Presentation on theme: "6.1 Ionic Bonding. Stable Electron Configurations When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not."— Presentation transcript:
6.1 Ionic Bonding
Stable Electron Configurations When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react. Noble gases have stable configurations with full valence electrons.
The chemical properties depend on the valence electrons. Lewis created a model of showing the valence electrons – Called the Electron dot diagram, or also the Lewis Dot Structure. – Nitrogen, Group 5A
Ionic Bonds Elements that do not have complete sets of valence electrons tend to react. Some elements achieve stable electron configurations through the transfer of electrons between atoms.
Transfer of Electrons
Formation of Ions In a neutral atom the number of protons is equal to the number of electrons. When an Ion is formed, the number of electrons is not equal to the protons. – It has an unbalanced charge called an ion.
The charge is represented by a (+) or a (-) sign. The goal is to create stable atoms.
Examples Chlorine has 17 electrons normally. – When it gains an electron it has 18, called an ION It now has a charge of 1-. Written as Cl 1- Negative Ions take the suffix “ide” in general. Chlorines Ion is Chloride
Negatively charged Ions are called ANIONS
Sodium ions have 11 protons and 10 electrons. One more proton than electron means it has a 1+ charge. Can be written as Na 1+
An ion with a positive charge is called a CATION
When a cation and an anion are close together a chemical bond forms. The type of chemical bond is an IONIC BOND.
Ionization Energy The amount of energy needed for an electron to move to a higher energy level. – Allows e- to overcome attraction of nucleus. – Takes more energy to remove e- from a nonmetal than a metal – Decreases down a group, increases across a period.
Trends in the Periodic Table
Drawing Ionic Compounds Draw an example of this….. Magnesium Chloride. 1. Draw electrons (dots) 2. Move e- to most stable configuration 3. Draw arrows to show new location 4. Write the new charge of the ions formed