Ionic Bonding
Valance Electrons; Electrons in the atom’s outermost orbitals, determine the chemical properties of an element.
In Ionic Bonding, valence electrons are lost from one atom and gained by another. This results in a more stable noble gas electron configuration.
Electron Dot Structures:
Represent the atomic nucleus and inner-level electrons, surrounded by dots representing all of the atom’s valence electrons.
The Dot structure shows how the electrons are being transferred to form the ions in the compound.
Chemical Bond:
The force holding two atoms together.
Can be formed by the attraction between the positive nucleus of one atom and the negative electrons of another. In other words, this is the attraction between positive ions and negative ions.
Cation Formation:
A positively charged ion.
These form when an atom loses one or more valence electrons in order to attain a noble gas configuration.
Ionic Bonding involves anions and cations for the transfer of electrons.
Anion Formation:
A negatively charged ion.
Formed from the gain of one or more electrons.
Electrons being transferred by elements such as non-metals produce negative ions.
Naming Anions:
To designate anions, add -ide to the end of the root name of the element.
At the end of each non-metal element’s root name, there is -ide at the end of it.
Ionic Bond:
The electrostatic force that holds oppositely charged particles together in an ionic compound.
They can be formed when two or more atoms lose or gain electrons to form an ion.
Oppositely charged ions attract each other.
Ionic Compounds:
Compounds that contain ionic bonds.
Made up of cations and anions that are mutually attracted to one another.
Crystal:
An ion with consistent spacing and a uniform pattern formed by its ions.
The attraction between positive and negative ions in a crystal is the ionic bond.
Crystal Lattice:
A three-dimensional structure arrangement of atoms, ions, and molecules inside a crystalline solid as points.
They form large, ordered, crystal lattices in which each ion is surrounded by ions of the opposite charge.
Electrolyte:
A substance that gives ions when dissolved in water.
When an ionic compound dissolves in water makes it a solution that's capable of conducting electricity.
Lattice Energy:
A concept that represents the energy required to completely separate one mole of an ionic compound into its constituent ions in the gas phase.
Quantifies the strength of the ionic bonds that hold ions together in a crystal lattice.
The value of the lattice energy corresponds to the strength of ionic bonding.
Things that affect Lattice Energy:
-The magnitude of the charge associated with the constituent ions and the distance between the ions.
-Affected by the charge of ions and the ion's radius.
It is directly proportional to the product of the charges of ions.
Electronegativity:
The measure of an atom’s ability to attract shared electrons to itself.
More electronegative elements have the tendency to form higher ionic character bonds with other elements.
Ionization energy:
The amount of energy required to remove an electron from a gaseous electron.
High ionization indicates the atom has a strong hold on its elements.
Ionic Radius:
The distance between the nucleus of an ion and the outermost shell of the ion.
Atomic Radius: Half of the distance between nuclei of identical atoms that are chemically bonded together.
A gaseous atom is an atom in its gaseous state, it has been excited from its original state and has been crossing all the forces of attraction to be free in the gaseous state.