Transcript Chapter 2: The Chemistry of Life

Chapter 2: The Chemistry of Life
http://www.chem.ufl.edu/~itl/2045_s00/matter/FG01_011.GIF
Chapter 2 Vocab
1.
2.
3.
4.
5.
6.
7.
8.
Reactant
Product
Activation energy
Substrate
Enzyme
Carbohydrate
Nucleic acid
Nucleotide
9. Protein
10. Amino acid
11. Lipid
12. pH scale
13. Acid
14. Base
15. Ionic bond
16. Covalent bond
2-1 Objectives
• 1. Use a periodic table to give atomic number
and mass.
• 2. Name simple ionic and covalently bonded
compounds.
Atom: the smallest unit of matter
• Subatomic particles
– 1. neutron
• a. In nucleus
• b. No charge
• c. Weight 1dalton
– 2. proton
• a. In nucleus
• b. + charge
• c.Weight 1 dalton
– 3. electron
•
•
•
•
a. Outside nucleus
b. Move at speed of light
c. Have a negative charge
d. Weight1/2000 of a dalton
http://www.wjcc.k12.va.us/ROBB/Atom%20Animation%20Resources_files/image003.gif
If you are not able, use the table!
http://www.corrosionsource.com/handbook/periodic/periodic_table.gif
Atomic Number and Weight
• 1. atomic number- number of protons in
nucleus
• 2. atomic weight- number of protons plus
neutrons in the nucleus of the atom (a.k.a. mass number)
http://www.wisegorilla.com/images/chemstry/PeriodicTable.gif
How many neutrons are in an atom?
Subtract the number of protons from the mass
number (which = p+n) to get the number of
neutrons
Mass number – atomic number = # of neutrons
Find the atomic number, atomic mass, and
# of protons, electrons and neutrons of the
following elements.
Atomic Mass #
#
#
#
#
protons electrons neutrons
Carbon
Hydrogen
Oxygen
Isotopes of Carbon
Isotopes of Carbon
Electron Shells
• 1. Energy Shells
– a. first level can only
have 2 electrons.
– b. second level can have
8 electrons.
– c. all other levels have 8.
• 2. The chemical
behavior of the atom is
determined by the
atom’s electron shell.
• 3. Valance Electronsoutermost shell
http://static.howstuffworks.com/gif/atom-h-he-li-na.gif
Problem? All atoms want to have their
valance electron shells full!
I wish I could be a noble gas!
http://www.csupomona.edu/~egoldstein/121/IMAGES/Periodic_noble.gif
Why does everyone want to be a noble
gas?
Hindenburg Video
http://www.youtube.com/watch?v=F54rqDh2mWA
Hindenburg Video 2
http://dsc.discovery.com/videos/mythbusters-burnblimp-burn.html
Chemical Bonds
• 1. Making of chemcial bonds Stores Energy.
• 2. The breaking of chemical bonds Releases Energy
Blah blah balh
Sdf
http://faculty.clintoncc.suny.edu/faculty/michael.gregory/files/Bio%20101/Bio%20101%20Lectures/energy/energy12.gif
Chemical Bonds
• 1. Covalent bond -The
sharing of a pair of
valance electrons by
two atoms.
Caring is
sharing!
http://www.school-for-champions.com/chemistry/images/bonding_types-water.gif
http://www.roboimages.com/image/ri33813/Care_Bears_Easter.jpg
Methane: covalent bonds
http://sixthsense.osfc.ac.uk/chemistry/bonding/GRAPHICS/gif15.CH4bp.gif
2. All non-metals form covalent bonds
• 1. glucose
• 2. water
• 3. carbon dioxide
• 4. sucrose
http://www.peoriaendocrine.com/images/diabetes_lecture/glucose.GIF
http://www.brooklyn.cuny.edu/bc/ahp/SDgraphics/PSgraphics/WaterMolecule.GIF
Common Prefixes
•
•
•
•
•
1 — mono
2 — di
3 — tri
4 — tetra
5 — penta
•
•
•
•
•
6 — hexa
7 — hepta
8 — octa
9 — nona
10 — deca
Naming Covalent Compounds
Prefix + First element
+
Prefix + Second Element + -ide
Example:
CO2 becomes Carbon dioxide
Unless! the element is bonded to itself (Ex: Cl2 = chlorine)
What is Dihydrogen Monoxide?
