ChemistryWiki | RecentChanges | Preferences
1) dsp3 hybridized
2)No NCl5 can not exist because as Q1 above stated the hybridization on the central atom is dsp3 hybridized. Since it requires that the N have an atomic d orbital to obtain this type of hybridized orbital and N (since it is in the 2nd energy level or it only has s and p orbitals) does not have them, it can hybridize so it can not exist.
3) Arrow over the more electronegative atom (or whatever way you memorize the symbol).
4) Ionic deltaEN> or = 1.7
polar bond is 1.7<deltaEN> or = 0.8
non-polar deltaEN<0.8
5) Assume polar prove non-polar
6) ionic/metallic, polar molecules, non-polar molecules
7) NH3 because all substances have hydrogen bonding so it is the one that has the most hydrogen bonds (3 of them). To be more correct (which you don't have to be), water is most likely has a higher IMF even though it only has 2 hydrogen bonding (due to the fact H-O has a stronger IMF than N-H and H-F is the strongest).
8) Evaporation is the process where liquid particles obtain enough energy to overcome their IMF and go in the gas phase for the following conditions: on the surface and at any temperature where there is a liquid phase up to but not including the boiling point of the liquid.
9) Unlike the answer above for evaporation, boiling occurs in the bulk liquid where a liquid particle needs to move other liquid particles away ( to obtain enough space to form a gas) which the other liquid particles are being pushed by atmospheric pressure. So the liquid particle can not push any other liquid particles away unless its vapor pressure is equal or greater than the atmospheric pressure (that is holding the other liquid particle from moving and creating that space for the liquid particle trying to get into gas phase).,
10.Distillation is the physical process of separating a mixture of liquid (and other phases) by boiling point differences. Both hexane and octane have London Dispersion Forces (LDF). Since octane has the higher molar mass (MW) and has the most electrons, then it will have more Instantaneous Dipoles that cause a greater LDF. Since it has a greater IMF, it will have less vapor particles in the gas phase, a lower vapor pressure and therefore a higher boiling point. Using this line of reasoning, hexane will boil first (have the lower boiling point).
11. Water is a polar molecule (exerts Hydrogen Bonding IMF or a partial CF) and oil is a non-polar molecule (exerts LDF or no CF). Since Like dissolves Like mean CF exerting substance will dissolve in each but oil is non-polar so they do not dissolve. Miscible or (immiscible is the words used instead of dissolve when 2 liquids mix.
12. No Substance B would more likely be the gas since its IMF is less than Substance A and for any given temperature there will be more Substance B particles in the gas phase so it would reach Patm at a lower temperature than Substance A.
13. Malleable is ability to exert a force onto (you are moving basic particles around) the substance and the substance does fall apart. Since there a "sea of free flowing valence electrons" (called delocalized) between every cation in the metal (part of metallic bond), then there is always an attractive force holding the electrons and cation together. In the "ionic bond" (compound) there is no "sea" just cation and anion. So when you the force moves the ions eventually two similar charged ion will be next to each other thereby exerting a repulsive force causing the substance to "break" apart.
14. *CCl4, deltaEN =0.5, 4 non-polar bonds, Tetrahedral (sym), NA, non-polar molecule, LDF
- BeCl2, deltaEN =1.5, 2 polar bonds, Linear (sym), Yes, non-polar molecule, LDF
- CS2, deltaEN=0.0, 2 non-polar bonds, Linear (sym), non-polar molecule, LDF
- NF3, deltaEN=1.0, 3 polar bonds, Pyramidal (not sym), polar molecule, dipole-dipole
15.
- H2O, 2 polar bonds, bent (not sym), No, polar molecule, Hydrogen bonding, greater IMF, less particle in gas phase, lower Pv, higher BP
vs.
- CH4, 4 non-polar bonds, Tetrahedral (sym), NA, non-polar molecule, LDF, lower IMF, more particle in gas phase, Higher Pv, lower BP
- CO, deltaEN=1.0, 1 polar bonds, Linear (sym), No, polar molecule, dipole-dipole, greater IMF, less particles in gas phase, lower Pv, higher BP
vs.
- N2, deltaEN=0.0, 1 non-polar bond, Linear (sym), NA, non-polar molecule, LDF, lower IMF, more particle in gas phase, higher, Pv, lower BP.