snc 2d1: chemistry workbook - mr. reid's science...

SNC 2D1: Chemistry Workbook

Name:___________________________________

www.stamfordscience.orgTable of Contents

• Introduction

• Learning Goals

• Vocabulary Checklist

• Assessment Check List

• “Big Idea” Chemistry Project

• Module 1 – physical and chemical properties, pure substances and mixtures, atomic structure (Bohr-Rutherford model), valence electrons and ionic charges

• Module 2 – periodic table, ionic charges within families, bonding (ionic, polyatomic, molecular)

• Module 3 – chemical reactions, conservation of matter, balancing equations, types of chemical reactions, acids & bases

• Review

Grade 10 Academic Science (SNC 2D1)

Introduction to Chemistry

Welcome to Chemistry!

As we move forward through the chemistry unit, we will review concepts you covered ingrade 9, such as physical and chemical properties, pure substances, mixtures and chemical changes.

We will also touch on new topics such as: why chemicals react, characteristics of chemical reactions and how these reactions can be represented. We will also analyze various safety and environmental issues related to chemical reactions and how chemical reactions can be used to address environmental challenges.

Ensure that you take the time to learn the material, do the practice work, ask for help sooner rather than later and use the assessment checklist to ensure that all items that all assessments of your learning are completed and submitted.

Good Luck!

Grade 10 Academic Chemistry Student Learning Goals/Checklist

By the end of this strand, I will be able to:

￢ use appropriate terminology related to chemistry (see vocabulary checklist).

￢ describe the relationships between chemical formulae, composition and names of binary compounds.

￢ identify simple ionic compounds, polyatomic compounds, molecular compounds and acids using the periodic table and a list of common polyatomic ions and write the formulae.

￢ classify physical and chemical changes.

￢ describe the types of evidence that indicate chemical change.

￢ describe, on the basis of observation, the reactants in and the products of a variety of chemical reactions.

￢ investigate the law of conservation of mass in chemical reactions and account for any discrepancies.

￢ explain, using the law of conservation of mass and atomic theory, the rationale for balancing chemical equations.

￢ write word equations and balanced chemical equations for simple chemical reactions.

￢ construct molecular models to illustrate the structure of molecules in simple chemical reactions and produce diagrams of these models.

￢ investigate simple chemical reactions, including synthesis, decomposition, and displacement reactions and represent them using word equations and balanced chemical equations.

￢ describe how the pH scale is used to classify solutions as acidic, basic or neutral

￢ plan and conduct an inquiry to classify some common substances as acidic, basic or neutral.

￢ describe the process of acid-base neutralization.

￢ analyse, on the basis of research, various safety and environmental issues associated with chemical reactions and their reactants and products.

￢ analyse how an understanding of the properties of chemical substances and their reactions can be applied to solve environmental challenges.

Grade 10 Academic Chemistry Vocabulary Checklist

By the end of this strand, these words/phrases should be familiar to you. Review your notes or stamfordscience.org for definitions.

□ atom□ balanced chemical equation□ chemical change□ chemical equation□ coefficient□ compound□ diatomic molecule□ electron□ element□ ion□ ionic compound□ law of conservation of mass□ matter□ metal□ molecular compound□ molecule□ multivalent element□ non-metal□ polyatomic ion□ product□ reactant□ shell□ skeleton equation□ state□ word equation

□ acid□ acid leaching□ acid precipitation□ acid-base indicator□ base□ neutral□ neutralization□ pH scale□ precipitate□ universal indicator

□ combustion□ decomposition reaction□ double displacement reaction□ fossil fuel□ hydrocarbon□ single displacement reaction□ synthesis reaction

Assessment Checklist

Throughout this course, we will use various assessment methods to provide “formative assessment”. That is, assessment FOR and AS learning. These are used to provide feedback and self reflection to improve your learning and understanding.

However, some items are used as an assessment OF your learning. These are listed in the chart below. You should keep track of these items and ensure that all of them are completed and submitted on time according to the class expectations (see first day handout).

