1. 6.1 – NOTES Bonding and Ions

2. Chemical Bonds
Definition of a chemical bond – a force that holds two atoms together; ionic, covalent, and/or metallic;

3. Would follow the basic equation: metal  metallic cation + e-
Formation of positive ions (cations) forms when an atom (metals!) lose one or more electrons to obtain a full shell/complete octet/noble gas configuration
the element is oxidized – loss of electrons; acts as the reducing agent;
LEO the lion says GER (Loss of Electrons is Oxidation; Gain of Electrons is Reduction)
Would follow the basic equation:
metal  metallic cation + e-

4. For example: sodium is a group I metal so it has one valence electron to lose. When this happens, sodium would have a +1 charge. So the equation looks like:
Na  Na+ + e-
Aluminum has three valence electrons and will have a resulting charge of +3. The equation is:
Al  Al e-

5. Would follow the basic equation: nonmetal + e-  nonmetallic anion
Formation of negative ions (anions) forms when an atom gains (nonmetals!) one or more electrons to obtain a full shell/complete octet/noble gas configuration;
the element is reduced – gain of electrons; acts as the oxidizing agent; OIL RIG (Oxidation Is Loss of electrons and Reduction Is Gain);
to designate an anion, “ide” is added to the root name of the element (will be helpful to know this on upcoming worksheets)
Would follow the basic equation:
nonmetal + e-  nonmetallic anion

6. For example: fluorine is a group 17 nonmetal so it needs to gain 1 electron. When this happens, fluorine would have a -1 charge. So the equation looks like:
F + e-  F-
Nitrogen needs three valence electrons and will have a resulting charge of -3. The equation is:
N + 3 e-  N3-
A helpful hint – the left side of the equation must be equal to the right side of the equation in terms of charge. So if you look at the nitrogen example, both sides have a net charge of -3.