Name Date Hour Honors Chemistry Final Exam Study Guide For problems 1-4, express each number in scientific notation 1.) 0.00000000007461 m 2.) 0.0000158 mi 3.) 0.00000632 m 4.) 0.000015 m ---------------------------------------------------------------------------------------------------------------------- 5.) Convert 3.55 kg to grams 6.) Convert 8944 mm to meters 7.) Convert 4598 mg to kilograms 8.) Convert 0.0187 L to milliliters 9.) Convert 22.5 in. To centimeters 10.) 126 ft to meters 11.) 825 yd to kilometers 12.) 2.4 in. To millimeters ---------------------------------------------------------------------------------------------------------------------- 13.) A gangsta needs to chase after the dirty thief who snitched his wallet. The thief is super fast but will get tired of running after running 10.0 km and the gangsta has a running pace of 7.5 mi/h. How many minutes will the gangsta be running before the thief gets tired? (Hint: 7.5 mi/h as a conversion factor between distance and time) 14.) A gangsta got in a fight and knocked out a guys tooth crown which is supposedly real gold. After testing it to determine its density he finds out that it displaces 10.7 ml of water and has a mass of 206 g. Could the gangsta have really scored himself some legit gold? 15.) An automobile gasoline tank holds 42 kg of gasoline. When the gasoline burns, 168 kg of oxygen are consumed and carbon dioxide and water are produced. What is the total combined mass of carbon dioxide and water that is produced?
16.) A common type of handwarmer contains iron powder that reacts with oxygen to form an oxide of iron. As soon as the handwarmer is exposed to air, the reaction begins and heat is emitted. Is the reaction between the iron and oxygen exothermic or endothermic? Draw an energy diagram showing the relative energies of the reactants and the products in the reaction. ---------------------------------------------------------------------------------------------------------------------- 17.) Which statements about protons are true? A.) Protons have twice the mass of neutrons B.) Protons have the same magnitude of charge as elections but are opposite in sign C.) Most atoms have more protons than elections D.) Protons have a charge of 1+ 18.) List the symbol and atomic number corresponding to each element A.) Carbon B.) Nitrogen C.) Sodium D.) Potassium E.) Copper 19.) Classify each element as a metal, nonmetal or metalloid A.) Sr B.) Mg C.) F D.) N E.) As 20.) Which elements would you expect to lose elections in chemical changes? A.) Potassium B.) Sulfur C.) Fluorine D.) Barium E.) Copper 21.) Classify each element as halogen, a noble gas, or neither A.) Cl B.) Kr C.) F D.) Ga E.) He 22.) Which pair of elements do you expect to be most similar? Why? A.) Si and P B.) Cl and F C.) Na and Mg D.) Mo and Sn E.) N and Ni
23.) Complete each ionization equation. A.) B.) C.) D.) 24.) Predict the ion formed by each element A.) Rb B.) K C.) Al D.) O 25.) Write the symbol for each isotope in the form A.) Cobalt-60 B.) Neon-22 C.) Iodine-131 D.) Plutonium-244 26.) Determine the number of protons and neutrons in each isotope: A.) B.) C.) D.) 27.) Use the law of constant composition to complete the table summarizing the amounts of nitrogen and oxygen produced upon the decomposition of several samples of dinitrogen monoxide. 28.) How many oxygen atoms are in each chemical formula? A.) H 3 PO 4 B.) Na 2 HPO 4 C.) Ca(HCO 3 ) 2 D.) Ba(C 2 H 3 O 2 ) 2 29.) Classify each compound as ionic or molecular A.) CS 2 B.) CuO C.) KI D.) PCl 3