• Name the following covalent
compounds:
a) SiF4
a)
b)
silicon tetrafluoride
N2S3
b) dinitrogen trisulfide
c)
HBr
c) hydrogen bromide (or
hydrobromic acid)
d)
Br2
d) bromine
Ionic Bonds
• 1.One atom “steals”
electrons from another to
complete its outer shell.
• Example: NaCl
– Because one atom has lost
an electron (Na) it has now
has an overall charge of +1
– Because the atom that took
the electron (Cl) now has
an extra electron, its overall
charge is -1
http://www.sci.sdsu.edu/classes/biology/bio100/truesdale/Lectures%2005/lec2/Image6.gif
4. Ionic Bonding: all metals
http://gcserevision101.files.wordpress.com/2009/02/halogen-ionic-bond.jpg
Name the following Ionic Compounds
• NaOH
• Sodium hydroxide
• KCl
• Potassium chloride
• H2 S
• Hydrogen sulfide
Naming Ionic
Compounds
Example:
Magnesium iodide
• Step 1: What chemical
symbols do you need?
• Step 1:
• Step 2: How many atoms of
each element are needed to
make the bond?
• Step 2:
a. Find the charges for each ion
using the periodic table
Mg
and
I
a. Mg = +2
I = -1
b. Mg(1)I(2) => MgI2
b. “Cross the charges”
2-2 Objectives
• 1. Analyze the properties of water.
• 2. Distinguish between acids and
bases.
Water is a Major Components of
Cells
1. 2/3 of all molecules in the
body (all your cells are
surrounded by water)
2. Water stores heat
efficiently.
a. sweating- helps release
heat
b. helps maintain
homeostasis by regulating
temperature
http://www.bigbrandwaterfilter.com/water_filter_images/waterdrop_embossed.gif
Water bonds to itself and other
surfaces
• Adhesion- between
different substances
*includes capillary
action
Cohesion-between similar
substances
nce/sp/en/syllabus/unit5/images/roots%26soil1.jpg&imgrefurl=http://resources.ed.gov.hk/~s1sci/R_S1Science/sp/en/syllabus/unit5/article-ce.htm&h=150&w=150&sz=6&tbnid=_euQe4K3sE8J:&tbnh=90&tbnw=90&hl=en&
Water Dissolves Many
Substances
• Solution- mixture in
which one or more
substances is evenly
distributed.
• Many important
substances are
dissolved in blood.
http://www.elmhurst.edu/~chm/demos/images/bluebottle.GIF
Polarity-molecules with an
electrical charge
• Water is a polar
molecule
• Only polar molecules
will dissolve in water
• Nonpolar molecules
will not dissolve in
water – oil
Polarity Video!
http://colossus.chem.umass.edu/genchem/whelan/class_images/Structure_of_Water.jpg
http://www.youtube.com/watch?v=VhWQ-r1LYXY&feature=player_embedded
Water molecules adhere to other polar molecules.
+
Hydrogen Bonds -
water molecule
+
+
+
+
-
-
+
+
+
-
-
HCl
hydrogen bond
+
+
+
Acids and Bases
• Water can be broken
down into acids and
bases
• Acids1) high concentration
of hydrogen ions.
2) pH less than 7
http://www.epa.gov/acidrain/site_students/images/phscale.gif
Acids and Bases
Bases –
1) Low concentration of
hydrogen ions
2) pH is greater than 7
7 is neutral-pure water
http://www.btinternet.com/~chemistry.diagrams/ph_scale.gif
pH (2)
More H+
More OH-
Review Question
• 1. What type of molecules will dissolve in
water?
• 2. What is a pH scale?
• 3. What is an acid and a base?
• 4. What is neutral on the pH scale.
• 5.Will oil dissolve in water?
• 6. Which has more hydrogen ions, an acid
or a base?
2-3 Objectives
• 1. Summarize the characteristics of organic
compounds.
• 2. Distinguish between carbohydrates, lipids
and proteins.
• 3. Describe the structure and function of
nucleic acids and ATP.
Organic Compounds
• Contain carbon usually bonded to
oxygen, hydrogen,
and other carbon
atoms.
• Most of the matter
in your body is
organic!
• These are
compounds that
usually come from
organisms
http://www.chemistryland.com/ElementarySchool/BuildingBlocks/Jungle500.jpg
Carbohydrates
http://www.exploratorium.edu/cookng/candy/images/sugar-molecule-1.gif
• 1.Made of carbon,
hydrogen, and oxygen
in a 1:2:1 ratio.
• 2. Key source of
energy-Found in fruits
and vegetables.
