CHEMISTRY HOMEWORK

Here are some of the answers to the homework.

The idea is to do the problem then check your answer. If you get it incorrect; go back and attempt to find the mistake. It is better for your understanding if you can find your own mistakes and learn from them.

----update 12/15/25 ----

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Chapter 3
Page 67, 96, 93
Page 67
#1) +, -
#2a) 9.314x10(3) b) 8.042x10(-2) c) 5.17x10(-5) d) 7.124369582x10(9)
#4) 35 mm
Page 96
#6a) 888100 b) 0.00008881 c) 773 d) 0.006398 e) 3400000 f) 47.4
#21) paper is smaller than smallest graduation
#52) lead
#57 0.843 g/ml
#72) 4.25
#76) 7.85 g/ml
Page 93
#6) 19 ml
#7a)orange b)blue c)can't tell d)blue

Worksheet #1
Scientific Notation section
1.1x10(2) next 5.72x10(-2) next 3.2x10(-3) next 2.93x10(4) next 8.88x10(4)

x & / section
top row) 1.17x10(8) next 1.38x10(-7)
2nd row) 3.12x10(-8) next 2.99x10(10)

Solve the following section
top row) 21.8 next 22 next 7.40 next 12
2nd row) 447.3 next 5.93 next 2343.4

Tell how many section
top row) 1, 4, 3, 3
2nd row) 3, 1, 1, 2
3rd row) 5, 4, 2, 3
4th row) 2, 4, 4, 7

last Solve the following section
top row) 20 next 7x10(4) or 70,000 next 2.1x10(3) or 2100 next 21
2nd row) 1.8x10(4) next 0.0652 next 36.2 next 43.0

Worksheet #4 & Page 75
Worksheet #4
#1) 390.99 Euro
#3) 1.5 L
#4) 0.020 oz. of platinum
#5) 3.9 days
#7) 110,000 km
Page 75
#4) a)3 b)3 c)4 d)3 e)4 f)6 g)4
#5) a)2 b)1 c)2 d)3
#7) a)2 b)3 c)2

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Chapter 1 & 2
Booksearch

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Chapter 4, 6, 19
Worksheet 3
#1) 1.81x10(24) atoms Al
#2) 37.4 mol Zn
#4) 18.9 grams Cl
#5) 0.0307 mol Ca
#7) 5.91x10(24) atoms O
#8) .822 grams C
#9) 4.95x10(22) atoms W
#10) 14.2 grams H
#11) 4.54x10(22) atoms C
#12) 596 grams S

Worksheet 1 and page 146
Worksheet 1
Ga row.) Gallium-70, 31, 31, 31, 39
Co row.) Cobalt-59, 27, 27, 27, 32
K row.) Potassium-39, 19, 19, 19, 20
Na row.) Sodium-23, 11, 11, 11, 12
Au row.) Gold-197, 79, 79, 79, 118
Cu row.) Copper-64, 29, 29, 29, 35
Hg row.) Mercury-201, 80. 80, 80, 121
bottom row.) O, Oxygen-16, 8, 8, 8, 8
a.) 5p+, 5e-, 6n
b.) 17p+, 17e-, 20n
c.) 13p+, 13e-, 14n
d.) 26p+, 26e-, 30n
Bottom Question: Tungsten-180, Tungsten-183, Tungsten-185, Tungsten-186
*Also write them as nuclear symbols. The 1st one is 180 over 74 and W (written as a nuclear symbol)
page 146
#19) proton (positive) (1 amu)
neutron (neutral) (1 amu)
electron (negative) (0 amu)
#22) different masses (different # of neutrons)
#23) atomic # = # of p+
mass# = p+ + n
can determine # of n
#27) p+, n, e-
a) 94, 150, 94
b) 95, 146, 95
c) 89, 138, 89
d) 55, 78, 55
e) 77, 116, 77
f) 25, 31, 25

Worksheet 39-2 and page 732, 718, 733, 717
worksheet 39-2
if you did it correct you will end with the isotope Pb-207
page 732
#4) same element, different mass, yes (same atomic #), no (different mass #)
#6) a
#7) increase by 1
page 718
#7) 18 hours
page 733
#26) 0.39 mg
page 717
PP 19.3) 20. years

