1. chemical reactions printable slides part...

1. Chemical Reactions printable Slides part One.notebook

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February 21, 2017

Title

Unit 3: Chemical Reactions

Intro Chemistry

Introduction• The study of substances and their reactions• Processes have a role in almost every aspect of everyday life• Key to developing new products & solutions to problems

• Learning about chemistry involves...o Mixing substances in test tubes

o Researching specific topicso Applying and extending knowledge

• As you learn about chemical processes, you will become more aware of the ways that chemistry‐related issues affect people's lives

Matter

Classification of Matter

Compounds Elements Solutions HeterogeneousMixtures

PureSubstances Mixtures

(anything that occupies space)

(all particles are the same) (2+ pure substances)

2+ elements

bonded together

1 type of atom

1 visible com

ponent

2+ visiblecom

ponents

5.1


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Pure Substances

Classification of MatterPure Substance• All the particles that make up the substance are the same; the substance has constant properties.

ElementsCannot be broken down into different types of atoms; they only contain one type of atom (ex. gold).Represented by a chemical symbol (ex. Au).

CompoundsContain two or more different elements (different types of atoms) bonded together in a fixed proportion.Identified by chemical formulas (ex. H2O).

Mixtures

Classification of MatterMixtures• Contain two or more pure substances that can be separated by physical means.

Homogeneous MixturesHave only one visible component.A.k.a. solutions.Not easily separated.

Heterogeneous MixturesContain two or more visible components. A.k.a. mechanical mixtures.Easier to separate by filtration, evaporation of the solvent, and by using ones hands to remove individual components.

Physical Property

Properties of Matter• A physical property is a characteristic of a substance o state o mass o volume o malleabilityo color o luster o density o crystal formo odor o texture o solubility o melting pointo hardness o ductility o viscosity o boiling point

Baking soda: white; crystalline solid @ room temp; dissolves in water to form a solution

Water: tasteless & odorless; liquid at standard atmospheric temperatures and pressures; very slightly blue, colourless in small quantities; boiling point = 100oC

o A physical change is a change in the size or form of a substance, and it does not change the chemical properties of the substance.


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Chemical Property

Properties of Matter• A chemical property is a characteristic behavior that occurs when a substance changes to a new substance Ex: reacts with acid, reacts with water, combusts

o The change itself is called a chemical change. A substance is changed into one or more new substances (ex: burning, cooking, and rusting)

p. 175 #14

Practice Questions p. 1751. Classify each of the following as a pure substance or a mixture.

Explain your choices.a) soapy water b) hydrogen gas c) sodium chloride

2. Classify each as an element or a compound. Explain your choices.a) hydrogen b) potassium carbonate c) water d) Mg

3. Draw separate sketches to represent substances made up of 10 particles of each of the following:a) an element b) a compound c) a mixture

4. Classify each of the following as a physical property or a chemical property. Explain your choices.a) gasoline is a clear, pink solutionb) gasoline burns in airc) water boils at 100oCd) electric current can split water into hydrogen and oxygen gas

Chemical Reactions

Chemical Reactions• Clues of chemical change: New colour

Heat or light

Bubbles

Precipitate

Difficult/impossible to reverse


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Chemical Reactions

Chemical Reactions• Chemical reactions have a standard format when written:

Reactants Products

A + B C + D• Chemical reactions can be used to make new substances and are also useful for identifying unknown substances (ex. testing for different gases).

Acid +

Limestone =

CO2 gas

p. 175 #58

Practice Questions p. 1755. When aluminum metal is added to hydrobromic acid, hydrogen

gas and an aluminum bromide solution are formed.a) Was this a chemical or a physical change? Explain.b) Which substances are reactants and which are products?

6. In your own words, describe the chemical tests that can be used to identify the following gases:a) hydrogen b) oxygen c) carbon dioxide d) water vapour

7. When sodium carbonate is added to water, it dissolves. When hydrochloric acid is added to the solution, the solution fizzes. What kinds of changes occurred? Explain.

8. (a) Why does a glowing splint (piece of wood) burst into flame when oxygen gas is tested?(b) When you test for hydrogen gas, another gas is involved. What is this other gas?

Periodic Table

Periodic Table of Elements• Helps to explain and predict both chemical and physical properties of different elements.• It is a means of organizing all of the elements.• Elements that are within the same column of the periodic table are called chemical families or groups.• Rows of the periodic table are called chemical periods.

