Chemistry Tri B Final Review

1
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
2
Chapter 8200

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

3
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

4
Chapter 8600

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

5
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)

6
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

7
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

8
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

9
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.

10
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

11
Chapter 91000

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

12
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

13
Chapter 10400

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

14
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

15
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

16
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

17
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?
• 12
• 9 moles

18
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?
• 22 or 11
• 32.10 g methane

19
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

20
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

21
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

22
Chapter 12200

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

23
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

24
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

25
Chapter 12800

• Use Hesss Law to calculate the delta H net of
  the equation 2S 2O2?2SO2 Given the equations
  2SO2 O2? 2SO3. Delta H
  -196kj 2S 3O2 ? 2SO3. Delta H -790kj
• -594kj

26
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.

27
Chapter 13200

• What is the conversion factor between atm and
  mmHg?
• How do gases transfer energy?
• 1atm 760mmHg
• converction

28
Chapter 13400

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

29
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

30
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

31
Chapter 131000

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

32
Work it200

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

33
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

34
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 DH 464.8kJ
• 228kj absorbed
• endo

35
Chapter Work it800

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

36
Chapter Work it1000

• What is the molecular formula for a substance
  with an empirical formula of CH2O and a molar
  mass of 150g/mol?
• C5H12O5

37
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