two bonds and eight lone pairs
26
No lone pairs
2
Zero
bp-4,lp-1
Boron typically forms three bonds and has no lone pairs due to its electron configuration.
Germanium typically forms four covalent bonds and has no lone pairs in its ground state.
In the case of carbon (C), it typically forms 4 bonds and has 0 lone pairs.
None.
There are three lone pairs present in chlorine atom
In SiCl4, silicon has no lone pairs because it forms four bonds with chlorine atoms, satisfying its octet rule.
Germanium, a group 14 element, has four valence electrons. In its most common oxidation state (+4), it forms four covalent bonds with surrounding atoms, using all of its valence electrons. Consequently, Germanium has no lone pairs in this state. However, in certain compounds or coordination complexes, the number of bonds and lone pairs can vary depending on the specific bonding scenario.
There are no lone pairs in the nitrate ion (NO3-). The nitrogen atom forms three sigma bonds with oxygen atoms, leaving no non-bonding pairs of electrons.
There are two lone pairs on the sulfur atom in SO2Cl2. The sulfur atom has a total of 6 valence electrons, with two bonds to oxygen atoms and two bonds to chlorine atoms. This leaves two lone pairs of electrons on the sulfur atom.
32
26
H2SO4 does not have any lone pairs. It has 2 bonding pairs shared between sulfur and oxygen in each of the O=S=O bonds. Each oxygen also has 2 unshared pairs of electrons.