CHAPTERS 2 & 3 BIOCHEMISTRY

CHEMISTRY!

EXAMPLES OF ELEMENTS C = ___________________ O = ___________________ H = ___________________ N = ___________________ P = ___________________ S = ___________________ Na = __________________ K = ____________________ I = ____________________ Cl = ___________________

ATOMS Atom = Subatomic particles: Proton = __________________ Neutron = _________________ Electron = _________________ _____________________________ _____________________________ _____________________________ __________________________________________ ___________________ that still maintains its properties

LETS DRAW A CARBON ATOM… 6 C

LETS DRAW A CARBON ATOM… Fill in Protons and Electrons Max # of electrons in shell 1 = _______ Max # of electrons in shell 2 = _______

CHECK FOR UNDERSTANDING! How many protons, neutrons, and electrons are in Iron, given the information in the periodic table ? P = N = E = 26 Fe Iron 55.85

PRACTICE DRAWING AN OXYGEN ATOM! 8 O

COMPOUNDS Compounds =

FORMULAS FOR COMPOUNDS 2H + O  H 2 O

FORMULAS FOR COMPOUNDS 2H + O  O HH

OrganicInorganic ALWAYS contains _____________ Usually contains ______________ Sometimes contains __________ Generally ____________________ Usually don’t contain _________ Generally come from the earth Generally ____________________

EXAMPLES: INORGANIC 2H + O  H 2 O H + Cl  HCl C + 2O  CO 2 Na + Cl  NaCl

EXAMPLES: ORGANIC ________________ ______ ________ _____________

BONDING! ___________________ Electrons __________________________ 7 N How to find the number of valence electrons: Answer =

THE OCTET RULE The octet rule states that all elements “want” to have the same configuration as the nearest noble gas. Example: What does magnesium (Mg) want to look like ? How might magnesium accomplish this ? A.K.A. ____________________________________________ ____________________________________________________ In most cases, this means ___________________________

THREE TYPES OF BONDING

COVALENT BONDING m/video/369/Covalent- Bond m/video/369/Covalent- Bond ______________________ = atom’s attraction for shared electrons/pull of electrons Nonpolar covalent bonds = _______________ ________________________ Polar covalent bonds = ________________________

IONIC BONDING Each atom has now become an Ion. An Ion is _______________ _______________________

HYDROGEN BONDS A hydrogen bond is the attractive interaction of a _________________________ with an ________________ ______________, such as nitrogen, oxygen or flourine.

IMPORTANCE OF HYDROGEN BONDING Properties of water:

MOLECULAR DIVERSITY DEPENDS ON... _______________ ● Length ● Branching ● Double bonds ● Rings ________________ ● Participate in chemical reactions in specific and unique ways. ● Polar → Hydrophillic

FUNCTIONAL GROUPS 1.) ________________ (-OH) = hydrogen bonded to oxygen then bonded to the carbon skeleton – Alcohols 2.) _______________ (-C=O) = carbon double bonded to an oxygen

3.) _____________ (-COOH) = doubled bonded oxygen AND a hydroxyl group 4.) _______________ (-NH2) = nitrogen bonded to two hydrogens and the carbon skeleton 5.) _______________ (-PO4) = phosphate bonded to four oxygen atoms

6.) _____________ (-CH3) = carbon bonded to three hydrogens – Gene Expression Take-Away Point : Small differences in functional groups = Large difference in form and function!

Which functional groups do you see in the molecules below?

GENERAL STRUCTURE Organic compounds are composed of hundred to thousands of individual molecules. These ____________________________________ The ______________________________________

MAKING POLYMERS! Monomers are linked together via ________________ ____________________________ What do you think is involved in this process???

DEHYDRATION SYNTHESIS

BREAKING POLYMERS! To break polymers (such as in digestion), cells use __________ What key words do you see?

HYDROLYSIS

MACROMOLECULES Four Types: Essential to maintaining life processes: cell function, storage, energy, homeostasis, and genetic information

CARBOHYDRATES The ratio of atoms is usually 1C:2H:1O or CH 2 O. Example: Glucose → C 6 H 12 O 6 Primary Function: Provide energy to cells.

TYPES OF CARBOHYDRATES Carbohydrates are classified according to size. One sugar is a: _________________________________ Two sugars make a: ____________________________ Many sugar molecules linked together is a: _______________________________________________

FORMATION OF MALTOSE (DISACCHARIDE) Glucose = C 6 H 12 O 6 Maltose = C 12 H 22 O 11

POLYSACCHARIDES Four Common Types: 1. _________ → Storage in Plants 2. _________ → Storage in Animals 3. _________ → Lettuce! 4. ______ → Exoskeleton

Lipids = They are _____________________, which means… Made of ____________________= LIPIDS

Monomers Glycerol contains the hydroxyl (OH) group. Fatty acids contain the carboxyl (COOH) group.

Long chains of hydrocarbons (carbon atoms with attached hydrogen atoms) Saturated fats contain only ________________ bonds between the carbon atoms. Unsaturated fats contain one or more _______________ or _______________ bonds between the carbon atoms. Fatty Acids

Saturated Fats have a strong link to arthrosclerosis (hardening of the arteries due to plaque buildup). Take a look at the structure of these two fats, and explain why.

STEROIDS Lipids where carbon skeleton contain four rings

PROTEINS Monomers : Structure of Amino Acids : R Group :

Protein Function Most important role = ___________ An enzyme is a Structure = Function

LINKING AMINO ACIDS!

NUCLEIC ACIDS: 3.14 PG 46 Two Types: ● DNA = Deoxyribonucleic acid ● RNA = Ribonucleic acid Monomers: Nucleotides Key Functional Group: Phosphate Group

More information to come in our DNA unit! -Complimentary bases -Transcription -Translation

REVIEW / STUDYING Please use the following materials to review for this unit test: PowerPoint Presentation Notes! Organic Molecules Review Guide! Organic Molecules Worksheet! Textbook Unit Outlines! JEOPARDY! Biochemistry Study Guide!