. Describe how you would use chemical tests including acid–base indicators to distinguish among the three compounds.
Consider the following organic molecules, which have approximately the same molar masses but might contain different functional groups:CH3CH2CH2CH2CH2CH3, CH3CH2CH2CH2CHCH2, CH3CH2CH2CH2CH2OH,
You are given samples of 1-propanol, pentane, and ethanoic acid. Describe how you would use chemical tests such as aqueous solubility and acid–base indicators, to distinguish among the three
Write the structural formula of the product of(a) The reaction of glycerol (1,2,3-trihydroxypropane) with stearic acid, CH3(CH2)16COOH, to produce a saturated fat;(b) The oxidation of 4-hydroxybenzyl
Rank the following acids in order of increasing acid strength: ClCH2COOH, Cl3CCOOH, CH3COOH, and CH3CH2COOH. Justify your answer.
Write the condensed structural formulas of the principal products of the reaction that takes place when(a) Ethylene glycol, 1,2-ethanediol, is heated with stearic acid, CH3(CH2)16COOH;(b) Ethanol
Rank methylamine, dimethylamine, and diethylamine in order of increasing base strength. Explain your rankings in relation to their molecular structure.
The monomer of the conducting polymer polyaniline is the compound aniline (aminobenzene).(a) Draw the structural formula of the aniline monomer.(b) What is the hybridization of the N atom in
segment of a protein is analyzed and found to contain the amino acid sequence Glu-Leu-Asp. Draw the Lewis structure of this segment, showing the peptide bonds.
Fibers of the conducting polymer polypyrrole are woven into radar camouflage cloth. Because it absorbs microwaves, rather than reflecting them back to their source, the cloth appears to be a patch of
The pKa values for phenol, o-nitrophenol, m-nitrophenol, and p-nitrophenol are 9.89, 7.17, 8.28, and 7.15, respectively. Explain the origin of these differences in pKa.
Acrylic resins are polymeric materials used to make warm yet lightweight garments. The osmotic pressure of a solution prepared by dissolving 47.7 g of an acrylic resin in enough water to make 500. mL
The average molar mass of a sample of polypropylene was determined by measuring the osmotic pressure of 500. mL of a solution of 3.16 g of polypropylene in benzene. A pressure of 0.0112 atm was
(a) Explain the differences among the primary, secondary, tertiary, and quaternary structures of a protein.(b) Identify the forces holding each structure together as covalent bonds or primarily
Haloalkanes may react with hydroxide ions, undergoing nucleophilic displacement of the halide ion to form an alcohol. A complication of such reactions is competition from elimination reactions rather
The protonated form of glycine (+H3NCH2COOH) has Ka1 = 4.47 * 10–3, and Ka2 = 1.66 * 10–10.(a) Write the chemical equations for the proton transfer equilibria.(b) What is the dominant form of
In the amide group, rotation is restricted about the CON bond, so that the C, N, and O atoms in that group are normally in the same plane. This rigidity is partly responsible for the secondary
Explain the process of condensation polymerization. How might the polymer obtained from benzene-1,2-dicarboxylic acid and ethylene glycol differ from Dacron?
Polyphosphazenes, which are used as heat-resistant polymers in the aerospace industry and as flexible scaffolds for bone regeneration, are inorganic polymers with the repeating unit (—PR2=N—)n,
The average molar mass of a hydrogen-bonded pair of nucleotides in a DNA molecule is 625 g · mol–1. Each successive pair is found at a distance of 340 pm along the chain. If the total length of
Propane torches are used for minor home repairs, but welders must use torches that burn acetylene (ethyne).(a) Write chemical equations for the combustion of propane and ethyne.(b) Calculate the
Pheromones are commonly called sex attractants, although they have other signaling functions, too. A pheromone of the queen bee is trans-CH3CO(CH2)5CH=CHCOOH.(a) Write the structural formula of the
Why are hydrocarbons with between one and four carbon atoms not suitable for gasoline?
What are the major problems associated with using coal as a fuel?
Propene and butane can be combined by the process called alkylation to form a straight-chain hydrocarbon used in gasoline. Write a chemical equation for the reaction.
