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Simple Explanation:
Types of Reactions:
Synthesis Reaction: When at least two substances combine to form a new substance.
Demonstration using symbols: A + B → AB
Decomposition Reaction: When a substance breaks into at least two simpler substances.
Demonstration using symbols: AB → A + B
Combustion Reaction: When a substance undergoes rapid exothermic reaction with an oxidizer.
Energy from the reaction is released as heat and light, with light emitted by excited particles in the reaction.
Fire may result from combustion, consisting of transient matter visibly transitioning from reactants to products, accompanied by the release of energy.
If a reactant is a hydrocarbon, its reaction with oxygen gas will produce specific amounts of CO₂ and H₂O, assuming sufficient oxygen is available for complete combustion.
Single Replacement Reaction: A chemical reaction where one element replaces another in a compound.
Demonstration using symbols: A + BC → AC + B
Double Replacement Reactions: A chemical reaction where two compounds exchange ions to form two new compounds.
One of the products must be in a state other than aqueous.
Demonstration using symbols: AB + CD → AD + CB
Neutralization reaction with strong acid and strong base: ACID + BASE → H₂O + Ionic Salt
Basic concepts and terms to know about chemical reactions:
Reactants: Substances that react in a chemical reaction.
Products: Substances formed as a result of reactants undergoing a chemical reaction.
Chemical Equation: Represents chemical reactions using formulas to show the reactants and products, along with their proportions.
Law of Conservation: Mass is not created nor destroyed in a chemical reaction. This means that the mass of reactants and products must equal.
The number of atoms of each element must be the same on both sides of the equation.
Coefficients and Subscripts: Coefficients are placed in front of chemical formulas to indicate how many moles of a substance are in a reaction. Subscripts are placed within chemical formulas to indicate the number of particles per substance.
States of Matter Notation: Indicates states of matter for substances in a reaction.
(s) - Solid Phase
(l) - Liquid Phase
(g) - Gas Phase
(aq) - Aqueous Phase
Endothermic Reactions: Reactions that absorb energy in order to react.
Exothermic Reactions: Reactions that give off energy in order to react.
Basic concepts and terms to know when calculating with chemical reactions:
Mole Ratios: The ratio of the amounts (in moles) of each substance involved in a balanced chemical reaction,
Information about ratios originates from the coefficients in the balanced chemical equation.
Excess Reactants: What reactants we have an excess amount of.
Limiting Reactants: What reactants run out first in a reaction.
Percent Yield: Measures efficiency of a reaction.
(Actual Yield ÷ Theoretical Yield) × 100
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