All Matches

Solution Library

Expert Answer

Textbooks

Search Textbook questions, tutors and Books

Oops, something went wrong!

Change your search query and then try again

Result Not Found

Books FREE
Tutors
Study Help
Ask a Question

Search
Sign In
Register

study help
sciences
chemical principles

Questions and Answers of Chemical Principles

Explain the difference between a weak-field ligand and a strong-field ligand. What measurements can be used to classify them as such?
Write the chemical equation that describes each of the following processes:(a) The production of chromium by the thermite reaction;(b) The corrosion of copper metal by carbon dioxide in moist
Explain why the density of mercury (13.55 g · cm–3) is significantly higher than that of cadmium (8.65 g · cm–3), whereas the density of cadmium is only slightly greater than that of zinc (7.14
Write the chemical equation that describes each of the following processes:(a) solid V2O5 reacts with acid to form the VO2+ ion;(b) solid V2O5 reacts with base to form the VO4 3– ion.
(a) Why is limestone added to a blast furnace?(b) Write chemical equations that show its reactions in the furnace.
In some older forms of the periodic table, zinc, cadmium, and mercury are classified as belonging to “Group 2B,” with the alkaline earth metals in “Group 2A.”(a) What is the justification of
The complexes(a) [RhF6]3– and(b) [Ni(ox)3]4– have highspin electron configurations. Predict the electron configurations and the number of unpaired electrons, if any, in each complex.
(a) Which types of ligands are π-acid ligands in general, strong field or weak field?(b) Which types of ligands are π-base ligands in general, strong field or weak field?
Which of the following ligands do you expect to form chelating complexes? Explain your reasoning. (a) Bipyridine (b) 1,10-Phenanthroline (c) Pyrimidine
(a) What reducing agent is used in the production of iron from its ore?(b) Write chemical equations for the production of iron in a blast furnace.(c) What is the major impurity in the product of
The energies of the 3d-orbitals are nearly unchanged across the d-elements in Period 4. However, the 3d-orbitals in zinc atoms have significantly lower energies and those of gallium atoms are even
The complexes (a) [Co(en)3]3+ and (b) [Mn(CN)6]3– have low-spin electron configurations. Predict the electron configurations and the number of unpaired electrons, if any, in each complex.
(a) Sketch the orbital energy-level diagrams for [MnCl6]4– and [Mn(CN)6]4–.(b) How many unpaired electrons are present in each complex?(c) Which complex absorbs the longer wavelengths of
What is the oxidation number of(a) V in VO2+;(b) Zn in [Zn(OH)4]2–?
Which of the following isomers of diaminobenzene can form chelating complexes? Explain your reasoning. (a) NH₂ NH, (b) NH₂ NH₂ (c) NH₂ NH,
Solutions of the [V(OH2)6]2+ ion are lilac in color and absorb light of wavelength 806 nm. What is the ligand field splitting in the complex in kilojoules per mole?
Identify the element with the higher first ionization energy in each of the following pairs:(a) Manganese and cobalt;(b) Manganese and rhenium;(c) Chromium and zinc;(d) Chromium and
Which of the following ligands can be polydentate? If the ligand can be polydentate, give the maximum number of places on the ligand that can bind simultaneously to a single metal center:(a) Chloride
Trigonal bipyramidal complexes in which a metal ion is surrounded by five ligands are rarer than octahedral or tetrahedral complexes, but many are known. Will trigonal bipyramidal compounds of the
What is the oxidation number of(a) Ti in BaTiO3;(b) Zn in Zn2(OH)2CO3?
Identify the element with the higher first ionization energy in each of the following pairs:(a) Iron and nickel;(b) Nickel and copper;(c) Osmium and platinum;(d) Nickel and palladium; (e)
Solutions of the [V(OH2)6]3+ ion are green and absorb light of wavelength 560 nm. What is the ligand field splitting in the complex in kilojoules per mole?
Draw an orbital energy-level diagram (like those in Figs.9D.3 and 9D.5) showing the configuration of d-electrons on the metal ion in each of the following complexes: (a) [Zn(OH2)6]2+; (b)
You are an engineer studying materials for computer hard-drive fabrication and need to predict the magnetic properties of the iron complexes you are investigating. Compare the magnetic properties