Item Keep inWorkbookor Hand-in

TotalMarks

DueDate

YourMark

Household Substances Book 5

Density Worksheets Book 4

Bohr Diagrams and Ionic Charges Book 4

Overall completion of Module 1 Book 4

Alien Periodic Table Hand-in 10

Ionic Charges and Chemical Families Book 6

Nomenclature Quiz Hand-in 11

Lab: Testing Ions Hand-In 10

Bonding Gizmo (Ionic or Covalent) Hand-In 8


Lab: Conservation of Mass Hand-In 8

Lab: Synthesis and Decomposition Rx Hand-In 8

Lab: Single and Double Displacement Rx Hand-In 8

PH Gizmo Hand-In 8

Lab: Acids and Bases Hand-In 8


Big Idea Chemistry Project Hand-In TBD

Unit Test ------ TBD

“Big Idea” Chemistry Project

Using one of the topics listed below, you must address the following points:

• What is the concern/issue/problem?• How has chemistry/science contributed to this issue?• How have other factors have contributed to this issue?• What are the long term environmental impacts?• What are some possible solutions?• How can chemistry/science help with these solutions?

The format for this report can be:

• a website www.weebly.com or www.wikispaces.com• a cartoon interview with a scientist www.xtranormal.com • a presimodo presentation www.presimodo.com• a power-point presentation• a double spaced typed written report (2-3 pages)• a “bristol-board” presentation

You may use one of the topics from the list. If you wish to do a different topic, you must get prior approval early in the unit.

• Acid Precipitation

• Ocean Acidification

• Keystone Pipeline and/or Northern Gateway Pipeline Controversy

• Oil spills in water ways (oceans, seas, etc)...think ocean tankers or offshore drilling

• Nanotechnology

• Smokestack emissions

A list of cited resources must also be included!!

http://www.weebly.com/

http://www.presimodo.com/

http://www.xtranormal.com/

http://www.wikispaces.com/

SNC 2D1 – Gr. 10 Academic Science

Module 1

– Physical and Chemical Properties

– Pure Substances and Mixtures

– Atomic Structure (Bohr-Rutherford model)

– Valence Electrons and Ionic Charges

Physical Properties Reference Table

Complete definitions/explanations for these physical properties from grade 9.

Property Definition/Explanationstate

colour

odour

taste

mass

volume

opacity

texture

hardness

brittleness

malleability

ductility

viscosity

solubility

density

melting point

boiling point

freezing point

Layer the following substances in the beaker below, based upon their given densities.

Substance Density (g/cm3)

Substance Density (g/cm3)

mercury (liquid)

13.60 Bromine (liquid)

3.10

cork 0.27 water 1.00saltwater 1.05 bronze 8.80

oil 0.89 lead 11.40egg 1.03 tin 7.30

copper 8.93 glass 2.60ice 0.92 rubber 1.20

chalk 2.00 platinum 14.20


Module 2

– Periodic Table

– Ionic Charges Within Families

– Bonding (ionic, polyatomic, molecular)

Periodic Table

Complete the following chart, using your periodic table.

Element Name Symbol Atomic Number

Group Number

Period Number

Metal orNon-metal

State Family

chlorine

magnesium

30

N

17 5

3 Alkali metal

17 liquid

argon

20

2 7

Naming Simple Binary Compounds

Complete the following chart by writing either the name or the formula as required.

CaCl2 Strontium Sulfide

Potassium Iodide Calcium Phosphide

MgO AlCI3

Aluminum Chloride Calcium Iodide

NaBr Rb3P

Al2O3 Barium Oxide

Lithium Nitride Barium Phosphide

CaO Radium Nitride

Barium Chloride Zinc Phosphide

Sodium Chloride Ag2O

ZnO Silver Iodide

Silver Bromide Lanthanum Chloride

Potassium Chloride Potassium Phosphide

Calcium Chloride Magnesium Nitride

Sodium Sulfide LiP3

Barium Fluoride Rubidium Oxide

Calcium Nitride Beryllium Nitride

CaO Yttrium Oxide

Li2O Indium Fluoride

NaBr AcP

MgO Cs2S

ZnO Na3P

Aluminum Oxide Strontium Chloride

Magnesium Sulfide Zinc Sulfide

KF K2S

FrBr Sodium Iodide

Naming Complex Binary Compounds (Multiple Valencies)

Complete the following chart by writing either the name or the formula as required. Some of the metals MAY have multiple valencies that need to be specified using the brackets in the name....be observant!!

Magnesium Oxide PbS

Li2O Sodium Fluoride

AlCl3 Aluminum Nitride

MgS Lithium Iodide

Calcium Oxide SnO2

Beryllium Oxide Na2S

Nickel(II) Chloride Mg3P2

CaO Magnesium Nitride

Aluminum Sulfide NiO

Copper(I) Bromide CuI

KBr Tin(II) Iodide

BeF Iron(III) Chloride

Calcium Phosphide PbCl4

Lead(II) Oxide FeP

Lead(IV) Fluoride CaF2

Na3N Tin(IV) Bromide

Al2O3 Copper(II) Sulfide

CuCl2 Iron(II) Oxide

Calcium Nitride K3P

FeBr3 AgF

Naming Polyatomic Compounds

Complete the following chart by writing either the name or the formula as required. Be careful...there is a mixture of both multiple and single valence metals.

