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Imfa BP Imfa MP Imfa V Imfa ST Imfa VP

The document discusses how various compounds' intermolecular forces of attraction affect their boiling point, melting point, viscosity, surface tension, and vapor pressure. Stronger intermolecular forces generally result in higher boiling points and melting points, as well as higher viscosity, surface tension, and lower vapor pressure. Compounds such as carbon tetrachloride and water have stronger intermolecular forces than methane and hydrogen sulfide due to factors like induced dipoles, hydrogen bonding, and surface area of interactions.

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Keren Keziah Tangarorang
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67 views4 pages

Imfa BP Imfa MP Imfa V Imfa ST Imfa VP

The document discusses how various compounds' intermolecular forces of attraction affect their boiling point, melting point, viscosity, surface tension, and vapor pressure. Stronger intermolecular forces generally result in higher boiling points and melting points, as well as higher viscosity, surface tension, and lower vapor pressure. Compounds such as carbon tetrachloride and water have stronger intermolecular forces than methane and hydrogen sulfide due to factors like induced dipoles, hydrogen bonding, and surface area of interactions.

Uploaded by

Keren Keziah Tangarorang
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Download as DOCX, PDF, TXT or read online on Scribd
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Compounds and their Boiling Melting Viscosity Surface Vapor

intermolecular forces of Point (BP) Point (V) Tension (ST) pressure (VP)
attraction (IMFA) (MP)
↑ IMFA ↑ IMFA ↑ IMFA
↑ IMFA ↑ IMFA ↑V ↑ ST ↓ VP
↑ BP ↑ MP
Higher Liquids with The
The the IMFA, stronger stronger
stronger higher will intermolecular these
the IMFA be the forces tend to forces, the
are, the viscosity have higher lower the
more surface rate of
evaporation
energy is tension than
and the
required, those with
lower the
so the weak vapor
higher the intermolecular pressure.
melting forces.
point is
CH4 (methane) CCl4 CCl4 CCl4 CCl4 CH4
- Van der Waals (only
have non-polar C-C and
C-H bonds)
CCl4 (carbon tetrachloride)
- Van der waals
(exhibited by all
molecules)

Reason: Carbon tetrachloride


exhibit a much stronger force
of attraction because electrons
are held much more loosely and
temporary dipoles are easily
induced.

(mas malaki kasi Chlorine


compare sa Hydrogen, and
because of that mas malayo ang
valence electrons sa nucleus –
meaning its loosely held kaya its
easier for fellow CCl4 to bond
with each other).
H2S H2O H2O H2O H2O H2S
- Dipole-dipole (it’s a
polar bent molecule)
- Van der waals
(exhibited by all
molecules)
-
H2O (water)
- Hydrogen Bonding
(because of O-H bond)
- Dipole-dipole
- Van der waals
(exhibited by all
molecules)

Reason: H2O have stronger


IMFA than H2S

CH3OH (methanol) CH3CH2OH CH3CH2OH CH3CH2OH CH3OH CH3OH


- Van der waals
- Hydrogen Bonding
- In addition,
CH3CH2OH (ethanol) this property
- Van der waals is heavily
- Hydrogen Bonding dependent on
the HB of a
Because ethanol have greater molecule, and
surface area and greater because
number of electrons dispersion
forces are
more
dominant
than the HB in
ethanol –
methanol
have higher
ST.
CH3COOH (acetic acid) CH3COOH CH3COOH CH3COOH CH3COOH CH3OCH3
- Van der waals
(exhibited by all
molecules)
- Hydrogen Bonding
(O-H bond)
- Dipole-dipole
CH3OCH3 (acetone)
- Van der waals
(exhibited by all
molecules)
- Dipole-dipole

Reason:
CH3COOH have stronger IMFA
than acetone because of the
hydrogen bonding.
Reference:

Molecule Lewis Structure Change in Bond Molecular Polarity of


Electronegativity Polarity Geometry Molecule

(you have to
look at the
periodic table
for this)
1. PCl5 |ENP – ENCl | Polar Trigonal Polar
Covalent Bipyramidal
= |2.2-3.0| Bond
= 0.8

2. BeCl2 |ENBe – ENCl | Polar Linear Polar


Covalent
= |1.5-3.0|
= 1.5

3. CH4 |ENC – ENH | Polar Tetrahedral Polar


Covalent
= |2.5 – 2.0|
= 0.5
4. OF2 |ENO – ENF | Polar Bent Nonpolar
Covalent Tetrahedral
= |3.5 – 4.0|
= 0.5

5. SF6 |ENS – ENF | Polar Octahedral Polar


Covalent
= |2.5 – 4.0|
= 1.5

From

and

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