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IGCSE Chemistry > Chemical Energetics > Flashcards

Chemical Energetics Flashcards

1
Q

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

A

Correct orientation
Sufficient energy

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2
Q

What does H mean

A

Enthalpy
Heat energy

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3
Q

What does ΔH mean

A

Enthalpy change
Amount of energy released or absorbed during a reaction

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4
Q

What does Ea mean

A

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

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5
Q

Activated complex

A

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

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6
Q

Describe an effective collision

A

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

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7
Q

2 chemical energetics reactions examples

A

Exothermic and endothermic

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8
Q

Exothermic reaction

A

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

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9
Q

Endothermic reactions

A

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

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10
Q

Examples of Exothermic reactions

A

Combustion
Oxidation
Neutralisation reactions

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11
Q

Examples of endothermic reactions (3)

A

Thermal decomposition
Photosynthesis
Cold packs for sportinjuries

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12
Q

Characteristics of Exothermic reactions (3)

A

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

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13
Q

Draw an Exothermic energy profile/level diagram

A
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14
Q

Characteristics of endothermic reactions (3)

A

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

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15
Q

Draw an endothermic energy profile

A
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16
Q

Draw a practical used to depict exo and endo thermic reactions

A
17
Q

Describe an Exothermic reaction in terms of bonds

A

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

18
Q

Describe an endothermic reaction in terms of bonds

A

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

19
Q

What is the bond energy rule

A

Bond breaking = Endothermic
Bond making = Exothermic

20
Q

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

A

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

21
Q

What is room temperature

A

25 degrees Celsius

22
Q

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

A

Cooler, because energy is absorbed from the solution

23
Q

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

A

Energy is released into the solution so the solution gets warmer

24
Q

Equilibrium definition

A

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

25
Q

What happens if you encourage the forward reaction

A

More product is produced

IGCSE Chemistry (21 decks)

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