Hydrogen exists as H2. This means it's symmetrical. This means that it's non polar. This literally leaves dispersion forces as the only answer.
Van der Waals forces. Depending on the text you're using, these may be broken down into further categories.
It always has van der Waals bonds and in liquid also has hydrogen bonds.
Van der Waal, or London Dispersion forces are present in gaseous H2.
hydrogen bonds
Water is a polar substance. In liquid water, this gives rise to hydrogen bonds between molecules, making it structurally more compact. However when water is heated up to steam, those hydrogen bonds break up and the molecules cannot be maintained globally as aggregates. The forces in play in steam are of collisional type and the polarity of the molecules does result in short-range attractive forces yielding negative second virial coefficients but in no way the molecules arrange themselves to conform to a hydrogen-bonded structure. The probability of simultaneous collision between several molecules though rare in steam may become important at high pressures below the critical point, but should not be confused with the structuration between neighbouring molecules in liquid water where hydrogen bonding takes place due to the closeness between water molecules. What is sure is that there is no hydrogen bonds above the critical point of steam. In steam hydrogen bonding is just not taking place for the molecules are too distant from each other. Collisional binary encounter does not generate hydrogen bonding!!!
because it is held together by weak intermolecular forces
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.
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)
No, they are large quantities of liquid water droplets.
No, they are not. The forces between molecules in steam are not as strong as those present in liquid water.
Surface Tension Is Directly Proportional To Intermolecular Forces, Hydrogen Bonding & Viscocity
Water molecules are linked by hydrogen bonds.
The molecules of water are held together by hydrogen bonding between molecules.These are electrostatic bonds (attraction forces between opposite charges) that hydrogen makes with the oxygen of neighbouring molecules. Hydrogen, when bonded to oxygen to form water molecules, is slightly positive and the oxygen in the water molecule is slightly negative. Hydrogen gets attracted to the neighbouring slightly negative oxygen atoms.This is great for life on Earth because small molecules the size of water tend to be gases but water is a liquid. It is a liquid due to the hydrogen bonding between molecules.
The predominant force between IBr molecules in liquid IBr is Van der Waals forces, specifically dipole-dipole interactions and London dispersion forces. These forces are responsible for holding the IBr molecules together in the liquid state.
Liquids are mobile because the intermolecular forces between their molecules are weak enough to allow the molecules to move around relative to one another. These intermolecular forces are the forces of attraction between the molecules, and they are what hold the molecules together in a liquid. However, the intermolecular forces in liquids are not as strong as the intermolecular forces in solids, so the molecules in a liquid are able to move around more easily. This is why liquids can flow and take the shape of their container. The strength of the intermolecular forces in a liquid depends on the type of liquid. For example, water has strong intermolecular forces because the molecules of water are polar, meaning that they have a positive end and a negative end. This polarity allows the water molecules to form hydrogen bonds with each other, which are very strong intermolecular forces. As a result, water is a very mobile liquid, but it is not as mobile as a gas, such as air. The mobility of a liquid can also be affected by temperature. As the temperature of a liquid increases, the molecules of the liquid move faster and the intermolecular forces become weaker. This is why liquids become more mobile as they heat up. For example, water at room temperature is a liquid, but it becomes a gas when it is heated to 100 degrees Celsius.visit- In conclusion, liquids are mobile because the intermolecular forces between their molecules are weak enough to allow the molecules to move around relative to one another. The strength of the intermolecular forces in a liquid depends on the type of liquid and the temperature of the liquid.
Due to weak secondary forces between molecules...
The main intermolecular force holding water molecules together in hydrogen bonding. Also, there are diplole-dipole interactions and London dispersion forces. But hydrogen bonds are the major force keeping water in the liquid state.
Water is a polar substance. In liquid water, this gives rise to hydrogen bonds between molecules, making it structurally more compact. However when water is heated up to steam, those hydrogen bonds break up and the molecules cannot be maintained globally as aggregates. The forces in play in steam are of collisional type and the polarity of the molecules does result in short-range attractive forces yielding negative second virial coefficients but in no way the molecules arrange themselves to conform to a hydrogen-bonded structure. The probability of simultaneous collision between several molecules though rare in steam may become important at high pressures below the critical point, but should not be confused with the structuration between neighbouring molecules in liquid water where hydrogen bonding takes place due to the closeness between water molecules. What is sure is that there is no hydrogen bonds above the critical point of steam. In steam hydrogen bonding is just not taking place for the molecules are too distant from each other. Collisional binary encounter does not generate hydrogen bonding!!!
Hydrogen bonds
Van der Waal forces determine the attractiveness of molecules to others outside of covalent and ionic bonds. For water, the dipole interaction between the slightly + hydrogen end of the molecules are attracted to the slightly - oxygen end.
because it is held together by weak intermolecular forces