1. AP Chemistry Summer Assignment
Measurements & Nomenclature

2. III. Significant Figures
h = 0.05 cm
l = 17.9 cm
w = 6.87 cm
III. Significant Figures
1. Calculate the area of the dark rectangle.
123
123 cm2
2. Calculate the volume of the object 6
6 cm3

3. III. Significant Figures
3. Calculate the sum of the length, width, and height.
24.82
24.8
24.8 cm
4. What is the length of each segment?
11 cm
10 cm A B C D
A = cm
B = cm
C = cm
D = cm

4. C. What is a significant figure?
B. Introduction:
When making measurements or doing calculation you should not keep more digits in a number than is ________. These rules of significant figures will show you how to determine the correct number of digits.
 C. What is a significant figure?
Significant figures in a measurement are all values (digits) known precisely, plus ______ digit that is estimated.
Example: Make the measurement with the correct significant figures.
justified
one
a. ____________
b. ____________
c. _____________
d. _____________
e. _____________
f. _____________
g. ____________
h. ____________ a. b. c. d. e. f. g. h.
9 cm
10 cm
0 cm
1 cm
9.24 cm
9.00 cm
9.0 cm
0.02 cm
9.88 cm
9.70 cm
9.8 cm
0.90 cm

5. How do you determine sig figs in a measurement that has already been recorded?
Sig Figs: The Rules
1. Every nonzero digit in a recorded measurement is significant.
Examples: 47,357 5 sig figs ________ 2
Zeros between nonzero digits are significant.
(“Sandwich rule”)
Examples: 1, sig figs
305 _______ 3
3. Zeros in front of all nonzero digit are not significant.
Examples: sig figs
______
______ 2 1

6. Zeros at the end of a number and to the right of a decimal point are significant.
Examples: sig figs ______ ________ 4 4
5. Zeroes at the end of a measurement where there is no decimal point are ambiguous. To clearly show the correct number of sig figs, these measurements should be written in scientific notation.
Examples: sig figs
sig fig
1,000,000 _______
1 - 7
Examples: Write the number 100,000 with (a) 1 sig fig,
(b) 3 sig figs, (c) 5 sig figs.
(a) 1 x 105
(b) 1.00 x 105
(c) x 105

7. E. Practice: 1. Determine the number of significant figures for each of the following measurement.
(a) (b) (c) (d) 10.54
(e) x (f) 15,000 (g) (h)
2. When completing calculations, it is often necessary to round the final answer to a particular number of significant figures (round up for 5 and above; keep digits the same for 4 and below). Round the above measurements to 2 significant figures. Example: = = _______________ 6 4 6 4
54000
0.0046
150,000 11
5.4 x 104
4.6 x 10–3
1.5 x 105 3
2-5 4 3
5.2 x 105
1.5 x 104 10
0.075
1.0 x 101
7.5 x 10–2
110
= 1.1 x 102

8. How many significant figures are in each of the following measurements?
24 mL
2 significant figures
3001 g
4 significant figures m3
3 significant figures
6.4 x 104 molecules
2 significant figures
560 kg
2-3 significant figures

9. 3. Determine the number of sig figs for each measurement
3. Determine the number of sig figs for each measurement. Round the measurements to 2 sig figs. If original measurement only contains 1 or 2 sig figs, leave the second line blank.
# sig figs Rounded Answer
_______ ______________
_______ ______________
3. 1,000,000 _______ ______________
x 102 _______ ______________
_______ ______________
_______ ______________
_______ ______________
x 10-6 _______ ______________
_______ ______________
_______ ______________ 2 4
1.3 x 102
1-7
1.0 x 106 4
5.7 x 102 5
410
= 4.1 x 102
3-5
80,000
= 8.0 x 104 6
3100
= 3.1 x 103 3
4.1 x 10-6 3
1.0 4
1.6

10. 3. Continued
_______ ______________
_______ ______________
_______ ______________
_______ ______________
_______ ______________
_______ ______________
_______ ______________
_______ ______________
_______ ______________
_______ ______________
# sig figs Rounded Answer 4 14 4
5.4
3-4
1300
= 1.3 x 103 3
5.7 x 10-3 4
0.81 5 18 4
100
= 1.0 x 102 4
3000
= 3.0 x 103 7
1.1 x 105 4 43

