chemical reactions and equations chemistry ms. wack
TRANSCRIPT
CHEMICAL REACTIONS AND EQUATIONS
CHEMISTRY
MS. WACK
CHEMICAL REACTIONS
In a chemical reaction, bonds are broken,
atoms are rearranged, and new bonds are
formed.
• Something “new” is produced.
H2 + O2 H2O
Clues that a chemical reaction has occurred:
• Odor
• Formation of a gas (may see bubbles)
• Precipitate formation
• Color Change (not always)
• New substances formed
• Energy is absorbed or released (not always)
General Description of a Chemical Reaction
Reactants Products
Word Equations : Use words and symbols to represent chemical reactions.
•Uses words and symbols to describe a chemical reaction
•Common symbols used:
(s) solid (l) liquid (g) gas (aq) aqueous—dissolved in water
heat is added to the reaction reversible reaction
a catalyst is added to the reactioncatalyst
+ separates reactants or separates products yields/produces
The starting substances in a
chemical reaction
The substances formed in a
chemical reaction
Write the word equations for the following
chemical reactions:
• Hydrogen gas reacts with chlorine gas to produce hydrogen chloride, a gas with a sharp odor.
• Calcium oxide is produced when a piece of calcium is burned in oxygen.
Word Equations
HYDROGEN + CHLORINE HYDROGEN CHLORIDE
CALCIUM + OXYGEN CALCIUM OXIDE
CHEMICAL EQUATIONS
• Formula Equations: Use chemical formulas and symbols to represent a chemical reaction.
– Keys to writing formula equations:• Write the word equation first—then, replace the words with
chemical formulas.• Make sure your formulas are correct!!!!!• Make sure that each element in the reactants is also in the
products and vice versa.• The arrow must always go to the right.
Write the formula equation for the
reaction of calcium burning in oxygen to
produce calcium oxide.
CHEMICAL EQUATIONS
LAW OF CONSERVATION OF MASS
• How does this law affect chemical equations?– The mass of the reactants must equal the mass of the products– The # of atoms of each element must be equivalent on both
sides of the reaction– Chemical reactions must be balanced
What are the #’s called?
Mg+2
2H2O 2H2 + O2
superscript
subscript coefficient
BALANCING EQUATIONS
Cd + HCl CdCl2 + H2
BALANCING EQUATIONS
MnSO4 MnO + SO3
H2SO4 + NaOH Na2SO4 + H2O
BALANCING EQUATIONS
+ +
Co + O2 Co2O3
BALANCING EQUATIONS
Write a balanced chemical equation for the
reaction in which magnesium reacts with nitrogen
to produce magnesium nitride.
BALANCING EQUATIONS
Write a balanced chemical equation for the combustion of methane (CH4) in oxygen to
produce carbon dioxide and water.
BALANCING EQUATIONS
Sodium phosphate is used to cut grease. Write a balanced equation for the reaction in which iron(II) chloride reacts with sodium phosphate to produce sodium chloride and
iron(II) phosphate.
BALANCING EQUATIONS
Magnesium metal and water combine to form solid magnesium hydroxide and hydrogen gas.
BALANCING EQUATIONS
HEAT IN CHEMICAL REACTIONS
• Most chemical reactions involve changes in energy.– The unit for energy is the Joule (J)
• This is because bond breaking requires energy and bond forming releases energy.
• Almost all chemical reactions either release or absorb energy
• This energy flow results in heat, either being absorbed or released.
EXOTHERMIC REATIONS• To the touch an exothermic reaction would
feel HOT because heat is being released to the surroundings
• In a chemical reaction that is exothermic, the energy would be represented in the chemical equation on the product side of the reaction (heat is formed/released).– C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g) + 2043 kJ
ENDOTHERMIC REACTIONS
• To the touch an endothermic reaction would feel cold because heat is being absorbed from the surroundings.
• In a chemical reaction that is endothermic, the energy would be represented in the chemical equation on the reactants side of the reaction (since heat is being absorbed/taken in).– C(s)+H2O(g) +113 kJ CO(g)+H2(g)
Identify each of the following reactions as either an endothermic reaction or an exothermic reaction.
a ) C2H4 2C + 2H2 + 52.3 kJ
b) B2H6 + 6H2O 2H3BO3 + 6H2 + 493.4 kJ
c) 2Fe + 3CO2 + 26.8 kJ Fe2O3 + 3CO
d) Br2 + Cl2 + 29.4 kJ 2BrCl
5 MAIN CLASSIFICATIONS OF CHEMICAL REACTIONS
• Synthesis Reactions
• Decomposition Reactions
• Combustion Reactions
• Single-Replacement Reactions
• Double-Replacement Reactions
Synthesis Reactions
• Always Have: 1 Product• General Format: A + B AB• Predicting the Product:
– The reactants come together to form one product
• If the reactants are a metal & a nonmetal then they will form an ionic compound—get the charges & crisscross
• If they are not, the product will be given
Examples of Synthesis Reactions
• Na + Cl2
Examples of Synthesis Reactions
• H2 + O2
• Al + S
Decomposition Reactions
• Always Have: 1 Reactant• General Format: AB A + B• Predicting the Product: Separate the
reactant into its elements• Example of Decomposition:
C6H12O6 C + H2O
Examples of Decomposition
• MgS
• Li2O
Combustion ReactionsCombustion Reactions
• Always have: Oxygen (O2) as a reactant
• General Formats:– CxHy + O2 CO2 + H2O
– A + O2 AxOy
• Predicting the product: – If its combustion between a hydrocarbon & oxygen
the reaction will produce CO2 & H2O
– If its combustion between an element and oxygen it is a synthesis reaction—get your charges and crisscross
COMBUSTION REACTIONS
• Always has elemental oxygen (O2) as one of the reactants
• Example: – Burning of methane:
• CH4 + O2 CO2 + H2O
– Burning of propane• C3H8 + O2 CO2 + H2O
– Synthesis of sodium oxide• Na + O2 Na2O
Examples• C2H2 + O2
• Na + O2
Single Replacement Reactions
• Always have: 1 element and 1 compound as the reactants and as the products
• General Format: A + BC B + AC• Activity Series: Lists the elements in order of their
reactivity. The more reactive elements can replace the less reactive elements– Elements higher on the list can replace elements lower on the
list
Which element can replace the other in a chemical reaction?
