APChemistry

Summer Assignment

Measurements & Nomenclature

III. Significant Figures

1. Calculate the area of the dark rectangle.

w A 122.973123123 cm2

2. Calculate the volume of the object

hw V 66.14865

6 cm3

h = 0.05 cm

l = 17.9 cm

w = 6.87 cm

III. Significant Figures

3. Calculate the sum of the length, width, and height.

hw 24.8224.824.8 cm

4. What is the length of each segment?

A = 10.07 cm

C = 10.50 cm

D = 11.00 cm

B = 10.23 cm

11 cm10 cm

A B C D

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.

a. ____________

b. ____________

c. _____________

d. _____________

e. _____________

f. _____________

g. ____________

h. ____________

a. b. c. d. e. f. g. h.

9 cm 10 cm 9 cm 10 cm 9 cm 10 cm 0 cm 1 cm

justified

one

9.24 cm9.88 cm

9.00 cm

9.70 cm

9.0 cm

9.8 cm

0.02 cm

0.90 cm

D.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 figs25 ________

2. Zeros between nonzero digits are significant. (“Sandwich rule”) Examples: 1,007 4 sig figs

305 _______

2

3

3. Zeros in front of all nonzero digit are not significant.Examples: 0.00238 3 sig figs

0.98 ______ 0.000006 ______

21

4. Zeros at the end of a number and to the right of a decimal point are significant.

Examples: 426.00 5 sig figs2.060 ______0.8080 ________

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: 120 2-3 sig figs3000 1-4 sig fig1,000,000 _______

44

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) 1.0000 x 105

E. Practice: 1. Determine the number of significant figures for each of the following measurement.

(a) 54320.0 (b) 0.004550 (c) 151309 (d) 10.54

(e) 5.20 x 105 (f) 15,000 (g) 10.04 (h) 0.0750

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: 0.0753 = 0.075 107.0 = _______________

540005.4 x 104

60.00464.6 x 10–3

4150,0001.5 x 105

6114

5.2 x 1053

1.5 x 1042-5

101.0 x 101

40.0757.5 x 10–2

3

110 = 1.1 x 102

How many significant figures are in each of the following measurements?

24 mL 2 significant figures

3001 g 4 significant figures

0.0320 m3 3 significant figures

6.4 x 104 molecules 2 significant figures

560 kg 2-3 significant figures

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 Answer1. 0.0037 _______ ______________2. 134.1 _______ ______________3. 1,000,000 _______ ______________4. 5.730 x 102 _______ ______________5. 410.50 _______ ______________6. 79500 _______ ______________7. 3071.04 _______ ______________8. 4.08 x 10-6 _______ ______________9. 0.998 _______ ______________10. 1.570 _______ ______________

2

1-745

3-56334

1.3 x 102

1.0 x 106

5.7 x 102

= 4.1 x 102

= 8.0 x 104

= 3.1 x 103

4.1 x 10-6

1.01.6

-------------

41080,0003100

4

3. Continued

11. 14.04 _______ ______________

12. 5.401 _______ ______________

13. 1340 _______ ______________

14. 0.00566 _______ ______________

15. 0.8120 _______ ______________

16. 18.009 _______ ______________

17. 100.5 _______ ______________

18. 3008 _______ ______________

19. 112040.0 _______ ______________

20. 43.05 _______ ______________

# sig figs Rounded Answer

4

4

3-4

3

4

5

4

4

7

4

= 1.3 x 1031300

14

5.4

5.7 x 10-3

0.8118

= 1.0 x 102

= 3.0 x 103

100

3000

1.1 x 105

43

4. Rules for Significant Figure in CalculationsMultiplication 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) 4.56 m x 1.4 m = 6.38 m2 (Round to TWO sig figs) = 6.4 m2

(a) 17.24 x 0.52 (b) 118.24 x 3.5 (c)

