Which of the following structures are isomers?

Refer to the color scheme given in Figure 3-3, and give the molecular formulas for the molecules whose balland- stick models are given here.

Give the molecular formulas for the molecules whose ball-and-stick models are given here. Refer to the color scheme in Figure 3-3.

Give the structural formulas of the molecules shown in Exercise 1 (b), (d), and (e).

Give the structural formulas of the molecules shown in Exercise 2 (b), (d), and (e).

Calculate the total number of (a) atoms in one molecule of trinitrotoluene (TNT), (b) atoms in 0.00102 mol (c) F atoms in 12.15 mol

Determine the mass, in grams, of (a) 7.34 mol (b) 3.16 * 1024 O2 molecules; (c) 18.6 mol (d) molecules of

The amino acid methionine, which is essential in human diets, has the molecular formula Determine (a) its molecular mass; (b) the number of moles of H atoms per mole of methionine; (c) the number of grams of C per mole of methionine; (d) the number of C atoms in 9.07 mol methionine.

Determine the number of moles of in a sample consisting of (a) molecules; (b) Br atoms; (c) 11.3 kg bromine; (d) 2.65 L liquid bromine

Without doing detailed calculations, explain which of the following has the greatest number of N atoms (a) 50.0 g (b) 17.0 g (c) 150 mL of liquid pyridine, (d) 1.0 mol

Without doing detailed calculations, determine which of the following has the greatest number of S atoms (a) 0.12 mol of solid sulfur, (b) 0.50 mol of gaseous (c) 65 g of gaseous (d) 75 mL of liquid thiophene,

Determine the number of moles of (a) in a 115 g sample (b) N atoms in 43.5 g of (c) N atoms in a sample of that has the same number of O atoms as 12.4 g C6H12O6

Determine the mass, in grams, of (a) mol (b) molecules of stearic acid, (c) a quantity of the amino acid lysine, containing 3.03 mol N atoms

The hemoglobin content of blood is about blood. The molar mass of hemoglobin is about and there are four iron (Fe) atoms in a hemoglobin molecule. Approximately how many Fe atoms are present in the 6 L of blood in a typical adult?

In white phosphorus, P atoms are joined into molecules (see Figure 3-5). White phosphorus is commonly supplied in chalk-like cylindrical form. Its density is For a cylinder of white phosphorus 6.50 cm long and 1.22 cm in diameter, determine (a) the number of moles of present; (b) the total number of P atoms.

Explain which of the following statement(s) is (are) correct concerning glucose (blood sugar), (a) The percentages, by mass, of C and O are the same as in CO. (b) The ratio of atoms is the same as in dihydroxyacetone, (c) The proportions, by mass, of C and O are equal. (d) The highest percentage, by mass, is that of H.

Explain which of the following statement(s) is (are) correct for sorbic acid, an inhibitor of mold and yeast. (a) It has a mass ratio of (b) It has the same mass percent composition as the aquatic herbicide, acrolein, (c) It has the same empirical formula as aspidinol, a drug used to C12H16O4 , kill parasitic worms. C3H4O. C:H:O 3 : 4 : 1. C6H8O2 , (CH2OH)2CO. C:H:O C6H12O6 . (d) It has four times as many H atoms as O atoms, but four times as much O as H by mass.

For the mineral torbernite, determine (a) the total number of atoms in one formula unit (b) the ratio, by number, of H atoms to O atoms (c) the ratio, by mass, of Cu to P (d) the element present in the greatest mass percent (e) the mass required to contain 1.00 g P

For the compound determine (a) the total number of atoms in one formula unit (b) the ratio, by number, of C atoms to H atoms (c) the ratio, by mass, of Ge to S (d) the number of g S in 1 mol of the compound (e) the number of C atoms in 33.10 g of the Compound

Determine the mass percent H in the hydrocarbon decane,

Determine the mass percent O in the mineral malachite,

Determine the mass percent H in the hydrocarbon isooctane,

Determine the mass percent in the hydrate

Determine the mass percent of each of the elements in the antimalarial drug quinine,

Determine the mass percent of each of the elements in the fungicide copper(II) oleate,

