Reactions have different forms {reaction types}: chain, synthesis, decomposition, substitution, metathesis, nucleophilic, electrophilic, and molecular rearrangement.
Phosphoric acid and sulfuric acid are catalysts for carbon-chain dealkylations {cracking, dealkylation}| {dealkylation}. Petroleum separation uses phosphoric acid, sulfuric acid, silicon oxide, and aluminum oxide. Silicon oxide and aluminum oxide build branched hydrocarbons. Olefins form on platinum with silicon oxide, followed by isomerization, ring formation, splitting, and hydrogenation.
Two chemicals can bind to make something with different properties than original chemicals {hypergolic}. For example, hydrazine and nitrogen tetroxide react when in contact to make nitrous oxide and water: N2H2 + NO4 -> 3 NO + H2O [where 2 and 4 are subscripts].
Pressure can cause luminescence {triboluminescence}.
Product can be reactant, which can make more product {chain reaction, chemistry}|. Reaction rate continually increases, until system physically disrupts.
One reactant can make two products {decomposition reaction}. Decomposition includes hydrolysis and dehydration reactions.
Chemical can attack negatively charged group {electrophilic reaction}.
Two compounds can make two new compounds {double replacement reaction} {metathesis reaction}. Acid-base reactions have metathesis. Metal compounds can catalyze carbon-carbon double-bond changes.
One reactant can change to same chemical in different configuration {molecular rearrangement}.
Chemical can attack positively charged group {nucleophilic reaction}.
Element and compound can make another element and another compound {single replacement reaction} {substitution reaction, inorganic}. Metal-atom to metal-ion oxidation has substitution.
Two reactants can make one product {synthesis reaction}. Synthesis includes polymerization, hydration, and oxidation reactions, like rusting and combustion.
Energy transfer can involve permanent change that cannot reverse {irreversible reaction}, because heat is made.
Energy transfer can have no friction or other opposing changes {reversible reaction}. In reversible reactions, external and internal temperatures and pressures are approximately the same. In reversible processes, system and surroundings are always in equilibrium. Reversible processes approximate slow energy transfer with small force and minimal resistance.
In reactions {spontaneous reaction}, activation energy can be less than difference in potential energy between transition state and products.
Chemical reactions can release or absorb thermal energy {heat of reaction}|.
Chemical reactions {endothermic reaction} absorb energy if product potential energy is higher than reactant potential energy. Endothermic reactions make complex molecules and require high temperature or strong light at specific frequency.
Chemical reactions {exothermic reaction} release energy {heat, reaction} if reactant potential energy is higher than product potential energy.
Reactions {monomolecular reaction} can have one reactant, as in SN1 and E1 reactions. Molecule vibrations and rotations can cause molecule to decay to new state, as in gas decays, Type I nucleophilic substitutions, Type I eliminations, dissolution, and state changes.
Reactions {bimolecular reaction} can have two reactants, as in SN2 and E2 reactions. Molecule collisions can form transition states and can transfer energy or functional groups, as in isomerizations, Type II nucleophilic substitutions, Type II eliminations, enzyme reactions, syntheses, and dimerizations.
Reactions {termolecular reaction} can have three reactants, as in enzymatic reactions.
5-Chemistry-Inorganic-Chemical Reaction
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Date Modified: 2022.0225