No. Sharing of six electrons would indicate a triple bond, such as that in nitrogen gas, N2. Sharing four would be a double bond, as in O2. Hope that helps :)
they'll only form 1 water molecule
Carbon (C) has 4-valence electrons. Each valence electron is capable of forming a single bond. Therefore, C can bond with up to four different atoms. Also the 4-valence electrons can form up to a triple bond (sp3 hybridization).
Oxygen likes to form single or double bonds. However it does form a triple bond in the case of CO (That is the only triple bond occurance to my knowledge)
With only 1 electron in its valence shell, the atom is likely to form an Ionic bond.
Nitrogen and sulfur can form a covalent bond with up to four bonds. This creates a strong bond between the two atoms which can be difficult to break.
No, metallic bonds only form between the atoms of a metal. Nitrogen and phosphorous are both nonmetals, and would be expected to form a covalent bond. However, I do not know if nitrogen and phosphorus bond with one another, since they are in the same group.
Chlorine cannot form a hydrogen bond only Nitrogen, Oxygen, and Flourine can
A Nitrogen molecule(N2) has a triple bond between it Nitrogen will only react only if the bond is broken. And since Chlorine cannot break this triple bond, under normal conditions, it does not react with nitrogen readily.
No. Sharing of six electrons would indicate a triple bond, such as that in nitrogen gas, N2. Sharing four would be a double bond, as in O2. Hope that helps :)
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Only oxygen. The halogens and hydrogen form single covalent bonds, and nitrogen forms a triple covalent bond.
they'll only form 1 water molecule
Ammonia can form four hydrogen bonds per molecule. The lone pair on nitrogen can accept one hydrogen to form a hydrogen bond, and the three hydrogen atoms can bond to lone pairs to form three additional hydrogen bonds. However, if ammonia is the only molecule present, this bonding pattern is problematic because each molecule only has one lone pair per three hydrogen atoms. Thus, an average molecule would likely only have two hydrogen bonds, out of the maximum of four.
The reason for this lies in the bond dissociation enthalpy of Nitrogen molecule, The two atoms are bonded by a triple bond whose enthalpy is 941.4 KJ mol-1 . So the two atoms are not very free to bond with others Not only this, the higher tendency of P to form catenation is its bigger size than N which makes the bond cleavage with other atoms easy.
The cause of polarity is the electronegativity difference between the atoms. This can occur with triple bonds. The only elents that readiliy form triple bonds are carbon and nitrogen. One example is acetonitrile H3CCN which has a triple bond between carbon and nitrogen and a high dipole moment, indicating bond polarity.
No; nitrogen can form single, double, or triple bonds.