Determine the percent, by mass, of the indicated element: (a) Pb in tetraethyl lead, once extensively used as an additive to gasoline to prevent engine knocking Pb(C2H5)4 , Cu(C18H33O2)2 . C20H24N2O2 . Cr(NO3)3 # 9 H2O. H2O C(CH3)3CH2CH(CH3)2 . Cu2(OH)2CO3 . C10H22 . (b) Fe in Prussian blue, a pigment used in paints and printing inks (c) Mg in chlorophyll, the green pigment in plant cells

All of the following minerals are semiprecious or precious stones. Determine the mass percent of the indicated element. (a) Zr in zircon, (b) Be in beryl (emerald), (c) Fe in almandine (garnet), (d) S in lazurite (lapis lazuli),

Without doing detailed calculations, arrange the following in order of increasing % Cr, by mass, and explain your reasoning: CrO,

Without doing detailed calculations, explain which of the following has the greatest mass percent of sulfur: SO2 , S2Cl2 , Na2S, Na2S2O3 , or CH3CH2SH.

Two oxides of sulfur have nearly identical molecular masses. One oxide consists of 40.05% S. What are the simplest possible formulas for the two oxides?

An oxide of chromium used in chrome plating has a formula mass of 100.0 u and contains four atoms per formula unit. Establish the formula of this compound, with a minimum of calculation.

Diethylene glycol, used to deice aircraft, is a carbon hydrogen oxygen compound with 45.27% C and 9.50% H by mass. What is its empirical formula?

The food flavor enhancer monosodium glutamate (MSG) has the composition 13.6% Na, 35.5% C, 4.8% H, 8.3% N, 37.8% O, by mass. What is the empirical formula of MSG?

Determine the empirical formula of (a) the rodenticide (rat killer) warfarin, which consists of 74.01% C, 5.23% H, and 20.76% O, by mass; (b) the antibacterial agent sulfamethizole, which consists of 39.98% C, 3.73% H, 20.73% N, 11.84% O, and 23.72% S, by mass.

Determine the empirical formula of (a) benzo-[a]pyrene, a suspected carcinogen found in cigarette smoke, consisting of 95.21% C and 4.79% H, by mass; (b) hexachlorophene, used in germicidal soaps, which consists of 38.37% C, 1.49% H, 52.28% Cl, and 7.86% O by mass.

A compound of carbon and hydrogen consists of 94.34% C and 5.66% H, by mass. The molecular mass of the compound is found to be 178 u. What is its molecular formula?

Selenium, an element used in the manufacture of photoelectric cells and solar energy devices, forms two oxides. One has 28.8% O, by mass, and the other, 37.8% O. What are the formulas of these oxides? Propose acceptable names for them.

Indigo, the dye for blue jeans, has a percent composition, by mass, of 73.27% C, 3.84% H, 10.68% N, and the remainder is oxygen. The molecular mass of indigo is 262.3 u. What is the molecular formula of indigo?

Adenine, a component of nucleic acids, has the mass percent composition: 44.45% C, 3.73% H, 51.82% N. Its molecular mass is 135.14 u. What is its molecular formula?

The element X forms the chloride containing 75.0% Cl, by mass. What is element X?

The element X forms the compound containing 59.6% Cl. What is element X?

Chlorophyll contains 2.72% Mg by mass. Assuming one Mg atom per chlorophyll molecule, what is the molecular mass of chlorophyll?

Two compounds of Cl and X are found to have molecular masses and % Cl, by mass, as follows: 137 u, 77.5% Cl; 208 u, 85.1% Cl. What is element X? What is the formula for each compound?

A0.1888 g sample of a hydrocarbon produces 0.6260 g and 0.1602 g in combustion analysis. Its molecular mass is found to be 106 u. For this hydrocarbon, determine its (a) mass percent composition; (b) empirical formula; (c) molecular formula.

Para-cresol (p-cresol) is used as a disinfectant and in the manufacture of herbicides. A 0.4039 g sample of this carbon hydrogen oxygen compound yields 1.1518 g and 0.2694 g in combustion analysis. Its molecular mass is 108.1 u. For p-cresol, determine its (a) mass percent composition; (b) empirical formula; (c) molecular formula.