11. 4. Rules for Significant Figure in Calculations Multiplication or Division: The number of sig figs in the result is the same number as the number in the least precise (least sig figs) measurement.
Example: (1) m x 1.4 m = 6.38 m2 (Round to TWO sig figs) = 6.4 m2
(a) x (b) x 3.5 (c)
8.9648
413.84
9.0
4.1 x 102
1.91
Addition or Subtraction: The result has the same number of decimal places as the least precise measurement used in the calculation.
Example: m m m = (Rounds to ONE place after the decimal) = 21.1 m
(1) 21 cm – 18.3 cm =
(2) mm mm =
3 cm mm

12. Significant Figures Multiplication or Division
The number of significant figures in the result is set by the original number that has the smallest number of significant figures
4.51 x =
= 16.5
3 sig figs
round to
3 sig figs
6.8 ÷ =
= 0.061
2 sig figs
round to
2 sig figs

13. Significant Figures Addition or Subtraction
The answer cannot have more digits to the right of the decimal
point than any of the original numbers.
89.332
1.1 +
90.432
one significant figure after decimal point
round off to 90.4
3.70
0.7867
two significant figures after decimal point
round off to 0.79

14. IV. Exponential Notation (_________ Notation)
Scientific
A. Chemistry examples:
1. Avogadro’s Number
2. Mass of an electron
6.022 x 1023 kg
9.11 x kg
B. Technique to change from positional notation to scientific notation:
1. Leave ___ number to the ______ of the decimal.
2. When the decimal is moved to the ______, the exponent is ____________.
3. When the decimal is moved to the ______, the exponent is ____________.
4. Number must contain the same number of ____________ as the original value. 1
left
left
(+) positive
right
(-) negative
Sig figs (S.F.)

15. C. Convert the following to scientific notation:
(3 s.f) ____________
____________
,000,000,000 (2 s.f.) ____________
____________
1.35 x 105
5.500 x 10-3
1.2 x 1011
4.441 x 10-8
D. Use of calculator with scientific notation:
1.61 x 10-19
Step 1: Enter the number
Step 2: Press the Expontent button ____ or ____
Step 3: Enter the exponent
Step 4: If negative exponent, use ____ key.
1.61 EE
EXP
+/-

16. E. Exponent problems (Use correct sig figs!)
Raising to a power Taking a root
Step 1: Enter number Step 1: Enter number
Step 2: Press Step 2: Press
Step 3: Enter power Step 3: Enter root
Step 4: Press Step 4: Press
Example: Example: xy
2nd xy = =
9.29 x 106
(a) (14.5)6 =
2.26
(b) (1.72 x 105)4 =
8.75 x 1020
0.0528

17. Scientific Notation The number of atoms in 12 g of carbon:
602,200,000,000,000,000,000,000
6.022 x 1023
The mass of a single carbon atom in grams:
1.99 x 10-23
N x 10n
N is a number
between 1 and 10
n is a positive or
negative integer

18. Scientific Notation Addition or Subtraction 568.762 0.00000772
move decimal left
move decimal right
n > 0
n < 0
= x 102
= 7.72 x 10-6
Addition or Subtraction
Write each quantity with the same exponent n
Combine N1 and N2
The exponent, n, remains the same
4.31 x x 103 =
4.31 x x 104 =
4.70 x 104

19. Scientific Notation Multiplication Division
(4.0 x 10-5) x (7.0 x 103) =
(4.0 x 7.0) x (10-5+3) =
28 x 10-2 =
2.8 x 10-1
Multiply N1 and N2
Add exponents n1 and n2
Division
8.5 x 104 ÷ 5.0 x 109 =
(8.5 ÷ 5.0) x =
1.7 x 10-5
Divide N1 and N2
Subtract exponents n1 and n2

20. Practice
1. If the mass, radius, and height of a cylinder are given, what would be the equation to find the Density?
2. Write the correct number of sig figs for each of the following numbers.
____ 5
35000____
2-5
3.167 x 109____ 4
100____
1-3
____ 6
____ 1
3. Calculate each problem with the correct sig figs and units.
( ) x 102 g =
12,852  1.29 x 104 g
__________
__________
9.8 x 103
(0.32)(25)(1223.4) =
__________
172.1 m
406.1 m – m =
0.029 or 2.9 x 10-2
__________
(0.0035) / (0.12) =
4. Calculate the following problem with the correct sig figs and units.
____________________
5.29 x 10-5 or 5.3 x 10-5