The compound C18H38 is a component of fuel oil that can be converted by a cracking process into two compounds suitable for use in gasoline. The compounds have the formulas CnH2n + 2 and CnH2n, with
Aromatization is a process used to improve the quality of gasoline by converting aliphatic hydrocarbons into aromatic ones.(a) When heptane is converted into toluene, a byproduct is formed. Does
Isomerization is a process used to improve the quality of gasoline by converting straight-chain hydrocarbons into branched ones. If octane is isomerized into a branched pentane, several structural
A gaseous compound used to make both bubble gum and automobile tires was analyzed to determine its properties and toxicity.(a) When 0.108 g of the compound was analyzed by combustion analysis, 0.352
Waste reduction is an important goal of the green chemistry movement. In many chemical syntheses in industry, not all the atoms required for the reaction appear in the product.Some end up in
Using concepts of ligand field theory, explain why ethylenediamine is a weaker field ligand than CO.
Using concepts of ligand field theory, explain why water is a weaker field ligand than ammonia.
Is the best description of the t2g-orbitals in [CoF6]3– bonding, antibonding, or nonbonding? Explain how you reached your conclusion.
Is the best description of the eg-orbitals in [Fe(OH2)6]3+ bonding, antibonding, or nonbonding? Explain how you reached your conclusion.
Is the best description of the t2g-orbitals in [Fe(CN)6]3– bonding, antibonding, or nonbonding? Explain how you reached your conclusion.
Is the best description of the t2g-orbitals in [Co(OH2)6]3+ bonding, antibonding, or nonbonding? Explain how you reached your conclusion.
(a) Describe each of the following ligands as either a π-acid, a π-base, or neither (see Exercise 9D.27):(i) NH3; (ii) ox; (iii) F–; (iv) CO.(b) Place them in order of increasing ligand field
Ligands that can interact with a metal center by forming a π-bond are commonly called π-acids and p-bases. The definitions of π-acid and π-base are similar to those used for Lewis acidity. A
Which of the following complexes can have cis and trans isomers? If such isomerism exists, draw the two structures and label the ions as cis or trans:(a) [Fe(OH)2(OH2)4]+; (b) [RuBr2(NH3)4]2+; (c)
Write the formulas for the oxoanions of the following elements in which the element is found with its highest oxidation number (see Fig. 9A.7). In each case, the charge of the oxoanion is given in
(a) Draw all the possible isomers of the square planar complex PtBrCl(NH3)2 and name each isomer.(b) How can the existence of these isomers be used to show that the complex is square planar rather
Hemoglobin contains one heme group per subunit. The heme group is an Fe2+ complex that is coordinated to the four N atoms in a porphyrin ligand in a square planar arrangement and to an N atom on the
Which d-orbitals on the metal ion are used to form π-bonds between metal ions and ligands in an octahedral complex?
Vanadium is used in steelmaking because it forms V4C3, which increases the strength of the steel and its resistance to wear. It is formed in the steel by adding V2O5 to iron ore as it is reduced by
An analytical chemist analyzed a yellow mineral salt found in the pigments used by a Renaissance artist. When hydrochloric acid was added, the mineral dissolved and formed an orange solution. The
(a) Estimate the ligand field splitting for (i) [CoF6]3– (λmax = 700. nm), (ii) [Co(NH3)6]3+ (λmax = 435 nm), and (iii) [Co(OH2)6]3+ (λmax = 540. nm), where λmax is the wavelength of the
(a) Estimate the ligand field splitting for (i) [CrCl6]3– (λmax = 740. nm), (ii) [Cr(NH3)6]3+ (λmax = 460. nm), and (iii) [Cr(OH2)6]3+ (λmax = 575 nm), where λmax is the wavelength of the
An analytical chemistry team analyzed a green mineral salt found in the glaze of an ancient pot. When they heated the mineral, it gave off a colorless gas that turned limewater milky white. When they
Suggest a reason why copper(II) compounds are often colored but copper (I) compounds are colorless. Which oxidation number results in paramagnetic compounds?
Suggest a reason why copper(II) compounds are often colored but copper (I) compounds are colorless. Which oxidation number results in paramagnetic compounds?
