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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

Give the bond order for each bond in the followingmolecules or ions:(a) CN−(b) CH3CN(c) SO3(d) CH3CH=CH2
In each pair of bonds, predict which is shorter.(a) B—Cl or Ga—Cl(b) Sn—O or C—O(c) P—S or P—O(d) C=O or C=N
In each pair of bonds, predict which is shorter.(a) Si—N or Si—O(b) Si—O or C—O(c) C—F or C—Br(d) The C—N bond or the CΞN bond in H2NCH2CΞN
Consider the nitrogen–oxygen bond lengths in NO2+, NO2−, and NO3−. In which ion is the bond predicted to be longest? In which is it predicted to be the shortest? Explain briefly
Hydrogenation reactions, which involve the addition of H2 to a molecule, are widely used in industry to transform one compound into another. For example, 1-butene (C4H8) is converted to butane
Ethanol can be made by the reaction of ethylene and water:Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Compare the value obtained to the value calculated from
Compare the carbon–oxygen bond lengths in the formate ion (HCO2−), in methanol (CH3OH), and in the carbonate ion (CO32−). In which species is the carbon–oxygen bond predicted to be longest?
Methanol can be made by partial oxidation of methane using O2 in the presence of a catalyst:Use bond dissociation enthalpies to estimate the enthalpy change for this reaction. Compare the value
Phosgene, Cl2CO, is a highly toxic gas that was used as a weapon in World War I. Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for the reaction of carbon monoxide
Consider the carbon–oxygen bond in formaldehyde (CH2O) and carbon monoxide (CO). In which molecule is the CO bond shorter? In which molecule is the CO bond stronger?
Oxygen atoms can combine with ozone to form oxygen:Using ΔrH° and the bond dissociation enthalpy data in Table 8.8, estimate the bond dissociation enthalpy for the oxygen–oxygen bond in ozone,
The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water:Using bond dissociation enthalpies, calculate the bond dissociation enthalpy of the O—F bond in OF2.
In boron compounds, the B atom often is not surrounded by four valence electron pairs. Illustrate this with BCl3. Show how the molecule can achieve an octet configuration by forming a coordinate
Which of the following compounds or ions do not have an octet of electrons surrounding the central atom: BF4−, SiF4, SeF4, BrF4−, XeF4?
In which of the following does the central atom obey the octet rule: NO2, SF4, NH3, SO3, ClO2, and ClO2−? Are any of these species odd-electron molecules or ions?
To estimate the enthalpy change for the reactionwhat bond dissociation enthalpies do you need? Outline the calculation, being careful to show correct algebraic signs. O₂(g) + 2 H₂(g) → 2
Draw resonance structures for the formate ion, HCO2− and then determine the C—O bond order in the ion.
Consider a series of molecules in which carbon is attached by single covalent bonds to atoms of second-period elements: C—O, C—F, C—N, C—C, and C—B. Place these bonds in order of increasing
Draw resonance structures for the SO2 molecule, and determine the formal charges on the S and O atoms. Are the S—O bonds polar, and is the molecule as a whole polar? If so, what is the direction of
What is the principle of electroneutrality? Use this rule to exclude a possible resonance structure of CO2.
Draw Lewis structures (and resonance structures where appropriate) for the following molecules and ions. What similarities and differences are there in this series?(a) CO2(b) N3−(c) OCN−
The equation for the combustion of gaseous methanol is(a) Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for this reaction. What is the enthalpy of combustion of
Which has the greater O—N—O bond angle, NO2− or NO2+? Explain briefly.
Dinitrogen monoxide, N2O, can decompose to nitrogen and oxygen gas:Use bond dissociation enthalpies to estimate the enthalpy change for this reaction. 2 N₂O(g) → 2 N₂(g) + O₂(g)
Compare the F—Cl—F angles in ClF2+ and ClF2−. Using Lewis structures, determine the approximate bond angle in each ion. Which ion has the greater bond angle?
Vanillin is the flavoring agent in vanilla extract and in vanilla ice cream. Its structure is shown here:(a) Give values for the three bond angles indicated.(b) Indicate the shortest carbon–oxygen
Acrylonitrile, C3H3N, is the building block of the synthetic fiber Orlon.(a) Give the approximate values of angles 1, 2, and 3.(b) Which is the shorter carbon–carbon bond?(c) Which is the stronger
Draw an electron dot structure for the cyanide ion, CN−. In aqueous solution, this ion interacts with H+ to form the acid. Should the acid formula be written as HCN or CNH?
