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: [[Collision Theory]] is based on the [[Kinetic Theory]] which [[explain]]s the motion of [[particle]]s in [[matter]].
: In [[Collision Theory]] [[particle]]s are said to [[collide]] with one another and that if two [[reactant]]s in a [[Chemical Reaction|reaction]] [[collide]] with enough [[energy]] this will cause them to [[Chemical Reaction|react]].
: [[Collision Theory]] indicates that the [[particle]]s of [[reactant]] must [[collide]] for the [[Chemical Reaction|reaction]] to occur.
===Temperature and Collision Theory===
===Pressure and Collision Theory===
The [[Particle Model]] explains [[explain]]s how increasing the [[pressure]] on a [[gas]], and compressing it, causes the [[particle]]s in that [[gas]] to [[collide]] more frequently (more often). This means at higher [[pressure]]s the [[particle]]s of [[reactant]]s will [[collide]] with each other more frequently, increasing the chances of them [[Chemical Reaction|reacting]] and increasing the [[Rate of Reaction|rate of reaction]]. ===Concentration and Collision Theory===The [[Particle Model]] [[explain]]s how a higher [[concentration]] of [[gas]], [[liquid]] or [[solute]] causes [[particle]]s to [[collide]] more frequently (more often). This means at higher [[concentration]] the [[particle]]s of [[reactant]]s will [[collide]] with each other more frequently, increasing the chances of them [[Chemical Reaction|reacting]] and increasing the [[Rate of Reaction|rate of reaction]]. ===Surface Area and Collision Theory===The [[Particle Model]] [[explain]]s how [[particle]]s in a [[solid]] [[vibrate]] around fixed positions. This means most of those [[particle]]s cannot [[collide]] with other [[reactant]]s. It is only the [[particle]]s on the surface of the [[solid]] that can have other [[reactant]]s [[collide]] with them. Therefore the larger the [[Surface Area|surface area]] the more frequently [[reactant]] [[particle]]s in a [[gas]] or [[liquid]] will [[collide]] with the [[reactant]] [[particle]]s in the [[solid]], increasing the [[Rate of Reaction|rate of reaction]].