Addition or Subtraction: The result has the same number of decimal places as the least precise measurement used in the calculation.Example: 12.11 m + 8.0 m + 1.013 m = 21.123 (Rounds to ONE place after the decimal) = 21.1 m

(2) 10000.00 mm + 25.116 mm =

10025.12 mm 3 cm

(1) 21 cm – 18.3 cm =

7.58

14.40 x 1.007

8.96489.0

413.841.9130343014.1 x 102

1.91

Significant FiguresMultiplication 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 3.6666 = 16.536366 = 16.5

3 sig figs round to3 sig figs

6.8 ÷ 112.04 = 0.0606926

2 sig figs round to2 sig figs

= 0.061

Significant FiguresAddition or Subtraction

The answer cannot have more digits to the right of the decimalpoint than any of the original numbers.

89.3321.1+

90.432 round off to 90.4

one significant figure after decimal point

3.70-2.91330.7867

two significant figures after decimal point

round off to 0.79

IV. Exponential Notation (_________ Notation)

A. Chemistry examples:

1. Avogadro’s Number

2. Mass of an electron

Scientific

602200000000000000000000 6.022 x 1023

0.000000000000000000000000000000911 kg9.11 x 10-31 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.Sig figs (S.F.)

right

(+) positiveleft

left1

(-) negative

C. Convert the following to scientific notation:

1. 135000 (3 s.f) ____________

2. 0.005500 ____________

3. 120,000,000,000 (2 s.f.) ____________

4. 0.00000004441 ____________4.441 x 10-8

1.2 x 1011

5.500 x 10-3

1.35 x 105

D. Use of calculator with scientific notation:

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 -19

1.61 19

1.61 00EXPEE

1.61

1.61 x 10-19

E. Exponent problems (Use correct sig figs!)

)10 x 280.1(

)10 x 44.4)(10 x (3.5 1.

22-

12-2

)10 x 8)(10 x 99.6(

)10 x 2.4)(10 x (1.76 2.

146

-4-2

= 1.2 x 1033

= 1 x 10-27

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 xy2nd

= =

(a) (14.5)6 =

(b) (1.72 x 105)4 =

9.29 x 106

8.75 x 1020

58.5 (a) 5

10 x 7.77 (b) 4 -6

2.26

0.0528

Scientific NotationThe 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:

0.0000000000000000000000199

1.99 x 10-23

N x 10n

N is a number between 1 and 10

n is a positive or negative integer

Scientific Notation568.762

n > 0

568.762 = 5.68762 x 102

move decimal left

0.00000772

n < 0

0.00000772 = 7.72 x 10-6

move decimal right

Addition or Subtraction

1. Write each quantity with the same exponent n

2. Combine N1 and N2 3. The exponent, n, remains

the same

4.31 x 104 + 3.9 x 103 =

4.31 x 104 + 0.39 x 104 =

4.70 x 104

Scientific NotationMultiplication

1. Multiply N1 and N2

2. Add exponents n1 and n2

(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

Division

1. Divide N1 and N2

2. Subtract exponents n1 and n2

8.5 x 104 ÷ 5.0 x 109 =(8.5 ÷ 5.0) x 104-9 =

1.7 x 10-5

http://micro.magnet.fsu.edu/primer/java/scienceopticsu/powersof10/

Practice1. If the mass, radius, and height of a cylinder are given, what would be the

equation to find the Density?

hrV ;V

mD :1 Step 2

2. Write the correct number of sig figs for each of the following numbers.

4. Calculate the following problem with the correct sig figs and units.

3. Calculate each problem with the correct sig figs and units.

hr

mD :2 Step

2

0.0030500____100____ 1.00006____

35000____.000008____3.167 x 109____

)3800)(862.2(

)365.0() 3164.4( 2

____________________

51-3 6

2-5 41

(24 + 100.35 + 0.0035 + 1.25) x 102 g = __________

(0.32)(25)(1223.4) =

406.1 m – 234.034 m =

(0.0035) / (0.12) =

__________

__________

__________0.029 or 2.9 x 10-2

172.1 m

9.8 x 103

12,852 1.29 x 104 g

5.29 x 10-5 or 5.3 x 10-5

V. Metric SystemA. Based on powers of 10

Ex. 1 m = ______ dm = ______ cm = ______ mm

B. Uses “___________” and “____________.”

liter (L)

