The definitions of strong and weak electrolytes relate to their ability to ionize in solution:
-
Strong Electrolytes: These substances completely ionize in solution. This means that when they dissolve in water, they break apart into their constituent ions entirely. Common examples of strong electrolytes include many salts (such as sodium chloride) and strong acids (like hydrochloric acid).
-
Weak Electrolytes: These substances only partially ionize in solution. This means that when they dissolve in water, only a fraction of the molecules dissociate into ions, while the rest remain in their molecular form. Examples of weak electrolytes include weak acids (like acetic acid) and weak bases (like ammonia).
Now, let's address the statements you provided:
-
Weak electrolytes are covalently bonded: This is generally true, as many weak electrolytes consist of covalent compounds that ionize only partially in solution.
-
Strong electrolytes completely ionize in solution: This is accurate.
-
Weak electrolytes never ionize in solution: This is incorrect. Weak electrolytes do ionize, but only partially.
-
Strong electrolytes do not completely ionize in solution: This is incorrect. Strong electrolytes do completely ionize in solution.
In summary, the main distinction is that strong electrolytes fully dissociate into ions, while weak electrolytes only partially dissociate.