Ionic Bonding
Atoms are most stable when they have a full outter shell. To accomplish this, sometimes they give up or take electrons from other atoms. As they give or take electrons, the number of negative electrons is no longer balanced by the positive protons (they are not equal in number anymore) and therefore the atom obtains a positive or negative charge and is called an ion. If the atom loses electrons, it has more protons than electrons and thus has a positive charge. Loss of one electron give a +1 charge. Loss of 2 electrons is a +2 charge and so on. If the atoms gains electrons, it now has more electrons than protons and thus has a negative charge. Gains of 2 electrons give a - 2 charge. Gains of 3 electrons gives a -3 charge and so on.
Ionic bonds occur when atoms give up and take electrons from each other and then their opposite charges attract the atoms and bond them together. A common example is with salt (NaCl), or sodium chloride. Sodium has 1 valence electron. Chloride has 7. Sodium would be more stable if it released the one valence electron and then dropped down to a full shell at the next level. Chloride has 7 in its outter shell but would be more stable with 8. Sodium releases its one electron and gains a +1 charge (because it now has one more proton than it has electrons). Chloride accepts the additional electron and gains a -1 charge. The opposide charges cause the two ions to bond.
Ionic bonds occur when atoms give up and take electrons from each other and then their opposite charges attract the atoms and bond them together. A common example is with salt (NaCl), or sodium chloride. Sodium has 1 valence electron. Chloride has 7. Sodium would be more stable if it released the one valence electron and then dropped down to a full shell at the next level. Chloride has 7 in its outter shell but would be more stable with 8. Sodium releases its one electron and gains a +1 charge (because it now has one more proton than it has electrons). Chloride accepts the additional electron and gains a -1 charge. The opposide charges cause the two ions to bond.