Solution manual chemistry k c timberlake 2nd edition

All three numbers including the zeros that follow a nonzero digit in a decimal number are 2.24 In a and b both pairs have three significant figures.. helium, He 4.29 of Element Symbol Nu

Chemistry in Our Lives

1.1 a Chemistry is the science of the composition and properties of matter.

b A chemist is a scientist who studies the composition and changes of matter.

c A chemical is a substance that is used in or produced by a chemical process.

1.2 Your friends may give a variety of definitions, most of which will probably not agree with the tionary definitions

dic-1.3 Many chemicals are listed on a vitamin bottle such as: vitamin A, vitamin B3, vitamin B12, vitamin

C, folic acid, etc

1.4 Many chemicals are listed on a cereal box such as: vitamin A, vitamin B6,vitamin B12, vitamin C,folic acid, sugar, salt, iron, etc

1.5 Typical items found in a medicine cabinet and chemicals they contain:

Antacid tablets: calcium carbonate, cellulose, starch, stearic acid, silicon dioxide Mouthwash: water, alcohol, glycerol, sodium benzoate, benzoic acid

Cough suppressant: menthol, beta-carotene, sucrose, glucose

1.6 Typical items found in cleansers are: water, ammonia, sodium silicate, and sodium phosphate

1.7 No All of these ingredients are chemicals

1.8 No All of these ingredients are chemicals

1.9 An advantage of a pesticide is that it protects crops from damage by various insects Somedisadvantages are that a pesticide can destroy beneficial insects, be retained in a crop that iseventually eaten by animals or humans, or pollute ground water

1.10 Some advantages of eating sugar is that it gives energy and tastes sweet Some disadvantages are

that sugar can lead to obesity and tooth decay

1.11 a A hypothesis proposes a possible explanation for a natural phenomenon.

b An experiment is a procedure that tests the validity of a hypothesis.

c A theory is a hypothesis that has been validated many times by many scientists.

d An observation is a description or measurement of a natural phenomenon.

1.12 a hypothesis

b observation

c experiment

d theory 1.13 (1) observation (2) hypothesis (3) experiment (4) observation (5) observation (6) theory 1.14 (1) observation (2) hypothesis (3) experiment

(4) experiment (5) observation (6) hypothesis or theory 1.15 There are several things a student can do to be successful in chemistry, including forming a study

group, going to lecture, working sample problems and study checks, working problems andchecking answers, reading the assignment ahead of class, going to the instructor’s office hours,and keeping a problem notebook

1.16 There are many things that make it difficult to learn chemistry, including not going to lecture

regularly, not working problems and study checks, not reading the assignment ahead of class, notgoing to the instructor’s office hours, and waiting until the night before an exam to study

1.17 a Form a study group.

c Visit the professor during office hours.

e Become an active learner.

1.18 a, c, d, and e.

1.19 Yes Sherlock’s investigation includes observations (gathering data), formulating a hypothesis,

testing the hypothesis, and modifying it until the hypothesis is validated

1.20 Sherlock meant that you should not propose a theory until you have data from experiments and

observations

1.21 a Determination of a melting point with a thermometer is an observation.

b Describing a reason for the extinction of dinosaurs is a hypothesis or theory.

c Measuring the speed of a race is an observation.

1.22 a observation

b observation

c hypothesis or theory 1.23 A hypothesis, which is a possible explanation for an observation, can be tested with experiments 1.24 Experimentation is used to test and verify a hypothesis.

1.25 b Another hypothesis needs to be written when experimental results do not support the previous

hypothesis

c More experiments are needed for a new hypothesis.

1.26 b Many experiments by many scientists validate the hypothesis.

1.27 A successful study plan would include:

b Working the sample problems throughout the chapter.

c Going to the instructor’s office during office hours.

1.28 A successful study plan would include:

b Forming a study group and discussing problems with others.

c Working problems in a notebook for reference before exams.

1.29 a (1) observation

b (2) hypothesis

c (3) experiment

d (2) hypothesis 1.30 a (1) observation

b (2) hypothesis

c (1) observation

d (1) observation

Measurements

2.1 a meter, length b gram, mass c liter, volume

d second, time e Celsius, temperature 2.2 a liter, volume b meter, length c kilogram, mass

d gram, mass e kelvin, temperature 2.3 a meter; both b kilogram, both c foot, neither

d second, both e Celsius, metric 2.4 a cubic meter, both b kelvin, SI c Fahrenheit; neither

d liter, metric e gram, metric 2.5 a gram; metric b liter; metric c Celsius; metric

d meter; both e second; both 2.6 a kelvin, SI b kilogram, both c liter, metric

d meter, both e cubic meter, both 2.7 a Move the decimal point left four places to give

b Move the decimal point left two places to give

c Move the decimal point right six places to give

d Move the decimal point right four places to give

e Move the decimal point right three places to give

f Move the decimal point left six places to give

2.9 a The value , which is also , is greater than

b The value , which is also , is greater than

c The value or 10 000 is greater than , or 0.0001

d The value or 0.068 is greater than 0.00052

2.11 a The standard number is 1.2 times the power of , or 10 000, which gives 12 000

b The standard number is 8.25 times the power of , or 0.01, which gives 0.0825

c The standard number is 4 times the power of , or 1 000 000, which gives 4 000 000

d The standard number is 5 times the power of , or 0.001, which gives 0.005

2.13 a The estimated digit is the last digit reported in a measurement In 8.6 m, the 6 in the first

decimal (tenths) place was estimated and has some uncertainty

b The estimated digit is the 5 in the second decimal (hundredths) place.

c The estimated digit would be the 0 in the first decimal (tenths) place.

2.14 a The estimated digit is the last digit reported in a measurement In 125.04 g, the 4 in the

hundredths place is estimated and has some uncertainty

b The estimated digit is the 7 in the third decimal (thousandths) place.

c The estimated digit would be the 8 in the first decimal (tenths) place.

