biological chemistry microbiology – chapter 2. interactive notebook: left side what is an atom?...
TRANSCRIPT
Interactive Notebook: Left Side
What is an atom?
What is an element?
What is the name of the table that keeps track of all the elements?
Why do biologists study chemistry??
Chemical changes in matter are essential to all life processes
All living things are made of the same kinds of matter that make up non-living things
If you learn how changes in matter occur you will understand the life processes of organisms
Elements
Elements – pure substances that cannot be broken down chemically into simpler kinds of matter
Of more than 100 elements fewer than 30 are important to livings
More than 90% of the mass of living things is composed of combinations of just: O, C, H and N
Elements
Chemical Symbol – usually part of the element’s name or the Latin word for the element
Organized into the periodic table of elements There are 118 elements, 94 are naturally occurring,
the rest are synthetic (made in particle accelerators) Elements listed by increasing atomic number Columns – groups of elements with similar properties
because of the number of electrons in their outer shell Rows - periods
Atoms – basic units of matter
-Atoms are the simplest particles of an element that retain all the properties of that element
-Atoms are so small that their true structure has not been observed
-Models of the atom help us understand their structure enough to predict how they will act in nature
Atoms
Structure – net electrical charge of zero a. Protons (charge +) 1 AWU b. neutron (charge 0) 1 AWU c. electrons (charge -) .008 AWU
AWU – atomic weight unit
Nucleus – central mass of an atom, contains protons and neutrons
Atoms
Electrons – high energy particles that move about the nucleus at high speeds in one of several different energy levels- Electrons in outer energy levels have more energy than those in inner energy levels
- Each energy level can only hold a certain number of electrons- 1st energy level can hold 2 electrons-2nd energy level can hold 8 electrons
- In most elements, the outer energy level is not filled
Atomic number – the number of protons in the nucleus of the atom
Atomic mass – the number of protons plus neutrons in the nucleus of the atom
Isotopes
Isotope – A different form of an element which has the same number of protons
and electrons, but has a different number of neutrons
Carbon (C):-atomic number is 6 - it has 6
protons-mass number is 12 – it has 6
protons and 6 neutrons-C14 – isotope that has 8 neutrons
Isotopes
Radioisotopes – radioactive element forms whose nuclei can undergo spontaneous change in which charged particles and radiant energy are released
Interactive Notebook: Left Side
What is the positively charged particle in an atom called?
What is the negatively charged particle in an atom called?
What is the neutral particle in an atom called?
What is an isotope?
Compound
1. A pure substance made up of two or more elements combined chemically
2. The properties of compound differ from the elements it is composed of – H2O vs. H and O
3. The proportion of each kind of element are fixed – Water always H2O
4. Elements combine and form compounds to become more stable
5. Elements are more stable when their outer electron shells are filled
Bonds
Chemical bonds – forces link two or more atoms
a. Covalent bonds – sharing of electrons (water H2O)
b. Ionic bonds – transfer of electrons (sodium chloride NaCl)
Molecules
A molecule is the simplest part of a substance that retains all of the properties of that substance and that can exist in a free state
Hydrogen gas (H2) Water (H2O)
2. INORGANIC CHEMISTRY
STUDY OF COMPOUNDS THAT DO NOT CONTAIN THE THREE ELEMENTS C, H, & O AT THE SAME TIME.
CAN CONTAIN TWO OF THOSE THREE AND ANY OF OTHER ELEMENTS
EXAMPLES OF INORGANIC COMPOUNDS:SODIUM CHLORIDE (SALT) NaCl, SULPHUR
DIOXIDE SO2
Interactive Notebook: Left Side
IF LIVING ORGANISMS CONTAIN THE SAME CHEMICALS FROM THE PERIODIC TABLE AS NON-LIVING THINGS: WHAT MAKES LIVING ORGANISMS
DIFFERENT?
3. ORGANIC CHEMISTRY
STUDY OF CARBON COMPOUNDS - CHEMICAL BASIS FOR LIVING CELLS ALWAYS C, H, & O SOMETIMES NITROGEN & PHOSPHORUS USUALLY SMALL AMOUNTS OF METALS
THERE ARE “FOUR” DIFFERENT CLASSES OF ORGANIC COMPOUNDS Carbohydrates Lipids Proteins Nucleic Acids
Carbohydrates
Organic compounds of C, H and O
Used as energy sources in cells
Also found in several cellular structures such as bacterial capsules
They are synthesized from water and carbon dioxide during photosynthesis
Carbohydrates
Monosaccharides (simple sugars) are the simplest carbohydrates
They are the building blocks for the larger carbohydrates (polysaccharides) like starch or cellulose.