Groups or Families Periods


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PT Metals

Periodic Table of Elementso Metals are toward the left side of the table and are located

below the staircase.‐ Tend to be shiny and malleable solids that are conductors of heat and electricity.

o Nonmetals are toward the right side of the table, above the staircase.‐ Tend to be dull and brittle. They are found to be solids, liquids, and gases, all of which are insulators.

o Metals and nonmetals located directly above and below the staircase that exhibit metallic and nonmetallic properties. These elements are also often referred to as metalloids.

Nov 68:21 PM

METALS

NONMETALS

METALLOIDS

1

2

3 4 5

18

Alkali Metals

Alkaline Earth Metals

Halogens

Noble Gases

PT Families

Periodic Table of Elementso There are four key families and each tends to have the same

physical and chemical properties.‐ Alkali metals – Group 1‐ Alkaline Earth metals – Group 2‐ Halogens – Group 17‐ Noble Gases – Group 18

o Hydrogen is unique because it exhibits properties of both metals and nonmetals. It is located above group one because it has one valence electron just like the alkali metals.


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Atomic Structure

Atomic Structure• The Bohr‐Rutherford Model of the atom

o Shows that atoms are composed of three subatomic particles:

Atomic Structure

Atomic StructureProtons are heavy and positively charged. Neutrons have approximately the same mass as protons, but they are neutral.Electrons have almost no mass and they are negatively charged.

Protons and neutrons are located at the dense core of the atom (the nucleus).

Atoms are electrically neutral because they have the same number of protons and electrons.

# + = # ‐

Nov 84:40 PM


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Atomic # & Weight

Atomic Structureo The atomic number of an element indicates the number of

protons it has in one atom.

o The atomic weight of an atom indicates the sum of protons and neutrons.‐ It is measured in atomic mass units (amu).

____ protons____ neutrons____ electrons____ amu



Energy Levels

Atomic Structureo The model represents the arrangement of electrons.

Electrons orbit the nucleus at different energy levels (aka orbits or shells)‐ 1st shell: 2 electrons

2nd ‐ 4th shells: 8 electrons each

‐ The farther away an electron is from its nucleus, the greater its energy and its tendency to be involved in chemical reactions.

‐ Electrons in the outer‐most shell (valence shell) are called valence electrons; they are involved in bonding.

o This theory only applies to elements up to 20 electrons.

Noble Gases Electrons

Atomic Structure• Noble gases (Family 18) have full orbits

o they don't have any spare electrons they're willing to share, nor do they need to borrow from others

o this is why they don't tend to react with other elements


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Atomic Notation

Atomic Notation

Nov 1010:24 AM

Atomic StructureDraw Bohr Diagrams for the following elements:

Name: Hydrogen Helium Lithium Beryllium

Symbol: ____________ _________ _________ _____________

Atomic #: ____________ _________ _________ _____________

Protons: ____________ _________ _________ _____________

Electrons: ____________ _________ _________ _____________

Diagram:

Compounds

Classification of Matter

Compounds Elements Solutions HeterogeneousMixtures

PureSubstances Mixtures

(anything that occupies space)

(all particles are the same) (2+ pure substances)

2+ elements

bonded together

1 type of atom

1 visible com

ponent

2+ visiblecom

ponents

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Octet Rule

Compounds• 2+ different elements bonded in a fixed proportion• Atoms want an arrangement of electrons like the nearest noble gas• Bonding shares/transfers electrons to become more stable

• This is called the octet rule.o Noble gases do not easily form compounds because their

electron arrangements are stable.

Types of Compounds

Compounds• There are three types of compounds:o Ionic – Electrons are transferred between metals and nonmetals o Molecular – Electrons are shared between nonmetals.o Metallic – electrons move freely around metals.

• A binary compound is simply a compound that consists of atoms only two different elements (ex. NaCl, SO3, CaS).

NaCl

KF

CO2

H2O

Mg2Sn

Fe3C

Chemical Formula

Compounds• A chemical formula is a combination of symbols that represent a particular compound. It indicates…o what elements are present, ando the number of each atom present

NaCl: ___ sodium, ___ chlorine

CO2 : ___ carbon, ___ oxygen

H2O: ___ hydrogen, ___ oxygen

Mg2Sn: ___ magnesium, ___ tin

KF: ___ potassium, ___ flourine

Fe3C: ___ iron, ___ carbon


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Atom to Ion

Compounds• Atoms become ions when they gain or donate valence electrons.o ionic charge is the # value of the charge (+/‐). o It is written as a superscript on the right of the symbol (ex. Ba2+).o Names of nonmetal ions end with “ide” (ex. F‐ is the fluoride ion).o Families tend to form ions with similar charges.

