enthalpy/ energy reactivity 1.1, 1.2, 1.3

Describes a reaction in which energy is transferred to the surroundings. eg. freezing, condensation, deposition, neutralization, combustion

Describes a reaction in which energy is transferred from the surroundings. eg. evaporation, melting, sublimation, photosynthesis, thermal decomposition

during exothermic reactions there is a release in energy as heat, the water molecules surrounding the site of reaction increases kinetic energy this results in an increase in temperature

The endothermic process of the evaporation of alcohol absorbs energy from the surroundings resulting in a decrease in temperature of the surroundings.

Energy stored in the chemical bonds between particles

reactants are lower in energy, they then absobr energy and products are found higher up in diagram

reactants are higher up in duagram, energy is released and products are then found more energtically stable and lower in the diagram

Measurement of heat energy within a system. It is symbolised in expressions by H. Enthalpy is the amount of heat energy contained in a substance

negative enthalpy change

positive enthalpy change

The heat energy transferred within a reaction under standard conditions with all substances present in their standard states. only 1 product, only 1 mol

Kj molˆ-1

technique used to measure the heat transfer during a physical or chemical process

Q= thermal energy in joules m= mass of psecies you are measuring temperture change of T= change in temperature

delta H= change in enthalpy Q= thermal energy n= number of moles of an identified reactant or product in the chemical reaction

exothermic reactions have more stable products because they are in lower energy levels while endothermic reactions have less stable products because they are in higher energy levels than reactants

The energy required to break one mole of chemical bonds in the gaseous state.

bond making= exothermic bond breaking= endothermic

because the energy required to break a specific type of bond (like C-H) varies depending on the surrounding molecular environment, making a single, exact value impractical.

Law that states that the total enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place, as long as the initial and final conditions are the same.

energy recquired to break bonds

difference between the energy taken in to break bonds and energy given out to make bonds

the change that goes from the reactants to the top of the peak while energy gained by reaction enthalpy change is only from reactants to products

degree to which ligand causes splitting of the d orbitals I-<Br-<S2-<Cl-<F-<OH-<H2O<SCN-<NH3<CN-