Resource for Worksheets CHEMCP1Workbookv411_12.doc Rsource for Worksheets-2

Here is a good example A chemical reaction occurs between solid Zinc Zn and Hydrochloric Acid solution HCl forming the products Zinc Chloride solution ZnCl 2 solution and Hydrogen Gas H

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College Preparatory Chemistry

Level 1

Worksheet Book

2011-2012

Science Department Framingham High School

1

Name: Date: Per: _

Table of Contents

Table of Contents 2

Scientific Method 5

Matter Tree 6

Element Symbols 7

Physical vs Chemical Properties 8

Physical vs Chemical Changes 9

Metrics and Measurement 10

Metric System Worksheet 1 11

Using the Correct Units 12

Scientific Notation 13

Significant Figures Worksheet 1 14

Significant Figures Worksheet 2 15

Significant Figures Worksheet 3 16

Density 17

Accuracy vs Precision 18

Temperature & its Measurement 19

Percentage Error 20

Atomic Structure 1 21

Atomic Structure 2 22

Isotopes & Average Atomic Mass 23

Wave Worksheet 24

Electron Configuration Worksheet #1 25

Electron Configuration Worksheet #2 26

Writing Chemical Equations. 27

Types of Reactions Worksheet 29

REDOX Worksheet 1 31

REDOX Worksheet 2 32

Balancing Equations Worksheet #1 33

Balancing Equations Worksheet #2 35

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Balancing Worksheet #3 37

Dimensional Analysis – or – Unit Analysis – or – Factor-Label Method #1 39

Dimensional Analysis – or – Unit Analysis – or – Factor-Label Method #2 40

Mole Worksheet 1 41

Mole Worksheet 2 42

Mole Worksheet 3 43

Molarity 1 44

Percent Composition Worksheet 45

Empirical and Molecular Formulas Worksheet 46

Stoichiometry Worksheet #1 47

Stoichiometry Worksheet #2 48

Stoichiometry #3 49

Stoichiometry Worksheet #4 50

Stoichiometry Worksheet #5 51

Limiting Reagent Worksheet 52

Freezing and Boiling Point Graph 54

Heat Calculations 55

Heat and Phase Changes 56

Heat and its Measurement 57

Thermochemistry Worksheet 1 58

Thermochemistry Worksheet 2 59

Nuclear Chemistry Worksheet 60

Boyles Law Worksheet 62

Charles’ Law 64

Temperature-Pressure Law 66

Gas Laws Worksheet #1 67

Gas Laws Worksheet #2 68

Gas Laws Worksheet #3 70

Gas Laws Worksheet #4 71

Gas Law Practice 73

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Bonding/Solutions Worksheet #1 74

Bonding/Solutions Worksheet #2 75

Bonding/Solutions Worksheet #3 76

Molarity Worksheet 2 77

Molarity Worksheet 3 78

Dilutions Worksheet 79

Rate Worksheet #1 80

Rate Worksheet #2 81

Rate Worksheet #3 82

Equilibrium Worksheet 83

Molarity, [H+], [OH-], pH, and pOH Relationships 85

Acid Base Worksheet #1 87

Acid Base Worksheet #2 88

Acid Base Worksheet #3 89

Acid Base Worksheet #4 90

Acids, Bases, Conjugate Acids and Conjugate Bases 91

Worksheet on pH and Strong Acid Base Reactions 92

Review Worksheet 1 93

Review Worksheet 2 94

Review Worksheet 3 95

Review Worksheet 4 96

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Scientific Method

Put the following steps of the scientific method in the proper order

_ Research the problem

_ Observe and record

_ Make a hypothesis

_ Identify the problem

_ Arrive at a conclusion

_ Test the hypothesis

Match the following terms with the correct definition:

g) factor that changes in an experiment

5

homogeneous mixture have the same composition all the way through A heterogeneous

mixture does not have the same composition all the way through

Classify the following as a substance or a mixture If it is a substance choose either element or compound If it is a mixture choose either heterogeneous or

homogeneous Choose 1 of the following:

Type of Matter ElementSubstanceCompound HomogeneouMixture

Element Symbols

Elements are given names and symbols When writing the formulas of compounds, symbols are much easier to use than the names We need to be familiar with the names and symbols of common elements The symbol of an element is usually taken from the first one or two letters of the name of the element However, sometimes the symbol comes from the Latin name of the element!