(Cation) (Anion)

p. 189 #14

p. 189 #1‐41. (a) How do metals form ionic compounds with nonmetals?

(b) Describe the process with an example.

2. Beryllium and fluorine react to form an ionic compound.(a) Which element is the metal and which is the nonmetal?(b) Draw Bohr diagrams of beryllium and fluorine.(c) How many electrons must each element gain or lose to form stable ions?(d) Draw sketches to show how this compound forms by transfer of electrons.(e) Indicate the ionic charges on the ions.(f) What is the overall charge on the compound?(g) What is the chemical formula of the compound?

3. Repeat question 2 for the compound formed by aluminum and fluorine.

4. What part of the atom is involved in making chemical bonds?

Characteristics

Ionic Compounds• Made up of a cation (metal) and an anion (nonmetal) because electrons were transferred from the metal to the nonmetal.

+1 ‐1


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Ionic Bonding

Ionic Compounds• Opposite charges attract, so opposing charges of the two ions cause them to be attracted to each other.o Ionic Bonding: force of attraction b/t oppositely charged ions.o Result = electrically neutral compoundo Examples:

NaCl 1 Na+ ion, 1 Cl‐ ion

CaF2 1 Ca2+ ion, 2 F‐ ions

Salts

Sodium Chloride NaCl

Copper Sulfate CuSO4

Potassium DichromateK2Cr2O7

Mercury SulfideHgS

Ionic Compounds• A solid ionic compound (ionic solid) is also known as a salt

o it is a solid consisting of oppositely charged ions.

Formula Writing

Ionic Compounds ‐ FORMULA WRITING1. Temporarily write the ionic charge above each symbol.2. Crisscross the ionic charges, using them as subscripts for the

opposite ions.3. Reduce the subscripts to the lowest numbers possible.

Calcium Phosphide


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Notes

o NOTE…§ There are no spaces between symbols when writing chemical

formulas.§ Be sure to capitalize the first letter of a chemical symbol. If

there is a second letter, it is always lowercase.§ There is no need to write a subscript if there is only one atom of

that element present.

Ionic Compounds ‐ FORMULA WRITING

BaCl2

Practice

Ionic Compounds ‐ FORMULA WRITING

p. 195 #2,3,5

p. 195 #2, 3, 52. Draw a Bohr diagram to show the electron transfer that occurs when magnesium (Mg) and fluorine (F) form the compound magnesium fluoride.

3. Write the formulas for the compounds formed by the following combinations of elements:a) lithium and fluorineb) calcium and brominec) sodium and nitrogend) aluminum and nitrogen

5. Write the formulas for the following compounds:a) sodium iodideb) beryllium fluoridec) magnesium oxided) aluminum sulfide


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Naming

Ionic Compounds ‐ NAMING• IUPAC: non‐governmental agency that is the recognized authority in developing standards for the naming of the chemical elements and their compounds

International Union of

Pure and Applied

Chemistry

• When naming, all letters should be lower‐case

http://www.iupac.org/

Binary Ionic Compounds

K2O potassium oxide

Ionic Compounds ‐ NAMING• Naming binary ionic compounds:o Write the name of the metal followed by the name of the nonmetal

ending in “ide”

NaCl sodium chloride

CaF2 calcium fluoride

p. 195 #1, 4, 6

1. (a) How does the sum of the charges on the positive ions compare to the sum of the charges on the negative ions in ionic compounds?

(b) Calculate the sum of the ionic charges in the compound Al2O3. Show your work.

4. Name each of the compounds formed by the following combinations of elements:(a) lithium & fluorine lithium fluoride(b) calcium & bromine calcium bromide(c) sodium & nitrogen sodium nitride(d) aluminum & nitrogen aluminum nitride

6. Write the names for the following compounds:(a) KCl potassium chloride(b) Na3P sodium phosphide(c) CaF2 calcium fluoride

p. 195 #1‐9

http://www.iupac.org/


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Polyvalent Ionic Compounds

Ionic Compounds ‐ NAMINGo Some metals can form more than one kind of ion – they are called

polyvalent metals.o Begin by writing the name of the metal and add a Roman numeral in

round brackets after it to indicate its ionic charge. Finish with the name of the nonmetal ending in “ide”.