Sodium Chlorate Pb3(PO4)2

Li2CO3 Aluminum Nitrate

K2SO4 Potassium Hydroxide

Lithium Phosphate Sn(ClO3)2

Calcium Carbonate NaOH

Ca(NO3)2 Beryllium Sulfate

Mg3(PO4)2 Sodium Bicarbonate

Al(HCO3)3 Magnesium Hydroxide

Aluminum Phosphate CuNO3

Copper(I) Chlorate FeSO4

NaNO3 Calcium Sulfate

Al(OH)3 Lead(II) Nitrate

CuSO4 Copper(II) Hydroxide

Iron(II) Phosphate Ca(HCO3)2

Calcium Chlorate K3PO4

FeClO3 Magnesium Sulfate

Copper(I) Sulphate Lithium Phosphate

Potassium Hydroxide Uranium(III) Carbonate

Mercury(I) Bromide Potassium Permanganate

Ag2SO4 Aluminum Phosphate

Zn(OH)2 BaSO4

CuSO4 Bi(OH)3

Naming Molecular/Covalent Compounds

Complete the following chart by writing either the name or the formula as required. Since this is molecular/covalent bonding remember to use the Greek prefixes as required.

CF4 Ammonia (Nitrogen Trihydride)

Carbon Dioxide Hydrogen Peroxide (Dihydrogen Dioxide)

Carbon Monoxide H2O

NF3 P2O3

P2O5 PCl3

Carbon Disulfide CCl4

Methane (Carbon Tetrahydride) SiO2

Cl2O5 BCl3


Module 3

– Chemical Reactions

– Conservation of Matter

– Balancing Equations

– Types of Chemical Reactions

– Acids & Bases

Writing Chemical Equations

1. What is the advantage of writing a chemical equation?

2. For the chemical equation propane + oxygen carbon dioxide + water , state:

a) the reactants b) the products: c) the purpose of the arrow

3. Write a word equation for the following reactions:

a) CaCl2 and Na2SO4 react to form CaSO4 and NaCl

b) AgNO3 reacts with KCl to produce AgCl and KNO3

c) In the process of cellular respiration, carbon dioxide, water and energy are produced when sugar is reacted with oxygen by the cell.

Reflect on the following word equations and predict what elements or compounds belong in the blank space.

a) Aluminum resists corrosion because it reacts with a gas in the air to form a protectice coating. The equation is:

aluminum + __________ aluminum oxide

b) When aluminum foil is place in a solution of copper(II) sulfate, the aluminum will displace copper from the solution and take its place:

aluminum + copper(II) sulfate copper + ________________

c) When solutions of potassium iodide and lead(II) nitrate are mixed, lead(II) iodide will precipitate out leaving the other compound in solution:

potassium iodide + lead(II) nitrate lead(II) iodide + _____________

Types of Chemical ReactionsBalance the following reactions and indicate which of the five types of chemical reaction are being represented:

1) ____ NaBr + ____ Ca(OH)2 ___ CaBr2 + ____ NaOH

Type of reaction: _____________________________

2) ____ NH3+ ____ H2SO4 ____ (NH4)2SO4

Type of reaction: _____________________________

3) ____ C5H9O + ____ O2 ____ CO2 + ____ H2O ***challenging

Type of reaction: _____________________________

4) ____ Pb + ____ H3PO4 ____ H2 + ____ Pb3(PO4)2

Type of reaction: _____________________________

5) ____ Li3N + ____ NH4NO3 ___ LiNO3 + ___ (NH4)3N

Type of reaction: _____________________________

6) ____ HBr + ___ Al(OH)3 ___H2O + ___ AlBr3

Type of reaction: _____________________________

SNC 2D1 CHEMISTRY STRAND REVIEW

1. For each of the following, suggest one or more situations in which chemical reactions are important.(a) in your home(b) at tourist resorts(c) in restaurants in your community(d) in another situation of your choice

2. Pure substances are used to produce newspapers, paper towels, clothing, and many consumer products you use daily. What happens to these pure substances when you no longer need these products? Suggest several answers.

3. Every Canadian province has emergency teams and procedures to deal with chemical spill situations. Why do you think it is important to have laws that cover an entire province?

