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Science 10 Unit A: Energy and Matter in Chemical Change 1

Unit A: Energy and Matter in Chemical Change

A1.1 IntroductionRead pages: 6-11

WHMISo Workplace Hazardous Materials Information Systemo There are three components to the WHMIS system:

___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________

WHMIS Symbols:


A1.2 Properties and classification of matterRead pages: 12-17

Physical PropertiesDescribe the physical appearance and composition of a substance:They include:

Chemical PropertiesDescribe how a substance will react chemically with another substance.They include:

Pure SubstanceAre only made up of one type of particle, all particles are identical.

Elements

____________________________________________________________________________

Are listed on the periodic table.

Eg. _________________________________________________________

Compounds

____________________________________________________________________________

Eg. CO2 – carbon dioxide

___________________________ _______________________________


Mixtures

_______________________________________________________________________________________

_______________________________________________________________________________________

SolutionIs uniform throughout, cannot see the different particles.

Eg. ____________________________________________________________________

Mechanical MixtureYou can see the different particles.

Eg. ____________________________________________________________________

SuspensionIs a mixture when the particles have different states.

Eg. ____________________________________________________________________

ColloidIs like a suspension but it is not easy to separate the parts.

Eg. ____________________________________________________________________


Chemical ReactionsThe following are signs that a chemical reaction has occurred:

1.

2.

3.

4.

5.

Assignment:Check and Reflect Page 17: Questions 1 - 9


Student Worksheet: Classification of Matter


A1.3 Atomic ModelsRead pages: 18-25

Aristotle [400 BC – 1500 AD]Thought that all matter is made up of only four elements:

o___________________________________________________o all of matter is some combination of these

four elements

Alchemy [1500 AD]In the 1500’s many scientists were________________________________________________________________________________________________________________________________________While they were not able to create gold they did discover many useful properties of matter such as:

o densityo boiling pointo melting pointo separation techniques

Dalton [1766-1844]Developed the _____________________________________________________________

o All matter is made up of tiny particles called atoms.o The atom is the smallest particle of matter and cannot be divided.o The atoms of an element are all identical in size and mass.o Atoms of different elements have

different properties.o Different atoms combine together in

specific ratios to form new substances.Eg H2O


JJ Thomson [1890s]Developed the

____________________________________________o Studied the properties of cathode rays.o Discovered the electron.o Within the atom there exists tiny negative

particles called electrons, the rest of the atom is a positive fluid sphere.

Ernest Rutherford [1908]Rutherford did the gold foil scattering experiment.

_________________________________________________o The atom has a small

positive, dense nucleus.o Most of the matter is found in

the nucleus.o The negative electrons orbit

the nucleus like planets orbit the sun.

Neils BohrBohr studied the bright lines in the visible spectrum of hydrogen.Bohr created a theory where _____________________________________________________________________________________________________________

o Electrons can occupy only specific orbits.o Each orbital can only hold a certain number of electrons.o For an electron to occupy an orbital it must has a specific amount of

energy (energy level).

Quantum MechanicalIn today’s model of the atom ______________________________________________________________________________________

o We have the greatest probability of locating electrons in certain regions around the atom.

o Depending on how many electrons an atom has and which energy level the electron is in then that electron can be found in a certain cloud formation.

o The electron can exist as a particle and as a wave at the same time.

Check and Reflect: 4 – 8 page 25A1.R Section 1 Review page 27


A2.1 Atomic StructureRead pages 28-38

ElementsAre made up of only one type of atom.

MetalsProperties include:

Non-metalsProperties include:

MetalloidsProperties include:


The Period TableAll of the elements have been organized onto the periodic table of elements. The elements are organized into rows and columns ______________________________________________________________________________________________________________________

GroupsElements are placed into _________________________________________.Elements in the same group/family have the same physical and chemical properties.

i. ____________________________________- Group IA- Very reactive metals- Li, Na, K, Rb, Cs, Fr

ii. _____________________________________- Group IIA- Reactive metals- Be, Mg, Ca, Sr, Ba, Ra

iii. _____________________________________- Group VIIA- Very reactive non-metals- F, Cl, Br, I, At

iv. _____________________________________- Group VIIIA- These elements are non-reactive- They do not form ions or compounds- He, Ne, Ar, Kr, Xe, Rn

PeriodsElements are placed into rows.Elements in the same row all have the same number of orbits and energy levels.

