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Chem I Unit 5 Reactions Chemical Reaction

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Chem I Unit 5 Reactions Chemical Reaction Chem I Unit 5 Reactions Chemical Reaction: a process in which one or more substances are converted into new substances with different physical and chemical properties Reactant: a substance that enters into a chemical reaction Product: A substance produces by a chemical reaction Chemical Reactions occur so that atoms can obtain a full set of valence electrons and become more stable Chemical Equations Chemical Equations: are used to describe what happens in a chemical reaction Identifies the reactants and the products Reactants → Products Types of Chemical Equations Word Equations: give the names of the reactants and products Magnesium + Nitrogen → Magnesium Nitride Formula Equations or Chemical Equations: use chemical symbols and formulas instead of names Coefficients: precede the symbol or formula and indicate the relative number of particles 3 Mg + N2 → Mg3N2 3 atoms of magnesium react with one molecule of nitrogen to yield one particle of magnesium nitride Practice Convert word equations below into formula equations Hint: H O N and the halogens all exist as diatomic molecules H2 = hydrogen O2 = Oxygen N2 = Nitrogen Cl2 = chlorine Br2 = Bromine F2 = Fluorine, etc. sulfur + oxygen → sulfur dioxide carbon dioxide + water → carbonic acid iron + copper (II) sulfate → iron (II) sulfate + copper Practice Convert word equations below into formula equations Hint: H O N and the halogens all exist as diatomic molecules H2 = hydrogen O2 = Oxygen N2 = Nitrogen Cl2 = chlorine Br2 = Bromine F2 = Fluorine, etc. sulfur + oxygen → sulfur dioxide S + O2 → SO2 carbon dioxide + water → carbonic acid CO2 + H2O → H2CO3 iron + copper (II) sulfate → iron (II) sulfate + copper Fe + CuSO4 → FeSO4 + Cu Balanced Chemical Equation: The Law of Conservation of Mass has been observed Matter can neither be gained nor lost through a chemical reaction For mass to remain constant the number of atoms of each element must be the same before and after a chemical reaction (Atoms Before = Atoms After) Example: 3 Mg + N2 → Mg3N2 Element Mg N Atoms Before 3 2 Atoms Afterward 3 2 Balancing Equations Write a formula equation with the correct symbols and formulas Count the number of atoms of each element on each side of the arrow Balance atoms by using coefficients Check work by counting atoms of each element K + Br2 → KBr Before: 1 K and 2 Br After: 1 K and 1 Br 2K + Br2 → 2KBr Before: 2 K and 2 Br After: 2 K and 2 Br Hints for Balancing Equations Check for Diatomic molecules H2 O2 N2 Cl2 Br2 I2 F2 Balance Polyatomic ions (if same poly. Ion on both sides → balance as a chunk) Metals Nonmetals “O” & “H” Recheck your count – it can take several steps! Balancing Example CH4 + O2 → CO2 + H2O Balance C 1C 1C Balance H 4H 2H Add Coefficient CH4 + O2 → CO2 + 2H2O Balance H 4H 4H Balance O 2O 2O + 2O = 4O Add Coefficient CH4 + 2O2 → CO2 + 2H2O Check all atoms C H O Before: 1 4 4 After 1 4 4 Practice: Balance the following Equations Fe + O2 → Fe2O3 C2H5OH + O2 → CO2 + H2O Practice: Balance the following Equations 4Fe + 3O2 → 2Fe2O3 C2H5OH + 3O2 → 2CO2 + 3H2O Writing Complete Chemical Reactions Complete Chemical Reactions: include the physical state of each reactant and product Written after the formula in parentheses: (g) = gas (l) = liquid (s) = solid (aq) = aqueous (dissolved in water) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) 1 molecule of Methane gas reacts with two molecules of oxygen gas to form 1 molecule carbon dioxide and 2 molecules of water Classifying Chemical Reactions Direct Combination (or synthesis) reactions: 2 or more simple reactants come together to form a single more complex product A + B → AB S + O2 → SO2 CO2 + H2O → H2CO3 Decomposition reactions: a single compound is broken down into two or more smaller compounds or elements AB → A + B 2H2O → 2H2 + O2 CaCO3 → CaO + CO2 Classifying Chemical Reactions Single Replacement Reactions: An uncombined element displaces an element that is part of a compound A + BX → AX + B Mg + CuSO4 → MgSO4 + Cu Double Replacement Reactions: atoms or ions from two different compounds replace each other AX + BY → AY + BX CaCO3 + 2HCl → CaCl2 + H2CO3 AgNO3 + CaCl2 → Ca(NO3)2 + AgCl Classifying Chemical Reactions Combustion reactions: reaction in which something is burned (reacted with oxygen) Many direct combination reactions