Fe3N2

iron (II) nitride

p. 195 #79

7. Write the formulas for the following compounds:

(a) copper(I) bromide

(b) copper(II) bromide

(c) iron(II) sulfide

8. Write the names for the following compounds:

(a) SnCl2

(b) SnCl4

(c) PbBr2

9. Write the formula and name of the compound formed by each of the following combinations of ions. (Some need Roman Numerals)

(a) Fe3+ & O2‐

(b) Ca2+ & F‐

(c) Cu+ & S2‐

p. 195 #7,8,9

Polyatomic Ionic Compounds

Ionic Compounds ‐ NAMINGo Polyatomic ion: atoms that tend to stay together and carry an

overall ionic charge (ex. Nitrate ion: NO3‐).


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Polyatomic Ionic Compounds

Ionic Compounds ‐ NAMINGo When writing the formula of a polyatomic ionic compound, add

brackets around the ion before showing the number you need.§ Ex. Ba(NO3)2 – barium nitrate

o Write the name of the metal first, then the polyatomic ion's name.

Fe(NO3)3

Pb(SO4)2

p. 198 #14

1. In your own words, explain what is meant by "polyatomic ion." Give two examples.

2. What happens to the ions in the compound sodium nitrate when it dissolves in water?

3. Write the formulas for the following compounds: (a) sodium phosphate

(b) calcium sulfate

(c) potassium chlorate

(d) aluminum hydroxide

(e) beryllium nitrate

(f) magnesium hydrogen carbonate

(g) nickel carbonate

4. Write the names for the following compounds:(a) K2CO3

(b) Na2SO4

(c) Al(HCO3)3

(d) AgNO3

p. 198 #1‐4

Acids

Ionic Compounds ‐ NAMINGo Acids form when hydrogen atoms combine with certain ions§ The hydrogen ion has an ionic charge of 1+ (H+).§ Acids have the subscript aq (aqueous) after their formula.

o To name acids, follow these simple guidelines:

H + ______ate = ____ic acid H2SO4 = sulfuric acidH + ______ite = ____ous acid H2SO3 = sulfurous acidH + element = hydro____ic acid HCl = hydrochloric acid

o An oxyacid is simply and acid formed when H+ combines with polyatomic ions that contain oxygen.


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Ionic Compounds Flow Chart

Formula Writing(given the name)

Criss‐cross the ionic charges & reduce if needed

Naming(given the formula)

"metal nonmetal+ide"

Polyvalent Metals

PolyatomicIons

Ionic Compounds(metal + nonmetal)

Flow Chart for Ionic Compounds

What do you do?

What do you do?

AcidsWhat do you do?

What do you do?

Molecular Compounds

Molecular Compounds• Most of the compounds encountered each day do not contain ions.• They contain neutral groups of atoms called molecules.

o Molecule: a molecular compound• Molecular compounds are made of nonmetals that are sharing electrons.

Molecular Compounds

Molecular Compounds• A covalent bond is a shared pair of electrons held between two nonmetal atoms. The nonmetals are held together to form a molecule.

• Diatomic Molecules are elements that exist naturally as molecules made of two atoms.

o H2, N2, O2, F2 , Cl2, Br2, I2 are all diatomic.


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Diatomic Molecules

Molecular Compounds“Start at 7, make a 7, and don’t forget the hat!”

Diatomic Molecules

Molecular CompoundsAdd the second atom to form each diatomic molecule of the group of 7

Formulas

4 3 2 1H

C N O FSi P S Cl

As Se BrI

Molecular Compounds• The number of electrons that nonmetals need to share to become stable is a clue to the number of covalent bonds it can form.

• The combining capacity (aka bonding capacity) is a measure of the number of covalent bonds that a nonmetal needs to form a stable molecule.• Use the crisscross method and reduce the subscripts if possible.

Combining Capacities of Nonmetal Atoms


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Formulas

Molecular Compounds 4 3 2 1H

C N O FSi P S Cl

As Se BrI

Step 1: Write the left‐most element first

Step 2: Write the combining capacities above the element symbols

Step 3: Crisscross the combining capacities to get subscripts

Step 4: Reduce the subscripts if possible

Step 5: Remove any "1" subscripts ‐ they're not needed

Carbon & sulfur

Naming Molecules

Molecular Compounds• Four of the many exceptions to naming rules:

water (H2O)ammonia (NH3)hydrogen peroxide (H2O2)methane (CH4)

• Prefixes are used to differentiate between molecules. ‐ The prefixes indicate the number of atoms present.

1 = mono 2 = di 3 = tri

4 = tetra 5 = penta 6 = hexa 7 = hepta

8 = octa 9 = nona 10 = deca

• If there is only one atom of the first element listed, the prefix MONO is not needed.

p. 204 #1,2,5,6

p. 204 # 1, 2, 5, 61. How can you tell the difference between ionic compounds and

molecular compounds?

