Chloromethane has a permanent dipole because of the chlorine molecule attached to the carbon, which means the chlorine has a partial negative charge while the carbon has a partial positive charge. These charges allow certain molecules of chloromethane to be "attracted" to other chloromethane molecules' oppositely charged regions (dipole-dipole interactions). These attractive intermolecular forces hold the molecules together and need to be broken in order for chloromethane to reach its boiling point, which requires a greater input of energy (heat).
In comparison, ethane only has the weakest intermolecular interactions holding the molecules together (van der Waals attractive forces / London forces). London forces are weak compared to dipole-dipole interactions and so less energy (heat) is required to break the bonds.
The result is that chloromethane has a higher boiling point than ethane because more heat is required to break the intermolecular bonds between chloromethane than is required to break the bonds between ethane.
Because ethanol is a polar molecule AND capable of hydrogen bonding (by C2H5-OH, an asymetric hydroxyl group) resulting in stronger intermolecular forces, it has a higher boiling point than methoxymethane.
Methoxymethane is less polar (symetrical H3C-O-CH3, though slightly bent) AND does not have a hydroxyl group, thus no hydrogen bonds between molecules.
The boiling point of methane is NOT higher, but lower than of propane (about 119 degrees lower), as can be seen from the table below:
Methane: Bp. −161 °C, 112 K
Propane: Bp. -42.1, 231.1 K
Both compounds are straight chained alkanes. (General formula CnH2n-2)
The general rule is the bigger the molecule in a group of similar compounds the higher boiling point it has. Methane is C1, butane is C4 - much bigger.
This is because methane is more stable or happier than ethane. It has a shorter carbon chain and less branching making it the harder one to boil.
The intermolecular forces in neon are weaker than those in methane
Boiling point of ethanol is higher than its isomer methane due to the presence of hydrogen bond in ethanol
no
because Xenon has more polarizable electrons.
stronger intermolecular forces of attraction
O2 because it has more electrons. Because of the higher number of electrons, it has higher dispersion forces (attractive forces). This means that more energy (heat) is required to unstick the molecules into a different state of matter.
It is a noble gas and so there are no intermolecular forces between the atoms meaning that it requires very little energy to seperate them.
Argon has the higher melting point.
because Xenon has more polarizable electrons.
stronger intermolecular forces of attraction
Whether or not the boiling point of neon is negative depends on the temperature scale used to describe the boiling point. If the boiling point is given in Celsius or Fahrenheit, the boiling point is negative. However, in Kelvin, which cannot be negative, the boiling point is positive.
O2 because it has more electrons. Because of the higher number of electrons, it has higher dispersion forces (attractive forces). This means that more energy (heat) is required to unstick the molecules into a different state of matter.
---- "The boiling point of Neon is -246.048 º C.The melting point of Neon is -248.67 º C." ----
The boiling point of Neon is -246.048 º C The melting point of Neon is -248.67 º C
Boiling Point 27.07 K Melting Point 24.56 K
Neon melts at -415.46 °F and boils at -410.94 °F
It is a noble gas and so there are no intermolecular forces between the atoms meaning that it requires very little energy to seperate them.
Melting Point- 100 degrees Freezing Point- 0 degree
Neon is defined as: a colorless odorless gaseous element that give a red glow in a vacuum tube; one of the six inert gasses; occurs in the air in small amount. Neon is neither a melting or boiling point.
The density of neon at a gas state is 0.89990g/l. The density of neon at its boiling point is 1.207g/cm3.