covalent

It is certainly less strong than a full covalent bond.

However, there is no clear evidence that other covalent attachments do not form.

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

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

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

Diamond for example is a 3-dimensional crystal, but its bonds are covalent.

It is the strongest one of the covalent type.

By this definition, the covalent radius of F is 71 pm.

More recent data can be found in Covalent radius.

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

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

Support binding can be physical, ionic, or covalent in nature.

The ionic chlorine turns into the covalent kind, which is what you want.

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

The same could be said about superconductivity in covalent semiconductors.

This technique works almost exclusively on samples with covalent bonds.

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

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

They contrast to the characteristics of a covalent bond.

In a standard covalent bond each atom contributes one electron.

Covalent bonds are the ones that hold molecules together.

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

This type of bond is sometimes called polar covalent.

This is because the bonding is partially covalent in character.

This was inorganic chlorine, the safe kind, not the bad covalent stuff we were looking for.