6. Shapes of Molecules and IMFs
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What is the order of repulsion between pairs?
bp-bp < bp-lp < lp-lp
Name the different bond shapes
linear, pyramidal, trigonal planar, tetrahedral, octahedral
How many bonded pairs does a compound with an octahedral shape have?
6
What happens in terms of nuclear charge and atomic radius across the periodic table L=>R
nuclear charge : increases atomic radius : decreases
Which are the most electronegative elements?
N, O, F, Cl
At what point does a polar covalent bond become ionic?
when electronegativity difference is greater than 1.8
What is a pure covalent bond?
one where no electronegativity difference is involved
What is a polar covalent bond?
when bonded atoms are different and have different electronegativity values leads to 1 atom having a greater attraction towards the bonding pair than the other
When is a covalent substance non-polar?
if there are no polar bonds if the dipoles cancel each other out i.e. the molecule is symmetrical
How do LDFs work?
instantaneous dipole shifting induced dipole in next molecule attract neighbouring molecules together
What happens to IMFs when the number of electrons in a substance increases?
larger instantaneous and induced dipoles therefore greater amount of induced dipole dipole interactions therefore stronger attractive forces between molecules