Name ____________KEY______________________ Period ______________Chemistry Final Exam STUDY/ Review Guide

MATTER:Fill in the following chart for TYPICAL Solids, Liquids and Gases (not water)

State of Matter

Particle Arrangemen

t Regular or Irregular

ShapeDefinite or Indefinite

Density Rank

1 = highest3 = lowest

Energy Rank1 = highest3 = lowest

Compressibility

Yes or No

Gas irreg Indef 3 1 Y

Liquid irreg Def 2 2 N

Solid reg Def 1 3 N

Atoms – draw a diagram of an atom of Lithium (mass number 7), labeling the following parts – nucleus, electron cloud, protons, neutrons, electrons

Label as: molecule, atom, compound, substance, homogeneous mixture, heterogeneous mixture

Substance/Molecule - H2O Substance / atom - A single particle of pure potassium Heterogeneous mixture - A sample of sand scooped from a beach Substance / ionic compound - Sodium chloride Homogeneous mixture - Iced tea Atom - The smallest particle of an element that retains all of its chemical

properties Heterogeneous mixture - Chicken soup

PHYSICAL AND CHEMICAL CHANGES AND PROPERTIESClassify the following as a chemical or physical property or chemical or physical change

________ 1. PC - Liquid collects on the side of a cold drink glass________ 2. CP - Hexane is flammable________ 3. CC - Baking soda decomposes in the cake, releasing CO2 to make it

fluffy.________ 4. PP - Copper II sulfate is blue.

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Nucleus – center of atomElectron cloud – outside of nucleusProtons – in nucleus with (+) symbolNeutrons – in nucleus with no symbolElectrons – in energy levels outside of nucleus

________ 5. PC - Ice is melting________ 6. PP - Pure water has a density of 1 g/cm3

STATES OF MATTER:Mark the statements as true or false. If false, make changes to correct the statement.

1. Liquids have the greatest amount of kinetic energy among the phases of matter – FALSE, gases do.

2. In general, a solid is the densest phase of matter. - TRUE3. Particles in a solid demonstrate rotation, vibration and translation. FALSE – no translation

4. The particles of liquids have low amounts of translation unless they are stirred. - TRUE

5. When a solid is melting, its temperature is still rising as it melts. – FALSE – holds steady

6. Both solids and liquids can flow. – FALSE – only liquids can flow7. Translation is the type of kinetic energy in which a particle moves from place to

place. - TRUE

DENSITY CALCULATIONSSolve the following problems involving density calculations. Show all work.What is the formula for density? D= m/v

A cube is 17 cm3 in volume with mass of 4.0 grams. Calculate its density.0.24g/cm3

If a ball has a density of 27.5 g/cm3, determine its volume if its mass is 626 g. 22.8g

METRIC UNITSPerform the following determinations.

________ 1. 1 kilometer (km) = _____1000____ meters (m)________ 2. 1 milligram (mg)= _____.001___ grams (g)________ 3. 1 liter (L) = __1000____ milliliters (mL)________ 4. 2.3 kilograms (kg)= ____2300_______ grams (g)________ 5. 12 meters (m) = ___________1200_______ centimeters (cm)

ATOMIC STRUCTURE:Fill in the following table with the appropriate informationSubatomic Particle

Charge LocationNucleus or electron

Relative Mass Order of Size 1= largest 3 = smallest

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cloudProton +1 Nucleus 1 amu 1

Neutron O Nucleus 1 amu 1(same!)

Electron -1 Electron cloud

1/1640th amu 3

PERIODIC TABLE:Answer the following questionsWhat number of valence electrons indicates the most stable arrangement? Which group on the periodic table fits this description without forming ions? 8 valence e-; noble gases

Elements on the periodic table are organized in order of increasing ____atomic number________.?

Elements are identified by the number of ___protons_____ in their nucleus. The number of ___electrons_______ and ____neutrons_______ may vary.

ORGANIZATION OF THE PERIODIC TABLELabel the following on the diagram below. Then, label the number of valence electrons inside the space for each group.

s-block p-block d-block f-blockmetals non-metals alkali metals alkali earth metalsAluminum group Carbon group Nitrogen group Oxygen GroupHalogens Noble Gases transition metals inner transition metals

s - block

d – blockTransition

Metals

p - block

f – blockInner Transition

Metals

Metals

Non-metals Metalloids Border stairstep

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ELECTRON CONFIGURATION:Write the full electron configuration for the following elements. Circle the valence electrons.

