Chapter 10 Chemical Reactions

An equation Describes a reaction Must be balanced to follow the Law of Conservation of Mass Can only be balanced by changing the coefficients. Has special symbols to indicate state, and if catalyst or energy is required.

Reactions Come in 5 types. Can tell what type they are by the reactants. Single Replacement happens based on the activity series. A+BX AX+B Double Replacement happens if the product is a solid, water, or a gas. AX+BY AY+BX

Reactions Come in 5 types. Can tell what type they are by the reactants. Synthesis- A + B AB Combustion- Oxygen combines with substance. 2H2(g)+ O2(g) 2H2O(g) Decomposition- AB A + B

The Process 1. Determine the type by looking at the reactants. 2. Put the pieces next to each other based on type 3. Use charges to write the formulas Elements get 2? 4. Use coefficients to balance the equation.

All chemical reactions have two parts Reactants - the substances you start with Products- the substances you end up with The reactants turn into the products. Reactants ® Products

In a chemical reaction The way atoms are joined is changed Atoms aren’t created or destroyed. Can be described several ways In a sentence Copper reacts with chlorine to form copper (II) chloride. In a word equation Copper + chlorine ® copper (II) chloride

Symbols used in equations Table 11.1 the arrow separates the reactants from the products Read “reacts to form” The plus sign = “and” (s) after the formula -solid (g) after the formula -gas (l) after the formula -liquid

Symbols used in equations (aq) after the formula - dissolved in water, an aqueous solution. ­ used after a product indicates a gas (same as (g)) ¯ used after a product indicates a solid (same as (s))

Symbols used in equations indicates a reversible reaction (More later) shows that heat is supplied to the reaction is used to indicate a catalyst used in this case, platinum.

What is a catalyst? A substance that speeds up a reaction without being changed by the reaction. Enzymes are biological or protein catalysts.

Skeleton Equation Uses formulas and symbols to describe a reaction doesn’t indicate how many. All chemical equations are sentences that describe reactions.

Convert these to equations Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form solid iron (II) chloride and hydrogen sulfide gas.

Convert these to equations Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water.

The other way Fe(g) + O2(g) ® Fe2O3(s)

The other way Cu(s) + AgNO3(aq) ® Ag(s) + Cu(NO3)2(aq)

Balancing Chemical Equations

Balanced Equation Atoms can’t be created or destroyed All the atoms we start with we must end up with A balanced equation has the same number of atoms of each element on both sides of the equation.

® O + C O C O O C + O2 ® CO2 This equation is already balanced What if it isn’t already?

® C C O O C O C + C + O2 ® CO We need one more oxygen in the products. Can’t change the formula, because it describes what actually happens

® C C O C O C O + O Must be used to make another CO But where did the other C come from? Must have started with two C 2 C + O2 ® 2 CO

Rules for balancing Write the correct formulas for all the reactants and products Count the number of atoms of each type appearing on both sides Balance the elements one at a time by adding coefficients (the numbers in front) Check to make sure it is balanced.

Never Change a subscript to balance an equation. If you change the formula you are describing a different reaction. H2O is a different compound than H2O2 Never put a coefficient in the middle of a formula 2 NaCl is okay, Na2Cl is not.

Example R P H O 2 1 4 4 2 2 H2 + H2O O2 ® 2 H2 + H2O O2 ® The equation is balanced, has the same number of each kind of atom on both sides Recount Changes the O Make a table to keep track of where you are at Need twice as much O in the product Also changes the H Need twice as much H in the reactant

Example R P 4 2 H 2 4 2 O 1 2 This is the answer 2 H2 + O2 ® 2 H2O Not this 2 O 1 2

Examples CH4 + O2 ® CO2 + H2O

Examples AgNO3 + Cu ® Cu(NO3)2 + Ag

Examples Al + N2 ® Al2N3

Examples P + O2 ® P4O10

Examples Na + H2O ® H2 + NaOH

Techniques If an atom appears more than once on a side, balance it last. If you fix everything except one element, and it is even on one side and odd on the other, double the first number, then move on from there. C4H10 + O2  CO2 + H2O

Predicting the Products Types of Reactions Predicting the Products

Types of Reactions There are too many reactions to remember Fall into categories. We will learn 5 types. Will be able to predict the products. For some we will be able to predict whether they will happen at all. Must recognize them by the reactants

#1 Combination Reactions Combine - put together 2 elements, or compounds combine to make 1 compound. Ca +O2 ® CaO SO3 + H2O ® H2SO4 We can predict the products if they are two elements. Mg + N2 ®

Write and balance Ca + Cl2 ®

Write and balance Fe + O2 ® iron (II) oxide

Write and balance Al + O2 ® Remember that the first step is to write the formula Then balance Also called synthesis reaction

Combining two compounds If they tell you it is combination, you will make one product Two compounds will make a polyatomic ion. CO2 + H2O → H2O + Cl2O7→

#2 Decomposition Reactions decompose = fall apart one reactant falls apart into two or more elements or compounds. NaCl Na + Cl2 CaCO3 CaO + CO2

#2 Decomposition Reactions Can predict the products if it is a binary compound Made up of only two elements Falls apart into its elements H2O

#2 Decomposition Reactions HgO

#2 Decomposition Reactions If the compound has more than two elements you must be given one of the products The other product will be from the missing pieces NiCO3 NiO + H2CO3(aq)® CO2 +

#3 Single Replacement One element replaces another Reactants must be an element and a compound. Products will be a different element and a different compound. Na + KCl ® K + NaCl F2 + LiCl ® LiF + Cl2

Na + KCl ® K + NaCl Cl K Na

F2 + 2 LiCl ® 2 LiF + Cl2 Cl Li Li F F Cl Li Li

#3 Single Replacement Metals replace metals (and hydrogen) Al + CuSO4 ® Zn + H2SO4 ® Think of water as HOH Metals replace one of the H, combine with hydroxide. Na + HOH ®

#3 Single Replacement We can tell whether a reaction will happen Some are more active than other More active replaces less active There is a list on page 333

#3 Single Replacement There is a list on page 333 Higher on the list replaces lower. If the element by itself is higher, it happens, if element by itself is lower, it doesn’t

#3 Single Replacement Note the * H can be replaced in acids by everything higher Only the first 4 (Li - Na) react with water.

