1. BONDING REVIEW You must know this: 1.Ionic bonds happen with a metal and a nonmetal transferring electrons. 2.Ionic bonds are never single, double or triple. 3.Because of the positive and negative ions, ionic bonds are inherently polar 4.Ionic bonds are the strongest of bonds, holding together by opposite charge. 5.Ionic bonds form ionic compounds. 6.Aqueous ionic compounds contain loose ions in water, and these solutions will conduct electricity. 7.Solutions that conduct electricity are electrolytes 8.Ionic compounds that cannot dissolve (ionize) in water are not electrolytes. 9.Ionic compounds that COULD ionize in water, but are solids are still electrolytes by definition, but cannot conduct electricity as solids 10.All ionic compounds that are melted contain loose ions and can conduct electricity 11.If you’re a compound and your first name is a metal, you are ionic

2. And this: 11.2 or more non metals that share valence electrons are making covalent bonds. 12.Most atoms follow the octet rule when sharing electrons (they fill outer orbital to 8e ─ ) 13.Skip this one, okay. 14.Electrons are shared evenly or not, depending upon the electronegativity differences between the atoms 15.An EN Difference of zero means the bond is nonpolar 16.A difference in EN Value means the bonds are polar 17.The greater the difference, the greater the bond polarity 18.Bonds can be polar due to this EN Difference, 19.Molecules can be polar due to their shape: Radial symmetry = nonpolar 20.Radial symmetry means cut through the center and get 2 equal sides 21.Molecules with radial symmetry are “balanced” and the polarity of the bonds is offset, or balanced. 22.Polar molecules are “sticky” and will have greater melting points, greater boiling points, and lower vapor pressure (won’t evaporate as well) 23.You can rank molecules, predict their physical properties (MP, BP, VP) by their shapes/their molecular polarities

3. Metallic bonding 24.Metals are thought to be packed cations with loose valence electrons 25.This arrangement explains malleability, ductility, and electrical conduction 26.Metals melted together with other metals, or even nonmetals, form into alloys Intermolecular bonding 30.There are three kinds of intermolecular bonding in HS Chem 31.The weakest is called ELECTRON DISPERSION, due to the constant movement of the electrons. All atoms and all compounds have this. 32.We usually look to group 17 to help explain this idea 33.Electrons move very fast but at an moment they are not spread out exactly evenly in the orbital 34.This temporary, instantaneous dispersion of electrons causes spots of positive and negative to exist in the valence orbital of any atom or compounds 35.These temporary polar spots are attracted to each other (when opposite) and this causes some weak but measurable intermolecular attraction. 36.The more electrons you have, the stronger these temporary moments of polarity can be: F 2 and Cl 2 have the fewest electrons, they are gases at STP because they have the weakest temporary moments of orbital polarity

4. 37.Br 2 has more electrons, and they move more and create stronger moments of polarity in the orbitals. Bromine is a liquid at STP because of this weak but ever strengthening attraction due to the movement of electrons. 38.I 2 has the most electrons in group 17 and has the strongest intermolecular attraction called electron dispersion force, and is a SOLID at STP. 39.The second intermolecular attraction is called DIPOLE ATTRACTION. This is caused by the semi-permanent molecular polarity of polar bonds in polar molecules. 40.SCl 2 has polar bonds and does not have radial symmetry, so it’s a polar molecule. It has a positive side most of the time (sulfur) and a negative side most of the time (chlorine). Sulfur from one molecule is most often attracted to chlorine of another molecule. This “magnetic” attraction is near constant. It’s weak, but stronger than electron dispersion. 41.The more polar the bonds in the polar molecules, the stronger this dipole attraction is.

5. 37.The third intermolecular attraction is called HYDROGEN BONDING. This is really just SUPER DUPER dipole attraction, which exists when hydrogen atoms are involved in the polar bonds. 38.Because relatively speaking, the H atoms have such low electronegativity values, the polarity that can develop with H-F is so much greater when compared to the polarity between SCl 2, they give this “SUPER-DUPER DIPOLE” a new name: hydrogen bonding. Odd Ball Bonding 44.Resonating bonds exist in ozone, or O 3. A double bond/single bond situation resonates back and forth because neither of these two bonds is stable as is. This double/single reverses to single/double, and back over and over 45.Coordinate covalent bonds exist when an atom “helps” another atom obtain an octet in an odd way. CO, carbon monoxide has a “normal” double polar covalent bond. This gives the oxygen an octet but not the carbon atom. In order to get an octet, the oxygen atom pushes two of it’s unshared pairs of electrons “into the middle” so that the carbon can borrow them as well.

6. 44.PCl 5 bonds in “normal” polar covalent bonds, but the phosphorous can “get” 10 valence electrons somehow. This breaks the octet rule, but it happens. 45.When ionic compounds dissolve into water, loose positive and loose negative ions float in the water. The water can only hold a certain amount of ions (saturation). 46.The water molecules will “orient” to the ions. For example, positive sodium cations are surrounded by water molecules, but only with the negative sides of the oxygen atoms of the water molecules. 47.The negative chloride ions in water will also be surrounded by water molecules, but only by the positive hydrogen sides of the water molecules.

7. You should instantly be able to decide if a compound is ionic or covalent You should know the difference between bond polarity and molecular polarity You should be able to determine which molecule has a lower vapor pressure (or higher BP) by it’s polarity, example: methane CH 4 and water H 2 O You should be able to rank bond polarity by electronegativity differences You should be able to rank intermolecular bond strength, giving examples of each You should be able to name bonds like: ionic, single/double/or triple, polar or nonpolar covalent bonds You should know your vocabulary You should be able to draw ionic and covalent compounds as Lewis Dot diagrams. You should be able to draw covalent compounds as structural diagrams You should know when a single dash, double dash, and triple dash are necessary

8. You should be able to explain the oddball bonding in ozone, carbon monoxide, phosphorous pentachloride You should be able to define and explain with examples allotropes You should be able to answer all 100 questions on the blue sheets that I handed out, and they are online (homepage, right side click bonding, click 100 questions about bonding) Etc.