writing simple chemical equations
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Writing Simple Chemical Equations. Balancing and Classification of Reactions. Chemical Reactions. Balanced c hemical equations represent chemical reactions A substance which undergoes a chemical change has taken part in a chemical reaction - PowerPoint PPT PresentationTRANSCRIPT
Writing Simple Chemical Equations
Balancing and Classification of Reactions
Chemical Reactions• Balanced chemical equations represent
chemical reactions• A substance which undergoes a chemical
change has taken part in a chemical reaction• Remember the differences between chemical
and physical change?Chemical Change Physical Change
Burning Melting
Rusting Freezing
Signs of a Chemical ReactionIndicators of a probable
chemical reaction– These may be present in some
physical changes too
1. Color Changes2. Precipitation of a solid from a
solution3. Energy changes, heat or light
absorbed or released4. Odor Changes; like baked bread5. Gas release- sometimes occurs
in physical change too
Mini-Lab 6.1 Energy ChangeQuestion: How can we observe energy changes?Background Information: • All chemical reactions involve an energy
change. • Sometimes the change is so small that special
detection instruments are needed to observe it.
• Sometimes they can be observed easily. • Light, heat, sound, kinetic and potential are all
forms of energy.
Mini-Lab 6.1 Energy ChangeProcedure: 1. Place 25g of iron powder and 1g of NaCl
in a reseal able bag2. Add 30g of vermiculite to bag, seal bag
and shake3. Open bag and add 5ml of water, reseal
and shake gently4. Hold bag in your hands, note any
changes you observe
Mini-Lab 6.1 Energy Change
Analysis: (answer the following in your notebook1. Did you observe energy changes? If so,
describe them2. Did a chemical reaction take place? What
kind of reaction?3. Can you think of anytime in the real world,
where this reaction might be useful? Explain
Exothermic Reaction
The Reaction has as one of the products, energy, in the form of heat!
Endothermic ReactionsThese reactions use energy from the surroundings, in the form of heat, as one of the reactants; creating a cold product!
Chemical Equations1. Describe all changes
that take place2. Identify the
substances that react
a. Called Reactants3. Identify the
substances formeda. Called Products
• Reactants: Iron and Oxygen
• Product: Iron(III) Oxide Rust
The Description of Changes• More than what can be observed• Ex. “bubbles are formed”, does not tell what gas is
formed • A Chemical Equation is how we represent the
changes taking place in a reaction• Word equations are the simplest way to
describe reactants and products• An arrow, between reactants and products,
represents change• + signs are used to separate reactants and to
separate products
Word Equations• Example:
The combining of Vinegar (acetic acid) and Baking soda results in a vigorous reaction, forming a bubbly product
The word equation: Vinegar + Baking Soda Sodium acetate + water +
Carbon Dioxide
Chemical Equations• Shorter than word equations • more exact and specific• Replace the names of the substances with their
chemical formulasExample: (the previous reaction) HC2H3O2 + NaHCO3 NaC2H3O2 + H2O + CO2(Vinegar) Sodium Sodium Acetate water Carbon dioxideAcetic acid Hydrogen
Carbonate
• By examining the equation you can determine EXACTLY what elements are involved and how many atoms of each
Balancing Chemical EquationsWhat is Balancing Equations?• Ensuring every atom in the reactants is present in the products in the same number and type!Why?
Law of Conservation of Matter: matter is neither created or destroyed, just transformed from one form to another
No creation, no destruction, just rearrangement!
Same Number and Type of Atoms
Balancing Chemical EquationsSteps of process:1. Write the chemical equation with all reactants on
one side, separated by a (+) sign 2. Draw an arrow pointing toward the products , also
separated by a (+) sign. (recall diatomic elements)3. Add symbols next to each compound, indicating
physical state of matter (solid-s, liquid-l, gas-g)4. Count the numbers of each type of element from
each side of the equation. 5. List the symbols and numbers of each.6. Change the coefficients as needed to ensure
conservation of matter. (numbers and types equal)
Example of Process• Chemical equation for aqueous magnesium chloride
plus silver nitrate solution making aqueous magnesium nitrate and solid silver chloride:
• Add symbols for physical state
• MgCl2(aq) + AgNO3(aq) Mg(NO3)2 (aq) + AgCl(s)
• Count number and type of elements on each side
Matter is not conserved! Numbers are different!
