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Regents Chemistry Vocabulary
Essential vocabulary needed to pass the NYS Chemistry Regents (modified from M. Rosengarten)
68
Chemistry
11th Grade
05/20/2012

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Term
Activation Energy
Definition
Energy required to start a chemical reaction. Can be determined by looking at a potential energy diagram (difference between the reactants and the highest point on the diagram).
Term
Allotrope.
Definition
Different molecular forms of the same element with different properties (due to different structures); examples: graphite and diamond (both carbon allotropes); oxygen and ozone (both oxygen allotropes)
Term
Alternate A/B Theory (Bronsted-Lowry Theory)
Definition
Acids donate H+ (protons), bases accept H+ (protons). (BAAD)
Term
Arrhenius Acid
Definition
a substance that dissolves in water to yield H+ (H3O+ or hydronium) ions.
Term
Arrhenius Base:
Definition
a substance that dissolves in water to yield OH- (hydroxide) ions.
Term
Artificial Transmutation
Definition
Nuclear reaction in which a nuclide is shot with another particle to produce a different element
Term
Avogadro’s Hypothesis
Definition
Equal Pressure, Volume & Temperature of different gases indicates that there are equal number of molecules (assuming ideal gas behavior).
Term
Cathode
Definition
The electrode where reduction occurs; due to the reduction of the cations in solution at the cathode, its mass will always increase. (AN OX, FAT RED CAT)
Term
Chemical Property
Definition
A property that changes the identity of the substance (i.e. flammability, rusting)
Term
Combustion
Definition
An organic compound, typically a hydrocarbon, reacts with O2 to form CO2 + H2O; always exothermic
Term
Compound
Definition
Substance that can be chemically decomposed into two or more elements; its name will not appear on Reference Table S.
Term
Conductivity
Definition
Ability to transfer electrical charge from one place to another; due to substance having freely moving charged particles (ions in aqueous solution; electrons in metallic substance)
Term
Covalent Bond
Definition
Bond formed when two nonmetal atoms share valence e-.
Term
Decomposition
Definition
Breaking a compound down into two or more substances
Term
Diatomic Molecule
Definition
Molecule made of two atoms of the same element (HOFBrINCl)
Term
Distillation
Definition
Separation of two substances based on differences in boiling point.
Term
Electrolyte
Definition
A substance that ionizes in water and conducts electricity.
Term
Electronegativity
Definition
An atom’s attraction to electrons in a chemical bond.
Term
Element
Definition
Substance that cannot be decomposed by chemical change.
Term
Empirical Formula
Definition
Simplest whole- number mole ratio of elements in compound
Term
Entropy
Definition
The state of randomness or disorder in the particles of a system.
Term
Equilibrium
Definition
A condition where the rate of forward and reverse reactions are equal; this is observed when the concentrations or pressures of the reactants and products no longer appear to be changing.
Term
Excited State
Definition
Where electrons are in higher PELs than they would normally be; the electrons have to absorb energy in order to go to the excited state.
Term
Exothermic
Definition
A change that results in an overall decrease in potential energy (by transferring energy out of the system – heat flows out). Endothermic reactions result in an overall increase in potential energy (by transferring energy into the system – heat flows in).
Term
Fermentation
Definition
Yeast enzyme zymase converts sugar into ethanol and carbon dioxide.
Term
Gram-Formula Mass
Definition
The sum of the contribution of atomic masses from each element found in a substance.
Term
Half-Life
Definition
The period of time for a radioactive substance to lose half of its radioactivity (i.e. only half of the original radioisotope is present after each successive half-life).
Term
Heat of Fusion
Definition
The amount of energy needed to melt 1 g of substance at its melting point.
Term
Heat of Reaction
Definition
The total amount of chemical potential energy lost or gained during a change (DH); can be determined by using Reference Table I for many reactions.
Term
Hydrogen Bonds
Definition
The strongest type of IMF; found between the hydrogen of one molecule and the F, O or N found on an adjacent molecule.
Term
Ideal Gas
Definition
One where the molecules are as small and far apart as possible so as to minimize the possible formation of IMF between adjacent molecules. Ideal gas conditions are best met when the gas sample is kept under low pressures and high temperatures (PLIGHT).