Use the information in Table 9C.1 to write the formula for each of the following coordination compounds:(a) Triamminediaquabromidocobalt(II) hydroxide(b) Dichloridobisethylenediaminecobalt(III)
Draw an orbital energy-level diagram (like those in Figs. 9D.3 and 9D.5) showing the configuration of d-electrons on the metal ion in each of the following complexes: (a) [Co(NH3)6]3+; (b)
New pharmaceuticals must be enantiomerically pure for use in human medicine. If you work for a large biotechnology company, you will need to be able to recognize chiral sites in complex molecules.
The concentration of nitrate ion can be determined by a multistep process. A sample of water of volume 25.00 mL from a rural well contaminated with NO3–(aq) was made basic and treated with an
Name each of the following complex ions and identify the oxidation number of the metal:(a) [Fe(CN)6]4–;(b) [Co(NH3)6]3+;(c) [Co(CN)5(OH2)]2–;(d) [Co(NH3)5(SO4)]+.
You are a scientist investigating complexes of titanium for use as photoactive coatings for selfcleaning windows. These coatings can oxidize organic materials (dirt) upon exposure to light, leaving a
Which members of the d-block, those at the left or at the right of the block, are likely to have the more strongly negative standard potentials? Explain your prediction.
Predict the major products of each of the following reactions and then balance the equations: (a) TiCl4(s) + Mg(s) A (b) COCO3(s) + HNO3 (aq) (c) V₂05(s) + Ca(1) A
Identify the number of valence electrons (including d-electrons) present in each of the following metal ions:(a) Ti2+;(b) Tc2+; (c) Ir+; (d) Ag+; (e) Y3+; (f) Zn2+.
The compound Cr(OH)3 is very insoluble in water; therefore, electrochemical methods must be used to determine its Ksp. Given that the reduction of Cr(OH)3(s) to Cr(s) and hydroxide ions has a
You are working in the chemical stockroom of a university, and a teaching assistant requests two inorganic reagents. You want to make sure you deliver the correct materials, so you need to compare
The tiny structures such as spheres and tubes formed by carbon atoms are the basis for a large part of the field of nanotechnology. Boron nitride forms similar structures.(a) What is the
The gas NO is released to the stratosphere by jet engines. Because it can contribute to the destruction of stratospheric ozone, its concentration is monitored closely. One monitoring technique
(a) Consider the substances shown in parts (a), (c), and (d) in the second illustration in Box 8F.1.(b) In which of these three parts of the figure will the interactions be the strongest?(c) In
Methanol, CH3OH, is a clean-burning liquid fuel being used as a replacement for gasoline. Calculate the theoretical yield in kilograms of CO2 produced by the combustion of 1.00 L of methanol (of
Carbon dioxide absorbs infrared energy during bending or stretching motions that are accompanied by a change in dipole moment (from zero). Which of the transitions pictured of Major Technique 1 on
One method for preparing hydrogen as a fuel from methanol uses a two-step process with the overall reaction CH3OH(l) + H2O(l) → 3 H2(g) + CO2(g). (a) What is the standard reaction enthalpy of this
Infrared radiation is absorbed only when there is a change in the dipole moment of the molecule as the molecule vibrates. Which of the following gases found in the atmosphere can absorb in the
(a) Draw the molecular orbital energy-level diagram for O2. Using the diagram, determine the bond order and magnetic properties of O2.(b) What molecular property of oxygen is explained by its
The nitrosonium ion, NO+, is isoelectronic with N2 and has two fewer electrons than O2. The ion is stable and can be purchased as its hexafluorophosphate (PF6–) or tetrafluoroborate (BF4–)
Account for the observation that melting and boiling points generally decrease from fluoride to iodide for ionic halides but increase from fluoride to iodide for molecular halides.
Give the formula for the acid corresponding to each of the following formal anhydrides:(a) N2O5;(b) P4O10;(c) SeO3.
Account for the observation that solubility in water generally increases from chloride to iodide for ionic halides with low covalent character (such as the potassium halides) but decreases from