WS #2, WS 40-1, page 729, 733
ws #2
#1) 107.963 amu
#2) 24.32 amu
#3) 28.11 amu
#4) We must account for how common each isotope is in nature.
ws 40-1
#2) 1, 3, 9, 27, 81, 243, 729
#3, 1st equation) 239 over 93 and Np (written as nuclear symbol)
#3, 2nd equation) 239 over 94 and Pu (written as nuclear symbol)
#4, 1st equation) 3
#4, 2nd equation) 80 over 32 and Ge (written as nuclear symbol)
#4, 3rd equation) 141 over 54 and Xe (written as nuclear symbol)
#5, both equations) 1 over 0 and n (written as nuclear symbol)
page 733
#34) fission is splitting atom into smaller atoms, fusion is combining atoms into larger atoms
#35) nuclear stuff is way, much more energy
#37) neutrons are absorbed to cause the reaction but more neutrons are produced causing the "chain reaction"
#54) a)T b)T and F (it depends on the type of decay) c)F (not on earth) d)T
#61) 48 grams

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Chapter 11 &4
Worksheet 1
#2a) +65.9 kcal and absorbed
#2b) -22.3 kcal and emitted
#2c) -43.6 kcal and emitted
#5) excited (high energy) e- go to a lower "orbit" (closer to the nucleus) and release the extra energy as light

Worksheet 2
#1) Aufbau Principle, Hund's Rule, Pauli Exclusion Principle
#6) a)8 b)8 c)2 (shells 1&2) d)3 (subshells 1s, 2s, 2p)
#7) a)15 b)15 c)3 (shells 1,2,3) d)5 (subshells 1s, 2s, 2p, 3s, 3p)
e- configuration section
C) 1s2,2s2,2p2 and orbital is 1s(up and down arrow),2s(up and down arrow),2p(up arrow and up arrow and empty orbital)
Zr) ends 4d2 and orbital ends 4d( up arrow and up arrow and 3 emtpy orbitals)
W) ends 5d4 and orbital ends 5d(4 up arrows and one empty orbital)

Worksheet 3
#1) 8 something somewhere
#2) a)P b)K g)Br j)Ce l)Ag
#3)
K a. [Ar]4s1 b. 4s1 c. K with one dot d. 1 valence e-

S a. [Ne]3s23p4 b. 3s23p4 c. S with two pairs of dots and two single dots d. 6 valence e-

V a. [Ar]4s23d3 b. 4s2 c. V with two single dots d. 2 valence e-

Mo a. [Kr]5s24d4 b. 5s2 c. Mo with two single dots d. 2 valence e-

Page 415, 421, 111, 133, 141, 146
Page 415
#7) atomic size decreases across a row, increases down a column
ionization energy increases across a row, decreases down a column
Page 421
#50) very reactive, soft compared to other metals
#51) very reactive, muliple states of matter in one group
#53) as we move to the right the nucleas becomes stronger (more protons) so it holds the electrons tighter
#54) as we move down there are more shells of electrons
#57) a) O b) Na c) Mg d) F
#58) a) Ar, S, Al, Na
b) Li, K, Rb, Cs
c) Kr, Br, As, Ca
#66) a)1 b)5 c)3 d)2
#75) a) F b) Lu c) Po d) Fr e) At or Ts f) Xe g) Lr
Page 133
#1) periodic means repeated properties are regular intervals
#2) similar properties
#4) nonreactive
#7)
Li 3 M alkali metal
Br 35 NM halogen
Kr 36 NM noble gas
Mg 12 M alkaline earth metal
Cu 29 M transition metal
Page 141
#2) F-1, anion
#3) Li+1, cation
#4) Group 1(+1), 2(+2), 13(+3), 14(+/-4), 15(-3), 16(-2), 17(-1), 18(no ion)
Page 146
#30) vertical, groups
#31) metals are bendable and conduct electricity, nonmetals are brittle and don't conduct electricity
#32) left of the stairs, more metals
#36) have properties of both metals and nonmetals, staircase
#43) Al+3 (10)
Fe+3 (23)
Mg+2 (10)
Sn+2 (48)
Co+2 (25)
Co+3 (24)
Li+ (2)
Cr+3 (21)
Rb+ (36)
Pt+2 (76)

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Chapter 12 (14 , 5)
Page 434, 449, 462
Page 434
#1) A chemical bond is a force that holds groups of atoms together. The e- is most important.
#4) O2 on the left, HF in the middle, NaCl on the right
Page 449
#1) An octet is a full shell (8 valence e-). This is good because it is low energy.
Page 462
#4) Cl2 is covalent nonpolar, HCl is covalent polar
#5) H2 is covlalent nonpolar, HF is covalent polar, NaF is Ionic
#6) Electronegativity tells how much an atom wants e- in a covalent bond
#8) a) H is most, K is least
b) F is most, Na is least
c) F is most, B is least
#9a) C b) PC c) PC d) I
#11a) H-O b) H-F c) H-F d) H-O
#25) + and - ions packed tightly in a repeating pattern