Atoms in Reactants Atoms in Products
Mg- 1 Mg- 1Cl- 2 Cl- 1Ag- 1 Ag- 1N-1 N-2O- 3 O- 6
Last StepChange the coefficients as needed to ensure
conservation of matter. MgCl2(aq) + AgNO3(aq) Mg(NO3)2 (aq) + AgCl(s)Atoms in reactants Atoms in products Mg- 1 Mg- 1 Cl- 2 Cl- 1 -2 Ag- 1 -2 Ag- 1 2 N-1 - 2 N-2 O- 3 -6 O- 6 How can I change the coefficients to make then the same?1. A 2 added before the AgNO3(aq) in the reactants, will balance both N and O2. Another 2 added before AgCl(s) in the products will balance both the Ag and
Cl
MgCl2(aq) + 2 AgNO3(aq) Mg(NO3)2 (aq) + 2 AgCl(s)
Write a Balanced Equation for Each of These Reactions
1. Sodium metal + chlorine gas sodium chloride crystals2. Propane gas + oxygen carbon dioxide + water + energy3. Zinc metal + hydrochloric acid zinc chloride solution +
hydrogenRemember: • use the oxidation numbers to construct octets and
determine formula compounds• Use your reference sheets for names of ionic substances
and covalent molecules. (check for diatomic molecules)
Answers
1. balance equations for ppt #1.docx2. balance equations for ppt #2.docx3. balance equations for ppt #3.docx
Let’s Use the Internet to Help us Practice!
• Using a computer, Your Brain and your Newly Acquired Skills, practice balancing – Complete at least 10 equations from the beginner level,
then 10 at the intermediate level.– Then try 2 or three advanced ones!
• Track your progress and record the number of trials it took for each equation in your notebook!
• Complete an exit ticket, indicating how many tries it took for each equation
• Leave your exit ticket on the laptop cart when you have put your computer away properly!
More Balancing!• Access the Following Site:• http://education.jlab.org/elementbalancing/index.html1. At least 10 Beginner equations and 10 Intermediate!
Beginner level
Number of trials
Intermediate level
Number of Trials
1 1
2 2
3 3
4 4
5 5
6 6
7 7
8 8
9 9
10 10
Advanced Level
Number of Trials
123
Exit Ticket1. Complete an exit ticket, indicating how many
tries it took for each equation.
2. Leave your exit ticket on the front table AFTER you have put your computer away properly!
Name___________________ EXIT TICKET Total number of beginner equations you tried _____Total number of trials on beginner equations ______Total number of intermediate equations you tried ______Total number of trials on intermediate equations ______How many advanced equations did you try?How well do you understand this process? Not at all, A little, mostly, I got it!
Other Sites You Can Use To Practice
• http://chemistry.csudh.edu/lechelpcs/rxnbalancingcsn7.html (pretty good, hard but shows solutions after 3 tries)
• http://funbasedlearning.com/chemistry/chemBalancer
• http://www.sciencegeek.net/Chemistry/taters/EquationBalancing.htm (All at Once)
Types Of Reactions• There are 5 major types of chemical
reactions1. Synthesis2. Decomposition3. Single displacement4. Double displacement5. Combustion
• Reactions can be categorized by recognizing patterns which occur.
Synthesis• Pattern to recognize synthesis• Whenever two or more substances
combine to form a single product, the reaction is synthesis.
Decomposition• Pattern to recognize synthesis• Whenever a compound is broken down into
two or more simpler substances it is a decomposition reaction.
Single-Displacement Reaction• Pattern to recognize single displacement• Whenever one element takes the place of
another in a compound, it is a single displacement reaction.
Let’s Classify these reactions!
