As indicated by the prefix "tetra" in the compound name, each molecule of carbon tetrafluoride contains 4 fluorine atoms.
4
The Si has no lone pairs, but each F has 6 lone pairs. Thus 6 x 4 = 24 lone pairs, total.
There are two lone pairs in SF4. Each lone pair is associated with one of the fluorine atoms, resulting in a distorted trigonal bipyramidal molecular geometry.
There are 2 lone pairs in TeO3^2-.
In phosphine (PH3), there are three lone pairs and three bonding pairs.
Germanium (Ge) has 2 lone pairs of electrons.
3 Lone pairs and one unpaired electron
The Si has no lone pairs, but each F has 6 lone pairs. Thus 6 x 4 = 24 lone pairs, total.
There are two lone pairs in SF4. Each lone pair is associated with one of the fluorine atoms, resulting in a distorted trigonal bipyramidal molecular geometry.
There is one lone pair in NF3. Nitrogen has 5 valence electrons, and in NF3, it forms 3 covalent bonds with fluorine atoms, leaving one lone pair of electrons.
There are 2 lone pairs in TeO3^2-.
There are two lone pairs on XeF4.
Every pair of electrons on the central atom (S) of the Lewis structure of SF6 is shared by an F atom, so therefore there are no lone pairs on the central atom.
In phosphine (PH3), there are three lone pairs and three bonding pairs.
Germanium (Ge) has 2 lone pairs of electrons.
No lone pairs
The H2O2 molecule has two lone pairs.
The molecule BeCl2 has zero lone pairs.