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Chemical Principles The Quest For Insight 7th Edition Peter Atkins, Loretta Jones, Leroy Laverman - Solutions

Salts of indium(III) are used in some nutritional supplements, despite known side effects, because it is claimed that they can enhance the speed of memory, balance hormones, and reduce the need for sleep. However, indium (I) salts are unstable in water and so cannot be used in the diet. If you
One way to understand the reactivities of compounds is to identify the strengths of their bonds, because weak bonds can often be broken easily. A guide to bond strength is bond order. Deduce the ground-state electron configuration of the fluorine molecule and calculate its bond
Place the following elements in order of increasing electronegativity: antimony, tin, selenium, and indium
Give the number of valence electrons (including d electrons) for each of the following elements:(a) Sb;(b) Si;(c) Mn;(d) B.
The fluoride SF4 is used in the pharmaceutical industry to synthesize fluorocarbons, some of which are used as anesthetics. Write the Lewis structure of sulfur tetrafluoride and give the number of electrons in the expanded valence shell.ANTICIPATE Sulfur, in Group 16, has six valence electrons; if
When you are assessing the properties of a compound, such as its ability to take part in a reaction, you need to know whether it is likely to have single or multiple bonds. Write the Lewis structures of(a) Water, H2O;(b) Methanal, H2CO; and(c) The chlorite ion, ClO2¯. Use the rules in Toolbox
Which of the following species are radicals?(a) NO2–;(b) CH3;(c) OH;(d) CH2O.
Draw a molecular orbital energy-level diagram and determine the bond order expected for each of the following diatomic species:(a) Li2;(b) Li2+;(c) Li2–. State whether each molecule or ion will be paramagnetic or diamagnetic. If it is paramagnetic, give the number of unpaired electrons.
Identification of the hybridization of an atom in a molecule can often act as a good guide to the kind of chemical reactions it can undergo and help in the interpretation of its spectroscopic observations. What is the hybridization of phosphorus in PF5?ANTICIPATE To form five bonds, five hybrid
The shapes of simple molecules are often relevant to their physical properties, and as you progress through your study of chemistry you will see how important it is to know whether a molecule is planar or not. Predict the electron arrangement and the shape of a nitrogen trifluoride molecule,
State the relative orientations of each of the following hybrid orbitals:(a) sp3;(b) sp;(c) sp3 d2;(d) sp2.
Draw the Lewis structure, including resonance structures where appropriate, for(a) The oxalate ion, C2O42– (there is a C—C bond with two oxygen atoms attached to each carbon atom);(b) BrO+;(c) The acetylide ion, C22–. Assign formal charges to each atom.
Draw the Lewis structure of(a) CCl4;(b) COCl2;(c) ONF;(d) NF3.
Below are ball-and-stick models of two molecules. In each case, indicate whether there must be, may be, or cannot be one or more lone pairs of electrons on the central atom. 120° (a) 180° (b)
The sulfate ion, SO42–, is present in a number of important minerals, including gypsum (CaSO4 · 2H2O), which is used in cement, and Epsom salts (MgSO4 · 7H2O), which is used as a purgative. Determine the dominant resonance structure of a sulfate ion from the three shown in (10a–10c) by
Place the following elements in order of increasing electronegativity: iodine, sulfur, bromine, oxygen, and arsenic.
Give the number of valence electrons (including d electrons) for each of the following elements:(a) V;(b) Fe;(c) Cd;(d) I.
Which of the following species are radicals?(a) NO3;(b) ICl2+;(c) CH2O;(d) HOCO.
Draw a molecular orbital energy-level diagram and determine the bond order expected for the following diatomic species:(a) B2;(b) B2–;(c) B2+. State whether each molecule or ion will be paramagnetic or diamagnetic. If it is paramagnetic, give the number of unpaired electrons.
