Biochemistry

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Covalent Bonds

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95 Terms

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Covalent Bonds

  • Sharing of valance electrons by 2 atoms

  • Strongest bond

  • form molecules in cell

    • Single Cov → sharing 1 pair of electrons

    • Double Cov → sharing 2 pairs of electrons

  • Polar & Non-polar Cov Bonds

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Polar Covalent Bonds

Unequal sharing of electrons in the cov. bond

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Electronegative Atom

Has a strong pull on electrons

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Non-Polar Covalent Bond

Equal sharing of electrons in cov. bond

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Ionic Bond

Transfer of electrons from 1 atom to another → causes both atoms to have a charge

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Cation

Pos Atom in ionic bond

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Anion

Neg Atom in Ionic bond

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Ion

Just a charged atom

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Weaker Bonds

  1. reenforce shape of large molecules

  2. help molecules adhere to each other

  3. allow for temporary interactions

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Hydrogen Bonds

  • form when H is cov. bonded to one atom and then is also attracted to another electroneg. atom

  • ex: H on H20 is attracted to O on another H2o molecule

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Water

  • all living orgs. need water

  • cell = 70-95% water

  • water is a polar molecule

    • able to h-bond with other polar molecules

4 emergent properties of water:

  1. Cohesion & Adhesion

  2. Temp Moderation

  3. Expansion Upon Freezing

  4. Versatility as a solvent

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Cohesion & Adhesion

Cohesion: H2O molecules stick to each other thru h-bonding

Adhesion: H2O molecules sticking to other polar molecules thru h-bonding

Both contribute to surface tension

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Surface Tension

  • how hard it is to break the surface of a liquid

  • Connect to cohesion and adhesion

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Temp. Moderation

  • water has a ^ specific heat

    • measure of how well a substance resists a change in temp (when it absorbs/ releases heat)

  • water resists a change in it’s temp

  • ex: biological relevance: bodies of water have stable temps

    • allows for the health of species that live there

    • milder climate

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Expansion upon Freezing

  • ice is ~10% less dense than water

  • ice floats on top of water

  • as liquid, water’s h-bonds are irregular/unstable

  • as solid, water’s h-bonds are stable/organized so h2o expands as it freezes

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Versatile Solvent

  • like dissolves like

  • H20 is polar

  • water can dissolve other polar substances

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Hydrophillic

  • water-loving

  • affinity for H2O

  • polar/charged particles/molecules, sodium chloride

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Hydrophobic

  • water fearing

  • repels water

  • ex: non-polar, non-ionic

  • Oil

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pH scale

  • relative concentration of H ions

  • Acids < 7, excess of H

  • Bases > 7, excess of OH

  • Neutral = 7

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Physiological pH

7.4

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Carbon Chem/ Orgo

  • Carbon can form macromolecules

  • Tetravalent

  • Major partners = (C, H, O, N)

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Macromolecules

  • diverse, large, and complex molecules

  • C forms

  • Carbs

  • Nucleic Acids

  • Protein

  • lipids

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Tetravalent

  • 4 valance electrons

  • can form 4 cov. bonds

  • ex: C

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Hydrocarbons

  • non-polar, hydrophobic

  • molecules made up of H & C

  • in living things, in lipids

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Functional Groups

  • 6 groups

  • components of macromolecule involved in chemical rxns

  • ex: phosphate

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Polymer

  • large molecules composed of building blocks called monomers

  • 3 macromolecules are polymers

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Monomer

  • cov. linked to form polymers

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Synthesis

  • to make something

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Dehydration Synthesis

  • allows the formation of polymers

  • h20 is taken away & a new cov. bond is left in its place

  • how monomers are added to make polymers

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Hydrolysis Rxns

  • reverse of dehydration synthesis

  • breaking w/ water

  • breaking apart polymers into monomers

  • h20 is added, breaks cov. bond b/w monomer & polymer chain

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Carbs

  • monomers = monosaccharides

  • molecular formula is usually multiple of CH2O

  • Sugars -ose

  • 2 monosaccharides → disaccharides

    • covalent bond = glycosidic linkage

    • b/w two monosaccs.