1.5 10
1 m7.5 105 g

6 10
5 m1.8 108 g

6.7 105 kg7.85 10
3 L1.4 10
4 s

5 10
6 cm4.8 102 g5.5 104 m

2.15 Measured numbers are obtained using some kind of measuring tool Exact numbers are numbers

obtained by counting or from a definition in the metric or the U.S measuring systems

2.16 a exact b measured c measured d measured

2.17 Measured numbers are obtained using some kind of measuring tool Exact numbers are numbers

obtained by counting or from a definition in the metric or the U.S measuring systems

a The value 6 oz of meat is obtained by measurement, whereas 3 hamburgers is a counted/

exact number

b None; both 1 table and 4 chairs are counted/exact numbers.

c Both 0.75 lb and 350 g are obtained by measurements.

d None; the values in a definition are exact numbers

2.18 a 5 pizzas b 6 nickels c 3 onions d 5 cars

2.19 a Zeros preceding significant digits are not significant.

b Zeros between significant digits are significant.

c Zeros after significant digits in a decimal number are significant.

d Zeros in the coefficient of a number written in scientific notation are significant.

e Zeros in a number with no decimal point are considered as placeholders only and not significant.

2.20 a significant b significant c not significant d not significant

e significant 2.21 a All five numbers are significant figures.

b Only the two nonzero numbers are significant; the preceding zeros are placeholders.

c Only the two nonzero numbers are significant; the zeros that follow are placeholders.

d All three numbers in the coefficient of a number written in scientific notation are significant.

e All four numbers including the last zero in a decimal number are significant.

f All three numbers including the zeros that follow a nonzero digit in a decimal number are

2.24 In a and b both pairs have three significant figures In d both pairs have two significant figures.

2.25 a 5 000 is the same as , which is written in scientific notation as

b 30 000 is the same as , which is written in scientific notation as

c 100 000 is the same as , which is written in scientific notation as

d 0.000 25 is the same as , which is written in scientific notation as

2.27 Calculators carry out mathematical computations and display without regard to significant figures.

Our task is to round the calculator’s answer to the number of significant figures or digits allowed

by the values of the original data

2.28 The number in the calculator display does not show the correct number of significant figures.

Thus, a significant zero must be added

2.29 To round a number, determine how many significant figures are kept and drop all remaining digits.

There is no change in the retained figures if the first digit dropped is 0 to 4 However, if the firstdigit dropped is 5 to 9, raise the last retained digit by 1

8.2 10
4 kg4.0 104 m

2.6 104 s5.1 106 g

2.5 10
42.5 1

a To round 1.854, drop the 4 and keep 1.85.

b To round 184.2038, drop 2038 and keep 184.

c To round 0.004 738 265, drop 8265 and increase the retained digits by 1, or 0.004 74.

d To round 8807 to three significant figures, drop 7 and increase the retained digits to 8810,

keeping a zero in the ones place as a placeholder In scientific notation:

e To round 1.832 149, drop 2149 and keep 1.83 as the rounded value.

2.31 a Drop 55 and increase the last digit by 1, which gives 56.9 m.

b Drop 25, and keep remaining digits as 0.00228 g.

c Drop 27, keep remaining digits, and add two zeros as placeholders, 11 500 s

d Add a significant zero to give three significant figures, 8.10 L.

2.33 a Because the value of 0.034 has 2 SFs, the answer 1.6 can have only 2 SFs.

b The measurement 5 has 1 SF, which allows 1 SF in the answer (0.01).

c The measurement 1.25 has 3 SFs, which allows 3 SFs in the answer (27.6):

d The measurement 25 has 2 SFs, which allows 2 SFs in the answer (3.5):

e The measurement has 2 SFs, which allows 2 SFs in the answer (0.14):

f The measurement has 1 SF, which allows 1 SF in the answer (0.8):

2.35 The answer of addition/subtraction problems has the same number of places as the measurement

with the largest place

45.48 cm 2 decimal places

+ 8.057 cm 3 decimal places53.54 cm 2 decimal places

2.8 104

(0.2465)(25)1.78  3.5

34.561.25  27.6

1.9 102 g

(1.15 104 s)8.81 103

23.45 g 2 decimal places104.1 g 1 decimal place

+ 0.025 g 3 decimal places127.6 g 1 decimal place

1.08 L 2 decimal places

0.585 L 3 decimal places0.50 L 2 decimal places

145.675 mL 3 decimal places

24.2 mL 1 decimal place

121.5 mL 1 decimal place

2.37 The km/h markings indicate how many kilometers (how much distance) will be traversed in

1 hour’s time if the speed is held constant The mph markings indicate the same distance traversed

but measured in miles during the 1 hour of travel.

2.38 On the speedometer, 80 kph is about 50 mph You are not exceeding the 55 mph speed limit if

your speedometer reads 80 km/hr (kph)

2.39 Because the prefix kilo means one thousand times, a kilogram is equal to 1000 grams.

2.40 Because the prefix centi means one hundredth, a centimeter is one hundredth of a meter.

2.42 a centimeter b kilogram c deciliter

d gigameter e microgram f picogram

2.44 a 1 decigram b 1 microgram c 1 kilogram

d 1 centigram e 1 milligram f 1 picogram

2.47 a A kilogram, which is 1000 g, is larger than a milligram (0.001 g).

b A milliliter, which is , is larger than a microliter

c A km, which is , is larger than a cm

d A kL, which is , is larger than a dL

2.49 Because a conversion factor can be inverted to give a second factor

2.50 Verify that the units cancel when the conversion factors are applied.

2.51 The numerator and denominator are from the equality:

2.55 The equalities between the metric prefixes can be written as two conversion factors.

46.0 km1.0 gal1.0 gal 46.0 km

1 mL0.65 g

0.65 g

1 mL

1 mL  0.65 g

1 s3.5 m

3.5 m

1 s3.5 m 1 s

1 in.2(2.54)2 cm2

(2.54)2 cm2

1 in.2

1 in.2 (2.54)2 cm2

1 L1.057 qt

1.057 qt

1 L1.057 qt 1 L

453.6 g

1 lb

1 lb453.6 g

1 lb  453.6 g

2.205 lb

1 kg

1 kg2.205 lb

(100 cm)3(1 m)3(1 m)3 (100 cm)3

2.59 When using a conversion factor, you are trying to cancel existing units and arrive at a new

(desired) unit The conversion factor must be set up to give unit cancellation

2.60 The new (desired) unit should be in the numerator of the conversion factor.

11.8 stones 14 lb

1 stone  1 kg

2.205 lb  74.9 kgPlan: stone : lb : kg

0.750 qt  1 L

1.057 qt  1000 mL

1 L  710 mLPlan: qt : mL

150 000 m2 1 km2

(1000)2 m2  0.15 km2Plan: m2 : km2

2840 mg 1 g

1000 mg  2.84 gPlan: mg : g

0.85 dL  100 mL

1 dL  85 mLPlan: dL : mL

800 mg 1 g

1000 mg  0.8 gPlan: mg : g

350 cm3 1 m3

(100)3 cm3  3.5  10
4 m3Plan: cm3: m3

0.0055 kg 1000 g

1 kg  5.5 gPlan: kg : g

5500 mL 1 L

1000 mL  5.5 LPlan: mL : L

175 cm 1 m

100 cm  1.75 mPlan: cm : m

The metal is lead.

