Download Instructions for AP/IB 2 Chem Summer Assignment Note

Instructions for AP/IB 2 Chem Summer Assignment
Note: Future AP/IB chemistry students are expected to learn the material in this
packet before class starts in the fall. Most of this is a review of names, formulas
and reactions that were learned in pre-AP/IB chemistry. Since this class is AP and
IB chemistry combined, there will not be enough time to review this material in
class.
Study the examples before completing the questions. For more detailed
information, download the chemical reactions power point from my webpage
(AP/IB 2 chemistry). Or go back and review your Chem I notes on ionic bonding,
covalent bonding and chemical reactions.
This assignment will count as a major grade and is due the second day of class. It
will be spot checked for correctness (i.e. it’s not just a completion grade; it will be
scanned and points deducted for things that are obviously not even close to the
correct answer).
AP/IB 2 Chemistry: Summer Assignment
Name_______________________
Memorize these element names and symbols:
H= hydrogen
He = helium
Li = lithium
Be = beryllium
B = boron
C = carbon
N = nitrogen
O = oxygen
F = fluorine
Ne = neon
Na =sodium
Mg = magnesium
Al = aluminum
Si = silicon
P = phosphorus
S = sulfur
Cl = chlorine
Ar = argon
K = potassium
Ca = calcium
Sc = scandium
Ti = titanium
V = vanadium
Cr = chromium
Mn = manganese
Fe = iron
Co = cobalt
Ni = nickel
Cu = copper
Zn = zinc
As = arsenic
Se = selenium
Br = bromine
Kr = krypton
Rb = rubidium
Sr = strontium
Pt = platinum
Ag = silver
Cd = cadmium
Sb = antimony
I = iodine
Xe = xenon
Cs = cesium
Ba = barium
Au = gold
Hg = mercury
Sn = tin
Pb = lead
Rn = radon
Ra = radium
U = uranium
Pu = plutonium
Bi = bismuth
Memorize these ion oxidation numbers:
A groups:
generally metals are cations (+) and nonmetals are anions (-)
Group #
1 A (alkali metals)
2 A (alkaline earth metals)
3A
4A
5A
6A
7 A (halogens)
8 A (noble gases)
Oxidation #
+1
+2
+3
+4 or -4 (depends)
-3
(except Bi5+)
-2
-1
No ions; no compounds
examples
Li+, Na+, K+
Mg2+, Ca2+, Ba2+
Al3+, Ga3+, In3+
C4+, C4names end in –ide N3-, P3-, As3O2-, S2-, Se2Ex: oxide, chloride F-, Cl-, Br-. I-
B groups (and tin and lead): Transition metals; most have multiple oxidation numbers
Ag+,
Zn2+ , Cd2+ ,
Ni2+, Ni3+
Hg+, Hg2+,
Cu+, Cu2+
Mn2+, Mn3+, Mn4+, Mn7+
Fe2+, Fe3+,
V2+, V3+, V4+, V5+
+2 is most common
Co2+, Co3+,
Cr2+, Cr3+, Cr6+
Pb2+, Pb4+,
Sn2+, Sn4+
Polyatomic ions (Memorize these!):
NO3- = nitrate
CN- = cyanide
MnO4- = permanganate
NO2- = nitrite
SCN- = thiocyanate
IO3- = iodate
BrO3- = bromate
SO42- = sulfate
HSO4- = hydrogen sulfate
S2O32- = thiosulfate
NH4+ = ammonium
(bisulfate)
SO32- = sulfite
HSO3- = hydrogen sulfite
C2O42- = oxalate
OH- = hydroxide
(bisulfite)
PO43- = phosphate
HPO42- = hydrogen phosphate
CO32- = carbonate
PO33- = phosphite
H2PO4- = dihydrogen phosphate
HCO3- = hydrogen carbonate
(bicarbonate)
-
ClO3 = chlorate
-
ClO2 = chlorite
-
2-
ClO4 = perchlorate
CrO4 = chromate
-
Cr2O72- = dichromate
ClO = hypochlorite
C2H3O2- or CH3COO- acetate or ethanoate
Determining the formula of a compound:
I.