21. V. Metric System A. Based on powers of 10
Ex. 1 m = ______ dm = ______ cm = ______ mm
B. Uses “___________” and “____________.” 10
100
1000
prefixes
Base units
1. Length
meter (m)
gram (g)
2. Mass
liter (L)
3. Volume
second (s)
4. Time
Joule (J)
5. Energy

22. C. Metric Prefixes: Memorize this table. Prefix. Symbol
C. Metric Prefixes: Memorize this table!!!! Prefix Symbol Multiplier/Factor
1. Peta P
2. Tera T
3. Giga G
4. Mega M
5. kilo k
6. hecto h
7. deka da
Base Unit m, g, L, s, J
8. deci d
9. centi c
10. milli m
11. micro µ
12. nano n
13. pico p

24. D. Examples: Multiplier ALWAYS goes with the _____________________.
Base Unit (m, L, g, s, J)
1 Mm = _____ m 1 µg = _____ g
1 Ts = _____ s 1 pm = _____ m
106
10-6
1012
10-12
E. Converting within the metric system using dimensional analysis:
Convert to base unit by canceling units (Top unit cancels with _______ unit).
Place the multiplier with the _____________________.
Place a ___ in front of the unit with ______.
To enter multiplier into the calculator, use a __ before the exponent key (NOT A 10).
Example: 10-6
bottom
base unit (m, L, g, s, J) 1
prefix 1
1 x 10-6
1 EE - 6
10 x 10-6

25. Volume – SI derived unit for volume is cubic meter (m3)
1 L = 1 dm3
1 mL = 1 cm3

26. Dimensional Analysis Method of Solving Problems
Determine which unit conversion factor(s) are needed
Carry units through calculation
If all units cancel except for the desired unit(s), then the problem was solved correctly.
How many mL are in 1.63 L?
1 mL = 10-3 L 1 mL
1.63 L x
= 1.63 x 103 mL
10-3 L
10 –3 L
1 mL
1.63 L x
= 1.63 x 10-3 L2 mL

27. F. Metric dimensional analysis examples:
1. Convert 3.6 nm to m.
2. Convert 55.6 g to Tg
3. Convert 575 cm to Mm.
4. Convert dag to pg.
5. Convert 78.5 km to m
6. Convert mL to GL.
3.6 x 100 nm
10-9 m
= 3.6 x 10-9 m 1 nm
5.56 x 101 g 1 Tg
= x Tg
1012 g
5.75 x 102 cm
10-2 m 1 Mm
= x 10-6 Mm 1 cm
106 m
4.56 x 10-1 dag
101 g 1 pg
= x 1012 pg 1
dag
10-12 g
7.85 x 101 km
103 m 1 m
= x 1010 m 1 km
10-6 m
5.90 x 10-4 mL
10-3 L 1 GL
= x GL 1 mL
109 L

28. Practice
6.5 x 10-5
1 x 107
4.4 x 104

29. Metric / English Conversion Factors (given on test):
Length Mass
1 inch = 2.54 cm 1 lb. = 16 oz. = 256 drams
1 meter = in 1 kg = lb.
1 mile = km 1 lb = g
1 furlong = 220 yd.
Volume Time
1 L = qt fortnight = 2 weeks
1 gal. = 4 qt. = 8 pt.
1 pt. = 2 cups
1 mL = 1 cm3
1 pt. = 16 fl. oz.