Ligand field theory predicts that different types of metal ions will form more stable complexes with certain types of ligands. From your understanding of ligand field theory, predict what types of
The concentration of Fe2+ ions in an acid solution can be determined by a redox titration with either KMnO4 or K2Cr2O7. The reduction products of these reactions are Mn2+ and Cr3+, and in each case
In aqueous solution, water competes effectively with bromide ions for coordination to Cu2+ ions. The hexaaquacopper(II) ion is the predominant species in solution. However, in the presence of a large
cis-Platin is an anticancer drug with a three-dimensional structure that can be viewed on the Internet.(a) What are the formula and systematic name for the compound cis-platin?(b) Draw any isomers
One structure of the octahedral complex FeCl2(NH3)3SCN is shown below. Draw all possible isomers of this complex. HN Cl CI Fe - SCN NH 3 NH
The complex [Co(CN)6]3– is pale yellow.(a) How many unpaired electrons are present in the complex?(b) If ammonia molecules replace the cyanide ions as ligands, will the wavelength of the
Molecular models of the iridium complex IrCl(CO) [P(C6H5)3]2 (ChemSpider ID 21106488) can be found on the Internet.(a) View the three-dimensional structure and determine the coordination geometry of
Ethylenediamine (en) forms a chelate complex with Co3+, [Co(en)3]3+. Are isomers of this complex possible and, if so, what type of isomers are they? N N Co N. [Co(en),]³+ N 3+ N H₂C-CH₂ N =
The complex [TiCl6]3– has a ligand field splitting of 160. kJ · mol–1 and forms an orange solution. What is the wavelength and color of the absorbed light?
Two chemists prepared a complex and determined its formula, which they wrote as [CrCl3NH3] · 2H2O. However, when they dissolved 2.11 g of the compound in water and added an excess of silver nitrate,
Is either of the following complexes chiral? If both complexes are chiral, do they form an enantiomeric pair? A (a) A B D C B (b) A · Α B
The complex [Ni(NH3)6]2+ has a ligand field splitting of 209 kJ · mol–1 and forms a purple solution. What is the wavelength and color of the absorbed light?
The complex [Ni(NH3)6]2+ has a ligand field splitting of 209 kJ · mol–1 and forms a purple solution. What is the wavelength and color of the absorbed light?
A solid pink salt has the formula CoCl3 · 5NH3 · H2O. When AgNO3 is added to the pink solution containing 0.0010 mol CoCl3 · 5NH3 · H2O, 0.43 g of AgCl precipitates. Heating the salt produces
Is either of the following complexes chiral? If both complexes are chiral, do they form an enantiomeric pair? C (a) B A B D A B (b) A A D
Which of the complexes [Cu(OH2)6]2+ or [CuBr6]4– absorbs at the longer wavelength?
Is there a correlation between the ligand field strength of the halide ions F–, Cl–, Br–, and I– and the electronegativity of the halogen? If so, can this correlation be explained by ligand
How many isomers are possible for [CoCl(NCS)(OH2)4]l · H2O? Consider all types of isomerism and draw each isomer.
Some of the properties of manganese differ markedly from those of its neighbors. For example, at constant pressure it takes 400 kJ (2 sf) to atomize 1.0 mol Cr(s) and 420 kJ to atomize 1.0 mol Fe(s),
Of the two complexes(a) [CoF6]3– and(b) [Co(en)3]3+, one appears yellow and the other appears blue. Match the complex to the color and explain your choice.
In a nickel-containing enzyme, various groups of atoms in the enzyme form a complex with the metal, which was found to have oxidation number +2 and to have no unpaired electrons. What is the most
How many isomers are possible for [Cr(NH3)5(NO2)]Cl2? Consider all types of isomerism and draw each isomer.
(a) Explain why a chromium(III) salt produces an acidic solution in water.(b) Explain why the slow addition of hydroxide ions to a solution containing chromium(III) ions first produces a gelatinous
Which of the elements scandium, molybdenum, and copper is most likely to form a chloride with the formula MCl4? Explain your decision.
Nickel(II) complexes with weak-field ligands such as the bromide ion have been found to be octahedral, but nickel(II) complexes with strong-field ligands have been found to be square planar. Explain
When the paramagnetic [Co(CN)6]4– ion is oxidized to [Co(CN)6]3–, the ion becomes diamagnetic. However, when the paramagnetic [Co(ox)3]4– is oxidized to [Co(ox)3]3–, the ion remains
Use Appendix 2B to determine whether an acidic potassium permanganate solution can oxidize(a) Chloride ions to chlorine and(b) Mercury metal to mercury (I) ions under standard conditions. 2B
Suggest the form that the orbital energy-level diagram would take for a square planar complex with the ligands in the xy plane, and discuss how the building-up principle applies. The dz2-orbital has
Which of the elements vanadium, chromium, and manganese is most likely to form an oxide with the formula MO3? Explain your decision.
