Unit 13 Chemical Reactions Chapter 7 P. Sci. Unit 13 Chemical Reactions Chapter 7

Essential Questions What is the difference between an endothermic reaction and an exothermic reaction. Distinguish among the five general types of chemical reactions.

What are the steps to balance a chemical equation? Explain chemical equilibrium in terms of equal forward and reverse reaction rates. Explain how the law of conservation of matter is related to balancing equations.

Review Chemical change –occurs when one substance changes into another substance. You will have to know how to write a chemical formula from a name. (last chapter) ex. Dihydrogen monoxide = H2O

Review cont. Law of Conservation of … Matter – Matter cannot be created nor destroyed, it can only be changed. Energy – Energy cannot be created nor destroyed, it can only be changed.

Chemical Reactions Occur when substances undergo chemical changes to form new substances. Atoms are re-arranged as bonds are broken and formed.

Reactants → Product Yields forms The chemicals you start with Produce Yields forms Reactants → Product The chemicals you start with What you end up with after the reaction occurs

Signs of a Chemical Reaction Production of a gas Production of a precipitant Change in color Change in odor Production of light or heat

Energy and Reactions All chemical reactions release or absorb energy – (heat, light, sound or electricity) To break bonds – takes energy To form bonds – releases energy

Energy and Reactions cont. endothermic – when more energy is required to break bonds than is released when new ones are formed. (ex: photosynthesis) exothermic – less energy is required to break the original bonds than is release when new bonds form. (ex: bioluminescence – fireflies.

Chemical energy is the energy stored in a chemical bond. Energy is conserved. Chemical energy is the energy stored in a chemical bond. Example: isooctane (gas) and oxygen plus a tiny spark will set off an explosion – the energy of the explosion comes from the chemical energy stored in the isooctane bonds.

Reaction Types There are 5 main types of chemical reactions. Synthesis Decomposition Single-displacement (replacement) Double-displacement (replacement) Combustion

Synthesis Reactions Ex.: 2H2 + O2 → 2H2O two or more substances combine to form another . A + B → AB Ex.: 2H2 + O2 → 2H2O Synthesis reactions always join substances so the product is a more complex compound than the reactants.

Decomposition Reaction opposite of synthesis – one substance breaks down into it’s parts. AB → A + B ex: 2H2O → 2H2 + O2 Decomposition reactions break apart so the reactants are more complex than the products.

Single-displacement Reactions When one element replaces another element in a compound. A + BC → AC + B Ex: Cu + 2AgNO3 → Cu(NO3)2 + 2Ag Generally, a more reactive element will take the place of a less reactive one.

Double-displacement Reactions The positive ion of one compound replaces the positive ion of the other to form two new compounds. AB + CD → AD + CB Ex: Ba(NO3)2 + K2SO4 → BaSO4 + 2KNO3

Combustion Reactions Use oxygen as a reactant AB + O2 → A + BO2 ex: 2CH4 + 3O2 →2CO + 4H2O Usually the products include water and a gas (CO, CO2)

Balancing Chemical Equations Chemical Equations summarize reactions by using formulas for each substance. Because of conservation of matter (mass) the left side (reactants) must equal the right side (products).

Steps for Balancing Equations Write the equation (write the reactants and products as chemical compound formulas and elements) Ex: H2 + O2 → H2O

Draw a table and fill in all elements in the equation as well as how many atoms of each element are on each side of the equation. Ex: H2 + O2 → H2O Element Reactants (left) Products (Right) H 2 O 1

If the reactant numbers are not the same as the product numbers for each element, you have to balance the equation. Element Reactants (left) Products (Right) H 2 O 2 1

Add co-efficients in front of the formulas until they balance. (remember – you can’t change the formula by changing subscripts – you can only change the amount of the substance you have. )

2 2 / + → 2 2 2 1 / / 4 2 Example H2 O2 H2 O H 4 O Un-balanced + → 2 H2 O2 H2 O 2 2 2 1 Element Reactants (left) Products (Right) Un-balanced H / / 4 4 balanced O / 2 balanced

Practice Balance the following equations: HgO → Hg + O2 N2 + H2 → NH3 KClO3 → KCl + O2 KBr + Cl2 → KCl + Br2 CO + O2 → CO2

Answers 2HgO → 2Hg + O2 N2 + 3H2 → 2NH3 2KClO3 → 2KCl + 3O2 2KBr + Cl2 → 2KCl + Br2 2CO + O2 → 2CO2