2.70 The volume of a cube, 2.0 cm on each edge, is calculated as follows:

A cube will displace its volume when submerged in water, so the final volume reading in eachgraduated cylinder is:

2.71 Density is the mass of a substance divided by its volume The densities of solids and liquids are

usually stated in or Density Mass (grams)

Volume (mL)

g/cm3g/mL

40.0 mL water 8.0 mL metal  48.0 mL total volume(2.0 cm)3  1 mL/1 cm3 8.0 mL

217 g metal19.2 cm3 metal  11.3 g/cm3

11.3 g/cm310.5 g/cm3

2.70 g/cm3

5.0 kg pecans 100 kg choc bars

22.0 kg pecans  2.205 lb

1 kg  50 lb of chocolate barsPlan: kg pecans : kg choc bars : lb (percent equality: 100.0 kg bars 22.0 kg pecans)

10.0 oz fertilizer  1 lb

16 oz  453.6 g

1 lb  15 g nitrogen

100.0 g fertilizer  43 g nitrogenPlan: oz : lb : g : g nitrogen (percent equality: 100.0 g fertilizer  15 g nitrogen)

1.25 g crust  2.1 g magnesium

100.0 g crust  0.026 g magnesiumPlan: g crust : g magnesium (percent equality: 100.0 g crust 2.1 g magnesium)

325 g crust 46.7 g oxygen

100.0 g crust  152 g oxygenPlan: g crust : g oxygen (percent equality: 100.0 g crust 46.7 g oxygen)

27.0 ft 12 in.

1ft  2.54 cm

1 in  1 m

100 cm  8.23 m (width)Plan: ft : in : cm : m : m2

78.0 ft 12 in.

1 ft  2.54 cm

1 in  1 m

100 cm  23.8 m (length)Plan: ft : in : cm : m

18.5 gal
12.2 gal  6.3 gal

46.0 L  1.057 qt

1 L  1 gal

4 qt  12.2 gal

b The height is measured with a ruler or tape measure; it is a measured number.

c The number of chairs is a counted number; it is exact.

d The area is measured with a ruler or tape measure; it is a measured number.

4.9C53.80C

0.250 lb130.3 mL  453.6 g

1 lb  0.870 g

mL24.0 g

20.0 mL  1.20 g/mL

d There are three significant figures in the width measurement.

e.

f Since there are three significant figures in the width and length measurements, there are three

significant figures in the area

2.78 a Length is 3.7 cm; the 7 is the estimated digit.

b Length is 2.50 cm; the 0 is the estimated digit.

c Length is 4.10 cm; the 0 is the estimated digit.

2.79 The volume of the object is: The mass is 8.24 g and the density is:

2.80 a This is cube 3, since it has sunk to the bottom.

b This is cube 4, since it is floating about one-third out of the water.

c This is cube 1, since it is floating about one-half out of the water.

d This is cube 2, since it is floating just at the surface of the water.

2.81 A is vegetable oil, B is water, and C is mercury.

2.82 A would be gold; it has the highest density and the smallest volume.

B would be silver; its density is intermediate and the volume is intermediate.

C would be aluminum; it has the lowest density and the largest volume.

2.83 a Drop 8 and increase retained digits by 1 to give 0.000 0126 L

b Drop 8 and increase retained digits by 1 to give

c Drop 111, keep retained digits, and add three zeros as placeholders to give ,

or

d Drop 03 and keep retained digits to give 58.7 m.

e Add 2 significant zeros to give

f Drop 26 and keep retained digits, 0.0108 g.

2.84 265 g 2.85

8.0 oz  6 crackers

0.50 oz  96 crackersPlan: oz : crackers

3.00 10
3 s1.25 105 m3

125 000 m33.53 102 kg

(1.26 10
5 L)

8.24 g4.6 mL  1.8 g/mL23.1 mL
18.5 mL  4.6 mL33.3 cm2

2.97 The difference between the initial volume of the water and its volume with the lead object will

give us the volume of the object

Using the density of lead, we can convert mL to the mass in grams of the lead object

Plan: L gas : mL gas : g gas : g oil : mL oil : cm3 oil

155 mL water 1.91 mL iron  1.77 mL lead  159 mL total volume

16 oz  453.6 g

1 lb  0.761 g/mL442.5 mL total
325.2 mL water  117.3 mL object

2.101 a.

b.

2.102 5.77 kg 2.103

2.104

2.105 Since the balance can measure mass to 0.001 g, the mass should be given to 0.001 g; you should

record the mass of the object as 34.075 g

2.106 The student who reports 5.8 cm is not reading to the nearest mm The others are estimating

differently

2.107 6.4 gal 2.108 a 79 cups b 314 cans c 157 tablets 2.109

2.111 a 43 g b 3.9 g copper c.

2.112 0.203 mm 2.113 75.7 mL 4.8 mL (silver)  2.6 mL (gold)  82.9 mL

2.8 cm3

6.9 104 kg

69 m33.8 102 g aluminum

3.0 L fat  1000 mL

1 L  0.94 g fat

1 mL fat  1 lb

453.6 g  6.2 lb fatPlan: L fat : mL : g : lb

45 kg body weight  3.0 kg fat

100.0 kg body mass  2.205 lb

1 kg  3.0 lb fatPlan: kg mass : kg fat : lb (percent equality: 100.0 kg mass 3.0 kg fat)

Matter and Energy

3.1 A pure substance has a definite composition A mixture has a variable composition.

a pure substance b mixture

c pure substance d pure substance 3.2 a mixture b pure substance

c mixture d pure substance 3.3 Elements are the simplest type of pure substance Compounds contain two or more elements in the

form composition throughout the mixture

a heterogeneous b homogeneous

c homogeneous d heterogeneous 3.6 a homogeneous b heterogeneous

c homogeneous d heterogeneous 3.7 a Color is a physical property.

b The ability of hydrogen to react with oxygen is a chemical property.

c The temperature at which a substance freezes is a physical property.

d The change in milk left in a warm room is a chemical property.