Ionic Compounds (have a metal and a nonmetal). Use the oxidation numbers to put the
ions together in the correct lowest whole number ratio.
Ex: sodium oxide
iron (III) chloride
zinc sulfate
aluminum hydroxide
Na+ and O2- = Na2O
Fe3+ and Cl- = FeCl3
(roman numeral III means +3)
Zn2+ and SO42- = ZnSO4
Al3+ and OH- = Al(OH)3
use ( ) if 2 or more of polyatomic ion
• You try; write the formula
1. ______________ sodium phosphate
2. ______________ ammonium bromide
3______________ lead (II) nitrate
4.______________ silver sulfide
5.______________ calcium carbonate
6. ______________ potassium dichromate
II.
Covalent Compounds (have 2 nonmetals; no ions; atoms share electrons)
Use the prefixes to determine the number of atoms (1= mono, 2 = di, 3 =tri, 4 tetra,
5= penta, 6 = hexa)
Ex: carbon tetrachloride = CCl4
dinitrogen tetroxide = N2O4
• You try; write the formula
7.__________ carbon dioxide
8.___________ diphosphorus pentoxide
9.__________ sulfur hexafluoride
10.___________ sulfur trioxide
III.
Acids (have H+ with an anion) put the ions together like the ionic ones.
There are 6 strong acids (these dissociate completely in aqueous solution; ex:
HCl exists as H+ and Cl- ions, not as molecules)
Memorize the six strong acids: HCl, HBr, HI, HNO3, H2SO4, HClO4
All others are weak! (dissociate only slightly into ions)
Ex: hydrochloric acid: H+ and Cl- = HCl
hydro…..ic has the –ide ion
(strong)
nitric acid;
H+ and NO3- = HNO3
-ic has –ate ion
(strong)
nitrous acid
+
-
H and NO2 = HNO2
-ous has the –ite ion
(weak)
•
You try; write the formula and indicate if weak or strong
11. _____________ acetic acid (ethanoic)
12._____________ hydrofluoric acid
13._____________ carbonic acid
14._____________ hypochlorous acid
15._____________ perchloric acid
16._____________ sulfuric acid
Naming Compounds
I.
Ionic: Name the metal, then the nonmetal; change the ending to –ide, -ite, or –ate
depending on the identity of the anion. Indicate the oxidation number if it has one
of the metals with more than one oxidation number.
Ex: KI = potassium iodide
Al2O3 = aluminum oxide
Ag2SO3 = silver sulfite
(NH4)2Cr2O7 = ammonium dichromate
CuCl2 = copper(II) chloride
Fe3(PO4)2 = iron(II) phosphate
• You try; name the compound
17._________________________ ZnO
18.________________________ KMnO4
19._________________________ NaClO3
20.________________________ NH4OH
21._________________________ LiH2PO4
22.________________________ PbSO4
23.__________________________ AlBr3
24.______________________ Ba(C2H3O2)2
25.__________________________SnCl4
25._______________________ Cu(NO3)2
26.__________________________ CdS
27.______________________ SrCrO4
28.___________________________ CaC2O4 29.______________________ NaCN
II.
Covalent Compounds (Binary compounds: 2 nonmetals)
Use prefixes to indicate the number of atoms (don’t use mono on the first element)
Prefixes: mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca
Ex: SiF4 = silicon tetrafluoride
30. ________________________ CO
32._________________________ N2O4
ending is -ide
S2Cl2 = disulfur dichloride
31.____________________________ PCl3
33.____________________________ CS2
Types of Chemical Equations: Writing Chemical Reactions
Learn the general formula for each type of reaction. If the reaction occurs in water solution,
you must give the net ionic equation. If it doesn't occur in aqueous solution, the
atoms/molecules do not exist as ions.
Writing the net ionic equation (water solution only!)
