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9 p+ to complete 9 p + Protons are identical in 10 n octet add 1 10 n the<br />
atom and ion.<br />
9 e- electron 10 e- Negative charge is<br />
10 charge - 1 charge<br />
caused by excess<br />
electrons *<br />
The "ide" ending in the name signifies a simple negative ion.<br />
Summary Principle of Ionic Compounds<br />
An ionic compound is formed by the complete transfer of electrons from a metal to a nonmetal and<br />
the resulting ions have achieved an octet. The protons do not change. Metal atoms in Groups 1-3<br />
lose electrons to non-metal atoms with 5-7 electrons missing in the outer level. Non-metals gain 1-4<br />
electrons to complete an octet.<br />
Octet Rule<br />
Elemental atoms generally lose, gain, or share electrons with other atoms in order to achieve the<br />
same electron structure as the nearest rare gas with eight electrons in the outer level.<br />
The proper application of the Octet Rule provides valuable assistance in predicting and explaining<br />
various aspects of chemical formulas.<br />
Introduction to Ionic Bonding<br />
Ionic bonding is best treated using a simple electrostatic model. The electrostatic model is simply an<br />
application of the charge principles that opposite<br />
charges attract and similar charges repel. An ionic<br />
compound results from the interaction of a positive<br />
and negative ion, such as sodium and chloride in<br />
common salt.<br />
Energy + Metal Atom ---> Metal (+) ion + e-<br />
The IONIC BOND results as a balance between<br />
the force of attraction between opposite plus and<br />
minus charges of the ions and the force of<br />
repulsion between similar negative charges in the<br />
electron clouds. In crystalline compounds this net<br />
balance of forces is called the LATTICE ENERGY.<br />
Lattice energy is the energy released in the<br />
formation of an ionic compound.<br />
DEFINITION: The formation of an IONIC BOND is<br />
the result of the transfer of one or more electrons<br />
from a metal onto a nonmetal.<br />
Metals, with only a few electrons in the outer<br />
energy level, tend to lose electrons most readily.<br />
The energy required to remove an electron from a<br />
neutral atom is called the IONIZATION<br />
POTENTIAL.<br />
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