4. Time second (s)

3. Volume

gram (g)2. Mass

meter (m)1. Length

Base unitsprefixes100010010

5. Energy Joule (J)

C. Metric Prefixes: Memorize this table!!!! Prefix Symbol Multiplier/Factor

1. Peta P 1015

2. Tera T 1012

6. hecto h 102

Base Unit m, g, L, s, J

3. Giga G 109

4. Mega M 106

5. kilo k 103

7. deka da 101

8. deci d 10-1

9. centi c 10-2

11. micro µ 10-6

10. milli m 10-3

12. nano n 10-9

13. pico p 10-12

D. Examples: Multiplier ALWAYS goes with the _____________________.

1 Mm = _____ m 1 µg = _____ g

1 Ts = _____ s 1 pm = _____ m

106 10-6

1012 10-12

Base Unit (m, L, g, s, J)

E. Converting within the metric system using dimensional analysis:1. Convert to base unit by canceling units (Top unit cancels

with _______ unit).

2. Place the multiplier with the _____________________.

3. Place a ___ in front of the unit with ______.

4. To enter multiplier into the calculator, use a __ before the exponent key (NOT A 10).

Example: 10-6

1

bottom

base unit (m, L, g, s, J)

prefix

1

1 x 10-6

10 x 10-6

1 EE - 6

Volume – SI derived unit for volume is cubic meter (m3)

1 L = 1 dm3

1 mL = 1 cm3

Dimensional Analysis Method of Solving Problems

1. Determine which unit conversion factor(s) are needed

2. Carry units through calculation

3. If all units cancel except for the desired unit(s), then the problem was solved correctly.

1 mL = 10-3 L

How many mL are in 1.63 L?

10-3

11.63 L x = 1.63 x 103 mL

10 –3 L1 mL

1.63 L x = 1.63 x 10-3 L2

mL

mL

L

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 0.456 dag to pg.

5. Convert 78.5 km to m

6. Convert 0.000590 mL to GL.

3.6 x 100 nm1

10-9= 3.6 x 10-9 m

5.56 x 101 g 11012

= 5.56 x 10-11 Tg

5.75 x 102 cm1

10-2= 5.75 x 10-6 Mm106

1

nmm

Tgg

cmm

mMm

4.56 x 10-1 dag1

101= 4.56 x 1012 pg10-12dag

g pg

7.85 x 101 km1

103= 7.85 x 1010 m10-6km

m m

5.90 x 10-4 mL1

10-3= 5.90 x 10-16 GL109mL

L GL

g

m

L

1

1

1

Practice

)10 x 1.6)(10 x 43.7)(10 x 000.2()10 x 356.4)(10 x (9.1

3.6-52-

-24

10 x 1.20010 x 7.8

.12

-3

6.5 x 10-5

1 x 107

4.4 x 104

)10 x 0.5()10 x (4 .2 4 2-3

Metric / English Conversion Factors (given on test):

Length Mass

1 inch = 2.54 cm 1 lb. = 16 oz. = 256 drams

1 meter = 39.37 in 1 kg = 2.205 lb.

1 mile = 1.609 km 1 lb = 453.6 g

1 furlong = 220 yd.

Volume Time

1 L = 1.057 qt. 1 fortnight = 2 weeks

1 gal. = 4 qt. = 8 pt.

1 pt. = 2 cups

1 mL = 1 cm3

1 pt. = 16 fl. oz.

