Chemistry Tri B Final Review

Chapter 8 Shape

it

Chapter 9

Reactionary

Chapter 10 Stoich

it

Chapter 11 Stoich Master

Chapter 12 Feel the heat

Chapter 13

Passing Gas

Work it

200 200 200 200 200 200 200

400 400 400 400 400 400 400

600 600 600 600 600 600 600

800 800 800 800 800 800 800

1000 1000 1000 1000 1000 1000 1000

Chapter 8200

• What is a Isomer? How are they the same, how are they different.– Same molecular formula, different

structural formula

Chapter 8400

• What are the three types of IMF? Describe them– Hydrogen bonding - FON– Dispersion- shift of electrons in a non

polar substance causing increased attractions between molecules

– Dipole-dipole- attraction between polar molecules

Chapter 8600

• Draw the structures formulas for NH3 and CH4? Are they polar or non-polar– NH3, polar (asymmetrical)

– CH4, non polar (symmetrical)

Chapter 8800

• What is an ionic bond? What is a non-polar covalent bond? A polar covalent bond?– Metal to nonmetal transfer of e-– Non-metal to non-metal with similar or

same EN (equal sharing of electrons)– Non-metal to non-metal with different

EN (unequal sharing of electrons)

Chapter 81000

• Write the formulas for magnesium fluoride, zinc oxide, oxygen, hydrogen fluoride. Indicate if they are ionic, polar or non-polar covalent. Write the polyatomic ions for hydroxide, nitrate, carbonate, sulfate and phosphate.

– MgF2 ionic

– ZnO ionic

– O2 non-polar covalent

– HF polar covalent

– OH- NO3- CO3

-2 SO4-2 PO4

-3

Chapter 9200

• What is the formula for Iron III oxide? Lead II Sulfate? What is the name of Sn(CO3)2 , Cr(OH)3, KNO3

– Fe2O3

– PbSO4

– Tin IV Carbonate– Chromium III hydroxide– Potassium nitrate

Chapter 9400

• Name the type of reaction HCl + Mg(OH)2 MgCl2 + H2O Hydrogen + oxygen produces water H2O2 H2O + O2 NaOH + Li LiOH + Na– Double Replacement– Direct Combination (syn)– Decomposition– Single Replacement

Chapter 9600

• State the Law of Conservation of Matter. How does it apply to balancing a chemical equation– Matter is neither created or destroyed– Must have the same number and

types of atoms on either side of the sign.

Chapter 9800

• How are ionic formulas balanced? How are equations balanced? Name the molecular compound N3F4, CO, P2O5.– Subscripts– Coefficients– Trinitrogen tetrafluoride, carbon

monoxide, diphosphorus pentaoxide

Chapter 91000

• What do you call a solid formed in a chemical reaction that separates from the solution?– A precipitate

Chapter 10200

• What is a formula mass? What is the formula mass of carbonate? What is the molar mass? What is the molar mass of carbon dioxide?– Sum of all the atoms in a formula – 60.01amu– Same as formula mass but expressed

as g/mol– 44.01g/mol

Chapter 10400

• How many water molecules are there in 0.5 moles of water?– 3 x 1023 molecules

Chapter 10600

• How many grams of water are in 3.000 moles of water? (the molar mass of water is 18.02g/mol) How many moles in 22.5g of water?– 54.06g water– 1.25mols water

Chapter 10800

• What is an empirical formula? If the empirical formula is CH4 and the molar mass is 64.2g/mol what is the molecular formula? – Smallest whole number ratio

(simplest terms)

– C4H16

Chapter 101000

• What is the branch of chemistry called that deals with mass relationships among reactants and products? What is an Activity Series used for?– Stoichiometry– Determine if a chemical reaction will

occur

Chapter 11200

• Given the equation N2 + 3H2 2NH3 what is the Molar Ratio of N2 to NH3? How many moles of hydrogen would be needed to make 6 moles of ammonia?– 1:2– 9 moles

Chapter 11400

• Given the combustion reaction of CH4 + 2O2 CO2 + 2H2O What is the molar ratio of oxygen to water? How many grams of methane would be needed to produce 2.000 moles of carbon dioxide?– 2:2 or 1:1– 32.10 g methane

Chapter 11600

• Given the reaction 2FeBr3 + 3Ca 3CaBr2 + 2Fe Which would limit the reaction 80.g of FeBr3 or 20.g of Ca? How many moles of Fe would be produced?– FeBr3.

