Ch. 2 Key Terms Flashcards
Nucleus
core of an atom containing protons and neutrons
Proton
positively charged particle that has mass of 1 amu and a charge of +1
Neutron
uncharged particle that has mass of 1 amu
Electron
negatively charged subatomic particle that resides outside the nucleus in the electron orbital, lacks functional mass and has a negative charge of -1
Atomic Number
number of protons in an atom
Mass Number
total number of protons and neutrons in an atom
Atomic Mass
calculated mean of the mass number for an element’s isotopes
Isotope
one or more forms of an element that have different numbers of neutrons
Radioisotopes
isotope that emits radiation composed of subatomic particles to form more stable elements
Periodic Table
organizational chart of elements indicating each element’s atomic number and mass, also provides key information about the elements properties
Chemical Reactivity
elements’ ability to combine and chemically bond with one another
Orbital
region surrounding the nucleus that contains electrons
Octet Rule
states that atoms are most stable when they hole eight electrons in their outermost shells
Valence Shell
outermost shell of an atom
Inert or Noble Gas
element with a filled valence shell that is unreactive with other atoms
Chemical Bond
interaction between two or more atoms that results in forming molecules
Chemical Reaction
process leading to rearranging atoms in molecules
Reactant
molecule that takes part in a chemical reaction
Product
molecule that is the result of a chemical reaction
Balanced Chemical Equation
when both sides of a chemical reaction have equal numbers of atoms
Compound
substance with at least two different elements
Irreversible Chemical Reaction
unidirectional chemical reaction
Reversible Chemical Reaction
bidirectional chemical reaction
Cation
positive ion formed when an atom loses electron
Anion
negative ion formed when an atom gains electron
Electron Transfer
movement of electrons from one element to another
Ionic Bond
chemical bond that forms between ions with opposite charges transferring electrons
Covalent Bond
type of strong chemical bond between same or different elements sharing electrons
Electrolyte
ion necessary for vital functions in the body
Polar Covalent Bond
type of covalent bond that forms when atoms share electrons unequally, resulting in oppositely charged regions of a molecule
Nonpolar Covalent Bond
type of covalent bond that forms when atoms share electrons equally
Electronegativity
the ability of some elements to attract electrons and acquire partial negative charges
Hydrogen Bond
weak bond between slightly charged hydrogen atoms and slightly negatively charged atoms in other molecules
Van der waals interactions
very weak interaction between molecules due to temporary charged attracting atoms that are very close together
Hydrophobic
quality of ions or polar molecules interacting well with other polar molecules
Hydrophilic
quality of uncharged nonpolar molecules that do not interact well with polar polecules
Specific Heat Capacity
the amount of heat one gram of a substance must absorb or lose to change its temperature by one degree Celsius
Calorie
amount of heat required to change the temperature of one gram of water by one degree celsius
Heat of Vaporization
high amount of energy required for liquid water to turn into water vapor
Evaporation
change from liquid to gaseous state at a body of waters surface, plant leaves, or an organisms skin
Solvent
substance capable of dissolving another substance
Sphere of Hydration
when a polar molecule surrounds charged or polar molecule that keeps them dissolved in a solution
Dissociation
process of atoms breaking off of molecules and forming ions
Cohesion
the tendency for water to stick to itself
Adhesion
the tendency for water to stick to other things
Surface Tension
tension at the surface of water that prevents molecules from separating created by cohesive forces in water
Capillary Action
the movement of water through a narrow space due to adhesion
Acid
molecule that donates hydrogen ions and increases the concentration of hydrogen ions in a solution
Base
molecule that donates hydroxide ions or binds excess hydrogen ions to decrease their concentration in a solution
pH Scale
the measurement of how acidic or basic water is ranging from 0-14
Buffer
a substance that resists change in pH by absorbing excess hydrogen ions or hydroxide ions
Organic Molecule
any molecule containing carbon (except carbon dioxide)
Hydrocarbon
organic molecule consisting entirely of carbon and hydrogen
Aliphatic Hydrocarbon
hydrocarbon consisting of a linear chain of carbon atoms
Aromatic Hydrocarbon
hydrocarbon consisting of closed rings of carbon atoms with alternating single and double bonds
Isomer
molecule that share a chemical formula but differ in the placement of their atoms and chemical bonds
Structural Isomer
isomers that share a chemical formula but differ in the placement of their chemical bonds
Geometric Isomers
isomers with similar bonding patterns that differ in the placement of atoms alongside a double covalent bond
Cis Configuration
when the carbons are bound on the same side of a double bond in a geometric isomer (resulting in a bend of the carbon backbone)
Trans Configuration
when the carbons are bound on the opposite side of a double bond in a geometric isomer (resulting in a more linear carbon backbone)
Enantiomers
molecules that share overall structure and bonding patterns but differ in how the atoms are placed three-dimensionally so that they are mirror images of each other
Functional Groups
group of atoms that provides a specific function to a carbon skeleton
Substituted Hydrocarbons
molecules with other elements in their carbon backbone
Seven Functional Groups
hydroxyl, methyl, carbonyl, carboxyl, amino, phosphate, sulfhydryl