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).

equivalent1

1 12

in. 12

ft. 1ft. 1

in. 12or

equivalent

mi. 1

ft. 5280or

ft. 5280

mi. 1

y 1

d 365.25or

d 365.25

y 1

yd. 1

ft. 3or

ft. 3

yd. 1

infinitely

The speed of sound in air is about 343 m/s. What is this speed in miles per hour?

1 mi = 1609 m 1 min = 60 s 1 hour = 60 min

343ms

x1 mi

1609 m

60 s

1 minx

60 min

1 hourx = 767

mihour

meters to miles

seconds to hours

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 ngg8.13 lb.

1453.6

lb.g

gng1

10-9= 3.69 x 1012 ng

y sd

8.37 y1

365yd

d

h24

1

= 2.64 x 1014 s

h min s

h1

min60

min1

s60

10-6 s

1 s

cm3

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

15 kL1 kL

LL

mL1

mL cm3

mL11

mi

160

mins

min h

h1

min60

ft5,280

mi1

103

10-3 = 1.5 x 107 cm3

ft.s

= 22,367 mi/h32,805 ft

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)?

in

160

mins

dh24

1

min h

h1min60

m1in39.37

121 ft

ms

pt

20 fl. oz.161

fl.oz.pt

ptqt4

8

g lb

qt1.057L1

ft mi

235 ms in ft5,280

mi1

= 1.26 x 104 mi/d

fl. oz. cm3qt L mLcm3

xL

mL1mL1

110-3

cm3

x x x x

= 591 cm3

(a)

(b) 591 cm3

11 g

glb1

453.6x x

cm3 = 1.30 lb

d

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 100.0 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?

min160 s

h1min60

m103

km11

365 dys

3.00 x 108 m

kmmin h

ms

mid

km

min160 s

min h

h1min60

ms

mi

y

dh24

1 1.6091

kmmi

= 5.88 x 1012 mi/y

100.0 m9.86 s m103

km11.609

1kmmi

= 22.7 mi/h

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.

cm3

VIII. Dimensional Analysis II: Square and cubic units

3.7 ft2

112 in

ftin12

1x x

ft = 532.8 in2

inft

= 5.3 x 102 in2

3.7 ft2

112 in

xft

2

= 532.8 in2 = 5.3 x 102 in2

mL

10-3

1 mLmL1

ft

cm2.54in1

L cm3 inin

x x x = 244.09 in34.0 L(a)

(b) 244.09 in3

121 ft

xin = 0.14 ft3

L1 3

= 2.4 x 102 in33

C. The density of gold is 19.3 g/mL. Calculate the density of gold in (a) lb/ft3, (b) kg/m3.

453.6

1

g

lb

cm3

mL

in1

cm2.54x

ft

in12

1x x x

lb

cm3 in ft

gmL

(a)

(b)

19.3 g

mL

1

1

3 3

= 1204.8 lb/ft3 = 1.20 x 103 lb/ft3

kg

m

gcm3

103

1

g

kg

m10-2

cm1x

19.3 g

cm3

3

x

= 19,300 kg/m3 = 1.93 x 104 kg/m3

cmm

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.

3r π3

4V

d = 2.85 dam 101= 2.85 x 103 cm10-2dam m

1

r = 1.425 x 103 cm

33)10 x (1.425 π3

4V

3r π3

4V

= 1.21 x 1010 cm3(a)

(b) 1.21 x 1010 cm3

xxcm3

g

g

kg1 1

1 103

= 1.21 x 107 kg

1

d = 2.85 dam

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)

(b)

min13.5 ft 12 = 4.1148 m39.37ft in1

1

V = l · w · d

V = 4.1148 m · 22 m · 2.25 m

= 203.68 m3

= 2.0 x 102 m3

2.0368 x 102 m3

x

cm10-2 m1

3

cm3

g

g

lb1 1

1 453.6

= 4.5 x 105 lb

x

x

x

x

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.

