Covalent bonding Flashcards
what is covalent bonding
the electrostatic attraction between protons in 2 nuclei and a shared pair of electrons between them ( pair of electrons effectively pull the protons in nuclei together)
Covalent bonding is…
A very strong attraction
what happens when non-metals bond
- they share pairs of electrons to get a full outer shell (covalent bonding)
why do simple molecular substances have low BPs
its the weak intermolecular forces (IMFs) that break, not the covalent bonds
As molecular mass increases…
so does strength of IMFs, therefore increasing BP
why are simple molecular substances not conductive
- conductivity requires charged particles that can move freely, but in this case there are no charged particles
describe C60 fullerene
unique simple molecule composed of 60 carbon atoms in a ball
Bp of C60 fullerene
- low (500-600), but not that low as high molecular mass
Characteristics of fullerene
soft and slippery solid- molecules can roll over each other easily
What are diamond, graphite and silicon dioxide examples of
giant covalent substances
diamond sublimation point
- very high
- lots of very strong covalent bonds in giant lattice
- lots of energy required to break all bonds
Structure of diamond lattice
- Every C makes 4 covalent bonds
- Tetrahedral shape
- strong, grid-like arrangement
why diamond not conduct electricity
no freely moving charged particles, as they are all neutral, and all electrons stuck inside atom or bond
uses of diamond
-used in cutting as extremely hard
structure of graphite lattice
- layers of hexagons of C atoms
- every C atom makes 3 bonds
- IMFs between each layer
- delocalised electrons inside each layer