Dimethylhydrazine is a carbon hydrogen nitrogen compound used in rocket fuels. When burned in an excess of oxygen, a 0.312 g sample yields 0.458 g and 0.374 g The nitrogen content of a 0.486 g sample is converted to 0.226 g What is the empirical formula of dimethylhydrazine?

The organic solvent thiophene is a carbon hydrogen sulfur compound that yields and when burned in an excess of oxygen. When subjected CO2 , H2O, SO2 N2 . H2O. CO2 CO2 H2O CO2 H2O to combustion analysis, a 1.3020 g sample of thiophene produces 2.7224 g 0.5575 g and 0.9915 g What is the empirical formula of thiophene?

Without doing detailed calculations, explain which of these compounds produces the greatest mass of when 1.00 mol of the compound is burned in an excess of oxygen:

Without doing detailed calculations, explain which of these compounds produces the greatest mass of when 1.00 g of the compound is burned in an excess of oxygen:

A1.562 g sample of the alcohol is burned in an excess of oxygen. What masses of and should be obtained?

Liquid ethyl mercaptan, has a density of 0.84 g/mL. Assuming that the combustion of this compound produces only and what masses of each of these three products would be produced in the combustion of 3.15 mL of ethyl mercaptan?

Indicate the oxidation state of the underlined element in (a) (b) (c) (d) (e)

Indicate the oxidation state of S in (a) (b) (c) (d) (e) S4O6 2-HSO4 . - S2O8 ; 2- S2O3 ; 2- ; SO3 2- ; FeO4 2-. C2H3O2 - CH4 ; SF4 ; Na2O2 ; ;

Chromium forms three principal oxides. Write appropriate formulas for these compounds in which the oxidation states of Cr are and respectively.

Nitrogen forms five oxides in which its oxidation states are and respectively. Write appropriate formulas for these compounds.

In many of its compounds, oxygen has an oxidation state of . However, there are exceptions. What is the oxidation state of oxygen in each of the following compounds? (a) (b) (c) (d)

Hydrogen and oxygen usually have oxidation states of +1 and -2, respectively, in their compounds. The OF2; O2F2; CsO2; BaO2. -2 following cases serve to remind us that there are exceptions. What are the oxidation states of the atoms in each of the following compounds? (a) (b) CsO3; (c) HOF; (d) NaAlH4.

Name these compounds: (a) SrO; (b) ZnS; (c) (d) (e) (f) (g) (h) (i) (j) (k) (l) (m) (n)

Name these compounds: (a) (b) (c) (d) (e) LiCN; (f) KIO; (g) (h) (i) (j) (k) (l) (m) (n)

Assign suitable names to the compounds (a) (b) (c) (d) (e) (f)

Assign suitable names to the compounds (a) ICl; (b) (c) (d) (e) (f)

Write formulas for the compounds: (a) aluminum sulfate; (b) ammonium dichromate; (c) silicon tetrafluoride; (d) iron(III) oxide; (e) tricarbon disulfide; (f) cobalt(II) nitrate; (g) strontium nitrite; (h) hydrobromic acid; (i) iodic acid; (j) phosphorus dichloride trifluoride.

Write formulas for the compounds: (a) magnesium perchlorate; (b) lead(II) acetate; (c) tin(IV) oxide; (d) hydroiodic acid; (e) chlorous acid; (f) sodium hydrogen sulfite; (g) calcium dihydrogen phosphate; (h) aluminum phosphate; (i) dinitrogen tetroxide; (j) disulfur dichloride. ClF3 ; SF4 ; BrF5 ; N2O4 ; S4N4 . SiF4 ; ClF5 ; N2O5 ; SF6 ; I2Cl6 . CS2 ; NH4C2H3O2 ; MgC2O4 ; Na2C2O4 . Ca(H2PO4)2 ; H3PO4 ; NaHSO4 ; Na2Cr2O7 ; CrO2 ; KIO3 ; Fe(OH)2 ; Ba(NO3)2 ; HNO2 ; HNO3 ; KClO4 ; HBrO3 ; H3PO3 . (NH4)2HPO4 ; Ca(HSO3)2 ; Cu(OH)2 ; Cs2SO4 ; Cr2O3 ; Fe2(SO4)3 ; Mg(HCO3)2 ; K2CrO4 ;

Write a formula for (a) the chloride of titanium having Ti in the O.S. ; (b) the sulfate of iron having Fe in the O.S. ; (c) an oxide of chlorine with Cl in the O.S. ; (d) an oxoanion of sulfur in which the apparent O.S. of S is and the ionic charge is .