(a) cm3qt Lfl.oz. pt mL

x

12 fl.oz. ptfl.oz.16

1x

x

x

x pt

qtqt2

11.057

LL

1 1 1110-3

mLmLcm3

= 354.77 cm3

(c)m

x

0.295 cm mcm1

10-2x

µm10-6

1= 2.95 x 103 µm

d = 15.4 in

h = ?d = 15.4 in x

cm1 in

2.54 = 39.116 cm

r = 19.558 cmhr πV 2

hr πV 2(b)

2r π

Vh

2

3

cm) (19.558 π

cm 354.77h = 0.295 cm

G. The volume of a red blood cell is 90.0 µm3. What is its diameter in mm? Assume it is spherical.

3r π3

4V

V = 90.0 µm3

3

π4

)0.90(3r = 2.780 µm

2.780 µmm

x

m mm110-6

x µm 10-3

1= 5.56 x 10-3 mmx

2

3

π4

)V(3r

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 = 2.70 cm

hr πV 2 V = (2.70 cm)2 • 12.2 cm

= 279.407 cm3

279.407 cm3

cm3 qtL fl.oz.ptmL

x

= 9.45 fl.oz.

pt fl.oz.11

x

x

x ptqt

qt1 1

1.057LL

21

161

10-3

mLmLcm3

x

Inorganic Nomenclature

Fig. 2.11

Be2

+

H+

I. Background:A. Periodic Table1. 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

HMetalloids

Al

Non-metalsMetals

Left of the staircase

Period

Group

2.4

B. Ions (Charged atoms)

1. ________: positively charged (lost e-).2. ________: negatively charged(gained e-).

C. Trends in the periodic table1. 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.

CationsAnions

Electrons

288 18

Ex.Column 1 (____________) Column 18 (___________)

Similarities: (________________) ______________

Li (___e-) Ne (___e-)

Na (___e-) Ar (___e-)

1 e- in outer shell Full outer shell

H (___ e-) He (___ e-)

Alkali Metals Noble gases

1 2

3 10

11 18

3. Atoms can gain or lose ___ to achieve a full outer shell (more stable).

4. Atoms will do what is _______ (least energy) i.e. Oxygen has 6 valence e-: easier to _____ 2 than to ____ 6.Group # of valence e- Gain or lose e- Charge

1

2

13

14

15

16

17

18

e-

easiestgain lose

+1+2

+3

-3

-2

-1

+/-4

0

Non-metals

only (above

staircase)

x

x

x

x

x

x

x

x

Lose 1

Lose 2

Lose 3

Lose or gain 4

Gain 3

Gain 2

Gain 1

II. Binary Ionic CompoundsA. Background info1. 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-metalgains e-loses e-

neutral

Metal

Transfer

Na Cl

Ca

B. Ex. NaCl (1 Na to every Cl)

O

(Metal 1st)

Sodium & chlorine

Li2O (2 Li for every 1 Oxygen)

Li+ O2

CaBr2 (2 Br for every 1 Calcium)

Calcium & bromine

(Metal 1st)

(Metal 1st)

Na+ Cl

Ca2+ Br

Lithium & oxygen

Ex.

Ex.

Ex. Aluminum & sulfur

Al

Al S

SS Al3+ S2

Al2S3 (3 Al for every 2 S)

Br

Br

Li

Li

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.4. The number “1” is never written (It is implied).5. Examples

Numberneutrallowest

Ex. Li+ O2-

(Aluminum oxide)(Lithium oxide)Li2O

Al2O3

Ex. Al3+ O2-

Ex. Ca2+ O2- Ex. Mg2+ N3-

Ca2O2Mg3N2

(Calcium oxide) (Magnesium nitride)

CaO

D. Nomenclature of binary ionic compounds (bi = 2).1. _____ is named first (name of atom).2. ____________ is named second, ending changed to ____.3. If the metal (cation) can have multiple charges, the

charge is written as a roman numeral (IUPAC). (Fe, Cu, Co, Hg, Mn, Sn, Pb)

