Bio 1151 Study Guide

CHAPTER 1
EVOLUTION- the process of change that has transformed life on Earth
BIOLOGY- scientific study of life
EMERGENT PROPERTIES- result from the arrangement and interaction of parts within a system
SYSTEMS BIOLOGY- constructs models for the dynamic behavior of whole biological systems
EUKARYOTIC CELL- has membrane enclosed organelles, the largest of which is usually the nucleus
PROKARYOTIC CELL- simpler and smaller, does not contain nucleus or other membrane enclosed organelles
DNA- (Deoxyribonucleic acid) substance of genes, genetic material, double helix form
GENES- units of inheritance that transmit information from parents to offspring
GENE EXPRESSION- the process of converting information from gene to cellular product
GENOME- is its entire set of genetic instructions
BIOINFORMATIC- use of computational tools to process a large volume of data, used in genomics
POSITIVE FEEDBACK- as more of the product accumulates; the process that creates it speeds up and more of the product is produced
NEGATIVE FEEDBACK- as more of a product accumulates, the process that creates it slows and less of the product is produced
CHAPTER 2
MATTER- anything that takes up space and has mass
ELEMENT- substance that cannot be broken down to other substances by chemical reactions
COMPOUND- substance consisting of two or more elements in a fixed ratio, has characteristics different from those of its elements
TRACE ELEMENT- those required by an organism in minute quantities
ATOM- smallest unit of matter that still retains the properties of an element
NEUTRONS- no electrical charge
ELECTRONS- negative charge
PROTONS- positive charge
ATOMIC NUCLEUS- formed by neutrons and protons
ATOMIC NUMBER- number of protons in its nucleus
MASS NUMBER- the sum of protons and neutrons in the nucleus
ATOMIC MASS- the atom’s total mass, can be approximated by the mass number
ISOTOPES- two atoms of an element that differ in the number of neutrons
RADIOACTIVE ISOTOPES- decay spontaneously, giving off particles and energy, can be used to date fossils, trace atoms through metabolic processes, diagnose medical disorders
ENERGY- the capacity to cause change
POTENTIAL ENERGY- the energy that matter has because if its location or structure
ELECTRON SHELL- an electron’s state of potential energy, consists of a specific number of orbitals
VALENCE ELECTRONS- electrons in the outermost shell (valence shell)
ORBITALS- the 3 dimensional space where an electron is found 90% of the time
CHEMICAL BOND- attractions between atoms
MOLECULE- consists of two or more atoms held together by covalent bonds
VALENCE- an atom’s bonding capacity
ELECTRONEGATIVITY- an atom’s attraction for the electrons in a covalent bond (the sharing of a pair of valence electrons by two atoms)
ION- a charged atom (or molecule)
CATION- a positively charged ion
ANION- a negatively charged ion
CHEMICAL REACTION- the making and breaking of chemical bonds
REACTANTS- starting molecules of a chemical reaction
PRODUCTS- final molecules of a chemical reaction
CHEMICAL EQUILBRUIM- reached when the forward and reverse reaction rates are equal
Types of Chemical Bonds A. COVALENT BOND- the sharing of a pair of valence electrons by two atoms, the shared electrons count as part of each atom’s valence shell, can form b/w atoms of the same elements B. SINGLE BOND- the sharing of one pair of valence electrons C. DOUBLE BOND- the sharing of two pairs of valence electrons D. NONPOLAR COVALENT BOND- the atoms share the electron equally E. POLAR COVALENT BOND- one atom is more electronegative, and the atoms do not share the electron equally F. IONIC BOND- an attraction between an anion and a cation, weak chemical bond G. HYDROGEN BOND- forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom, weak chemical bond H. VAN DER WAALS INTERACTION- attractions between molecules that are close together because electrons are distributed asymmetrically in molecules or atoms, they can result in “hot spots” of positive or negative charges
STRUCTURAL FORMULA- represents atoms and bonding ( H-H )
MOLECULAR FORMULA- further abbreviated ( H2 )
CHAPTER 3
ADHESION- an attraction between different substances, for example, between water and plant cell walls
COHESION- hydrogen bonds hold water molecules together, helps the transport of water against gravity in plants
SURFACE TENSION- a measure of how hard it is to break the surface of a liquid, related to cohesion
KINETIC ENERGY- energy of motion
HEAT- measure of the total amount of kinetic energy due to molecular motion
TEMPERATURE- measures the intensity of heat due to the average kinetic energy of molecules
CALORIES- (cal) the amount of heat required to raise the temperature of 1g of water by 1°C
SPECIFIC HEAT- the amount of heat that must be absorbed or lost for 1g of that substance to change its temperature by 1°C
HEAT OF VAPORIZATION- the heat a liquid must absorb for 1g to be converted to gas
EVAPORATIVE COOLING- process of surface cooling after a liquid evaporates, helps stabilize temperatures in organisms and bodies of water
SOLUTION- liquid that is a homogeneous mixture of substances
SOLUTE- the substance that is dissolved
AQUEOUS SOLUTION- one in which water is the solvent
HYDRATION SHELL- a sphere of water molecules containing a dissolved ionic compound
HYDROPHILIC- substance is one that has an affinity for water
HYDROPHOBIC- substance is one that does not have an affinity for water (oils)
MOLECULAR MASS- the sum of all masses of all atoms in a molecule
MOLARITY- (M) the number of moles of solute per liter of solution
ACIDS- any substance that increases the H+ concentration of a solution (Ex. pH>7 or vinegar)
BASES- any substance that reduces the H+ concentration of a solution (Ex. pH