chapter 2 the chemistry of life. california state standards 1h: most macromolecules in cells and...
TRANSCRIPT
Chapter 2Chapter 2
THE CHEMISTRY OF THE CHEMISTRY OF LIFELIFE
California State Standards
1h: most macromolecules in cells and organisms are synthesized from a small collection of simple precursor
4e: proteins can differ from one another in the number and sequence of amino acids
1b: enzymes are proteins that catalyze biochemical reactions without altering the reactions equilibrium and the activities of enzymes depend on the temperature, ionic conditions, and the pH of the surroundings
CHAPTER 2: THE CHEMISTRY OF LIFE The first job of a biologist is to understand the chemistry of life. 2-1 The Nature of Matter A. Atoms
___________= the basic unit of matter (has volume and mass; solid, liquid, gas, and plasma)
Atoms are made
Atoms
subatomic particles called protons,
neutrons, and electrons
= protons - -
= neutrons - -
= electrons -
-
-
_______________=center of an atom.Home to protons and neutrons.
Carbon AtomCarbon Atom
Positively charged1 amu
No charge
1 amu
Electronegative charge1/1840 amu
electrons travel in regions outside the nucleus called orbitals
Nucleus
B B. Elements Elements=
More than _____known kinds;
Found on the
100 2 dozen are common in living organisms
pure substances that consists entirely of one type of atom
Periodic table
Reading the Periodic Table Example: The element Carbon (only made of carbon atoms)
6
CCarbon12.011
Section 2-1
An Element in the Periodic Table
____________usually 1-2
letters
_______________= # Protons + # neutrons in an atom; the average of one elements isotopes
____________ of the element
Atomic number =
SYMBOL
MASS NUMBER
NAME
Number of protons in an atom; different for each element
Isotopes are the various forms of an atom that differ based on the number of neutrons in the nucleus such as C 14. The isotopes that differ from the most common form are often radioactive or unstable.
C. Chemical Compounds 1. Chemical compound=
Example: Sodium Chloride = Table salt Forms when
sodium and chlorine combine in a 1:1 ratio
2. Chemical formula=
Example: Sodium Chloride= NaCl 3. ____________________________ of a molecule Example: = white crystalline solid
= a soft silvery metal that reacts explosively with water
= poisonous greenish gas
a substance formed by the combination of 2 or more elements in definite
proportions.
a short hand that shows chemical composition
Chemical properties
NaCl Na
Cl
D. Chemical Bonds
• Atoms in compounds are
• Involves the
• 2 main types of bonds are: ___________ and _________
held together by links called chemical bonds.
interaction of electrons
covalent ionic
1. Ionic Bondsa.
b. ion=
are formed by the transfer of one or more electrons from one atom to another.
an atom that has a positive or negative charge as a result of gaining or losing electrons.
FORMING AN IONIC BOND
Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na +) Chloride ion (Cl -)
Transferof electron
Protons +11Electrons -11Charge
Protons +17Electrons -17Charge
Protons +11Electrons -10Charge
Protons +17Electrons -18Charge
Section 2 -1
Figure 2 - 3 Ionic Bonding
0 0 +1 -1
c. Opposite charges attract creating a bond between the ions
2. Covalent Bonds
a. formed by the
b. Sharing means
c. atoms sharing 2 electrons= __ electrons=double bond 6 electrons=
d. _________________= The smallest unit of most chemical compounds (those joined with covalent bonds)
sharing of electrons between 2 atoms.
that the moving electrons are actually traveling in the orbitals of both atoms.
single bond 4
triple bond
Molecule
What property of water explains why this insect can stand on water?
2-2
Why does ice float?
Solid (Ice) Liquid (water) Gas (water vapor)
Ice is less dense than water.
Water is Polar—uneven distribution of electrons
Hydrogen bonds
Water Cohesion & Adhesion
Water propertieshttp://www.uni.edu/~iowawet/H2OProperties.htmlhttp://www.ccs.k12.in.us/chsBS/kons/kons/physical_properties_of_water.htm
Solution
Water has a pH of 7 which means that [H+] = [OH-]
Acids contain higher concentrations of [H+] ions than water.Bases contain lower concentrations of [H+] ions than water.