3.8 a physical property b chemical property

c chemical property d physical property 3.9 a The change of water from gas to liquid is a physical change.

b The reaction of cesium with water is a chemical change.

c The melting of gold from solid to liquid is a physical change.

d The change in shape is a physical change.

e Dissolving sugar in water only separates the sugar molecules: it is a physical change.

3.10 a physical change b chemical change

c physical change d chemical change

e physical change

3.11 a The reactivity of a substance is a chemical property.

b The state of a substance is a physical property.

c The color of a substance is a physical property.

d The reaction with hydrogen is a chemical property.

e The temperature at which a substance melts is a physical property.

3.12 a physical property b chemical property

c physical property d chemical property

e physical property

3.13 The Fahrenheit temperature scale is still used in the United States A normal body temperature is

on this scale To convert her temperature to the equivalent reading on the Celsius scale, thefollowing calculation must be performed:

Because a normal body temperature is her temperature of would be a mild fever

3.14 Because Mexico uses the Celsius temperature scale, he is accustomed to setting the oven’s

temper-ature in Celsius degrees I would advise him that ovens in the United States are calibrated inFahrenheit degrees and that we would need to determine the equivalent of on the Fahrenheitscale, as follows:

We would set the oven to 350°F and watch the cooking time carefully

3.15 In temperature calculations, the number of significant figures is determined by the measured

tem-perature The values of 32 and 1.8 are exact

3.19 At the top of the hill, the energy of the car is in the form of potential energy As it descends,

po-tential energy is converted to kinetic energy When the car reaches the bottom, all its energy is netic energy

ki-3.20 As the elevator moves to the top of the ramp, the skier’s potential energy increases As the skier

goes down the ramp (ski jump), potential energy is converted to kinetic energy

3.21 a potential; stored energy b kinetic; energy of motion

c potential; stored energy d potential; energy of motion

1.8 (175
C)  32  347
F

175
C

37.7
C37.0
C,

(99.8
F  32)1.8  37.7
C98.6
F

3.22 a potential b potential c kinetic d kinetic 3.23 a Using a hair dryer converts electrical energy into heat energy (the air is warmed) and

mechanical energy

b Using a fan converts electrical energy into mechanical energy.

c Burning gasoline converts chemical energy into mechanical energy as the car is propelled

down the road and heat energy as the engine warms up

d Radiant energy is converted into heat energy by the solar water heater.

3.24 a Electrical energy becomes radiant and heat energies when the filament glows.

b Burning gas converts chemical energy into radiant and heat energies.

c Electrical energy is converted into heat energy.

d The chemical energy of the log is converted into radiant and heat energies.

3.25 a (2) light bulb

b (3) hydroelectric power plant

c (1) heater 3.26 a (3) ceiling fan

b (2) automobile engineering plant

c (1) battery 3.27 a.

3.29 Copper, which has the lowest specific heat, would reach the highest temperature.

3.30 Because the final temperature of B is lower, that means that B has a higher specific heat.

3.31 a.

b.

3.33 The heat required is given by the relationship: Heat

If heat is added, q is if heat is lost q is

0.325 kJ

8100 cal

1 cal4.184 J  1100 cal

 1000 J

1 kJ 4.5 kJ

415 J

 1 kcal

1000 cal  3.5 kcal

3500 cal

3.40 To calculate heat, we need the mass of the water, its specific heat, and the temperature change.

Then divide the heat energy absorbed by the water (which is equivalent to the energy released bythe combustion of fuel) by the grams of octane burned, as follows:

 11.5 kcal/g48.1 kJ/g

121
C55.3
C

m  SH 

6.75 kJ50.0 g  0.385 J/g
C 

m  SH 

7.10 kJ150.0 g 4.184 J/g
C 

31.6 g15.1 g

113 g26.6 g

T  SH 

14 200 J(42
C  185
C)  0.523 J/g
C 

225 J32.0
C  0.129 J/g
C  54.5 g

3.41 a Because the orange juice contains both carbohydrate and protein, two calculations will be

needed:

b.

c.

d Three calculations are needed:

3.42 a Three calculations are needed:

4.184 kJ  932 kcal  930 kcal (rounded)

 3900 kJ (rounded to tens place)Total: 1156 kJ  2550 kJ  190 kJ  3896 kJ (not rounded)

All values are rounded to the tens place.

c With just carbohydrate present, only a single calculation is required

d.

3.44 a is a homogeneous mixture because it has the same properties throughout.

3.45 b and c are heterogeneous mixtures because they are not the same throughout the mixture.

3.46 a homogeneous b heterogeneous c heterogeneous

d homogeneous e heterogeneous f homogeneous 3.47 gold 250 J or 59 cal; aluminum 240 J or 58 cal; silver 250 J or 59 cal

The heat needed for samples of the metals is almost the same

kcal for total mealsleeping

b running

d element e mixture 3.50 a heterogeneous b homogeneous c homogeneous

d heterogeneous e homogeneous

3.51 a Appearance is a physical property.

b The melting point of gold is a physical property.

c The ability of gold to conduct electricity is a physical property.

d The ability of gold to form a new substance with sulfur is a chemical property.

3.52 a physical property b chemical property

c physical property d physical property

3.53 a Plant growth is a chemical change

b A change of state from liquid to solid is a physical change.

c Chopping wood into smaller pieces is a physical change.

d Burning wood, which forms new substances, is a chemical change

1090 kcal 1 hr/750 kcal  1.5 hr running

750 kcal/hr

1090 kcal 1 hr/60 kcal  18 hr sleeping

60 kcal/hr

 1090 kcal(11 g  60 g)  4 kcal/g  280 kcal  (9  9  80 kcal)

(3 g(31 g 29 g)  4 kcal/g  130 kcal  (11  9  100 kcal) 34)  4 kcal/g  260 kcal  (29  9  260 kcal)10.0 cm3

880 kJ 1 kcal

4.184 kJ  210 kcal

 880 kJTotal 881 kJ

3.54 a physical change b physical change

c chemical change d chemical change 3.55 a Tablets are solid b Helium in a balloon is a gas c Milk is a liquid.

d Air is a mixture of gases e Charcoal is a solid.

3.59 3.60 3.61 3500 kcal 3.62 This question requires three calculations to obtain the total kcal.