Worksheet 1 & Bubble WS
worksheet 1
NaF Ionic, a transfer of 1e- from Na to F
NH3 Covalent, 3 boxes or circles showing sharing (2e- in each box)
K2S Ionic, a transfer of 1e- from each K to S
HCl Covalent, 1 box or circle showing sharing (2e- in the box)
CH4 Covalent, 4 boxes or circles showing sharing (2e- in each box)
MhCl2 Ionic, a transfer of 2e- from Mg, 1e- to each Cl
H2 Covalent, 1 box or circle showing sharing (2e- in the box)
O2 Covalent, 2 boxes or circles showing sharing (2e- in each box)
N2 Covalent, 3 boxes or circles showing sharing (2e- in each box)
Al2S3 Ionic, a transfer of 3e- from each Al, 2e- to each S
bubble ws (some of the bubbles have more than 1 correct option, so put anything that makes sense)

Worksheet 2A
#1) do it
#2) a molecule with a charge
#4a) Barium Sulfate
#4b) Barium Sulfide
#4d) Lead IV Oxide
#4e) Ammonium Bicarbonate
#4h) Zinc II Phosphate
#4i) Potassium Nitrate
#5c) K2S
#5e) FeO
#5h) Sr(NO3)2
#5i) Na3PO4
#6) ammonium row: NH4Cl, (NH4)2CO3, NH4OH, (NH4)2SO4, (NH4)3PO4, NH4NO3
iron (II) row: FeCl2, FeCO3, Fe(OH)2, FeSO4, Fe3(PO4)2, Fe(NO3)2
aluminum row: AlCl3, Al2(CO3)3, Al(OH)3, Al2(SO4)3, AlPO4, Al(NO3)3

Page 463
#33) a) 32 b) 17 c) 30 d) 14
#34a) N in the middle with a pair of e-, three single bonds each to a H
#34b) C in the middle, four single bonds each to a Cl, and each Cl has 3 pairs of e-
#34c) N in the middle with a pair of e-, three single bonds each to a Cl, and each Cl has 3 pairs of e-
#34d) Si in the middle, four single bonds each to a Br, and each Br has 3 pairs of e-
#35a) N in the middle with a pair of e-, three single bonds each to a Br, and each Br has 3 pairs of e-
#35b) one single bond, and F has 3 pairs of e-
#36a) O in the middle with two pairs of e-, two single bonds each to a Cl, and each Cl has 3 pairs of e-
#37a) S in the middle, four single bonds each to a O, and each O has three pairs of e-, entire thing in brackets with -2
#37b) P in the middle, four single bonds each to a O, and each O has three pairs of e-, entire thing in brackets with -3
#37c) S in the middle, three single bonds bonds to a O, and each O has three pairs of e-, entire thing in brackets with -2

Worksheet 3 and page 462
#3) AB3E has a pair of unshared e- on the central atom which push the "B" atoms together. AB3 doesn't have unshared e- on the central atom.
#4 I2) single bond and each I has 3 pairs of dots, linear, nonpolar
#4 SiH4) Si in middle with 4 single bonds, tetrahedral, nonpolar
#4 HCN) C in middle with single bond to H and triple bond to N and N has 1 pair of dots, linear, polar, + pole near H and - near N
#4 HCl) single bond and 3 pairs of dots on Cl, linear, polar, + pole near H and - near Cl
#4 BI3) B in middle with two single bonds each to a I with 3 pairs of dots and one double bond to I with 2 pairs of dots, triangular planar, nonpolar
#4) SiS2) Si in middle with two double bonds each to S with two pairs of dots, linear, nonpolar
Page 462
#16a) arrow pointing towards F, + pole on P, - pole on F
#16d) no arrow and no poles, it's nonpolar
#54) least polar is P-S (technically, N-N is even less because it is nonpolar)

