Chem 20 Review Section 1 Worksheets

Chapter 1 Checklist

• You should remember all these concepts and ideas from Science 10. Have you mastered the concepts, applications, and skills associated with the following items? Check them off when you are confident in your understanding.

• Make sure you review this sheet prior to the Review Unit Exam.

Knowledge

classify matter as pure and mixtures as homogeneous and heterogeneous (1.2)

interpret the periodic table of the elements (1.3)

use atomic theory to explain the periodic table (1.4)

classify elements and compounds, and know the properties of each class (1.3, 1.4)

explain and predict chemical formulas for and name ionic and molecular compounds, acids, and bases (1.5, 1.6)

identify the state of matter of substances (1.5, 1.6)

write chemical equations when given reactants and products (1.5, 1.6)

classify scientific knowledge as qualitative and quantitative, as observations and interpretations, and as empirical and theoretical (1.1)

STS

describe the natures of science and technology (1.1)

describe the application of some common chemicals (1.3, 1.5, 1.6)

Skills

use a textbook, a periodic table, and other references efficiently and effectively (1.1–1.6)

interpret and write laboratory reports (1.1, 1.2, 1.3, 1.4, 1.6)

select and use diagnostic tests (1.2, 1.3, 1.4, 1.5, 1.6)

Key Terms

1.1 science

technology

chemistry

observation

interpretation

empirical knowledge

theoretical knowledge

empirical hypothesis

empirical definition

generalization

scientific law

law of conservation of mass

1.2 matter

pure substance

mixture

heterogeneous mixture

homogeneous mixture

element

entity

atom

compound

chemical formula

1.3 periodic law

family

group

period

semi-metal

standard ambient temperature and pressure (SATP)

metal

nonmetal

alkali metal

alkaline-earth metal

halogen

noble gas

main group element

transition element

Chemistry 20 – Review Unit Page 1


1.4 theoretical hypothesis

theoretical definition

theory

mass number

atomic number

ion

monatomic ion

cation

anion

1.5 ionic compound

molecular compound

acid

base

neutral

aqueous solution

polyatomic ion

formula unit

empirical formula

hydrate

1.6 molecule

molecular formula

diatomic molecule

Chemistry 20 – REVIEW UNITAssignment – Changes in Matter / Energy and Matter

1. Classify each of the following as a physical, chemical or nuclear change. Also give evidence or reason for your answer.

Example Type of Change Evidence / Reason

1 Water freezes.

2 An egg is fried.

3 A cake is baked.

4 Concrete sets.

5 Air and gasoline are mixed.

6 Milk sours.

7 Air and gasoline are ignited.

8 An apple ripens.

9 Latex paint dries.

10 A light bulb is turned on.

11 Uranium changes to lead.

12 Salt melts ice on a road.

13 Dew forms on the grass.

14 Solar heat is produced in the sun.

15 Solar cells produce electricity.

16 Fluorescent lights are turned on.

17 Plants use sun energy to produce oxygen.

18 Dry ice is placed in water to form a fog.

19 You see the Northern Lights in the sky.

20 You eat food to gain energy.


2. Determine whether the following situations represent primarily kinetic or potential energy.

a) A moving car. _______________

b) Water held behind a dam. _______________

c) Food _______________

d) Electricity _______________

e) Sunlight travelling from the sun. _______________

f) A wound clock spring. _______________

g) A stick of dynamite. _______________

h) A charged car battery. _______________

3. What factors determine the kinetic energy of a moving object?

4. For the sketch of the period table below, label the table’s sections.

5. Highlite the characteristics of each of the following.

Metals Nonmetals Metalloids Noble Gases

Characteristics



Chemistry 20 – Matter, Energy and The Periodic TableClassification Assignment

1. For each type of matter, categorize the following as a:

• Pure substance – element• Pure substance – compound• Homogeneous mixture• Heterogeneous mixture