30.) What are the basic units--single atoms, molecules, or formula units--that compose each substance? A.) BaBr 2 B.) Ne C.) I 2 D.) CO 31.) Name each ionic compound. In each of these compounds, the metal forms more than one type of ion. A.) CrCl 2 B.) CrCl 3 C.) SnO 2 D.) PbI 2 32.) Name each ionic compound containing a polyatmoic ion A.) Ba(NO 3 ) 2 B.) Pb(C 2 H 3 O 2 ) 2 C.) NH 4 I D.) KClO 3 E.) CoSO 4 F.) NaClO 4 33.) Write a formula for each ionic compound. A.) Copper (II) Bromide B.) Silver Nitrate C.) Potassium Hydroxide D.) Sodium Sulfate E.) Potassium Hydrogen Sulfate F.) Sodium Hydrogen Carbonate 34.) Name each molecular compound. A.) SO 2 B.) NI 3 C.) BrF 5 D.) NO E.) N 4 Se 4 35.) How many moles of atoms are in each elemental sample? A.) 1.34 g Zn B.) 24.9 g Ar C.) 72.5 g Ta D.) 0.0223 g Li 36.) How many atoms are in each elemental sample? A.) 16.9 g Sr B.) 26.1 g Fe C.) 8.55 g Bi D.) 38.2 g of P
37.) Complete the table: 38.) Determine the number of moles of molecules (or formula units) in each sample. A.) 38.2 g sodium chloride B.) 36.5 g nitrogen monoxide C.) 4.25 kg carbon dioxide D.) 2.71 mg carbon tetrachloride 39.) Complete the table: 40.) Calculate the mass percent composition of nitrogen in each compound. A.) N 2 O B.) NO C.) NO 2 D.) N 2 O 5 41.) Iron ores have different amounts of iron per kilogram of ore. Calculate the mass percent composition of iron for each iron ore: Fe 2 O 3 (hematite), Fe 3 O 4 (magnetite), FeCO 3 (siderite). Which ore has a the highest iron content? 42.) The rotten smell of decaying animal carcass is partially due to a nitrogen-containing compound called putrescine. Elemental analysis of putrescine shows that it consists of 54.50% C, 13.73% H, and 31.77% N. Calculate the empirical formula of putrescine. 43.) The molar masses and empirical formulas of several compounds containing carbon and chlorine are as follows. Find the molecular formula of each compound. A.) 284.77 g/ mol, CCl B.) 131.39 g/mol, C 2 HCl 3 C.) 181.44 g/mol, C 2 HCl
44.) Butanedione, a component of butter and body odor, has a cheesy smell. Elemental analysis of butanedione gave the mass percent composition: C, 55.80%; H, 7.03%; O, 37.17%. The molar mass of butanedione is 86.09 g/mol. Determine the molecular formula of butanedione. 45.) Write a balanced chemical equation for each chemical reaction. A.) Solid lead (II) sulfide reacts with aqueous hydrochloric acid to form solid lead (II) chloride and dihydrogen sulfide gas. B.) Gaseous carbon monoxide reacts with hydrogen gas to form gaseous methane (CH 4 ) and liquid water C.) Solid iron (III) oxide reacts with hydrogen gas to form solid iron and liquid water D.) Gaseous ammonia (NH 3 ) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water E.) Solid magnesium reacts with aqueous copper (I) nitrate to form aqueous magnesium nitrate and solid copper F.) Gaseous dinitrogen pentoxide decomposes to form nitrogen dioxide and oxygen gas G.) Solid calcium reacts with aqueous nitric acid to form aqueous calcium nitrate and hydrogen gas H.) Liquid methanol (CH 3 OH) reacts with oxygen gas to form gaseous carbon dioxide and gaseous water I.) Solid Vanadium (V) Oxide with hydrogen gas to form solid vanadium (III) oxide and liquid water J.) BaO 2 (s) + H 2 SO 4 (aq) --> BaSO 4 (s) + H 2 O 2 (aq) K.) Co(NO 3 ) 3 (aq) + (NH 4 ) 2 S(aq) --> Co 2 S 3 (s) + NH 4 NO 3 (aq) L.) Li 2 O(s) + H 2 O(l) --> LiOH(aq) M.) Hg 2 (C 2 H 3 O 2 ) 2 (aq) + KCl(aq) --> Hg 2 Cl 2 (s) + KC 2 H 3 O 2 (aq) 46.) Determine whether each compound is soluble or in-soluble. For the soluble compounds, identify the ions present in solution. A.) NaC 2 H 3 O 2 B.) Sn(NO 3 ) 2 C.) AgI D.) Na 3 (PO 4 )
47.) Determine whether each equation for a precipitation reaction is correct. Correct any incorrect equations. If no reaction occurs, write NO REACTION. A.) Ba(NO 3 ) 2 (aq) + (NH 4 ) 2 SO 4 (aq) --> BaSO 4 (s) + 2 NH 4 NO 3 (aq) B.) BaS(aq) + 2 KCl(aq) --> BaCl 2 (s) + K 2 S(aq) C.) 2 KI(aq) + Pb(NO 3 ) 2 (aq) --> PbI 2 (s) + 2 KNO 3 (aq) D.) Pb(NO 3 ) 2 (aq) + 2 LiCl(aq) --> 2 LiNO 3 (s) + PbCl 2 (aq) 48.) A solution contains an unknown amount of dissolved calcium. Addition of 0.112 mol of K 3 PO 4 causes complete precipitation of all the calcium. How many moles of calcium were dissolved in the solution? What mass of calcium was dissolved in the solution?