Ionic and Covalent Bonds Chemical Essay

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Crystalline solids with high melting points are formed through ionic bonding. These crystalline solids can be dissolved in water or other polar solvents. Ionic compounds are solid and good conductors of electricity (Ophardt, 2003).

Additionally, ionic bonds are formed when a metallic element gives up one or more electrons thus forming a positive ion. A positive ion is also known as a cation and has a stable electron configuration. Cations enter non-metallic elements and cause it to become a negative electron. These negative electrons are also known as anions and also have a stable electron configurations. Electrostatic forces attract cations and anions to each other. Examples of ionic compounds include calcium chloride, CaCl2, and potassium oxide, K2O (Clark, 2000).

Covalent bonds, on the other hand, do not give up, gain, or transfer electrons, but rather share electrons equally. Covalent bonds form between atoms in a compound when atoms have a similar ability to gain and/or lose ions. While ionic bonds are formed between metals and non-metals, covalent bonds are formed by combining non-metals. Covalent bonds require that molecules exist in their true form. Electrostatic forces are not present among covalent molecules. Covalent molecules exist in liquid and gaseous forms at room temperatures. Multiple covalent bonds can be formed because atoms do not have to lose or gain electrons.

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The sharing of electrons allow for multiple bonds to form.

The strongest covalent bonds are found between atoms of similar electronegativities. Electronegativity occurs when an atom attracts electrons to itself and forms negative ions. Covalent bonds do not require for the bonding atoms to be the same element, rather it only requires that these bonding atoms share a similar electronegativity. Covalent bonds are formed due to the ease of sharing electrons rather than losing or gaining the required amount of electrons for the atom to become a gas. Examples of covalents bonds include carbon dioxide, CO2, and formaldehyde, CH2O (Electron Configurations & the Periodic Table, 1999).

Reference:

Clark, J. (2000). "Ionic (Electrovalent) Bonding." Chemguide: Helping You Understand

Chemistry. Retrieved from

Decelles, P. (2001). "Chemical Bonds." The Entangled Bank, Dr. Paul's Virtually Biology

Show. Web. Retrieved from

Electron Configurations & the Periodic Table. (1999). Virtual Text of Organic Chemistry.

Retrieved from

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