Chemical Equations and ReactionsChemical Reaction: one or more substances are changed

into one or more different substanceOriginal substances- reactantsNew stuff- products

Indication of a Chemical Reaction:

1) Evolution of heat or light

2) Production of a gas

3) Formation of a precipitate (a solid that is produced during a chemical reaction

4) Color change

5) Odor production

Chemical Equations• The law of conservation of mass must be satisfied• Coefficients: small whole number that appears in front of a

formula in a chemical equation• Word equation:

methane + oxygen carbon dioxide + water• Formula equation:

CH4(g) + O2(g) CO2(g) + H2O(g) (not balanced) CH4(g) + 2O2(g) CO2(g) + 2H2O(g) (balanced)

• Balancing: make sure that the number of moles of an element are equal on both sides of the equation

• Catalyst: substance that a changes the rate of a chemical reaction but can be recovered unchanged.

Symbols used in Chemical Equations

Yeilds reversible reaction (s) a solid (l) a liquid (g) a gas(aq) aqueous solution (dissolved in water)

a gas a precipitateheat reactants are heated MnO4 formula of a catalyst used to alter the rate2 atm pressure at which the reaction is carried out 0 C temperature at which the reaction is carried out

H2 + Cl2 2HCl1 mol H2 1 mol Cl2 2 mol HCl 2.02 g H2 70.90 g Cl2 2 x 36.46 = 72.92 g HCl

Diatomic molecules: H2, F2, Cl2 , Br2, I2, O2, N2

Balancing:

1) write out word equation is the problem is a written

2) balance atoms one at a time

3) first balance atoms that are combined into a formula

4) then balance polyatomic ions

5) Balance H atoms and O atoms after all other elements are balanced

6) Check the number for all atoms on both sides!! They have to be equal

Types of Chemical ReactionsCombustion Reactions: substance combines with oxygen,

releasing a large amount of energy (light/ heat)- Carbon Compounds + O2 : always get CO2 + H2O C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g)

Synthesis Reaction: (composition reaction) two or more substances combine to form a new compound.

A + X AX

• Reactions of elements with Oxygen and Sulfur:- 2Mg(s) + O2(g) 2MgO(s)

• Metals and Halogens : - 2Na(s) + Cl2(g) 2NaCl(s)

• Metal Oxides and Water: CaO(s) + H2O(l) Ca(OH)2(s)

Decomposition Reaction: single compound breaks down into two or more simpler substances- Opposite of synthesis reaction- usually only takes place if energy (electricity/ heat) is added AX A + X

• Electrolysis: decomposition of a substance by an electric current

• If H in the compound you get H2OIf C in the compound you will get CO2

If O and no H or C, then you get O2

• H2SO3 SO2 + H2O

Single Replacement (displacement) Reaction: when one element replaces a similar element in a compound A + BX AX + B Y + BX BY + X

• Mg(s) + 2HCl(aq) H2(g) + MgCl2(aq)

• Group 1 & 2 metals + H2O metal hydroxides + H2(g)

• d-block metal + H2O metal oxides + H2(g)

Double Replacement Reactions: ions of 2 compounds exchange places in an aqueous solution to form new AX + BY AY + BX

• FeS(s) + 2HCl(aq) H2S(g) + FeCl2(aq)

Solubility Rules• 1. Alkali metals (gr. 1) and Ammonium compounds are soluble in water (aq).• 2.  Nitrates, acetates, and chlorates are soluble (aq).• 3. Most chlorides, bromides, and iodides are soluble (aq), except those of

silver, mercury (I), and lead (s)• 4. Most sulfates are soluble (aq), except those of barium, strontium, calcium,

lead, and mercury (s).• 5.  Most carbonates, phosphates, and sulfites are insoluble (s), except those of

alkali metals (gr. 1) and ammonium (aq). • 6.  Most sulfides are insoluble (s), except those of calcium, strontium, alkali

metals (gr.1) and ammonium (aq). • 7. Most oxides are insoluble (s), except those of calcium, barium, and alkali

metals (gr. 1) and ammonium (aq)• 8. Most hydroxides are insoluble (s), except those of barium, and alkali

metals (gr. 1) and ammonium (aq)