Worksheet 4
#2 left column) CCl4, CO, P2O5, N4F6
#2 right column) SiO2, SO3, As2S3, C8Br9
#3 left column) carbon dioxide, phosphorus pentachloride, sulfur dioxide, dinitrogen tetroxide, diarsenic pentoxide
#3 right column) carbon tetrachloride, carbon disulfide, phosphorus tribromide, carbon tetraiodide, heptasilicon octaiodide
#4) polar dissolves in polar, nonpolar dissolves in nonpolar
#5) water soluble pens are polar (like water), permanent pens are nonpolar
#6) Hint: look up the term "induced dipole" (by the way, "dipole" means two poles, so it basically means "polar")
#7) two of the same atom covalently bonded together

Worksheet 5 & 2B
WS 5
#1a) intermolecular forces are bewteen molecules
#1a) weaker
#2) "inter" is between and "intra" is within
#4) as the molecule gets bigger the LDF force gets bigger
#5) CH4 only has LDF (so weakest), PH3 has LDF & DD (so middle strength), NH3 has LDF & DD & HB (so strongest)
#6) all only have LDF but as the molecule gets more electrons the LDF gets stronger
#7) HCl is a molecule (covalent) with only Intermolecular Forces (which are weak). LiCl is ionic (much stronger)
#8) C25H52 is so BIG it has a lot of electrons (so big LDF). In this case the LDF is even stronger than the LDF, DD, HB of water.
WS 2B
#1a) FeBr2
#1b) FeBr3
#1c) Cu(NO3)2
#1e) SiO4
#1f) NaC2H3O2 or NaCH3COO (*Note: you will have to look up the polyatomic ion "acetate")
#1g) SnO2
#1h) SBr3
#1j) Mg3(PO4)2
#1k) Li2CrO4
#1m) K2CO3
#1n) (NH4)2SO4
#2a) Nitrogen Dioxide
#2b) Silver(I) Iodide
#2c) Silver(III) Nitrate
#2e) NH4OH
#2g) Sodium Chromate
#2h) SF
#2i) Iron(II) Sulfate
#2j) Fe3(PO4)2
#2k) Trisulfur Heptanitride
#2l) Al(HCO3)3
#2m) NiCO3

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Chapter 6, 7, 8.3, 9
Worksheet #1
#3) 215.21 g/mol
#5) 40.4 g NaOH
#7) 3.0x10(24) FU KOH
#9) 6.9x10(22) atoms Ca
#12) 3.5x10(24) total atoms
#13) 8.96x10(-5) mol Juglone
#14) 334 g CaCl2
#15) 5x10(15) MC Isopentyl acetate

Worksheet #2
#3) BaCl2 • 5H2O
#5) Sodium Bromide Tetrahydrate
#7) Potassium Hydroxide Dihydrate
#10) 52.13 %C
#11) 13.2 %H
#12) 34.72 %O

Worksheet #3
#1) C3H4O3
#2) CH
#5) Na2SO3
#7) Fe2S3
#8) C6H12O6 and it is glucose
#10) C8H10N4O2

Worksheet #4
#1) 3 , 1 , 1 , 3
#4) 16 , 3 , 8
#6) Cl2(g) + 2LiI(s) --> 2LiCl(s) + I2(s)
#8) CH4(g) + 2O2(g) --> ("spark" over the arrow) CO2(g) + 2H2O(l)
#10) K2CO3(s) + BaCl2(s) --> 2KCl(s) + BaCO3(s)
#11) 4Fe(s) + 3O2(g) --> 2Fe2O3(s)
#12) C6H12O6(s) + 6O2(g) --> 6CO2(g) + 6H2O(l)

Worksheet "Types of Chemical Reactions" 
Model 1 Set A) Synthesis B) Decomposition C) Single Replacement D) Double Replacement
#4) D, B, A, C
#5) combine, break apart, replace
#7) Yes, . . . 
#8) Yes, . . . 
#9) Both, . . . 
#10) Yes, . . . 
#11) No
#12b) Decomposition
#13) S, DR, D, SR, DR, SR, S, D 
#14a) MgO b) O2 c) MgO2 d) O e) 2Mg + O2 --> 2MgO
#21) C and H in the compound
#22a) 5CO2 + 6H2O
#23a) 2C3H7OH + 7O2 --> 6CO2 + 4H2O

Worksheet #5
#4a) Combustion
#4b) 15.8 mol O2
#4c) 9.00 mol CO2
#5a) 2.10 g CO
#6) 2.44 g N2
#7) 1680 g NaOH