– 0.27 mol

Chapter 11800

• What is the formula for %yield? Given MgO + H2O Mg(OH)2 Which would limit the reaction 20.g of MgO or 20.g of H2O? What would the % yield be if 24.0g of Mg(OH)2 were produced?– Actual(measured) / Expected(calculated) x

100– MgO– 83%

Chapter 111000

• What volume of oxygen at STP is required to burn 500.g of glucose? If 600.g of CO2 are produced what is the % yield? C6H12O6 + 6O2 6CO2 + 6H2O – 373L – 81.9%

Chapter 12200

• What is the amount of heat required to raise the temperature of one gram of a substance by 1°C called? What are the units for specific heat?– specific heat– J/g*oC

Chapter 12400

• What is the sign of an exothermic rxn? What happens to the temperature of the surroundings during an exothermic rxn?– negative– It increases

Chapter 12600

• Standard pressure is? How much heat is transferred when 9.22g of glucose reacts with excess oxygen C6H12O6 + 6O2 6CO2 + 6H2O delta H= -2803kj– 1atm– 144kj

Chapter 12800

• Use Hess’s Law to calculate the delta H net of the equation 2S + 2O22SO2 Given the equations 2SO2 + O2 2SO3. Delta H = -196kj 2S + 3O2 2SO3. Delta H = -790kj– -594kj

Chapter 121000

• What do you do to the sign of the delta H in calculating a net equation if you have doubled the coefficients?– Double it.

Chapter 13200

• What is the conversion factor between atm and mmHg?

• How do gases transfer energy?– 1atm = 760mmHg– converction

Chapter 13400

• Convert .75atm to mmHg? Convert 825mmHg to atm– 570mmHg– 1.09atm

Chapter 13600

• When do gases diffuse fastest, hot or cold temps? Which is more dense a liquid or a gas of the same substance? Describe a gas/liquid solubility curve

–Hot. Higher temp higher KE faster movement!–Liquid–Inverse

Chapter 13800

• If you decrease the pressure on a container what will happen to the volume? Which gas will diffuse faster CO or CO2 explain your answer. What will be the new pressure on a container that was 2L at 1atm if the volume was changed to 1L?– It increases– CO the gas molecules are smaller– 2atm

Chapter 131000

• True or false. When gas particles collide they transfer energy to each other. Explain your answer– False. Collisions are perfectly elastic.

Work it200

• If the empirical formula is XY4, which are possible molecular formulas? X2Y4, X3Y6, X2Y8 or X5Y10

– X2Y8

Chapter Work it400

• Write the balance equation for gaseous oxygen reacting with gaseous hydrogen to create liquid water? Convert 64g of O2(g) to liters

– O2(g) + 2H 2(g) 2H2O(l) .

– 45L

Chapter Work it600

• How much heat is transferred if 150.g of manganese (IV) oxide react given 2MnO2 2MnO + O2. H= +264Kj Is this reaction endo or exothermic? CCaC2 + CO H = 464.8kJ – 228kj absorbed– endo

Chapter Work it800

• What is the empirical formula for a compound containing 2.128g Cl and 1.203 g Ca? – CaCl2.

Chapter Work it1000

• What is the molecular formula for a substance containing 54.1% Ca, 43.2% O and 2.7% H?– Ca(OH)2

Final Jeopardy

• Aluminum reacts spontaneously with bromine to produce AlBr3. If 45.0 g of Al react with 45.0 g of Bromine, which is the limiting reactant?  What is the percent yield if 31.0g of AlBr3 are actually produced?– Bromine– 61.9%