Unit 7 Flashcards
Balance combustion reactions
C then H then O
Single replacement
-Many single replacement reactions involve the reaction between a metal and an aqueous ionic solution.
-Metal atoms are exchanged during the reaction.
-Reactions between metals and aqueous acids produce an aqueous ionic compound and hydrogen gas. -Reactions between metals and water produce metal hydroxides and hydrogen gas.
Double Replacement
-These types of reactions often involve the aqueous solutions of ion containing compounds.
-The mixing of ionic aqueous solutions results in a double replacement reaction.
-The cation of one reactant will replace the cation in the other reactant.
Combustion Reactions:
-Combustion reactions involves the oxidation of organic compounds (compounds composed of the elements carbon and hydrogen, sometimes including oxygen) in the presence of oxygen to produce carbon dioxide, water, and energy in the form of heat and light.
-The incomplete combustion of hydrocarbons occurs when there is not enough oxygen required to completely oxidize the fuel.
-Carbon, carbon monoxide (a toxic gas), and water are produced instead of carbon dioxide and water.
Redox reaction
-all single replacement reactions are redox reactions
-all combustion reactions are redox reactions
-redox reactions is where we have a transfer of electrons
-oxidation is loss of electrons
-reduction is gain of electrons
-double replacement is never a redox reaction
-anytime you can produce a pure element from a compound its a redox reaction
-if a decomposition is a compound breaking down into pure elements its a redox reaction (NOT a large compound breaking into 2 smaller compounds)
-in a synthesis reaction the reverse is true if you have two pure elements combining to form a compound its a redox reaction (NOT two smaller compounds combining to a large compound)
Oxidation reaction
Loss of electrons
Reduction reactions
Gain of electrons
Acid-base neautralization
If you mix an acid (aq) and base (aq) you produce a liquid product (salt and water ?)
Solubility Rules
To identify a precipitation reaction from a balanced chemical equation by the following rules:
• It is a double replacement reaction involving two aqueous ionic solutions. • There is a solid product—if there is no solid product, it is not a precipitation reaction.
Acid-Base neutralization reactions
-double replacement reactions between aqueous solutions of acids and bases
-During the reaction, the hydroxide (OH-) and hydrogen (H+) ions in solution join together to form neutral liquid water and a salt
-The salt is formed from the cation of the base and the anion of the acid
-In order for complete neutralization to occur, there must be equal amounts of OH- and H+ ions in solution since one OH- and one H+ ion produces one H2O molecule.
-Most common neutralization reactions involve metal hydroxides (i.e. NaOH, Ca(OH)2, KOH, etc.) and an acid, with the products always being a salt and liquid water.
- The salt is formed from the metal cation from the base and the non-metal cation from the acid.
-Reactions between acids and metal carbonates or bicarbonates are also common.
-The products are a salt, carbon dioxide, and liquid water.
Redox Reactions
OILRIG
OXIDATION is loss
REDUCTION is gain
-and they occur simultaneously leading to the shortened term “redox” reactions
-The species losing the electrons is said to be oxidized and causes the reduction of the other reactant.
-Thus, any substance that is oxidized is called the “reducing” agent.
-Likewise, a substance that is reduced, causes the oxidation of the other reactant making it the “oxidizing” agent.
-Oxidation may involve the gain of oxygen atoms or the loss of hydrogen atoms.
-Likewise, reduction may sometimes involve the gain of hydrogen atoms and the loss of oxygen atoms.
-Many of the reactions that we have already discussed can be classified as redox reactions. The following reaction types may be classified as redox reactions:
1. Single replacement/displacement
2. Combustion
3. Synthesis/combination
Molar mass
g/ 1 mol
Percent yield
% yield = actual yield/theoretical yield x 100
