Here are the essential concepts you must grasp in order to answer the question correctly.
Covalent Bonds
Covalent bonds are formed when two atoms share one or more pairs of electrons. This type of bond typically occurs between nonmetals, allowing them to achieve a full outer electron shell, which stabilizes the atoms. An example is the bond between two hydrogen atoms in a hydrogen molecule (H2).
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Ionic Bonds
Ionic bonds are formed through the transfer of electrons from one atom to another, resulting in the formation of charged ions. This type of bond usually occurs between metals and nonmetals, where the metal loses electrons to become a positively charged cation, and the nonmetal gains electrons to become a negatively charged anion. A classic example is the bond between sodium and chlorine in sodium chloride (NaCl).
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Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. The difference in electronegativity between two atoms determines the type of bond they will form: a large difference typically leads to ionic bonding, while a small difference results in covalent bonding. For instance, fluorine has a high electronegativity, which influences its bonding behavior with metals like zinc.
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Dipole Moment (Simplified) Concept 1