3.63 Water has a higher specific heat than sand, which means that a large amount of energy is required

to cause a significant temperature change Even a small amount of energy will cause a significanttemperature change in the sand

8400 kJ 1000 J

1 kJ  8 400 000 J

18.9 kJ0.50 g oil  1000 J

3.71 The heat lost by the water is equal to the heat gained by the copper, for both:

For water:

For copper:

3.72 The meal contains a total of 21 g protein, a total of 38 g fat, and a total of 124 g carbohydrate The

total caloric content of the meal must be determined to answer the question

Using Table 3.11, 1.8 hr of swimming are needed to “burn off ” the caloric content of the meal

3.73 a 45 g protein, 140 g carbohydrate, 53 g fat

b 71 g protein, 210 g carbohydrate, 84 g fat

c 98 g protein, 290 g carbohydrate, 120 g fat 3.74

3.75 a 26.5 g b 54.5 g

Answers to Combining Ideas Chapters 1–3

CI 1 a five significant figures

1670 J62.0
C  0.385 J/g
C50.0 g 8.0
C  4.184 J/g
C  1670 J (not rounded)q  m  T  SH  50.0 g  (24.0
C  16.0
C)  4.184 J/g
C 

CI 2 a 330 km

b $15.50

c 4.6 hr (4 hr 40 min) d.

(15.6
F  32)1.8  9.11
C17.6 mL water 5.8 mL nails  23.4 mL new volume level

Heat m  SH  T  9147.5 g  0.129 Jg
C  7
C  1 kJ

1000 J  8 kJ

T  29  22  7
C

T  (85  32)
1.8  29
C T (72  32)/1.8  22
C

4.3 a carbon b chlorine c iodine d mercury

e fluorine f argon g zinc h nickel 4.4 a helium b phosphorus c sodium d magnesium

e calcium f bromine g cadmium h silicon 4.5 a sodium (Na) and chlorine (Cl)

b calcium (Ca), sulfur (S), and oxygen (O)

c carbon (C), hydrogen (H), chlorine (Cl), nitrogen (N), and oxygen (O)

d calcium (Ca), carbon (C), and oxygen (O) 4.6 a hydrogen (H) and oxygen (O)

b sodium (Na), hydrogen (H), carbon (C), and oxygen (O)

c sodium (Na), oxygen (O), and hydrogen (H)

d carbon (C), hydrogen (H), and oxygen (O) 4.7 a C, N, and O are in Period 2.

b He is the element at the top of Group 8A (18).

c The alkali metals are the elements in Group 1A (1).

d Period 2 is the horizontal row of elements that ends with neon (Ne).

4.8 a Group 1A (1) b Period 2 c Group 8A (18) d Group 7A (17) 4.9 a alkaline earth metal b transition element c. noble gas

d alkali metal e halogen 4.10 a noble gas b alkaline earth metal c transition element

d halogen e alkaline earth metal 4.11 a C b He c Na d Ca e Al

4.13 On the periodic table, metals are located to the left of the heavy zigzag line, nonmetals are elements

to the right, and metalloids (B, Si, Ge, As, Sb, Te, Po, and At) are located along the line

e nonmetal f nonmetal g metalloid h metal

e nonmetal f nonmetal g nonmetal h metal 4.15 a electron b proton c electron d neutron 4.16 a neutron b proton and neutron c electron d electron 4.17 Rutherford determined that the two most massive subatomic particles, protons and neutrons, are

located in a very small, central region of the atom called the nucleus

4.18 Because protons are present in the nucleus of every element and protons are the positively charged

b number of particles (protons plus neutrons) in the nucleus

c number of neutrons

d nothing useful 4.25 a lithium, Li b fluorine, F c calcium, Ca d zinc, Zn

e neon, Ne f silicon, Si g iodine, I h oxygen, O 4.26 a hydrogen, H b sodium, Na c potassium, K d iron, Fe

e bromine, Br f silver, Ag g phosphorus, P h helium, He

4.29

of Element Symbol Number Number of Protons Neutrons Electrons

of Element Symbol Number Number of Protons Neutrons Electrons

4.31 a Because the atomic number of aluminum is 13, every Al atom has 13 protons An atom of

alu-minum (mass number 27) has 14 neutrons Neutral atoms have the samenumber of protons and electrons: 13 protons, 14 neutrons, and 13 electrons

(27
13  14 n)

b Because the atomic number of chromium is 24, every Cr atom has 24 protons An atom of

chromium (mass number 52) has 28 neutrons Neutral atoms have the samenumber of protons and electrons: 24 protons, 28 neutrons, and 24 electrons

c Because the atomic number of sulfur is 16, every S atom has 16 protons An atom of sulfur

(mass number 34) has 18 neutrons Neutral atoms have the same number ofprotons and electrons: 16 protons, 18 neutrons, and 16 electrons

d Because the atomic number of iron is 26, every Fe atom has 26 protons An atom of iron (mass

number 56) has 30 neutrons Neutral atoms have the same number of protonsand electrons: 26 protons, 30 neutrons, and 26 electrons

4.32 a 1 proton, 1 neutron, 1 electron

b 7 protons, 7 neutrons, 7 electrons

c 14 protons, 12 neutrons, 14 electrons

d 30 protons, 40 neutrons, 30 electrons

4.35 a.

b They all have the same atomic number (the same number of protons and electrons).

c They have different numbers of neutrons, which is reflected in their mass numbers.

d The atomic mass of sulfur on the periodic table is the average atomic mass of all the naturally

occurring isotopes of sulfur

4.36 a.

b They all have the same atomic number (the same number of protons and electrons).

c They have different numbers of neutrons, which is reflected in their mass numbers.

d The atomic mass of strontium on the periodic table is the average atomic mass of all the

natu-rally occurring isotopes of strontium

4.37 The mass of an isotope is the mass of an individual atom The atomic mass is the weighted

aver-age of all the naturally occurring isotopes of that element

4.38 The mass number gives the number of protons and neutrons in an atom; the atomic number gives

the number of protons

4.39 Because the atomic mass of copper is closer to 63 amu, there are more atoms of

4.40 The mass of F on the periodic table should be very close to 19 amu.

4.41 Because the atomic mass of iron is 55.85 amu, the most abundant isotope is

4.42 The atomic mass of Zn is the weighted average of the masses of the five isotopes.

4.43 4.44 63.55 amu 4.45 The electrons surrounding a nucleus have specific energies Electrons with similar energies will

be found grouped together within a specific energy level

4.46 The first energy level is filled with 2 electrons The second energy level can hold a maximum of 8

electrons Because we are only considering the first 20 elements, the third energy level will have 8electrons and the fourth energy level will have only 2 electrons in it

