chemical reactions chapter 19. synthesis reaction (combination reaction) - the combination of two or...
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Synthesis Reaction (combination reaction) -
• the combination of two or more substances to form a compound
Element or compountd + element or compound compound
General form A + B AB
Decomposition Reaction:
• is the breakdown of one substance into two or more other substances
• compound two or more elements
• AB A + B
Single Displacement Reaction:
• One element replaces another element in a compound.
element + compound element + compound
A + BC AC + B
Single Displacement
• We can predict which metal will replace another using an Activity Series, shown in the diagram, which lists metals according to how reactive they are.
• A metal will replace any less active metal.
Double Displacement Reaction:
• Two elements replace each other in compounds.
• A precipitate is an insoluble compound that comes out of solution during this type of reaction.
AB + CD AD + CB
MgCO3 + 2HCl MgCl2 + H2CO3
• An exothermic reaction in which a substance combines with oxygen forming products in which all elements are combined with oxygen. (Burning) Energy is usually released in the form of heat and light.
CxHy + O2 CO2 + H2O + heat/light
Oxidation Reduction Reactions
• Oxidation-reduction reactions- chemical changes that occur when electrons are transferred between reactants.
• Also called REDOX reactions
• Oxidation
• Modern definition - loss of electrons
• Reduction
• Modern definition - gain of electrons
• Oxidation and reduction always occur simultaneously. One process cannot occur without the other.
Oxidation Reduction Reactions
Redox reactions
• Chemical reactions involving electron transfer of this sort often involve oxygen, which is very reactive, pulling electrons from metallic elements.
• Corrosion of metal is a visible result.
Lavoisier and the Conservation of Mass
• Chemical reactions are taking place all around you and even within you.
• A chemical reaction is a change in which one or more substances are converted into new substances.
Lavoisier and the Conservation of Mass
• The substances that react are called reactants.
• The new substances produced are called products.
• This relationship can be written as follows:
Lavoisier and the Conservation of Mass
• The French chemist Antoine Lavoisier established that the total mass of the products always equals the total mass of the reactants.
Lavoisier and the Conservation of Mass
• For example, the mass of the candles and oxygen before burning is exactly equal to the mass of the remaining candle and gaseous products.
Writing Equations
• Scientists have developed a shorthand method to describe chemical reactions.
• A chemical equation is a way to describe a chemical reaction using chemical formulas and other symbols.
Choosing Coefficients
• Finding out which coefficients to use to balance an equation is often a trial-and-error process.
How to Balance Equations:
1. Use Pencil!
2. Use coefficients (numbers in front of the formulas), to balance the equation. (DO NOT change the Formulas. DO NOT CHANGE THE SUBSCRIPTS!)
3. Draw a line to separate the reactants from the products.
How to Balance Equations:
4. Write down all elements that are on each side of the equation.
5. Balance polyatomic ions that appear on both sides of the equation as single units. (Ex: Count sulfate ions, not sulfur and oxygen separately)
6. Balance elements one at a time.
How to Balance Equations:
7. Balance H and O last.
8. Save the one that is in the most places for very last.
EXAMPLES: What kind of reactions are these?_____Na + _____Cl2
_____Fe + _____O2
_____Al + _____Cl2
_____H2O + _____CO2
____NaCl
____Fe2O3
H2CO3
____AlCl3
2
232
2
4
3 22
EXAMPLES: What kind of reactions are these?
___Zn + ___HCl
___Cl2 + ___KI
___ZnCl2 + ___H2
___KCl + ___I2
2
22
EXAMPLES: What kind of reactions are these?____C3H8 + ____O2
____Mg + ____O2
____CO2 + ____H2O
____MgO
3 45
22
Energy Exchanges
• A dynamic explosion is an example of a rapid chemical reaction.
• Most chemical reactions proceed more slowly, but all chemical reactions release or absorb energy.
• This energy can take many forms, such as heat, light, sound, or electricity.
• Chemical bonds are the source of this energy.
• When most chemical reactions take place, some chemical bonds in the reactants are broken, which requires energy.
• In order for products to be produced, new bonds must form. Bond formation releases energy.
More Energy Out
• Chemical reactions that release energy are called exergonic reactions.
• In these reactions less energy is required to break the original bonds than is released when new bonds form.
• As a result, some form of energy, such as light or heat is given off by the reaction.
• The familiar glow from the reaction inside a glow stick is an example of an exergonic reaction, which produces visible light.
Heat Released
• When the energy given off in a reaction is primarily in the form of heat, the reaction is called an exothermic reaction.
• The burning of wood and the explosion of dynamite are exothermic reactions.
More Energy In
• Sometimes a chemical reaction requires more energy to break bonds than is released when new ones are formed.
• These reactions are called endergonic reactions.
• The energy absorbed can be in the form of light, heat or electricity.
Thermal Energy Absorbed
• When the energy needed is in the form of heat, the reaction is called an endothermic reaction.
• Some reactions are so endothermic that they can cause water to freeze.
• Certain types of ice packs are an example of this.