2-2 Properties of Water- Refer to reader’s guide 2-3 Carbon Compounds
A. The Chemistry of Carbon1. Carbon has ________________ which means
carbon can form _________________
2. Living organisms are made up of molecules that consist
3. Carbon can bond with itself forming
Methane Acetylene Butadiene Benzene Isooctane
Section 2-3
Figure 2-11 Carbon Compounds
4 valence electrons 4 covalent bonds.
of carbon, hydrogen, oxygen, phosphorus, nitrogen and sulfur.
chains of unlimited length and form, rings, and complex structures.
B. Macromolecules1. Macromolecules=
2. Polymerization=
3. Monomers=
4. The _____ groups of organic compounds found in living things are:•• ••
are giant molecules consisting of 1000+ smaller molecules.
process of joining small molecules to form large molecules
small units that form polymers (large molecules)
4
carbohydrates lipids nucleic acids
proteins
Polymerizationhttp://www.uwsp.edu/chemistry/tzamis/additionpolymer.html
Made of
Example
Function Monomer
Carbohy-drate
C,H,O
1:2:1
GlucoseC6H12O6
1.Stores Energy -animals =
-plants =
2. Structural
Purposes-
-
Monosaccharide =
Mono + mono +mono=
Lipids Mostly
C, H
Verylittle O
1. Stores Energy
2. Form cell membranes
3. Waterproof coverings
4. Chemical messengers
1 glycerol3 fatty acidsSaturated-
Unsaturated-
GLYCOGEN
STARCH
PLANT CELL WALLS (CELLULOSE)
CHITIN (INSECT EXOSKELETON)
SINGLE SUGAR
POLYSACCHARIDE
FATSOILSWAXESSTEROIDS NO DOUBLE
BONDS IN FATTY ACID
AT LEAST ONE DOUBLE BOND
Challenge QuestionWhy are most unsaturated fats liquid at room temperature?
• Unsaturated
Nucleic acids
C HO P N
Stores and transmits hereditary information
Nucleotide=
1.
2. 3.
Proteins
CH O N
methionine
Shape determines function1.
2. pump small molecules in and out of the cell3. aids in cell movement
Amino acids
Made of
Example Function Monomer
DNA/RNA
5-C SUGAR
PHOSPHATE GROUP
NITROGENOUS BASE
20 KINDS
HELPS CONTROL RATE OF REACTIONS (ENZYMES)
Carbohydrates
Lipids
Nucleic acids
• Nucleic acids are polymers of nucleotides joined together to make large macromolecules.
• The important nucleic acids are deoxyribonucleic acid(DNA) and various types of ribonucleic acids(RNA).
Proteins
• Protein are the building blocks of our body. We find protein in our bones, and muscles. We find protein in our hair and nails. There is protein in our brain, and also protein is part of our blood.
Summaryhttp://www.chemistryland.com/ElementarySchool/BuildingBlocks/BuildingOrganic.htm
CarbonCompounds
include
that consist of
which contain
that consist of that consist of that consist of
which contain which contain which contain
Carbohydreat
Concept Map
Carbohydrates Lipids Nucleic acids Proteins
Sugars and starches
Fats and oils Nucleotides Amino Acids
Carbon,hydrogen,
oxygen
Carbon,hydrogen,
oxygen
Carbon,hydrogen,oxygen, nitrogen,
phosphorus
Carbon,hydrogen,oxygen,
nitrogen,
Concept Summary
Choose from the following: lipids, nucleotides, amino acids, fats and oils, sugars and starches, carbohydrates, nucleic acids, proteins
IQ Quiz: Chapter 21. What kind of compounds did we test in the lab?2. What chemical was used to test for simple sugars?3. What was a positive result?4. If we want to see if peanuts have fat in them what
could we do?5. How do we know if it is positive?6. What did copper sulfate and sodium hydroxide test
for?7. What was a positive result?8. If I had a bowl of cereal and Iodine fell into my cereal
and turned a blue-black color what do I know is in my cereal?
9. Name a food that had more than 1 compound in it? (tested positive for more than 1 test)
10. What are the four most common elements in living things?
2-4 Chemical Reactions and Enzymes A. Chemical Reactions =process that changes, or
transforms one set of chemicals into another. Always involves changes in chemical bonds.
