bio 2 test 1 ch1-8

element

substance that cannot be broken down to other ssubstances by chem rxn

when elements form chem bonds, they create

molecules n compounds

molecules

group of elements bonded tg

ex) o2

compounds

2 or more diff types of elements bonded tg

how many of 92 elements are essential to life

20-25%

trace elements (less than 0.01% mass)

• required in minute quantities

• STRONG IMPACT

• ex) B, Cr, Cu (protein), Fe (blood)

4 elements essential to life (96% of body)

• drives neurons/mucles

oxygen, carbon, hydrogen, nitrogen

toxic elements

too much of certain element=toxic

ex) Ar inc= cancer

atom

smallest unit of matter that retains properties of element

subatomic particles

neutrons, protons, electrons

atomic nucleus

neutrons+protons

neutron mass = proton mass measurements

identical, measured in daltons or amu

mass #

protons + neutrons

Li- atomic #=3, mass= 6.94, what is neutron#

4

energy

capacity to cause change

potential energy

energy that matter has due to location

electron’s potential energy

• farthest from nucleus (ELECTRON SHELL) = most PE
  

high PE, low KE

at the top

low PE, high KE

close to ground

what determines the chemical behavior of an atom?

the distribution of electron chells

valence electrons

• in outermost shell= valence shell

chemically inert

• full valence shell

• no sharing/giving electrons

• ex) noble gases

atoms w incomplete valence shells form what

share/give electrons= IONIC/COVALENT bonds

covalent bonds

• share electrons

• electrons count for both valence shells

• single, double, triple bonds

• electronegativity

• ex) h2

electronegativity

• atom’s attraction for electrons

• stronger electroneg=greedy= pulls atoms to itself

• IN COVALENT BONDS

• UP & RIGHT

nonpolar covalent bonds

share electrons equally

STROGNEST= need lotta energy to break

polar covalent bonds

1 atom more electroneg= electrons not shared equally

ionic bonds

• strip electrons from bonding partner

• attraction of cation and anion

• TRANSFER elections (IONS)

• EASY TO BREAK

weak chemical bonds

• NEED in life

• reversible= advantage

weak chemical bonds includes

• H+ bonds

• Van der Waals interations

• bonds btwn ionic compunds dissolved in water

H+ bonds

H atom attracted to electroneg atom

POLAR COVALENT BONDS

Van der Waals Interactions

• not constantly sharing election

• attracted to those closest

• occur by chance if E are asymm

• LEAST ENERGY to break= TEMP BONDS

gecko using ___ to stick their feet to tree

van der waals interactions

what determines how molecule interact

molecular shape and charge

ex) receptor shapes

molecular shape/function

small diff= diff cell activity

ex) T n estrogen exact same except extra H+ in estrogen

what gives water its emergent properties

H+ bonds (particial - and + charge)

water’s 4 emergent properties for life*

• cohesion/adhesion

• moderate temp

• expand when freezing

• versatile solvent

polarity of water

allow to interact w other h2o or diff substances

cohesion= high surface tension

h+ bond of water to water= hard to break surface of liquid

water moderating temp

• water absorbs heat from warm air

• release stored heat to cooler air

heat

• thermal energy TRANSFERRED from 1 matter to another

• WARM to COOL

heat transfer

measured by CALORIES

calories

amount of heat required to raise temp of 1g of ater by 1 degree C

why does water resists changes in temp

high specific heat (1 cal/g/degree C)

ex) metal pan heats faster than h2o in pot

why does water have high specific heat

H+ bonds

water’s high specific heat

• heat absorbed=h+ bonds break

• heat released=h+ form

• less temp change near oceans

heat of vaporization

• heat a liquid must absorb for 1g to convert to gas

evaporative cooling

• liquid evaporates, surface cools

• ex) sweat= heat transfers to h2o from skin, h2o evaporates

water expands upon freezing

H+bonds in ice= ordered/tighter= less dense

water: solvent of life

grape solvent bc h+ bonds & partical +/-

aqueous solution

water=solvent

ionic compounds dissolved in h2o

each ion is surrounded by HYDRATION SHELL

charge of hydrophillic

charged or partically charged

charge of hydrophobic

no charge

create barriers

only want other hydrophobes

organic chem

study of compounds w carbon

ex) living organisms, macromolecules

carbon bonds

• form large, complex molecules w covalent bonds

• 4 VALENCE ELECTRONS= variety of combos

hydrocarbons

hydrogen & carbon

• in fats (adipose tissue)