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Chapter 14
Page 525, 531, 542
Page 525
#1) inter is between molecules, intra is withing molecules
#2) No, it is an intermolecular force
Page 531
#4) water has LDF, DD, and HB but methane only has LDF
#6) boiling is throughout at the boiling point, evaporation is only at the surface and at any temperature
Page 542
#8) more LDF because more electrons
#12) solid water is less dense than liquid, most things are the opposite of this
#19) intra, inter
#24) evaporation is liquid to gas and requires input of energy, condensation is gas to liquid
#45) g
#46) f
#47) i
#48) d
#57) covalent bond is stronger, breaking it is difficult
#60) volatile means it vaporizes easily, volatile liquids have a high vapor pressure and low intermolecular forces

Page 537, 538, 543
Page 537
Practice Problem 14.4) a)Covalent Molecular b)Ionic c) Metallic
Page 538
#1) Salt is Ionic, sugar is Covalent Molecular
#2) Covalent Molecular is help together with Intermolecular Forces, the other 3 are held together with bonds
#4) metals are bendable
#5) a)Covalent Molecular b)Covalent Molecular c)Ionic d)Metallic
Page 543
#35) Ionic is made of ions (usually a metal and a nonmetal). Example: NaCl solid is made of Na+ and Cl- ions
Molecular is made of molecules (no ions) (always nonmetals). Example: H2O solid is made of H2O molecules
#38) ionic bonds are stronger than intermolecular forces
#39) weaker
#50) a
#51) c
#52) l

Page 525 and 542
Page 525
#5) same substance
#6) energy is separating the particles
#8) 33.35kJ to melt 100.0 g of ice, and 14.73g of water could be vaporized
Page 542
#22a) vaporization is completely searating the particles
#22b) 10.9 kJ
#22c) -2.00 kJ
#22d) 1.13 kJ
#44) j

Worksheet #2 and worksheet VP & B
worksheet #2
#1b) H2O
#4) solid is more dense
#5) solid is less dense
#6a) CH2O
#6b) H2O
#7a) about .39 atm
#7b) about 85 °C
#7c) about 75 °C
#8) -56.6 kJ
#9) 2.92 kJ / mol
worksheet VP & B
(Note: answers are approximate due to reading of the graph)
#1) 37 °C
#2) 69 °C
#3) 98 °C
#4) 375 torr
#5) 190 torr
#6) 60 torr
#7) 53 °C
#8) 82 °C
#9) 110 °C
#10) C

Final Exam Review
#1a) 0.0350L
#1b) 5.32m
#1c) 5360ml
#1d) 615g
#2) 21.22cc (Note: cc is same as ml)
#3) (physical:) ice melting into water (chemical:) iron rusting with water
#4) 92protons, 92electrons, 146neutrons, mass # = 238
#5) An atom that has a different number of neutrons and a different mass #
#6a) 39
#6b) 8
#6c) 13
#7) 6.0x10(23) atoms Zn
#8) 1.20x(24) molecules O2
#9) 2.71x10(24) atoms
#10) 12.2800amu
#11) 2.000 mol Ca
#12) 3.012x10(23) atom
#13) simplest is the lowest atom to atom ratio, molecular is the real formula of the compounds
#14) CuCl2
#15) C2H6
#16a) 1, 3, 2
#16b) 0.2033mol N2
#16c) 31.26g NH3
#17) 2K(s) + Br2(l) --> 2KBr(s)
#18) Synthesis
#19) 2Al(s) + 6HCl(aq) --> 3H2(g) + 2AlCl3(s)
#20) Single Replacement (or Single Displacement)
#21) proton about equal to neutron, and electron is MUCH less
#22) increase up and right. F is the highest
#23) increase down and left
#24) metals (most of the table, middle, left, and bottom), nonmetals (right side), metalloids (touching the "staircase")
#25) halogens = F,Cl, Br, I (group 17)
alkali = Li, Na, K, etc. (group 1)
alkali earth metals = Be, Mg, Ca, etc. (group 2)
#26) energy needed to remove an e-
#27) +2, -1, 0
#28) conduct electricity always, have luster, are malleable, are ductile, conduct heat
#29) 1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p5 then [Ar]4s2,3d10,4p5 then 4s2,4p5
#30) a.)14 b.)3 c.)26
#31) two arrows on a 1s orbital, two arrows on a 2s orbital, 5 arrows on a 2p orbital
#32) capitol N with 5 dots (3 single and 2 paired)
#33) S in middle with two single bonds, each to H, and two pairs of e- on the S, then bent shape
#34a and b and d) 1s2,2s2,2p6
#34c) 1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p6
#34e) 1s2,2s2,2p6,3s2,3p5
Same e- config. are N-3, Al+3, Ne
#35) covalent = sharing, ionic = transfer, metallic = sea of
#36) Mr. Jones
#37) a)potassium nitride b)oxygen c)ammonium chloride d)copper(II) chloride e)lithium chloride f)calcium chloride g)iron(III) oxide h)dinitrogen tetroxide
#38) a)Na2O b)CCl4 c)MgF2 d)Cu3N e)K3PO4 f) Ca(NO3)2
#39) metals, nonmetals
#40) 2C4H10 + 13O2 --> 8CO2 + 10H2O
#41) Covalent
#42) solid at room temp., high MP, conduct electricity in liquid form
#43) LDF, DD, HB
#44) light (photons)
#45) geometry (shape) and electronegativity
#46) No (overall arrowness cancels)
#47) double covalent bond
#48) look at your notes
#49) a)metallic b)cov. mol. c)cov. net. d)ionic
#50) 2.5g
#51) look at notes
#52) heat in vs. heat out
#53) 72.71% O

