All Questions
Tagged with intermolecular-forces inorganic-chemistry
22 questions
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Melting Point Order of Benzene Derivatives
Q)Compare the melting points of the following?
o-Hydroxybenzaldehyde
o-Methoxybenzaldehyde
p-Hydroxybenzaldehyde
p-Methoxybenzaldehyde
My attempt: Intermolecular H-bonding increases melting point ...
- 77
9
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1
answer
881
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Are London dispersion forces in xenon tetrafluoride strong enough to make it a solid?
Xenon_tetrafluoride ($\ce{XeF4}$) is a well-known square-planar molecule with no dipole moment. Molecules are thus have to be bound to each other by London dispersion forces (LDF) which are known to ...
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1
answer
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Why does AsH3 have a higher boiling point than HBr?
Aside from the general trend of the boiling points of the hydrides, I noticed how the group 15 hydrides somehow "overtook" the group 17 ones in boiling point, which felt weird.
Notably, H-...
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Why is the van der Waals constant b of NH3 less than that of N2?
According to the actual data, van der Waals constant $b$ of $\ce{NH3}$ gas is $\pu{0.0371 L mol-1}$ and that of of $\ce{N2}$ gas is $\pu{0.0387 L mol-1}$.
But it should be,
$$b_{\ce{NH3}}>b_{\ce{...
- 208
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1
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Why do some hydrates need to be heated over 100 Celsius to evaporate the water?
If the boiling point of water is at 100 °C, why does a hydrate need to be heated higher than that to evaporate water from the crystals? Does it have anything to do with their intermolecular forces?
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Why is the boiling point of fluorine lower than that of oxygen?
Fluorine boils at -188.1 °C and oxygen boils at -183 °C, but shouldn't $\ce{F2}$ boil after $\ce{O2}$?
Despite being electronegative elements, both are nonpolar molecules and posses dispersion forces ...
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Why is boiling point of carbon tetrachloride greater than silicon tetrachloride?
$\ce{CCl4}$ and $\ce{SiCl4}$ both are non polar molecules thus London forces must be the only forces of interaction.
Then London forces are supposed to be greater in $\ce{SiCl4}$ due to its larger ...
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2
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Ozone in ozone layer [closed]
If ozone is a gas, and gases have the highest entropy, then how does the ozone gas stay within a few layers of the atmosphere, even though they span for kilometers?
user92006
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1
answer
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DNA pairs (adenine-thymine, guanine-cytosine) [closed]
Well I was wondering why adenine pairs with thymine and cytosine pairs with guanine.
From those pictures:
Thymine has the lowest acidity and adenine has the biggest acidity.
So it is logical that ...
user82418
-1
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1
answer
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How can we find out the type of bonding present in a compound or a molecule?
For example, if the bonding in diamond, ice, MgO or CO2 is to determine, how can I find it out? How to determine van der Waals forces?
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dipole–dipole interactions: OCR Sample Paper wrong? [closed]
I was doing OCR A Level Chemistry A, H432/01 Periodic table, elements and physical Sample Question Paper.
Question 6 was:
The boiling point of hydrogen bromide is –67 ºC.
The boiling point of ...
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6
votes
2
answers
1k
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Why is the Van der Waals constant of water lesser than benzene?
Van Der Waals constant of water and benzene ($a$) are $5.537$ and $18.82$ respectively.
I have read that the value of Van Der Waals constant indicates the extent of attractive forces.
By this, ...
- 61
0
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1
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292
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Van der Waals interaction and magnetic dipole dipole interaction
I have a conceptual question that bothers me.
From what I understand, van der Waals forces are the primary source of inter-molecular interaction. There are three different possible origins for van ...
- 69
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1
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Why is the boiling point of polonium less than that of tellurium?
My textbook states that polonium has a lower boiling point than tellurium because it has weaker intermolecular forces of attractions (van der Waals forces).
Why are van der Waals forces of attraction ...
- 2,239
1
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1
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Why is the boiling point of hydrogen sulfide higher than that of hydrogen chloride?
The boiling point of $\ce{H_2S}$ is higher than $\ce{HCl}$. Is this due to the greater number of hydrogen bond that $\ce{H_2S}$ can form compared to $\ce{HCl}$? I found this explanation for the ...
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Why is the melting point of PCl3 less than that of PCl5?
From just the IB chemistry bonding chapter information, you would normally deduce that $\ce{PCl3}$ and $\ce{PCl5}$ are both covalent molecules.
However, as $\ce{PCl3}$ has a dipole moment, it has ...
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5
votes
1
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602
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Reversed size dependence in ion solubility
My book says that solubility increases with interionic distance, because the attractive forces between ions gets smaller. However, if one of the ions in a binary ionic system is very large compared to ...
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2
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Most likely intermolecular force in aqueous ethanol
The most likely interaction to be found in an aqueous solution of ethanol is
A. London dispersion forces
B. Hydrogen bonding
C. Dipole-dipole interactions
D. Ion-dipole interactions
I am split ...
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1
answer
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Why do ethanethiol molecules have stronger London dispersion forces than those of ethanol?
I know that, molecules with higher molecular weight tend to form London forces. Is there any other reason which makes Ethanethiol to have strong London dispersion forces as compared to Ethanol?
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Why don't molecules of ionic compounds exist?
My book says:
As single ions of a metal are not associated in the solid with single ions of a non metal, separate units of ionic compounds do not exist. It is, therefore, wrong to talk of a ...
user4973
2
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1
answer
1k
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Hydration of lithium salts
Why are lithium salts heavily hydrated? I am not able to understand this because I feel salts of larger cations like Caesium should be more hydrated because of the larger size, they can able to hold ...
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Do metallic bonds contain London dispersion forces?
On our chemistry exam, a question asks "Which force is present between Fe particles? a) Van der Waals b) Metallic"
At first it seemed obvious that it was metallic; however, upon closer reading, it ...
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