Solubility Examples

Ex: Predict compounds, solubility, and then balance

1. (NH4)2S (aq) + Cd(NO3)2 (aq)

 

2. Mercury (II) chloride (aq) + potassium sulfide (aq)  

 

3. Sodium carbonate (aq) + calcium chloride (aq)  

Activity Series• Activity: ability of an element to react• the more an element reacts with other substances, the greater

the activity is.• Metals: the greater the activity, the greater it loses electrons

(to form cations) • Non-metals: the greater the activity, the greater it gains

electrons (to form anions) • Activity series: a list of which elements a particular element

can replace in a single replacement reaction - predicts whether or not a chemical reaction will occur 2Al(s) + 3ZnCl2(aq) 3Zn(s) + 2AlCl3(aq)Co(s) + 2NaCl(aq) no reaction

 

React vigorously with Acids to produce H2 gas

 

React with Acids to produce H2 gas

Do not react with Acids

Li  MOST REACTIVE

React vigorously with liquid water to form H2 gas

    

 

React slowly with liquid water but readily with steam to form H2 gas

   

      

 

 LEAST REACTIVE

K

Ba

Ca

Na

 

Mg

Al

Zn

Cr

Fe

Cd

Co

Ni

Sn

Pb

 

H2

 

Cu

Hg

Ag

Au

Oxidation Numbers- used for covalent bonds and instead of charges (ions)1) Atoms of a pure element have an oxidation number

“0”. Pure Na or O2 have an oxidation # equal to “0”2) More electronegative element has oxid # = to its

charge (if it were an anion). Least electronegative element has oxid # = to its charge (if it were a cation).

3) Oxygen is -2, except when it is O2, then it is -14) Hydrogen is +1, except when with a metal, it is -15) the sum of the oxid. #s is equal to zero (neutral),

except for a polyatomic ion, when the sum is equal to the ion’s overall charge. (NO3

-1)

Redox Reactions• Reduction and Oxidation Reactions• Reduction Reaction: gain electrons

– Gaining electrons results in a more negative charge and therefore reduced! GER

– Cl2 + 2e- 2Cl- , the chlorine diatomic molecule goes from oxidation state 0 to a chlorine ion with a –1 charge

• Oxidation Reaction: lose electrons– Losing electrons results in less negative charge LEO

– Increase in oxidation state (charge) because more positive (ie. Less negative)

– Na Na+ + e- , sodium goes from oxidation state 0 to a sodium ion with a +1 charge

• Reduction: when an atom/molecule turns into a negative ion it is reduced, made more negative.

• Oxidation: when an atom of/molecule turns into a positive ion it is oxidized, made more positive.

• H2 + Cl2 2HCl0 0 +1 -1

• 2H2O + 2Cl2 4HCl + O2

• Academic: look in book for examples and go over on board.

StoichiometryGrams X (molar mass) mol X

mol X (mol ratio) mol Y

mol Y (molar mass) grams Y• Mole ratio: conversion factor that relates the amounts in

moles of any two substances involved in a chemical reaction

• 2Al2O3(l) 4Al(s) + 3O2(g)

2 mol Al2O3 or 4 mol Al 4 mol Al 2 mol Al2O3

3 mol O2 or 2 mol Al2O3

2 mol Al2O3 3 mol O2

Limiting Reactants• The reactant that limits the amounts of the other reactants

that can combine in a chemical reaction(it also limits the amount of product that can form)

• look at moles, not grams

Excess reactant: The substance that is not used up

• To determine the limiting reactant- must convert to moles

– moles for all substances must be for the same reactant

– convert moles of Y to moles of X, then compare to original moles of X

Percent Yeild

• The ratio of the actual yield to the theoretical yield• percent yield = actual yield x 100

theoretical yield• Given: the actual yield of a product

the mass (grams) of some reactant

1) first change the mass of reactant to grams of product using molar mass, then mole ratio, then molar mass

2) This will be theoretical yield