Matter Substance(s) Present Classification

1 Charcoal C

2 Table salt NaCl

3 Oxygen O2

4 Neon gas Ne

5 Sulfur trioxide SO3

6 Pure water H2O

7 Tap water H2O, minerals

8 Salt water H2O, NaCl

9 Sand SiO2

10 Glucose C6H12O6

11 Hydrochloric acid HCl

12 Brass Cu - Zn

13 Glass SiO2, Na2CO3, CaCO3

14 Aluminum can Al

15 Pizza varies

16Iron filings and powdered sulfur

Fe, S8

17 Blood lots of good stuff

18 Crude oil lots of good stuff

19 Alcohol and water C2H5OH, water


2. Define each of the following and give one example of each.

a) nonmetal

b) alloy

c) molecule

d) ionic compound

e) pure substance

f) noble gas

g) heterogeneous mixture

h) phase

i) ore

j) oxide

k) element

3. Describe how you could separate each of the following mixtures.

a) oil and vinegar

b) alcohol and water

c) iron fillings and salt

d) blood

e) sand and rocks


Chemistry 20 – Review UnitIsotopes and Atomic Mass

1. Isotopes of an element have an equal number of _____________ and ______________ but a different number of

________________.

2. The ______________________ of an element is equal to the number of protons located in its nucleus or the number of electrons surrounding the nucleus in a natural atom.

3. The protons and neutrons in an atom contribute most to the ____________________ of that particular element.

4. The number of __________________ in the nucleus of chlorine atoms may vary.

5. Atoms with the same number of protons but with a different number of neutrons in the nucleus are called

____________________.

6. The relative average mass of all naturally occuring isotopes of a particular element is called the

________________________.

7. Identify the following elements:

A. Atom A has 50 electrons.B. Atom B has a charge of 33+ on its nucleus.C. Atom C has 123 neutrons and 80 electrons.D. Atom D has 28 protons and 31 neutrons.

8. Fill out the chart below:

Symbol NameAtomic Number

Mass Number

Protons Neutrons Electrons

31P

carbon - 14

35 44 36

29 34 27

92 143


Chemistry 20 – Review UnitThe Structure of the Atom

Drawing Bohr Models of the Atom

For each of the elements listed in the abbreviated periodic table below, draw an energy level representation of the atom, showing the number of protons, neutrons and electrons in their respective energy levels.


1A

1

8A

2

2A 3A 4A 5A 6A 7A

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

Chemistry 20 – Review UnitThe Structure of the Atom

Drawing Bohr Models of Ions

For each of the elements listed in the abbreviated periodic table below, draw an energy level representation of the ion, showing the number of protons, neutrons and electrons in their respective energy levels.

1A

1

8A

2

2A 3A 4A 5A 6A 7A

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18


Chemistry 20 – Review Unit Subatomic Particles and the Structure of the Atom

1. The theory that all matter was composed of unbelievably small particles called atoms was proposed by the Greek philosophers and revived in 1804 by __________________________________.

2. The theory that an atom was a positively charged mass in which negatively charged electrons were embedded like raisins in a bun or plums in a

plum pudding was suggested in 1898 by ________________________________.

3. The Nuclear Model for atoms where electrons surrounded a small, massive nucleus was suggested in 1911 by ________________________________.

4. The theory that electrons move around the nucleus of an atom in specific energy levels and where the atom was pictured as a miniature solar system was proposed in 1913 by ______________________.

5. The present model of the atom in which electrons occupy probability regions called orbitals is known as the ________________________________ model.

6. The neutron was discovered by ____________________________. 7. A neutral atom contains an equal number of _____________ and_____________.

8. A small, but massive, structure in the center of an atom is called the _____________ consisting of _____________ and ______________.

9. The extranuclear region of the atom, which makes up most of the volume of the atom, is occupied by _________________________.

10. Nearly all of the mass of any atom is made up of ___________ and ____________.

11. The elements in the Periodic Table are arranged horizontally in order of increasing ___________________.

12. Each period, except the first, starts with the _____________________ family and ends with the ______________________ family.

13. The heavy “staircase” line on the Periodic Table divides the __________ from the _______________.

14. Vertical arrangements of elements in the periodic table are called ____________ or ____________. 15. Elements 4, 12, and 20 are closely related chemically. The name of this family is ___________ _________________. The name of one other

element from this family is _______________.

16. An unknown element is a colorless gas at room temperature. Upon heating with lithium no reaction occurs. The family of elements to which this unknown element belongs is _____________________.


17. A soft metal reacts vigorously with water to produce hydrogen gas, H2(g). This metal probably belongs to the ___________________________ family.

