Covalent Bond - Two atoms Share electrons Polar Covalent Bond - Two atoms share electrons, but one atom has the electron closer to itself more of the time because it has a higher electronegativity (affinity for electrons) Ionic bond - Two atoms transfer electrons from one atom to another, which forms a bond Lewis Structure - The formula of a molecule depicted by atoms with surrounding electrons represented as dots Valence Electrons - The electrons in the outer most region (shell) of the atom, still associated with that atom Non-Metals typically include the right side of the periodic table, which are usually gases at room temperature. They have no luster as solids, either. Different Bond Types - Usually either covalent, ionic (explained above) or metallic bonds, which are interactions between metal atoms due to periodic charge differences between the atoms. Solution Covalent Bond - Two atoms Share electrons Polar Covalent Bond - Two atoms share electrons, but one atom has the electron closer to itself more of the time because it has a higher electronegativity (affinity for electrons) Ionic bond - Two atoms transfer electrons from one atom to another, which forms a bond Lewis Structure - The formula of a molecule depicted by atoms with surrounding electrons represented as dots Valence Electrons - The electrons in the outer most region (shell) of the atom, still associated with that atom Non-Metals typically include the right side of the periodic table, which are usually gases at room temperature. They have no luster as solids, either. Different Bond Types - Usually either covalent, ionic (explained above) or metallic bonds, which are interactions between metal atoms due to periodic charge differences between the atoms..

1. Covalent Bond - Two atoms Share electrons Polar Covalent Bond - Two atoms
share electrons, but one atom has the electron closer to itself more of the time because it has a
higher electronegativity (affinity for electrons) Ionic bond - Two atoms transfer electrons from
one atom to another, which forms a bond Lewis Structure - The formula of a molecule depicted
by atoms with surrounding electrons represented as dots Valence Electrons - The electrons in
the outer most region (shell) of the atom, still associated with that atom Non-Metals typically
include the right side of the periodic table, which are usually gases at room temperature. They
have no luster as solids, either. Different Bond Types - Usually either covalent, ionic (explained
above) or metallic bonds, which are interactions between metal atoms due to periodic charge
differences between the atoms.
Solution
Covalent Bond - Two atoms Share electrons Polar Covalent Bond - Two atoms
share electrons, but one atom has the electron closer to itself more of the time because it has a
higher electronegativity (affinity for electrons) Ionic bond - Two atoms transfer electrons from
one atom to another, which forms a bond Lewis Structure - The formula of a molecule depicted
by atoms with surrounding electrons represented as dots Valence Electrons - The electrons in
the outer most region (shell) of the atom, still associated with that atom Non-Metals typically
include the right side of the periodic table, which are usually gases at room temperature. They
have no luster as solids, either. Different Bond Types - Usually either covalent, ionic (explained
above) or metallic bonds, which are interactions between metal atoms due to periodic charge
differences between the atoms.