Formic acid is an important starting material for some polymers. Its structure makes it useful for the synthesis of strong polymer chains. Account for the structure of a formic acid molecule, HCOOH, in terms of hybrid orbitals, bond angles, and σ- and π-bonds. The C atom is attached to an H atom,
When organic chemists think about how molecules undergo change during a reaction, they commonly find it helpful to write down a scheme that includes Lewis structures. Write the Lewis structure for acetic acid, CH3COOH, which is found in vinegar.The formula of acetic acid suggests that the molecule
The orientation of bonds on a central atom of a molecule that has no lone pairs can be one of the following. What is the hybridization of the orbitals used by each central atom for its bonding pairs:(a) Tetrahedral;(b) Trigonal bipyramidal;(c) Octahedral;(d) Linear?
You can’t always guess a molecular shape from its chemical formula; even quite simple molecules can have surprising shapes. Predict the shape of a sulfur tetrafluoride molecule, SF4.ANTICIPATE You might guess that SF4 has a tetrahedral geometry. However, you need to be aware that sulfur is
Draw three Lewis structures that follow the octet rule (including the most important structure) for the isocyanate ion, CNO–. State which of the three Lewis structures is the most important and explain why.
Draw the Lewis structure of(a) SCl2;(b) AsFr3;(c) SiH4;(d) InCl3
Draw the Lewis structure of(a) OF2;(b) NHF2;(c) SiO2;(d) BrF3.
Draw the structures and name the shapes of the following molecules:(a) HCN;(b) CH2F2.
Which of these compounds has bonds that are primarily ionic?(a) BBr3;(b) BaBr2;(c) BeBr2.
Stratospheric ozone, O3, protects life on Earth from harmful ultraviolet radiation from the Sun. Suppose you are an atmospheric chemist; to understand the spectroscopic and structural properties of ozone, you would need to know how its electrons are arranged. Suggest two Lewis structures that
Give the ground-state electron configuration expected for each of the following ions:(a) S2–;(b) As3+;(c) Ru3+;(d) Ge2–.
Draw the Lewis structure, including typical contributions to the resonance structure (where appropriate, allow for the possibility of octet expansion, including double bonds in different positions), for(a) Periodate ion;(b) Hydrogen phosphate ion;(c) Chloric acid;(d) Arsenate ion.
(a) On the basis of the configuration of the neutral molecule F2, write the molecular orbital configuration of the valence molecular orbitals for(i) F2–; (ii) F2+; (iii) F22–.(b) For each species, give the expected bond order.(c) Which are paramagnetic, if any?(d) Is the highest-energy
Because the polarity of a molecule affects its physical properties, you need to know whether a molecule is polar or nonpolar when predicting how it might interact with other molecules. Predict whether(a) A boron trifluoride molecule, BF3, and (b) An ozone molecule, O3, are polar.ANTICIPATE The
How many σ -bonds and how many π -bonds are there in(a) H2S and(b) SO2?
Which do you expect to have the greater lattice energy, iron(III) chloride or iron(II) chloride? Explain your answer.
Draw the Lewis structure of(a) Cl2O;(b) N2 F2;(c) SO3;(d) BrF4¯.
Which of these compounds has bonds that are primarily covalent?(a) CaCl2 ;(b) CsCl;(c) CCl4.
Draw the structures and name the shapes of the following molecules:(a) SeF6;(b) IF7.
If you were an analytical chemist, one test you might use for the presence of iron(III) ions is to add a solution of potassium thiocyanate, KSCN; a blood-red color indicates that a compound of iron and the thiocyanate ion has formed. Write three Lewis structures with different atomic arrangements
Give the ground-state electron configuration expected for each of the following ions:(a) V4+;(b) Fe3+;(c) Cd2+;(d) I–.
Draw the Lewis structure, including typical contributions to the resonance structure (where appropriate, allow for the possibility of octet expansion), for(a) Formate ion (HCO2–);(b) Hydrogen phosphite ion;(c) Bromate ion;(d) Selenate ion.
