What causes high melting and boiling points?
The more energy needed, the higher the melting point or boiling point . Since the electrostatic forces of attraction between oppositely charged ions are strong, their melting and boiling points are high.
What is considered a high boiling point?
A liquid at high pressure has a higher boiling point than when that liquid is at atmospheric pressure. For example, water boils at 100 °C (212 °F) at sea level, but at 93.4 °C (200.1 °F) at 1,905 metres (6,250 ft) altitude. For a given pressure, different liquids will boil at different temperatures.
What determines melting and boiling point?
The higher the temperature, the faster the molecules move, or the faster they vibrate. … So the melting point is the temperature at which molecules in a solid can move past each other and form a liquid. The boiling point, on the other hand, involves liquids and gases.
Which metal has high melting and boiling point?
Metals usually have high melting point and boiling point. Forexample, iron, cobalt and nickel have high melting and boiling point. Tungsten has thehighest melting point. There are some exceptions – gallium and caesium have very low melting points.
What affects melting and boiling points?
The intermolecular forces between water molecules are stronger than those between oxygen molecules. In general, the bigger the molecule, the stronger the intermolecular forces, so the higher the melting and boiling points.
Do alkynes have higher boiling points?
Alkynes have higher boiling points than alkanes or alkenes, because the electric field of an alkyne, with its increased number of weakly held π electrons, is more easily distorted, producing stronger attractive forces between molecules.
Do alcohols have higher boiling points?
The boiling points of alcohols are much higher than those of alkanes with similar molecular weights. … Most of this difference results from the ability of ethanol and other alcohols to form intermolecular hydrogen bonds. (See chemical bonding: Intermolecular forces for a discussion of hydrogen bonding.)