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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

Give the electron configurations for the ions Li2+ and Li2− in molecular orbital terms. Compare the Li—Li bond order in these ions with the bond order in Li2.
When potassium and oxygen react, one of the products obtained is potassium superoxide, KO2. The anion in this compound is the superoxide ion, O2−. Write the electron configuration for this ion in
Calcium carbide, CaC2, contains the acetylide ion, C22−. Sketch the molecular orbital energy level diagram for the ion and the electron dot structure.(a) How many net σ and π bonds does the ion
Platinum hexafluoride is an extremely strong oxidizing agent. It can even oxidize oxygen, its reaction with O2 giving O2+PtF6−. Sketch the molecular n orbital energy level diagram for the O2+ ion.
When sodium and oxygen react, one of the products obtained is sodium peroxide, Na2O2. The anion in this compound is the peroxide ion, O22−. Write the electron configuration for this ion in
Among the following, which has the shortest bond and which has the longest: Li2, B2, C2, N2, O2?
Assume the energy level diagram shown in Figure 9.16 can be applied to the heteronuclear molecule ClO.(a) Write the electron configuration for chlorine monoxide, ClO.(b) What is the highest-energy,
The nitrosyl ion, NO+, has an interesting chemistry. Assume the molecular orbital diagram shown in Figure 9.16 applies to NO+.(a) Is NO+ diamagnetic or paramagnetic? If paramagnetic, how many
Consider the following list of small molecules and ions: C2, O2−, CN−, O2, CO, NO, NO+, C22−, OF−.Identify(a) All species that have a bond order of 3(b) All species that are paramagnetic(c)
Draw the Lewis structure for AlF4−. What are its electron-pair and molecular geometries? What orbitals on Al and F overlap to form bonds between these elements? What are the formal charges on the
What is the O—S—O angle and the hybrid orbital set used by sulfur in each of the following molecules or ions?(a) SO2(b) SO3(c) SO32−(d) SO42−
Sketch the resonance structures for the nitrate ion, NO3−. Is the hybridization of the N atom the same or different in each structure? Describe the orbitals involved in bond formation by the
Numerous molecules are detected in deep space. Three of them are illustrated here.(a) Are these compounds isomers?(b) Indicate the hybridization of each C atom in each molecule.(c) What is the value
Sketch the resonance structures for the N2O molecule. Is the hybridization of the N atoms the same or different in each structure? Describe the orbitals involved in bond formation by the central N
Acrolein, a component of photochemical smog, has a pungent odor and irritates eyes and mucous membranes.(a) What are the hybridizations of carbon atoms 1 and 2?(b) What are the approximate values of
Compare the structure and bonding in CO2 and CO32− with regard to the O—C—O bond angles, the CO bond order, and the C atom hybridization.
The organic compound below is a member of a class known as oximes.(a) What are the hybridizations of the two C atoms and of the N atom?(b) What is the approximate C—N—O angle? Η :0-H H=C=C=N: Η
The compound sketched below is acetylsalicylic acid, commonly known as aspirin.(a) What are the approximate values of the angles marked A, B, C, and D?(b) What hybrid orbitals are used by carbon
Phosphoserine is a less-common amino acid.(a) Identify the hybridizations of atoms 1 through 5.(b) What are the approximate values of the bond angles A, B, C, and D?(c) What are the most polar bonds
Lactic acid is a natural compound found in sour milk.(a) How many π bonds occur in lactic acid? How many σ bonds?(b) What is the hybridization of atoms 1, 2, and 3?(c) Which CO bond is the shortest
Cinnamaldehyde occurs naturally in cinnamon oil.(a) What is the most polar bond in the molecule?(b) How many σ bonds and how many π bonds are there?(c) Is cis-trans isomerism possible? If so, draw
The simple valence bond picture of O2 does not agree with the molecular orbital view. Compare these two theories with regard to the peroxide ion, O22−.(a) Draw an electron dot structure for O22−.
