Untitled Flashcards Set

  • NO2- Nitrite                  NO3- Nitrate

  • SO3-2  Sulfite                SO4-2 Sufate



  • Covalent Bonds are when atoms/ions SHARE electrons



  • Ionization Energy:

How strongly an atom holds onto its electrons



  • Electron Affinity:

How much an atom WANTS more electrons



  • Polar= NOT SHARED EQUALLY



  • Polar Covalent compounds will have a slightly positive charge on one side of the molecule and a slightly negative charge on the other

  • These are usually HYDROPHILIC (Love Water)

  • When there is a center charge for both positive and negative charges we call that a DIPOLE or a Dipole  MOMENT

  • Something that is Polar is able to dissociate (or dissolve) something that is ionic into its individual ions by pulling them apart 

We call these solutions SOLVENTS

  • The stronger the Solvent, the more easily it can break apart the LATTICE STRUCTURE of the ionic Compound.

  • Water has a high Polar Electronegativity and is one of the best solvents



  • Because the nonpolar compound will have similar charges (or very small differences) the overall molecule will not pull an electron more towards one side or the other



  • No Poles of Charge



  • These are HydroPHOBIC (They fear/dislike water)



  • The Shape/Structure of a Molecule Can affect its polarity as well.



  • As seen in the CO2 example, even though Carbon and Oxygen are Polar by electronegativity, the shape cancels out the charges



  • We will cover this more when we learn about VSPER



  • When Covalent bonds are formed, the Electrons are SHARED between the atoms, So we need to draw them connected together



  • We show bonded pairs with a line connecting the atoms together



  • Sometimes Electrons will bond in MORE than a Single Pair



  • If the bond between two atoms has TWO PAIRS (4 electrons) Shared, then we call it a DOUBLE BOND



  • If there is THREE PAIRS (6 electrons) shared, then we call it a TRIPLE BOND





3.92400 x 10 up 5 right

4.391 x 10-3 left