Write a formula for (a) an oxide of nitrogen with N in the O.S. ; (b) an oxoacid of nitrogen with N in the O.S. ; (c) an oxide of carbon in which the apparent O.S. of C is ; (d) a sulfur-containing oxoanion in which the apparent O.S. of S is and the ionic charge is .

Name the acids: (a) (b) (c) (d)

Supply the formula for the acids: (a) hydrofluoric acid; (b) nitric acid; (c) phosphorous acid; (d) sulfuric acid.

Name the following compounds and specify which ones are best described as ionic: (a) (b) (c) (d) .

Name the following compounds and specify which ones are best described as ionic: (a) (b) (c) S2Cl2; (d) Mg(ClO)2; (e) Cl2O.

Without performing detailed calculations, indicate which of the following hydrates has the greatest % by mass: and

Without performing detailed calculations, determine the hydrate of that contains almost exactly 50% by mass.

Anhydrous can be used to dry liquids in which it is insoluble. The is converted to which can be filtered off from the liquid. What is the minimum mass of anhydrous needed to remove 12.6 g H2O from a tankful of gasoline? CuSO4 CuSO4 # CuSO4 5 H2O, CuSO4 H2O, Na2SO3 LiC2H3O2 # 2 H2O. CuSO4 # 5 H2O, Cr2(SO4)3 # 18 H2O, MgCl2 # 6 H2O, H2O

Anhydrous sodium sulfate, absorbs water vapor and is converted to the decahydrate, How much would the mass of 24.05 g of anhydrous increase if converted completely to the decahydrate?

A certain hydrate is found to have the composition 20.3% Cu, 8.95% Si, 36.3% F, and 34.5% by mass. What is the empirical formula of this hydrate?

An 8.129 g sample of is heated until all the water of hydration is driven off. The resulting anhydrous compound, weighs 3.967 g. What is the formula of the hydrate?

Which of the following names is most appropriate for the molecule with the structure shown below? (a) butyl alcohol; (b) 2-butanol; (c) 1-butanol; (d) isopentyl alcohol.

Which of the following names is most appropriate for the molecule (a) dimethyleneacetic acid; (b) propanoic acid; (c) butanoic acid; (d) oxobutylalcohol. CH3(CH2)2COOH?

Which of the following structures are isomers?

Which of the following structures are isomers?

Write the condensed structural formulas for the organic compounds: (a) heptane (b) propanoic acid (c) 2-methyl-1-pentanol (d) fluoroethane

Write the condensed structural formulas for the organic compounds: (a) octane (b) heptanoic acid (c) 3-hexanol (d) 2-chlorobutane

Give the name, condensed structural formula, and molecular mass of the molecule whose ball-and-stick model is shown. Refer to the color scheme in Figure 3-3.

Give the name, condensed structural formula, and molecular mass of the molecule whose ball-and-stick model is shown. Refer to the color scheme in Figure 3-3.

The mineral spodumene has the empirical formula . Given that the percentage of lithium-6 atoms in naturally occuring lithium is 7.40%, how many lithium-6 atoms are present in a 518 g sample of spodumene?

A particular type of brass contains Cu, Sn, Pb, and Zn. A 1.1713 g sample is treated in such a way as to convert the Sn to 0.245 g , the Pb to 0.115 g , and the Zn to 0.246 g . What is the mass percent of each element in the sample?

A brand of lunchmeat contains 0.10% by mass of sodium benzoate, How many mg of Na does a person ingest by eating 2.52 oz of this meat?

