INTERMOLECULAR FORCES AND ATOMIC PROPERTIES.
There are 2 types of forces, namely intra and intermolecular forces.
Intra force between atoms (Hydrogen and O2) Requires massive amts
of energy to break these bonds (chemical change, irreversible)
Inter Force between molecules (multiple water molecules) Doesn’t
require as much energy as with intra. (Physical change, reversible (water
to ice for eg))
Intermolecular forces:
Not all interactions between molecules are equal. Here's the lineup from
strongest to weakest:
1. Ion-dipole forces VIP relationship. Tis when ion (like Na⁺) is
attracted to partial charge on polar molecule (H₂O for eg). Main
force at work when salts dissolve in H₂O. (like when celeb (ion) gets
surrounded by fans (H₂O molecules)
2. Hydrogen bonding Strongest bond, special type of dipole-dipole
force. Occurs when H is directly to small, highly electronegative
atom (N,O,F)
3. Dipole-Dipole forces Attraction between + end of one polar
molecule and negative end of another.
4. London forces Weakest, but most common/universal force.
Exists in all molecules, polar or non-polar. Electrons can be unevenly
distributed, creating a temporary dipole, which induces a dipole in a
neighbouring molecule. Larger molecules with more electrons have
stronger, more easily polarised clouds.
It’s like when a paparazzi is taking pics of celeb, the flash is a
temporary pt of attraction (partial negative charge) but the celeb
has a far larger attraction (more e-) and stronger temporary
attraction
ATOMIC SIZE COVALENT vs Van Der Waals radius
Covalent radius Half the distance between nuclei of 2 bonded atom. Is
like your personal space when hugging friends
Van der Waals radius Half the distance between nuclei of 2 identical
non-bonded atoms just “touching” each other. Personal space on a
crowded bus, when you don’t wanna touch mense
The rule Van der Waals radius is ALWAYS larger than covalent radius.
Friends allowed to get closer than strangers.
BOND ORDER & LENGTH
There are 2 types of forces, namely intra and intermolecular forces.
Intra force between atoms (Hydrogen and O2) Requires massive amts
of energy to break these bonds (chemical change, irreversible)
Inter Force between molecules (multiple water molecules) Doesn’t
require as much energy as with intra. (Physical change, reversible (water
to ice for eg))
Intermolecular forces:
Not all interactions between molecules are equal. Here's the lineup from
strongest to weakest:
1. Ion-dipole forces VIP relationship. Tis when ion (like Na⁺) is
attracted to partial charge on polar molecule (H₂O for eg). Main
force at work when salts dissolve in H₂O. (like when celeb (ion) gets
surrounded by fans (H₂O molecules)
2. Hydrogen bonding Strongest bond, special type of dipole-dipole
force. Occurs when H is directly to small, highly electronegative
atom (N,O,F)
3. Dipole-Dipole forces Attraction between + end of one polar
molecule and negative end of another.
4. London forces Weakest, but most common/universal force.
Exists in all molecules, polar or non-polar. Electrons can be unevenly
distributed, creating a temporary dipole, which induces a dipole in a
neighbouring molecule. Larger molecules with more electrons have
stronger, more easily polarised clouds.
It’s like when a paparazzi is taking pics of celeb, the flash is a
temporary pt of attraction (partial negative charge) but the celeb
has a far larger attraction (more e-) and stronger temporary
attraction
ATOMIC SIZE COVALENT vs Van Der Waals radius
Covalent radius Half the distance between nuclei of 2 bonded atom. Is
like your personal space when hugging friends
Van der Waals radius Half the distance between nuclei of 2 identical
non-bonded atoms just “touching” each other. Personal space on a
crowded bus, when you don’t wanna touch mense
The rule Van der Waals radius is ALWAYS larger than covalent radius.
Friends allowed to get closer than strangers.
BOND ORDER & LENGTH
