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5) Form the ionic bonds for: AlCl_(3) NaF Al_(2)O_(3) Li_(2)O

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1. **$AlCl_{3}$**: Aluminum (Al) loses three electrons to form $Al^{3+}$, and each Chlorine (Cl) gains one electron to form $Cl^{-}$. The formula $AlCl_{3}$ indicates one $Al^{3+}$ ion and three $Cl^{-}$ ions.<br />2. **NaF**: Sodium (Na) loses one electron to form $Na^{+}$, and Fluorine (F) gains one electron to form $F^{-}$. The formula NaF indicates one $Na^{+}$ ion and one $F^{-}$ ion.<br />3. **$Al_{2}O_{3}$**: Each Aluminum (Al) loses three electrons to form $Al^{3+}$, and each Oxygen (O) gains two electrons to form $O^{2-}$. The formula $Al_{2}O_{3}$ indicates two $Al^{3+}$ ions and three $O^{2-}$ ions.<br />4. **$Li_{2}O$**: Each Lithium (Li) loses one electron to form $Li^{+}$, and each Oxygen (O) gains two electrons to form $O^{2-}$. The formula $Li_{2}O$ indicates two $Li^{+}$ ions and one $O^{2-}$ ion.

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Ionic bonds form between metals and non-metals through the transfer of electrons, resulting in positively charged cations and negatively charged anions. The metal loses electrons to become a cation, and the non-metal gains electrons to become an anion.

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5) Form the ionic bonds for: AlCl_(3) NaF Al_(2)O_(3) Li_(2)O

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