Write the symbol for the following elements:

Physical vs Chemical Properties

A physical properties is observed with the senses and can be determined without destroying the object For example, color, shape, mass, length and odor are all examples

Classify the following properties as either chemical or physical by putting a check

in the appropriate column

Physical Property Chemical Property

9 Reacts with water to form a gas

10 Reacts with a base to form water

Physical vs Chemical Changes

In a physical change, the original substance still exists, it has only changed form

In a chemical change, a new substance is produced Energy changes always accompany chemical changes

Classify the following as being a physical or chemical change

1 Sodium hydroxide dissolves in water

2 Hydrochloric acid reacts with potassium hydroxide to produce a

salt, water and heat

3 A pellet of sodium is sliced in two

4 Water is heated and changed to steam

5 Potassium chlorate decomposes to potassium chloride & oxygen

gas

6 Iron rusts

7 When placed in H2O, a sodium pellet catches on fire as

hydrogen gas is liberated and sodium hydroxide forms

13 Pancakes cooking on a griddle

14 Grass growing in a lawn

15 A tire is inflated with air

16 Food is digested in the stomach

17 Water is absorbed by a paper towel

Metrics and Measurement

Scientists use the metric system of measurement, based on the number 10 It is

important to be able to convert from one unit to another

Answer: To go from milli (m) to the BASE UNIT, liters, count on the above chart

three places to the left Move the decimal point three places to the left

Metric System Worksheet 1

Fill in the number line below

Using the Correct Units

For each of the following commonly used measurements, indicate its symbol Use the symbols to complete the following These may be used more than once

_ kilogram _ millimeter _ kilometer _ gram

1) Colas may be purchased in two or three _ bottles

2) The mass of a bowling ball is 7.25 _

3) The length of a common housefly is about 1 _

4) The mass of a paperclip is about 1 _

5) One teaspoon of cough syrup is about 5 _

6) The speed limit on the highway is usually 106.6 _/h or 29 _/s

7) The length of the small intestine in man is about 6.25 _

8) Viruses such as AIDS, polio and flu range in length from 17 to 1000 _

9) Adults require 1,000 _ of calcium to meet the U.S RDA

10) In a vacuum light can travel 300 km in one _

11) The mass of a proton is 1.67 x 10 -18 _

12) Blue light has a wavelength of about 500 _

13) One mole of oxygen gas at STP occupies 22.4 _

14) Myoglobin, a protein that stores oxygen, has a mass of 2.98 x 10 -14 _

15) Buttery popcorn contained in a large 1 _ bowl has a mass of about 50 _ of

fat and about 650 calories

16) The dying comet fragments that continued to batter Jupiter travel at speeds of

about 58,117 _/ _ or about 130,000 miles per hour

17) The human heart has a mass of about 1.05 _

18) Stand with your arms raised out to your side The distance from your nose to your

outstretched middle finger is about 1 _

19) The body mass of a flea is about 0.5 _ and it can jump about 20 _ high.20) On a statistical basis, smoking a single cigarette lowers your life expectancy by

642,000 _ or 10.7 minutes

Scientific Notation

Scientists very often deal with very small and very large numbers, whichcan lead to a lot of confusion when counting zeros! We have learned to expressthese numbers as powers of ten

Scientific notation takes the form of M x 10n, where 1 < M < 10 and “n”

represents the number of decimal places to be moved Positive “n” indicates thestandard (decimal) form is larger than zero whereas a negative “n’ would indicate a number smaller than zero

Convert the following into scientific notation:

Convert the following into standard notation:

Example 1: Convert 1,500,000 to scientific notation

We move the decimal point so that there is only one digit to its left,

a total of 6 places

1,500,000 = 1.5 x 106 (“n” is positive because original number is larger than 0)

Example 2: Convert 0.000025 to scientific notation

For this example, we move the decimal point 5 places to the right, again so that there is only one digit to its left

0.000025 = 2.5 x 10-5 (“n” is negative because original number is smaller that 0)

Example 3: Convert the 9.6 x 10-4 into standard notation

Because “n” is negative, this indicates that the number is smaller than 0 This means that we move the decimal point 4 places to the left

Significant Figures Worksheet 1

Rules for Significant Figures

(all bold numbers are significant)

1 All non-zero digits are significant

Addition and Subtraction: Round off the answer to the place of the number with the leastnumber of decimal places

Significant Figures Worksheet 2

1 Determine the number of significant figures in the following, then write the

numbers in scientific notation:

# ofSignificantFigures

Significant Figures Worksheet 3

For all of the following, remember to record your answer to the correct number of

Which has a greater mass, air or lead? Most of you would answer lead, but actually this question does not have an answer To compare these two things you need to know how much of each you have A large amount of air could have a greater mass than a small amount of lead To compare different things, we have to compare the masses of each that occupy the same space, or volume This is called density

Density = Mass

VolumeYou can remember that density is a broken heart (M/V)

Solve the following problems Remember to use the correct number of significant figures!

1) What is the density of carbon dioxide gas if 0.196 g occupies a volume of

100 mL.?

_2) A block of wood 3.0 cm on each side has a mass of 27 g What is the density

of this block?

