Studied by 20 people
Group
Collums going left to right
Period
Rows going top to bottom
Periodic Trends
Atomic radius
The radius of an atom; increases going top to bottom on the Periodic table
Ionization energy
measure of the difficulty in removing an electron from an atom or ion
Neutron
Neutral; found in the nucleus of atoms
Proton
Positive; Found in the nucleus of atoms
Electron
Negative; Found orbiting the nucleus of atoms
Valence Electron
Electrons on the outer most ring of atoms
Alpha Decay
nuclear decay process where an unstable nucleus changes to another element by shooting out a particle composed of two protons and two neutrons (similar to that of a helium particle)
Beta Decay
Decay in which a Proton is converted into a neutron, releasing an electron and changing and element
Gamma Decay
emission of electromagnetic radiation of an extremely high frequency i.e. very high energy, giving out excess energy in order to stabilize the unstable nucleus
Electromagnetic Spectrum
the range of frequencies of electromagnetic radiation and their respective wavelengths and photon energies
Wavelength
distance between waves of energy
Frequency
number of waves which occur over a period of time
Electron configuration
distribution of electrons of an atom
Orbital
location of an electron around an atom
Molecular Geometry
three-dimensional arrangement of the atoms that constitute a molecule
Isotope
An atom which has equal protons but differing neutrons
Reactivity
The ability of an element to interact with other elements
Dipole/Polar
Points at which a molecule has differing electronegativity
Non-polar
Compound which does not differ in electronegativity
Polarity/Partial Charge
separation of electric charge in a molecule
Ionic Bonds
chemical bond formed when one atom gives up one or more electrons to another atom
Electronegativity
the tendency for an atom of a given chemical element to attract shared electrons when forming a chemical bond
Transfer electrons
Electrons which relocate to another atom
Polyatomic Ion
ion which despite having multiple atoms, behaves as a single unit.
Cation
positively charged ion
Anion
negatively charged ion
Covalent Bond
sharing of electron pairs between atoms
Lewis Dot Structures
Visual form of drawing chemicals using letters and dots
Noble Gas
Elements on the right side of the Periodic table; unreactive and 8 Valence electrons
Structural Formula
Drawn images to depict a chemical formula visually
Octet Rule
the rule which states Bonded atoms tend to have 8 Valence electrons, that of a noble gas.
Lone Pair Electrons
pair of Valence electrons which aren't used to form a bond between atoms
Bonded Pair Electrons
2 electrons which reside in the same orbital
Unpaired Electrons
electrons which aren't paired, orbit alone
Single Bond
chemical bond involving 2 Valence electrons
Double Bond
chemical bind involving 4 Valence electrons
Triple Bond
chemical bond involving 6 Valence electrons rather than 2 or 4, having three bonds
HONC 1234
rule which states that Hydrogen has 1 bond, oxygen 2, nitrogen 3, and carbon 4.
Combustion
reaction resulting in Fuel + O2 → CO2 + H2O.
Combination
process in which chemicals combine to form a single product
Decomposition
process in which chemicals break down into smaller components
Double displacement
chemical process involving the exchange of bonds between two reacting chemical species
Single displacement
chemical reaction in which one element is replaced by another in a compound
Chemical equation
equation involving chemicals
Reactant
substance that takes part in and undergoes change during a reaction.
Product
The stuff created in a reaction
Mole
Unit of measurement used to describe having 6.02x10^23 of a substance
Avogadro's Number
6.02x10^23 (mole)
Molar Mass
the mass in grams of one mole of a substance
Dimensional Analysis
a method used to convert one unit to a different unit
