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52 Cards in this Set

  • Front
  • Back
Atom (def.)
Smallest unit of matter that enter into chemical reactions.
Structure of an Atom
Nucleus : protons, neutrons
Electrons
Atomic weight of protons and neutrons
1
Most abundant chemical elements in living organisms
Hydrogen (H)
Carbon (C)
Nitrogen (N)
Oxygen (O)
Isotopes (def.)
Atoms with the same number of protons, but a different number of neutrons.
Atomic Number (def.)
Number of protons in nucleus.
Why do atoms form bonds with each other?
For electron stability. Atoms are happiest when outer shells have 2 or 8 electrons. If not, they try to share to achieve this.
Atomic Weight (def.)
Total number of protons and neutrons in the nucleus.
Compound (def.)
A molecule that contains at least two different kinds of atoms, e.g. water, H2O (hydrogen and oxygen).
Ionic Bond (def.)
Attraction between ions of opposite charge that holds them together to form a stable molecule.
Ion (def.)
A negatively or positively charged atom or group of atoms. The charge results from electrons being donated or accepted.
Covalent Bond (def.)
Chemical bond formed by two atoms sharing one or more pairs of electrons. Strong bond.
Examples: H2 (hydrogen), CH4 (methane)
Hydrogen Bond (def.)
A bond in which a hydrogen atom that is covalently bonded to one oxygen or nitrogen atom (polar molecule) is attracted to another oxygen or nitrogen atom. Weak bond. Does not form molecules, but serves as bridge.
Exergonic vs. Endergonic Reactions (def.)
Exergonic reaction releases more energy than it absorbs.
Endergonic reaction absorbs more energy than it releases.
Synthesis vs. Decomposition Reactions (def.)
Synthesis reactions are building reactions (anabolism).
Decomposition reactions are breaking down reactions (catabolism).
Anabolism vs. Catabolism (def.)
Anabolism is a synthesis reaction in a living organism.
Catabolism is a decomposition reaction in a living organism.
What property of water is most relevant to dissolving table salt?
Water is a solvent due to its polarity.
pH (def.)
"pH" stands for "potential of hydrogen".
Base vs. Acid (pH)
Base: higher pH
Acid: lower pH
Neutral: [H+] = [OH-]
Water : unique properties
Liquid vs. ice
Cohesive and adhesive (surface tension)
Solvent
Heat sink (resists temperature change)
Calorie (def.)
Energy required to raise 1 ml (1 g) of water by 1 deg C.
ph Scale (def.)
Negative logarithm or the hydrogen ion concentration. pH = -log [H+].
Increase/decrease by ph 1 equals ten-fold increase/decrease in base/acidity.
What class of organic molecule tends to be most non-polar?
Lipids
Which class or organic molecule contains RNA?
Nucleic acids
Organic Molecule Components
Carbon
Hydrogen
Functional Group (def.)
Specific groups of atoms that are most commonly involved in chemical reactions and are responsible for most of the characteristic chemical properties and many of the physical properties of a particular organic compound.
Functional Group (ex.)
Alcohol (O-H)
Ketone (C=O)
Amino (NH2)
Ester (O=C-O)
Ether
Phosphate
Carboxyl
Macromolecule (def.)
Very large molecule made up of small organic molecules.
Polymer (def.)
Large molecule formed by covalent bonding of many repeating small molecules called monomers.
Dehydration Synthesis (def.)
Reaction that involves the elimination of a hydrogen atom from one monomer and a hydroxyl group from the other. The hydrogen atom and hydroxyl group combine to form water.
R -- OH + H --> R -- R' + H2O
What lipid makes up membranes?
Phospholipids
Carbohydrate (def.)
Organic compound that is made up of carbon, hydrogen, and oxygen atoms.
Chemical Formula of Carbohydrate
(CH2O)n
Monosaccharide (def.)
Simple sugar molecule containing from 3 to 7 carbon atoms.
Disaccharide (def.)
Bond of two monosaccharides in a dehydration synthesis reaction.
Hydrolysis (def.)
Reverse of dehydration synthesis.
Addition of water to molecule resulting in breakdown into smaller, simpler molecules.
Examples of Carbohydrates
Starch (storage polysaccharide in plants)
Glycogen (storage in animals)
Cellulose (cell wall structure)
Lipid (def.)
Fat.
Nonpolar, thus insoluble in water.
Function in energy storage and provide the structure of membranes and some cell walls.
Triglyceride (def.)
Simple lipid.
Contains an alcohol (glycerol) and 3 fatty acids. Long hydrocarbon chains.
Saturated vs. Unsaturated Fats
Unsaturated has double bonds and is not saturated with hydrogen.
Saturated fats become solid more easily.
Phospholipid (def.)
Complex lipid made up of glyerol, two fatty acids, and, in place of a third fatty acid, a phosphate group bonded to one of several organic groups.
Polar head; nonpolar tail.
What lipid makes up membranes?
Phospholipids
Proteins (def.)
Organic molecules that contain carbon, hydrogen, oxygen, and nitrogen.
Examples of proteins in cells
Enzymes
Transporter proteins
Peptide Bond (def.)
Bonds between amino acids.
Levels of Protein Structure
Primary (basic squence)
Secondary (3D motif, e.g. helix, sheet)
Tertiary (whole protein structure)
Quaternary (more than 1 peptide)
Amino Acid (def.)
Building block of proteins.
Contain at least on carboxyl (--COOH) group and one amino (--NH2) group attached to the same carbon atom (alpha-carbon).
20 different amino acids in proteins.
Conjugated Proteins (def. / ex.)
Combinations of amino acids with other organic or inorganic components. Named by their non-amino acid component, e.g. glycoprotein (sugar), nucleoprotein (nucleic acid)
Nucleic Acid : building block
Nucleotide (phosphate-sugar base)
DNA
Deoxyribonucleic acid.
String of deoxyribonucleotides.
Four bases: ATCG.
Genetic material.
RNA
Ribonucleic acid.
Less stable than DNA.
Bases: AUGC.
Genetic messenger.
ATP (def.)
Adenosine triphosphate.
High-energy phosphate bond.
Principal energy-carrying molecule of all cells; indispensible to the life of the cell.