Term
Intermolecular Forces of Attraction
Definition
Attractions between adjacent molecules (i.e. the attraction between two adjacent water molecules in a sample of water). A bond holds together atoms inside ONE molecule.
Term
Ionic Bond
Definition
A type of chemical bond formed when a metal atom transfers a valence electron to a nonmetal atom; the metal ion assumes a positive charge and the nonmetal assumes a negative charge.
Term
Ionization Energy
Definition
The energy required to remove the most loosely bound valence electron in an atom.
Term
Isomer
Definition
A compound that contains the same molecular formula but a different structural formula
Term
Isotopes
Definition
Atoms of the same element (same number of protons) with different numbers of neutrons; the result would be the two isotopes having different mass numbers.
Term
Law of Conservation Of Mass
Definition
Mass cannot be created or destroyed during any reaction.
Term
Mass Number
Definition
The total number of protons plus neutrons in the nucleus; the electrons are considered to have negligible mass and therefore do not contribute to the overall mass of the atom.
Term
Molarity
Definition
A measure of concentration of a solution; moles of solute dissolved per liter of solution (Reference Table T).
Term
Molecular Formula
Definition
Actual number of atoms of each element in molecule
Term
Molecule-Ion Attraction
Definition
Attraction for polar solvent molecules to ions in solution; causes some ionic compounds to dissolve in water (Reference Table F)
Term
Monatomic
Definition
Atoms of noble gas that have a stable octet without having to bond.
Term
Natural Decay
Definition
An unstable nucleus emits radiation to become more stable; this is a spontaneous process determined by the half-life of the element and the neutron to proton ratio found in the nucleus.
Term
Network Solids
Definition
Crystal lattice of covalently bonded nonmetal or metalloid atoms (i.e. C or Si)
Term
Neutralization
Definition
An acid reacts with a base to form a salt and water.
Term
Nuclear Charge
Definition
The positive charge of the nucleus due to the number of protons.
Term
Nuclear Fission
Definition
A large nucleus is split into two smaller nuclei (i.e. uranium bombarded with neutron)
Term
Nuclear Fusion
Definition
Two small nuclei combine to make one larger nucleus (i.e. formation of helium from two hydrogen atoms)
Term
Orbital
Definition
Location around a nucleus where an electron is most likely to be found; tied to the wave-mechanical model (modern model) of the atom.
Term
Oxidation Number
Definition
Charge of an atom or ion
Term
Oxidation
Definition
The loss of electrons (OIL RIG)
Term
Percent Composition
Definition
Ratio of part to whole multiplied by 100 to make the fraction into a percentage (Reference Table T).
Term
Petroleum (crude oil)
Definition
A mixture of hydrocarbons refined through fractional distillation into its component fuels.
Term
pH
Definition
Measure of the relative acidity of a solution; –log [H3O+] ions in solution, each pH change of 1 is a 10-fold change in strength
Term
Polar Covalent Bond
Definition
Sharing electrons unevenly due to a difference in electronegativity values between the two nonmetal elements comprising the chemical bond.
Term
Polar Molecule:
Definition
Molecule which contains an asymmetric distribution of charge (SNAP)
Term
Potential Energy
Definition
Energy stored in the chemical bonds of substances.
Term
Redox Reaction
Definition
A reaction where one or more elements changes charge; the simultaneous loss (oxidation) and gain (reduction) of electrons in a chemical reaction.
Term
Salt Bridge
Definition
Completes the circuit and allows for migration of ions in a voltaic (galvanic) cell.
Term
Saponification
Definition
Fats react with bases to form soap and glycerol.
Term
Saturated
Definition
A solution with the maximum quantity of solute dissolved at a given temperature. A saturated solution is an example of an equilibrium system in which the rate of dissolving equals the rate of crystallization.
Term
Solution
Definition
Homogeneous mixture made of solute dissolved into a solvent.
Term
Spontaneous
Definition
A reaction which, once started, goes all the way to completion without outside interference.
Term
Sublimation
Definition
Phase change from a solid to a gas.
Term
Temperature
Definition
The average kinetic energy of the molecules in a system.
Term
Transition Metal
Definition
Elements in groups 3-12 that form colored solutions.
Term
Valence Electrons
Definition
Electrons in the outermost principal energy level.
Term
Voltaic Cell
Definition
Uses a spontaneous redox reaction to convert stored chemical potential energy into electrical energy (makes an electrical current).
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