Show:
Bonding
IMF’s
Shapes
Allotropes
Hybrids
100
Also called an intramolecular force
Chemical bond
100
Caused by instantaneous dipoles
Van der Waals forces
100
Bond angle in trigonal planar
120°
100
What are the allotropes of carbon?
Graphite, diamond and fullerenes (C60)
100
Describe the bonding in benzene
6 sigma bonds, 3 pi bonds delocalized over ring – very stable
200
Valence electrons
Electrons in outer main energy level/shell
200
What makes a molecule have a permanent dipole?
It contains polar bond(s) and is assymetrical
200
Shape of CH4
Tetrahedral
200
Bonding and electron arrangement in diamond
Giant covalent, tetrahedral
200
Draw resonance structures of NO3-
See board!!
300
Formula of compound formed from Ca and phosphate
Ca3(PO4)2
300
State and explain boiling point trend in halogens
Increases with molar mass (F2-I2) as more electrons means more van der Waals forces
300
Bond angle in NH3
Around 107°
300
Hybridization of C in the 3 allotropes of carbon
sp2 in graphite and C60, sp3 in diamond
300
Draw the resonance hybrid of ozone, O3
See board!!
400
Consists of 1 pi and 1 sigma bond
Double bond
400
What determines whether two substances will mix and dissolve well?
Like dissolves like, substances with the same intermolecular forces will dissolve in each other
400
Electron distribution and shape of XeF2
Trigonal bipyramidal overall, linear
400
Structure of Si and SiO2
Similar to diamond: tetrahedral giant covalent
400
Which orbitals are in sigma and pi bonds?
s and p orbitals are in sigma bonds, p orbitals are in pi bonds
500
What is a polar bond?
Covalent bond where atoms have high difference in electronegativity (0.5-1.7)
500
What is a hydrogen bond?
A dipole-dipole interaction between a polar H and N, O or F.
500
Electron distribution, shape and bond angles in SF4
Trigonal bipryamidal, see-saw, 90°, 117-120° and 180°
500
Conductivity of allotropes of carbon
None in diamond. Weak in C60 and graphite due to delocalized electrons. Graphite's is stronger than C60.
500
Bond order in carbonate, CO32-
4 pairs of e- / 3 positions = 1.333