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Helium 1s2

Barium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2

Fluorine 1s2 2s2 2p5

Strontium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2

Oxygen 1s2 2s2 2p4

Neon 1s2 2s2 2p6

BONDINGDraw the covalent structure for the following chemical formulas. Name the shape of the molecule.

a) PBr3

b) SO2

c) SO3

d) PO43-

Indicate the correct word(s) to complete each sentence.________ 1. Ionic bonds are formed between metals and non-metals________ 2. Covalent bonds are formed between non-metals and other

non-metals.________ 3. Metals do not form bonds with other metals________ 4. The transition metals lose electrons to form ions.________ 5. When comparing degree of polarity between two bonds, the

bond with the greatest polarity has the largest difference between the two atoms in the bond.

ELECTRON DOT STRUCTURESDraw the electron dot structure of the valence electrons for the following elements. Indicate which, if any, fulfill the “octet rule” when neutral. If they do not fulfill the octet rule when neutral, indicate the number of electrons gained or lost for the atom to fulfill the rule. Sodium

Magnesium Mg

Aluminum Al

Silicon Si

Phosphorus P

Sulfur S

Chlorine Cl

Argon Ar

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ION FORMATIONFill in the following table regarding ionsElement Group Name Ion Type

cation/anionCharge# and +/-

Metal / Non-Metal

Sodium Alkali metals cation +1 Metal

Selenium Oxygen group

anion -2 Non-metal

Boron B/Al group cation +3 Metalloid

Phosphorus Nitrogen group

anion -3 Non-metal

Calcium Alkaline Earth cation +2 Metal

Fluorine Halogens anion -1 Non-metal

Radon Noble Gases none none Non-metal

Phosphorus Nitrogen group

anion -3 Non-metal

BONDINGFill in the following table regarding ionic bondingCation Charge Anion Charge Balanced

FormulaChemical Name

Calcium +2 Sulfur -2 CaS Calcium sulfide

Strontium +2 Chlorine -1 SrCl2 Strontium chloride

Aluminum +3 Iodine -1 AlI3 Aluminum iodide

Cesium +1 Nitrogen -3 Cs3N Cesium nitride

Magnesium

+2 Oxygen -2 MgO Magnesium oxide

Boron +3 Phosphorus

-3 BP Boron phosphide

Sodium +1 Fluorine -1 NaF Sodium fluoride

POLYATOMIC IONS

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Fill in the following chart Cation Formula

and Charge

Anion Formula and Charge

Balanced Formula

Chemical Name

Calcium Ca +2 Hydroxide OH -1 Ca(OH)2 Calcium hydroxide

Strontium Sr +2 Nitrate NO3 -1 Sr(NO3)2 Strontium nitrate

Ammonium

NH4 +1 Acetate C2H3O2 -1 NH4C2H3O2 Ammonium acetate

Cesium Cs +1 Chlorate ClO3 -1 CsClO3 Cesium chlorate

Magnesium

Mg +2 Cyanide CN -1 Mg(CN)2 Magnesium cyanide

Boron B +3 Sulfate SO4 -2 B2(SO4)3 Boron sulfate

Sodium Na +1 Nitrite NO2 -1 NaNO2 Sodium nitrite

BALANCING EQUATIONS AND REACTION SYMBOLSBalance all equations. Label reaction type for all reactions.1. N2(g) + 3H2(g) 2NH3(g) SYNTHESIS

2. 2KClO3(s) ∆ 2KCl(aq) + 3O2(g) DECOMPOSITION

3. 2NaCl(s) + F2(g) 2NaF(aq) + Cl2(g) SINGLE REP.

4. 2AgNO3(aq) + MgCl2(aq) 2AgCl↓ + Mg(NO3)2(aq) DOUBLE REP.

5. C3H8(l) + 5O2(g) 3CO2(g) + 4H2O(l) COMB.

Answer the following questions based upon the formulas above.1. Rewrite #4 as a word equation. Dissolved silver nitrate and dissolved magnesium chloride react to form solid solver chloride and dissolved magnesium nitrate.

2. What does the subscript “(g) “in #1 and subscript “(s)” indicate in equation 2? Gas; solid

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3. Does equation 3 take place in water? How do you know? Yes; the NaF is dissolved

4. Write the formula for the precipitate in equation 4. Rewrite its name in word format. AgCl↓, silver chloride

5. Write the 3 criteria for identifying a combustion reaction. Hydrocarbon and oxygen are reactants; products are always CO2 and H2O

6. What does “∆” indicate in equation 2? How can you indicate a catalyst in a reaction? Heat; symbol will be written over the arrow.