_3) An irregularly shaped stone was lowered into a graduated cylinder holding a volume of water equal to 2.0 mL The height of the water rose to 7.0 mL If the mass of the stone is 25 g, what is the density?

_4) A 10.0 cm3 sample of copper has a mass of 89.6 grams What is the density

of copper?

_5) Silver has a density of 10.5 g/cm3 and gold has a density of 19.3 g/cm3

Which would have a greater mass, 5 cm3 of silver or 5 cm3 of gold?

_6) Five milliliters of ethanol has a mass of 3.9 g, and 5.0 mL of benzene has a mass of 4.4 grams Which liquid is denser?

_7) A sample of iron has the dimensions of 2 cm x 3 cm x 2 cm If the mass of this rectangular shaped object is 94 g, what is the density of iron?

_8) Three liquids are immiscible (they do not mix) They are placed in the same container Liquid A has a density of 4.5 g/mL, liquid B has a density of 3.2 g/mL,and 4.5 grams of liquid C has a volume of 1.3 mL

Which liquid will rise to the top? _ Which liquid will sink to the bottom?

_

Accuracy vs Precision

1 What is meant by the term “accuracy”?

2 What is meant by the term “precision”?

3 Under what circumstances could a series of measurements of the same

quantity be precise but inaccurate?

4 Which of the following synonyms or characteristics apply to the concept of

accuracy and which apply to precision?

5 Three students made multiple weighings of a copper cylinder, each using a

different balance The correct mass of the cylinder had been previously

determined to be 47.32 g Describe the accuracy and precision of each student’s measurements

Temperature & its Measurement

Temperature (which measures the average kinetic energy of the molecules) can be measured using three common scales: Celsius, Kelvin, & Fahrenheit We use the

following formulas to convert from one scale to another Celsius is the scale most

desirable for laboratory work Kelvin represents the absolute scale Fahrenheit is the oldEnglish scale, which is never used in lab!

Complete the following table

1

0C2

-273 C

6

294 K7

Percentage Error

Percentage error is a way for scientists to express how far off a laboratory value is from the commonly accepted value

The formula is:

Determine the percentage error in the following problems:

% error =  Accepted Value – Experimental Value  x 100

Accepted value

 ~ absolute value

This structure can be written as part of a chemical symbol.

Complete the following table:

Write a formula to determine the mass # of an atom

Write a formula to determine the charge on an atom (ion)

4 What three subatomic particles make up the atom? What are the relative masses of each?

5 What is the charge on each of the three particles listed in number 4?

6 How is an ion formed?

7 What is an isotope?

8 What is needed to determine the average atomic mass of an element?

9 If element Q has three isotopes, calculate the average atomic mass given the following data:

a Isotope A has a relative abundance of 78% and a mass of 230

b Isotope B has a relative abundance of 15% and a mass of 228

c Isotope C has a relative abundance of 7% and a mass of 232.

Isotopes & Average Atomic Mass

Elements come in a variety of isotopes, meaning they are made up of atoms with the same atomic number but different atomic masses These atoms differ in the number

of neutrons

The average atomic mass is the weighted average of all of the isotopes of an atom

Determine the average atomic masses of the following:

b i nH0.2% Com

Wave Worksheet

c=  E=h h=6.626 x 10 -34 Js c=3.00 x 10 8 m/s 1m = 10 9 nm

= h/(mv) The diagram on the left represents a wave.

Use the information to answer the following questions.

1) What is the wavelength of this wave

2) If it took 3.75 x 10 -17 seconds for the wave to go through 2.5 cycles, what is the frequency of the wave?

3) How many nodes are in the wave on the right?

4) a)Calculate the energy of one photon of the light wave depicted in the figure

b) calculate the energy from 1 mole of photons of this wave

5a) How are frequency and wavelength related?

b) calculate the wavelength associated with a frequency of 500 Hz

c) Calculate the frequency of Ultra violet light with a wavelength of 308 nm

6) Calculate the energy associated with red light with a wavelength of 600 nm

7) Why don’t massive objects (such as a baseball) have an observable wavelength, yet an

electron does?

4.5 x 10-9m

Electron Configuration Worksheet #1

1 What are valence electrons?

2 How many valence electrons do the following elements have

Electron Configuration Worksheet #2

1 Write the abbreviated (short cut method) electron configuration for the following elements:

Writing Chemical Equations.

So far in chemistry we have discussed many different types of reactions In chemistry, we use words to describe the reaction, but we use symbols in order to make things simpler

Sometimes, a chemical reaction can even look more like a math equation, and in many cases it is very similar.

Here is a good example

A chemical reaction occurs between solid Zinc (Zn) and Hydrochloric Acid solution (HCl) forming the products Zinc Chloride solution (ZnCl 2 ) solution and Hydrogen Gas (H 2 ).