1. 2 Na + Cl2 2NaCl2. PCl5 PCl3 + Cl2
3. 2Al + Fe2O3 2Fe + Al2O3
4. 2Ag2O 4Ag + O2
5. Cl2 + 2KBr 2KCl +Br2
6. CaO + SiO2 CaSiO3
Answers1. 2 Na + Cl2 2NaCl 2 substances combine so it is synthesis!2. PCl5 PCl3 + Cl2
A single compound is broken down into two simpler substances- it is decomposition!
3. 2Al + Fe2O3 2Fe + Al2O3
One element takes the place of another, it is single displacement!
Answers Continued
4. 2Ag2O 4Ag + O2
Decomposition5. Cl2 + 2KBr 2KCl +Br2
Single-displacement6. CaO + SiO2 CaSiO3
Synthesis
Double-Displacement Reactions• Pattern to recognize a double-displacement• Whenever the positive ions of two ionic
compounds are interchanged, it is a double displacement reaction.• At least one product must be a precipitate of
water!
Combustion Reaction• Pattern to recognize combustion• Whenever a substance combines rapidly
with OXYGEN to form one or more oxides, is a combustion reaction.
Let’s Apply what we have learned!
• Classify these reactions:1. PbCl2 + Li2SO4 PbSO4 + 2LiCl2. CH4 + 202 CO2 + 2H2O3. C6H1206 + 602 6CO2 + 6H2O4. BaCl2 + H2SO4 2HCl +BaSO4
Answers1. PbCl2 + Li2SO4 PbSO4 + 2LiCl Interchanged
cations, so Double-displacement2. CH4 + 202 CO2 + 2H2O substance combines with
Oxygen and forms an oxide, so Combustion3. C6H1206 + 602 6CO2 + 6H2O Combustion4. BaCl2 + H2SO4 2HCl +BaSO4 Double-
displacement
Compare and Contrast Types Of ReactionsReaction Type General Equation
Synthesis Element/compound + Element/compound compoundExamples: 2 Na + Cl2 2NaCl CaO + SiO2 CaSiO3
Decomposition Compound two or more elements/compoundsExamples: PCl5 PCl3 + Cl2
2Ag2O 4Ag + O2
SingleDisplacement
Element a + compound bc element b + compound acExample: 2Al + Fe2O3 2Fe + Al2O3
Cl2 + 2KBr 2KCl +Br2
DoubleDisplacement
Compound ac + compound bd compound ad + compound bcExample: PbCl2 + Li2SO4 PbSO4 + 2LiCl BaCl2 + H2SO4 2HCl +BaSO4
Combustion Element/Compound + Oxygen OxideExample: CH4 + 202 CO2 + 2H2O C6H1206 + 602 6CO2 + 6H2O
Factors that Affect Direction Of Reactions• External factors modify the direction of
reactions• Many can change direction: Called Reversible– Like charging and draining a battery
• Adding or removing energy as heat can affect direction– Endothermic reactions; added heat pushes reaction
to the right– Exothermic reactions; added heat pushes the
reaction to the left
Reversibility of Reactions• Not all reactions are reversible– Like fuel burns, food is digested and paint hardens– New products are formed and at least one reactant is
used up• Some reactions automatically reverse to establish
equilibrium– No net (overall) change– Reactants and products change place, forming at about
the same rate– Reactants are never used up because they are always
being used then reformed from products– Ex. CaCo3 CaO + CO2
Initiating a Reaction• For a reaction to occur, particles must collide
with sufficient force to cause electrons to rearrange.
• The amount of energy needed to cause a reaction is called Activation Energy– Slow reactions have high activation energy
• To determine reaction rate, measure how quickly one reactant disappears or one product appears
• Factors which affect Rate of Reaction
Factors that Affect Rate Of Reactions1. Temperature; most reactions speed up
with higher temp2. Concentration; raising the concentration
of a reactant can speed up a reaction3. Catalysts; speeds up rate w/out being
changed by the reaction (enzymes in cells)
4. Inhibitor; slows down a reaction (preservatives)