Chemical Energetics

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

Front (Question)

What do particles need to collide with in order for a substance to react

Back (Answer)

Correct orientation Sufficient energy

Front (Question)

What does H mean

Back (Answer)

Enthalpy Heat energy

Front (Question)

What does ΔH mean

Back (Answer)

Enthalpy change Amount of energy released or absorbed during a reaction

Front (Question)

What does Ea mean

Back (Answer)

Activation energy Minimum amount of energy colliding particles must have to react

Front (Question)

Activated complex

Back (Answer)

High energy state a reaction goes through in order to change reactants into products

Front (Question)

Describe an effective collision

Back (Answer)

Reactants have the sufficient activation energy, become an activated complex, form products

Front (Question)

2 chemical energetics reactions examples

Back (Answer)

Exothermic and endothermic

Front (Question)

Exothermic reaction

Back (Answer)

When energy is transferred to the surroundings so the temperature of the surroundings increase

Front (Question)

Endothermic reactions

Back (Answer)

When energy is absorbed from the surroundings so the temperature of the surroundings decrease

#10

Front (Question)

Examples of Exothermic reactions

Back (Answer)

Combustion Oxidation Neutralisation reactions

#11

Front (Question)

Examples of endothermic reactions (3)

Back (Answer)

Thermal decomposition Photosynthesis Cold packs for sportinjuries

#12

Front (Question)

Characteristics of Exothermic reactions (3)

Back (Answer)

ΔH is negative Products have less energy than reactants Energy is released into solution, causing it to warm

#13

Front (Question)

Draw an Exothermic energy profile/level diagram

Back (Answer)

#14

Front (Question)

Characteristics of endothermic reactions (3)

Back (Answer)

ΔH is positive Products have more energy than reactants Energy is absorbed from solution (gets cooler)

#15

Front (Question)

Draw an endothermic energy profile

Back (Answer)

#16

Front (Question)

Draw a practical used to depict exo and endo thermic reactions

Back (Answer)

#17

Front (Question)

Describe an Exothermic reaction in terms of bonds

Back (Answer)

Energy needed to break bonds is less than the energy produced when new bonds are made

#18

Front (Question)

Describe an endothermic reaction in terms of bonds

Back (Answer)

The energy needed to break bonds is more than the energy released when new bonds are made

#19

Front (Question)

What is the bond energy rule

Back (Answer)

Bond breaking = Endothermic Bond making = Exothermic

#20

Front (Question)

How do you calculate the change in Enthalpy and what is the unit

Back (Answer)

Bond energy of reactants - Bond energy of products kJ/mol

#21

Front (Question)

What is room temperature

Back (Answer)

25 degrees Celsius

#22

Front (Question)

Does the solution get warmer or cooler in an endothermic reaction and why

Back (Answer)

Cooler, because energy is absorbed from the solution

#23

Front (Question)

Does the solution get warmer or cooler in an exothermic reaction and why

Back (Answer)

Energy is released into the solution so the solution gets warmer

#24

Front (Question)

Equilibrium definition

Back (Answer)

State achieved when the forward and reverse reactions occur at the same rate and the concentration of the reactants and products stay constant