The strong force.
The weak force.
The electro-magnetic force.
The gravitational force.
Yes, there are. Depending on its size it may have a large gravitational field, also the negative parts of all matter is attracted to the positive parts as well.
The strong force. The weak force. The electro-magnetic force. The gravitational force.
When forces of attraction are negligible among particles, the substance tends to exist in a gaseous state at ordinary conditions. The particles are far apart and exhibit random motion, resulting in a high degree of kinetic energy that overcomes any weak intermolecular forces present.
Gases have the maximum intermolecular space among the three states of matter (solid, liquid, gas). This is because gas particles are far apart and have weak forces of attraction between them, allowing them to move freely and occupy a larger volume.
In a liquid, the particles are in constant motion but are still close enough to each other to maintain some level of attraction. The intermolecular forces in a liquid (such as van der Waals forces or hydrogen bonding) prevent the particles from spreading out as much as gas particles, which have weaker intermolecular forces. This is why liquids have a definite volume and take the shape of their container, but not to the extent of gases.
Scientists can sometimes ignore the forces of attraction among particles in a gas under ordinary conditions because the kinetic energy of gas particles is much greater than the attractive forces between them. This means that the particles move around freely and independently of each other, resulting in the ideal gas behavior that doesn't consider intermolecular forces. This simplification allows for easier mathematical modeling and analysis of gas behavior.
Scientists can ignore intermolecular forces in a gas under ordinary conditions because gases have weak forces of attraction compared to liquids and solids. The particles in a gas are far apart and move freely, resulting in negligible interaction between individual particles. Hence, the effects of these weak forces are often minimal and can be disregarded for many practical purposes.
According to the kinetic theory of gases, one assumption is that the forces of attraction between particles can be ignored, particularly under ordinary conditions. However, a key point that is not an assumption of the kinetic theory is that gas particles occupy a significant volume compared to the total volume of the gas, which is incorrect; the theory assumes that gas particles themselves have negligible volume. Additionally, the theory assumes that gas particles are in constant, random motion and collide elastically with one another and the walls of their container.
Less than the energy released as attractions form between solute and solvent particles. This is the amount of energy required to break the attraction among the solute particles and among the solvents.
The name of the force present in all molecules that results from the movement of electrons is called London dispersion forces. The force of attraction between the positive end of one molecule and the negative end of another molecule is dipole .
In a gas, the particles are typically moving at high speeds and are far apart, so the forces of attraction between them are negligible. Interactions between gas particles are more controlled by collisions than by attractive forces.
Because the force of attraction among the molecules are less, moreover vanderwall force of attraction is also weak.