Welcome to AP Biology

Mrs. Marcum

Big Idea 1: The process of evolution drives the diversity and unity of life.Big Idea 2: Biological systems utilize free energy and molecular building blocksto grow, to reproduce, and to maintain dynamic homeostasis.Big Idea 3: Living systems store, retrieve, transmit, and respond to informationessential to life processes.Big Idea 4: Biological systems interact, and these systems and theirinteractions possess complex properties.

Remember!• Register for AP Central

• Free/Reduced Lunch = 3 = $200 extra KEES

• AP Exam: Monday, May 9

• December 16 - Open Heart Surgery - $14

• Teacher webpage

• Remind 101: text 81010 message: @2hca

• Absent: retrieve papers from extra tray

• Bellwork board

Chemistry Topics

• Atomic Structure

• Atomic mass, atomic number, isotopes

• Chemical Bonding

• pH scale

How Matter is Organized

•Chemical Elements•Forms all matter

•Substances that cannot be split into simpler substances by ordinary chemical means.

•Have letter abbreviations called chemical symbols.

•Most common elements in living things C, H, N, O, P, S (96%)

•Trace elements are present in tiny amounts (Fe, Mn, Cu)

Structure of Atoms

• An element is a quantity of matter composed of atoms of the same type.

Atoms contain:• Nucleus: protons (p+) &

neutrons (neutral charge)• Electrons (e-) surround the

nucleus as a cloud (electron shells are designated regions of the cloud)

http://web.visionlearning.com/custom/chemistry/animations/CHE1.3-an-animations.shtml

Atomic Number and Mass Number

• Atomic number is number of protons in the nucleus.

• Mass number is the sum of its protons and neutrons.

• Isotope atoms of same element with different number of neutrons (Carbon-14 & Carbon-12)

• A hepatobiliary iminodiacetic acid (HIDA) sc

A hepatobiliary iminodiacetic acid (HIDA) scan

Ionic Bonds

•When an atom loses or gains a valence electron, ions are formed (Figure 2.4a).

•Positively and negatively charged ions are attracted to one another.

Covalent Bonds– Covalent bonds are

common and are the strongest chemical bonds in the body.

• Covalent bonds may be nonpolar or polar.– In a nonpolar covalent

bond, atoms share the electrons equally; one atom does not attract the shared electrons more strongly than the other atom

Van der Waals interactions

• Electrons are not always symmetrically distributed in nonpolar molecules

• Occur only when atoms and molecules are very close to each other

• Weak

Polar Covalent Bonds• Unequal sharing of electrons between atoms.

In a water molecule, oxygen attracts the hydrogen electrons more strongly

Polar Covalent Bonds

Hydrogen Bonds

– are weak intermolecular bonds; they serve as links between molecules.

– help determine three-dimensional shape of large molecules

– Important in giving water its properties essential for life

Biologically important weak bonds helps stabilize 3 dimensional shape of large

molecules(DNA and proteins).

Hydrogen Bonds

Because water is polar molecule, it can form Hydrogen Bonds.

Because of the Hydrogen Bonds, water has some very UNIQUE Properties!

Because water is polar molecule, it can form Hydrogen Bonds.

Because of the Hydrogen Bonds, water has some very UNIQUE Properties!

6 Properties of Water

• 1. Water is a Powerful Solvent– Solute, Solution, Solvent– Hydrophobic vs Hydrophilic– Shell of hydration

2. Water is attractiveWater adheres to a surface due to 2 properties:

AdhesionCohesion

These 2 properties allow for capillary action.

• 3. Water has High Surface Tension– Strong interaction of water molecules– Water striders, whirly gigs, skipping

rocks

• 4. Water has a High Specific Heat– High heat is required to increase the

temp. of water and a great deal of heat must be lost in order to decrease the temp. of water.

• 5. High Heat of Vaporization– A great deal of energy must be

present in order to break the Hydrogen bonds to change water from liquid to gas

• 6. Water has a high freezing point and lower density as a solid than a liquid– Water’s maximum density is 4 degrees Celsius

http://nedbook.adam.com/pages/IPWeb/systems/buildframes.html?fluids/acihomeo/01

Normal pH range of arterial blood 7.35-7.45

Acidosis – blood pH below 7.35*depression of synaptic transmission in CNS

Disorientation, coma, death

Alkalosis – blood pH above 7.45*overexcitability of CNS and peripheral nerves

Nervousness, muscle spasms, convulsions and death

Figure 2.13

Buffers•Buffers stabilize pH of a

solution by accepting or donating H+.

• Organisms use buffers to maintain homeostasis.