REACTIONS STOCHIOMETRY and Limiting Reactants:Perform the following stochiometric calculations. Make sure you have a balanced equation first!CH4 + 2O2 CO2 + 2H2OHow many grams of O2 are needed to react with 9.02 g of CH4? 36.1 g O2

2. N2 + 3H2 2NH3How many grams of NH3 are formed when 11.7 g of H2 react? 65.9 g H2

3. 2C + O2 2COHow many grams of carbon are needed to produce 0.98 g of CO? 0.82 g C

4. Silicon dioxide (quartz) reacts with hydrogen fluoride to produce silicon(IV)fluoride and water by the reaction SiO2 + 4HF SiF4 + 2H2O. Determine which is the limiting reactant if 2.0 mol HF is combined with 4.5 mol SiO2? 2.0 mol HF is limiting

5. Using the reaction above, determine which is limiting and which is excess when 46.3 g of SiO2 react with 25.0 g of HF. 25.0 g HF is limiting

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Phase Changes – temperature vs. time:

Phase changes (step diagram) Indicate the following on the graph above.melting, vaporization, solid being heated, liquid being heated, gas being heated, freezing, condensation

Answer the following questions based upon the diagram above.1. Which interval(s) on the graph above indicate a change in kinetic energy? A—B; C-D and E above

2. Which intervals on the graph above indicate a change in potential energy? B-C and D-E

3. At lines A-B and C-D the graph shows plateaus - the temperature is not changing while heat energy is still being added. Describe what the heat is doing to particles of the substance. Breaking bonds

TEMPERATURE

(°C)

TIME (seconds)

GRAPH OF TEMPERATURE VS. TIME FOR A SUBSTANCE BEING HEATED

180170160150140130120110100

908070605040302010

0

A

BD

E

C

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4. Explain the difference between vaporization and evaporation. Give an example for each. Vaporization (boiling) is where the substance becomes liquid from inside and the surface. Evaporation is vaporization from the surface only.

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GASES:Name and describe the three types of particle motion. Indicate the phases of matter that exhibit each.Rotation (spinning in place) – all phasesVibration (shaking in place) – all phasesTranslation (moving from place to place) – Liquid and Gas only

Describe the “Kinetic Theory of Gases” and list the three assumptions associated with it. What volume does one mole of any gas occupy at STP? 22.4 LKinetic theory states that all matter is composed of particles and the particles are in constant motion. Particles are small hard spheres which are not attracted or repelled from each other. They move in straight lines until they impact with something. Between the particles is empty space.

Define “phase change.” This is a physical change which involves changes in the bonds between particles, types of particles, and the types of particle motion. No chemical bonds are made or broken.

Define these types of phase changes. Give an example of where you might experience each.Melting - solid to liquid

Freezing - liquid to solid

Evaporation - liquid to gas (surface only)

Vaporization - liquid to gas

Condensation - gas to liquid

Sublimation - Solid to gas

GAS LAWS:Solve the following problems using the gas laws

1. A gas with volume of 5.3 L at 17°C decreases to -3°C. Find the new volume.

2. A 2.1 L sample of gas a standard pressure is moved to a 5.2 L container. Find the new pressure.

3. An aerosol can contains gas at 15 atm and 25°C. Find the pressure inside the can at 100.°C

4. Find the number of moles of gas in a container at the following conditions – 6.0 atm, 3.6 L, and 118°C.

5. A gas at 742 mmHg and -18°C occupies 1.7 L. Find the volume of the gas at STP.

6. Define absolute zero. Give the temperature for it in both °C and K. -273°C and 0K; temp at which all particle motion ceases

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7. A mixture of four gases is stored at 1187.3 mmHg. H2 is 127 mmHg, O2 is 350 mmHg and CO2 is 642 mmHg. Find the partial pressure of the Helium in the mixture. 68.3 mmHg

8. Under what conditions does a gas stop acting “ideal” and begin acting “real?” low temps / high pressure

9. What volume does one mole of any gas occupy at STP? 22.4L

CONVERSIONSPerform the following conversions.1. 26C to K 299K2. -52C to K 325K3. 89 K to C 184°C4. 304 K to C 31°C

5. 23.5 atm to mmHg 17900 mmHg

6. 89 kPa to Torr 670 Torr7. 768 mmHg to atm 1.01 atm8. 11.2 atm to kPa 1130 kPa

WATER AND SOLUTIONS:Draw a picture of a water molecule. Indicate the poles on this polar molecule.

