# data[].attributes.body
A game/sport using bows and balled arrows to tag out opponents in a manner similar to dart tag, paintball or tagball.

# data[].attributes.body
Quidditch is a sport of two teams of seven players each mounted on a broomstick, and is played on a hockey rink-sized pitch. The sport was created in 2005 at Middlebury College in Vermont, and was loosely inspired by the fictional game Quidditch in the Harry Potter books by author J. K. Rowling.

# data[].attributes.body
Disc golf is a flying disc sport in which players throw a disc at a target; it is played using rules similar to golf. Most disc golf discs are made out of polypropylene plastic, otherwise known as polypropene, which is a thermoplastic polymer resin used in a wide variety of applications.

# data[].attributes.body
1. Disc Golf
2. Quidditch
3. Dodgebow

# data[].attributes.body
Dipole-Dipole interactions result when two dipolar molecules interact with each other through space. When this occurs, the partially negative portion of one of the polar molecules is attracted to the partially positive portion of the second polar molecule.

# data[].attributes.attachment_link.description
Dipole-Dipole interactions result when two dipolar molecules interact with each other through space. When this occurs, the partially negative portion of one of the polar molecules is attracted to the …

# data[].attributes.body
Hydrogen bonding, interaction involving a hydrogen atom located between a pair of other atoms having a high affinity for electrons; such a bond is weaker than an ionic bond or covalent bond but stronger than van der Waals forces.

# data[].attributes.attachment_link.readable_text
This article was most recently revised and updated by

hydrogen bonding, interaction involving a hydrogen atom located between a pair of other atoms having a high affinity for electrons; such a bond is weaker than an ionic bond or covalent bond but stronger than van der Waals forces. Hydrogen bonds can exist between atoms in different molecules or in parts of the same molecule. One atom of the pair (the donor), generally a fluorine, nitrogen, or oxygen atom, is covalently bonded to a hydrogen atom (―FH, ―NH, or ―OH), whose electrons it shares unequally; its high electron affinity causes the hydrogen to take on a slight positive charge. The other atom of the pair, also typically F, N, or O, has an unshared electron pair, which gives it a slight negative charge. Mainly through electrostatic attraction, the donor atom effectively shares its hydrogen with the acceptor atom, forming a bond. Because of its extensive hydrogen bonding, water (H ₂O) is liquid over a far greater range of temperatures that would be expected for a molecule of its size. Water is also a good solvent for ionic compounds and many others because it readily forms hydrogen bonds with the solute. Hydrogen bonding between amino acids in a linear protein molecule determines the way it folds up into its functional configuration. Hydrogen bonds between nitrogenous bases in nucleotides on the two strands of DNA ( guanine pairs with cytosine, adenine with thymine) give rise to the double-helix structure that is crucial to the transmission of genetic information.

The Editors of Encyclopaedia Britannica Erik Gregersen.

# data[].attributes.attachment_link.title
Hydrogen bonding | Definition, Examples, & Facts

# data[].attributes.attachment_link.description
Hydrogen bonding, interaction involving a hydrogen atom located between a pair of other atoms having a high affinity for electrons; such a bond is weaker than an ionic bond or covalent bond but stronger than van der Waals forces. Hydrogen bonds can exist between atoms in different molecules or in the same molecule.

# data[].attributes.body
The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction.

# data[].attributes.attachment_link.readable_text
London Dispersion Forces

The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction. London forces are the attractive forces that cause nonpolar substances to condense to liquids and to freeze into solids when the temperature is lowered sufficiently.

Because of the constant motion of the electrons, an atom or molecule can develop a temporary (instantaneous) dipole when its electrons are distributed unsymmetrically about the nucleus.

A second atom or molecule, in turn, can be distorted by the appearance of the dipole in the first atom or molecule (because electrons repel one another) which leads to an electrostatic attraction between the two atoms or molecules.

Dispersion forces are present between any two molecules (even polar molecules) when they are almost touching.

Molecular Size
Dispersion forces are present between all molecules, whether they are polar or nonpolar.

Larger and heavier atoms and molecules exhibit stronger dispersion forces than smaller and lighter ones.

In a larger atom or molecule, the valence electrons are, on average, farther from the nuclei than in a smaller atom or molecule. They are less tightly held and can more easily form temporary dipoles.

The ease with which the electron distribution around an atom or molecule can be distorted is called the polarizability.

London dispersion forces tend to be:

stronger between molecules that are easily polarized.

weaker between molecules that are not easily polarized.

Molecular Shape
The shapes of molecules also affect the magnitudes of dispersion forces between them.

At room temperature, neopentane (C₅H₁₂) is a gas whereasn-pentane (C₅H₁₂) is a liquid.

London dispersion forces between n-pentane molecules are stronger than those between neopentane molecules even though both molecules are nonpolar and have the same molecular weight.

The somewhat cylindrical shape of n-pentane molecules allows them to come in contact with each other more effectively than the somewhat spherical neopentane molecules.

Physical Consequences of London Dispersion Forces
Cl ₂ and Br₂ have approximately the same shape and neither is polar.

1. Upon cooling, both Cl₂ and Br₂ form solids. Why?

2. At 25oC, chlorine (Cl₂) is a gas whereas bromine (Br₂) is a liquid. Why?

Click here to check your answer.

# data[].attributes.attachment_link.description
London Dispersion Forces The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction.

# data[].attributes.body
1. London Dispersion Forces
2. Hydrogen bonding
3. Dipole-dipole interactions

# data[].attributes.body
An intermolecular force is the force that mediates interaction between molecules, including the electromagnetic forces of attraction or repulsion which act between atoms and other types of neighboring particles, e.g. atoms or ions.

An intramolecular force is any force that binds together the atoms making up a molecule or compound, not to be confused with intermolecular forces, which are the forces present between molecules.