What we have to do is translate this into a chemical equation.

When we say a reaction occurs between Solid Zinc and Hydrochloric acid solution, we

symbolize this by saying

Zn (s) + HCl (aq)

The “s” in subscript parentheses refers to Solid Phase Zinc The “aq” in subscript

parentheses refers to a solution of HCl in water.

When we say a reaction occurs between substances (elements or compounds), we mean they are reactants and should be placed on the left side of the equation When we say forms, produces, or becomes, we put a forms arrow.

A chemical reaction occurs between solid Zinc (Zn) and Hydrochloric Acid solution (HCl) forming

Zn (s) + HCl (aq)  After forms, becomes, yields, or makes, we have the products, or what the reactants react to form There should be some difference in how the products are arranged in a chemical reaction.

A chemical reaction occurs between solid Zinc (Zn) and Hydrochloric Acid solution (HCl) forming

the products Zinc Chloride (ZnCl 2 )solution and Hydrogen Gas (H 2 )

We finish the reaction by placing the products in the equation.

Zn (s) + HCl (aq)  ZnCl 2(aq) + H 2(g)

Try some of the following examples:

1 Solid Aluminum (Al) reacts with Chlorine gas (Cl 2 ) forming Aluminum Chloride (solution) (AlCl 3 )

(Next page for More!)

2 Solid Copper reacts with an aqueous solution of Silver Nitrate (AgNO 3 ) forming Solid Silver (Ag) and Copper II Nitrate Cu(NO 3 ) 2 solution.

3 Methane gas (CH 4 ) reacts with Oxygen gas (O 2 ) producing Carbon Dioxide gas and Water gas.

4 Solid Calcium Nitrate (Ca(NO 3 ) 2 ) decomposes forming solid calcium oxide (CaO) and Nitrogen Dioxide gas (NO 2 )

5 Sodium Chloride Solution (NaCl) reacts with Silver Nitrate solution (AgNO 3 ) producing solid Silver Chloride (AgCl) and Sodium Nitrate solution (NaNO 3 ).

6 Aqueous Acetic Acid (CH 3 COOH) neutralizes Sodium Hydroxide (NaOH) solution yields

Aqueous Sodium Acetate (NaCH 3 COO) and liquid water.

7 Sulfuric Acid gas (H 2 SO 4 ) reacts with Ammonia gas (NH 3 ) forming ammonium Sulfate solid {(NH 4 ) 2 SO 4 }

Types of Reactions Worksheet

1 Balance the following reactions Then, indicate the type of reaction for each

h Zn + AgNO3  Zn(NO3)2 + Ag

_

(Next page for More!)

2 Write and balance the equations for the following reactions Be sure to include the state of matter for example (s) for solid

a aqueous sodium chloride reacts with aqueous lead (II) nitrate to yield a lead (II) chloride precipitate and aqueous sodium nitrate

b silver nitrate reacts in solution with potassium chromate to yield a silver chromate precipitate and soluble potassium nitrate

c solid calcium carbonate reacts with hydrochloric acid [HCl(aq)] to yield aqueous calcium chloride, carbon dioxide gas, and liquid water

d solid aluminum hydroxide reacts with nitric acid to yield soluble aluminum nitrate and liquid water

e aqueous sodium hydroxide reacts with carbon dioxide gas to yield soluble sodium carbonate and liquid water

3 Determine the type of reaction, predict the products and balance the following:

a N 2 + H 2 

b Sn + Cl 2 

c Fe + HCl 

d MgCl 2 + LiI 

REDOX Worksheet 1

Worksheet Part 1) Assigning Oxidation Numbers

Assign oxidation numbers to all of the elements in each of the compounds below

Worksheet Part 2) Redox

For the equations below, identify the substance that is oxidized, the substance that is reduced, the oxidizing agent, and the reducing agent Then write the oxidation half reaction and the reduction half reaction

4) Cu + AgNO3 Cu(NO3)2 + 2Ag

REDOX Worksheet 2

Oxidation State Worksheet

In each of the following chemicals, write the formulas and determine the oxidation states

12) 2 H2 + O2  2 H2O

Element oxidized: Element reduced:

Balancing Equations Worksheet #1

Balance the following equations;

6 _AlBr3 + _K2SO4  _KBr + _Al2(SO4)3

(Next page for More!)

Balancing Equations Worksheet #2

Balance the following equations;

4 _Al + _NaOH  _Na3AlO3 + _H2

6 _Al2(SO4)3 + _Ca(OH)2  _Al(OH)3 + _CaSO4

7 _Al2(SO4)3 + _NaHCO3  _Al(OH)3 + _Na2SO4 + _CO2

(Next page for More!)

8 _BaO + _C + _N2  _Ba(CN)2 + _CO