I need definitions for chemistry and I can't

come up with any

heterogeneous reaction
homogeneous reaction
activation energy
activation energy
activated complex
elementary reaction

Heterogeneous reaction - a chemical reaction in which the reactants are in different phases. Some examples are,

Liquid-solid: alkylation with AlCl3 catalyst
Gas-liquid: gas absorption with reaction
Gas-liquid-solid: hydrogenation of liquids

Homogeneous reaction - a chemical reaction in which the reactants are in the same phase.

Activation energy (Ea) - minimum energy required in order to initiate a certain chemical reaction. In collision theory, even if the reactants are in proper orientation and collided, they still won't react if they don't have enough Ea.

Activated complex - a species in a transition state. (not sure about this one though)

Elementary reaction - a reaction in which the stoichiometric coefficients in the balanced chemical reaction is equal to the exponents used the rate equation, or (if that isn't very clear), elementary reactions follow simple rate laws for we can determine it directly from the chemical reaction. For example,
rA + sB -> tC
rate law: rA = -k * (A)^r * (B)^s

hope this helps~ `u`

I think it's nice that you can get someone to do your work for you but I don't understand why you can't look up these definitions in your text/notes and if you don't have text/notes use Google.

Sure! I can help you with that. Let's start with the definitions for the terms you mentioned:

1. Heterogeneous reaction: A heterogeneous reaction is a chemical reaction that occurs between substances in different phases (e.g., solid, liquid, gas). For example, the reaction between a solid catalyst and a gas to produce a different gas is considered a heterogeneous reaction.

2. Homogeneous reaction: A homogeneous reaction is a chemical reaction that occurs between substances in the same phase (e.g., all reactants and products are in the gas phase or all in the liquid phase). These reactions are also called solution reactions because they often occur in solution (e.g., a reaction between two dissolved substances).

3. Activation energy: Activation energy is the minimum amount of energy required for a chemical reaction to occur. It is the energy that particles must possess in order to overcome the energy barrier and react with each other. If the energy of the colliding particles is less than the activation energy, the reaction will not take place.

4. Activated complex: An activated complex, also known as a transition state, is a high-energy and short-lived intermediate state that molecules go through during a chemical reaction. It represents the maximum point on the reaction energy diagram, where the reactant molecules have absorbed enough energy to start forming new bonds and transform into the products.

5. Elementary reaction: An elementary reaction is a single step or an individual step in a complex reaction mechanism. It describes the way molecules directly interact during a chemical reaction. Elementary reactions are usually written as simple chemical equations and are often combined to form the overall reaction mechanism.

To find these definitions, you can refer to chemistry textbooks, online encyclopedias, chemistry glossaries, or reputable scientific websites like those of universities or scientific institutions. These sources can provide accurate and detailed explanations of these terms and their significance in chemistry.