Chapter Two: The Chemistry Of Life Flashcards
Chemistry
Study of all molecules
Biochemistry
Study of all molecules that compose living organisms
Element
Simplest form of matter to have a unique chemical property
6 main elements found in the body
Hydrogen Oxygen Phosphorus Carbon Calcium Nitrogen
Mineral
Inorganic elements that are extracted from soil by plants and passes up the food chain to humans
- 4% of body weight
- significant contribution to body structure
Electrolytes
Mineral salts needed for nerve and muscle function
Isotope
Varieties of an element that differ from one another only in the number of neutrons
Radioisotopes
Unstable isotopes that decay and give off radiation
Every element has at least one
Radioactivity
Process of decay
Physical Half-Life…or radioisotopes
Time needed for 50% to decay into a stable state
Biological Half-Life…of a radioisotope
Time required for 50% to disappear from the body
Ion
Charged particles with unequal numbers of protons and electrons
Ionization
The transfer of electrons from one atom to another
Cation
Particles that lose electrons
POSITIVE CHARGE
Anion
Particles that gain an electron
NEGATIVE CHARGE
3 Important Characteristics of Electrolytes
- Chemical reactivity
- Osmotic effects(influence water movement)
- Electrical effects on nerve and muscular tissue
Free Radical
Short lived particles
odd number of electrons
Produced by normal metabolic reactions of the body, radiation, and by chemicals
Trigger reactions that destroy molecules
Cause tissue damage, aging, cancer, and heart problems
Antioxidants
Chemical that neutralizes free radicals
Created by the body and obtained in diet
Molecules
Chemical particles composed of two or more atoms united by a chemical bond
Compound
Molecules composed of two or more elements
Isomers
Identical molecular formula
different arrangement of atoms
What are the four types of chemical bonds
Covalent
Hydrogen
Ionic
Van def Walls force
Ionic bond
Attraction of a cation to an anion
Weak
Disassociates in water
Hydrogen Bond
Weak attraction of slightly positive hydrogen in one molecule to an oxygen or nitrogen in another
Van der Walls Forces
Weak, brief attraction between neutral atoms
Weakest of all bonds
Single Covalent Bond
Sharing 1 electron
Double Covalent Bond
Share 2 electrons
Nonpolar Covalent Bond
Electrons are equally attracted to both nuclei
Strongest bond
Polar Covalent Bond
Electrons more attracted to one nucleus over the other
Mixture
substances are physically blended
not chemically combined
(each substance keeps its own chemical properties
5 Properties of Water
Thermal stability Adhesion Cohesion Chemical reactivity Solvency
3 Important Structural Aspects of Water
- Atoms are joined by polar Covalent bonds
- Molecule is V shaped with a 105 angle
- Individual water molecules joined by hydrogen but bonds
Solvency
Ability to dissolve other chemicals
Water=”UNIVERSAL SOLVENT”
Hydrophilic
Dissolve in water
Hydrophobic
Do not dissolve in water
Adhesion
Tendency of one substance to cling to another
Cohesion
Tendency of like molecules to cling to each other
Solute
Substance being dissolved
Solvent
Substance doing the dissolving
3 types of mixtures
Solutions
Colloids
Suspensions
Solutions
Properties?
Consists of solute and solvent
Properties
- solute particles are so small(less that 1nm) that the solute and solvent cannot be visually distinguished from each other
- transparent- do NOT scatter light
- will pass through most membrane
- particles will stay mixed
Colloids
Properties?
In body generally a mix of protein and water
Properties
- solute particles range from 1 to 100nm
- scatter light-cloudy
- particles can NOT pass through most selectively permeable membranes
- particles will stay mixed
Suspensions
Properties?
Blood is most common suspension in the body
Properties
- solute particles are above 100nm
- generally cloudy or opaque
- particles can NOT pass through and selectively permeable membrane
- particles will separate
Acid
And proton donor
release H+
Base
Any proton acceptor
Accepts H+
pH
Negative logarithm of H+ molarity
0-14
Lower the pH the more hydrogen ions the solution has= more acidic
Kinetic Energy
Example?
Types?
Energy in motion, energy doing work
Example: Water being released from a dam
Types:
Heat: energy of molecular motion
Electromagnetic energy: energy of moving packets of radiation called photons
Potential Energy
Example?
Types?
Energy contained in an object because of its position or internal state but that is not doing work at the time
Example: water behind a dam
Types:
Chemical Energy: stored in molecular bonds
Free Energy: available in a system to do useful work
Chemical Reaction
Process in which a covalent or ionic bond is formed or broken
3 Types of Chemical Reactions
DES
Decomposition
Synthesis
Exchange Reactions
Decomposition Reaction
Large molecule breaks down into two or more smaller ones
AB—> A+B
Synthesis Reaction
Two or more small molecules combine to form a larger one
A+B—>AB
Exchange Reaction
Two molecules exchange atoms or group of atoms
AB+CD—>ABCD—>AC+BD
3 Things that Effect Reaction Rates
- Reactants are more concentrated
- The temperature rises
- Catalysts are present
Catalysts
temporarily binds to reactants, hold them in orientations that facilitate the reaction
Speeds up reactions without changing itself
Catabolism
Energy releasing decomposition reactions
- breaks covalent bonds
- produces smaller molecules
Anabolism
Energy storing synthesis reactions
- production of proteins and fats
- driven by energy from catabolism
Oxidation
&
Oxidizing Agent
Any chemical reaction in which a molecule gives up electrons and releases energy
Agent: the electron accepting molecule
* oxygen is a common electron acceptor
Reduction
&
Reducing Agent
Any chemical reaction in which a molecule gains electrons and energy
Agent: electrons donating molecule
4 Carbon Compounds found in Body
- Carbohydrates
- Lipids
- Proteins
- Nucleic Acid
Macromolecules
Very large organic molecule
Polymer
Macromolecule made of a repetitive series of identical or similar subunit called monomers
Hydrolysis
Digestion
Breaks covalent bond that links monomers
Splitting polymer by adding water
Dehydration Synthesis
How living cells form polymers
Takes water away to link monomers
3 Disaccharides
Sucrose
Lactose
Maltose
3 Monosaccharides
Glucose
Fructose
Galactose
3 polysaccharides
Define each
Glycogen: energy storage in animals
- only polysaccharide found in human tissue
- made by liver after a meal
Starch: energy storage in plants
*significant digestible in human diet
Cellulose: structural polysaccharide that gives strength to the cell wall of plants
5 Primary Lipids
STEP F
Steroids Triglycerides Eicosanoids Phospholipids Fatty acids
Peptide Bond
Joins the amino group of one amino acid to the carboxyl group of the next
Denaturation
Extreme conformational change that destroys function
7 Functions of Protein
CCCSMRM
Communication Cell adhesion Catalyst Structure Movement Recognition and Protection Membrane Transport
Enzyme
Proteins that function as biological catalysts
- enable biochemical reactions to occur rapidly at normal body temp
- can be altered by temp, pH
Substrate
Substance an enzyme acts upon
Cofactor
A non protein partner needed for the reaction
- essential to function
- bind to enzyme to take the proper “lock” formation
Coenzyme
A cofactor that is organic