Eg. Li, Be, B, C, N, O, F, Ne


Subatomic ParticlesThe atom is made up of three types of subatomic particles:

Particle Symbol Charge Mass LocationProton 1.67 x 10-27 kgNeutron 1.67 x 10-27 kgelectron 9.11 x 10-31 kg

atomic mass number

atomic number

Atomic Mass Number____________________________________________________________.Is the mass of 1 mole of atoms.

Atomic Number____________________________________________________________.The number of electrons is equal to the number of protons in one atom.

Example:Chromium RuProtons: ___________ _______________Electrons: ___________ _______________Neutrons: ____________________ _______________________

2452.00Cr


Formation of IonsAtoms of the same element will always have the same number of protons.

When an atom _________________________________________ it will become an ion.

MetalsWill form _________________________________They _____________________________________ electrons from the outer orbit

Non-metalsWill form _____________________________They _______________________________ to gain extra electrons


Octet Ruleo Atoms strive to have _______________________ in their outermost orbit.o Atoms will give away or steal electrons until it has a complete and

stable outer orbital. o The number of electrons in the outer orbital is called ___________________

_________________________________o The number of electrons an atom will gain or lose to reach a stable

orbit is called the _______________________________.o Example:

o Sodium Valance electrons: _________ valance number: ___________________________ ion: _______________

o Chlorine Valance electrons: _________ Valance number: ___________________________ Ion: _________________

Lewis Dot Structureso A Lewis diagram is a model where the valance electrons are drawn as

dots around the atom.o This model shows ___________________________________________________________

________________________________________________________________________________o Examples:


o How Ions Form Compoundso When atoms combine to form an ionic compound the _______________________

_____________________________________________________________________________________o One ion will become positive and the other ion will become negative. o Each atom ends up with a

complete outer orbit with 8 electrons each.

Examples:

1. Complete the following for each atom

Atom Atomic Number

1st orbit 2nd orbit 3rd orbit Valance # Ion

Na


NCl

2. For each of the following draw the Lewis dot structure and write the atom as an ion:

a. Li

b. S

Check and Reflect: 1 – 12 page 39


A2.2 Naming Ionic and Molecular CompoundsRead pages: 40-49

Ionic Compoundso An ionic compound is formed when ___________________________________________

_____________________________________________________________________________________o An ionic compound is formed because the metal ion becomes positive and

the non-metal ion becomes negative so they _________________________________

____________________________.

Ionic Compound Formulaso For two atoms to form an ionic compound there must be __________________

_____________________________ between the negative ions and the positive ions.1. Write the correct formula for the ionic compound.

a. Li F

b. Ca2 Cl

c. K O2


d. Al 3 S2

Naming Ionic Compoundso {metal} {non-metal} + “ide”o Example:

o Sodium + chlorine ______________________________

2. Name each compound above in #1.

3. Write the formula given the name

a. lithium oxide

b. strontium chloride

Assignment: Worksheet A2.2: Ionic Compounds Worksheet #1- simple ionic compounds

Multivalent Elementso Some metals have the ability to form __________________________________________

________________________________.o These elements are usually the transitional-earth metals.o Examples:

o Iron (II): Fe2+, iron (III): Fe3+

o Copper (I): Cu+, Copper (II): Cu2+

4. Write the equation for each of the following

a. Iron (III) oxide

b. Copper (II) bromide

5. Given the formula write the correct chemical name:

a. CrO

b. Co2S3


Polyatomic Ionso A polyatomic ion is made up of ______________________________________.o Polyatomic ions can combine in ______________________________.o Suffixes

“ite” has fewer atoms of an atom “ate” has more atoms of an element Sulfite: ___________ Sulfate: ___________

o Compounds containing polyatomic ions follow the same balancing rules as all other ionic compounds.

o Naming polyatomic compounds: {metal} + {polyatomic ion} the name of the polyatomic ion does not change (it has been married

once already)Example:

Calcium carbonate

1. Write the correct chemical formula for the following:

a. sodium sulfite

b. magnesium nitrate

c. ammonium sulfide

Assignment: Ionic Compounds Worksheet #2


Molecular Compoundso A molecular compound is created when _________________________________________

__________________________________.o When non-metal atoms form molecules they must ______________________________,

they form _________________________________. By sharing electrons the outer orbits still have _______________________________.


o Because non-metals atoms ______________________________ the same two elements they ________________________________________(we cannot predict the ratio in a molecular compound)

o To name molecular compounds we use a prefix system for naming.o Examples:

a. SO, ______________________________b. SO2, ______________________________c. SO3, ____________________________________________________________d. SO4, ____________________________________________________________e. P3O5, ____________________________________________________________

o A number of molecular compounds have common names:

