2. How Many Lone Pairs And Bonded Pairs Are There In XeO2Cl2?

XeO2Cl2 is a molecule consisting of one xenon atom, two oxygen atoms, and two chlorine atoms.

To determine the number of lone pairs and bonded pairs in XeO2Cl2, we first need to draw its Lewis structure.

When we do so, we find that the xenon atom is located at the center, with an oxygen atom bonded to each side and a chlorine atom bonded to each oxygen. The structure looks like this:

Cl O

\ /

Xe

/ \

Cl O

Each bond represents a pair of electrons shared between the two atoms it connects. Therefore, there are two Xe-O bonds and two Xe-Cl bonds, for a total of four bonded pairs in the molecule.

To determine the number of lone pairs, we count the number of valence electrons around the central xenon atom and subtract the number of electrons involved in bonding. Xenon has 8 valence electrons, and each oxygen contributes 6 electrons to the bonding pairs, while each chlorine contributes 7 electrons. This gives us a total of:

8 + 2(6) + 2(7) = 36 electrons involved in bonding

Since xenon needs 8 electrons to achieve a full octet, we subtract the electrons involved in bonding from this total to find the number of lone pairs:

8 - 36/2 = 8 - 18 = 10 electrons = 5 lone pairs

Therefore, there are 4 bonded pairs and 5 lone pairs in XeO2Cl2.