1. Reactants=
2. Products=
EXAMPLE: HCl H + Cl
elements or compounds that enter a reaction
elements or compounds produced by a reaction
B. Energy in Reactions
• Activation Energy=
C. Enzymes
1. Catalyst=
energy that is needed to get a reaction started
a substance that speeds up the rate of a chemical reaction without changing itself.
AE without enzyme
AE with enzyme
reactants
products
Reaction with no enzyme
Reaction with an enzyme
2. Catalysts ___________________________in a chemical reaction.lower the activation energy
3. ______________ are ___________________ that speed up favorable (spontaneous) reactions.
4. Enzymes _____________ chemical reactions that take place in cells.
5. Enzymes are
Enzymes biological catalysts
speed up
very specific
D. Enzyme Action1. The Enzyme-Substrate Complex a. Enzymes provide a site where reactants can be
brought together to react (increasing the rate of reaction by reducing the activation energy)
Glucose
Substrates
ATP
Substratesbind toenzyme
Substratesare convertedinto products
Enzyme(hexokinase)
ADPProducts
Glucose -6-phosphate
Productsare released
Section 2 -4
Figure 2 - 21 Enzyme Action
Active site=
Enzyme ActivitySite on the enzyme where the substrate attaches
The reactants of a catalyzed reaction
Enzyme-substrate complex
b. Enzymes are not
2. Regulation of Enzyme Activity - Enzyme activity depends on environmental
factors such as: (enzymes in the stomach function best around pH=2) (human enzymes function best around 37°C)
consumed in the reaction; after products are formed, the enzyme is recycled.
pH
temperature
-Ionic conditions (coenzymes)-Substrate concentration (greater the concentration the greater the rate of the reaction)
http://www.lewport.wnyric.org/JWANAMAKER/animations/Enzyme%20activity.html
http://www.kscience.co.uk/animations/model.swf
Warm-up questions
1. Describe the difference between ionic and covalent bonds. Provide an example for each.
Warm-up
1. What are the 4 organic macromolecules which make up living organisms.
2. What are the monomers (building blocks) to these macromolecules.
Warm-up
1. What is a catalyst?
2. What are enzymes?
3. How do catalyst work?
4. What affects the activity of an enzyme?
Review
1. The positively charged particle in an atom is the
a. Neutronb. Ionc. Protond. electron
Review
2. Two or more different atoms are combined in definite proportions in any
a. Symbolb. Isotope c. Element d. Compound
Review
3. A covalent bond is formed by the
a. Transfer of electronsb. Sharing of electrons c. Gaining of electronsd. Losing of electrons
Review
4. When you shake sugar and sand together in a test tube, you cause them to form a
a. Compoundb. Mixturec. Solutiond. suspension
Review
5. A compound that produces hydrogen ions in solution is
a. Saltb. Acidc. Based. polymer
Review
6. In polymerization, complex molecules are formed by the joining together of
a. Macromoleculesb. Carbohydratesc. Polymersd. monomers
Review
8. Proteins are polymers formed from
a. Lipidsb. Carbohydratesc. Amino acidsd. Nucleic acids
Review
9. An enzyme speeds up a reaction by
a. Lowering activation energyb. Raising activation energyc. Releasing energyd. Absorbing energy
Review
10. In a chemical reaction, a reactant binds to an enzyme at a region known as the
a. Catalystb. Productc. Substrated. Active site
Standardized Test Prep
1. An attraction between different substances
2. Lower a chemical reaction’s activation energy
3. The elements or compounds that enter into a chemical reaction
Choose: Cohesion Adhesion Catalysts Reactants Products
STP
4. Which one of the following is NOT an organic molecule found in living organisms
a. Protein b. Nucleic acidc. Carbohydrated. Sodium chloridee. lipid
STP
5. Which combination of particle and charge is correct?
a. Proton: +b. Electron: +c. Neutron: -d. Proton: -e. Electron: 0
STP
6. In which of the following ways do isotopes of the same element differ?
a. # neutrons onlyb. #protons onlyc. #neutrons and protonsd. #protons and masse. #neutrons and mass
STP
7. Which of the following molecules is made up of glycerol and fatty acids?
a. Sugarsb. Starchesc. Lipidsd. Nucleic acidse. Proteins
STP
8. Nucleotides consist of a phosphate group, a nitrogenous base, and a
a. Fatty acidb. Starchc. Lipidd. 5 carbon sugare. 6 carbon sugar