1. First memorize the six strong acids and solubility rules for salts (ionic compounds).
Strong Acids
hydrochloric, hydrobromic, hydroiodic, sulfuric, nitric, perchloric
these are completely dissociated into ions so write them as separated ions:
ex: HCl is really H+ and Cl-
HNO3 is really H+ and NO3-
do not write weak acids like this! acetic acid stays as HC2H3O2
Solubility Rules
i) soluble salts: all nitrates, acetates, alkali metals compounds and ammonium compounds
are always soluble (no exceptions).
ii) insoluble salts: compounds of lead, silver, cadmium and mercury (except those trumped
by rule i )
iii) Compounds of calcium, barium, strontium and transition metals are insoluble except
halides (and those trumped by rule i)
These three rules don't cover every possible compound, but they include most compounds that
appear on the AP or IB test. So write soluble compounds as separated ions. Insoluble compounds
precipitate from the solution as a solid. Do not separate the ions for a solid.
ex: calcium nitrate, Ca(NO3)2 is soluble so it exists as Ca2+ and 2 NO3- in solution
lead (II) hydroxide is insoluble so keep it as Pb(OH)2
2. Write the complete equation predicting the products.
3. Cancel the spectator ions. These are ions that are unchanged (must be exactly the same
form on both sides of the equation.
4. Balance the equation using lowest whole number coefficients.
Double Replacement Reaction:
AB + CD → AD + CB (occurs in solution always)
Ex: aqueous solutions of silver nitrate and sodium carbonate are mixed.
Ag+ + NO3- + Na+ + CO32- → Ag2CO3 + Na+ + NO3-
silver carbonate is insoluble
sodium nitrate is soluble
net ionic:
2 Ag+ + CO32- ---> Ag2CO3
sodium and nitrate are spectator ions;
they cancel out and should not appear in the answer
Ex: aqueous solutions of barium chloride and copper(II) sulfate are mixed
Ba2+ + Cl- + Cu2+ + SO42-→ BaSO4 + Cu2+ + Cl-
barium sulfate is insoluble
copper(II) chloride is soluble
net ionic:
Ba2+ + SO42- ---> BaSO4
copper and chloride are spectator ions
Ex: 1-molar hydrochloric acid is neutralized by an equal volume of 1-molar potassium hydroxide
H+ + Cl- + K+ + OH- → K+ + Cl- + H2O
potassium chloride is soluble; water is
not an ionic compound (not made of ions)
leave it intact
net ionic: H+ + OH----> H2O
potassium and chloride are spectator ions
• You try: Write the net ionic equation for these double replacement
reactions:
34. A solution of lead(II) nitrate is added to a solution of sodium iodide.
35. Solutions of calcium acetate (ethanoate) and lithium phosphate are mixed
36. Equal volumes of equimolar nitric acid and sodium hydroxide solutions are mixed
37. A few drops of aqueous nickel (II) nitrate are added to a solution of sodium sulfide
38. Some acetic acid (ethanoic acid) is added to sodium hydroxide solution.
Single Replacement Reaction: A + BC → AC + B
or
BA + C
these occur in aqueous solution so give the net ionic form.
Ex: a piece of zinc metal is placed in a solution of copper(II) sulfate
Zn + Cu2+ + SO42- → Zn2+ + SO42- + Cu
zinc sulfate is soluble
copper product is solid, metallic copper
net ionic: Zn + Cu2+ → Zn2+ + Cu
sulfate is a spectator ion; don't cancel the
solid metal and its dissolved ion (they are
different forms)
Ex: chlorine gas is bubbled through a solution of lithium bromide
Cl2 + Li+ + Br-→ Br2 + Li+ + Cl-
lithium chloride is soluble
chlorine gas and elemental bromine are
both diatomic (HOBrFINCl) elements
net ionic: Cl2 + 2 Br- ---> Br2 + 2 Cl-
lithium ions are spectator ions
Ex: a piece of magnesium metal is added to a solution of sulfuric acid
Mg + H+ + SO4- → Mg2+ + SO42- + H2
magnesium sulfate is soluble
net ionic : Mg + 2 H+ ---> Mg2+ + H2
sulfate is spectator; can't cancel solid
magnesium metal with dissolved magnesium
metals displace hydrogen from an acid.
ion ! hydrogen gas is diatomic
Ex: sodium metal reacts with water
Na + H2O → NaOH + H2
sodium hydroxide is soluble;
net ionic: Na + 2 H2O ----> Na+ + 2 OH- + H2
alkali metals and alkaline earth metals react with water to form hydrogen gas.
This is why sodium explodes in water.