• 3. Monosaccharidessingle sugars,
– A. the building blocks
of carbs
– B. Ends in-ose
• Examples: glucose,
fructose, maltose
http://vienna-doctor.com/images/Pictures/carbohydrates.jpg
Disaccharides and
Polysaccharides
• 4. Disaccharides- two
sugars
glucose + fructose =
sucrose
5. Polysaccharides
-a. macromolecule made
of many sugars.
-b. storehouse for energy
Excess Energy is stored as:
-c. starch-in plants
d. glycogen- in animals
e. cellulose-found in plant
cell walls
http://www.pecanbread.com/new/saccharides.jpg
Let’s Draw a Glucose molecule!
• 1. Draw the carbon ring
– It has 6 sides
• 2. Number the carbons 16
• 3. Label # 6 carbon
• 4. carbons 1, 2, 4 are the
same, have OH on the
bottom.
• 5. # 4 carbon is a HO!
• 6. # 3 carbon is odd, OH
on top
http://www.thefreshloaf.com/files/u12441/alpha-D-glucose%20ring.gif
http://kentsimmons.uwinnipeg.ca/cm1504/Image71.gif
Dehydrations synthesis: making
carbohydrates
Taking water away to join molecules
• 1. Dehydrate means to
take water away.
• 2. #1 and #4 carbon
will form a bond by
removing water.
• 3. What is left?
http://www.uq.edu.au/_School_Science_Lessons/16.3.1.4ach.GIF
Lipids- are nonpolar
• Fats, phospholipids,
steroids(cholesterol)
and waxes.
• Found in plant
pigments such as
chlorophyll.
• Fats are lipids that
store energy
– Saturated fat- animal
fat, solid at room
temp.
– Unsaturated fat-plant
oils, liquid at room
http://www.bodybuilding.com/fun/crisco1k.jpg
http://cwx.prenhall.com/bookbind/pubbooks/hillchem3/medialib/media_portfolio/text_images/CH09/FG09_16-05Box.JPG
http://www.healingtouchwebhelp.net/image/heart31.jpg
http://www.chemistryland.com/ElementarySchool/BuildingBlocks/Lipids.jpg
Lipids are made by combining two
types of molecules
• 1. glycerol
– A three carbon alcohol
• 2. 3 fatty acids
– Long hydrocarbon
chains.
– Non polar
http://faculty.clintoncc.suny.edu/faculty/michael.gregory/files/Bio%20101/Bio%20101%20Lectures/Biochemistry/glycerol,%20fatty%20acids,%20triglyceride.gif
Dehydration Synthesis: lipids
Lipids: Fats
Saturated vs. Unsaturated
Structural
formula of a
saturated fat
molecule
Stearic acid, a
saturated fatty
acid
Structural formula
of an unsaturated
fat molecule
Oleic acid, an
unsaturated
fatty acid
(a) Saturated fat
(b) Unsaturated fat
cis double
bond causes
bending
Proteins
• Made of chains of
amino acids
• There are 20 known
amino acids
• These 20 amino acids
are found in all
biological species.
• Collagen-protein
found in skin
• Hemoglobin, blood
clots, and muscles.
http://images.apple.com/science/profiles/proteinfolding/images/proteins.jpg
http://www.cybered.net/library/Teaching_Resources/Biology/Genetic_Engineering/Image_Gallery/GeneticEng-Proteins.jpg
All Amino Acids have the same basic
structure
• 1. alpha carbon- makes center
of amino acid
• 2. amino group
• 3. Carboxyl group- this is an
acid
• 4. a single hydrogen
• 5 . Variable group-R
– There are 20 R groups
– Therefore there are 20
different amino acids in all
living things
http://www.contexo.info/DNA_Basics/images/aminoacidsweb.gif
Let’s draw an amino acid
• 1. draw the alpha
carbon
• 2. put in amino group.
• 3. put in carboxyl group
• 4. Hydrogen
• 5. R group (variable)
http://www.aloeveraibs.com/wp-content/uploads/2008/08/aminoacidstruc.jpg
Amino Acids form bonds
•
•
•
•
1. forms peptide bond.
2. Oxygen is taken from the carboxyl group
3. Hydrogen is taken from the Amino group
4. Called Dehydration Synthesis
Peptide Bonds: dehydration
synthesis
http://bill.srnr.arizona.edu/classes/182/PeptideBond-HiRes.JPEG
Nucleic Acids
http://www.duke.edu/web/MAT/jennifer_sohn/unit/images/what_is_rna1.gif
• Made of nucleotides.