Molecular elementso Many of the non-metal elements exist in molecular form:

Assignment: Molecular Compounds Worksheet #2

Name FormulaH2O(l)

CO2(g)

C6H12O6(s)

C12H22O11(s)

CH4(g)

NH3(g)

H2O2(l)

C3H8(g)

Element FormulaHydrogenNitrogenOxygenFluorineChlorideBromineIodinePhosphorusSulfurOzone


Check and Reflect: 1 – 11 page 50


A2.3 Properties of Ionic and Molecular CompoundsRead pages 51-60

Properties of ionic compoundsooooooooo an ionic compound is also referred to as “a salt”

Solubility of Ionic Compoundso some ionic compounds are more soluble than otherso a substance that dissolves well is considered very solubleo an ionic compound that is soluble in a solution is written as ___________________,

a an ionic compound that is not soluble will be written as ______________________

Solubility Table

Ion Group 1NH4

+

H3O+ (H+)

ClO3-

NO3-

ClO4-

CH3COO- Cl-

Br-

I-

SO42- S2- OH- PO4

3-

SO32-

CO32-

VerySoluble

All All Most Most Most Only with: Group 1Group 2NH4

+

Only with:Group 1NH4

+

Sr2+

Ba2+

Tl+


+

SlightlySoluble

None None

Only with:Ag+

Hg+

Only with:Ag+

Pb2+

Hg+

Cu+

Tl+

Only with:Ca2+

Sr2+

Ba2+

Ra2+

Pb2+

Ag+

Most Most Most


Examples:

1. Which of the following compounds will most likely dissolve in water?a. NaNH4

b. LiClc. CaSd. KOHe. AgClf. CaSO4

g. Cu(OH)2

Properties of Molecular Compoundso Molecular compounds are compounds made up of ___________________________

_____________________________________________o The non-metal atoms are held together by ________________________________, the

atoms share electrons which make a _____________________________________.o The attraction between neighboring molecules is weak so ___________________

__________________________________________o Molecular compounds can also make crystalline structures that crumble

easily.o Molecular compounds _______________________________________________ because they

are made up of non-metal atoms.

Special Properties of Watero ______________________________________, one side is slightly positive and the other

side is slightly negative.o The molecules form an electrostatic attraction to each other.o Water has the following properties:

_________________________, water molecules are attracted to other water molecules

_________________________, water molecules are attracted to other molecules

_________________________________, because of cohesion water makes a strong surface force

_________________________________, water can crawl up a straw or edge of a container because of adhesion

Conducts heat __________________________________ Specific heat capacity


Phases of Water (Ice)o Ice (solid) is less dense than the liquid form of water because of the

molecular formation of water, ordered molecular structureo _________________________________________________________________________________

__________________________________________o Water (lakes) freezes from the top down.

Assignment: Check and Reflect: 1 – 9 Page 61


A2.4 Acids and BasesRead pages 62-68

Properties of Acidsoooooo

Properties of Basesoooooo

ph Scaleo pH is an indication of the ________________________________________ in a solutiono the higher the concentration of H+ ions the stronger the acid, the higher the

pH acids: _________________ neutral _________________ bases: _________________


Indicatorso an acid-base

indicator is a chemical that is

used to determine if a solution is ________________________________________o an indicator ________________________________________________________________________o different indicators will change colour for different pH ranges:o universal indicator is a mixture of several indicators that change colour as

the pH changes to different ranges

Naming Acidso acids are named based on the non-metal anion in the compound

Examples:

Formula Compound Common Acid nameHS(aq) Hydrogen sulfideH2SO3(aq) Hydrogen sulfiteH2SO4(aq) Hydrogen sulfate

IUPAC naming system for acids:[International Union of Pure and Applied Chemistry]

Formula Compound IUPAC name

Anion Compound name Acid name“ide” Hydrogen (anion)-

ideHydro (anion)-ic acid

“ite” Hydrogen (anion)-ite (anion)-ic acid“ate” Hydrogen (anion)-ate (anion)-ous acid


HS(aq) Hydrogen sulfideH2SO3(aq) Hydrogen sulfiteH2SO4(aq) Hydrogen sulfate

1. Name the following acids:a. H3N(aq)

b. HNO2(aq)

c. HNO3(aq)

d. H3PO4(aq)

