2013-14 Chemistry 1st Semester Final Exam Topics and Review- Chapters 1-8

Review Questions:

  1. Round each number to four significant figures and write it in scientific notation:

a. 9367958 b. 0.7728c. 0.000037001d. 19873460000

  1. Write each in conventional notation:

a. 8.2001112 x 105b. 3.23876 x 10-4c. 1.09857 x 101

  1. Scientific and Standard Notation:

a. Convert 0.00012 to scientific notation b. convert 5.63 x 10-2 to regular notation

  1. Significant Figures: Review rules for using significant figures.

a. How many sig figs are in the following:

(1)0.5(2)500(3)500.(4)500.0

(5)0.05(6) 0.050(7)56008(8)6.53 x 106

  1. Rounding:

a. 3.41236cm to 3 sig figsb. 3459.23 to 3 sig figsc. 2.0104 to 4 sig figs

d. 0.853479 to 4 sig figse. 49673.56 to 4 sig figsf. 0.00256 to 1 sig fig

  1. Math with Significant Figures: Calculate each with the correct amount of significant figures

a. 5.2 x 1.00 =b. 6.3489 + 7.7 =c. (3.4x103)–(2.1x102) =

  1. 8.940 / 2.39 =e. 149.0 kg + 3388.228 kg + 2.98 kg =
  1. (1.092 x 103m) – (4.33 x 106m) = g.
  1. convert 5.72g to Kgi. Convert 275.6mL to L
  1. Products vs Reactants: Identify the product(s) and reactant(s) of the following reaction:

a. NaOH + HCl NaCl + H2Ob. H2O  H2 + O2

  1. Temperature conversions

Convert to Celsius: a. 57Fb. -24.7Fc. 212K

Convert to Fahrenheit: a. -31Cb. 78.22Cc. 237K

Convert to Kelvin: a. 8.23Cb. 91Fc. -40 F

  1. Density: What is the equation for density? ______What are the units? ____, _____, _____

a.The density of an item is 0.933Kg/L. find the volume of a 4.9909g sample.

b.The mass of an item is 4234g and the volume is 893cm3. What is the density in kg/L?

c.What is the density of an object that measures 5.60cm by 3.3cm by 1.456cm and has a mass of 2.34g?

dAn irregularly shaped object with a density of 3.556g/mL is dropped into a graduated cylinder filled with 22.56mL of water. If the water level rises to 44.5mL, what is the mass of the object?

e.What is the volume of an object with a density of 8.03g/cm3 and a mass of 6.00 x 102g?

Matter: Define the following: heterogeneous, homogeneous, mixture, compound, element, distillation, filtration, chemical property, physical property, isotope, metal, nonmetal, metalloid, ductile, malleable.

a. Classify each of the following as an element [E], a compound [C], or a mixture [M].

Gold / Distilled Water / Ocean water / Ice (from tap water) / A chocolate sundae
Air / Carbon dioxide / Silver / Sugar / A Big Mac®

b. Classify the following as pure substances [P] or as mixtures [M]:

Air / Black coffee / Distilled water / sugar
Gold / mercury / oxygen / salt water
Alcohol / Kool aid / Beach sand / dirt

c. Classify the following as heterogeneous [He] or as homogeneous [Ho]:

sand & salt mixture / hydrogen / iron / salt water
unfiltered air / iron with rust / pure water / Chocolate chip cookie
tossed salad / Can of pepsi / Bucket of ocean water / Cup of black coffee

11. Physical vs Chemical Properties/Changes

a. Salt dissolves in waterb. HCl acid reacts with Mg to produce H2 gas.

c. A piece of copper is cut in half.d. A sugar cube is ground up.

e. Water is heated and changed to steam.f. Iron rusts

g. Ethyl alcohol evaporatesh. ice melts

i. Density

12. Scientific symbols:

  1. Write the complete chemical symbol for the ion with 84 protons, 125 neutrons, and 80 electrons.
  2. Write the complete chemical symbol for the ion with 27 protons, 32 neutrons, and 25 electrons.
  3. Write the complete chemical symbol for the ion with 73 protons, 108 neutrons, and 68 electrons.

