AP CHEM

2013-2014 AP CHEMISTRY STUDENTS 

There is no “required” summer assignment but I will not teach the 1 st unit (Chp 1 - Classification of matter, states 

of matter, scientific notation, significant figures) when school starts. If you want a little less work the first few 

days of school, complete the attached worksheets before school starts. A test will be given on these topics the 1 st 

week of school. This means that if you are solid on these concepts there is nothing to worry about this summer. 

If you are a little weak on these concepts you will need to spend some time before school starts reading and 

studying. If you want unit 2 to be a little less hectic you can use some of your summer time to start learning the 

common cations, anions and polyatomic ions on the last page of this handout. You will need to come by my 

classroom (rm 208) by Tuesday, June 4 th , to check out a book and ask any questions you might have. 

Have a great summer 

Mr. Duncan 

keith.duncan@ksd.org

© Adrian Dingle’s Chemistry Pages 2004, 2005, 2006, 2007, 2008, 2009, 2010. All rights reserved. 

These materials may NOT be copied or redistributed in any way, except for individual class instruction. 

Revised August 2009 

AP Common Ions 

CATIONS (+ve) 

ANIONS (-ve) 

Name 

Symbol/ 

Formula 

Alternative* 

Name 

Symbol/ 

Formula 

Alternative* 

Aluminum Al 3+ Bromide Br - 

Ammonium 

+ 

NH 4 Bromate (I) BrO - (Hypobromite) 

Arsenic (III) As 3+ Bromate (III) 

- 

BrO 2 (Bromite) 

Arsenic (V) As 5+ Bromate (V) 

- 

BrO 3 (Bromate) 

Barium Ba 2+ Bromate (VII) 

- 

BrO 4 (Perbromate) 

Bismuth (III) Bi 3+ Carbonate 

2- 

CO 3 

Bismuth (V) Bi 5+ Chlorate (I) ClO - (Hypochlorite) 

Cadmium Cd 2+ Chlorate (III) 

- 

ClO 2 (Chlorite) 

Calcium Ca 2+ Chlorate (V) 

- 

ClO 3 (Chlorate) 

Chromium (II) Cr 2+ Chlorate (VII) 

- 

ClO 4 (Perchlorate) 

Chromium (III) Cr 3+ Chloride Cl - 

Cobalt (II) Co 2+ Chromate 

2- 

CrO 4 

Cobalt (III) Co 3+ Cyanide CN - 

Copper (I) Cu + (Cuprous) Dichromate 

2- 

Cr 2O 7 

Copper (II) Cu 2+ (Cupric) Dihydrogen Phosphate 

- 

H 2PO 4 

Hydrogen H + Ethanoate 

- 

C 2H 3O 2 (Acetate) 

Hydronium H 3O + Fluoride F - 

Iron (II) Fe 2+ (Ferrous) Hydride H - 

Iron (III) Fe 3+ (Ferric) Hydrogen Carbonate 

- 

HCO 3 (Bicarbonate) 

Lead (II) Pb 2+ (Plumbous) Hydrogen Oxalate 

- 

HC 2O 4 (Binoxalate) 

Lead (IV) Pb 4+ (Plumbic) Hydrogen Phosphate 

2- 

HPO 4 

Lithium Li + Hydrogen Sulfate 

- 

HSO 4 (Bisulfate) 

Magnesium Mg 2+ Hydrogen Sulfide HS - (Bisulfide) 

Manganese (II) Mn 2+ Hydrogen Sulfite 

- 

HSO 3 (Bisulfite) 

Manganese (IV) Mn 4+ Hydroxide OH - 

Mercury (I) 

2+ 

Hg 2 (Mercurous) Iodate (I) IO - (Hypoiodite) 

Mercury (II) Hg 2+ (Mercuric) Iodate (III) 

- 

IO 2 (Iodite) 

Nickel (II) Ni 2+ Iodate (V) 

- 

IO 3 (Iodate) 

Potassium K + Iodate (VII) 

