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2013-02-28 07:50:09
2013-02-28 07:50:09

SiH4. since it's mass is larger then CH4, London constraints are stronger.

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CH3Br has a higher boiling point.


CH3OH has the highest boiling point of the three.


This is carbon tetrachloride with the boiling point +76,72 oC.



NH3 is heavier then CH4, and NH3 has hydrogen bonding.


Metahne does not have a higher boiling point than methane. Fluoromethane, CH3F, has a boiling point of 195K, -78.2C, methane, CH4, has a boiling point of 109K approx -164 C. I make that fluoromethane has a higher temeprature boiling point than methane. This is what you would expect, London dispersion forces will be greater in CH3F as it has more electrons than CH4. CH3F is polar and there will be dipole dipole interactions which will not be present in CH4.


CBr4 is larger than CH4, so it has a higher London dispersion, a type of Intermolecular force. Higher force means longer time to bring the substance to boil, thus a higher boiling point.


Yes, Boiling point of ammonia, NH3: - 33,34 0C Boiling poit of methane, CH4: - 161,6 0C


ch3nh2, because it has hydrogen bonding going on.


Due to H bonds NH3 has high boiling point.CH4 has weak London forces


No. CH4 has a very low boiling point of about -162 degrees C.


Methane (CH4) is a gas; the boiling point is at -164 0C.


NH3 is a polar molecule, so the molecules attract each other like magnets.CH4 is completely symmetrical, so it is non polar.Therefore, NH3 has a higher boiling point because it takes more energy to knock its molecules away.


The bonds between H and O are stronger than the bonds between C and H.


Both NH3 and HCl exhibit hydrogen bonding as intermolecular forces, whereas CH4 does not. This makes CH4 have a lower boiling point. Since there are 3 hydrogen atoms in NH3 and only 1 in HCl(g), the intermolecular forces would be expected to be greater in NH3 than in HCl.


Because octane has more carbons, and the more carbons you have the higher the melting point. also octane is a gas that is very close to nonane (which is the first liquid) and that would mean it has a larger boiling point that methane (which is a gas that is the first one CH4). that is why octane has a larger boiling point that methane. Also, you can also figure it out the boiling points of each and look at the differences.


Chloromethane, or CH4, is a haloalkane, and the most abundant organohalogen in the atmosphere. It has a boiling point of -23.8 degrees Celsius.


Both have no lone pairs.They have even bonds


CH4, due to the least number of carbon atoms.


Think relationships here... really London Dispersion Force is like an acquaintance, Dipole Dipole is like boyfriend/girlfriend and Hydrogen Bonding is like marriage. Now out of the three London dispersion is the easiest to break the bonds, Di Pole Di pole are a little harder to break up and Hydrogen bonding are the hardest to break up the bonds. Hydrogen Bonding will always have the strongest bond. London dispersion is when for a split second their is a short attraction and doesn't last long. It is very weak therefore making this non- polar. Dipole Dipole means 2 opposite sides. Positive and negative charges. This molecule is a Polar molecule. Hydrogen Bonding is a Polar molecule which attaches itself to either N,O,or F. A melting point takes a low energy to melt so the bonds are weak. the higher the boiling temperature the stronger the bonds. Think H20. Melting is comparing how hard it is to separate the molecules. Same Concept. Ex.1.) CH4 / LiCl CH4 more soluable / LiCl low soluability CH4 low melting point / LiCL higher melting point CH4 low boiling point/ LiCL Higher boiling point CH4 London Dispersion / LiCl Dipole Dipole Example2: H2O / NaCl H2O high boiling point/ NaCl lower boiling point H2O Hydrogen bonding/ NaCl Dipole Dipol


Silane SiH4 is a gas molecule similar to methane CH4 where the carbon has been replaced by Silicon. It is roughy twice as heavy as methane and is pyrophoric.


CH4's melting point is -182 C. In the context of the usual type of question about melting points, CH4 has a very low melting point because the attractions between CH4 molecules are very weak.


Methane: -164 0CPhosphine: - 87,7 0CAmmonia: -33,34 0CWater: +100 0C


Ammonia (NH3) has hydrogen bonding intermolecular forces, whereas methane (CH4) does not. In addition, ammonia is polar, and so also has dipole-dipole forces and methane does not. Thus, it takes more energy (higher temperature) to boil and melt ammonia than it does methane.



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