Chapter 2: The Chemistry of LifeName ______

Biology 5.0Date ______Period: ______

Section 2.1: The Nature of Matter

Chemistry: What do I already know?
Three Subatomic Particles / Atomic Symbol
Proton:
Neutron:
Electron:
  • Valence Electrons
/
Atomic Number:
Mass Number:
Atomic Mass:

Covalent Bond - ______

Ions - ______

Cation – ______

Anion – ______

Ionic Bond – ______

Molecule – ______

______

Counting Atoms

Na2SO4

Ca(OH)2

3 Fe2(SO3)3

Isomers – ______

______

Section 2.2: Properties of Water

What do I already know?

Water

The Water Molecule:

Water has a number of unique properties:

1

Water is a polar molecule:

What is a polar molecule?
  • An distribution of ______
  • The molecule becomes ______on each ______
  • It means that the electrons are ______
/ What does it look like?

Hydrogen Bonding:

Because of their partial positive and negative charges, polar molecules such as water can attract each other.

Hydrogen Bonding
Because of their partial and
charges, molecules such as water can each other.
The attraction between a on one water molecule and the on another is known as a . / What does it look like?

Cohesive and Adhesive Properties:

Cohesion / Adhesion
Example: Surface Tension
/ Example: Capillary Action

High Heat Capacity:

What is Heat Capacity?
Why is it so high for water?

Water is the Universal Solvent. Why is it considered the Universal Solvent? ______

______

Hydrophobic / Hydrophilic
Examples: / Examples:

Why is WATERconsidered theUniversal Solvent?______

______

MIXTURES: Homogeneous and Heterogeneous

What is a mixture?
Examples:

Examples of Mixtures:

Homogeneous Mixture / Heterogeneous Mixtures
Examples: / Examples:

Parts of Solution:All solutions contain…

Solvent / Solute

Application

One / Two

Acids, Bases, and pH:

The water molecule dissociates:

Acids / Bases

pH Scale

The pH scale ______

______

0______7______14

Interpreting the pH scale:

Classifying Acids and Bases
Acid / Base

What are BUFFERS?

  • Weak acids or bases that can ______

______

  • Produced
  • The pH value in most cells is ______
  • The pH of stomach acid is ______
  • The pH of the blood is ______

Chemical Reactions and Enzymes (Section 2.4):

Energy

Forms of Energy:

 



 

Potential
Energy
Kinetic
Energy
Free
Energy
Activation
Energy

What is a chemical reaction?

Reactants:

Products:

Bonds are

In the chemical reaction below, write R over the reactants and P over the products. What does  mean?

CO2 + H2O  C6H12O6 + O2

Types of Reactions:

Exergonic
Endergonic

Energy Changes in a Chemical Reaction:

The graphs below show the amount of energy present during two chemical reactions. One of the reactions is an energy-absorbing reaction, the other is an energy-releasing reaction. Label the type of reaction for each, label the energy level for the reactants and products, then draw an arrow on each to show the energy of activation.

Type of Reaction: ______Type of Reaction: ______

Enzymes

Enzyme
Catalyst
Substrate
Active Site

How an Enzyme Works

  1. Enzymes act on a . (Shapes fit together like a lock and a key)
  2. A small area on the enzyme, called the , can attract and hold only a specific .
  3. The enzyme acts as a , which accelerates the of the chemical reaction.
  4. The enzyme needed by weakening the chemical bonds in the substrate.
  5. The enzyme is then .

Regulation of Enzyme Activity

  • Enzymes work best at certain and .
  • Most enzymes in humans work best at C
  • Denaturation –
  • Enzyme becomes
  • and can cause denaturation
  • Some enzymes can be

1