4. Suppose a train derailment spills sodium hydroxide into some soil. Use your knowledge of chemical reactions to suggest how an emergency response team could neutralize the effects of this chemical.

5. Write the symbols for the following ions.(a) cesium (b) oxide (c) nickel(III) (d) tin(II) (e) titanium(IV)

6. Write the name of the following ions.(a) Mg + 2 (b) Ag +1 (c) F –1 (d) N - 3 (e) Au +1

7. (a) What kind of electric charge do metallic ions possess?(b) What kind of electric charge do nonmetallic ions possess?

8. What elements make up “the group of 7”. What is special about them?

9. What is the difference between a molecule that is an element and a molecule that is a compound?

10.How many occupied shells are there in a neon atom?

11. What kinds of elements combine to form ionic compounds?

12.What kinds of elements combine to form molecular compounds?

13.State the law of conservation of mass.

14.Where are the reactants and the products located in a chemical equation?

15.What is the typical range of numbers on the pH scale? What is the pH range of bases What is the pH range of acids?

16.What kinds of substances are the reactants in a neutralization reaction?

17.How can you identify an acid and a base from their chemical formulas?

18.What type of chemical reaction is represented by these general chemical equations?(a) A + B → AB(b) CxHy + O2 → CO2 + H2O

19.Complete and balance each equation below. The products are all solid ionic compounds.(a) Na + Br2 →(b) Mg + F2 →(c) Al + Cl2 →

20.Suppose the reactants of a chemical reaction include a compound and a metallic element. What type of chemical reaction will occur?

21.What is the difference between an ion and an atom?

22.Name three elements that form negatively charged ions and three that form positive ions.

23.The figure below shows a Bohr diagram of a calcium atom.(a) How many electron shells are shown?(b) How many valence electrons are in the valence shell?(c) The charge on a calcium ion is +2. Explain how this diagram might have been used to predict this charge.

24.Draw the Bohr Diagram for: Ne, O-2, Al+3 and N-3. What do you notice about their electron arrangements? What word do we use to describe this?

25.State 3 members of each of the following families: halogen, noble gas, alkali metals and alkaline earth metals.

26.Suppose that a student placed a small piece of lithium metal into a beaker of water. The student observed a chemical reaction, in which a hissing sound was produced along with bubbles. Decide if these changes could indicate a chemical reaction. Then, explain your thinking.

27.Predict how acid precipitation might cause changes that affect the organisms in a lake.

28.Classify each of the following chemical reactions and balance them if necessary:

(a) NiCO3(aq) + Fe(s) → FeCO3(aq) + Ni(s)

(b) C5H10(l) + O2(g) → CO2(g) + H2O(l)

(c) Li4C(s) + Ca(s) → Li(s) + Ca2C(s)

(d) C6H14(g) + O2(g) → CO2(g) + H2O(l)

(e) CsF(aq) + AlBr3(aq) → CsBr(aq) + AlF3(s)

29.Write the names of the following ioniccompounds.(a) BeO (f) MnCl2(b) KCl (g) K2SO4

(c) SrBr2 (h) Li3PO4

(d) Al2S3 (i) Cr(OH)2

(e) Ca3P2 (j) NH4HCO3

30.Write the formulas for the following ionic compounds.(a) sodium bromide(b) beryllium phosphide(c) copper(I) oxide(d) palladium(IV) nitrate(e) ammonium sulphate(f) ammonium nitrate

31.Write the names of the following binary molecular compounds:(a) S2O3

(b) P2S5

(c) OF2

(d) N2O3

(e) CO2

32.Write the formulas of the following binary molecular compounds:(a) sulphur hexafluoride

(b) carbon disulphide(c) dinitrogen monoxide(d) carbon tetrachloride(e) carbon monoxide

33.For each of the following word equations, identify the type of chemical reaction it represents.(a) methane (CH4) + oxygen → carbon dioxide + water

(b) barium + oxygen → barium oxide

(c) aluminum bromide + fluorine → aluminum fluoride + bromine

(d) magnesium chloride → magnesium + chlorine

(e) lithium sulphate + barium chloride → lithium chloride + barium sulphate

(f) nitric acid + barium hydroxide → barium nitrate + water

34.Write the skeleton equation and balanced chemical equation for each of the following chemical reactions.(a) carbon disulphide + oxygen → carbon dioxide + sulphur dioxide

(b) lead(II) nitrate + sodium sulphate → lead(II) sulphate + sodium nitrate

(c) potassium bromide + silver nitrate → silver bromide + potassium nitrate

snc 2d1: chemistry workbook - mr. reid's science...

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