The important natural sources of boron compounds are the minerals kernite, and borax, . How much additional mass of mineral must be processed per kilogram of boron obtained if the mineral is borax rather than kernite? Na2B4O7 # 10 H2O Na2B4O7 # 4 H2O C6H5COONa. PbSO4 Zn2P2O7 SnO2 LiAlSi2O6

To deposit exactly one mole of Ag from an aqueous solution containing requires a quantity of electricity known as one faraday (F). The electrodeposition requires that each ion gain one electron to become an Ag atom. Use appropriate physical constants listed on the inside back cover to obtain a precise value of the Avogadro constant, .

By analysis, a compound was found to contain by mass; the remainder was oxygen. What is the oxidation state of chromium in this compound? What is the name of the compound?

Is it possible to have a sample of that weighs What is the smallest possible mass that a sample of can have? Express your answer to the second question in appropriate SI units so that your answer has a numerical value greater than 1. (See Table 1.2 for a list of SI prefixes.)

What is the molecular formula of a hydrocarbon containing n carbon atoms and only one double bond? Can such a hydrocarbon yield a greater mass of than when burned in an excess of oxygen?

A hydrocarbon mixture consists of 60.0% by mass of and 40.0% of . When 10.0 g of this mixture is burned, 29.0 g and 18.8 g are the only products. What is the formula of the unknown hydrocarbon?

A 0.732 g mixture of methane, , and ethane, , is burned, yielding 2.064 g . What is the percent composition of this mixture (a) by mass; (b) on a mole basis?

The density of a mixture of and water is The percent composition of the mixture is to be determined by converting to If 32.0 mL of the mixture gives 65.2 g , then what is the percent composition of the mixture?

All the silver in a 26.39 g sample of impure silver is converted to silver chloride. If 31.56 g of silver chloride are obtained, then what is the mass percent of silver in the sample?

In the year 2000, the Guinness Book of World Records called ethyl mercaptan, , the smelliest substance known. The average person can detect its presence in air at levels as low as . Express the limit of detectability of ethyl mercaptan in parts per billion (ppb). (Note: 1 ppb means there is 1 g per billion grams of air.) The density of air is approximately at room temperature.

Dry air is essentially a mixture of the following entities: , , Ar, and . The composition of dry air, in mole percent, is 78.08% , 20.95% , 0.93% Ar, and 0.04% CO2. (a) What is the mass, in grams, of a sample of air that contains exactly one mole of the entities? (b) Dry air also contains other entities in much smaller amounts. For example, the mole percent of krypton (Kr) is about . Given that the density of dry air is about at room temperature, what mass of krypton could be obtained from exactly one cubic meter of dry air?

A public water supply was found to contain 1 part per billion (ppb) by mass of chloroform, . (a) How many molecules would be present in a 225 mL glass of this water? (b) If the in part (a) could be isolated, would this quantity be detectable on an ordinary analytical balance that measures mass with a precision of g?

A sample of the compound weighing 0.1131 g reacts with barium chloride and yields 0.2193 g What must be the atomic mass of the metal M? [Hint:All the from the appears in the .]

The metal M forms the sulfate . A 0.738 g sample of this sulfate is converted to 1.511 g . What is the atomic mass of M? [Hint: Refer to Exercise 98.] BaSO4 M21SO423 SO4 MSO4 BaSO4 2- BaSO4. MSO4 ;0.0001 CHCl3 CHCl3 CHCl3 1.2 g>L 1.14 * 10-4 % N2 O2 N2 O2 CO2 1.2 g>L C2H6S C2H6S 9 * 10-4 mmol>m3 C2H6S 1NH422SO4 H2SO4 1NH422SO4. 1.78 g>mL. H2SO4 C2H6 CO2 CH4 CO2 H2O CxHy C3H8 CO2 H2O

. A 0.622 g sample of a metal oxide with the formula is converted to 0.685 g of the sulfide, MS. What is the atomic mass of the metal M?

. often occurs in table salt (NaCl) and is responsible for caking of the salt. A 0.5200 g sample of table salt is found to contain 61.10% Cl, by mass. What is the % in the sample? Why is the precision of this calculation so poor?