• Blood pH is 7.4 • Carbonic Acid helps to maintain

this pH

Friday November 13,

2015• Bellwork: crossword puzzle

Isomers – compounds that have the same chemical formula but

differ in structure

differ in covalent arrangements

differ in spatial arrangements

Mirror images of each other pg. 62

TuesdayNovember 17

• Grab A Worksheet from the Bellwork Tray

• Matching:

• A. Phosphate 1. donates Hydrogen ions

• B. Sulfhydrl 2. aldehyde

• C. Carboxyl 3. transfer energy

• D. Amino 4. stabilizes protein structure

• E. Hydroxyl 5. alcohol; polar

• F. Carbonyl 6. accepts Hydrogen ions

Sulfhydryl Group

Tryptophan

All living organisms require 4 types of Organic Compounds:

1. Carbohydrates2. Lipids3. Proteins4. Nucleic Acids

**All contain**: Carbon Hydrogen Oxygen

1. Carbohydrates

• All carbs contain C,H,O in a 1:2:1 ratio

• Functions: Energy & structural support

• Exist as:a. Monosaccharides

b. Disaccharides

c. polysaccharides

a. Monosaccharide“simple sugar”

3 Forms1. Glucose - made by plants;

source of energy

2. Fructose - found in fruits; Sweetest!!

3. Galactose – found in milk

These are ISOMERS – same chemical formula but different structures.

b. Disaccharide“double sugar”

3 Forms1. Sucrose – Table Sugar

glucose + fructose

2. Maltose - Malt Sugar glucose + glucose

3. Lactose – Milk Sugarglucose + galactose

•How do monosaccharides form disaccharides?

• Hydrolysis• Dehydration synthesis (condensation reaction)

– Glycosidic linkage – covalent bond between 2 mono’s

https://www.youtube.com/watch?v=ZMTeqZLXBSo

c. Polysaccharide“Many Sugars”

3 Forms – All composed of repeating units of glucose.

1. Glycogen – Energy storage in animals. (Liver & Muscles)

2. Starch - Energy storage in plants (Roots, Stems, Leaves)

3. Cellulose - Gives strength & rigidity to plant cell(Fiber Prevents Colon Cancer)

Monosaccharide vs Polysaccharide

• Add a pipette full of each food to each test tube• Add a 15 drops of Benedicts to each tube• Heat for 3-5 minutes, orange, green, red = +• Wash out test tubes• Load tubes again• Add a 4 drops of iodine• Dark blue, purple, blackish = +• Wash test tubes• Record data on board

Functional group Quiz

2. Lipids• Nonpolar / insoluble / hydrophobic

• 5 types: triglycerides, phospholipids, steroids, waxes, glycolipids

• Fx: insulation, cushion, energy storage, hormones, membrane structure, protection against pathogens, repel water, water conservation

Four Ring Structure of Steroids

Glycolipid

• 3rd Carbon in glycerol is bound to a carb chain instead of a phosphate group.

• Behaves like a phospholipid because the carbohydrate is hydrophilic

• Found in cell membrane and functions in identification of the cell

Waxes

December 1Tuesday

• Get out multiple choice review sheet from yesterday

3. Proteins • Found in: meat, eggs, nuts, beans, tofu

• Uses in body: muscle, hormones, enzymes, energy, transport of oxygen (hemoglobin), support, hair, nails, skin, blood clots (fibrin)

• Monomers of proteins are amino acids

• Amino acids join together by peptide bond

Copyright 2009, John Wiley & Sons, Inc.

Formation of a Dipeptide Bond

• Dipeptides formed from 2 amino acids joined by a covalent bond called a peptide bond– dehydration synthesis

• Polypeptides chains contain 10 to 2000 amino acids.

Primary Structure: ex.: lysozome

• Catalyzes hydrolysis of carbohydrates

Secondary Structure:Alpha helix: ex. hair

stabilized by hydrogen bonds

Beta pleat ex. silk

Tertiary Structure:

Protein channels

Quaternary Structure:ex.: hemoglobin

Enzymes

• Most enzymes are proteins; some RNA

• Speed up chemical rxn; biological catalyst

• Shape of protein allows it to bond to specific molecules called substrates, causes a change in shape

• maltase: maltose 2 glucose• lipase: lipids fatty acids• protease: proteins amino acids

**works best under certain temperatures

Enzymes

4. Nucleic AcidsDNA and RNA • Oganic molecules that contain

carbon, hydrogen, oxygen, nitrogen, and phosphorus.

• Deoxyribonucleic acid (DNA) = Genetic Code.

• Ribonucleic acid (RNA) relays instructions from the genes in the cell’s nucleus to guide each cell’s assembly of amino acids into proteins by the ribosomes.

• ATP – energy molecule• Monomers = nucleotides

Nucleic Acids

• There is a base-pairing rule:

– A always bonds across from T

– C always bonds across from G

• A and G, called purines, are structures composed of two rings

• C and T are pyrimidines – singled-ringed structures

• A purine always pairs with a pyrimidine and vice versa

Nucleic Acids• Because of this, if one strand of DNA is

known, the other strand can be deciphered

• If we know that one strand of DNA has the sequence:

ATCGGCA

• The other side must be:TAGCCGT