MetalNon-metal -ide

4. Formula to name:a. Li2O _________________b. Al2O3 _________________c. CaO _________________d. Mg3N2 _________________

Lithium oxideAluminum oxideCalcium oxideMagnesium nitride

e. Fe2O3 __________________ (___________________)

f. SnO2 __________________ (___________________)

g. CuCl ___________________ (___________________)

h. MnN ____________________ (___________________)

Iron ___ oxide Ferric oxide

Tin ___ oxide Stannic oxide

Copper __ chloride Cuprous chloride

Manganese ___ nitride Manganic nitride

2(x) + 3(-2) = 0

x = +3

1(x) + 2(-2) = 0

x = +4

1(x) + 1(-1) = 0

x = +1

1(x) + 1(-3) = 0

x = +3

(IV)

(I)

(III)

(III)

5. 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

Co3+ S2- Co2S3

Sr2+ I – SrI2

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 ____________.

cyanideammoniumhydroxide

always

parentheses

single

Ions Formula Name

Fe2+ OH- Fe(OH)2

Iron (II) hydroxide

Ca2+ CN- Ca(CN)2 Calcium cyanide

NH4+ O2- (NH4)2O Ammonium oxide

Na+ CN- NaCN(No Parentheses b/c only 1)

Sodium cyanide

Co3+ OH- Co(OH)3

Cobalt (III) hydroxideCobaltic hydroxide

Ferrous hydroxide

Examples:

III. Helpful Hints to Memorize OxyanionsA. 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_______ateper______ate = 1 more oxygen

**ALL forms have the SAME charge!**

A Guide to Determine Whether the –ate Formula is –XO3 or –XO4:

B C N

Cl

Br

I

Si P S

As Se

1

2

3

4

5

6

1 2 13 14 15 16 17 18

Transition Metals

A Guide to Determine What the Charge of the Oxy-Anion is:

B C N

Cl

Br

I

Si P S

As Se

1

2

3

4

5

6

1 2 13 14 15 16 17 18

Transition Metals

-1-2-3

-1

-1

-1

-2-3- 4

-2-3

B. Examples:

Borate = ________ Carbonate = ________

Nitrate = ________ Chlorate = ________

Nitrite = ________ Perchlorate = ________

BO33- CO3

2-

NO3-

NO2- ClO4

-

ClO3-

C. “_____” = Sulfur replacing an oxygen.Ex. Sulfate = ________ Thiosulfate = ________Ex. Cyanate = ________ Thiocyanate= ________

SO42- S2O3

2-

OCN- SCN-

Thio-

IV. Ternary Compounds: (compounds containing ___ or more elements).

1. Name the _______2. Find the appropriate name of the _______.3. Formula to name:

3

cationanion

a. Li2SO4 _______________

b. Fe(NO3)3

_________________________

Iron ___ (_____) nitrate

1(x) + 3(-1) = 0

x = +3

Lithium sulfate

(III) ferric

c. CdC2O4 __________________

d. Cu3AsO3 ___________________________

e. Mn2SiO4 ________________________________

f. (NH4)2SO4 __________________

Cadmium oxalate

Copper __ (_______) arsenite

Manganese __ (___________) silicate

Ammonium sulfate

3(x) + 1(-3) = 0

x = +1

2(x) + 1(-4) = 0

x = +2

(I) cuprous

(II) manganous

4. 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

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: _______________________

watercrystal name

Zinc sulfate

Calcium carbonate

Copper (I) (cuprous) oxalate

heptahydrate

dihydrate

trihydrate

5H20CaCl2

H20Cu(C2H3O2)2

VI. Binary Molecular CompoundsA. Molecular (________) compounds1. Non-metal to __________. ______of staircase including

hydrogen2. ________ of electrons.

Ex.

