Chemical Bonds (ionic)

Chemical Bonds: Ionic

Stability in Bonding Some elements combine chemically and no longer have the same properties they did before forming a compound. A chemical formula is composed of symbols and subscripts indicating the number of atoms of an element in a compound.

Atoms form compounds when the compound is more stable than the separate atoms: Atoms are STABLE when they have 8 valence (outer) electrons. (Octet Rule)

Noble gases are more chemically stable than other elements because they have a complete outer energy level. Elements that do not have full outer energy levels are more stable in compounds.

Atoms can lose, gain, or share electrons to get a stable outer energy level. A chemical bond is the force that holds atoms together in a compound.

Types of Bonds An ion is a charged particle because it has more or fewer electrons than protons. When an atom loses an electron, it becomes a positively charged ion; a superscript indicates the charge.

Na+

When an atom gains an electron, it becomes a negatively charged ion.

Cl-

An ionic compound is held together by the ionic bond – the force of attraction between opposite charges of the ions. The result of this bond is a neutral compound. The sum of the charges of the ions is zero.

Ionic bond – electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions. Forms NaCl.

Ionic Bonds: One Big Greedy Thief Dog!

Lets Practice what we’ve learned!

Octet Rule = atoms tend to gain, lose or share electrons so as to have 8 electrons C would like to Give Up or Gain 4 electrons N would like to Gain 3 electrons O would like to Gain 2 electrons