#3 Single Replacement Al + HCl ®

#3 Single Replacement Fe + CuSO4 ®

#3 Single Replacement Pb + KCl ®

#3 Single Replacement Al + H2O ®

#3 Single Replacement What does it mean that Ag is on the bottom of the list?

#3 Single Replacement Nonmetals can replace other nonmetals Limited to F2 , Cl2 , Br2 , I2 The order of activity is that on the table. Higher replaces lower. F2 + HCl ® Br2 + KCl ®

#4 Double Replacement Two things replace each other. Reactants must be two ionic compounds or acids. Usually in aqueous solution NaOH + FeCl3 ® The positive ions change place. NaOH + FeCl3 ® Fe3+OH- + Na+Cl- NaOH + FeCl3 ® Fe(OH)3 + NaCl

3NaOH + FeCl3 ® Fe(OH)3 + 3NaCl

#4 Double Replacement Will only happen if one of the products doesn’t dissolve in water and forms a solid or is a gas that bubbles out. or is a covalent compound usually water. Polyatomic ions don’t change from side to side

Complete and balance assume all of the reactions take place. CaCl2 + NaOH ® CuCl2 + K2S ® KOH + Fe(NO3)3 ®

Complete and balance KOH + Fe(NO3)3 ® H3PO4 + Ca(OH)2 ®

How to recognize which type Look at the reactants E for element C for compound E + E Combination C Decomposition E + C Single replacement C + C Double replacement

Last Type Combustion A compound composed of only C H and maybe O is reacted with oxygen If the combustion is complete, the products will be CO2 and H2O. If the combustion is incomplete, the products will be CO and H2O. or just C and H2O. O2 will always be the second reactant

Ionic Compounds and acids Fall apart into ions when they dissolve That’s why they conduct electricity when dissolved. So when we write them as (aq) they are really separated NaCl(aq) is really Na+(aq) and Cl-(aq) K2SO4 (aq) is really K+(aq) and SO42-(aq)

Reactions in aqueous solutions Many reactions happen in solution Makes it so the ions separate so they can interact. Solids, liquids, and gases are not separated, only aqueous

Complete Ionic Equation Every aqueous compound is written as separate ions Solids, liquids and gases as whole compounds MgCl2(aq) + PbSO4(aq) → MgSO4(aq) + PbCl2(s) Is really Mg2+(aq) + Cl-(aq) + Pb2+(aq) + SO4(aq) → Mg2+(aq) + SO4(aq) + PbCl2(s)

Write the complete ionic equation for FeBr3(aq) + KOH(aq) → KBr (aq) + Fe(OH)3(s) Fe3+(aq) Br-(aq) K+(aq) OH-(aq) K+(aq) Br-(aq) Fe(OH)3(s) + + + → + +

Write the complete ionic equation for CaCl2(aq) + MgSO4(aq) → CaSO4(s) + MgCl2(aq)

Write the complete ionic equation for Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + HOH(l)

The complete ionic equation is Fe3+(aq)+ Br-(aq) + K+(aq) +OH-(aq) → K+(aq) +Br-(aq) + Fe(OH)3(s) K+ and Br- don’t change. They are spectator ions Could be eliminated Fe3+(aq) +OH-(aq) →Fe(OH)3(s) This is what really changes

Net ionic equation Shows only those particles that change before and after. Eliminate spectator ions Needs to be balanced in terms of both mass and charge Fe3+(aq) +OH-(aq) →Fe(OH)3(s) Fe3+(aq) +3 OH-(aq) →Fe(OH)3(s)

Write the net ionic equation HCl (aq) + Ba(OH)2 (aq) → BaCl2(s) + HOH (l)

Write the net ionic equation Al + FeSO4(aq) → Al2(SO4)3(aq) + Fe

Write the net ionic equation Cl2(s) + NaI(aq) → NaCl(aq) + I2(s)

Write the net ionic equation K2CO3(aq) + MgI2(aq) → MgCO3(s) + KI(aq)

Net ionic equations Written for single and double replacement.

Predicting precipitates Solids formed from aqueous solution. You can predict them if you know some general rules for solubility.

These things are soluble Salts with alkali metals and ammonium Salts of nitrates and chlorates Salts of sulfates except Ag+, Pb2+, Hg22+, Ba2+, and Sr2+ Salts of chlorides except Ag+, Pb2+, and Hg22+

These things are insoluble Carbonates, phosphates, chromates, sulfides, and hydroxides Unless they fall under rule # 1

Is it soluble? LiBr Ba(NO3)2 CaSO4 PbCl2 CaCO3 K2CO3 Cd(ClO3)2

Is there a reaction? For double replacement- has to make gas, solid or water. Water from an acid- H+ and a hydroxide- OH- makes HOH Solids- from solubility rules Exchange ions and see if something is insoluble

Is there a reaction? MgSO4 + NaOH → H2SO4 + KOH → K3PO4 + FeF3→