(a) On the basis of the configuration for the neutral molecule N2, write the molecular orbital configuration of the valence molecular orbitals for(i) N2+; (ii) N2 2+; (iii) N2 2–.(b) For each species, give the expected bond order.(c) Which are paramagnetic, if any?(d) Is the highest-energy
Explain the trend of decreasing lattice energies of the chlorides of the Group 2 metals down the group.
How many σ-bonds and how many π -bonds are there in(a) NO and(b) N2 O?
Draw the Lewis structure of(a) Tetrahydridoborate ion, BH4–;(b) Hypobromite ion, BrO–;(c) Amide ion, NH2–.
For each pair, determine which compound has bonds with greater ionic character:(a) HCl or HI;(b) CH4 or CF4;(c) CO2 or CS2 .
(a) What is the shape of a ClO2+ ion?(b) What is the expected OClO bond angle?
Give the ground-state electron configuration expected for each of the following ions:(a) Cu+;(b) Bi3+;(c) Ga3+;(d) Tl3+.
Draw the Lewis structure of each of the following reactive species, all of which are found to contribute to the destruction of the ozone layer, and indicate which are radicals:(a) Chlorine monoxide, ClO;(b) Dichloroperoxide, Cl—O—O—Cl;(c) Chlorine nitrate, ClONO2 (the central O atom is
The ground-state electron configuration of the ion C2 n- is σ2s 22s*2π2p 4σ2p2. What is the charge on the ion, and what is its bond order?
Draw resonance structures for the trimethylenemethane anion C(CH2)32– in which a central carbon atom is attached to three CH2 groups (CH2 groups are referred to as methylene).
State the hybridization of the atom in boldface red type in each of the following molecules and ions:(a) Be Cl2 ;(b) BH3;(c) BH4–;(d) SiF4.
Draw the Lewis structure of(a) Nitronium ion, ONO+; (b) Chlorite ion, ClO2–;(c) Peroxide ion, O22–;(d) Formate ion, HCO2 –.
For each pair, determine which compound has bonds with greater ionic character:(a) PH3 or NH3;(b) SO2 or NO2;(c) SF6 or IF5.
(a) What is the shape of a ClO2 – ion?(b) What value is expected for the OClO bond angle?
Give the ground-state electron configuration expected for each of the following ions:(a) Zr4+;(b) Os3+;(c) Cs+;(d) P 3 2 .
Draw the Lewis structure of each of the following species and indicate which are radicals:(a) The triiodide ion, I3–;(b) The methyl cation, CH3+;(c) The methyl anion, CH3–;(d) Chlorine dioxide, ClO2.
The ground-state electron configuration of the ion B2 n- is σ2s 22s*2π2p3. What is the charge on the ion, and what is its bond order?
Show how resonance can occur in the following organic ions:(a) Acetate ion, CH3CO2;(b) Enolate ion, CH2COCH3–, which has one resonance structure with a C=C double bond and an —O– group on the central carbon atom;(c) Allyl cation, CH2 CHCH2+;(d) Amidate ion, CH3 CONH– (the O and the N
State the hybridization of the atom in boldface red type in each of the following molecules and ions:(a) SF6;(b) ClO3–;(c) NO3–;(d) OCCl2 .
The following Lewis structure was drawn for a Period 3 element. Identify the element. CI :0: E- :15: - CI:
Identify the hybrid orbitals used by the atom in boldface red type in each of the following species:(a) BF3;(b) AsF3;(c) BrF3;(d) SeF3+ .
Compounds having bonds with a high covalent character tend to be less soluble in water than similar compounds that have low covalent character. Use electronegativities to predict which of the following compounds is the more soluble in water:(a) AlCl3 or KCl;(b) MgO or BaO.