2. a) What kinds of atoms form molecular compounds?b) How do the atoms in molecular compounds form stable electron configurations?c) What type of bond holds atoms together in molecules?

5. Name the following compounds, using prefixes:a) CBr4 b) NI3 c) OF2 d) SiCl4

6. Write chemical formulas for and name the molecular compounds forms by the following pairs of elements.a) silion & oxygen b) nitrogen & hydrogenc) phosphorus & chlorine d) sulfur & brominee) oxygen & fluorine f) carbon & chlorine


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Organic Compounds

Organic Compounds• Organic compounds are molecular compounds that contain carbon atoms as the “backbone” of the structure.

• The simplest organic molecule is methane (CH4) because it only has one carbon.

• Many naturally occurring organic compounds come from plants (ex. carbohydrates such as cellulose, starch, glucose, etc.).

Hydrocarbons

Organic Compounds• Hydrocarbons are organic compounds that are made of hydrogen and carbon only and are found in various combinations.

o A mixture of hydrocarbons makes up fossil fuels like oil and natural gas.

p. 207 #15

p. 207 #1‐51. a) What are organic compounds?

b) What are the most common elements present in organic compounds?c) What is the combining capacity of carbon?d) Why is carbon called the backbone of organic molecules?

2. What are two sources of different kinds of organic compounds?

3. a) What elements are present in hydrocarbon molecules?b) How are hydrocarbons produced naturally?

4. a) What is meant by the term "fossil fuel"?b) Name three examples of fossil fuels.

5. Give five uses for natural gas and petroleum products.


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Mar 1010:14 AM

Total Mass (g) (reactants and apparatus )

PREDICTION (g)

(mass of products and apparatus)

Total Mass (g)

(products and apparatus )

QUALITATIVE observations of reactants and productsiron (III) chloride

sodium hydroxide

Qualitative observations of reaction

iron (III) hydroxide

sodium chloride

Table 1. Measuring Masses in a Chemical Reaction

Conservation of Mass

Chemical Reactions ‐ EQUATIONS• The Law of Conservation of Mass states that, in a chemical reaction, the total mass of the reactants (starting materials) is always equal to the total mass of the products (the materials produced).

MASS OF REACTANTS = MASS OF PRODUCTS

o Example: methane + oxygen à water + carbon dioxide

o Total mass = 10g total mass = 10 g total mass

o What would happen if a gas was produced?

Word Equation

Chemical Reactions ‐ EQUATIONS• A word equation is a chemical reaction represented by the names of the substances involved; it indicates what reacts and what is produced.

copper + silver nitrate à silver + copper (II) nitrate

o Left side = reactants; Right side = productso An arrow points from the reactants toward the productso Each reactant and each product is separated by a plus (+) sign


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Skeleton Equation

Chemical Reactions ‐ EQUATIONS• A skeleton equation is a chemical reaction represented by formulas of the reactants instead of the chemical names.

copper + silver nitrate à silver + copper (II) nitrate

Cu + AgNO3 à Ag + CuNO3

iron + oxygen à iron(III) oxide

zinc + hydrochloric acid à hydrogen + zinc chloride

hydrogen + oxygen à water vapour

p. 219 #24

p. 219 #2‐42. Examine the following word equation:

propane + oxygen à carbon dioxide + watera) List all the reactants in this reaction

b) List all the products in this reaction

c) What is the purpose of the arrow in the word equation?

3. Write word equations for the following reactions:a) CaCl2 and Na2SO4 react to form CaSO4 and NaCl

b) BaCO3 reacts when heated to produce BaO and CO2

c) AgNO3 reacts with KCl to produce AgCl and KNO3

4. Write word equations to represent the following chemical reactions:a) Carbon dioxide and water are produced in human cell respiration. The reactants are sugar and an important gas that humans need to survive.

b) Stalactites form in caves when calcium bicarbonate reacts to form calcium carbonate, water, and carbon dioxide gas.

Balanced Equation

Chemical Reactions ‐ EQUATIONS• A balanced chemical equation is a skeleton equation with coefficients in front of certain reactants and/or products to ensure that there are an equal number of atoms of each type on each side of the arrow.