isomers

compounds with same molecular formula but diff structure/properties

• structural isomers

• cis-trans isomers

• enantiomers

structural isomers

same molecules but diff covalent arrangements of their atoms (diff branching)

cis-trans isomers

same molecules but same covalent bonds but diff spatial arrangements

cis: same side

trans: opp sides

enantiomers

same molecules but mirror images

• important in pharm/toxicology

• show sensitivity to subtle changes

organic molecules’ distintive properties depend on

carbon skeleton and R-group

functional groups

coponents of org molecules in chem rxn

• arrangment give molecules its properties

High macromolecule makes up most/ DA WORKERS

Proteins

Where are macromolecules unique properties arise from

orderly arrangements of their atoms

who is not a macromolecule, why

Lipids

NO REPEAT MONOMERS

Who r true polymers, why

Carbs, proteins, nucleic acids

MONOMERS REPEAT

BUILT N BROKEN DA SAME

proteins that speed up chem rxns

enzymes

dehydration rxn

BOND monomers by LOSING water

hydrolysis

BREAK polymers by ADDING water

what make up lipids

hydrocarbons + alcohol

how are monosaccharides classified?

location of carbonyl group (C=O) AND # of carbons in carbon skeleton

• SAME STRUCTURE, DIFF DEPEND ON CARBONYL GROUP

why do sugar have lots of energy/main source of fuel

carbon bonds

• break to give energy

glycosidic linkage

covalent bond in sugars

monomer (glucose)+monomer (glucose)

determents of polysaccharides shape/function

monomers + position of glycosidic linkage

polysaccharide storage in plants

STARCH

made of glucose monomers line, no branching

where do plants store starch

as GRANULES in CHLOROPLASTS n plastids

what is the simplest form of starch

amylose

UNBRANCHED

amylopectin

somewhat branched starch= ENZYMES attach to break= give energy

storage polysacc in plants

starch

UNBRANCHED

storage polysacc in animals

glycogen

BRANCHED

where is glycogen stored

liver and muscles

need energy to break toxins/move muscles

hydrolysis of glycogen releases what

glucose when sugar is needed

cellulose

polysacc of glucose

STRENGTH in CELL WALLS= hard to digest

glycosidic linkages of cellulose

beta= orientation of glucose

STR8 N UNBRANCHED= strong

• easy for glucose’s hydroxyl (OH-) to H+ bond to cellulose’s hydroxyl (trans)

• alt OH- crates parallel stack

glycosidic linkages of starch

alpha

HELICAL= soft/squishy

• easy to access glucose

• easy for glucose’s hydroxyl (OH-) to H+ bond to starch’s hydroxyl (cis)

enzymes that hydrolyze alpha bond in starch, cant hydrolyze ___?

beta linkages in cellulose

how does celluose break down if enzymes cant do it?

passes as insoluble fiber

• some microbes use enzymes

chitin

provides structural support for cell walls of FUNGI n insects’ EXOSKELETON

unifying feature of lipids

mix poorly w water

3 biologically important lipids

fats, phospholipids, steroids

2 monomers of fats

GLYCEROL n FATTY ACIDS

glycerol

1 of 2 lipid monomers

• 3 carbon alc w hydroxyl (OH) group attached to each carbon

fatty acids

1 of 2 lipid monomers

• carboxyl (C=O) group attached to long carbon skeleton

• carbon skeleton varies in length & H+

ester linkage creating glycerol+fatty acid

triacylglycerol

How can the fatty acids in a fat be diff from each other

Did length n diff saturation of H+ n C

#H+ in saturated fatty acids

Max # of H+

Solid @ room temp

Most animal fats

Unsaturated fatty acids

Have 1 or more double bonds

Liquid @ room temp

Plant & fish fats

Hydrogenation

Converts unsaturated fats to saturated fats by adding H+

Diet rich in saturated fats contributes to

Cardiovascular disease