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lab02a.qxd 11/15/13 3:29 PM Page 93 9. Some chemical elements show more than one oxidation number, depending on the compound. The preceding rules may be used to determine their values. Consider the compounds FeCl2 and FeCl3. Since the chlorine atom has an oxidation number of –1 when combined with a metal (rule 5e), the oxidation numbers of iron are +2 in FeCl2 and +3 in FeCl3. An extensive listing of oxidation numbers and charges for monoatomic ions and polyatomic ions are presented in Dry Lab 2C, Table D2C.1. Procedure Overview: The oxidation number of an element in a selection of compounds and ions is determined by application of the rules in the Introduction. Your instructor will indicate the questions you are to complete. Answer them on a separate piece of paper. Be sure to indicate the date, your lab section, and your desk number on your Report Sheet. Dry Lab Procedure 1. Indicate the oxidation number of carbon and sulfur in the following compounds. a. CO d. Na2C2O4 g. SO2 j. Na2SO3 m. SCl2 b. CO2 e. CH4 h. SO3 k. Na2S2O3 n. Na2S2 c. Na2CO3 f. H2CO i. Na2SO4 l. Na2S4 O6 o. SOCl2 2. Indicate the oxidation number of phosphorus, iodine, nitrogen, tellurium, and silicon in the following polyatomic ions. Remember that the sum of the oxidation numbers for a polyatomic ion must equal the charge of the ion. a. PO4 3– d. P3O10 5– g. IO– j. NO2– m. N2O22– b. PO33– e. IO3– h. NH4 + k. NO+ n. TeO4 2– c. HPO4 2– f. IO2 – i. NO3– l. NO2+ o. SiO32– 3. Indicate the oxidation number of the metallic element(s) in the following compounds. None of the compounds listed are peroxides. a. Fe2O3 g. CrO3 m. MnO2 b. FeO h. K2CrO4 n. PbO2 c. CoS i. K2Cr2O7 o. Pb3O4 d. CoSO4 j. KCrO2 p. ZrI4 e. K3CoCl6 k. K2MnO4 q. U3O8 f. CrCl3 l. Mn2O7 r. UO2Cl2 Dry Lab 2A 93 lab02b.qxd 11/15/13 9:55 AM Page 96 Note that the end vowel of the Greek prefix is occasionally omitted from the spelling for clarity in pronunciation. Hydrates Prefixes are also used for the naming of hydrates, inorganic salts in which water molecules are a part of the crystalline structure of the solid. The waters of hydration (also called waters of crystallization) are bound to the ions of the salt and, in most cases, can be removed with the application of heat (see Experiment 5). For example, barium chloride is often purchased as barium chloride dihydrate: BaCl2•2H2O. The formula of iron(III) chloride hexahydrate is FeCl3•6H2O. The formula for Epsom salt (Figure 5.1) is MgSO4•7H2O, magnesium sulfate heptahydrate. Binary Acids A binary acid is an aqueous solution of a compound formed by hydrogen and a more electronegative nonmetal. To name the acid, the prefix hydro- and suffix -ic are added to the root of the nonmetal name. Writing Formulas from Names Formula Name HCl(aq) HBr(aq) H2S(aq) hydrochloric acid hydrobromic acid hydrosulfuric acid In writing formulas for compounds, it is mandatory that the sum of the oxidation numbers of the elements equals zero(see Dry Lab 2A, rule 8). The name of the compound must dictate how the formula is to be written. Example D2B.1 Write the formula for calcium nitride. Calcium is in group 2A and therefore has an oxidation number of +2 : Ca2+. The nitrogen atom is always –3 when combined with a metal: N3–. Therefore, for the sum of the oxidation numbers to equal zero, there must be three Ca2+ (a total of +6) for every two N3– (a total of –6); the formula is Ca3N2. Dry Lab Procedure 96 Procedure Overview: Given the formula of the compound, the proper names for a large number of compounds are to be written. Given the name of the compound, the formulas for a large number of compounds also are to be written. Your instructor will assign the exercises you are to complete. Answer them on a separate piece of paper. Be sure to indicate the date, your lab section, and your desk number on your Report Sheet. Use the rules that have been described. 1. Name the following binary salts of the representative elements. a. Na3P d. CaC2 g. Ca3P2 j. K2S m. NH4Br p. AlCl3 b. Na2O e. CaI2 h. KCN k. K2Te n. (NH4)2S q. Al2O3 c. Na3N f. CaH2 i. KOH l. K2O2 o. NH4CN r. AlN 2. Name the following salts according to the old -ic, -ous system and the Stock system. a. CrS g. HgCl2 m. CoO b. Cr2O3 h. Hg2Cl2 n. CoBr3•6H2O c. CrI3•6H2O i. HgO o. SnF4 d. CuCl j. Fe2O3 p. SnO2 e. CuI2 k. FeS q. Cu2O f. CuBr2•4H2O l. FeI3•6H2O r. Fe(OH)3 Inorganic Nomenclature II. Binary Compounds lab02b.qxd 11/15/13 9:55 AM Page 97 3. Name the following binary acids. a. HF(aq) d. HBr(aq) b. HI(aq) e. H2Te(aq) c. H2Se(aq) f. HCl(aq) 4. Name the following binary compounds consisting of two nonmetals or a metalloid and a nonmetal. a. SO2 d. SF6 g. N2O5 j. SiCl4 m. AsH3 p. XeF4 b. SO3 e. SCl4 h. N2S4 k. SiO2 n. AsF5 q. XeF6 c. S4N4 f. NO2 i. NF3 l. AsCl3 o. HCl r. XeO3 5. Write formulas for the following compounds consisting of a metal cation and a nonmetal anion. a. ferrous sulfide h. nickel(III) oxide b. iron(III) hydroxide i. chromium(III) oxide c. ferric oxide j. titanium(IV) chloride d. aluminum iodide k. cobalt(II) chloride hexahydrate e. copper(I) chloride l. cobaltous oxide f. cupric cyanide tetrahydrate m. mercury(I) chloride g. manganese(IV) oxide n. mercuric iodide 6. Write formulas for the following compounds consisting of two nonmetals (or a metalloid and a nonmetal). a. hydrochloric acid g. iodine pentafluoride b. hydrosulfuric acid h. krypton difluoride c. hydroiodic acid i. tetrasulfur tetranitride d. silicon tetrafluoride j. dichlorine heptaoxide e. arsenic pentafluoride k. phosphorus trihydride (phosphine) f. xenon hexafluoride l. tetraphosphorus decoxide 7. Write formulas and name the binary compounds resulting from matching all cations with all anions in each set. Set 1 Set 2 Set 3 Cations Anions Cations Anions Cations Anions K H (aq)* Na Fe3 Cu Cl S2 F CN I Co2 Co3 Pb2 Pt4 Ba2 P3 Br O2 F OH Mn3 Sn2 NH4 Hg22 Ce4 O2 N3 S2 Se2 I *Name as acids 8. Write formulas for the chemicals shown in the margin on page 95. Dry Lab 2B 97
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Surname 1
Student’s name
Professor’s name
Course
Date