When the paramagnetic [Fe(CN)6]3– ion is reduced to [Fe(CN)6]4–, the ion becomes diamagnetic. However, when the paramagnetic [FeCl4]– ion is reduced to [FeCl4 ]2–, the ion remains
Which of the following coordination compounds can have cis and trans isomers? If such isomerism exists, draw the two structures and name the compound:(a) [CoCl2(NH3)4] Cl · H2O; (b)
Use Appendix 2B to determine whether an acidic sodium dichromate solution can oxidize(a) Bromide ions to bromine and(b) Silver (I) ions to silver(II) ions under standard conditions. 2B STANDARD
Give the systematic name and chemical formula of the principal component of(a) Rutile;(b) Hematite;(c) Pyrolusite;(d) Chromite.
Suggest a chemical test for distinguishing between(a) [Ni(SO4)(en)2]Cl2 and [NiCl2(en)2]SO4;(b) [NiI2(en)2]Cl2 and [NiCl2(en)2]I2.
Draw the structures of all possible isomeric forms of CrBrClI(NH3)3. Which isomers are chiral?
The trigonal prismatic structure shown in the illustration was once proposed for the complex CoCl2(NH3)4. Use the fact that only two isomers of the complex are known to rule out the prismatic
Which oxoanion, MnO4– or ReO4–, is expected to be the stronger oxidizing agent? Explain your choice.
Iron in blood serum can be measured by reducing it to Fe2+ and reacting it with ferrozine to form [Fe(ferrozine)3]4–, a purple complex that has a maximum absorbance at 562 nm.The molar absorption
How many chelate rings are present in(a) [Ru(ox)3]3–;(b) [Fe(trien)]3+ (trien is triethylenetetramine);(c) [Cu(dien)2]2+? H₂N H₂N triển dien NH ΝΗ ΝΗ NH₂ NH,
Identify the type of structural isomerism that exists in each of the following pairs of compounds or ions: (a) [Pt(OH₂)4] [PtCl6] and [PtCl₂(OH₂)4] [PtCl4] (b) [Cr(en)3] [Co(ox)3] and
By considering electron configurations, suggest a reason why iron(III) is readily prepared from iron(II) but the conversion of nickel(II) and cobalt(II) into nickel(III) and cobalt(III) is much more
(a) Describe the trend in the stability of oxidation states moving down a group in the d-block (for example, from chromium to molybdenum to tungsten).(b) How does this trend compare with the trend
The total concentration of cis- and trans-[CoCl(en)2SCN]+ in a solution can be studied at 540 nm, where both isomers have ε = 175 L · mol–1 · cm–1. In one experiment the absorbance of a
A hexagonal planar structure was once proposed for the CrCl3(NH3)3 complex. Use the fact that only two isomers of the complex are known to rule out the hexagonal planar structure.
Before the structures of octahedral complexes were established, various means were used to explain the fact that d-metal ions could bind to a greater number of ligands than expected on the basis of
Identify the type of structural isomerism that exists in each of the following pairs of compounds: (a) [Co(NH3),(NO₂)] Br₂ and [Co(NH3),(ONO)] Br₂ (b) [Pt(NH3)4(SO4)](OH), and [Pt(NH3)4(OH)₂
By considering electron configurations, explain why gold and silver are less reactive than copper.
Explain why the density of vanadium (6.11 g · cm–3) is significantly less than that of chromium (7.19 g · cm–3). Both vanadium and chromium crystallize in a body-centered cubic lattice.
Describe the changes that may take place in a compound’s properties when weak-field ligands are replaced by strong-field ligands.
With the help of Table 9C.1, determine the coordination number of the metal ion in each of the following complexes:(a) PtBr2(NH3)2;(b) [Ni(en)2I2]+;(c) [Co(ox)3]3–;(d) [Mn(CO)5]–. TABLE 9C.1

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