Bonding Flashcards
(30 cards)
Carbonate ions
CO3(2-)
Nitrate Ions
NO3(-)
Hydroxide Ions
OH (-)
Sulfate Ions
SO4(2-)
Ammonium Ions
NH4(+)
Ionic Lattice Properties
-repeating units of identical structure
-soluble
-polar
-high melting points -strong ionic bonds
Ionic Bonding
The electrostatic attraction between ions of opposite charges
Very strong but weaker than covalent
Principle of Electroneutrality
States the overall charge of an ionic formula must be zero. Add or subtract cations (+) / Anions (-) to find the neutral formula
When to ionic compounds conduct electricity and why
when molten and in solution because the elections can move and carry a charge through the structure
Dative Bond / Co-ordinate bond
A covalent bond that forms when both electrons in the bond come from one atom
Dative Bond eg
ammonium ion - one ammonium molecule which is attached to a hydrogen with its lone pair
(both electrons come from the ammonia)
Which intermolecular forces are stronger
Hydrogen bonds > permanent dipole-dipole >induced dipole dipole
Temporary dipole
There is a rapid change in electron density . The electrons around a molecule move very rapidly. causing a partial charge that changes rapidly
Induced Dipole / Van Der Waals force
A temporary dipole interacts with molecules nearby
either attracting or repelling electrons
this induces a dipole caused by the initial dipole.
they are attracted to eachother
permanent dipole
The second strongest molecular interaction
Permanent dipole have delta + on one side and delta - on the other
The molecules in the liquid or solid with arrange themselves in this fashion
Where are permanent dipole interactions found
only between polar molecules
what do u call a molecule with a permanent dipole
A polar molecule
Hydrogen Bond
a dipole dipole interaction so strong it’s considered a bond
Where are hydrogen bonds found
Where H is bonded ti either O, N or F
eg. water , hydrogen fluoride, ammonia
Why do hydrogen bonds form
When a H atom bonds to an extremely electronegative atom it develops a string delta + charge
because H is so small it has a high charge density in this situation
Electronegativity
The tendency for an atom to attract electrons in a covalent bond
Which repel more Lone or paired e-
Lone pairs are held closer to the nucleus of the atom do they repel more as they are physically closer
Trend in repulsion strength (bond angles) -most to least
Lone pair - lone pair
lone pair - bonding pair
Bonding pair - bonding pair
Bond angles of a linear molecule
180⁰
2 electron pairs