(52
24  28 n)

4.49 a 2, 4 b 2, 8, 8 c 2, 8, 6 d 2, 8, 4 e 2, 8, 3 f 2, 5 4.50 a 2, 8, 5 b 2, 8 c 2, 6 d 2, 8, 8 e 2, 8, 3 f 2, 8, 4

4.53 a boron, B: 2, 3 aluminum: 2, 8, 3 b 3 c Group 3A (13) 4.54 a fluorine, F: 2, 7 chlorine: 2, 8, 7 b 7 c Group 7A (17) 4.55 a. , Group 2A (2) b. , Group 7A (17) c. , Group 6A (16)

4.56 a. , Group 1A (1) b. , Group 4A (14) c. , Group 8A (18)

4.57 The number of dots is equal to the number of valence electrons as indicated by the group number.

a Sulfur has 6 valence electrons Group 6A (16)

b Nitrogen has 5 valence electrons Group 5A (15)

c Calcium has 2 valence electrons Group 2A (2)

d Sodium has 1 valence electron Group 1A (1)

e Potassium has 1 valence electron Group 1A (1)

4.58 a 4A (14), b 6A (16), c 7A (17),

d 1A (1), e 7A (17),

4.61 Alkali metals are members of Group 1A (1), and each has 1 valence electron.

4.62 Halogens are members of Group 7A (17), and each has 7 valence electrons.

4.63 a The ionization energy decreases going down a group: Br, Cl, F

b Going across a period from left to right, the ionization energy generally increases: Na, Al, Cl

c The ionization energy decreases going down a group: Cs, K, Na 4.64 a C, O, N b S, P, Cl c As, P, N

4.65 a Br, which is above I in Group 7A (17), has a higher ionization energy than I.

b Al has a higher ionization energy than K because ionization energy increases going left to right

and decreases going down a group

c P has a higher ionization energy than Si because ionization energy increases going left to right

across a period

4.67 a false b true c true d false

4.68 a X is Cl, chlorine This isotope has 17 protons and 20 neutrons.

b X is Fe, iron This isotope has 26 protons and 30 neutrons.

c X is Sn, tin This isotope has 50 protons and 66 neutrons.

d X is Sn, tin This isotope has 50 protons and 74 neutrons.

e X is Cd, cadmium This isotope has 48 protons and 68 neutrons

c and d are both isotopes of Sn, tin.

NmNm

MM

ClLi

FO

C

KNaCaNS

4.69 a Both have 20 neutrons.

b Both have 16 protons.

c Not the same.

d Both have 22 neutrons.

4.70

The atoms b and d are isotopes of boron; c and e are isotopes of carbon

4.72 a metal b metalloid c nonmetal d metalloid e nonmetal 4.73 a 3, Li b 86, Rn c 24.31, Mg d 19.00, F

4.74 a 32, Ge b 83, Bi c 39.10 amu, K d 210, At 4.75 Any element with a two-letter symbol has the first letter capitalized and the second letter in lower-

case CO would indicate a compound made of the two elements carbon and oxygen

4.76 a Incorrect The symbol for copper is Cu b Incorrect The symbol for silicon is Si.

c Correct as written d Incorrect The symbol for fluorine is F.

e Incorrect The symbol for potassium is K f Correct as written.

g Correct as written h Incorrect The symbol for lead is Pb 4.77 a Mg, magnesium b Br, bromine c Al, aluminum d O, oxygen 4.78 a Group 1A (1), Period 4 b Group 5A (15), Period 3

c Group 4A (14), Period 2 d Group 8A (18), Period 2 4.79 Any two of the following in each part are correct responses:

a Group 7A (17), fluorine, chlorine, bromine, iodine, or astatine

b Group 8A (18), helium, neon, argon, krypton, xenon, or radon

c Group 1A (1), lithium, sodium, potassium, rubidium, cesium, or francium, but not hydrogen

d Group 2A (2), beryllium, magnesium, calcium, strontium, barium, or radium 4.80 a metal b metal c metal

d nonmetal e metal f nonmetal 4.81 a False A proton has a positive charge.

b False The neutron has about the same mass as a proton.

c True

d False The nucleus is the tiny, dense, central core of an atom.

e True 4.82 a True

b True

c False The charge of the electron is equal but opposite to the charge of the proton.

d False The proton and the neutron have about the same mass.

e False The atomic number is the number of protons.

4.83 a protons b protons c alkali metals 4.84 a mass b halogens c metals

12

6C10

5B13

6C11

4.85 a lithium, Li b fluorine, F c calcium, Ca d arsenic, As

e tin, Sn f cesium, Cs g gold, Au h oxygen, O 4.86 a hydrogen, H b sodium, Na c chromium, Cr d iron, Fe

e bromine, Br f silver, Ag g bismuth, Bi h uranium, U 4.87 a 25 protons, 25 electrons b 30 protons, 30 electrons

c 53 protons, 53 electrons d 12 protons, 12 electrons

e 19 protons, 19 electrons 4.88 a 6 protons, 6 electrons b 20 protons, 20 electrons

c 27 protons, 27 electrons d 17 protons, 17 electrons

e 48 protons, 48 electrons 4.89 a 13 protons, 14 neutrons, 13 electrons

b 24 protons, 28 neutrons, 24 electrons

c 16 protons, 18 neutrons, 16 electrons

d 26 protons, 30 neutrons, 26 electrons

e 54 protons, 82 neutrons, 54 electrons 4.90 a 10 protons, 12 neutrons, 10 electrons

b 53 protons, 74 neutrons, 53 electrons

c 35 protons, 40 neutrons, 35 electrons

d 55 protons, 78 neutrons, 55 electrons

e 78 protons, 117 neutrons, 78 electrons

4.94 Nuclear Number of Number of Number of

Name Symbol Protons Neutrons Electrons

4.96 No The atomic mass is the weighted average of the eight naturally occurring isotopic masses.

Both have mass number of 18

d. 16 18X Both have 8 neutrons

8X

18

8X17

8X16

8X

18

8X17

8X16

8X

51Cr

51Fe

4.98 a.

b All these isotopes contain 30 protons and 30 electrons Zinc-64 contains 34 neutrons, zinc-66

contains 36 neutrons, zinc-67 contains 37 neutrons, zinc-68 contains 38 neutrons, and zinc-70contains 40 neutrons