Which of the following molecules or ions are paramagnetic? What is the highest occupied molecular orbital (HOMO) in each one? Assume the molecular orbital diagram in Figure 9.16 applies to all of
The CN molecule has been found in interstellar space. Assuming the electronic structure of the molecule can be described using the molecular orbital energy level diagram in Figure 9.16, answer the
Nitrogen, N2, can ionize to form N2+ or add an electron to give N2−. Using molecular orbital theory, compare these species with regard to(a) Their magnetic character, (b) Net number of π
Which of the homonuclear, diatomic molecules of the second-period elements (from Li2 to Ne2) are paramagnetic? Which have a bond order of 1? Which have a bond order of 2? Which diatomic molecule has
The structure of amphetamine, a stimulant, is shown below. (Replacing one H atom on the NH2, or amino, group with CH3 gives methamphetamine, a particularly dangerous drug commonly known as
Menthol is used in soaps, perfumes, and foods. It is present in the common herb mint, and it can be prepared from turpentine.(a) What are the hybridizations used by the C atoms in the molecule?(b)
Suppose you carry out the following reaction of ammonia and boron trifluoride in the laboratory.(a) What is the geometry of the boron atom in BF3? In H3N→BF3?(b) What is the hybridization of the
Ethylene oxide is an intermediate in the manufacture of ethylene glycol (antifreeze) and polyester polymers. More than 4 million tons are produced annually in the United States. The molecule has a
The elements of the second period from boron to oxygen form compounds of the type XnE—EXn, where X can be H or a halogen. Sketch possible Lewis structures for B2F4, C2H4, N2H4, and O2H2. Give the
The compound whose structure is shown here is acetylacetone. It exists in two forms: the enol form and the keto form.The molecule reacts with OH− to form an anion,[CH3COCHCOCH3]− (often
The sulfamate ion, H2NSO3−, can be thought of as having been formed from the amide ion, NH2−, and sulfur trioxide, SO3.(a) What are the electron-pair and molecular geometries of the amide ion and
Draw the two resonance structures that describe the bonding in the acetate ion. What is the hybridization of the carbon atom of the —CO2− group? Select one of the two resonance structures and
Carbon dioxide (CO2), dinitrogen monoxide (N2O), the azide ion (N3−), and the cyanate ion (OCN−) have the same geometry and the same number of valence shell electrons. However, there are
Draw the two resonance structures that describe the bonding in SO2. Then describe the bonding in this compound using MO theory. How does MO theory rationalize the bond order of 1.5 for the two S—O
When two amino acids react with each other, they form a linkage called an amide group, or a peptide link. (If more linkages are added, a protein or polypeptide is formed.)(a) What are the
Draw a Lewis structure for diimide, H—NP=OH. Then, using valence bond theory, describe the bonding in this compound. What orbitals overlap to form the bond between nitrogen atoms in this compound?
What is the maximum number of hybrid orbitals that a carbon atom may form? What is the minimum number? Explain briefly.
Consider the three fluorides BF4−, SiF4, and SF4.(a) Identify a molecule that is isoelectronic with BF4−.(b) Are SiF4 and SF4 isoelectronic?(c) What is the hybridization of the central atom in
Three of the four π molecular orbitals for cyclobutadiene are pictured here. Place them in order of increasing energy. (See Figures 9.13, 9.15, 9.16, and 9.18 and the relation of orbital energy and
What is the connection between bond order, bond length, and bond energy? Use ethane (C2H6), ethylene (C2H4), and acetylene (C2H2) as examples.
When is it desirable to use MO theory rather than valence bond theory?
Show how valence bond theory and molecular orbital theory rationalize the O—O bond order of 1.5 in ozone.
Borax has the molecular formula Na2B4O5(OH)4. The structure of the anion in this compound is shown below. What is the electron pair geometry and molecular geometry surrounding each of the boron atoms
Let’s look more closely at the process of hybridization.(a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them?(b) Do
A model of the organic compound allene is shown below.(a) Explain why the allene molecule is not flat. That is, explain why the CH2 groups at opposite ends do not lie in the same plane.(b) What is
Melamine is an important industrial chemical, used to make fertilizers and plastics.(a) The carbon-nitrogen bond lengths in the ring are all the same length (about 140 pm). Explain.(b) Melamine is
Should the energy required to break one of the H—F bonds in HF2− (HF2− → HF + F−) be greater than, less than, or the same as the energy required to break the bond in HF (HF→ H+ F).
The following problem is taken from the Theoretical Examination of the 44th annual International Chemistry Olympiad in 2012, a competition attended by four secondary school students from each of
Bromine forms a number of oxides of varying stability.(a) One oxide has 90.90% Br and 9.10% O. Assuming its empirical and molecular formulas are the same, draw a Lewis structure of the molecule and
Urea reacts with malonic acid to produce barbituric acid, a member of the class of compounds called phenobarbitals, which are widely prescribed as sedatives.(a) What bonds are broken and what bonds
The pressure of a gas is 440 mm Hg. Express this pressure in units of(a) Atmospheres, (b) Bars, and(c) Kilopascals.