Give the formula for the formal anhydride of each of the following acids:(a) H2CO3;(b) B(OH)3.
The Topics on the main group elements in this Focus are organized by group. Discuss whether it would be helpful to organize the elements according to period and give examples of trends that could be
For each of the following oxides, state whether the compound is acidic, basic, or amphoteric.(a) CuO;(b) P2O3;(c) ClO2;(d) GeO2.
For each of the following oxides, state whether the compound is acidic, basic, or amphoteric.(a) NO2;(b) Al2O3;(c) B(OH)3;(d) MgO.
Suppose 25.00 mL of an aqueous solution of iodine was titrated with 0.0250 m Na2S2O3(aq), with starch as the indicator. The blue color of the starch–iodine complex disappeared when 18.33 mL of the
Thiosulfuric acid, H2S2O3, has a structure similar to that of sulfuric acid, except that a sulfur atom has replaced one terminal oxygen atom. How would you expect the physical and chemical properties
The concentration of F– ions can be measured by adding an excess of lead(II) chloride solution and weighing the lead(II) chlorofluoride (PbClF) precipitate. Calculate the molar concentration of
Classify each of the following hydrides as saline, molecular, or metallic:(a) B2H6;(b) SiH4;(c) CaH2;(d) PdHx, x < 1.
The ground state of O2 has two unpaired π* electrons with parallel spins. There are two known low-lying excited states of O2. State A has the two π* electrons with the spins antiparallel but in
Classify each of the following hydrides as saline, molecular, or metallic:(a) LiH;(b) NH3;(c) HBr;(d) UH3.
(a) Use the data in Appendix 2B to decide which of ozone and fluorine is the stronger oxidizing agent in water.(b) Does your answer depend on whether the reaction is carried out in acidic or basic
Isoelectronic species have the same number of electrons.(a) Divide the following species into two isoelectronic groups: CN–, N–, NO2 –, C2 2–, O3.(b) Which species in each group is likely to
Write the balanced chemical equation for the reaction between calcium and hydrogen.
Write the balanced chemical equation for the reaction between potassium and hydrogen.
Like the atoms of elements, molecules have ionization energies.(a) Define the ionization energy of a molecule.(b) Predict which of these compounds has a higher ionization energy and justify your
The interhalogen ClFx has been used as a rocket fuel. It reacts with hydrazine to form the gases hydrogen fluoride, nitrogen, and chlorine. In one study of this reaction, ClFx gas is introduced into
When lead(II) sulfide is treated with hydrogen peroxide, the possible products are either lead(II) sulfate or lead(IV) oxide and sulfur dioxide.(a) Write balanced equations for the two
The interhalogen IFx can be made only by indirect routes. For example, xenon difluoride gas can react with iodine gas to produce IFx and xenon gas. In one experiment, xenon difluoride is introduced
(a) Draw the Lewis structure and assign a hybridization scheme to the atoms in the P4 molecule.(b) Explain why the bonds in this molecule are regarded as strained.
Which bond distance is longer:(a) The Li–Cl distance in lithium chloride or the K–Cl distance in potassium chloride;(b) The K–O distance in potassium oxide or the Ca–O distance in calcium
Describe the trend in acidity of the binary hydrogen compounds of the Group 16 elements and account for the trend in terms of bond strength.
(a) Examine the structures of diborane, B2H6, and Al2Cl6. Compare the bonding in these two compounds. How are they similar?(b) What are the differences, if any, in the types of bonds
What is the pH of 0.010 m NaHS(aq)?
Chlorine occurs as the oxoanions ClO–, ClO2 –, ClO3 –, and ClO4 – in many chemical stockrooms. However, fluorine forms no stable oxoanions. Explain this observation.
(a) Which of the following species has the greatest polarizing power: sodium ions, magnesium atoms, aluminum ions?(b) Explain your answer.
Explain the observations that NH3 is a weak Brønsted base in water, whereas NF3 is not.
The standard enthalpy of formation of SiCl4(g) at 298 K is –662.75 kJ · mol–1 and its standard molar entropy is 1330.86 J · K–1 · mol–1. Calculate the temperature at which the reduction
The azide ion forms many ionic and covalent compounds that are similar to those of the halides. (a) Write the Lewis formula for the azide ion and predict the N—N—N bond angle.(b) Compare the
