chemistry final review 2 nd semester, 2014-2015. unit 1: basics how many sig figs are in the...
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Chemistry Final Review
2nd Semester, 2014-2015
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Unit 1: Basics
• How many sig figs are in the following numbers?
• 2300• 2• 314• 3• 2.06• 3
• 0.0025• 2• 9.001• 4• 6.02x1023
• 3• 587.0• 4
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Unit 1: BasicsDiscuss the following in terms of accuracy
and precision
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Unit 1: Basics
• List the three mole conversions you learned at the beginning of the year.
• 1 mol = 6.02x1023 particles (atoms, molecules, ions, etc)
• 1 mol = molar mass in grams from the periodic table
• 1 mol = 22.4 L of GAS at STP see how that makes more sense now ?
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Unit 1: Basics• Write the following in standard or scientific
notation• 2.71x104
• 27100• 6.4x10-3
• 0.0064• 2687• 2.687x103
• 0.012654• 1.2654x10-2
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Unit 1: Basics
• What is the equation for density?• Density = mass volume• What are the common units for density?• g/mL or g/cm3
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Unit 1: Basics
• Give an example of an element and an example of a compound.
• Element: He, C, Mn• Compound: CO2, NaCl, etc (anything with more
than one element)
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Unit 1: Basics
• Write the equation for percent yield.• % yield = actual x 100 expected• Write the equation for percent error.• % error = (actual-expected) x 100 expected
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Unit 2: Atoms & Periodic Table
• Complete the following table:Element/ion
Atomic number
Atomic mass
Protons Neutrons electrons
Fe
Cl-
K+
26 55.85 26 2630
17 17 181835.45
19 1819 2039.10
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Unit 2: Atoms & Periodic Table
• Positive ions form when:• Atoms lose electrons (usually metals, on left of
table)• Negative ions form when:• Atoms gain electrons (usually nonmetals, on right
of table)• Why do atoms form ions?• To become more stable, get the configuration of
a noble gas.
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Unit 2: Atoms & Periodic Table
• The halogens make a charge of ____ when they become ions.
• -1• The alkali metals make a charge of ___ when
they become ions.• +1• The alkali earth metals make a charge of ___
when they become ions.• +2
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Unit 2: Atoms & Periodic Table
• The halogens make a charge of ____ when they become ions.
• -1• The alkali metals make a charge of ___ when
they become ions.• +1• The alkali earth metals make a charge of ___
when they become ions.• +2
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Unit 2: Atoms & Periodic Table
• What are the three types of nuclear decay?• Alpha, Beta, Gamma• What type of particle does each emit?• Alpha = helium nucleus (2 protons, mass of 4)• Beta = electron (no mass, -1 proton)• Gamma = high energy (no mass, no proton
change, but product is more stable)
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Unit 2: Atoms & Periodic Table
• Complete the following:• Type of Decay• ________ 99m
43Tc 9943Tc + ______
• ________ 24795Am 0
-1e + _____
• ________ 17593Np 4
2He + ____
00γ
24796Cm
17191Pa
Gamma
Beta
Alpha
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Unit 2: Atoms & Periodic Table
• Draw a Bohr model for Beryllium.
• Draw a Bohr model for Silicon.
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Unit 2: Atoms & Periodic Table
• There will be no electron configuration on the final (s, p, d, f).
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Unit 3: Compounds & Bonding
• Which types of elements participate in ionic bonding?
• Metals (+) and non-metals (-) (also polyatomic ions)
• Which types of elements participate in covalent bonding?
• Non-metals and non-metals (they share electrons instead of charges sticking together)
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Unit 3: Compounds & Bonding
Name the following compounds:
• MgO• Magnesium oxide• AlF3
• Aluminum fluoride• NiSO4
• Nickel (II) sulfate• FeCl2
• Iron (II) chloride
• N2O5
• Dinitrogen pentoxide• SF4
• Sulfur tetrafluoride
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Unit 3: Compounds & Bonding
• Describe a polar bond.• Covalent bond (non-metal and non-metal) in
which electrons are shared UNEVENLY (one atom is more electronegative than the other).
• Draw a water molecule and show its polarity.
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Unit 3: Compounds & Bonding
• There will be no molecular shapes on the final.