are also combustion reactions: 4 Fe + 3 O2 → 2 Fe2O3 General form of reaction: CxHyOz + O2 → CO2 + H2O When compounds containing carbon and hydrogen (can also have oxygen) burn the products always include carbon dioxide and water CH4 + O2 → CO2 + 2H2O C2H5OH+ 3O2 →2 CO2 + 3H2O Classifying Chemical Reactions Neutralization reactions: are a special case of double replacement reaction. One of the reactants is an acid (starts with H), one is a base (ends with OH). The products are always a salt and water. All ionic compounds are salts. General form of reaction: AOH + HX → AX + HOH Neutralization reactions occur in water Ca(OH)2 + 2 HCl → CaCl2 + 2 H2O AgOH + HNO3 → AgNO3 + H2O The Unique Bonding of Carbon Carbon’s half filled valence level and relatively small size give it unique bonding properties It is one of the few elements that forms 4 bonds and the only one that does so in such a large variety of combinations: Carbon bonds with itself to form long chains or ring structures These bonds are strong, short and covalent so the structures are very stable Each Carbon in the chain or ring can form 4 single bonds, 2 double bonds, 1 double & 2 single bonds, 1 single and 1 triple bond. Thus a HUGE variety of compounds containing carbon exist These compounds provide the framework for most of the molecules that living organisms make or use. This is why in general carbon containing compounds are called Organic compounds. Hydrocarbons: are compounds made of hydrogen and carbon Predicting Reaction Products In a single replacement reaction metals replace metals or hydrogen and nonmetals replace nonmetals. Example: Cl2 + 2KI → 2KCl + I2 The activity series can be used to predict whether one metal will replace another An activity series of metals is a listing that ranks metals according to their relative reactivity A metal can replace only those metals below it on the list Predicting Products Double replacement reactions are likely to proceed if at least one of the products is a molecular compound, a precipitate, or a gas. Solubility rules can be used to help determine whether a product will be a precipitate Precipitate: solid formed when two aqueous substances react Solubility Rules: for solubility in water Compounds that contain these ions are generally soluble Alkali metals and ammonium ions - Acetate ion (C2H3O2 ) - Nitrate ion (NO3 ) Halide ions (X), except AgX, Hg2X2 and PbX2 Sulfate ion except SrSO4, BaSO4, and PbSO4 Compounds that contain these ions are generally insoluble -2 Carbonate ion (CO3 ) except with rule 1 ions -2 Chromate ion (CrO4 ) except with rule 1 ions -2 Phosphate ion (PO4 ) except with rule 1 ions Sulfide ion (S2-) (CaS, SrS, BaS and rule 1 exceptions are soluble) -2 Hydroxide ion (OH ) (Ca(OH)2, Sr(OH)2, and Ba(OH)2 and rule 1 exceptions are soluble Reaction Rate Many reactions are reversible – once there are enough products, the products can change back into reactants Chemical Equilibrium is the state in which the concentration of the reactants and products remain constant with time because the rate at which they are formed in each reaction equals the rate at which they are consumed in the opposite reaction (forward rate = reverse rate) Le Chatelier’s Principle: Conditions affect equilibrium. Thus different conditions will affect the relative amount of products that are formed. Conditions that affect Rate Concentration: the amount of a substance Adding a substance to a system at equilibrium causes the system to consume that substance Add a reactant – increase forward rate – more products are produced Add a product – increase reverse rate – more reactants are produced Pressure: affects some gaseous system Increase pressure – the reaction will shift in the direction that produces fewer molecules of gas Example: In the reaction below fewer gas molecules are produced by the forward reaction. An increase in pressure will favor production of product 2 NO2 (g) N2O4 (g) Conditions that Affect Rate Temperature: to determine the affect of temperature you must know whether the reaction is endothermic or exothermic: Exothermic reactions – give off heat Endothermic reactions – absorb heat If the forward reaction is exothermic the reverses is endothermic and vice versa If the reaction is exothermic: adding heat will drive the reverse reaction – producing more reactants. If the reaction is endothermic, adding heat will drive the forward reaction – producing more products .
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