30. VI. Conversion Factors:
A. Whenever two measurements are equal, or ___________, a ratio of these two measurements will equal __.
  Example: ___ ft. = ___ in. can be written as the following ratios:
B. Conversion factor: ratio of ___________ measurements.
C. Write conversion factors for the following pairs of units:
a. miles and feet
b. days and year
c. yard and feet
D. Assume all conversion factors are _________ significant. (Use initial number to determine sig figs).
equivalent 1 1 12
equivalent
infinitely

31. The speed of sound in air is about 343 m/s
The speed of sound in air is about 343 m/s. What is this speed in miles per hour?
meters to miles
seconds to hours
1 mi = 1609 m
1 min = 60 s
1 hour = 60 min
343 m s x
1 mi
1609 m
60 s
1 min x
60 min
1 hour x
= 767 mi
hour

32. VII. Dimensional Analysis I
Units (___________) are used to solve a problem. 
Examples:
A. The average human brain weighs 8.13 lb. What is the mass in ng?
B. How many microseconds in 8.37 years? Write answer in scientific notation.
Dimensions lb g ng
8.13 lb.
453.6 g 1 ng
= x 1012 ng 1
lb. g
10-9 y d h
min s s
8.37 y
365 d 24 h 60
min 60 s 1 s 1 y 1 d 1 h 1
min
10-6 s
= x 1014 s

33. C. A container contains 15 kL. Convert this to cm3.
D. Apollo 13 re-entered the Earth’s atmosphere at a speed of 32,805 ft/s. What was the speed in miles per hour (mph)? kL L mL
cm3
15 kL
103 L 1 mL 1
cm3
= 1.5 x 107 cm3 1 kL
10-3 L 1 mL
ft. s mi
min h
32,805 ft s 60 s 60
min 1 mi
= 22,367 mi/h 1
min 1 h
5,280 ft

34. E. An arrow moves towards you at 235 m/s
E. An arrow moves towards you at 235 m/s. How many miles could the arrow move in one day?(Assume the arrow never falls to the Earth).
F. (a) Determine the number of cm3 in a 20.0 fl. oz. bottle of Coke. (b) What is the mass of the Coke in pounds, assuming that it is the density of water (1 g / mL)? m s in ft mi
min h d
235 m s 60 s 60
min 24 h
39.37 in 1 ft 1 mi 1
min 1 h 1 d 1 m 12 in
5,280 ft
= x 104 mi/d
fl. oz. pt qt L mL
cm3
cm3 g lb
(a)
20 fl. oz. 1 pt 4 qt 1 L 1 mL 1
cm3 x x x x x 16
fl.oz. 8 pt
1.057 qt
10-3 L 1 mL
= 591 cm3
(b)
591 cm3 1 g 1 lb x x
= lb 1
cm3
453.6 g

35. G. The speed of light is 3. 00 x 108 m/s
G. The speed of light is 3.00 x 108 m/s. How many miles does light travel per year?
H. Carl Lewis set the world record for the m dash on August 25, 1991 in the finals of the World Track Championships with a time of 9.86 seconds. What was his average speed in miles per hour? m s km mi
min h d y s
3.00 x 108 m 60 s 60
min 24 h
365 d 1 km 1 mi 1
min 1 h 1 d 1 y
103 m
1.609 km
= x 1012 mi/y m s km mi
min h
100.0 m
9.86 s 60 s 60
min 1 km 1 mi 1
min 1 h
103 m
1.609 km
= mi/h

36. VIII. Dimensional Analysis II: Square and cubic units
A. Convert 3.7 ft2 to in2.
B. The engine in a Jeep Cherokee is 4.0 L. Calculate the engine volume in (a) in3, and (b) ft3. ft in
3.7 ft2 12 in 12 in x x
= in2
= 5.3 x 102 in2 1 ft 1 ft 2
3.7 ft2 12 in x
= in2
= 5.3 x 102 in2 1 ft L mL
cm3 in in ft 3
(a)
4.0 L 1 mL 1
cm3 1 in x x x
= in3
10-3 L 1 mL
2.54 cm
= 2.4 x 102 in3 3
(b)
in3 1 ft x
= ft3 12 in

37. C. The density of gold is 19. 3 g/mL
C. The density of gold is 19.3 g/mL. Calculate the density of gold in (a) lb/ft3, (b) kg/m3. g mL lb
(a)
cm3 in ft 3 3
19.3 g mL 1 lb 1 mL
2.54 cm 12 in x x x x
453.6 g 1
cm3 1 in 1 ft
= lb/ft3
= x 103 lb/ft3 g
cm3 kg
(b) m 3
19.3 g
cm3 1 kg 1 cm x x
103 g
10-2 m
= 19,300 kg/m3
= x 104 kg/m3

