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Observation
Knowledge about the world received through the senses of instrumentation
Fact
Something that is known to be consistent with reality
Law
A brief statement that summarizes past observations and predicts future ones
Hypothesis
A tentative interpretation or explanation that can be tested through observation
Theory
An explanation of some aspect of the natural world that has been substantiated through repeated experiments or facts gathered over time
Accurate
Value that is close to the actual “correct” value being measured
Precise
Measurement that is repeatable
Matter
Anything that has mass and takes up space
Atom
The smallest possible component of matter capable of stable existence
Element
A pure substance composed of all one type of atom
Molecule
A chemical combination of two or more elements in fixed proportions
Compound
A pure substance composed of more than one type of atom, but cannot physically be separated into different substances
Mixture
Substances which can be physically separated into different substances
Homogenous
A mixture with uniform appearance and properties throughout
Heterogenous
A mixture with physically distinguishable components
Solution
A homogenous mixture of two or more compounds
Homonuclear
Molecule composed of atoms of the same type
Heteronuclear
Molecule composed of multiple types of atoms
Monatomic
Molecule composed of one atom
Diatomic
Molecule composed of two atoms
Triatomic
Molecule composed of three atoms
Polyatomic
Molecule composed of more than three atoms
Fusion
Physical change from solid to liquid
Freezing
Physical change from liquid to solid
Vaporization
Physical change from liquid to gas
Condensation
Physical change from gas to liquid
Sublimation
Physical change from solid to gas
Deposition
Physical change from gas to solid
Law of Conservation of Mass
In a chemical reaction, matter is neither created nor destroyed
Law of Definite Proportions
All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements
Law of Multiple Proportions
When two elements (A and B) form two different compounds, the masses of B that combine with 1 gram of A can be expressed as a ratio of small whole numbers
Cathode Ray Experiment
Determined the charge:mass ratio of electrons
Oil Drop Experiment
Determined the charge and mass of electrons
Gold Foil Experiment
Determined the location of protons in an atom
Bombardment Experiment
Determined the presence of neutrons in an atom
Proton
Subatomic particle that gives an atom its identity
Neutron
Subatomic particle that has no charge
Electron
Subatomic particle that determines the reactivity of an element
Ionic Charge
The number of protons minus the number of electrons
Isotopes
Atoms with the same number of protons but different numbers of neutrons
Mass Number
The number of protons and neutrons combined
Atomic Number
The number of protons
Periodic Law
When the elements are arranged in order of increasing atomic number, certain sets of properties recur periodically
Periods
Rows on the periodic table
Groups
Columns on the periodic table
Alkali Metal
Elements belonging to Group 1 on the periodic table
Alkaline Earth Metal
Elements belonging to group 2 on the periodic table
Halogen
Elements belonging to group 7 on the periodic table
Noble (inert) Gas
Elements belonging to group 8 on the periodic table
Electromagnetic Radiation
Oscillating electric and magnetic fields
Wavelength
Distance from one crest to the next
Frequency
Number of cycles that pass a point in a given unit of time
Period
Time it takes for a complete wave unit to pass through a point
Amplitude
Height (intensity) of a wave
Interference
Addition of wave amplitudes when the waves overlap
Diffraction
Waves bend when they encounter an obstacle that is about the same size as the wavelength
Photoelectric effect
Electrons are sometimes ejected upon irradiation of a metal surface
Work Function
The energy it takes for an electron to escape its binding energy to the atom
de Broglie Wavelength
The wavelength any matter has by virtue of its momentum
Heisenberg’s Uncertainty Principle
The position and momentum of an object cannot be known simultaneously with infinite precision
Schroödinger Equation
Describes the state (position and energy) of an atom’s electrons
Node
Where the value of a wavefunction is 0
Pauli Exclusion Principle
No two electrons in an atom may have the same set of four quantum numbers
Coulomb’s Law
Potential energy associated with the attraction and repulsion of charged particles
Shielding
Valence electrons “feel” less pull from the nucleus than core electrons do
Penetration
The possibility of high-energy electrons approaching areas closer to the nucleas
Degenerate States
States that have the same energy as each other
Core electrons
Electrons in inner “n” levels (n < n_max)
Valence electrons
Electrons in the outermost (highest) “n” level
Ground State
The configuration of electrons in which all electrons are in as low an energy orbital as possible
Excited state
Any configuration in which at least one electron is in a higher-than-baseline energy orbital
Aufbau Principle
Fill electrons from low energy to high energy
Hund’s Rule
Maximize spin alignment in degenerate orbitals and don’t pair spins unless necessary
Isoelectronic
Species containing the same electron configuration
Effective nuclear charge
The amount of protons an orbiting electron “feels”
Paramagnetic
Electron configurations with unpaired electrons
Diamagnetic
Electron configurations with no unpaired electrons
Ionization Energy
Amount of energy needed to remove an electron from an atom/ion
Electron Affinity
Amount of energy gained or released whne an atom or ion gains an electron
Pauling Electronegativity
The power of an atom in a molecule to attract electrons to itself
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