• Tin or Barium
• Iodine or Bromine
Single Replacement Reactions
• General Format: A + BC B + AC• Predicting the Product: If the single
element is more reactive than the similar element in the compound, those two elements will switch spots. This will form an element and a new ionic compound.
Examples of Single Replacement Reactions
• Zn + Cu(NO3)2
• Cu + Zn(NO3)2
• Cu + AgNO3
More examples of Single Replacement Reactions
• Zn(s) + H2SO4(aq)
• Na(s) + H2O(l)
• Sn(s) + NaNO3(aq)
• Cl2(g) + NaBr(aq)
Double Replacement Reactions
• Always have: 2 compounds in the reactants (typically ionic compounds) and 2 compounds in the products
• General Format: AX + BY BX + AY• Double replacement reactions occur if one of the
products will be a molecular compound (such as H2O), a precipitate or a gas.
• Predicting the product: The metals will switch places—get the charges and crisscross– Types of products: water, gas, or precipitate
+ +
Double Replacement Reactions
+ +
• Precipitate: An insoluble solid formed from two aqueous solutions.
SOLUBILITY RULESSolubility Rules: On the solubility chart on back of your
periodic table:
“s” = precipitate, “aq” = aqueous (not a precipitate)GENERAL
SOLUBILITY RULES
Examples of Double Replacement Reactions
• BaCl2(aq) + K2CO3(aq)
• FeS(s) + HCl(aq)
• CaCO3 + HCl
DISSOCIATION
• Double replacement reactions occur between 2 ionic compounds in aqueous solution.– When ionic compounds dissolve in water, they
dissociate into the cation and anion of the compound.
• DISSOCATION: The separation of ions that occurs when an ionic compound dissolves
Complete Ionic Equation
An equation that shows dissolved ionic compounds as dissociated free ions.
Chemical Equation:
AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
Complete Ionic Equation:Ag+(aq) + NO3
-(aq) + Na+(aq) + Cl-(aq) AgCl(s) + Na+(aq) + NO3-(aq)
Net Ionic Equation
An equation for a reaction in solution that shows only those particles that are directly involved in the
chemical change.
A net ionic equation shows only the particles involved in the reaction and is balanced with respect to both mass and
charge.
Spectator Ion: An ion that appears on both sides of an equation and is not directly involved in the reaction.
Chemical Equation:
AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
Complete Ionic Equation:Ag+(aq) + NO3
-(aq) + Na+(aq) + Cl-(aq) AgCl(s) + Na+(aq) + NO3-(aq)
Any ions that appear on both sides, cross out, they are spectator
ions and are not involved in the chemical reaction.
Net Ionic Equation: The ionic equation rewritten without the spectator ions.
Ag+(aq) + Cl-(aq) AgCl(s)
Once the net ionic equation is written, make sure all atoms are balanced and all charges are balanced.
Example 1
Chemical Equation:
Pb(s) + AgNO3(aq) Ag(s) + Pb(NO3)2(aq)
Complete Ionic Equation:
Net Ionic Equation:
Once the net ionic equation is written, make sure all atoms are balanced and all charges are balanced.
Example 2
Chemical Equation:
FeCl3(aq) + KOH(aq) Fe(OH)3(s) + KCl(aq)
Complete Ionic Equation:
Net Ionic Equation:
Once the net ionic equation is written, make sure all atoms are balanced and all charges are balanced.
Example 3
Word Equation:
sodium carbonate + barium nitrate
Chemical Equation:
Complete Ionic Equation:
Net Ionic Equation:
Once the net ionic equation is written, make sure all atoms are balanced and all charges are balanced.
Exceptions to the Rules
• Many synthesis reactions are also combustion reactions but not all combustion reactions are synthesis reactions
• There are other reactions that do not fit neatly into 1 of the 5 categories.
5 GENERAL FORMATS• Synthesis: A + B AB
– 1 product
• Decomposition: AB A + B– 1 reactant
• Combustion: CxHy + O2 CO2 + H2O X + O2 XyO
– O2 is one of the reactants
• Single Replacement: A + BC B + AC– 1 element + 1 compound on both sides of the rxn
• Double Replacement: AB + CD CB + AD– 2 compounds on both sides of the rxn