  • 3 or more monosaccs. → produces polysaccharides

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Monosaccharides

Monomers of Carbs

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Disaccharides

2 or more monosaccharides

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Polysaccharides

  • 3 or more monosaccharides

  • Glycogen

  • Chitin

  • Starch

  • Cellulose

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Glycosidic Linkage

Covalent bond between monosaccharides

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Glycogen

  • Animal: Energy Storage

  • helical shape

  • stored in liver & muscles

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Chitin

  • Animal: Structural

  • linear shape

  • exoskeleton of arthropods

  • ex: surgical thread

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Starch

  • Plant: enegry storage

  • helical shape

  • store starch in chloroplasts

*plants access energy by breaking down starch

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Cellulose

  • Plant Structure

  • linear

  • straight form string building material

  • major compound of plant cells

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Proteins

  • macromolecules

  • have diverse fxns

  • do all jobs in the cell

  • Made of amino acids and polypeptides

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Amino Acids

monomer of proteins

20 types

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Polypeptide

polymer of protein

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Peptide Bond

cov. bond b/w monomers

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R group

  • part of the a.a that is different from 1 a.a to another

  • connected to main carbon

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Primary Structure

  • sequence of a.a monomers

  • held together by peptide bonds (strong bonds)

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Secondary Structure

  • coils and folds in the polypeptide

  • result from h-bonding

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Tertiary Structure

  • caused by interactions b/w R groups of the a.a’s

  • Every protein has tertiary, secondary, and primary structure

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Quaternary Structure

  • only found in proteins made of multiple polypeptides

  • 2 or more polypeptides

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Denaturation

  • loss of protein shape ( 2nd, 3rd, & 4th structure)

  • denatured protein = biologically inactive ( loses function)

  • 1st structure is not effected b/c it is held together by cov. bonds

  • Causes:

    • extreme pH

    • high temps

    • high salinity

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Renaturation

  • protein gaining shape & function again

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Nucleic Acids

  • DNA & RNA

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RNA

  • ribonucleic acid

  • Monomers: A, G, C, U

  • Sugar: Ribose

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DNA

  • Deoxyribonucleic acid

  • genetic code

  • directs the synthesis of proteins

  • Letters: A, G, C, T

  • Pentose: deoxyribose

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Nucleotide

Monomer of nucleic acids

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Polynucleotide

Polymer of nucleic acids

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Phosphodiester Linkage

Cov. bond b/w monomers

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Lipids

  • do not form polymers

  • mainly hydrocarbons

  • most important:

    • fats

    • phospholipids

    • steroids

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Fats (Triglycerides/triglycerals)

  • 3-carbon molecule w/ hydroxyl group attached to each carbon

  • 3 fatty acids = carboxyl group + hydrocarbon (16-18 carbons)

  • fatty acids attached to glycerol thru dehydration syn.

  • major function = energy storage

  • Sat & UnSat

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Phospholipids

  • Phosphate -

  • made up pf glycerol + 2 F.A + 1 P

  • F.A = hydrophobic

  • P = hydrophilic

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Steroids

  • carbon stack w/ 4 fused rings and functional groups attached

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Ester Linkage

Cov. bond b/w lipids

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Saturated Fats

  • saturated w/ H

  • no double bonds b/w carbon

  • solid at room temp

  • animal fats

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Unsaturated Fat

  • “unsaturated with H”

  • 1 or more double bonds w/ carbon

  • oils

  • liquid at room temp

  • * double bond prevents tight packing of molecules

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Metabolism

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Metabolic Pathway

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Catalyze

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Catabolic

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Anabolic

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Non-Spontaneous

  • requires input of energy

  • cannot

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Spontaneous

  • occur w/o input of energy

  • can be fast or slow

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Free Energy (G)

  • potential energy that can do work in a cell

  • Change in G for a rxn = G final - G initial

  • Rxns w/ a - Change in G are spontaneous

  • rxns w/ a + change in G are non-spontaneous/anabolic/endergonic

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Exergonic

  • - Change in free eneergy (G)

  • release G (used to do work in the cell)

  • Exergonic / Catabolic / Spontaneous

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Endergonic

  • consume/ Use G

  • Store G in molecules

  • Endergonic / Non-Spontaneous / Anabolic

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Mechanical Work

Physical change

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Transport Work

Moving substances across membrane

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Chemical Work

Ex: Synthesis of polymers

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ATP

  • Energy molecules

  • Hydrolysis rxn breaks a p-p cov bod

    • G is released

    • products are ADP + P

  • Renewable resource

  • Energy Intermediate

    • stores potential energy

    • provides G for cellular work

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Energy Coupling

exergonic process drives endergonic process

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