Assignment: Worksheet – A2.4 Naming acids


Baseso Most bases contain an __________________________________o Bases _____________________________________ because they react with oils and

greaseo Some common bases:

Base Name Common name UseNaOH(aq) Sodium hydroxideNH4OH(aq) Ammonium

hydroxideMg(OH)2(aq) Magnesium hydroxide

Acids and Bases in Your Bodyo Our bodies contain a variety of substances each substance has a specific pH:

Saliva – 6.4 Blood – 7.35 Stomach – (1-2) Small intestine – 8.5 Large intestine – (5.5-7.0) Urine – 6.4

o It is important that our bodies maintain this pH balanceo ______________________________, is a substance that helps to maintain a pH level in

a solution, it resists change in pH

Acids and Bases in the Homeo acids and bases serve a variety of functions in our homeso some typical acids are:

o _________________________________________________________________________o some typical bases are:

o _________________________________________________________________________


Neutralizationo a type of chemical reaction where ______________________________________________

_____________________________________________________is called a neutralizationo the products of a neutralization reaction are always:

_____________+_______________--> ____________________+______________________

HClaq NaOHaq H 2Ol NaClaqo carbon dioxide is produced only when one of the compounds contain the

carbonate moleculeo eg vinegar + baking soda

Assignment: Check & Reflect


A2.5 Our Chemical SocietyRead pages: 70-75

Issues Related to Chemicalso some chemicals are hazardous because of:

____________________________________________________________ how they are produced ________________________________________________________________________________ their effect on the ecosystem

Environmental Effectso some chemicals are harmful because of how they effect components within

the environmento some harmful chemicals ____________________________________________________________

____________________________________________

o CFC’s chlorofluorocarbons come from Freon used in __________________________________________________ can stay in the atmosphere for up to 50 years _________________________________________, the ozone helps to protect the

Earth from harmful UV, and X-Rays from the sun

o Greenhouse gases (________________________) most of the greenhouse gases come from the _____________________________

______________________________ levels of greenhouse gases in our atmosphere are increasing the greenhouse gases are trapping in heat and the temperatures

around the Earth are increasing

o Acid Precipitation other products of the combustion of fossil fuels are ____________________

________________________________________________________ particulates enter the Earth’s atmosphere and return in the form of

_____________________________________________ ______________________________________________________________________________

_________________________________


Health Concernso Many people use chemical substances for recreational purposeso Some of these chemicals are ____________________________________________o Some of these chemicals _____________________________________

o Alcohol (CH3CH2OH(l)) alcohol is considered a drug because of its effects on the body excessive amounts can

__________________________________________________ ______________________________________________________________________

repeated use can lead to physical and psychological dependence, ______________________________________________

o Nicotine and tobacco products __________________________________________________________________________ The use of tobacco products have been related to high incidences of

cancer

Benzeneo Benzene is a hazardous chemical that is both toxic and flammable o Many products are made using benzene

________________________________________________________________o Benzene is a regulated chemical so there are strict regulations about its

transportation and storageo Because of its toxic effects any ____________________________________________________

is hazardous Workers must take specific steps for protection, WHMIS

Chemistry Related Careerso Because we use so many different chemicals there are many careers that

involve chemistry: Chemical engineers Chemistry teachers ___________________________________________ ___________________________________________________________ Cosmetics Household product design

o Almost each person works or interacts with chemicals everyday Food and cooking _____________________________________________ Gas and transportation _____________________________________________ Manufactured products

A2.R Section 2 Review pages 76-77


AQ.2 Quiz 2


A3.1 Examples of Chemical ChangeRead pages: 79-85

During a chemical reaction a ________________________________________________________________________________________________________________________

Example:Methane + oxygen water + carbon dioxide + (energy)____________________ _______________________________

Showing States in a Chemical Formulao In some chemical reactions the products may be in the form of a

_______________ or in the form of a ____________________________o The symbol (aq) means that in solution the compound will

________________________________________.o In any chemical equation it is important that you show the state of each

element or compound in the reactiono Examples

CH 4(g) O2(g) H2O(g) CO2(g) energy

CaC2(s ) H2O(l ) Ca OH 2(s) C2H2(g)

Which compounds are gases?

Which compounds are solid?

Which compounds are liquid?

Which of these was an element?


Energy Changeso ____________________________________________________________________________________

_________________________________________.

Phase Changeo When a substance changes state there is a characteristic change in

energy that occurs.o In a pure substance the phase changes

(_____________________________________________________________)

o In a mixture there are a variety of phase changes.

