Water's polarity (uneven charge distribution) attracts and surrounds ionic substance ions, breaking their bonds and enabling dissolution.

Large electronegativity difference, typically between a metal and non-metal, drives electron transfer and formation of oppositely charged ions.

Atoms combine to achieve a stable electron configuration (usually octet or noble gas-like), gaining stability and lowering their energy.

Similar electronegativity and non-metal combination lead to electron sharing, creating covalent bonds and stable configurations for both atoms.

Ionic compounds have strong electrostatic forces between ions, while polar covalent compounds have shared electron pairs with a dipole moment.

Crystalline, high melting point, and water-soluble, it's most likely an ionic compound with strong ion-dipole interactions.

Dipole compounds have uneven electron distribution, resulting in positive and negative ends like water.

Methane's symmetrical tetrahedral shape with equal electron sharing across hydrogen and carbon atoms creates a nonpolar molecule with no overall dipole moment.

a. High melting/boiling points, water-soluble, conduct electricity in solution (mobile ions), brittle/hard (strong ionic bonds).

b. Varying melting/boiling points, solubility depends on polarity, poor conductors in solid state (localized electrons), softness/flexibility varies.

Electrovalent compounds dissociate into mobile ions in solution/molten state, allowing them to carry electric current and conduct electricity.

Water's bent shape and oxygen's higher electronegativity create positive hydrogen and negative oxygen ends, making it a polar molecule with unique properties and solvent abilities.