Question - What type of bonding is associated with compounds that have the following characteristics:
• High melting points
• Conduct electricity in the molten state
• Solutions conduct electricity
• Normally crystalline solids at room temperature
Explain your reasoning.
Answer - There are three different types of bonds: ionic, covalent, and hydrogen. Ionic bonds have high melting points, conduct electricity in the molten state, have solutions that conduct electricity, and are normally crystalline solids at room temperature. According to Simon, Reece, and Dickey (2007) ionic bonding is the transfer of electrons, from two electrically neutral atoms, in order to create a stable (full) outer shell. After this occurs occurs "both atoms are now ions, the term for atoms that are electrically charged as a result of gaining or losing electrons" (Simon, Reece, and Dicky, 2007). Being electrically charged, they are able to conduct electricity. Also, most ionic bonds are "soluble in water, but insoluble in non-polar solvents. They require much more energy than covalent bonds to break the bond between them." (Covalent Bonds vs Ionic Bonds) Due to requiring more energy to break the bond, they have a higher melting point. Ionic bonds are formed between a metal and a non-metal.
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