Exothermic Reactiono Release energy usually in the form of __________________________________o The energy of the products is ____________________ than the energy of the

reactants. (______________________________________________________________)o Example:

CH 4(g ) O2(g) H2O(g) CO2(g) energy

Endothermic Reactiono Energy is absorbed from the surrounding environment, usually

__________________________________________________________________o The energy of the products is________________________ than the energy of

the reactants. (___________________________________________________)o Example:

Ba OH 2(s) NH 4SCN Ba SCN 2(aq) NH 4OH (aq)

Biochemical Reactionso Two important biochemical reactions are:

o Cellular Respiration This is how living organisms (cells) get energy from glucose. Is an __________________________________________.

o Photosynthesis This is how plants get energy from the sun. Is an ___________________________________________.


Evidence of a Chemical Reactiono In all chemical reactions a new substance is produced that has its own

characteristic properties.o Indicators of a chemical change:

Conservation of Masso Mass is conserved in all chemical reactions.o In all chemical reactions ______________________________________________________ the

mass of the reactants.o Example:

o2AgNO3(aq ) Cu(s ) Cu NO3 2(aq)

2Ag(s )

(33.98g) (6.36g) (______________) (21.57g)

Assignment Check and Reflect: 1 – 11 P. 85


A3.2 Writing Chemical EquationsRead pages: 86-89

Chemical Equationso a word equation describes the reactants and products of a chemical reaction

____________________________o a chemical equation _______________________________________________________________

to identify the reactants and products in a chemical reactiono a chemical equation is more useful because:

o _____________________________________________________________________________

o _____________________________________________________________

Example:

Word equation

Silver nitrate + copper copper nitrate + silver

Chemical equation

Practice:Write the following as a chemical equation:

1. potassium + oxygen potassium oxide

2. scandium + nitrite scandium nitrite

3. sulfur + oxygen sulfate

Worksheet: A3.2 Writing chemical equations


Balancing Chemical Equationso in all chemical reactions mass is conserved so we ______________________________

_____________________________________ for each element in the reactants and in the products

o it is important that we balance any chemical equation that we write

Examples:Balance each of the following chemical equations

a. Na(s) + Cl2(g) NaCl(s)

b. H2(g) + O2(g) H2O(l)

c. N2(g) + H2(g) NH3(g)

d. Na(s) + H2O(l) NaOH(aq) + H2(g)

e. CH4(g) + O2(g) H2O(g) + CO2(g)

f. Pb(s) + H3PO4(aq) H2(g) + Pb3(PO4)2(s)

g. AgNO3(aq) + CuSO4(aq) Ag2SO4(s) + Cu(NO3)2(aq)

Worksheet A 3.2 Balancing Chemical Equations


Check & reflect 6 – 9 p. 90


A3.3 Five Common Chemical ReactionsRead pages: 91-105

There are five common types of Chemical Reactions:

I. Formation Reaction (Synthesis)o During a formation reaction two or more elements __________________________

_____________________________________________________

o A formation reaction is also referred to as a __________________________________.

o Many formation reactions are ____________________________, that is heat is given off during the reaction.

A + B AB

Example:

magnesium + oxygen magnesium oxide

Practice:Complete the reaction by writing the product, write the chemical equation, then balance.

1. aluminum + chlorine

2. carbon + hydrogen methane

Text: Practice problems: 2, 3, 4 p. 92, 93Skill Practice: 1, 2, 3 p. 93


II. Decompositiono During a decomposition reaction __________________________________________

into its component elements.o Many decomposition reactions are ____________________________, that means

that energy must be added to the reaction to break apart the existing chemical bonds.

AB A + B

Example:

Water + energy (electricity) hydrogen + oxygen

Practice:

1. calcium oxide

2. aluminum sulfide

Text Practice problems: 5 p. 94


III. Hydrocarbon Combustiono During a combustion reaction a __________________________________________

_______________________________________________________________________________

_________________________________________________

o Combustion reactions are _________________________________. o The potential energy of the reactants is higher than the energy of the

products so during the reaction heat energy was released.