. When 2.750 g of the oxide of lead is strongly heated, it decomposes and produces 0.0640 g of oxygen gas and 2.686 g of a second oxide of lead. What is the empirical formula of this second oxide?

. A 1.013 g sample of is dissolved in water and the sulfate ion precipitated as . The mass of pure, dry obtained is 0.8223 g. What is the formula of the zinc sulfate hydrate?

. The iodide ion in a 1.552 g sample of the ionic compound MI is removed through precipitation. The precipitate is found to contain 1.186 g I. What is the element M?

. An oxoacid with the formula has a formula mass of 178 u, has 13 atoms in its formula unit, contains 34.80% by mass, and 15.38% by number of atoms, of the element E. What is the element E, and what is the formula of this oxoacid?

. The insecticide dieldrin contains carbon, hydrogen, oxygen, and chlorine. When burned in an excess of oxygen, a 1.510 g sample yields 2.094 g and 0.286 g . The compound has a molecular mass of 381 u and has half as many chlorine atoms as carbon atoms. What is the molecular formula of dieldrin?

. A thoroughly dried 1.271 g sample of is exposed to the atmosphere and found to gain 0.387 g in mass. What is the percent, by mass, of in the resulting mixture of anhydrous and the decahydrate?

. The atomic mass of Bi is to be determined by converting the compound to . If 5.610 g of yields 2.969 g , what is the atomic mass of Bi?

. A piece of gold (Au) foil measuring is treated with fluorine gas. The treatment converts all the gold in the foil to 1.400 g of a gold fluoride. What is the formula and name of the fluoride? The density of gold is .

. In an experiment, 244 mL of chlorine gas combines with iodine to give 1.553 g of a binary compound. In a separate experiment, the molar mass of the compound is found to be about . What is the molecular formula of this compound?

. All-purpose fertilizers contain the essential elements nitrogen, phosphorus, and potassium. A typical fertilizer carries numbers on its label, such as 5-10-5 . These numbers represent the % N, % P2O5 , and % respectively. The N is contained in the form of a nitrogen compound, such as or (urea). The P is generally present as a phosphate, and the K as KCl. The expressions % and % were devised in the nineteenth century, before the nature of chemical compounds was fully understood. To convert from % to % P and from % to % K, the factors 2 mol and 2 mol must be used, together with molar masses. (a) Assuming three-significant-figure precision, what is the percent composition of the 5-10-5 fertilizer in % N, % P, and % K? (b) What is the % in the following compounds (both common fertilizers)? (i) (ii) (c) In a similar manner to the 5-10-5 fertilizer described in this exercise, how would you describe a fertilizer in which the mass ratio of to KCl is 5.00:1.00? (d) Can a 5-10-5 fertilizer be prepared in which and KCl are the sole fertilizer components, with or without inert nonfertilizer additives? If so, what should be the proportions of the constituents of the fertilizer mixture? If this 5-10-5 fertilizer cannot be prepared, why not?

. A hydrate of copper(II) sulfate, when heated, goes through the succession of changes suggested by the photograph. In this photograph, (a) is the original fully hydrated copper(II) sulfate; (b) is the product obtained by heating the original hydrate to 140 C; (c) is the product obtained by further heating to 400 C; and (d) is the product obtained at 1000 C. A 2.574 g sample of was heated to 140 C, cooled, and reweighed. The resulting solid was reheated to 400 C, cooled, and reweighed. Finally, this solid was heated to 1000 C, cooled, and reweighed for the last time. Original sample 2.574 g After heating to 140 C 1.833 g After reheating to 400 C 1.647 g After reheating to 1000 C 0.812 g (a) Assuming that all the water of hydration is driven off at 400 C, what is the formula of the original hydrate? (b) What is the formula of the hydrate obtained when the original hydrate is heated to only 140 C? (c) The black residue obtained at 1000 C is an oxide of copper. What is its percent composition and empirical formula?