d. Write the complete chemical symbol for the ion with 31 protons, 39 neutrons, and 28 electrons

13. Subatomic Particles: How many protons and neutrons are in the following:

a. 244Pub. 133Cs c. 277Acd. 57Fe

14. Subatomic Particles with ions: Determine the number of protons, electrons and neutrons

d.O -2 How many protons, electrons, neutrons, atomic number, mass number

e. Na+1 How many protons, electrons, neutrons, atomic number, mass number

f.Na+1 is a cation or an anion?

g.O-2 is a cation or an anion

15.Subatomic particles with ions and isotopes: Fill in the following chart:

Element / Symbol / Atomic # / Atomic Mass / Protons / Electrons / Neutrons / Gained/Lost electrons / Family Name / Metal/
nonmetal
/metalloid
1 / 1 / 0
2 / 2 / 2
Cl 1- / 35
6 / 6 / 0
K 1+ / 39
Zinc / 35 / Lost 2
Gold / Au3+ / 79 / 118

16. Naming Compounds: Name the following:

a. SeOb. B2O3c. AsBr3d. SnO2e. CuSf. Ca3N2g. NH4NO2

h. AgNO3i. Ba(OH)2j. KC2H3O2 k. Li2CO3l. Fe2(SO4)3m. HBr n. HC2H3O2

o. HNO2

17. Formula Writing:Give the formulas for the following:

a. barium nitride b. silver iodide c. sulfur hexafluoride d. carbon tetrachloride

e. magnesium acetatef. iron (II) sulfateg. zinc chromateh. cobalt (II) carbonate

i. calcium bromidej. lithium sulfite k. nitric acid l. sulfurous acid

m. copper (II) permanganate n. phosphoric acido. iron (III) oxide

18. Types of Reactions: Determine the type of reaction:

a. H3PO4 + 3KOH ------> K3PO4 + 3H2O

b. Ag2O ----> Ag + O2(g)

c. N2 + H2---> NH3

d. C12H22O11(s) ----> 12C(s) + 11H2O(g)

e. AgNO3+NaCl----> AgCl + NaNO3

f. HCl + NaOH ---> H2O + NaCl

g. H2(g) + O2(g) ----> H2O(g)

h. Zn(s) + H2SO4(aq) ----> ZnSO4(aq) + H2(g)

19. Redox Reactions: Determine which of the following are redox (oxidation-reduction) reactions. For the reactions that are redox, determine which element was oxidized and which was reduced.

a. Ag + S ---> Ag2S

b. Al+ CuCl2 ---> AlCl3 + Cu

c. ZnBr2+AgNO3---->Zn(NO3)2+ AgBr

d. NaI + F2---> NaF + I2

20. Average Atomic Mass: Calculating Average Atomic Mass:

Rubidium has two common isotopes 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

21. Dimensional analysis: Show all work. Make sure that your answer has the correct number of significant figs and is in scientific notation.

a.7500000μL = ? mLb. 15673.35dL/hour = ?mL/weekc.1.56 x 10-4GL = ? qts.

b.89751236lbs = ?mge. 52.30km/hr = ? m/sf.5.25x103 kg = ? mg

g.111109g to lbsh. 5400in to mii.19cm to ft

j.36cm to milesk. 16 weeks to secl.54 yds to mm

23. More Naming Compounds: Name the following:

a. H3PO4 b. CsOH c. Li2Od. Ca(OH)2e. CaBr2f. Fe2O3

g. H2SO4h. FeCO3i. SO3j. BaCO3k. Al(OH)3l. NaC2H3O2

m. Na2SO3n. H2CO3o. LiHp. COq. MgBr2r. SnBr2

s. N2Ot. NH4Fu. HCO3v. K2O

24. Writing Chemical Equations with states: For the following descriptions of chemical reactions, write and balance the chemical equations. Include the physical states (aq, s, l, g).

a. When zinc metal and sulfur powder are heated, they form solid zinc sulfide.

b. When sodium metal is placed in a beaker of water, hydrogen gas and sodium hydroxide solution are formed.

c. Aqueous iron (III) chloride will react with aqueous sodium hydroxide to produce aqueous iron (III) hydroxide and aqueous sodium chloride.

