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2 p orbitals
The answer is: 2p orbitals
To form a pentahydride, nitrogen has to undergo sp3d hybridisation. However, nitrogen does not have any 'd' orbitals and hence cannot form pentahydride.
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Half filled orbitals or empty orbitals
2 p orbitals
Nitrogen (N) is atomic number 7, so has 7 electrons in the ground state. The configuration is1s2 2s2 2p3. From this, one can see that the 1s is full, as is the 2s. So, the number of completely filled orbitals is TWO.
3 The electron configuration for nitrogen is 1s22s22p3.
The answer is: 2p orbitals
nitrogen is more reactive. neon has completely filled orbitals and is hence stable and unreactive.
no, it has three p electrons
To form a pentahydride, nitrogen has to undergo sp3d hybridisation. However, nitrogen does not have any 'd' orbitals and hence cannot form pentahydride.
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Half filled orbitals or empty orbitals
They are both sp2 hybridized orbitals.
Thus the total number of atomic orbitals in the fourth energy level of an atom is 16.
A neutral nitrogen atom has 7 protons and 7 neutrons in its nucleus and 7 electrons in orbitals around the nucleus.