- 

IO 4 (Periodate) 

Silver Ag + Iodide I - 

Sodium Na + Manganate (VII) 

- 

MnO 4 (Permanganate) 

Strontium Sr 2+ Nitrate 

- 

NO 3 

Tin (II) Sn 2+ (Stannous) Nitride N 3- 

Tin (IV) Sn 4+ (Stannic) Nitrite 

- 

NO 2 

Zinc Zn 2+ Oxalate 

2- 

C 2O 4 (Ethandioate) 

Oxide O 2- 

Peroxide 

2- 

O 2 

Phosphate 

3- 

PO 4 

Phosphide P 3- 

Phosphite 

3- 

PO 3 

Sulfate 

2- 

SO 4 

Sulfide S 2- 

Sulfite 

2- 

SO 3 

Thiosulfate 

2- 

S 2O 3 

Thiocyanate SCN - 

* In the case of the cations, the alternative names are generally redundant in modern chemistry, but the anions sometimes use the alternate 

names. E.g. the oxyhalogen ions (bromate, chlorate, iodate etc.) are usually referred to by the alternate names, but HSO 3 - is more 

commonly called Hydrogen Sulfite. In each case where two names are given, the more common one used in the United States is 

underlined. 

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© Adrian Dingle’s Chemistry Pages 2004, 2005, 2006, 2007, 2008, 2009, 2010. All rights reserved. 



POLYATOMIC IONS 

+2 +1 -1 -2 -3 

Hg 2 

2+ 

NH 4 

+ 

BrO - 

- 

BrO 2 

- 

BrO 3 

- 

BrO 4 

- 

C 2H 3O 2 

ClO - 

- 

ClO 2 

- 

ClO 3 

- 

ClO 4 

CN - 

- 

HCO 3 

- 

HC 2O 4 

- 

H 2PO 4 

HS - 

- 

HSO 3 

- 

HSO 4 

IO - 

2- 

CO 3 

2- 

C 2O 4 

2- 

CrO 4 

2- 

Cr 2O 7 

2- 

HPO 4 

2- 

SO 3 

2- 

SO 4 

2- 

S 2O 3 

- 

IO 2 

- 

IO 3 

- 

IO 4 

- 

MnO 4 

- 

NO 2 

- 

NO 3 

OH - 

SCN - 

PO 3 

3- 

PO 4 

3- 

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© Adrian Dingle’s Chemistry Pages 2004, 2005, 2006, 2007, 2008, 2009. All rights reserved. 



AP WORKSHEET 1a: Significant Figures 

1. Determine the number of significant figures in each of the following. (6) 

(a) 0.7680 

(b) 1230.00 

(c) 1000.01 

(d) 120.0 

(e) 1.09 x 10 4 

(f) 0.0080060 

2. Use a calculator to find the results of the following and then round the answer to the correct 

number of significant figures. (6) 

(a) 34.66 + 333.0 

(b) 1.23 + 9.66 

(c) 445 - 1.22 

(d) 18.2 + 1.998 

(e) 10.2 – 1.34 

(f) 100 - 23 

3. State the significant figure rule that is associated with “captive zeros”. (1) 

4. State the significant figure rule that is associated with “leading zeros”. (1) 

5. State the significant figure rule that is associated with “trailing zeros”. (1) 

6. State the significant figure rule that is associated with addition and subtraction operations. (1) 

7. State the significant figure rule that is associated with multiplication and division operations. 

(1) 

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8. Use a calculator to find the results of the following calculations and then round the answer to 

the correct number of significant figures. (6) 

(a) 12 x 11.45 

(b) (1.23 x 10 3 ) x (6.4 x 10 2 ) 

(c) 5.233 x 6.324 

(d) 34 / 22 

(e) (1.8 x 10 5 ) / 14 

(f) 100.23 / 5.22 

9. Round each of the following to three significant figures. (6) 

(a) 167.789 

(b) 0.0000456922 

(c) 23.00567 

(d) 3.4569 

(e) 7903.0005 

(f) 11.044 

10. How many significant figures in each of the following? (6) 

(a) 654.001 nm 

(b) 6.02 x 10 23 particles 

(c) 1.0079 g 

(d) 13 neutrons 

(e) 11.22201 mg 

(f) 

0.004504 g 

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AP WORKSHEET 1b: Unit Conversions 

This worksheet utilizes the conversions given at this web site http://www.onlineconversion.com 

1. Perform the following conversions. In each case show the full, dimensional analysis. Source 

any conversion factors from the web site above. An example is given below. (6) 

Question: 3.00 cm to mm. 