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SECOND SEMESTER
Chapter 13 (3)
Page 98, 504, 507
Page 98
#47) a) 118K b) 473K c) 221K
#48) a) 2°C b) 172°C c) -273°C d) -196°C e) 9727°C f) -271°C
Page 507
#2) collisions of gases under gravity
#4) b) 0.989atm c) 1.01atm d) 758.1mmHg f) 819.3mmHg

Page 501, 508, and Graham's Law WS
Page 501
#6) Pressure Total = Pressure of O2 + Pressure of water vapor
PO2 = Ptotal - PH2O
Page 508
#32) 745 torr
#33) 732 mmHg
#61a) 1450. torr
#61b) O2
Graham's Law WS
#1) 236 m/s
#2) 341 m/s
#3) 52.8 m/s
#4) 83.79 g/mol and Krypton
#5) 70.8 g/mol and Chlorine (Cl2)
#6) H2S

WS #3
#1) 9.10 L H2
#2) 0.313 L O2
#3) 236 L NO
#5) 159 L N2
#6) 0.629 mol H2
#7) 1.00 mol N2
#9) 0.00313 mol NH3

Page 508
#20a) 5130 mmHg
#20b) -16 °C
#20c) 0.201 L
#20d) 0.0248 mol
#21) 2.01 L
#22) 3.66 g H2
#33) (2nd question) 0.0197 mol O2

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Chapter 15 & 8.1
WS #1
#1a) suspension b) solution c) colloid d1) solution d2) suspension d3) colloid d4) colloid
#2a) hetero b) homo. c) homo.
#3a) elec. b) nonelec. c) nonelec. d) nonelec. e) elec. f) elec.
#5) warm soda will go flat first 'cuz gases are less soluble in higher temperature solvents
#7a) aq b) aq) c) org d) org e) aq f) aq g) org h) org
#8) NaCl
#9) KNO3
#10a) NH3 and Ce2(SO4)3
#10b) gas
#12a) about 14°C
#12b) about 50°C
#13a) about 80
#13b) about 103 g KNO3 in 100 g H2O
#14) about 124 g KNO3
#15) 300. g H2O
#16) a pickle (of course)

WS #1B
#1) 20.0 % sugar
#2) 12.1 % salt
#3a) .250 M NaOH
#3b) .0830 M Pb(NO3)2
#3c) .662 M NaCl
#4a) 596 g CaSO4
#4b) 7.01 g KOH
#4c) .490 g NH4Br
#5) Measure 20.0 g NaOH. Put in a 1000ml (1L) volumetric flask. Fill to line with water and mix.

WS#2
#2a) NaCl(s) --> Na+(aq) + Cl-1(aq)
#2b) Li2SO4(s) --> 2Li+(aq) + SO4-2(aq)
#2d) Cu(NO3)2(s) --> Cu+2(aq) + 2NO3-1(aq)
#2e) C12H22O11(s) --> C12H22O11(aq)
#2f) KOH(s) --> K+(aq) + OH-(aq)
#2h) FeO(s) --> Fe+2(aq) + O-2(aq)
#2j) Mg(NO3)2(s) --> Mg2+(aq) + 2NO3-1(aq)
#5) C12H22O11 < K2SO4 < NaCl
#6) all three solutions would be the same