In a plasma display panel (PDP), an electrical discharge causes the ionization of gases, producing UV radiation that strikes a phosphor, which generates red, green, or blue light depending on which phosphor coats the cell. Millions of such cells are combined to create an image. Estimate the
Air molecules are constantly striking your face. How fast are they moving when they collide with you? Calculate the root mean square speed of nitrogen molecules at 20. °C.ANTICIPATE Because a sound wave is propagated by the movement of molecules, you should expect that typical speeds are about
Robert Boyle measured pressure in inches of mercury (inHg). On a day when the atmospheric pressure was 29.85 inHg, he trapped some air in the tip of a J-tube (1) and measured the difference in height of the mercury in the two arms of the tube (h). When h 5 12.0 in., the height of the gas in the tip
Do all the molecules of a gas strike the walls of their container with the same force? Justify your answer on the basis of the kinetic model of gases.
Investigators are studying the physical properties of a gas to be used as a refrigerant in an air-conditioning unit. Because refrigerants are used at low temperature and high pressure, they cannot be treated as ideal gases. A table of van der Waals parameters shows that for a certain refrigerant a
The drawing below shows a tiny section of a flask containing two gases. The orange spheres represent neon atoms and the blue spheres represent argon atoms.(a) If the partial pressure of neon in this mixture is 420. Torr, what is(a) The partial pressure of argon;(b) The total pressure?
One reason that copper is so valuable is its high malleability, which is related to its structure. Suppose you have been asked to examine how different types of heat treatment affect the crystal structure of copper. One way to detect a change in structure is from the density. After one heat
Glucose (C6H12O6) and benzophenone (C6H5COC6H5) are examples of compounds that form molecular solids. The structures of glucose and benzophenone are given here.(a) What types of forces hold these molecules in a molecular solid?(b) Which of the two solids has the higher melting point?
The pressure of a sample of hydrogen fluoride is lower than expected and, as the temperature is increased, rises more quickly than the ideal gas law predicts. Suggest an explanation.
You are working on an organic synthesis and need to change a solvent to one that has a higher boiling point. Which would you expect to have the higher boiling point, p-dichlorobenzene (3) or o-dichlorobenzene (4)?PLAN When two compounds have different dipole moments but are otherwise very similar,
Identify the types of attractive intermolecular interactions that might arise between molecules of each of the following substances:(a) NH2OH;(b) CBr4;(c) H2SeO4;(d) SO2.
Estimate the relative density (compared to pure aluminum) of magnalium, a magnesium–aluminum alloy in which 30.0% of the aluminum atoms have been replaced by magnesium atoms without distortion of the crystal structure.
A sample of hydrogen chloride gas, HCl, is being collected by bubbling it through liquid benzene. Assume that the molecules pictured as spheres show a representative sample of the mixture of HCl and benzene vapor (⚫represents an HCl molecule and ⚪ a benzene molecule).(a) Use the figure to
How does the change in electrical resistance of a semiconductor differ from that of a metallic conductor as temperature is increased?
Meteorologists monitor changes in atmospheric pressure to help predict future weather patterns. A drop in pressure is often a sign of an approaching storm system. Suppose the height of the column of mercury in a barometer is 760. mm at 15°C. What is the atmospheric pressure in pascals? At 15°C,
Predict how each of the following properties of a liquid varies as the strength of intermolecular forces increases and explain your reasoning:(a) Boiling point;(b) Viscosity;(c) Surface tension.
In an automobile engine, the piston compresses a mixture of gasoline vapor and air before ignition occurs. The combined gas law can be used to calculate the new pressure. Assume that, when the piston is pushed in, the volume inside the chamber is decreased from 100. cm3 to 20. cm3 before ignition.
The pressure needed to make synthetic diamonds from graphite is 8 * 104 atm. Express this pressure in(a) Pa;(b) kbar;(c) Torr;(d) lb · in.–2.
