0
Using intermolecular forces explain why water is a liquid at room temperature but ammonia is a gas.?
Lbeard
The simplest answer is polarity. As I'm sure you know, both water and ammonia form hydrogen bonds with like molecules. But the critical difference is that water is a polar molecule and has a dipole moment, whereas ammonia is non-polar and does not have a dipole moment. A dipole moment is the result of polar bonds. It is important to note that having polar bonds DOES NOT necessarily make a molecule polar. Imagine that the bonds on a molecule pushes the nucleus in the direction of the bond. In a molecule with all of its bonds evenly spaced and of the same type (Hydrogen to Nitrogen, for example), such as in NH3, all of the bonds cancel each other out. But in a molecule with its bonds unevenly spaced, such as in H2O, the bonds do not cancel each other out, resulting in a dipole moment.
Wiki User
∙ 14y ago
Add your answer:
Earn +20 pts
Why is water a liquid at room temperature whereas ammonia is a gas at room temperature?
The answer lies in what is know as intermolecular forces. There three basic types: london dispersion forces (which all molecules have), dipole to dipole forces and hydrogen bonding. The stronger these forces the more the molecules have a tendancy to stick together. I listed the forces from weakest to strongest. Since water has hydrogen bonding its intermolecukar forces are the strongest and over powers the atmospheric forces and energies trying to tear the molecules away from eachother. Ammonias intermolecular forces are not strong enough under normal temperature and pressure so the molecules and individual gas molecules.
WHY ammonia has higher boiling point then phosphine?
NH3 exhibits hydrogen bonding in addition to dispersion forces. This significantly increases the intermolecular force, and raises the boiling point. PH3 does not exhibit hydrogen bonding and the dominant intermolecular force holding these molecules together is dispersion forces. (Dispersion forces also known as Van Der Waal Force)
What is the predominant intermolecular force of methane ammonia nitrogen triflouride?
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
Sulfur dioxide is compartively non ideal at 273K but behaves ideally at 327C.Explain it?
increasing the temperature increases the intermolecular spaces and decreases the intermolecular forces,thus increasing ideality.... so at high temperature of 327c sulphurdioxide is ideal as compared to 273k
What are the intermolecular forces of Carbon tetrabromide?
London Dispersion Forces.
What is the intermolecular ammonia and ammonia?
The intermolecular forces are hydrogen bonding.
What are the intermolecular forces in ammonia?
Hydrogen Bonding
How do intermolecular forces determine a substance's state?
If the intermolecular forces are great enough they can hold the molecules together as a liquid. If they are even stronger they will hold the molecules together as a solid. Water has nearly the same mass as methane and ammonia molecules, but the greater molecular forces between water molecules causes the water to be liquid at room temperature, while ammonia and methane, with weaker intermolecular forces, are gases at room temperature.
What intermolecular forces explain why water is a liquid at room temperature?
You think probable to hydrogen bonds.
Why do ammonia has higher melting and boiling point than methane?
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.
Why do ammonia has higher boiling point than methane in terms of intermolecular forces?
it doesn't
What temperature melts a solid?
The temperature at which intermolecular forces push the molecules apart
How do you explain the solubility of compounds?
List all the intermolecular forces between solutes2) List all the forces between solvents3) List all the intermolecular forces between solvent and solute4) State the energy comparisons.
Why is water a liquid at room temperature whereas ammonia is a gas at room temperature?
The answer lies in what is know as intermolecular forces. There three basic types: london dispersion forces (which all molecules have), dipole to dipole forces and hydrogen bonding. The stronger these forces the more the molecules have a tendancy to stick together. I listed the forces from weakest to strongest. Since water has hydrogen bonding its intermolecukar forces are the strongest and over powers the atmospheric forces and energies trying to tear the molecules away from eachother. Ammonias intermolecular forces are not strong enough under normal temperature and pressure so the molecules and individual gas molecules.
What type(s) of intermolecular forces are expected between NH3 molecules?
Ammonia form hydrogen bonds.
Explain how the size of hydrocarobon molecules affects the strength of intermolecular forces?
The longer the hydrocarbon chain, the stronger the intermolecular forces. This leads to higher boiling point, and these chains are likely to be less useful.
What does a high boiling temperature indicate about a substances?
intermolecular forces are hard to overcome...apex
