The total number of lone pairs of electrons on oxygen atoms of ozone is

Ozone $$(O_3)$$ contains three oxygen atoms. Since oxygen belongs to Group 16, each oxygen atom contributes 6 valence electrons.

Total valence electrons in ozone:

$$3 \times 6 = 18 \text{ electrons}$$

The Lewis structure of ozone contains one double bond and one single bond between the oxygen atoms:

$$O = O - O \leftrightarrow O - O = O$$

The bonding electrons account for:

$$1 \text{ double bond} + 1 \text{ single bond} = 4 + 2 = 6 \text{ electrons}$$

Therefore, the remaining non-bonding electrons are:

$$18 - 6 = 12 \text{ electrons}$$

These 12 electrons are present as lone pairs.

For the double-bonded terminal oxygen:

$$4 \text{ non-bonding electrons} = 2 \text{ lone pairs}$$

For the central oxygen:

$$2 \text{ non-bonding electrons} = 1 \text{ lone pair}$$

For the single-bonded terminal oxygen:

$$6 \text{ non-bonding electrons} = 3 \text{ lone pairs}$$

Hence, total lone pairs in ozone are:

$$2 + 1 + 3 = 6$$

Therefore, the total number of lone pairs present in $$O_3$$ is

$$\boxed{6}$$