Boyle continued to add mercury to the apparatus in Exercise 3B.1 until the height of the trapped air had been reduced to 6.85 in.. Assuming that atmospheric pressure had not changed, what was the pressure of the trapped air at that point (in inHg)?Exercise 3B.1Robert Boyle measured pressure in
How does the frequency of collisions of the molecules of a gas with the walls of the container change as the volume of the gas is decreased at constant temperature? Justify your answer on the basis of the kinetic model of gases.
The four flasks below were prepared with the same volume and temperature. Flask I contains He atoms, Flask II contains Cl2 molecules, Flask III contains Ar atoms, and Flask IV contains NH3 molecules. Which flask has(a) The largest number of atoms;(b) The highest pressure;(c) The greatest (mass)
Cesium chloride is being studied as an alternative treatment for cancer. Its medicinal effect is thought to be related to the large size of its cation. Estimate the density of cesium chloride from its crystal structure.ANTICIPATE The densities of ionic compounds are typically a few grams per cubic
Under what conditions of temperature and pressures would you expect a real gas to have(a) Z < 1;(b) Z > 1?
Chloromethane (CH3Cl) and acetic acid (CH3COOH) form molecular solids.(a) What types of forces hold these molecules in a molecular solid?(b) Which of the two liquids has the higher freezing point?
Chemists often gain insight into physical properties through examination of trends in closely related molecules. Explain the trend in the boiling points of the hydrogen halides: HCl, 285 °C; HBr, 267 °C; HI, 25 °C.PLAN Stronger intermolecular forces result in higher boiling points. The dipole
Identify the types of attractive intermolecular interactions that might arise between molecules of each of the following substances:(a) H2S;(b) SiH4;(c) N2H4;(d) CHF3.
The carbon dioxide generated by the personnel in submarines and spacecraft must be removed from the air and the oxygen recovered. Submarine design teams have investigated the use of potassium superoxide, KO2, as an air purifier because it reacts with carbon dioxide and releases oxygen (FIG.
Estimate the relative density (compared to pure copper) of aluminium bronze, an alloy that is 8.0% by mass aluminium.Assume no distortion of the crystal structure.
Normally, in electrically conducting materials, the current is treated as being carried by electrons as they move through a solid.In semiconductors, it is also common to treat the current as being carried by the “holes” in the valence band.(a) Explain how holes move through a solid
A piece of sodium metal was added to a flask of water on a day when the atmospheric pressure was 757.5 Torr. The sodium reacted completely with the water to produce 137.0 mL of a mixture of hydrogen gas and water vapor at 24°C, at which temperature the vapor pressure of water is 22.38
Predict how each of the following properties of a liquid changes as the temperature increases and explain your reasoning:(a) Boiling point;(b) Viscosity;(c) Surface tension.
The pressure recorded for an argon gas cylinder is 35.0 lb · in.–2. Convert this pressure into(a) kPa;(b) Torr;(c) Bar;(d) Atm.
If you were designing an air-conditioning system in which a cooling effect is achieved by the expansion of a gas, you might need to assess the pressure changes of the gas as it underwent changes in both temperature and volume. A sample of gas of volume 500. mL at 28.0°C was found to exert a
The following data were collected for a gas sample consisting of 1.00 mol of molecules in a rigid container.(a) Determine the volume of the sample.(b) Plot the data either by hand or using a spreadsheet. Now suppose you add an additional 1.00 mol of gas molecules into the same volume. Plot the
Through a series of photochemical and enzymatic steps, carbon dioxide and water participate in photosynthesis to produce glucose and oxygen according to the equationGiven that the partial pressure of carbon dioxide in the troposphere is 0.26 Torr and that the temperature is 25°C, calculate the
What is the molecular formula of a compound of empirical formula CH that diffuses 1.24 times more slowly than krypton at the same temperature and pressure?
Two identical flasks are each filled with a gas at 20°C and 100 atm. One flask contains NH3 and the other an equal amount of H2.(a) In which flask do the molecules have the greater root mean square speed?(b) In which flask are the deviations from ideality stronger? Explain your reasoning.

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