Questions from pages 93, 96 and 97

Page 93
Question 1
Oxidation number of carbon and sulfur
a. CO=+1
b. CO2=+4
c. Na2CO3=+3
d. Na2C2O4=+6
e. CH4=+4
f. H2CO=-1
g. SO2=+4
h. SO3=+5
i. Na2SO4=6
j. Na2SO3=+5
k. Na2S4O6=-6
l. Na2S4O6=-6
m. SCL2=+4

Surname 2

n. Na2S2=+2
o. SOCL2=+2
QUESTION 2
Oxidation number of iodine, phosphorus, tellurium, nitrogen and silicon
a. PO43-=-3
b. PO33-=-3
c. HPO42-=-2
d. P3O105-=-5
e. IO3-=-1
f. IO2-=-1
g. IO-=-1
h. NH4+=+1
i. NO3-=-1
j. NO2-=-1
k. NO+=+1
l. NO2+=+1
m. N2O22-=-2
n. TeO42-=-2
o. SiO32-=-2
QUESTION 3
Oxidation number of metallic elements
a. Fe2O3=+3
b. FeO=+1

Surname 3

c. CoS=+2
d. CoSO4=+2
e. K3CoCI6=+1
f. CrCI3=+3
g. CrO3=+5
h. K2CrO4=+1
i. K2Cr2O7=+2
j. KCrO2=+1
k. K2MnO4=+1
l...


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