. Some substances that are only very slightly soluble in water will spread over the surface of water to produce a film that is called a monolayer because it is only one molecule thick. A practical use of this phenomenon is to cover ponds to reduce the loss of water by evaporation. Stearic acid forms a monolayer on water. The molecules are arranged upright and in contact with one another, rather like pencils tightly packed and standing upright in a coffee mug. The model below represents an individual stearic acid molecule in the monolayer. (a) How many square meters of water surface would be covered by a monolayer made from 10.0 g of stearic acid? [Hint: What is the formula of stearic acid?] (b) If stearic acid has a density of estimate the length (in nanometers) of a stearic acid molecule. [Hint: What is the thickness of the monolayer described in part a?] (c) A very dilute solution of oleic acid in liquid pentane is prepared in the following way: 0.895 g>mL. 4.6 * 10-15 cm2. 85 cm2. 1.00 mL solution (3) + 9.00 mL pentane :solution (4). 1.00 mL solution (2) + 9.00 mL pentane :solution (3); 1.00 mL solution (1) + 9.00 mL pentane :solution (2); 1.00 mL oleic acid + 9.00 mL pentane : solution (1); A0.10 mL sample of solution (4) is spread in a monolayer on water. The area covered by the monolayer is Assume that oleic acid molecules are arranged in the same way as described for stearic acid, and that the cross-sectional area of the molecule is The density of oleic acid is Use these data to obtain an approximate value of Avogadro s number.

. In your own words, define or explain the following CaClO2 ; terms or symbols: (a) formula unit; (b) (c) molecular compound; (d) binary compound; (e) hydrate.

. Briefly describe each of the following ideas or methods: (a) mole of a compound; (b) structural formula; (c) oxidation state; (d) carbon hydrogen oxygen determination by combustion analysis.

. Explain the important distinctions between each pair of terms: (a) molecular mass and molar mass; (b) empirical and molecular formulas; (c) systematic and trivial, or common, name; (d) hydroxyl and carboxyl functional group.

. Explain each term as it applies to the element nitrogen. (a) atomic mass; (b) molecular mass; (c)molar mass.

. Which answer is correct? One mole of liquid bromine, (a) has a mass of 79.9 g; (b) contains Br atoms; (c) contains the same number of atoms as in 12.01 g (d) has twice the mass of 0.500 mole of gaseous

. Three of the following formulas might be either an empirical or a molecular formula. The formula that must be a molecular formula is (a) (b) (c) NaCl; (d)

. The compound contains (a) 17 atoms per mole; (b) equal percents by mass of C and H; (c) about twice the percent by mass of O as of N; (d) about twice the percent by mass of N as of H.

. The greatest number of N atoms is found in (a) 50.0 g (b) 17.0 g (c) 150 mL of liquid pyridine, (d)

. consists of 65% F by mass. The atomic mass of the element X must be (a) 8 u; (b) 11u; (c) 31 u; (d) 35 u.

. The oxidation state of I in the ion is (a) (b) +1; (c) +7; (d) +8.

. The formula for calcium chlorite is (a) (b) (c) (d)

. Aformula unit of the compound has nearly equal masses of (a) S and O; (b) N and O; (c) H and N; (d) Cu and O.

. An isomer of the compound is (a) (b) (c) (d)

. A hydrate of contains almost exactly 50% by mass. What is the formula of this hydrate?

. Malachite is a common copper-containing mineral with the formula (a) What is the mass percent copper in malachite? (b) When malachite is strongly heated, carbon dioxide and water are driven off, yielding copper(II) oxide as the sole product. What mass of copper(II) oxide is produced per kg of malachite?

. Acetaminophen, an analgesic and antipyretic drug, has a molecular mass of 151.2 u and a mass percent composition of 63.56% C, 6.00% H, 9.27% N, and 21.17% O. What is the molecular formula of acetaminophen?

. Ibuprofen is a compound used in painkillers. When a 2.174 g sample is burned in an excess of oxygen, it yields 6.029 g and 1.709 g as the sole products. (a)What is the percent composition, by mass, of ibuprofen? (b) What is the empirical formula of ibuprofen?

. Appendix E describes a useful study aid known as concept mapping. Using the method presented in Appendix E, construct a concept map illustrating the different concepts in Sections 3-2 and 3-3.