38. D. A spherical container with a diameter of 2
D. A spherical container with a diameter of 2.85 dam is filled with water. (a) Determine the volume of the sphere in cm3. (b) Determine the mass of the water in kilograms.
d = dam
d = dam
101 m 1 cm
= x 103 cm 1
dam
10-2 m
r = x 103 cm
(a)
= x 1010 cm3
(b)
1.21 x 1010 cm3 1 g 1 kg x x 1
cm3
103 g
= x 107 kg

39. E. The dimensions of a swimming pool are 13. 5 ft. x 22 m x 225 cm
E. The dimensions of a swimming pool are 13.5 ft. x 22 m x 225 cm. (a) Determine the volume of the pool in m3. (b) Determine the mass of the water in pounds.
(a)
V = l · w · d
13.5 ft 12 in 1 m
= m x x 1 ft
39.37 in
V = m · 22 m · 2.25 m
= m3
= 2.0 x 102 m3 3 1 g 1 lb
(b)
x 102 m3 1 cm x x x
10-2 m 1
cm3
453.6 g
= 4.5 x 105 lb

40. F. A 12.0 fl. oz. soda spilled onto the floor into a cylindrical puddle with a 15.4 inch diameter. Calculate the depth (height) of the puddle in μm.
d = 15.4 in
d = 15.4 in
2.54 cm
= cm x
h = ? 1 in
r = cm
(a)
fl.oz. pt qt L mL
cm3
12 fl.oz. 1 pt 1 qt 1 L 1 mL 1
cm3 x x x x x 16
fl.oz. 2 pt
1.057 qt
10-3 L 1 mL
= cm3
(b)
= cm
(c)
0.295 cm
10-2 m 1 µm
= x 103 µm x x 1 cm
10-6 m

41. G. The volume of a red blood cell is 90. 0 µm3
G. The volume of a red blood cell is 90.0 µm3. What is its diameter in mm? Assume it is spherical.
V = 90.0 µm3
= µm
2.780 µm
10-6 m 1 mm 2
= x 10-3 mm x x x 1 µm
10-3 m

42. H. The lid of a soup can is 5. 40 cm across and the can is 12
H. The lid of a soup can is 5.40 cm across and the can is 12.2 cm high. What is the volume of the can in fluid ounces?
d = 5.40 cm
h = 12.2 cm
r = cm
V = (2.70 cm)2 • 12.2 cm
= cm3
cm3 mL L qt pt
fl.oz.
cm3 1 mL
10-3 L
1.057 qt 2 pt 16
fl.oz. x x x x x 1
cm3 1 mL 1 L 1 qt 1 pt
= fl.oz.

43. Inorganic Nomenclature

44. Fig. 2.11 H+
Be2+

45. 1. Column: _______ or _______ (Similar properties) 2. Row: _______.
I. Background:
A. Periodic Table
1. Column: _______ or _______ (Similar properties)
2. Row: _______.
3. _______: Left of staircase (Majority of the elements).
4. ___________: right of staircase.
Exception: _____(non-metal)(____________________)
5. ____________: touching the staircase.
Exception: ___ (metal).
group
family
period
Metals
Non-metals H
Left of the staircase
Metalloids
Gagag Al

46. Period
Group
2.4

47. Ions (Charged atoms)
1. ________: positively charged (lost e-).
2. ________: negatively charged(gained e-).
C. Trends in the periodic table
1. Using the planetary model – (simplified model of atom)
2. Energy levels can contain a maximum of:
1st energy level: ____
2nd energy level: ____
3rd energy level: ____ (____)
3. _________ are the keys to chemical bonds.
Cations
Anions 2 8 8 18
Electrons

48. Ex.
Column 1 (____________) Column 18 (___________)
Alkali Metals
Noble gases
H (___ e-) 1
He (___ e-) 2
Ne (___e-) 10
Li (___e-) 3
Na (___e-) 11
Ar (___e-) 18
Similarities: (________________) ______________
1 e- in outer shell
Full outer shell