Answer: 

3.00 cm 10 mm 

 

 

 

1 cm 

= 30 mm 

(a) 120 J to MJ 

(b) 3 m to cm 

(c) 400 miles to km 

(d) 25 hectares to acres 

(e) 34 inches to ft 

(f) 

289 s to hrs 

2. Perform the following conversions. In each case you do NOT need to show the full, 

dimensional analysis. Source any conversion factors from the web site above. (6) 

(a) 120000 J to kJ 

(b) 13 kg to lbs 

(c) 83.2 K to o C 

(d) 48 mins to ms 

(e) 34 o F to o C 

(f) 

13.2 kg to lbs 

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3. Perform the following sequences of conversions. In each case show the full, dimensional 

analysis. Source any conversion factors from the web site above. An example is given below. 

(6) 

Question: 3.00 cm to m VIA mm. 

Answer: 

3.00 cm 10 mm 

0.001 m 

 

 

= 0.03 m 

 

1 cm 

1 mm 

(a) 679 nm to cm VIA m 

(b) 23 miles to m VIA km 

(c) 567 feet to m VIA yd 

(d) 12 L to UK gal VIA mL 

(e) 8 MJ to J VIA kJ 

(f) 

418 s to hrs VIA min 

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AP WORKSHEET 1s: Matter & Measurement Summary 

1. Classify each of the following as either, an element, a compound or a mixture. If you 

classify something as a mixture then also state whether it is a homogeneous or a 

heterogeneous mixture. (10) 

(a) Helium 

(b) Nitrogen 

(c) Pure water 

(d) Pure table salt (sodium chloride) 

(e) Flat (un-carbonated) Coca-Cola 

(f) 

Air 

(g) Fruit cake 

2. Classify the following as either chemical or physical changes. (3) 

(a) Ice melting 

(b) Gasoline burning 

(c) Evaporation of perfume from an open bottle 

3. Mercury is a liquid metal that has a density of 13.58 g/mL. Calculate the volume of mercury 

that must be poured out in order to obtain 0.5000 g of Mercury. (2) 

4. Classify the following as either quantitative or qualitative observations. (4) 

(a) My eyes are brown 

(b) My neck size is 17 inches 

(c) My average grade last year was 79% 

(d) Physics is a difficult subject 

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5. Give an example of a natural law (other than the law of conservation of mass). (1) 

6. Convert these numbers to scientific notation. (2) 

(a) 35800000000000 

(b) 0.00000000821 

7. Round the following numbers to four figures. (6) 

(a) 2.16347 x 10 5 

(b) 4.000574 x 10 6 

(c) 3.682417 

(d) 7.2518 

(e) 375.6523 

(f) 21.860051 

8. Perform the following conversions. (5) 

(a) 0.75 kg to milligrams 

(b) 1500 millimeters to km 

(c) 2390 g to kg 

(d) 0.52 km to meters 

(e) 65 kg to g 





9. Complete the following table of temperatures, performing the appropriate conversions. (18) 

Kelvin Fahrenheit Celsius 

200. 

23.0 

0.000 

180. 

45.0 

500. 

350. 

97.0 

30.0 

10. An experiment is performed in which the molar mass of a gas is found to be 48.45 g mol -1 . 

The published (actual) value is 52.98 g mol -1 . Calculate the percentage error. (2) 

11. Distinguish carefully between precision and accuracy. (2)

AP CHEM

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