Energy Lecture - Chapter 5

Front 1

Energy:

Back 1

The ability to do work

Front 2

How many states does energy exist in?

Name them.

Back 2

2 States

Kinetic Energy
Potential Energy

Front 3

Kinetic Energy

Back 3

The energy of motion (mechanical)

Front 4

Potential Energy

Back 4

Stored energy that can be used for motion (chemical)

Front 5

All the work carried out by living organisms involves the transformation of __________ energy is transformed into ____________ energy

Back 5

Potential energy into kinetic energy

Front 6

All forms of energy can be converted to what?

Back 6

Heat

Front 7

What is the most convenient form of energy to measure?

Back 7

Heat

Front 8

Thermodynamics

Back 8

The study of energy or heat changes

Front 9

Describe the 1st Law of Thermodynamics

Back 9

1.) Total amount of energy in the universe remains constant
2.) energy can change from one state to another but can never be created or destroyed
3.) during energy conversions some energy is lost as heat energy

Front 10

Describe the 2nd Law of Thermodynamics

Back 10

1.) The amount of disorder, or entropy, in the universe is increasing
2.) Increasing entropy means that energy is transforming from potential to heat energy
3.) lost energy increases disorder

Front 11

Without _______ input of energy, disorder would prevail and life would be impossible.

Back 11

Input

Front 12

Certain types of organisms capture energy from the sun and use it to build what?

Back 12

Molecules!

Front 13

What is happening during a chemical reaction?

Back 13

Chemical bonds are being being created and broken.

Front 14

The molecules involved in the beginning of a chemical reaction are called what?

Back 14

Reactants or Substrates

Front 15

The molecules involved in the end of a chemical reaction are called referred to as???

Back 15

Products

Front 16

How many types of chemical reactions are there?

Name them and describe how each is unique.

Back 16

There are 2 types of chemical reactions.
1.) Endergonic reactions have products with more energy than the reactants. Endergonic reactions are not spontaneous and require energy to occur.
2.) Exergonic reactions have producs with less energy than the reactants. Exergonic reactions ARE spontaneous and energy is RELEASED when the reaction occurs.

Front 17

All chemical reactions require what to occur?

Back 17

Activation Energy

Front 18

Activation Energy

Back 18

Energy required for all chemical reactions to occur. The activation energy initiates a chemical reaction be destabilizing existing chemical bonds.

Front 19

Describe the process by which a chemical reaction can be made more spontaneous.

Back 19

Catalysis - a process of lowering the activation energy.

Front 20

Metabolism

Back 20

Sum of biochemial reactions in the cell

Front 21

Describe how enzymes work

Back 21

Enzymes are the catalysts of chemical reactions: enzymes bind to the "binding site" on the surface of the reactant (substrate) and stress the molecular bonds to make the reaction more likely to occur.

Front 22

Active Site

Back 22

Surface of the enzyme that binds to a reactant

Front 23

Binding Site

Back 23

Surface of a reactant that binds to an enzyme