3. Non-metals can often combine in several different ways.Ex.

covalentnon-metal Right

Sharing

Cl Cl (Both Cl need “1” electron)

CO2CO

B. Nomenclature of binary molecular compounds:1. Greek prefixes are used:

mono = hexa =

di = hepta =

tri = octa =

tetra = nona =

penta = deca =

2. The prefix “_______” is omitted for the 1st element.Ex.

CO = _________________

1

2

3

4

5

6

7

8

9

10

mono

Carbon monoxide

3. For oxides the ending “______” is omitted.a. N2O = ____________________

b. N2O3 = ____________________

c. N2O4 = ____________________

d. NO= ____________________

e. NO2 = ____________________

f. NO5= ____________________

o or aDinitrogen monoxide

Dinitrogen trioxide

Dinitrogen tetroxide

Nitrogen monoxide

Nitrogen dioxide

Nitrogen pentoxide

Compound

Ionic Covalent (Charges Cancel Out) (No Charges)

1. 1.2. 2.3. 3.

Metal / Non-metalNo Prefixes!!!Li20

Non-metal onlyPrefixesI2O4

Ex.

1. _______________________

2. _____________________

Diphosphorus pentoxide

NCl3

P2O5

Nitrogen trichloride

Metal Non-metal

= Lithium oxide = Diiodine tetroxide

VI. 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 “___”.4. Add the word ______.Ex. HBr = _________________________

HCl = _________________________HCN = ________________________

hydrogen

H20 H2O2

do nothydro

anionic

acidHydrobromic AcidHydrochloric AcidHydrocyanic Acid

D.Ternary Acids: Contain ____ or more elements, __________ oxygen.

1. Acids formed with anions that contain ______ become ____ acids.

HNO3 (NO3- = _______) __________

HClO4(ClO4- = ___________) _____________

H2SO4(SO42- = ________) ___________

H3PO4(PO43- = ___________) _______________

Nitrate Nitric acid

Perchlorate Perchloric acid

Sulfate Sulfuric acid

Phosphate Phosphoric acid

3including

-ate-ic

2. Acids formed with anions that contain ____ become ______ acids.HNO2 (NO2

- = ________) ____________

HClO2 (ClO2- =_________) _____________

H2SO3 (SO32- =________) ______________

-ite -ous

Nitrite Nitrous acid

Chlorite Chlorous acid

Sulfite Sulfurous acid

3. Name to formula:

a. cyanic acid __________________ ________

b. dichromic acid ______________________ _______

c. hypochlorous acid _____________________ _______

d. hydrosulfuric acid _______________ ______

OCN- (Cyanate) HOCN

Cr2O72- (Dichromate) H2Cr2O7

ClO- (Hypochlorite) HClO

S2- (Sulfide) H2S

H+

H+

H+

H+

Compounds

Ionic Covalent

(Metal / Non-metal)

Binary Ternary

Acids

Contain H+

Binary Ternary

w/ oxygen

Hydrates Hydrates

• 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

• Non-metal / Non-metal

• Uses prefixes, -ide

• I2O7 Diiodine heptoxide

• No oxygen

• Hydro__ic acid

• ie, Hydrochloric acid

HCl

• -ate—ic

acid

• H2CO3

Carbonic

acid

• -ite---ous

acid

• H2SO3

Sulfurous

acid

• w/ H2O

• Uses prefixes

• ie. Calcium chloride

dihydrate

CaCl2 2H2O

•

• w/ H2O

• Uses prefixes

• ie. Calcium carbonate

trihydrate

CaCO3 3H2O

•

2.7

EOCP 2.88Mg2+

HCO3- Mg(HCO3)2

Sr2+ Cl-

Fe(NO2)3

Strontium chloride

Mn2+ ClO3- Mn(ClO3)2

Iron (III) nitrite

Tin (IV) bromideSn4+ Br-

Cobalt (II) phosphateCo3(PO4)2

Mercury (I) iodideHg2I2

Copper (I) carbonateCO32-Cu+

Li3NN3-Li+

Aluminum sulfideAl2S3