Glucose, galactose and fructose are examples of isomers – they have the same chemical formula: C6H12O6 but the way the elements are put together and their properties are different
Simple Sugars C6H12O6
GLUCOSEIs the main source of energy for most living organisms
Half of the world’s carbon exists as glucose
Disaccharides
Double sugars – composed of two monosaccharides held together by covalent bonds
They are made from glucose molecules through dehydration synthesis – water is removed as the new bonds are formed
Examples are: maltose – found in barley and used to ferment beer lactose – found in milk and digested by bacteria to form
yogurt, sour cream and cheese sucrose – table sugar and is the starting point in wine
fermentation and may be a cause of tooth decay
Polysaccharides
Large compounds formed by joining together 100’s or 1000’s of glucose molecules Starch – used by bacteria as an energy source Cellulose – a component of the cell walls of plants and
molds and also used as an energy source by microorganisms
Interactive Notebook: Left Side
What are the 4 classes of organic compounds?
What 3 elements are carbohydrates made up of?
What carbohydrate is considered a universal source of energy?
B. LIPIDS
Dissolve in organic solvents, but not in water
Like carbohydrates, they are composed of C, H, and O, but with much less O
The best known lipids are fats
Fats are important long-term energy sources for living things they provide more calories than carbohydrates or proteins
Fats are also components of cell membranes
LIPIDS
Fats consist of a 3 carbon glycerol molecule and up to 3 long-chain fatty acids
2 major types of fatty acids: Saturated – contain the maximum number of H
atoms Unsaturated – contain less than the maximum
number of H atoms Unsaturated fatty acids are good for us – they
lower the levels of cholesterol in the blood
Lipid molecules are sparingly to insoluble in water. Lipids are hydrophobic because the molecules consist of long, 18-22 carbon, hydrocarbon backbones with only a small amount of oxygen containing groups. Lipids serve many functions in organisms. They are the major components of waxes, pigments, steroid hormones, and cell membranes. Fats, steriods, and phospholipids are very important to the functioning of membranes in cells and will be the focus of this tutorial. Fats (triacylglycerols)
LIPIDS
Other types of lipids: Waxes – long chains of fatty acids
Bee’s wax Plant leaves
Phospholipids – contain a phosphate group Cell membranes
Steroids – composed of several rings of carbon atoms with side chains Cholesterol Estrogen Testosterone
C. PROTEINS
Most abundant organic compounds of living thingsThey can be:
Structural Enzymes – regulate the rate of chemical reactions
They are composed of chains of amino acids
Each amino acid contains Carbon atom Amino group (NH2) Carboxyl group (COOH) Another side group
Proteins
Amino acids are joined together by peptide bonds
The sequence of amino acids is extremely important
One change can alter the protein (mutations)
Protein Structure: Primary – AA sequence (straight line) Secondary – AA chain twists into a corkscrew pattern ( 2-D) Tertiary – Protein folds back upon itself (3-D)
Proteins
Protein structure animation
D. NUCLEIC ACIDS
Some of the largest molecules found in organisms DNA – genetic material of the chromosomes that carries
the genetic code RNA – cell messenger that functions in protein construction
Composed of nucleotides Carbohydrate molecule (ribose or deoxyribose) Phosphate group Nitrogenous base
DNA – adenine, guanine, cytosine, thymine RNA – adenine, guanine, cytosine, uracil
Nucleic Acids
DNA is located in the chromosomes of the cell
It passes on the genetic information and directs protein synthesis
DNA molecule consists of 2 single strands of DNA in opposite directions arranged in a double helix ladder
Nucleic acids can not be altered without disrupting or killing the organism – this can help us control microorganisms
DNA Structure Animation
Acids and Bases
Degree of acidity or alkalinity is very important to living systems
You may hear the term pH a lot
What does this mean?
Acids and Bases
Water molecules can dissociate (separate) into:
Hydroxide Ions OH-
Hydronium Ions H3O+
Acids and Bases
- pH is a measure of a solution’s hydronium ion concentration
-pH is a scale of 0-14
- an acid = more hydronium ions (H3O+)
- a base = more hydroxide ions (OH-)
Acids and Bases
Acids : Have more hydronium ions Have a sour taste In concentrated forms can be very corrosive
Example:
Strong acid – HCl (hydrochloric acid) Weak acid – CH3COOH (vinegar)
Acids and Bases
Bases : Have more hydroxide ions Have a bitter taste Tend to feel slippery because they react with the oil
on our skin to form soap
Example:
Strong base – NaOH (sodium hydroxide) Weak base – NH4 (ammonia)
Acids and Bases
pH scale ranges from 0 – 14:
Solution with a pH of 0 is very acidic Solution with a pH of 14 is very basic Solution with a pH of 7 is neutral pH can be measured with pH paper or a pH meter