Honors Biology 2011-12

What you will learn…1. Levels of organization2. Why Chemistry?3. Life’s elements4. Chemical Bonding5. Polar Covalent Bond6. Electronegativity and Water7. Thee Hydrogen Bond8. Properties of Water/Structural

Explanation/Significance For Life9. Solutions10. Acids/Bases/pH/Buffers

1. How do we organize living things?BiosphereEcosystemCommunityPopulationOrganismOrgan SystemOrganTissueCellOrganelleMacromoleculeMoleculeAtom

2. Why Chemistry?To understand the structures and functions

of living organisms, it’s essential to know the basis of all living things.

The properties of life emerge from the arrangement of its chemical parts into higher and higher levels of biological organization.

At the base of the hierarchy of living things:atoms, elements, and molecules

3. Life requires elements!There are about 25 chemical elements

required for life.Oxygen, Carbon, Hydrogen, and Nitrogen

make up about 96% of the human body Essential ingredients of the major biological

macromolecules: fats, proteins, and sugarsCalcium, Phosphorus, Potassium, Sulfur,

Sodium, Chlorine, and Magnesium account for the remaining 4%. Involved in functions such as bone formation, nerve

signaling, and DNA synthesis

3. What makes up an element?Each element consists of one kind of atomAtoms consists of three subatomic particles:

Protons are positive and located in the nucleus of the atom (represents atomic number)

Neutrons are neutral and located in the nucleus (add to protons to determine mass number)

Electrons are negative and found on orbitals around the nucleus

4. Chemical BondsAtoms can bind with each other to form more

complex forms of matter called compounds.There are two basic types of bonds:

Covalent bond – electrons are shared between atoms forming a molecule

Ionic bond – electrons are lost or gained by atoms and the oppositely charged ions are held together by electrostatic attraction.

5. Covalent Bond- PolaritySome molecules with covalent bonds share

the electrons equally or the molecule is symmetrical – nonpolar molecules (Ex. Oil)

Some molecules have an uneven electron sharing. One atom attracts the electrons more in the bond than the other – polar molecules (Ex. Water)

5. Water!

6. ElectronegativityElectronegativity

An atom’s attraction for its electrons, including shared electrons.

6. Electronegativity and WaterUnequal sharing of electrons produces what

is called a polar covalent bond. The pulling of shared electrons closer to the more

electronegative atom makes that atom partially negative and the other atom partially positive.

Oxygen is one of the most electronegative elements, and thus attracts the shared electrons in H2O much more strongly than H does.

the O atom has a slight negative charge and each H atom a slight positive charge.

The V shape and its polar covalent bonds make water a polar molecule

7. Hydrogen bonding in Water!

7. Thee Hydrogen Bond In addition to strong polar covalent bonds, water also

forms bonds with other water molecules. This bond, called a Hydrogen Bond, attaches the H+

from one molecule to the O- of another moleculeOne water molecule can have up to four hydrogen bonds.

The molecules of water are constantly moving in relation to each other, and the hydrogen bonds are continually breaking and reforming at timescales faster than 200 femtoseconds.[13]

However, this bond is sufficiently strong to create many of the peculiar properties of water

The hydrogen bond, and the polar nature of water, are essential properties allowing for many unique features of water.

8. WATER!!

Property of Water 11. Property:

Water as ice is less dense than liquid water1. Structural Explanation:

Ice takes on a more regular, tetrahedral structure so the molecules are further from each other.

Significance for Life:Life can exist under ice

Property of Water 22. Property:

Water has a low viscosity2. Structural Explanation:

Small molecules2. Significance for Life:

Water can for through very small spaces, capillaries

Property of Water 33. Property:

Water is liquid at room temperature3. Structural Explanation:

Hydrogen bonds3. Signifance For Life:

Water is a medium aquatic life, water is found inside cells

Property of Water 44. Property:

Water is colorless with a high transmission of visible light

4. Structural Explanation: Small, stable molecule, no excitable electrons

4. Significance For Life:Small, stable molecule, no excitable electrons

Property of Water 55.Property:

Water has strong adhesive (water sticks (adheres) to other molecules or surfaces) and cohesive (water sticks together) forces.

5. Stuctural Explanation:Polarity- adhesion/ Hydrogen bonds- cohesion

5. Significance For Life:Adhesive (water can stick to plant tissue during

transpiration)/ Cohesive (water can stick to other water molecules during transpiration)

Property of Water 66. Property:

Water is classified as a universal solvent because many substances can dissolve in water.