• Nucleotides contain a
sugar, phosphate and
a nitrogen base.
• DNA-double stranded
and makes up
chromosomes
• RNA-single stranded,
used in making
proteins.
DNA and RNA
http://images2.clinicaltools.com/images/gene/dna_versus_rna_reversed.jpg
ATP-Adenosine Triphosphate
• Energy currency for
the cells.
• Cells need a
constant supply of
ATP to function.
http://www.colorado.edu/epob/academics/web_resources/cartoons/atp.gif
Review Questions
• 7. In what ratio is carbon, hydrogen and oxygen
found in carbohydrates?
• 8. All sugars end in what?
• 9. What is the difference between a
polysaccharides, disaccharide, and a
monosaccharide?
• 10. Give and example of 2 polysaccharides.
• 11. What are the two types of fats?
• 12. What are proteins made up of ?
• 13. Name two types of nucleic acids.
Objective 2-4
• 1. Describe the role of enzymes in chemical
reactions.
• 2. Explain how enzymes work.
Organisms Need Energy for Life
Processes
• Energy- the ability to move
or change matter.
• A. Energy is stored and
released by chemical
reactions.
• B.Reactants and products
• Chemical reaction absorb
and release energy
– 1.Freezing water
releases energy
– 2.Melting ice absorbs
energy
http://www.windows.ucar.edu/teacher_resources/activities_3x3.jpeg
Energy is needed to start a
chemical reaction.
• 1. Activation energythe energy needed to
start a chemical
reaction.
• 2. Chemical push!
http://www.colorado.edu/intphys/Class/IPHY3430-200/image/04-3.jpg
Enzymes help biochemical
reactions occur.
• A. allows reactions to
occur quickly and at low
temperatures.
• B. increases the speed of
chemical reactions.
• C. most are proteins.
• D. act as catalysts-reduce
the amount of activation
energy required.
• E. helps maintain
homeostasis.
http://w3.dwm.ks.edu.tw/bio/activelearner/06/images/ch06c1.jpg
Enzymes End in ase
https://www.google.com/search?q=lactose+and+lactase+reaction&source=lnms&tbm=isch&sa=X&ei=Mkc
3UufDMtPH4AP6goEY&ved=0CAcQ_AUoAQ&biw=1440&bih=805&dpr=1#facrc=_&imgdii=_&imgrc
=_W7J_yOT05rFmM%3A%3BO8f3SM6l45zgtM%3Bhttp%253A%252F%252Fwww.chemicalconnection
.org.uk%252Fchemistry%252Ftopics%252Fimages%252Fpp8.jpg%3Bhttp%253A%252F%252Fwww.che
micalconnection.org.uk%252Fchemistry%252Ftopics%252Fview.php%253Ftopic%253D5%2526headingn
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Enzymes affect specific substances.
http://library.thinkquest.org/3659/orgchem/lock-key-enzyme.gif
http://www.blc.arizona.edu/courses/181summer/graphics/graphics%20lect7/Life7e-Fig-06-10-0%203D%20fit%20of%20enzyme%20and%20substrate.jpg
• 1.Substrate-substance on which an enzyme
acts.
– A. amylase- breaks starch down into glucose
• 2.Active Site
– A deep folds in the surface of the enzyme.
– B. substrate fits into the active site
Enzymes are Biological Catalysts
http://www.staff.uni-mainz.de/lieb/tierphys/enzyme.gif
Three things that effect enzyme
action.
• 1. amount of enzyme concentration
• 2. Temperature
• 3. pH
https://www.google.com/search?q=lactose+and+lactase+reaction&source=lnms&tbm=isch&sa=X&ei=Mkc3UufDMtPH4A
P6goEY&ved=0CAcQ_AUoAQ&biw=1440&bih=805&dpr=1#facrc=_&imgdii=_&imgrc=19PXmfPEXBeumM%3A%3B
nTw62t7ir_X6M%3Bhttp%253A%252F%252Fweb.mit.edu%252Fkevles%252Fwww%252Flactose.gif%3Bhttp%253A%252F%252
Fweb.mit.edu%252Fkevles%252Fwww%252Fnomilk.html%3B677%3B233
Review Questions
•
•
•
•
14. What is activation energy?
15. What is a catalyst?
16. Why are enzymes important?
17. Where does the substrate bind to on the
enzyme?
• 18. What do all enzymes end in?
• 19. What three thing can effect how an
enzyme works?