The cyanate ion, OCN−, has the least electronegative atom, C, in the center. The unstable fulminate ion, CNO−, has the same molecular formula, but the N atom is in the center.(a) Draw the three
The formula for nitryl chloride is ClNO2 (in which N is the central atom).(a) Draw the Lewis structure for the molecule, including all resonance structures.(b) What is the N—O bond order?(c)
Explain why(a) XeF2 has a linear molecular structure and not a bent one.(b) ClF3 has a T-shaped structure and not a trigonal-planar one.
Amides are an important class of organic molecules. They are usually drawn as sketched here, but another resonance structure is possible.(a) Draw a second resonance structure of the structure above.
The molecule shown here, 2-furylmethanethiol, is responsible for the aroma of coffee:(a) What are the formal charges on the S and O atoms?(b) Give approximate values of angles 1, 2, and 3.(c) Which
Use the bond dissociation enthalpies in Table 8.8 to estimate the enthalpy change for the decomposition of urea to hydrazine, H2N—NH2, and carbon monoxide. (Assume all compounds are in the gas
Dihydroxyacetone is a component of quick tanning lotions. (It reacts with the amino acids in the upper layer of skin and colors them brown in a reaction similar to that occurring when food is browned
Molecules in space:(a) In addition to molecules such as CO, HCl, H2O, and NH3, glycolaldehyde has been detected in outer space. Is the molecule polar?(b) Where do the positive and negative charges
Acrolein is used to make plastics. Suppose this compound can be prepared by inserting a carbon monoxide molecule into the C—H bond of ethylene.(a) Which is the stronger carbon–carbon bond in
The molecule pictured below is epinephrine, a compound used as a bronchodilator and antiglaucoma agent.(a) Give a value for each of the indicated bond angles.(b) What are the most polar bonds in the
It is possible to draw three resonance structures for HNO3, one of which contributes much less to the resonance hybrid than the other two. Sketch the three resonance structures, and assign a formal
You are doing an experiment in the laboratory and want to prepare a solution in a polar solvent. Which solvent would you choose, methanol (CH3OH) or toluene (C6H5CH3)? Explain your choice.
Uracil is one of the bases in RNA, a close relative of DNA.(a) What are the values of the O—C—N and C—N—H angles?(b) There are two carbon–carbon bonds in the molecule. Which is predicted to
Guanine is present in both DNA and RNA.(a) What is the most polar bond in the molecule?(b) What is the N–C=N angle in the 6-member ring?(c) What is the N–C=N angle in the 5-member ring?(d) What
Methylacetamide, CH3CONHCH3, is a small molecule with an amide link (CO—NH), the group that binds one amino acid to another in proteins.(a) Is this molecule polar?(b) Where do you expect the
A paper published in the research journal Science in 2007 (S. Vallina and R. Simo, Science, Vol. 315, p. 506, January 26, 2007) reported studies of dimethylsulfide (DMS), an important greenhouse gas
Bromine-containing species play a role in environmental chemistry. For example, they are evolved in volcanic eruptions.(a) The following molecules are important in bromine environmental chemistry:
Acrylamide, H2C=CHCONH2, is a known neurotoxin and possible carcinogen. It was a shock to all consumers of potato chips and french fries a few years ago when it was found to occur in those
Draw the Lewis structure for chloroform, CHCl3. What are its electron-pair and molecular geometries? What orbitals on C, H, and Cl overlap to form bonds involving these elements?
Draw the Lewis structure for NF3. What are its electron-pair and molecular geometries? What is the hybridization of the nitrogen atom? What orbitals on N and F overlap to form bonds between these
Draw the Lewis structure for hydroxylamine, H2NOH. What is the hybridization for nitrogen and oxygen in this molecule? What orbitals overlap to form the bond between nitrogen and oxygen?
Draw the Lewis structure for 1,1-dimethylhydrazine [(CH3)2NNH2, a compound used as a rocket fuel]. What is the hybridization for the two nitrogen atoms in this molecule? What orbitals overlap to form
A line in the Balmer series of emission lines of excited H atoms has a wavelength of 410.2 nm (Figure 6.10). What color is the light emitted in this transition? What quantum levels are involved in
A table wine has a pH of 3.40. What is the hydronium ion concentration of the wine? Is it acidic or basic?
