Nitrogen can form three covalent bods.
An example is ammonia (NH3) with the bond angle 106,7o.
Nitrogen can form a maximum of three single covalent bonds, one with each of its three 2p electrons.
six (n-1)!
Nitrogen is diatomic because it can form three covalent bonds between two nitrogen atoms; this is a function of the orbital structure and the number of electrons which allows the third covalent bond to form in the same direction. In contrast, phosphorus has many more electrons than nitrogen and is unable to form three covalent bonds with one other atom - the electron orbitals get in the way and mechanically/electrostatically prevent the third bond from forming. Therefore, pure elemental phosphorus must make sufficient bonds between several atoms rather than just between two.
Elemental nitrogen has 7 electrons.Thus, the first (or K) shell of electrons contains 2 of them (the maximum that the K shell can accommodate).The second (or L) shell of electrons contains the remaining 5, however, the maximum number of electrons that the L shell can accommodate is 8.Therefore, elemental nitrogen has three unpaired electrons that can be used to form covalent bonds.In ammonia (NH3) all three of those unpaired electrons are paired with hydrogen atoms.Leaving only a single unshared pair of electrons in the L shell.Technically, the pair of electrons in the K shell are also an "unshared" pair but they are unavailable for covalent activity so are generally not considered as such.
The atomic weight is14.00674
maximum number of covalent bonds typically formed by fluorine is 1
Nitrogen can form a maximum of three single covalent bonds, one with each of its three 2p electrons.
The number of unpaired electrons determines the number of covalent bonds that can be formed by an atom.
Covalent bonds do not "make up" anything; they merely hold the atoms that carry the mass of the substance together. If the questioner means, "How many covalent bonds are in a nitrogen molecule with formula N2" the answer is "one triple covalent bond."
Nitrogen can form 3 covalent bonds. Nitrogen has 5 valence electrons. If nitrogen is to remain neutral complete the following equation number of valence = number of non-bonding electrons + (1/2) bonded electrons 5 = 2 + (1/2) 6
3 covalent bonds (as in ammonia).
A single covalent bond is formed by two electrons
three
Sulphur has six valence electrons and hence it can form maximum of six covalent bonds as in SF6.
It can make maximum 2 covalent bonds as element of atomic number 7 has 5 valence electrons while element having 16 atomic number have 6 valence electrons.
4
3 in neutral molecules: e.g. 3 in ammonia (3 single N-H covalent bonds); 3 in a nitrogen molecule (a triple N-N covalent bond) However 2 electrons are not used in bonding, and these can form another covalent bond in which both electrons come from the nitrogen. This is a dative or coordinate covalent bond and will result in an ion e.g. ammonium ion, NH4+