Intermolecular Hydrogen bonding because hydrogen ion is less electronegative
and Oxygen ion is more electronegative.
Dr.Chandramauly Sharma(drcrsharma@in.com)
There are several intermolecular forces in water. However, by far the most significant force is hydrogen bonds, which are a type of dipole-dipole force. Hydrogen bonds exist between a hydrogen on one molecule of oxygen and the lone pair of electrons on the oxygen in another water molecule.
A special type of intermolecular force exists between water molecules called hydrogen bonding which raises its boiling point significantly with respect to its isovalent homologs. Hydrogen is unique among the elements because it has a single electron which is also a valence electron.
Particles in liquid state does not hav intermolecular forces that are as strong as that in solid state, neither are the attractive forces as weak as those in gaseous state. The particles are free to move abt but still are attracted by intermolecular forces. This explains why liq has fixed vol but no fixed shape.
There are three principal intermolecular forces between water molecules.
Starting from the strongest, they are;
hydrogen bonding > dipole attractions > Van de Waal's forces
Water molecules are linked by hydrogen bonds.
the molecules have charged regions
Glycerol have hydrogen bonds,but this intermolecular forces are slightly weaker than in water
When CH3CH2OH and H2O are mixed together to form a homogenous solution, CH3CH2OH forms additional hydrogen bonding with water molecules.
Nothing. Hydrogen bonds are very strong. When ice is melted, only weak intermolecular forces of attraction that exist between H2O molecules will be broken.
Coulombic (electrostatic) forces, mostly for the calcium and bromide ions. Hydrogen bonding for the water molecules.
It contain acetate and chaotrope. It disrupts the intermolecular forces between water molecules,allowing proteins and other macromolecules to dissolve more easily.
Glycerol have hydrogen bonds,but this intermolecular forces are slightly weaker than in water
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.
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.
Melting involve that intermolecular forces are weakened.
When CH3CH2OH and H2O are mixed together to form a homogenous solution, CH3CH2OH forms additional hydrogen bonding with water molecules.
weak intermolecular forces because dry ice with sublime
The main intermolecular forces between water molecules are hydrogen bonds which are pretty strong as far as intermolecular forces go. Between hydrocarbon chains (oil) the main intermolecular force are London force which are weaker. For two liquids to be miscible the intermolecular forces between them have to be similar in strength or they won't dissolve. Water and oil have different strengths of intermolecular bonds so don't mix.
The intermolecular forces between water molecules are lowered at the water surface and some molecules escape in the atmosphere. Evaporation is increased by temperature.
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.
Hydrogen bonding
Nothing. Hydrogen bonds are very strong. When ice is melted, only weak intermolecular forces of attraction that exist between H2O molecules will be broken.
By heating the intermolecular forces are weakened and liquid molecules can escape as a gas.