1. Apply electronegativity values and the position of two elements on the periodic table to determine the type of dominant bonding that occurs; ionic, polar covalent or nonpolar covalent Describe the lattice structure of ionic compounds and apply this to explain the physical properties of ionic compounds Describe the model of metallic bonding and apply this to explain the physical properties of metals State and explain the relationship between number of bonds, bond length and bond strength.

2. Apply electronegativity values and the position of two elements on the periodic table to determine the type of dominant bonding that occurs; ionic, polar covalent or nonpolar covalent Electronegativity -is the ability to attract electrons. -The trend in electronegativity is that it decreases down a group and increases across a period. -Metals want to give up electrons so they have very low electronegativity values.(Francium has the lowest value) -Nonmetals want to gain the electrons so they have very high electronegativity values.(Fluorine has the highest value) -It is generally recognized that a difference of 1.8 unit between the electronegativity of the atoms forming the compound will result in a compound that is predominately ionic. - Below this value the bonds are predominately covalent Location on Periodic Table The further apart the elements are on the periodic table the more likely they will be ionic.

3. The forces of electrostatic attraction between ions cause them to surround themselves with ions of opposite charge. As a result the ionic compound takes on a predictable 3-D crystalline structure known as an ionic lattice.

4. Apply the lattice structure to explain the physical properties of ionic compounds PHYSICAL PROPERTIESINFLUENCE OF LATTICE STRUCTURE -solids at room temperature -have high melting and boiling points The forces of electrostatic attraction between the ions in the lattice are strong and thus require high energy to break the attraction -are non-conductors as solids but good conductors when dissolved in water or in the molten state In order for a substance to conduct an electrical current, it must contain ions that are free to move and carry an electrical current. This is possible when the ionic compounds are dissolved or are melted (molten state) are very soluble in water and other polar solvents At the contact surface, partial charges in the water molecules are attracted to ions of opposite charge in the lattice and separate. This ions them become surrounded by the water molecule and are said to be hydrated

5. Describe the model of metallic bonding and apply this to explain the physical properties of metals PHYSICAL PROPERTIES OF METALINFLUENCE OF BONDING Good conductorsElectron are delocalized and free to move MalleableThe space between the delocalized electrons allow the metal to be flattened and the electrons moved closer to each other DuctileSame as Malleability

6. State and explain the relationship between number of bonds, bond length and bond strength. Bond typeBond lengthBond strengthExplanation SinglelongestweakestOnly one pair of electrons in bond and the bond is long making it weak Doubleintermediate Contains two pairs of electrons making it a little stronger TripleshorteststrongestContains three pairs of electrons making it strong and thus shorter