The average barometric pressure at an altitude of 10 km is 210 mm Hg. Express this pressure in atmospheres, bars, and kilopascals.
Indicate which represents the higher pressure in each of the following pairs:(a) 534 mm Hg or 0.754 bar(b) 534 mm Hg or 650 kPa(c) 1.34 bar or 934 kPa
Put the following in order of increasing pressure: 363 mm Hg, 363 kPa, 0.256 atm, and 0.523 bar.
A sample of nitrogen gas has a pressure of 67.5 mm Hg in a 500.-mL flask. What is the pressure of this gas sample when it is transferred to a 125-mL flask at the same temperature?
A 5.0-mL sample of CO2 gas is enclosed in a gastight syringe (Figure 10.2) at 22°C. If the syringe is immersed in an ice bath (0°C), what is the new gas volume, assuming that the pressure is held
A sample of CO2 gas has a pressure of 56.5 mmHg in a 125-mL flask. The sample is transferred to a new flask, where it has a pressure of 62.3 mmHg at the same temperature. What is the volume of the
You have 3.5 L of NO at a temperature of 22.0°C. What volume would the NO occupy at 37°C? (Assume the pressure is constant.)
You have 3.6 L of H2 gas at 380 mm Hg and 25°C. What is the pressure of this gas if it is transferred to a 5.0-L flask at 0.0°C?
You have a sample of CO2 in flask A with a volume of 25.0 mL. At 20.5°C, the pressure of the gas is 436.5 mm Hg. To find the volume of another flask, B, you move the CO2 to that flask and find that
You have a sample of gas in a flask with a volume of 250 mL. At 25.5°C, the pressure of the gas is 360 mm Hg. If you decrease the temperature to −5.0°C, what is the gas pressure at the lower
A sample of gas occupies 135 mL at 22.5°C; the pressure is 165 mm Hg. What is the pressure of the gas sample when it is placed in a 252-mL flask at a temperature of 0.0°C?
Ammonia gas is synthesized by combining hydrogen and nitrogen:(a) If you want to produce 562 g of NH3, what volume of H2 gas, at 56°C and 745 mm Hg, is required?(b) Nitrogen for this reaction will
Nitrogen trifluoride is prepared by the reaction of ammonia and fluorine.If you mix NH3 with F2 in the correct stoichiometric ratio, and if the total pressure of the mixture is 120 mm Hg, what are
Chlorine trifluoride, ClF3, is a valuable reagent because it can be used to convert metal oxides to metal fluorides:(a) What mass of NiO will react with ClF3 gas if the gas has a pressure of 250 mm
Relative humidity is the ratio of the partial pressure of water in air at a given temperature to the vapor pressure of water at that temperature. Calculate the mass of water per liter of air under
What mass of water vapor is present in a dormitory room when the relative humidity is 55% and the temperature is 23°C? The dimensions of the room are 4.5 m2 floor area and 3.5 m ceiling height. (See
You have a 550.-mL tank of gas with a pressure of 1.56 atm at 24°C. You thought the gas was pure carbon monoxide gas, CO, but you later found it was contaminated by small quantities of gaseous CO2
Methane is burned in a laboratory Bunsen burner to give CO2 and water vapor. Methane gas is supplied to the burner at the rate of 5.0 L/min (at a temperature of 28°C and a pressure of 773 mm Hg). At
Group 2A metal carbonates are decomposed to the metal oxide and CO2 on heating:You heat 0.158 g of a white, solid carbonate of a Group 2A metal (M) and find that the evolved CO2 has a pressure of
Iron forms a series of compounds of the type Fex(CO)y. In air, these compounds are oxidized to Fe2O3 and CO2 gas. After heating a 0.142-g sample of Fex(CO)y in air, you isolate the CO2 in a 1.50-L
One way to synthesize diborane, B2H6, is the reaction(a) If you have 0.136 g of NaBH4 and excess H3PO4, and you collect the resulting B2H6 in a 2.75-L flask at 25°C, what is the pressure of the
You are given a solid mixture of NaNO2 and NaCl and are asked to analyze it for the amount of NaNO2 present. To do so, you allow the mixture to react with sulfamic acid, HSO3NH2, in water according
You have 1.249 g of a mixture of NaHCO3 and Na2CO3. You find that 12.0 mL of 1.50 M HCl is required to convert the sample completely to NaCl, H2O, and CO2.What volume of CO2 is evolved at 745 mm Hg
A mixture of NaHCO3 and Na2CO3 has a mass of 2.50 g. When treated with HCl(aq), 665 mL of CO2 gas is liberated with a pressure of 735 mmHg at 25°C. What is the weight percent of NaHCO3 and Na2CO3 in
