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Electronegativity
how strongly the nucleus of an atom attracts the electrons of other atoms in a bond.
Hunds Rule
when an electron is added to a subshell, it will always occupy an empty orbital if one is available.
important information
The periodic table gives you basic but ________ about each element.
Subshells
________- a subdivision of electron shells separated by orbitals (s, p, d, & f)
Orbital
________- the position surrounding an atoms nucleus where electrons are most likely to be found at any given moment.
Energy Level
________- fixed distances from the nucleus of an atom where electrons may be found (1- 7)
Isotopes
Atoms of an element with different number of neutrons.
Molarity
(M)- moles of solute /liters of solution.
Aufbau Principle
when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy.
Electron Affinity
the energy change that occurs when an electron is added to an atom in its gaseous state.
Pauli Exclusion Principle
two electrons which share an orbital can not have the same spin.
Electrostatic Force
the attraction between opposite charges.
Symbol
The unique symbol that represents an element on the periodic table.
Ionization Energy
the energy required to remove an electron from an atom.
Mass Number
The sum of an atoms protons and neutrons.
Valence Electrons
the electrons in the outermost s and p subshells.
Avogadros Number
The number of atoms that are in a single mole of any given element (6.022 x 10^23 particles)
Atomic Radius
the approximate distance from the nucleus of an atom to its valence electrons.
Empirical Formula
The simplest ratio of one element to another in a compound.
Symbol
The unique symbol that represents an element on the periodic table
Atomic Number
The number of protons located within the nucleus of an element
Molar Mass
The average atomic mass of an atom and also the average mass per mol of the atom
Periods
the horizontal rows of the periodic table
Groups
the vertical columns of the periodic table
The two rows offset beneath the table are alternatively called the Lanthanides (4f) and the Actinides (5f)
Rare Earth Metals or Inner Transition Metals
Mass Number
The sum of an atoms protons and neutrons
Isotopes
Atoms of an element with different number of neutrons
Avogadros Number
The number of atoms that are in a single mole of any given element (6.022 x 10^23 particles)
Molarity(M)
moles of solute/liters of solution
Empirical Formula
The simplest ratio of one element to another in a compound
Molecular Formula
The actual formula for a substance
Electrostatic Force
the attraction between opposite charges
Coulombs Law
Force of attraction = q1q2/r^2
Energy Level
fixed distances from the nucleus of an atom where electrons may be found (1-7)
Subshells
a subdivision of electron shells separated by orbitals (s, p, d, & f)
Orbital
the position surrounding an atoms nucleus where electrons are most likely to be found at any given moment
Electron Configuration
the complete description of the energy level and subshell that each electron on an element inhabits
Aufbau Principle
when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy
Pauli Exclusion Principle
two electrons which share an orbital cannot have the same spin
Hunds Rule
when an electron is added to a subshell, it will always occupy an empty orbital if one is available
Valence Electrons
the electrons in the outermost s and p subshells
Atomic Radius
the approximate distance from the nucleus of an atom to its valence electrons
Ionization Energy
the energy required to remove an electron from an atom
Electronegativity
how strongly the nucleus of an atom attracts the electrons of other atoms in a bond
Electron Affinity
the energy change that occurs when an electron is added to an atom in its gaseous state
Effective Nuclear Charge
The net attractive force of the nucleus on the valence electrons (approximately equal to the number of protons - core electrons)
Note 
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