4.99 a 82 protons, 126 neutrons, 82 electrons b.

c. , bismuth

4.100 a 47 protons, 60 neutrons, 47 electrons b.

c. , cadmium

4.101 a N, Group 5A (15), electron arrangement 2, 5

b Na, Group 1A (1) electron arrangement 2, 8, 1

c S, Group 6A (16), electron arrangement 2, 8, 6

d B, Group 3A (13), electron arrangement 2, 3

4.102 a C, Group 4A (14), electron arrangement 2, 4

b Si, Group 4A (14), electron arrangement 2, 8, 4

c P, Group 5A (15), electron arrangement 2, 8, 5

d Ar, Group 8A (158), electron arrangement 2, 8, 8

4.103 Calcium has a greater net nuclear charge than K The least tightly bound electron in Ca is further

from the nucleus than in Mg and needs less energy to remove

4.104 The least tightly bound electron in Cl is further from the nucleus than in F and needs less energy

to remove Chlorine has 7 protons and sulfur has 6, so it is easier to remove the valence electronfrom sulfur

4.105 a Na is on the far left of the heavy zigzag line Na is a metal.

b F at the top of Group 7A (17) and to the far right in Period 2 has the highest ionization energy.

c Na has the lowest ionization energy and loses an electron most easily.

d Cl is found in Period 3 in Group 7A (17).

4.107 4.108

4.109

4.110

M121 120.89 amu42.70 / 100 122.90 amu  57.30 /100  M121 121.75 amu

 52.40/100  207.98 amu  207.22 amu1.40 / 100 203.97 amu  24.10 /100  205.97 amu  22.10/100  206.98 amu

ArPSiCBSNaN

Names and Formulas of Compounds

5.1 a When a sodium atom loses its valence electron, its second energy level has a complete octet.

b Group 1A (1) and 2A (2) elements can lose 1 or 2 electrons to attain a noble gas arrangement.

Group 8A (18) elements already have an octet of valence electrons, so they do not lose or gainelectrons and are not normally found in compounds

5.2 a When a chlorine atom gains a valence electron, its third energy level has a complete octet.

b Group 7A (17) elements can gain 1 electron to attain a noble gas arrangement Group 8A (18)

elements already have an octet of valence electrons, so they do not lose or gain electrons andare not normally found in compounds

5.3 Atoms with 1, 2, or 3 valence electrons lose those electrons to form ions

a. has an electron arrangement 2, 8, which is the same as neon (Ne)

b. has an electron arrangement 2, 8, which is the same as neon (Ne)

c. has an electron arrangement 2, 8, 8, which is the same as argon (Ar)

d. has an electron arrangement 2, 8, which is the same as neon (Ne)

e. has an electron arrangement 2, 8, which is the same as neon (Ne)

5.7 Atoms form ions by losing or gaining electrons to achieve the same electron arrangement of theirnearest noble gas Elements in Groups 1A (1), 2A (2), and 3A (13) lose valence electrons,whereas elements in Groups 5A (15), 6A (16), and 7A (17) gain valence electrons to completeoctets

a Mg loses 2 b P gains 3 c Group 7A (17) gains 1

5.10 a 8 protons, 10 electrons b 19 protons, 18 electrons

c 35 protons, 36 electrons d 16 protons, 18 electrons

e 38 protons, 36 electrons 5.11 A metal and a nonmetal are most likely to form an ionic compound.

a (Li and Cl) and c (K and O) would form ionic compounds.

5.12 b (Mg and Cl) and d (K and S) will form ionic compounds.

5.13 a Potassium loses 1 , and chlorine gains 1

b Calcium loses 2 , and two chlorine atoms each gain 1

c Each of three sodium atoms lose 1 , and the nitrogen gains 3

5.19 a Chlorine in Group 7A (17) gains 1 electron to form chloride ion

b Potassium in Group 1A (1) loses 1 electron to form potassium ion

c Oxygen in Group 6A (16) gains 2 electrons to form oxide ion

d Aluminum in Group 1A (1) loses 3 electrons to form aluminum ion

5.21 a potassium ion b sulfide ion c calcium ion d nitride ion 5.22 a magnesium b barium c iodide d chloride 5.23 In the name for an ionic compound, the metal ion is named first followed by the nonmetal ion

name ending in ide.

a Ions: aluminum and oxide

b Ions: calcium and chloride

c Ions: sodium Na
and oxideO2  : sodium oxide

CaCl2

 2(
)
1(2)  0

O2

2Li
Ions: Li
and O2 : Li2O

 1(3
)
3(1)  0

I

Al3
Ions: A13
and I : AlI3

 3(
)
1(3)  0

N3

3K
Ions: K
and N3 :K3N

 2(
)
1(2)  0

S2 2Na

Ions: Na
and S2  :Na2S

K3N

Li2SAlCl3

 2(3
)
3(2)  03S2 

2Al3

Al2S3

 1(2
)
2(1)  02Cl

AlBr3

 2(
)
1(2)  0

O2 2Na

d Ions: magnesium and nitride

e Ions: potassium and iodide

f Ions: barium and fluoride

5.24 a magnesium chloride b potassium phosphide c lithium sulfide

d lithium bromide e magnesium oxide f strontium bromide 5.25 A Roman numeral is used to specify the positive charge on the transition metal in the compound,

when that transition metal can have more than one cation

5.26 Because calcium ion only has a charge, the name calcium is sufficient However, copper ionscan have either a or a charge, which requires a Roman numeral to indicate which copperion is present

5.27 a iron(II) b copper(II) c zinc

d lead(IV) e chromium(III) f manganese(II) 5.28 a silver b copper(I) c iron(III)

d tin(II) e gold(III) f nickel(II) 5.29 For metal ions with variable charge, determine the ionic charge and use it as a Roman numeral

following the name of the metal

5.30 a silver phosphide b lead(II) sulfide c tin(IV) oxide

d gold(III) chloride e chromium(III) oxide f cobalt(II) sulfide 5.31 a.