Many nitrate salts can be decomposed by heating. For example, blue, anhydrous copper(II) nitrate produces the gases nitrogen dioxide and oxygen when heated. In the laboratory, you find that a sample
A compound containing C, H, N, and O is burned in excess oxygen. The gases produced by burning 0.1152 g are first treated to convert the nitrogen-containing product gases into N2, and then the
You have a gas, one of the three known phosphorus–fluorine compounds (PF3, PF5, and P2F4). To find out which, you have decided to measure its molar mass.(a) First, you determine that the density of
A 1.50 L constant-volume calorimeter (Figure 5.12) contains C3H8(g) and O2(g). The partial pressure of C3H8 is 0.10 atm and the partial pressure of O2 is 5.0 atm. The temperature is 20.0°C. A
A 1.0-L flask contains 10.0 g each of O2 and CO2 at 25°C.(a) Which gas has the greater partial pressure, O2 or CO2, or are they the same?(b) Which molecules have the greater rms speed, or are they
If equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false.(a) The pressure
Which of the following compounds would be expected to form intermolecular hydrogen bonds in the liquid state?(a) CH3OCH3 (dimethyl ether)(b) CH4(c) HF(d) CH3CO2H (acetic acid)(e) Br2(f) CH3OH
Which of the following compounds would be expected to form intermolecular hydrogen bonds in the liquid state?(a) H2Se(b) HCO2H (formic acid)(c) HI(d) acetone, (CH3)2CO 0 H-C-OH formic acid
Considering intermolecular forces in the pure substance, which of these substances exists as a gas at 25°C and 1 atm?(a) CH3CH2CH2CH3 (butane)(b) CH3OH (methanol)(c) Ar
In each pair of ionic compounds, which is more likely to have the more negative enthalpy of hydration? Briefly explain your reasoning in each case.(a) LiCl or CsCl(b) NaNO3 or Mg(NO3)2(c) RbCl or
When salts of Mg2+, Na+, and Cs+ are placed in water, the ions are hydrated. Which of these three cations is most strongly hydrated? Which one is least strongly hydrated?
Ethanol, CH3CH2OH, has a vapor pressure of 59 mm Hg at 25°C. What quantity of energy as heat is required to evaporate 125 mL of the alcohol at 25°C? The enthalpy of vaporization of the alcohol at
Answer the following questions using Figure 11.12:(a) What is the approximate equilibrium vapor pressure of water at 60°C?(b) At what temperature does water have an equilibriumvapor pressure of 600
The enthalpy of vaporization of liquid mercury is 59.11 kJ/mol. What quantity of energy as heat is required to vaporize 0.500 mL of mercury at 357°C, its normal boiling point? The density of mercury
Answer the following questions using Figure 11.12:(a) What is the equilibrium vapor pressure of diethyl ether at room temperature (approximately 20°C)?(b) Place the three compounds in Figure 11.12
Which member of each of the following pairs of compounds has the higher boiling point?(a) O2 or N2(b) SO2 or CO2(c) HF or HI(d) SiH4 or GeH4
Assume you seal 1.0 g of diethyl ether (Figure 11.12) in an evacuated 100.-mL flask. If the flask is held at 30°C, what is the approximate gas pressure in the flask? If the flask is placed in an ice
Refer to Figure 11.12 to answer these questions:(a) You heat some water to 60°C in a lightweight plastic bottle and seal the top very tightly so gas cannot enter or leave the carton. What happens
Vapor pressure curves for CS2 (carbon disulfide) and CH3NO2 (nitromethane) are drawn here.(a) What are the approximate vapor pressures of CS2 and CH3NO2 at 40°C?(b) What type(s) of intermolecular
Equilibrium vapor pressures of benzene, C6H6, at various temperatures are given in the table.(a) What is the normal boiling point of benzene?(b) Plot these data so that you have a graph resembling
Place the following four compounds in order of increasing boiling point:(a) C5H12(b) CCl4(c) C2H6(d) Ne
Vapor pressure data are given here for octane, C8H18.Use the Clausius–Clapeyron equation to calculate the molar enthalpy of vaporization of octane and its normal boiling point. Temperature (°C)
You are comparing three different substances, A, B, and C, all liquids and having similar molar masses. The vapor pressure at 25°C for substance A is less than the vapor pressure for B at this

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