(FINAL) Chemistry Notebook 2016-17

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Metals, with only a few electrons in the outer energy level, tend to lose electrons most readily. The
energy required to remove an electron from a neutral atom is called the IONIZATION POTENTIAL.
Energy + Metal Atom ---> Metal (+) ion + e-
Non-metals, which lack only one or two electrons in the outer energy level have little tendency to lose
electrons - the ionization potential would be very high. Instead non-metals have a tendency to gain
electrons. The ELECTRON AFFINITY is the energy given off by an atom when it gains electrons.
Non-metal Atom + e- --- Non-metal (-) ion + energy
The energy required to produce positive ions (ionization potential) is roughly balanced by the energy
given off to produce negative ions (electron affinity). The energy released by the net force of
attraction by the ions provides the overall stabilizing energy of the compound.
Notes Section:
Ionic Compounds Example:
Ions are completely different in physcial and chemical properties from their neutral atom of the element
Ions are positive(+) or negative(-) based on excess of protons(+) or electrons (-)
Formation of Positive Ions:
It's easier for rare gases to get rid of their ve- to go down to prior energy levels to be stable
ex: Na* -> (to form ion, lose electron) -> Na(+1)
Ion Charge:
Protons stay the same in the atom or ion, only electrons change
Summary Principle of Ionic Copmounds:
Ioninc compounds are formed by the complete transfer of electrons from a metal to non-metal, resulting
in octet ions.
Metals in groups 1,2, and 13 lose electrons to non-metals in groups 15-17 that need 1-3 electrons
Octet Rule:
Elemental atoms lose/gain/share atoms to achieve the electron structure of the prior noble gas
The Octet Rule assists in predicting and explaining various chemical formulas
Intro to Ionic Bonding:
Ionic compounds result from positive(+) and negative(-) ions
Ionic bonds result from attraction between opposite charges and repulsion from like charges.
In crystalline compounds, the net balance is called Lattice Energy, which is the energy released in the formation
of an ionic compound
Ionic Bond- the result of the transfer of 1 or more electrons from a metal to a non-metal
Ionization Potential- energy required to remove na electron from a neutral atom
Electron Affinity- energy given off by an atom when it gains electrons
Energy released by the net force of attraction by ions provides overall stabilizing energy of the compound
(Ionization potential is balaced by Electron Affinity)