49. Non-metals only (above staircase)
Atoms can gain or lose ___ to achieve a full outer shell (more stable).
Atoms will do what is _______ (least energy) i.e Oxygen has 6 valence e-: easier to _____ 2 than to ____ 6. e-
easiest
gain
lose
Group
# of valence e-
Gain or lose e-
Charge 1 2 13 14 15 16 17 18 x
Lose 1 +1 x
Lose 2 +2 x
Lose 3 +3 x
Lose or gain 4
+/-4
Non-metals only (above staircase) x
Gain 3 -3 x
Gain 2 -2 x
Gain 1 -1 x

50. Non-metal Metal loses e- gains e- Transfer neutral
II. Binary Ionic Compounds
A. Background info
1. Metal / ___________ ( _______ is always written first).
2. One element ________ and the other ________.
3. ___________ of e-
4. Charged ions attract one another (opposites attract).
5. The compound is _________
Non-metal
Metal
loses e-
gains e-
Transfer
neutral

51. B. Ex.
Sodium & chlorine
NaCl (1 Na to every Cl)
(Metal 1st)
Na Cl
Na+ Cl
Ex.
Calcium & bromine
CaBr2 (2 Br for every 1 Calcium) Br
(Metal 1st) Ca
Ca2+ Br Br
Ex.
Lithium & oxygen
Li2O (2 Li for every 1 Oxygen)
(Metal 1st) Li
Li O2 O Li
Ex.
Aluminum & sulfur
Al2S3 (3 Al for every 2 S) Al S
Al3+ S2 S Al S

52. C. Shortcut to determining formula (Criss-Cross method):
1. ________ from charge becomes the subscript.
2. All ionic compounds are _________ (no + or -).
3. Subscripts are written in ________ possible ratio.
The number “1” is never written (It is implied).
Examples
Number
neutral
lowest
Ex. Al O2-
Ex. Li+ O2-
Al2O3
Li2O
(Aluminum oxide)
(Lithium oxide)
Ex. Ca2+ O2-
Ex. Mg2+ N3-
Mg3N2
Ca2O2
CaO
(Calcium oxide)
(Magnesium nitride)

53. D. Nomenclature of binary ionic compounds (bi = 2).
1. _____ is named first (name of atom).
2. ____________ is named second, ending changed to ____.
If the metal (cation) can have multiple charges, the charge is written as a roman numeral (IUPAC).
(Fe, Cu, Co, Hg, Mn, Sn, Pb)
Metal
Non-metal
-ide
4. Formula to name:
a. Li2O _________________
b. Al2O3 _________________
c. CaO _________________
d. Mg3N2 _________________
Lithium oxide
Aluminum oxide
Calcium oxide
Magnesium nitride

54. Iron ___ oxide
(III)
Ferric oxide
e. Fe2O3 __________________ (___________________)
f. SnO2 __________________ (___________________)
g. CuCl ___________________ (___________________)
h. MnN ____________________ (___________________)
2(x) + 3(-2) = 0
x = +3
Tin ___ oxide
(IV)
Stannic oxide
1(x) + 2(-2) = 0
x = +4
Copper __ chloride
(I)
Cuprous chloride
1(x) + 1(-1) = 0
x = +1
Manganese ___ nitride
(III)
Manganic nitride
1(x) + 1(-3) = 0
x = +3

55. Be2+ F – BeF2 K+ Br – KBr Sn2+ O2- SnO Co2S3 Co3+ S2- SrI2 Sr2+ I –
Name to formula:
a. Beryllium fluoride ____________ ___________
b. Potassium bromide ____________ ___________
c. Tin (II) oxide ____________ ___________
d. Cobaltic sulfide ____________ ___________
e. Strontium iodide ____________ ___________
Be2+ F –
BeF2
K+ Br –
KBr
Sn2+ O2-
SnO
Co2S3
Co3+ S2-
SrI2
Sr2+ I –

56. 6. Polyatomic Ion: A group of atoms with a _______ charge.
Ex. (1) CN- =
(2) NH4+ =
(3) OH- =
a. Polyatomic ions will _______ stay together as a group.
b. If there is more than one polyatomic ion, it must be placed in ____________.
single
cyanide
ammonium
hydroxide
always
parentheses