WS#3
WS#3
#1 top row) S , S , I , I
#2) precipitate
#5 1st one) net equation is Cl-(aq) + Ag+(aq) --> AgCl(s) spectator ions are K+ and NO3-1
#5 3rd one) no reaction
#5 4th one) net equation is Sr+2(aq) + 2OH-(aq) --> Sr(OH)2(s) spectator ions are NO3-1 and Na+

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Acids and Bases (chapter 16, 8.2, 15.2)
WS #1 & #2
WS#1
#3) strong acids ionize completely, weak acid ionize partially
#4) HI(aq) --> H+(aq) + I-(aq)
HF(aq) <----> H+(aq) + F-(aq)
HNO3(aq) --> H+(aq) + NO3-1(aq)
C3H7COOH(aq) <----> H+(aq) + C3H7COO-(aq)
NH4+1(aq) <----> H+(aq) + NH3(aq)
#5) Take one H+ off of H3PO4, then take one H+ off of H2PO4-1, then take one H+ off of HPO4-2
#6) H2SO4 (sulfuric acid) from burning coal and HNO3 (nitric acid) from burning gasoline
WS#2
#3) NaOH(s) --> Na+(aq) + OH-(aq)
F-(aq) + HOH <----> HF(aq) + OH-(aq)
Sr(OH)2(s) --> Sr+2(aq) + 2OH-(aq)
Zn(OH)2(s) <----> Zn+2(aq) + 2OH-(aq)
NH3(l) + HOH <----> NH4+1(aq) + OH-(aq)
NO2-1(aq) + HOH <----> HNO2(aq) + OH-(aq)
LiOH(aq) --> Li+(aq) + OH-(aq)

WS#3
#3a) H+ + OH- --> HOH
#3b) C6H13COOH + OH- --> HOH + C6H13COO-
#3c) HF + OH- --> HOH + F-
#3d) H+ + NH3 --> NH4+1
#3e) H+ + S-2 --> HS-
#3f) H+ + OH- --> HOH
#6) 1st one) A, B, CA, CB
2nd one) B, A, CA, CB
3rd one) A, B, CA, CB
4th one) A, B, CA, CB

WS#4
#1) HOH <----> H+ + OH-
#2) H+ and OH- concentrations
#5a) 2.5x10(-11) M
#5b) 5.6x10(-6) M
#5c) 2.9x10(-11) M
#5d) 1.1x10(-2) M
#5e) 1.0x10(-7) M
#7a) H+ = 2.5x10(-2)M, OH- = 4.0x10(-13)M
#7a) H+ = 1.6x10(-11)M, OH- = 6.3x10(-4)M
#7a) H+ = 3.5x10(-5)M, OH- = 2.9x10(-10)M
#7a) H+ = 2.6x10(-12)M, OH- = 3.8x10(-3)M

WS#5
#1-4) answers on WS

WS#6 & page 585
WS#6
#1) moles of acid and moles of bas
#3) indicators change color at different pH values
#4 left question) answers on WS
#4 right question) a) base b) acid c) >7
#5) 0.0600 M NaOH
#6) 0.115 M KOH
#7) 71.6 ml
#8) Regarding Q5 and Q6, neutral. Regarding Q7, acidic
#9) Regarding Q5 and Q6, Litmus or Bromthymol Blue. Regarding Q7, Methyl Red or Methyl Orange
#10) 140 g/mol
#11) 7650 g/mol or 7670 g/mol (it depends on how you do the calculation)
Page 585
#31a) 0.0372 M NaCl
#31b) 0.186 M NaOH
#32HCl) 56 ml 12.1 M HCl
#32HNO3) 42 ml 15.9 M HNO3
#33) Measure 6.21ml of 3.02 M NaOH, add it to a 125ml volumetric, add water up to 125ml, mix and ENJOY!

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Heat and Rates
WS #1 & page 354
worksheet #1
#7) 3.0 kcal
#8) .32 kcal
#9) .60 kcal
#10) 4.32 kcal
#11) -4.32 kcal
#12) 29.1 kcal
#13) all are endo. except #11 is exo.
Page 354
#4) 1.9x10(4)cal also known as 7.8x10(4)J
#5) Silver > Iron > Aluminum
#6) c = 0.39 so Copper

WS#2
#2) 4.6 kcal
#3) -4.80 kcal
#4) 23.5 kcal

WS#3
#1 H2O) H2(g) + .5O2(g) --> H2O + 285.8kJ
#1 NO) 90.3kJ + .5N2(g) + .5O2(g) --> NO(g)
#1MnSO4) Mn(s) + S(s) + 2O2(g) --> MnSO4(s) + 1065.2kJ
#2 C3H8) C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O + 2219.2kJ
#5) -1680kJ, -547kJ, 39.5g H2O