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Unit 3: Compounds & Bonding• List and describe the 4 types of Intermolecular
forces (IMF).• Dispersion forces (weakest, between nonpolar
molecules)• Dipole-dipole interaction (stronger, between
polar molecules)• Hydrogen-bonding (STRONG, between molecules
with N, O, or F bonded to H, explains water’s high boiling point)
• Ion-molecule interaction (strongest, how water dissolves salt – pulls apart the ions)
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Unit 4: Energy Transfer
• Draw a heating curve for water.
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Unit 4: Energy Transfer
• Label the Q-equations for each section.
Q=mcΔT
Q=mHv
Q=mHf
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Unit 4: Energy Transfer
• Find the value for Hf, c, and Hv in your data book.
• Hf = 79.72 cal/g• C = 1.0 cal/g°C• Hv = 539.4 cal/g
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Unit 7: SolutionsUse Table E to determine
the solubility of each substance:
ammonium chloride barium
carbonate silver iodide mercury
(II) bromide
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ammonium chloride soluble
barium carbonate nearly insoluble
silver iodide nearly insoluble
mercury (II) bromide slightly soluble
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Unit 7: SolutionsUse Table D:
1. How many grams of sodium nitrate will dissolve in 100 g of
water at 25 C?2. How many grams of ammonia (NH3) will dissolve in 100 g of
water at 100C?3. If 140 g of KI is dissolved in 100 g
of water at 30 C, is the solution saturated, supersaturated, or
unsaturated?
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92 g
7 g
unsaturated
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Unit 8: EquilibriumDescribe a system at
equilibrium for each case:liquid and gas phases of the same substance in a closed
container reactants and products in a
chemical systema saturated solution
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33A.liquid + gas in a closed container with equal # of molecules condensing as are evaporating; rate of condensing = rate of evaporatingrate of forward reaction is equal to rate of reverse reactionrate of dissolving is equal to rate of precipitation or crystal growth/formation
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Unit 8: EquilibriumUse LeChatelier’s Principle and
the following reaction:
PCl3(g)+3NH3(g)P(NH2)3(g)+3HCl(g)
If [PCl3] increases then [HCl]…If pressure increases then [NH3]…
If [P(NH2)3] increases then [HCl]…
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35A.
If [PCl3] is increased then [HCl]… increases.
If pressure is increased then [NH3]…is constant.
If [P(NH2)3] is increased then [HCl]…decreases.
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The last seven questions will give you practice doing
basic chemistry conversions and
doing stoichiometry.
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44.
How many moles are in 3.6 g of sodium chloride?
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44A.
0.062 mol
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45.
What is the volume of 2.3 moles of oxygen? (at STP)
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45A.
52 L
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46. How many atoms of mercury are in 5.0 moles of mercury?
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46A.
3.0 x 1024 atoms
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47. How much space does 64 g of oxygen
occupy?
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47A.
45 L O2
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48. What is the mass of 3.75 x 1022
molecules of CO2?
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48A.
2.74 g CO2
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49. In ammonia production, nitrogen and hydrogen are synthesized into ammonia (NH3). What mass of ammonia will be produced from 1.5 kg of nitrogen assuming that hydrogen is in excess? (Hint: first write the complete, balanced equation)
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49A.
N2 (g) + 3H2 (g) 2NH3(g)
1.8 kg NH3
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50. A solution made from 5.0 g of copper (II) sulfate is mixed with a solution containing excess calcium nitrate. A precipitate of calcium sulfate is formed.
a) Write the complete, balanced
equation for the reaction. b) Write the complete ionic
equation for the reaction. c) Write the net ionic equation for
the reaction.
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50. A solution made from 5.0 g of copper (II) sulfate is mixed with a solution containing excess calcium nitrate. A precipitate of calcium sulfate is formed.
Continued: d) How much (mass) calcium
sulfate is expected? e) If the amount of CaSO4
measured in the experiment was 3.99 g, what is the percent error?
f) What is the percent yield?
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50A.a) CuSO4 (aq) + Ca(NO3)2 (aq)CaSO4 (s) + Cu(NO3)2 (aq)
b)Cu2+ +SO42-+ Ca2+ + 2NO3
- CaSO4 (s) +Cu2+ + 2NO3-
c)SO42- + Ca2+ CaSO4(s)
d)4.3 g CaSO4
e)-7.2%f)93%