  1. The Haber process is a chemical process by which hydrogen gas reacts with nitrogen gas to form ammonia. Write and balance a chemical equation for this reaction.
  2. One of the problems with space travel is the building up of carbon dioxide produced by the astronauts. The typical procedure is to react the carbon dioxide with lithium hydroxide to form lithium carbonate and liquid water. Write and balance a chemical equation for this reaction.
  3. Aluminum metal burns in pure oxygen to produce solid aluminum oxide.
  4. Hydrogen sulfide gas reacts with oxygen gas to form water vapor and solid sulfur.
  5. Hydrogen gas and iron (III) oxide powder react to form liquid water and solid iron powder.

25. Predicting Products: Write balanced molecular equations for the following: If they are double replacement or acid base then also show states of all parts of reaction. Some may not have reactions.

a.magnesium plus nitric acid

b. tricarbon dihydride plus oxygen

c. calcium chloride plus sulfurous acid

d. zinc plus copper (II) sulfate

e. ammonium sulfate plus lead (II) nitrate

f. Iron (III) chloride decomposes

g. sodium plus oxygen

h. dicarbon heptaoxide plus oxygen

i. sodium carbonate and potassium chloride

j. tricarbon octohydride and oxygen

k. aluminum and sulfuric acid

l. barium chloride and sodium sulfate

26. Molar Conversions: Complete the following table- SHOWALLWORK!!!!!

mass of sample / moles of sample / particles of sample
4.24g hexacarbon hexahydride
0.224mol water
2.71 x 1022 molecules carbon dioxide
0.297g nitric acid
1.26mol hydrochloric acid
4.21 x 1024 molecules magnesium acetate
1478mg ammonium carbonate
1.400 x 103 mol beryllium permanganate
9.97654 x 1023 molecules hypochlorous acid
  1. Percent composition: Find the percent compositions of specified elements in the following compounds:
  2. CuBr2 _____% of Cub. NaOH ______% of OH

c. ammonium sulfide _____% of Sd. Hydrochloric acid _____% of H

e. aluminum sulfate _____ % of Of. Mg(NO3)2 ______% Of Mg

28. Empirical Formulas: Determine the empirical formulas for the following compounds.

a.An oxide of chromium has the followingpercent composition: 68.4% Cr and 31.6% O.

b.The percent composition of a new compound is 63.5% silver, 8.2% nitrogen and 28.3% oxygen.

c.a 170.00g sample of an undentified compound contains 29.84g sodium, 67.49g chromium and 72.67g of oxygen.

d.A 60.00g sample of tetraethyl lead contains 38.43g of lead, 17.83g of carbon, and 3.74g of hydrogen.

29. Molecular formulas:Determine the empirical and molcular formulas for the following compounds.

a. A compound containing 5.9265% H and 94.0735% O has a molar mass of 34.01468g/mol.

b. The empirical formula for trichloroisocyanuric acid, the active ingrediant in many household bleaches, is OCNCl. The molar mass of this compound is 242.41g/mol.

c. Determine the molecular formula of a compound with an empirical formula of NH2 and a formula mass of 32.06 amu.

d. Phenyl magnesium bromide is used as a Grignard reagent in organic synthesis. Determine its empirical formula AND molecular formula if its molar mass is 181.313g/mol and it contains 39.7458% C, 2.77956% H, 13.4050% Mg and 44.0697% Br