Example

Methane + oxygen carbon dioxide + water + (energy)

Practice:

1. propane C3H8(g) + oxygen

2. glucose + oxygen

Text: Practice Problem: 6 p. 95


Solubility of Ionic Compoundso some ionic compounds are more soluble than otherso a ionic compound that ___________________________________________________________

_____________________________________________________________________________________o an ionic compound that is soluble in a solution is written as __________________,

a an ionic compound that is not soluble will be written as _____________________, it will form a ____________________________

Solubility Table

Ion Group 1NH4

+

H3O+ (H+)

ClO3-

NO3-

ClO4-

CH3COO- Cl-

Br-

I-

SO42- S2- OH- PO4

3-

SO32-

CO32-

VerySoluble

All All Most Most Most Only with: Group 1Group 2NH4

+


+

Sr2+

Ba2+

Tl+


+

SlightlySoluble

None None

Only with:Ag+

Hg+

Only with:Ag+

Pb2+

Hg+

Cu+

Tl+

Only with:Ca2+

Sr2+

Ba2+

Ra2+

Pb2+

Ag+

Most Most Most

Examples:

Which of the following compounds are very soluble and which are slightly soluble?

a. NaNH4

b. LiClc. CaSd. KOHe. AgClf. CaSO4

g. Cu(OH)2


IV. Single Replacemento During a single replacement reaction an ionic compound reacts with

another element, the chemical bond in the compound breaks apart and then _____________________________________________________________________________________________________________

o The other two ions will have a ____________________________________ (bond) this is why they combine to form a different compound.

A + BC B + AC

D + BC C + BD

Example:

Sodium chloride + silver silver chloride + sodium

Practice:Complete the word equation and predict the products.Write the appropriate chemical equation, indicate if a precipitate is formed. Balance the equation.

1. Lithium sulfate + calcium

2. Chlorine + copper I bromide

Text: Skill practice: 1 – 4 p. 97


V. Double Replacemento During a double replacement reaction two ionic compounds in a solution

will combine and then _________________________________________________________

___________________________________________________________________________________

o One pair of ions will have a _______________________________________ (bond) this is why a different compound is formed.

o Quite often a _________________________________________ as a result of a double replacement reaction.

AB(aq) + CD(aq) AD(s) + CB(aq)

Example:

sodium chloride + silver nitrate sodium nitrate + silver chloride

Practice:Complete the word equation and predict the products.Write the appropriate chemical equation, indicate if a precipitate is formed. Balance the equation.

1. Potassium iodide + silver nitrate

Text: Practice problem: 9, 10, 11, 12 p. 100 – 105

Assignment: Worksheet A 3.3 Reaction TypesCheck and Reflect: 1 – 8 p. 106


A3.4 The Mole Read pages: 107-111

Avogadro’s Numbero The quantity that chemists use to measure _______________________________________

is present in a sample is called the _______________________________o The number of atoms or particles in one mole is Avogadro’s Number

o 1 mole = ____________________________________

Atomic Masso the atomic mass of an element is the mass of 1 mole of atoms of that element

that is the mass of 6.02 x 1023 atoms.o For example:

o 6.02 x 1023 atoms of Carbon weigh: __________________o 6.02 x 1023 atoms of Oxygen weigh: __________________

Where did the atomic masses of all of the elements come from?o By looking at how atoms combine to form compounds scientists were able to

find the atomic masses of all of the elements as they were _______________________________________________________________________.

o Today’s periodic table is based on _____________________________________________o After finding the atomic numbers and the atomic masses ____________________

then created the _______________________________________.

Finding the Atomic Mass of a Compoundo The atomic mass of 1 mole of a compound will be the sum of the atomic

masses of each of the elements in the compound.o ________________________________________________________________________________________

o Example: what is the atomic mass of one mole of

a. H2O(l): 2 H + 1 O = 2(1.01) + 1 (16.00) = 18.02 g/mol

b. CO2(g) : 1 C + 2 O =

c. Na3PO4(s):

d. Ca(NO3)2(s):


Converting Moles to Grams (mass)

m mass (g)n molesM molar mass

Examples: Find the mass of

a. 3 moles of NaCl(s)

b. 2 Fe2SO4(s)

c. 4.5 Zn(NO2)2(s)

Converting Grams (mass) to Moles

Examples: How many moles are there for each compound given the mass.

a. 65.0 g of: NaOH(s) 1 mole: NaOH(s) = 40.00 g

n mM

60.0g40.00g

1.5 mol

b. 348.75 g of: CoSO4(s)

c. 880.10 g of: Cr(NO3)2(s)

Text: Practice Problems: 13 – 20 p . 108, 109Check & Reflect: 1 – 11 p. 112

A3.R Section Three Review p. 113AR Unit A Review p. 117-121

m nM n mM

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