Make the following conversions. In each case, tell whether the solution is acidic or basic. Data given in Example 4.8 (a) (b) (c) (d) pH 5.25 [H3O+] 6.7 x 10-10 M 2.2 x 10-6 M 2.5 x 10-² M
Two students titrate different samples of the same solution of HCl using 0.100 M NaOH solution and phenolphthalein indicator (Figure 4.12). The first student pipets 20.0 mL of the HCl solution into a
Two beakers sit on a balance; the total mass is 167.170 g. One beaker contains a solution of KI; the other contains a solution of Pb(NO3)2. When the solution in one beaker is poured completely into
What determines the directionality of energy transfer as heat?
Ethanol, C2H5OH, boils at 78.29°C. How much energy, in joules, is required to raise the temperature of 1.00 kg of ethanol from 20.0°C to the boiling point and then to change the liquid to vapor at
Write a balanced chemical equation for the formation of CH3OH(ℓ) from the elements in their standard states. Find the value for ∆fH° for CH3OH(ℓ) in Appendix L.Data given in Appendix L
Write a balanced chemical equation for the formation of CaCO3(s) from the elements in their standard states. Find the value for ∆fH° for CaCO3(s) in Appendix L.
(a) Write a balanced chemical equation for the formation of 1 mol of Cr2O3(s) from Cr and O2 in their standard states. (Find the value for ∆fH° for Cr2O3(s) in Appendix L.) (b) What is the
Use Appendix L to find the standard enthalpies of formation of oxygen atoms, oxygen molecules (O2), and ozone (O3). What is the standard state of oxygen? Is the formation of oxygen atoms from O2
Three 45-g ice cubes at 0°C are dropped into 5.00 × 102 mL of tea to make iced tea. The tea was initially at 20.0°C; when thermal equilibrium was reached, the final temperature was 0°C. How much
Peanuts and peanut oil are organic materials and burn in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume
Suppose that an inch (2.54 cm) of rain falls over a square mile of ground (2.59 × 106 m2). (Density of water is 1.0 g/cm3.) The enthalpy of vaporization of water at 25°C is 44.0 kJ/mol. How much
Isomers are molecules with the same elemental composition but a different atomic arrangement. Three isomers with the formula C4H8 are shown in the models below. The enthalpy of combustion (∆cH°)
Several standard enthalpies of formation (from Appendix L) are given below. Use these data to calculate(a) The standard enthalpy of vaporization of bromine. (b) The energy required for the reaction
When 0.850 g of Mg was burned in oxygen in a constant-volume calorimeter, 25.4 kJ of energy as heat was evolved. The calorimeter was in an insulated container with 750. g of water at an initial
Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation
A piece of gold (10.0 g, CAu = 0.129 J/g ∙ K) is heated to 100.0°C. A piece of copper (also 10.0 g, CCu = 0.385 J/g ∙ K) is chilled in an ice bath to 0°C. Both pieces of metal are placed in a
Calculate ∆rH° for the reaction 2 C(s) + 3 H₂(g) + ¹/2O₂(g) given the information below. C(s) + 0₂(g) → CO₂(g) A,Hº = -393.5 kJ/mol-rxn 2 H₂(g) + O₂(g) → 2
You have the six pieces of metal listed below, plus a beaker of water containing 3.00 × 102 g of water. The water temperature is 21.00°C.(a) In your first experiment you select one piece of metal
In the lab, you plan to carry out a calorimetry experiment to determine ∆rH for the exothermic reaction of Ca(OH)2(s) and HCl(aq). Predict how each of the following will affect the calculated value
Answer the following questions based on Figure 6.2: (a) Which type of radiation involves less energy, x-rays or microwaves? (b) Which radiation has the higher frequency, radar or red light? (c)
Sublimation of 1.0 g of dry ice, CO2(s), forms 0.36 L of CO2(g) (at −78°C and 1.01 × 105 Pa). The expanding gas can do work on the surroundings. Calculate the amount of work done on the
In the reaction of two moles of gaseous hydrogen and one mole of gaseous oxygen to form two moles of gaseous water vapor, two moles of products are formed from three moles of reactants. If this
Traffic signals are often now made of LEDs (lightemitting diodes). Amber and green ones are pictured here. (a) The light from an amber signal has a wavelength of 595 nm, and that from a green signal
Consider the colors of the visible spectrum. (a) Which colors of light involve less energy than green light? (b) Which color of light has photons of greater energy, yellow or blue?(c) Which color
Suppose you are standing 225 m from a radio transmitter. What is your distance from the transmitter in terms of the number of wavelengths if (a) The station is broadcasting at 1150 kHz (on the AM
Green light has a wavelength of 5.0 × 102 nm. What is the energy, in joules, of one photon of green light? What is the energy, in joules, of 1.0 mol of photons of green light?
