This uneven distribution of charge is what makes water a polar molecule, with a partial negative charge (δ-) near the oxygen and partial positive charges (δ+) near the hydrogen atoms. However, oxygen also possesses two lone pairs of electrons that are not involved in bonding.
H2O Lone Pairs and Their Impact on Water's Physical Properties
The central oxygen atom forms two covalent bonds with hydrogen atoms, sharing one electron from each hydrogen. They repel the bonding pairs, compressing the H-O-H angle from the expected 109.
As a reactant, water can act as a nucleophile, using its lone pairs to attack electron-deficient atoms. Calculating the Total Valence Electrons The calculation of valence electrons in H2O is a straightforward application of periodic table principles.
H2O Lone Pairs and Their Impact on Physical Properties
This arrangement results in a bent molecular shape with a bond angle of approximately 104. Furthermore, the polar nature derived from this electron arrangement allows water molecules to attract each other through hydrogen bonding.
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