57. Cobalt (III) hydroxide Co(OH)3 Co3+ OH- Cobaltic hydroxide
Examples:
Ions
Formula
Name
Iron (II) hydroxide
Fe2+ OH-
Fe(OH)2
Ferrous hydroxide
Ca2+ CN-
Ca(CN)2
Calcium cyanide
NH4+ O2-
(NH4)2O
Ammonium oxide
NaCN
(No Parentheses b/c only 1)
Sodium cyanide
Na+ CN-
Cobalt (III) hydroxide
Co(OH)3
Co3+ OH-
Cobaltic hydroxide

58. III. Helpful Hints to Memorize Oxyanions
In learning the formulas and charges of common oxyanions, start with the –ate form. From it follows that:
hypo______ite = 2 less oxygens
_______ite = 1 less oxygen
_______ate
per______ate = 1 more oxygen
**ALL forms have the SAME charge!**

59. A Guide to Determine Whether the –ate Formula is –XO3 or –XO4:1 2 3 4 5 6 13 14 15 16 17 18
Transition Metals B C N Si P S Cl As Se Br I

60. A Guide to Determine What the Charge of the Oxy-Anion is:1 2 3 4 5 6 13 14 15 16 17 18
Transition Metals -3 -2 -1 B C N
- 4 -3 -2 -1 Si P S Cl -3 -2 -1 As Se Br -1 I

61. ClO4-
Examples:
Borate = ________ Carbonate = ________
Nitrate = ________ Chlorate = ________
Nitrite = ________ Perchlorate = ________
BO33-
CO32-
NO3-
ClO3-
NO2-

62. C. “_____” = Sulfur replacing an oxygen.
Ex. Sulfate = ________ Thiosulfate = ________
Ex. Cyanate = ________ Thiocyanate= ________
Thio-
SO42-
S2O32-
OCN-
SCN-

63. IV. Ternary Compounds: (compounds containing ___ or more elements).
1. Name the _______
2. Find the appropriate name of the _______.
3. Formula to name: 3
cation
anion
a. Li2SO4 _______________
b. Fe(NO3)3 _________________________
Lithium sulfate
Iron ___ (_____) nitrate
(III)
ferric
1(x) + 3(-1) = 0
x = +3

64. c. CdC2O4 __________________
d. Cu3AsO3 ___________________________
e. Mn2SiO4 ________________________________
f. (NH4)2SO4 __________________
Cadmium oxalate
Copper __ (_______) arsenite
(I)
cuprous
3(x) + 1(-3) = 0
x = +1
Manganese __ (___________) silicate
(II)
manganous
2(x) + 1(-4) = 0
x = +2
Ammonium sulfate

65. Name to formula:
a. Potassium thiocyanate: __________ _________
b. Aluminum permanganate: __________ _________
c. Plumbic acetate: ____________ ___________
d. Cobalt (III) oxalate: ____________ ___________
e. Sodium hypochlorite: __________ __________
K+ SCN-
KSCN
Al3+ MnO4-
Al(MnO4)3
Pb+4 C2H3O2-
Pb(C2H3O2)4
Co3+ C2O42-
Co2(C2O4)3
Na+ ClO-
NaClO

66. V. Nomenclature of Hydrates
A. Hydrate: Ionic compound with ______ molecules stuck in the _______ lattice. The water is included in the ______ and formula.
1. ZnSO4 7 H20: __________________________
2. CaCO3 3 H2O: __________________________
3. Cu2C2O4 2H2O: _________________________________
4. Calcium chloride pentahydrate: _____________
5. Cupric acetate monohydrate: _______________________
water
crystal
name
Zinc sulfate
heptahydrate
Calcium carbonate
trihydrate
Copper (I) (cuprous) oxalate
dihydrate
CaCl2
5H20
Cu(C2H3O2)2
H20

67. VI. Binary Molecular Compounds
A. Molecular (________) compounds
1. Non-metal to __________. ______of staircase including hydrogen
2. ________ of electrons.
Ex.
3. Non-metals can often combine in several different ways.
covalent
non-metal
Right
Sharing
Cl Cl
(Both Cl need “1” electron) CO
CO2

68. Nomenclature of binary molecular compounds:
Greek prefixes are used:
mono = hexa =
di = hepta =
tri = octa =
tetra = nona =
penta = deca = 1 6 2 7 3 8 4 9 5 10
2. The prefix “_______” is omitted for the 1st element.
Ex.
CO = _________________
mono
Carbon monoxide