CH4 + 2O2 à 2H2O + CO2


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Chemical Equations

Chemical Reactions ‐ EQUATIONS• Steps to writing balanced chemical equations:

iron + oxygen à iron oxide

1. Write the skeleton equation

Fe + O2 à Fe3O4

2. Count the # of atoms of each type in reactants & products

Atom Reactants ProductsFe 1 3O 2 4

3. Multiply each of the formulas by the appropriate coefficients to balance the number of atoms.

3Fe + 2O2 à Fe3O4

Apr 141:46 PM

p. 229 #23

p. 229 #2,32. Copy the following skeleton equations into your notebook, then

balance the equations.a) Na + Cl2 à NaCl b) K + O2 à K2O

c) H2 + O2 à H2O d) H2 + Cl2 à HCl

e) N2 + H2 à NH3 f) CO + O2 à CO2

g) Al + Br2 à AlBr3 h) N2H4 + O2 à H2O + N2

i) CH4 + O2 à CO2 + H2O

3. For each of the following, write the correct skeleton equation, and then balance it to form a chemical equation:a) copper(II) oxide + hydrogen à copper + water

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

c) calcium + water à calcium hydroxide + hydrogen gas

d) lead(II) sulfide + oxygen à lead + sulfur dioxide

e) hydrogen sulfide à hydrogen + sulfur


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Types of Reactions

Chemical Reactions ‐ TYPES• There are five main types of chemical reactions:

CDAB AC BD

Double Displacement

BC ACA B

Single Displacement

AAB BDecomposition

A B ABSynthesis

Combustionfuel + oxygen oxides + energy

Types of Reactions

Chemical Reactions ‐ TYPES• There are five main types of chemical reactions:

Double Displacement

Single Displacement

DecompositionSynthesis

Combustionthe explosive relationship

the hook‐up the break‐up

the other man/woman the full switcheroo

Combustion

Chemical Reactions ‐ TYPES1. Combustion Reaction§ Often called burning , it is the very rapid reaction of a substance with oxygen to produce oxides.§ Energy is produced, mainly in the form of heat and light.§ NOTE: When hydrocarbons burn (i.e. react with oxygen)

they always produce carbon dioxide & water. § When oxygen is a reactant and the products are carbon

dioxide and water, it is a combustion reaction.§ Example: C3H8 + 5O2 à 3CO2 + 4H20


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Synthesis

Chemical Reactions ‐ TYPES2. Synthesis Reaction§ Also called formation reactions.§ Two or more smaller compounds combine to form a larger

compound (ex. A + B à AB).

§ Example: H2 + O2 à H2O(balanced chemical equation: 2H2 + O2 à 2H2O)

§ Example: CO2 + H2O à H2CO3 (aq)

Decomposition

Chemical Reactions ‐ TYPES3. Decomposition Reaction§ Opposite of synthesis reactions.§ A larger compound decomposes into elements or smaller

compounds (ex. AB à A + B).

§ Example: H2O à H2 + O2(balanced chemical equation: 2H2O à 2H2 + O2)

§ Example: 2NI3 à N2 + 3I2§ Example: NH4NO3 à N2O + 2H2O

Single Displacement

Chemical Reactions ‐ TYPES4. Single Displacement Reaction§ One element displaces or replaces another element in a

compound.§ A cation will only switch with the other cation, or an anion

will only switch with the other anion.§ Example: A' + AB à A + A'B

B' + AB à B + AB'§ Example: Mg + 2AgNO3 à 2Ag + Mg(NO3)2§ Example: Br2 + CaI2 à I2 + CaBr2


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Double Displacement

Chemical Reactions ‐ TYPES5. Double Displacement Reaction§ Different elements displace each other or exchange places to

form two new compounds.§ The cations will pair up with the anions of the other

compounds.§ Example: AB + A'B' à AB' + A'B§ Example: Pb(NO3)2 + 2KI à PbI2 + 2KNO3

p. 247 15

p. 247 #1‐51. What do synthesis and single displacement reactions have in common?

2. What do decomposition and double displacement reactions have in common?

3. Which two types of reactions seem to be opposites?

4. Identify each of the following reactions as one of the types of reactions:a) barium + sulfur à barium sulfide

b) bromine + sodium iodide à iodine + sodium bromine

c) barium nitrate + sodium sulfide à barium sulfide + sodium nitrate

d) lithium carbonate à carbon dioxide + lithium oxide

e) lead(II) oxide à lead + oxygen

f) calcium + water à hydrogen + calcium hydroxide

g) sulfur trioxide + water à sulfuric acid

5. Write skeleton and balanced chemical equations for each of the reactions in question 4.

Jan 282:41 PM

1. chemical reactions printable slides part...

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