18. The most reactive metal is ____________ and the most reactive nonmetal is _________________.

19. The elements that make up the B groups on the Periodic Table are called the ___________________.


Chemistry 20 – Review Unit Naming Common Substances

Chemical Formula

s, l, g, aq

Name of Substancei, m, or a

Common Name or Use

1 sodium chloride table salt, rock salt

2 CaCO3 marble, limestone, chalk

3 sodium bisulfate Sani-flush

4 sodium hydroxide Drano, Easy-Off, caustic soda

5 CaO quicklime, lime

6 MgSO4 ⋅ 7 H2O Epsom salts

7 carbon dioxide dry ice, soda pop, fire extinguishers

8 acetic acid vinegar

9 carbon ---- charcoal, graphite, diamond, fuels

10 calcium sulfate plaster of Paris, gypsum (drywall)

11 Na2SiO3water glass (preserving eggs, fireproofing,

adhesive cement)

12 Ca(HCO3)2 hard water chemical

13 magnesium hydroxide milk of magnesia

14 potassium chloride potash, fertilizer

15 sodium thiosulfate pentahydrate photographic hypo, antichlor

16 sodium hypochlorite laundry bleach

17 Na2CO3 washing soda, soda ash, water softener

18 HCl (acid) muriatic acid, gastric juice

19 potassium nitrate saltpeter, preserving meats, gun powder

20 CuSO4 ⋅ 5 H2O bluestone

21 Mg ---- flashbulb wire

22 carbon and iron ---- steel alloys

Chemical Formula

s, l, g, aq


Common Name or Use


23 magnesium oxide magnesium tablets for dietary substances

24 KIpotassium or iodine tablets for dietary

supplement

25 H2SO4 car battery acid

26 silicon carbide ---- carborundum (adhesive)

27 Ca(OH)2 slaked lime

28 potassium hydroxide caustic potash

29 mercury in thermometers

30 S8 brimstone

31 carbon tetrachloride toxic cleaning and fire extinguisher fluid

32 NH4Cl dry cell batteries

33 NH4OH ---- ammonia cleanser

34 SiO2 ---- sand, rocks

35 zinc dry cell battery cases, galvanizing nails

36 boric acid eye wash

37 NH4NO3 fertilizer ingredient

38 ammonium sulfate fertilizer ingredient

39 NaClO3 weed killer

40 calcium chloride de-icer, wetting solution

41 I2 tincture of iodine in alcohol

42 KMnO4 aquarium fungicide

43 NaHSO3 yeast inhibitor

44 phosphoric acid rust remover

45 stannous fluoride once used as a toothpaste additive

Chemical Formula

s, l, g, aq


Common Name or Use

46 FeSO4 iron pills, dyes, inks

47 C2H5OH grain alcohol, rubbing alcohol


48 CH3OH wood alcohol, methyl hydrate

49 methane natural gas

50 sucrose table sugar

51 diphosphorous pentoxide fertilizer ingredient

52 NaHCO3 baking soda

53 lead and lead (IV) oxide ---- plates in car batteries

54 water best used solvent

55 W ---- light bulb filament

56 dinitrogen oxide laughing gas

57 Na2SO4 ⋅ 10 H2O in medicines

58 aluminum sulfate water clarifier

59 NaNO3 in fertilizers

60 aluminum hydroxide dye fixer, water clarifier


Chemistry 20 – Review UnitNaming Acids

Acid Formula Ionic Name Acid NameOxo or Binary

eg HCl(aq) hydrogen chloride hydrochloric acid

1 HCN(aq)

2 hydrogen bromide

3 HClO3(aq)

4 HNO3(aq)

5 permanganic acid

6 HNO2(aq)

7 HClO(aq)

8 sulfurous acid

9 H3BO3(aq)

10 hydrogen fluoride

11 CH3COOH(aq)

12 H2SO4(aq)

13 H2SO3(aq)

14 oxalic acid

15 phosphoric acid

16 stearic acid

17 H2CO3(aq)

18 hypochlorous acid

19 HClO4(aq)

20 hydrogen chromate

21 H2S(aq)

22 hydrogen benzoate

23 H2SiO3(aq)

24 HCN(aq)

25 oxous acid


Education

Chem 20 Review Section 1 Worksheets