5.37 The most common forms of negatively charged polyatomic ions end in ate; one O less end in ite.

A hydrogen in front is named as hydrogen or bi.

a bicarbonate b ammonium c phosphate

d hydrogen sulfate e hypochlorite

5.39 a sulfate b carbonate c phosphate d nitrate e perchlorate

5.40 a hydroxide b hydrogen sulfite (or bisulfite) c cyanide d nitrite

e chromate 5.41

HCO3

Ba3(PO4)2Ba(HSO4)2

BaCO3Ba(NO2)2

Ba 2

Cu3(PO4)2Cu(HSO4)2

CuCO3Cu(NO2)2

Cu 2

Li3PO4LiHSO4

Li2CO3LiNO2

Pb(HPO4)2Pb(HCO3)4

Pb(NO3)4

Pb(SO3)2

Pb 4

Al2(HPO4)3Al(HCO3)3

5.43 a The polyatomic ion is the compound is sodium carbonate

b The polyatomic ion is the compound is ammonium chloride

c The polyatomic ion is the compound is lithium phosphate

d The polyatomic ion is the compound is copper(II) nitrite

e The polyatomic ion is the compound is iron(II) sulfite

f The polyatomic ion is C2H3O2;the compound is potassium acetate

5.44 a. potassium hydroxide b. sodium nitrate

c. copper(II) carbonate

d. sodium hydrogen carbonate (or sodium bicarbonate)

5.45 Write the positive and negative ions Then use charge balance to write the formula.

5.47 a This is an ionic compound with ion and the sulfate polyatomic ion The correct

name is aluminum sulfate

b This is an ionic compound with ion and the carbonate polyatomic ion The correctname is calcium carbonate

c This is an ionic compound with and Because chromium has variable valences, aRoman numeral is used to indicate the charge The correct name is chromium(III) oxide

d This is an ionic compound with sodium ion and the polyatomic ion The correctname is sodium phosphate

e This ionic compound contains two polyatomic ions, ammonium and sulfate It isnamed ammonium sulfate

f This is an ionic compound containing the variable metal ion and oxide ion It isnamed using the Roman numeral as iron(III) oxide

5.48 a cobalt(III) phosphate b magnesium phosphate

c iron(II) sulfate d magnesium sulfate

e copper(I) oxide f tin(II) fluoride 5.49 The nonmetallic elements that are not noble gases are likely to form covalent bonds.

5.50 A bond forms between Na and Cl when an electron is lost by Na and gained by Cl.

The bond that forms is an ionic bond A bond forms between N and Cl when a pair of electrons,one from each atom, is shared between the two atoms The bond that formed is a covalent bond

5.51 a When two H atoms share, each has 2 valence electrons In there is 1 bonding pair and no

lone pair

b The Br atom achieves an octet by sharing a valence electron with one H atom to give 8 valence

electrons, 1 bonding pair, and 3 lone pairs on the Br atom

c Each Br atom achieves an octet by sharing 1 valence electron to give a total of 14 valence

electrons, 1 bonding pair between the Br atoms, and 6 lone pairs (3 lone pairs for each Br atom)

5.52 a 8 valence electrons, 2 bonding pairs, and 2 lone pairs

b 8 valence electrons, 3 bonding pairs, and 1 lone pair

c 20 valence electrons, 2 bonding pairs, and 8 lone pairs 5.53 When naming covalent compounds, prefixes are used to indicate the number of each atom as

shown in the subscripts of the formula The first nonmetal is named the same as the element; the

second nonmetal changes the ending of the element name to ide.

a one phosphorus atom and three (tri) bromine atoms; phosphorus tribromide

b one carbon atom and four (tetra) bromine atoms; carbon tetrabromide

c one silicon atom and two oxygen atoms; silicon dioxide

d one hydrogen atom and one fluorine atom; hydrogen fluoride

e one nitrogen atom and three (tri) iodine atoms; nitrogen triiodide

Mg(HCO3)2(NH4)2O

Al(ClO3)3

3CO32 : Fe2(CO3)32Fe3

2PO43 : Zn3(PO4)23Zn2

2NO3 : Fe(NO3)2

Fe2

SO42 : Na2SO42Na

2OH : Ba(OH)2

Ba2

ClO;

SO42;HCO3;

CO32;

NO3;

OH;

5.54 a carbon disulfide b diphosphorus pentoxide c dichlorine oxide

d phosphorus trichloride e dinitrogen tetroxide 5.55 When naming covalent compounds, prefixes are used to indicate the number of each atom as

shown in the subscripts of the formula The first nonmetal is named the same as the element; the

second nonmetal changes the ending of the element name to ide.

a two (di) nitrogen atoms and three (tri) oxygen atoms; dinitrogen trioxide

b one nitrogen atom and three (tri) chlorine atoms; nitrogen trichloride

c one silicon atom and four (tetra) bromine atoms; silicon tetrabromide

d one phosphorus atom and five (penta) chlorine atoms; phosphorus pentachloride

e one sulfur atom and three (tri) oxygen atoms; sulfur trioxide 5.56 a silicon tetrafluoride b iodine tribromide c carbon dioxide

d sulfur dioxide e dinitrogen oxide 5.57 The prefixes in the names of covalent compounds indicate the number of each type of atom, which

is placed as a subscript in the formula When there is no prefix there is one atom in the formula

a carbon (1C) and tetrachloride

b carbon (1C) and monoxide

c phosphorus (1P) and trichloride

d dinitrogen (2N) and tetroxide

5.59 The prefixes in the names of covalent compounds indicate the number of each type of atom, which

is placed as a subscript in the formula When there is no prefix, there is one atom in the formula

a oxygen (1O) and difluoride

b boron (1B) and trifluoride

c dinitrogen (2N) and trioxide

d sulfur (1S) and hexafluoride

5.61 a aluminum chloride b sulfur trioxide c dinitrogen oxide

d tin(II) nitrate e copper(II) chlorite 5.62 a nitrogen b magnesium hypobromite c silicon tetrafluoride

d nickel (II) sulfate e iron (III) sulfide 5.63 a 15 protons make it phosphorus; 18 electrons gives a charge of

b 8 protons and 8 electrons make it a neutral oxygen (O) atom.

c 30 protons make it zinc; 28 electrons gives a charge of

d 26 protons make it iron; 23 electrons gives a charge of 5.64 a X is in Group 1A (1); Y is in Group 6A (16) b ionic

(6F) SF6(3O) N2O3(3F) BF3(2F)  OF2

N2O

IF5SiCl4

SO2

 N2O4(4O)

(3Cl)  PCl3

 CO(1O)

 CCl4(4Cl)

Electron-dot Formula of Period Symbols Compound Name of Compound

5.68

5.69

5.70

Formula of Name of Electron Arrangements Electron-dot Symbols Compound Compound

Ca3P2P

Ca

Li2SS

Li