Pure water and sodium chloride crystals are both poor conductors of electricity by themselves. However, if sodium chloride crystals are dissolved in pure water, the solution becomes a good conductor of electricity.
How does this phenomenon demonstrate the theory of ionic bonding?
A. It shows that the attractive forces between ions are not as strong as those between water molecules.
B. It shows that water molecules are necessary for bonding to occur between positive and negative ions.
C. It shows that atoms with similar electronegativity values will share electrons equally in chemical bonds.
D. It shows that the bonds in sodium chloride crystals are made up of charged ions rather than neutral atoms.
it is B?
The solution of water and salt are good conductor of electricity because the process of dissolving makes the electrons in their atoms free to move.
The correct option is A.
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Yes, you are correct. The phenomenon described demonstrates the theory of ionic bonding because it shows that water molecules are necessary for bonding to occur between positive and negative ions. Therefore, option B is the correct answer.
Yes, it is B. The phenomenon of sodium chloride crystals becoming a good conductor of electricity when dissolved in pure water demonstrates the theory of ionic bonding because it shows that water molecules are necessary for bonding to occur between positive and negative ions.
When sodium chloride (NaCl) is solid, it consists of a lattice of positively charged sodium ions (Na+) and negatively charged chloride ions (Cl-), held together by strong ionic bonds. These ions are not free to move in solid form, so solid sodium chloride is a poor conductor of electricity.
However, when sodium chloride is dissolved in pure water, the water molecules surround the sodium and chloride ions and interact with them. The oxygen atom in water molecules has a partial negative charge, while the hydrogen atoms have partial positive charges. These partial charges on water molecules are attracted to the oppositely charged sodium and chloride ions, forming a hydration shell around them.
The hydration of sodium and chloride ions by water molecules weakens the ionic bonds between the ions in the crystal lattice. As a result, the sodium and chloride ions separate from each other and become free to move within the solution. These free-moving ions can carry electric charges, allowing the solution of sodium chloride in water to conduct electricity.
Therefore, it is evident that water molecules play a crucial role in breaking the ionic bonds and facilitating the movement of ions, making the solution a good conductor of electricity. This observation supports the theory of ionic bonding, as it highlights the significance of water molecules in bonding between positive and negative ions.