If 2.00 g of sodium peroxide is dissolved to form 200. mL of an aqueous solution, what will be the pH of the solution? For H2O2, Ka1 = 1.8 * 10–12 and Ka2 is negligible.
Suggest reasons why the following interhalogens are not stable:(a) ICl5;(b) IF2;(c) ClBr3.
(a) Which of the following species has the greatest polarizability:chloride ions, bromine atoms, bromide ions?(b) Explain your answer.
The normal boiling point of NH3 is –33°C and that of NF3, which has a greater molar mass, is –129 °C. Explain this difference.
Predict the relative oxidizing strengths of H2XeO4 and H4XeO6. Explain your conclusions.
The saline hydrides all react rapidly with water. They also react similarly with liquid ammonia.(a) Write a balanced equation for the reaction of CaH2 with liquid ammonia.(b) Would it be best to
(a) Draw the Lewis structure for oleum, (HO)2OSOSO(OH)2, prepared by treating sulfuric acid with SO3.(b) Determine the formal charges on the sulfur and oxygen atoms.(c) What is the oxidation
Draw the Lewis structure of BrF3. What is the hybridization of the bromine atom in the molecule?
Calculate the values of ΔHr°, ΔSr°, and ΔGr° for the reaction 2 CO(g) + O2(g) → 2 CO2(g) at 25°C and estimate the temperature at which the equilibrium constant becomes less than 1.
The common acid anhydrides of phosphorus are P4O6 and P4O10. Write the formulas of their corresponding acids and chemical equations for the formation of the acids by the reaction of the anhydrides
In the gas phase, BeCl2 forms a dimer by forming chlorineatom bridges like those in the AlCl3 dimer. Draw the Lewis structure of the BeCl2 dimer and assign formal charges.
Many gallium compounds have structures that are similar to those of the corresponding aluminum and boron compounds. Draw the Lewis structure and describe the shape of Ga2Cl6.
(a) Which element has the greater electron affinity: bromine or selenium?(b) Explain your answer.
Methanoic acid (formic acid), HCOOH, forms dimers in the gas phase. Propose a reason for this behavior.
Predict the relative acid strengths of H2XeO4 and H4XeO6. Explain your conclusions.
Hydrogen burns in an atmosphere of bromine to give hydrogen bromide. If 135 mL of H2 gas at 273 K and 1.00 atm combines with a stoichiometric amount of bromine and the resulting hydrogen bromide
(a) Draw the Lewis structure of H2O2 and predict the approximate H—O—O bond angle.(b) Which of the following ions will be oxidized by hydrogen peroxide in acidic solution: (i) Cu+; (ii) Mn2+;
Draw the Lewis structure of Cl2O. Predict the shape of the Cl2O molecule and estimate the Cl—O—Cl bond angle.
Calculate the values of ΔHr°, ΔSr°, and ΔGr° for the production of high-purity silicon by the reaction SiO2(s) + 2 C(s, graphite) → Si(s) + 2 CO(g) at 25°C and estimate the temperature at
The common acid anhydrides of nitrogen are N2O, N2O3, and N2O5. Write the formulas of their corresponding acids and chemical equations for the formation of the acids by the reaction (in one case,
(a) Draw the Lewis structure of BeCl2.(b) Predict the Cl—Be—Cl bond angle.(c) What hybrid orbitals are used in the bonding in BeCl2?(d) Why does MgCl2 not have the same structure?
Many gallium compounds have structures that are similar to those of the corresponding aluminum and boron compounds. Draw the Lewis structure and describe the shape of GaBr4–.
(a) Which element has the greater electron affinity: bromine or chlorine?(b) Explain your answer.
The enthalpy of dissociation of hydrogen bonds, ΔHHBond, is a measure of their strength. Explain the trend seen in the data for the following pure substances, which were measured in the gas phase:
Complete and balance each of the following reactions: (a) XeF (s) + H₂O(1)→XeO3(aq) + HF(aq) (b) Pt(s) + XeF₁(s) (c) Kr(g) + F₂(g)- → electric discharge

Showing 800 - 900 of 3011

First
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
Last

Get In Touch

About Us
Contact Us
Career
Jobs
FAQ
Campus Ambassador

Company Info

Security
Copyrights
Privacy Policy
Terms & Condition
SolutionInn Fee
Scholarship

Services

Sitemap
Fun
Definitions
Become Tutor
Study Help Categories
Recent Questions
Expert Questions

Copyright © 2024 SolutionInn All Rights Reserved.

Get the SolutionInn - Study Help App