WS#5
#1) 2NO + Cl2 --> 2NOCl
#4) N2 + 2O2 --> 2NO2
#5) -132.7kJ
#8) -1458.8kJ
#9) -149.6kJ
#10) -198.0kJ
#11) +178.5kJ

WS dG and Friends
#10a) 115kJ/mol and NO
#10b) -623kJ/mol and YES
#10c) -135kJ/mol and YES
#11) -394.40kJ/mol and YES

WS Ea
#5) dH reverse = +150kJ, Ea' = +250kJ and exothermic
#6) dH reverse = -136kJ, Ea' = +18kJ and endothermic
#7) dH forward = +39kJ, dH reverse = -39kJ and endothermic

WS#7 & page 638, 665
worksheet #7
#1) steps of a reaction
#2) Reactions require 2 things. Enough energy (Ea) and proper orientation
#4) Look at your notes. *Please notice it is all about collisions.
#5) Slowest step
#6) H2 + Cl2 --> 2HCl
#7) step #1
#8) NO2 + O --> NO + O2
#9) O3 + O --> 2O2
#11) 1.05x10(-5) M/hr
#12) 9.67x10(-5) M/min
page 638
#2) a catalyst provides a new path (mechanism) that has a lower Activation Energy
#3) at lower temperatures particles move slower, so they have less collisions AND collisions have less energy
page 665
#56) No, orientation also matters
#57) particles move faster so more collisions and the collisions have more energy
#75a) new path with a lower Ea
#75b) 2, because lower Ea
#75c) reaction can go both directions (we'll discuss this more next unit)

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Chapter 17 (equilibrium)
Page 638, 662
page 638
#6) rates of opposing reaction
#7) No, a particle may react (but the opposite reaction is also happening, AT THE SAME RATE!)
page 662
#14) because (even though more product is being made) product is turning into reactant
#21) Keq = 6.80
#22) Keq = 4.85x10(-6)
#38) lots of product and not much reactant, YES
#39) No (low amount of product), No (not useful to produce product), this is our next lesson
#41) [O3] = 1.8x10(-8) M
#42) Keq = 2.1x10(-3)
#72) 2nd picture it has reached equilibrium, 2 molecules of A2B reacted

WS#2
#1) Reactions shift to counteract a "stress" placed upon the equilibrium. This means they try to get back to equilibrium.
#2) R, R, L
#3) R, L, L, L, R, R, L, R
#5) more, less, more, more, same
#6a) in lungs Hb(O2)4, in cells HbH4(4+)
#6b) favored is Hb(O2)4, paper bag helps because increase CO2 causes increase H+ so Hb(O2)4 goes down
#6c) this decreases H+ so an increase of Hb(O2)4

WS#3
#1) right
#2) right
#3) left
#4) left, right, left
#6) no change, no change
#7) Keq = [C]3[D]2[E] / [A] [B]2 and 310 (*hey, look at significant figures)
#8) increase N2O4, decrease NO2, increase T, decrease P
#9) increase N2, increase O2, decrease NO, decrease T
#11) mostly reactant @ equilibrium
#12) mostly product @ equilibrium
#13) about equal reactant and product @ equilbrium
#14a) down, up, up, up
#14b) up, up, up, down
#14c) down, up, down, down
#14d) down, down, up, down
#14e) up, up, down, down

WS#1
*see the ws

WS#4
*see the ws

WS#5
*see the ws

WS#7
#2) a)left b)right c)left d)right e)left f)left
#3) increase SO2, increase O2, decrease SO3, decrease Temp., increase Pressure
#4) It would not shift.
#5) increase pressure and remove NH3 as a liquid
#7) 8.4 M HI
#8) 0.443
#9) B
#10) the one with 5.0x10(-1)
#11) 2.6x10(-8)
#12) 3.3
#13) 0.100 M KOH
#14) B

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O-Chem (with a little polymer and also a little redox)
WS #1 & #2

WS#3 & 4

WS#5

Page 673, 700
page 673
18.1a) Cu is ox. and O2 is red.
18.1b) Cs is ox. and F2 is red.
page 700
#1) oxidation is the loss of e-
#2) reduction is the gain of e-
#20) Br- is ox. and Ag+ is red.
#24a) Cu(s) --> Cu+2(aq) + 2e-
#24b) e- + Fe+3(aq) --> Fe+2(aq)