Answer:The correct explanation for the VSEPR (Valence Shell Electron Pair Repulsion) geometry of a water molecule is:
It is bent because there are two bonded pairs and two lone pairs around oxygen.
In VSEPR theory, the shape of a molecule is determined by the repulsion between electron pairs in the valence shell of the central atom. Water (H2O) has two hydrogen atoms bonded to a central oxygen atom. Oxygen has six valence electrons, and each hydrogen contributes one valence electron, making a total of eight valence electrons around the oxygen atom.
When we consider the electron pairs around the oxygen atom, we have two bonded pairs (the two pairs from the hydrogen atoms) and two lone pairs (the pairs that are not involved in bonding). According to the VSEPR theory, electron pairs (both bonded and lone pairs) repel each other and try to position themselves as far apart as possible to minimize repulsion.
In the case of water, the two lone pairs of electrons exert a stronger repulsion compared to the bonded pairs. As a result, the bonded pairs are pushed closer together, causing the molecule to adopt a bent shape. This bent shape is responsible for the VSEPR geometry of water.
To summarize, the VSEPR geometry of a water molecule is bent because there are two bonded pairs and two lone pairs around the oxygen atom.
Step-by-step explanation: