Heat energy changes in chemical reactions GapFill

Energy is always  createddiscovereddestroyedconservedprovidedreleased during chemical reactions. There may be a change in the  humiditycolourpolaritytemperaturemagnetismpressure of the surroundings due to energy being taken in or given out by the molecules. Reactions in which the surroundings get warmer are called  heatingyieldingproductivegenerativeexothermicoxidative, e.g. combustion,  activationminingpolymerisationburningprecipitationneutralisation and the reactions of hand warmers, and reactions in which they get colder are called  unproductivereductivesterilisingresistingendothermiccooling, e.g. thermal  chromatographydistillationfractionationdecompositionhydrogenationoxidation reactions. Reactions will only occur if particles collide with sufficient  anglesorientationsenergytangentsmassesdirections.

One way of representing reactions is using a reaction  tableprofileboardslidermodelgradient, which shows the energy of the reactants and products. The height of the curve from the reactants is the  activation energytotal energymaximum reactivityinitiation energyenergy debtenergy peak, and the difference between the reactants and products is the  energy changetotal energyenergy productactivation energyenergy costenergy pay-off of the reaction.

When bonds are  reshapedbrokenheatedcreatedstrengthenedtwisted in the reactants, energy is taken in. When bonds are  formeddestroyedreshapedreactedloosenedunravelled in the products, energy is released. A reaction is exothermic if the energy released is  in a different form tonot equal toequal toin the same form asless thangreater than the amount taken in.