• You try: Write the net ionic equation for these single replacement
reactions
39. A piece of copper wire is placed in a test tube containing silver nitrate solution.
40. Elemental bromine is added to a solution of potassium iodide.
41. Zinc metal is placed in a solution of hydrochloric acid.
42. Calcium metal is added to water.
43. A piece of nickel metal is placed in a solution of copper(II) nitrate
44. A small piece of potassium metal is dropped in a beaker of water.
45. Magnesium metal reacts with a solution of acetic acid (ethanoic acid)
Synthesis Reaction: A + B → AB
usually do not occur in water solution
don't need the net ionic form
Ex: A piece of aluminum metal is dropped into a container of iodine vapor.
2 Al + 3 I2 → 2 AlI3
iodine is diatomic; if metal with nonmetal, use
oxidation numbers to get the ionic compound formula
Ex: Sulfur trioxide gas is streamed into a flask containing calcium oxide
SO3 + CaO → CaSO4
two simple compounds make a more complex compound;
make sure the product is an actual compound
Ex: Nitrogen gas reacts with hydrogen gas in the presence of an iron catalyst
Fe
3 H2 + N2 → 2 NH3
The Haber Process (know this one by heart!)
Ex: Carbon dioxide gas is bubbled through water
CO2 + H2O → H2CO3
nonmetal oxides always react with water to make
an acid
Ex: Magnesium oxide is added to water
MgO + H2O → Mg(OH)2
metal oxides react with water to make a base
net ionic: MgO + H2O ----> Mg2+ + 2 OH-
this is in water and magnesium
hydroxide is slightly soluble
• You try: Write balanced equations for these reactions
46. Calcium metal reacts with nitrogen gas
47. A piece of aluminum foil is added to a container of liquid bromine
48. Hydrogen gas reacts with chlorine gas
49 .Sulfur trioxide gas is bubbled through water
50. Solid calcium oxide is added to water
51. Elemental carbon combines with oxygen gas.
Decomposition Reaction: AB → A + B
usually do not occur in solution
Ex: Mercury (II) oxide is heated.
2 HgO → 2 Hg + O2
Ex: Molten sodium chloride is electrolyzed
2 NaCl → 2 Na + Cl2
Ex: Hydrogen peroxide decomposes in the presence of a manganese (IV) oxide catalyst.
MnO2
2 H 2 O2 → 2 H 2 O + O 2
Know this reaction !!
Ex: Calcium carbonate is heated
CaCO3 → CaO + CO2
metal carbonates decompose into the metal oxide
and carbon dioxide gas
Ex: Sodium chlorate is heated
2 NaClO3 → 2 NaCl + 3 O2
metal chlorates decompose into the metal chloride
and oxygen gas
Ex: Hydrochloric acid solution is added to solid sodium bicarbonate
HCl + NaHCO3 → NaCl + H2CO3
this occurs in solution so need net ionic form
H+ + Cl- + NaHCO3 → Na+ + Cl- + H2O + CO2
this reaction is double replacement
and decomposition; carbonic acid
sodium bicarbonate is a solid (not dissolved)
breaks down into water and carbon
do not separate a solid into ions
dioxide.
net ionic: H+ + NaHCO3 ---> Na+ + H2O + CO2
• You try: Write reactions for these decomposition reactions.
53. Molten aluminum oxide is electrolyzed.
54. Electrolysis of water
55. Solid sodium carbonate is heated.
56. Solid potassium chlorate is heated.
57. A catalyst of potassium iodide is added to hydrogen peroxide
58. Several drops of nitric acid are added to solid calcium carbonate
Combustion Reaction: CxHyOz + O2 → CO2 + H2O
(complete; enough O2)
when insufficient oxygen, it also produces CO and C
You should know names and formulas of common organic compounds. See the power
point on organic chemistry on my web page (on pre-AP chem tab)
Ex: butane gas burns in an excess amount of oxygen
2 C4H10 + 13 O2 → 8 CO2 + 10 H2O
Ex: Complete combustion of ethanol
C2H5OH + 3 O2 → 2 CO2 + 3 H2O
• You try: Write reactions for these combustion reactions:
59. Complete combustion of propane gas
60. Complete combustion of methanol