Violet light has a wavelength of about 410 nm. What is its frequency? Calculate the energy of one photon of violet light. What is the energy of 1.0 mol of violet photons? Compare the energy of
The most prominent line in the emission spectrum of aluminum is at 396.15 nm. What is the frequency of this line? What is the energy of one photon with this wavelength? Of 1.00 mol of these photons?
The most prominent line in the emission spectrum of magnesium is 285.2 nm. Other lines are found at 383.8 and 518.4 nm. In what region of the electromagnetic spectrum are these lines found? Which is
Place the following types of radiation in order of increasing energy per photon: (a) Yellow light from a sodium lamp (b) X-rays from an instrument in a dentist’s office (c) Microwaves in a
Place the following types of radiation in order of increasing energy per photon: (a) Radiation within a microwave oven(b) Your favorite radio station(c) Gamma rays from a nuclear reaction(d) Red
The most prominent line in the spectrum of mercury is at 253.652 nm. Other lines are located at 365.015 nm, 404.656 nm, 435.833 nm, and 1013.975 nm. (a) Which of these lines represents the most
An energy of 3.3 × 10−19 J/atom is required to cause a cesium atom on a metal surface to lose an electron. Calculate the longest possible wavelength of light that can ionize a cesium atom. In what
The most prominent line in the spectrum of neon is found at 865.438 nm. Other lines are located at 837.761 nm, 878.062 nm, 878.375 nm, and 885.387 nm. (a) In what region of the electromagnetic
You are an engineer designing a switch that works by the photoelectric effect. The metal you wish to use in your device requires 6.7 × 10−19 J/atom to remove an electron. Will the switch work if
Consider only transitions involving the n = 1 through n = 5 energy levels for the H atom (see Figures 6.7 and 6.10). (a) How many emission lines are possible, considering only the five quantum
What are the wavelength and frequency of the radiation involved in the least energetic emission line in the Lyman series? What are the values of ninitial and nfinal?
Consider only transitions involving the n = 1 through n = 4 energy levels for the hydrogen atom (see Figures 6.7 and 6.10).(a) How many emission lines are possible, considering only the four quantum
The energy emitted when an electron moves from a higher energy state to a lower energy state in any atom can be observed as electromagnetic radiation. (a) Which involves the emission of less energy
If energy is absorbed by a hydrogen atom in its ground state, the atom is excited to a higher energy state. For example, the excitation of an electron from n = 1 to n = 3 requires radiation with a
Calculate the wavelength and frequency of light emitted when an electron changes from n = 3 to n = 1 in the H atom. In what region of the spectrum is this radiation found?
Calculate the wavelength and frequency of light emitted when an electron changes from n = 4 to n = 3 in the H atom. In what region of the spectrum is this radiation found?
An electron moves with a velocity of 2.5 × 108 cm/s. What is its wavelength?
A beam of electrons (m = 9.11 × 10−31 kg/electron) has an average speed of 1.3 × 108 m/s. What is the wavelength of electrons having this average speed?
Calculate the wavelength, in nanometers, associated with a 46-g golf ball moving at 30. m/s (about 67 mph). At what speed must the ball travel to have a wavelength of 5.6 × 10−3 nm?
A rifle bullet (mass = 1.50 g) has a velocity of 7.00 × 102 mph (miles per hour). What is the wavelength associated with this bullet?
(a) When n = 4, what are the possible values of ℓ?(b) When ℓ is 2, what are the possible values of mℓ?(c) For a 4s orbital, what are the possible values of n, ℓ, and mℓ?(d) For a 4f

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