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Bonding
Hey just need a bit of advice on some of these homework questions,
1)How are the hydrogen molecules held together in liquid hydrogen?
In a loosened covalent bond.
2)Explain why methane has a higher boiling temperature than hydrogen. (H2 Tb/k= 21 and CH4 Tb/k = 112)
Methane has a higher boiling temperature as it contains 4 covalent bond so needs more energy than H2 which only has 1 covalent bond.
3) The electronegativity of hydrogen, carbon and chlorine are 2.1, 2.5 and 3.0, respectively. Use these values to exaplin why the boiling temperature of hydrogen chloride is greather than that of methane. ( HCL Tb/K = 188)
No idea about this one all I can think is it's a different type of bonding in HCl...
1)How are the hydrogen molecules held together in liquid hydrogen?
In a loosened covalent bond.
2)Explain why methane has a higher boiling temperature than hydrogen. (H2 Tb/k= 21 and CH4 Tb/k = 112)
Methane has a higher boiling temperature as it contains 4 covalent bond so needs more energy than H2 which only has 1 covalent bond.
3) The electronegativity of hydrogen, carbon and chlorine are 2.1, 2.5 and 3.0, respectively. Use these values to exaplin why the boiling temperature of hydrogen chloride is greather than that of methane. ( HCL Tb/K = 188)
No idea about this one all I can think is it's a different type of bonding in HCl...
button16
Hey just need a bit of advice on some of these homework questions,
1)How are the hydrogen molecules held together in liquid hydrogen?
In a loosened covalent bond.
2)Explain why methane has a higher boiling temperature than hydrogen. (H2 Tb/k= 21 and CH4 Tb/k = 112)
Methane has a higher boiling temperature as it contains 4 covalent bond so needs more energy than H2 which only has 1 covalent bond.
3) The electronegativity of hydrogen, carbon and chlorine are 2.1, 2.5 and 3.0, respectively. Use these values to exaplin why the boiling temperature of hydrogen chloride is greather than that of methane. ( HCL Tb/K = 188)
No idea about this one all I can think is it's a different type of bonding in HCl...
1)How are the hydrogen molecules held together in liquid hydrogen?
In a loosened covalent bond.
2)Explain why methane has a higher boiling temperature than hydrogen. (H2 Tb/k= 21 and CH4 Tb/k = 112)
Methane has a higher boiling temperature as it contains 4 covalent bond so needs more energy than H2 which only has 1 covalent bond.
3) The electronegativity of hydrogen, carbon and chlorine are 2.1, 2.5 and 3.0, respectively. Use these values to exaplin why the boiling temperature of hydrogen chloride is greather than that of methane. ( HCL Tb/K = 188)
No idea about this one all I can think is it's a different type of bonding in HCl...
1. Van der Waal's forces (induced dipole - dipole interactions, also called London bonding forces)
2. Induced Dipole-dipole forces are directly proportional to the RMM of the molecules. H2 = 2 CH4 = 16 so CH4 has stronger intermolecular bonding and a higher b.p.
3. HCl is a polar molecule as the difference in electronegativeity between H and Cl is appreciable, and therefore the intermolecular forces are permanent dipole-dipole forces which are stronger than Van der Waals''s forces
you appear to be a little confused about the difference between intER and intRA molecular forces.
read up on this at intermolecular forces
The first one is right, Second one I think you need to mention that Methane contains 4 strong C-H bonds compared to Hydrogens 1 weak bond.
Hydrogen has a low electronegativity compared to Chlorine, Therefore there's a strong attraction between them [Stronger than CH4]
Hydrogen has a low electronegativity compared to Chlorine, Therefore there's a strong attraction between them [Stronger than CH4]
Godsize
The first one is right, Second one I think you need to mention that Methane contains 4 strong C-H bonds compared to Hydrogens 1 weak bond.
Hydrogen has a low electronegativity compared to Chlorine, Therefore there's a strong attraction between them [Stronger than CH4]
Hydrogen has a low electronegativity compared to Chlorine, Therefore there's a strong attraction between them [Stronger than CH4]
hey G. take care when dealing with the forces of attractions between molecules (intermolecular) and the forces (intramolecular bonding) within a molecule - they are completely different.
Hey Charco 
Yep, Exactly what I was thinking. I badly need to brush up on my AS chemistry.
Yep, Exactly what I was thinking. I badly need to brush up on my AS chemistry.Related discussions
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