Covalent.
A covalent bond. Ionic bonds form crystals, not molecules.
diatomic molecules are made up of two atoms. These two atoms can either be the same of different chemical elements. Depending on what elements are in place well that depends on what kind of bonding. For example in class i learned that a homo-nuclear diatomic molecule is non-polar and covalent.
Covalent.
Non metals (groups 17, 16, 15)
Because in some covalent bonds, the electrons forming the bond are equally as likely to be near one of the bonded nuclei as the other, while in some covalent bonds the electrons forming the bond are more likely to be one of the bonded nuclei than the other. The first instance is most purely illustrated in diatomic molecules of elements such as hydrogen, nitrogen, oxygen, and the halogens in which the two bonded atoms have exactly equal electronegativity values, while the second occurs when the bonded atoms have very different electronegativities, as in hydrogen halides.
A covalent bond. Ionic bonds form crystals, not molecules.
diatomic molecules are made up of two atoms. These two atoms can either be the same of different chemical elements. Depending on what elements are in place well that depends on what kind of bonding. For example in class i learned that a homo-nuclear diatomic molecule is non-polar and covalent.
Covalent.
Hydrogen bonds are weak, but they are able to hold the backbones together. If covalent bonds held the templates together instead, the bonds would be even weaker and would likely break.
Non metals (groups 17, 16, 15)
No, they are both halogens and nonmetals with a electronegativity too close together to form an ionic bond. They, if ever bonded, would form a covalent, or polar covalent bond.
Because in some covalent bonds, the electrons forming the bond are equally as likely to be near one of the bonded nuclei as the other, while in some covalent bonds the electrons forming the bond are more likely to be one of the bonded nuclei than the other. The first instance is most purely illustrated in diatomic molecules of elements such as hydrogen, nitrogen, oxygen, and the halogens in which the two bonded atoms have exactly equal electronegativity values, while the second occurs when the bonded atoms have very different electronegativities, as in hydrogen halides.
A covalent bond is most likely to be polar when there is a large difference in the electronegativity of the two atoms that form the bond.
It means their electronegativity is equal and they are likely to be diatomic in nature. O=O, An oxygen-oxygen bond for example. Otherwise it means the two atoms ( or more ) are so close in electronegativity that there is no polarity on the molecule. Usually nonmetal to nonmetal.
Covalent bonds usually form between two nonmetals/
nonmetal with high electronegativity.
hydrogen and oxygen