6. Structural Explanation:Water is classified as a universal solvent

because many substances can dissolve in water.6. Significance For Life:

Water is a medium for the chemical reactions of life/ main transport medium (dissolved minerals and ions in water for plants)

Property of Water 77. Property:

High heat of fusion- a significant amount of energy is required before water can change state

7. Structural Explanation:Hydrogen bonds

7. Significance For Life:Contents of cells are unlikely to freeze

Property of Water 88. Property:

Water has a high heat of vaporization.8. Structural Explanation:

Hydrogen bonds8. Significance For Life:

Heat is lost by evaporation of water. Sweating causes rapid cooling.

Property of Water 99. Property:

Water has a high specific heat capacity (water can absorb a large amount of energy for only a small rise in temperature).

9. Structural Explanation:Hydrogen bonds

9. Significance For Life:Aquatic environments are thermally stable.

Organisms have stable internal temperatures when external temperature fluctuate.

Property of Water 1010. Property:

Water has a high surface tension (caused by cohesion).

10. Structural Explanation:Close attraction between water molecules, H-

bonds 10. Significance For Life:

water forms droplets on surfaces and runoffs

8. Properties of Water (refer to chart)1. Water as ice is less dense than liquid water2. Water has a low viscosity3. Water is liquid at room temperature4. Water is colorless with a high transmission of visible light5. Water has strong adhesive (water sticks (adheres) to

other molecules or surfaces) and cohesive (water sticks together) forces.

6. Water is classified as a universal solvent because many substances can dissolve in water.

7. High heat of fusion- a significant amount of energy is required before water can change state

8. Water has a high heat of vaporization.9. Water has a high specific heat capacity (water can absorb

a large amount of energy for only a small rise in temperature).

10. Water has a high surface tension (caused by cohesion).

8. Structural Explanations (refer to chart)1. Ice takes on a more regular, tetrahedral structure

so the molecules are further from each other.2. Small molecules3. Hydrogen bonds4. Small, stable molecule, no excitable electrons5. Polarity- adhesion/ Hydrogen bonds- cohesion6. Hydrogen bonds, polar, small molecules7. Hydrogen bonds8. Hydrogen bonds9. Hydrogen bonds10. Close attraction between water molecules, H-

bonds

8. Significance For Life (refer to chart)1. Life can exist under ice2. Water can for through very small spaces, capillaries3. Water is a medium aquatic life, water is found inside cells4. light can penetrate tissues in plants and also aquatic

environments5. Adhesive (water can stick to plant tissue during transpiration)/

Cohesive (water can stick to other water molecules during transpiration)

6. Water is a medium for the chemical reactions of life/ main transport medium (dissolved minerals and ions in water for plants)

7. Contents of cells are unlikely to freeze8. Heat is lost by evaporation of water. Sweating causes rapid

cooling.9. Aquatic environments are thermally stable. Organisms have

stable internal temperatures when external temperature fluctuate. 10. water forms droplets on surfaces and runoffs

9. SolutionsA solution is a liquid consisting of a uniform

mixture of two or more substances.The dissolving agent is the solvent and the

solute is the substance dissolved. When water is the solvent, the result is an

aqueous solution.For example, water is the solvent in blood and

in plant sap.

10. Acids and basesIn aqueous solutions, water molecules can

break apart (dissociate) into ions. The ions formed are H+ (hydrogen ion) and

OH- (hydroxide ion).Some chemical compounds contribute

additional H+ to an aqueous solution, while others remove H+ from it.

10. AcidsAcids are compounds that contain hydrogen

and can dissolve in water to release hydrogen ions into solution.  Increase the concentration of hydrogen ionsFor example, hydrochloric acid (HCl) dissolves

in water as follows:HCl H +

(aq ) +  Cl-(aq)

10. BasesBases as substances that dissolve in water to

release hydroxide ions (OH-) into solution and removes H+. decrease the concentration of hydrogen ions

(by accepting them).  For example, a typical base according to the

Arrhenius definition is sodium hydroxide (NaOH):

NaOH   Na+ (aq)  +  OH-

(aq)

10. pH scaleThe acidity or basicity of something, therefore,

can be measured by its hydrogen ion concentration.

pH is a measure of the balance between hydrogen ions (H+) and hydroxide ions (OH-) in an aqueous solution. Solutions with pH = 7 are neutral (for example,

pure water) Solutions with pH < 7 are acidic Solutions with pH > 7 are basic (or “alkaline”)

10. BuffersBuffers:

A buffer solution is one which resists changes in pH when small quantities of an acid or a base are added to it.

They can resists changes in pH by accepting H+ when it is in excess and donating H+ when it is depleted.

For example, your blood has buffers that help to ensure an optimal pH is maintained in your body.

10. pH IndicatorsChemical compound added to a solution to

determine the pH visually. Example: Red cabbage juice contains a

pigment molecule that will change color based on pH: Very acidic solutions will turn a red color. Neutral solutions result in a purplish color. Basic solutions appear in greenish-yellow