Explain why polar molecules are often soluble in water while non-polar molecules are not. Include discussion on the intermolecular processes involved in dissolving.
soluble = IMF solute and IMF solvent are similar; water is polar = h-bonding and dipole dipole; nonpolar solute = dispersion (way weaker than IMF in solvent)
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15
State the electron domain, molecular shape, bond angle/s and polarity: SO3
3, trigonal planar, 120, non-polar
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15
State the electron domain, molecular shape, bond angle/s and polarity: [NH4]+
4, tetrahedral, 109.5, non-polar
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15
State the electron domain, molecular shape, bond angle/s and polarity: CH2O
3, trigonal planar, 120, polar
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shark
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banana
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10
Explain why HCl is more soluble in water than Cl2.
HCl is a polar molecule (forms ion-dipole interaction with water) while Cl2 is non polar
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seesaw
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banana
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15
State the electron domain, molecular shape, bond angle/s and polarity: HCN
2, linear, 180, polar
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15
State the electron domain, molecular shape, bond angle/s and polarity: PH3
4, trigonal pyramidal, 107, polar
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10
Explain why the melting point of HF does not follow the trend of the other hydrogen halides.
HF has hydrogen bonding as its main IMF; while HCl, HBr, HI have dipole-dipole which is a generally weaker IMF than Hydrogen bonding
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15
Explain the following trend in boiling points: CH4 < C2H6 < C3H8
All molecules are nonpolar = only dispersion forces = increase in mass = stronger dispersion forces = higher BP
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15
State the electron domain, molecular shape, bond angle/s and polarity: BF3
3, trigonal planar, 120, non-polar
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10
State the relationship between IMF and vapor pressure
A liquid with weak intermolecular forces evaporates more easily and has a high vapor pressure.
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shark
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fairy
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baam
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10
Give the two common materials used in TLC as the stationary phase
