There are three lone pairs present in chlorine atom
3 Lone pairs and one unpaired electron
NO2 has one lone pair of electrons.
The electron dot formula for hydrogen chloride (HCl) shows one bond between hydrogen and chlorine with two lone pairs of electrons around chlorine. So, it would be written as H:Cl with two dots around the Cl to represent the lone pairs.
2
In SiCl4, silicon has no lone pairs because it forms four bonds with chlorine atoms, satisfying its octet rule.
CLO2 (chlorine dioxide) has one lone pair of electrons on the chlorine atom.
The Lewis dot structure for HOCl shows oxygen with two lone pairs of electrons, chlorine with three lone pairs of electrons, and hydrogen with one lone pair of electrons. The oxygen is double bonded to the chlorine.
Two lone pair on the central selenium and three lone pairs on each chlorine. So total of eight lone pairs.
Lone-pair electrons, Bonded pairs of electrons
In $\ce{NiCl2}$, the nickel atom typically exhibits a coordination number of 6. This means that there are no lone pairs of electrons on the nickel atom, since all of its electrons are involved in bonding with the chlorine atoms to form the complex.
In NCl3, nitrogen has five valence electrons and three of these electrons are used to form covalent bonds with the three chlorine atoms. This leaves nitrogen with two lone pairs of electrons. Lone pairs are non-bonding pairs of electrons that are not involved in chemical bonding but still contribute to the overall electron density around the nitrogen atom.
There are two non-bonding pairs of electrons in Cl4. Each chlorine atom in Cl4 has 7 valence electrons, forming single covalent bonds with the other chlorine atoms, leaving two lone pairs on each chlorine atom.
The Lewis dot structure of chlorine monoxide (ClO) consists of oxygen at the center with a single bond to chlorine. Oxygen has 6 valence electrons and chlorine has 7, making a total of 13 valence electrons in the structure. Oxygen has three lone pairs of electrons and chlorine has one lone pair, satisfying the octet rule for both atoms.
There will be a total of 10 lone pairs of electrons. In NI3, each I will have 3 lone pairs (total of 9) and the N will also have 1 lone pair, for a grand total of 10 lone pairs.
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.
In ClF3, there are two lone pairs of electrons on the central chlorine atom in addition to the three bonding pairs with fluorine atoms. This makes a total of five valence electrons not involved in bond formation.
Carbon disulfide (CS2) has 2 lone pairs of electrons on the sulfur atom, giving a total of 2 lone pairs in the molecule.