covalent bond

It is certainly less strong than a full covalent bond.

This is in agreement with the expectations from the covalent bond structure.

They are a little looser than covalent bonds, if water is around.

The chains of covalent bonds continues in all directions without end.

In others, the atoms share electrons and form covalent bonds.

Also, each carbon atom can form 4 single covalent bonds.

This structure is similar to that of diamond, and both have extremely strong covalent bonds.

This theory is used to explain the covalent bond formation in many molecules.

This technique works almost exclusively on samples with covalent bonds.

Therefore, a single bond is a type of covalent bond.

Covalent bonds are the ones that hold molecules together.

They are still elements, regardless of their covalent bonds.

A covalent bond forms when two atoms share a pair of electrons.

Single covalent bonds are formed when two atoms share an edge, as in structure C below.

The sulfate is attached to the sugar with a covalent bond.

They contrast to the characteristics of a covalent bond.

This happens, but it is a lot weaker than an equal-partners covalent bond.

When this happens, yes, it is an actual covalent bond that is being cut.

They also have single covalent bonds between their carbons.

This process involves the formation of a palladium-carbon covalent bond.

In a standard covalent bond each atom contributes one electron.

There are two electrons shared per single covalent bond.

With an electronegativity of 2.5, carbon prefers to form covalent bonds.

Each fluorine is attached to the sulfur by a single covalent bond.

Melting point: High, due to the large amount of energy required to rearrange the covalent bonds.