Write a definition and example for each of the following.Polar – charges on the water molecules (O is slight negative while H is slight positive)

Surface tension – “skin” on water (water strider)

Surfactant - breaks H-bonds (soap)

Specific heat – amount of energy required to raise one g of water by 1°C (1 cal)

Hydrogen bonds – bond b/w adjacent water molecules b/w – O and + H (drops on a penny)

a) Why does solid ice float on liquid water? H-bonds hold water molecules apart; increases spaces between molecules

b) How does soap help to clean dirty dishes? Soap is a surfactant which breaks H-bonds and allows the soap and oil to mix

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MOLAR MASS AND PERCENT COMPOSITIONFind the gram formula mass for the following formulas

BaCl2 208.236 g/mol CuSO4 159.608 g/mol

NaNO3 84.994 g/mol Ba(OH)2 171.3438 g/mol

Determine the percent composition of the followingS in CuSO4 20.1% NO3 in NaNO3 72.9% H2O in CuSO4 * 5 H2O

36.1%

Empirical and Molecular FormulasA compound sample is made of 40.68 g C, 5.08 g H and 54.24 g O. Its molar mass is 118.1 g/mol. Determine the empirical and molecular formula.

A compound sample contains 174.86 g iron and 75.14 g oxygen. Molar mass is 160.0 g mole. Determine the molecular formula.

Acids and BasesWhat helps you to recognize an acid when you look at a chemical formula? What are the general characteristics of acids? H (hydrogen) ion; smell strongly, corrosive, react with bases and metals; conduct electricity

What helps you to recognize a base when you look at a chemical formula? What are the general characteristics of bases? OH (hydroxide) ion; slippery corrosive; react with acids

What two products are always formed from the neutralization of an acid and base? Water and salt

Write the chemical equation for the neutralization of hydrochloric acid and sodium hydroxideHCl + NaOH NaCl + H2O

Write the chemical equation for the neutralization of sulfuric acid and potassium hydroxideH2SO4 + 2 KOH K2SO4 + 2 H2O

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Data Analysis, Significant Figures and Sources of Error:Students want to determine the percent of water in a compound. They heat the substance in a watch glass in order to drive off the water. The raw data they collected is found below. Use this information to answer the questions.

Item CuSO45H2OMass of Empty Watch Glass 46.25 gMass of Watch Glass and Compound before heatingCuSO45H2O

70.65 g

Mass of Watch Glass and Compound after heatingCuSO4

63.33 g

a. What is the mass of the sample of CuSO45H2O they started with?24.40g

b. What is the mass of the water lost?7.32g

c. From the given data, calculate the percent water in the compound. 30.%

d. What is the mass of one mole of this entire compound?249.684 g/mol

e. What is the mass of just the water that is trapped in 1 mole of this compound?

90.074 g/mol

f. From the two previous questions, determine the actual percent (accepted value) of water that makes up this compound.

36.1%

g. Assuming that the accepted value of % water should be 36.1%, determine the % error for this lab group’s results.

16.9 %

h. If their experiment showed the percentage of water to be too low, how might this error have occurred?

Incomplete evaporation

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Determine the number of significant figures in each of the following numbers.

a. 13,000 2

b. 13,000. 5

c. 0.00013 2

d. 9.0 x 109 2

Solve the following correctly, and include the correct label and number of significant figures in your response.

a. A box measures 1.613 m by 6.213 m by 5.15 m. Determine the volume of the box.

51.6 m3

b. You measured the mass of a beaker as 16.255 g. When you added water to the beaker, you measured the mass as 36.04g. Determine the mass of the water in the beaker.

19.79g

c. In B above, what should you have done to allow you to record the mass of the water to the thousandth of a gram?

Read your mass decimal measurement to a thousandth of a gram. (0.001g)

State the rules for use of significant figures within calculations:For addition and subtraction?Round to the same number of decimal places as the addend with the fewest decimals

For multiplication and division?Round to the same number of significant figures as the multiplicand or divisor with the

fewest significant figures.

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That’s it! If you would like additional practice for any of the topics covered on this exam – see me!

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