69. For oxides the ending “______” is omitted.
a. N2O = ____________________
b. N2O3 = ____________________
c. N2O4 = ____________________
d. NO = ____________________
e. NO2 = ____________________
f. NO5 = ____________________
o or a
Dinitrogen monoxide
Dinitrogen trioxide
Dinitrogen tetroxide
Nitrogen monoxide
Nitrogen dioxide
Nitrogen pentoxide

70. Compound
Ionic Covalent
(Charges Cancel Out) (No Charges) 1.
2. 2.
3. 3.
Metal / Non-metal
Non-metal only
No Prefixes!!!
Prefixes
Li20
= Lithium oxide
I2O4
= Diiodine tetroxide
Metal
Non-metal
Ex.
_______________________
_____________________
P2O5
Diphosphorus pentoxide
NCl3
Nitrogen trichloride

71. Nomenclature (Acids)
A. Acids: Compounds that contain __________ as the positive ion (H+).
B. Exceptions: _____ (water) & ______ (hydrogen peroxide).
C. Binary Acids: Acids that ___ ____ contain oxygen.
1. Use prefix “______”
2. Add stem or full name of ______.
3. Add suffix “___”.
Add the word ______.
Ex. HBr = _________________________
HCl = _________________________
HCN = ________________________
hydrogen
H20
H2O2 do
not
hydro
anion ic
acid
Hydrobromic Acid
Hydrochloric Acid
Hydrocyanic Acid

72. Ternary Acids: Contain ____ or more elements, __________ oxygen.
Acids formed with anions that contain ______ become ____ acids.
HNO3 (NO3- = _______) __________
HClO4(ClO4- = ___________) _____________
H2SO4(SO42- = ________) ___________
H3PO4(PO43- = ___________) _______________ 3
including
-ate
-ic
Nitrate
Nitric acid
Perchlorate
Perchloric acid
Sulfate
Sulfuric acid
Phosphate
Phosphoric acid

73. -ous
Acids formed with anions that contain ____ become ______ acids.
HNO2 (NO2- = ________) ____________
HClO2 (ClO2- =_________) _____________
H2SO3 (SO32- =________) ______________
-ite
Nitrite
Nitrous acid
Chlorite
Chlorous acid
Sulfite
Sulfurous acid
Name to formula:
a. cyanic acid __________________ ________
b. dichromic acid ______________________ _______
c. hypochlorous acid _____________________ _______
d. hydrosulfuric acid _______________ ______ H+
OCN- (Cyanate)
HOCN H+
Cr2O72- (Dichromate)
H2Cr2O7 H+
ClO- (Hypochlorite)
HClO H+
S2- (Sulfide)
H2S

74. • • Compounds Ionic Covalent Binary Ternary Acids Binary Ternary
(Metal / Non-metal)
Binary Ternary
Acids
Contain H+
Binary Ternary
w/ oxygen
Hydrates Hydrates
Non-metal / Non-metal
Uses prefixes, -ide
I2O7 Diiodine heptoxide
2 elements
-ide
Roman numeral
(if needed)
ie. Calcium chloride
CaCl2
3 or more elements
Anion is named
Roman numerals
(if needed)
ie. Calcium carbonate
CaCO3
No oxygen
Hydro__ic acid
ie, Hydrochloric acid
HCl
-ate—ic
acid
H2CO3
Carbonic
-ite---ous
acid
H2SO3
Sulfurous
w/ H2O
Uses prefixes
ie. Calcium chloride
dihydrate
CaCl H2O •
w/ H2O
Uses prefixes
ie. Calcium carbonate
trihydrate
CaCO H2O •

75. 2.7

76. EOCP 2.88 Mg(HCO3)2 Mg2+ HCO3- Cl- Strontium chloride Sr2+ Fe(NO2)3
Iron (III) nitrite
Mn2+
ClO3-
Mn(ClO3)2
Sn4+
Br-
Tin (IV) bromide
Co3(PO4)2
Cobalt (II) phosphate
Mercury (I) iodide
Hg2I2
Cu+
Copper (I) carbonate
CO32-
Li+
N3-
Li3N
Al2S3
Aluminum sulfide