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Covalent Bonding and Electronegativity

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Explore the intricacies of covalent bonding, where atoms share electrons, and how differences in electronegativity lead to polar covalent bonds. Understand the Pauling scale of electronegativity and how factors like nuclear charge and atomic radius influence it. Discover periodic trends and how bond types are affected by electronegativity differences. Additionally, learn how molecular geometry can affect the overall polarity of molecules with symmetrical shapes.

Understanding Covalent and Polar Covalent Bonds

Covalent bonding is a fundamental chemical interaction where two atoms share one or more pairs of valence electrons, stabilizing both atoms involved. In a pure covalent bond, as seen in diatomic molecules like chlorine gas (Cl2), the electrons are shared equally due to identical electronegativity values. However, when atoms of different electronegativities bond, such as in hydrochloric acid (HCl), the shared electrons are drawn more toward the more electronegative atom, resulting in a polar covalent bond. This bond exhibits a dipole moment, a vector quantity that represents the magnitude and direction of the partial charges, with the chlorine atom acquiring a partial negative charge (δ-) and the hydrogen atom a partial positive charge (δ+).
Molecular model with colored spheres representing hydrogen, carbon, oxygen and nitrogen atoms, connected by rods to indicate chemical bonds.

Electronegativity and Bond Polarity

Electronegativity, denoted by the symbol χ, is an atom's tendency to attract and hold onto shared electrons in a chemical bond. The disparity in electronegativity between two bonded atoms dictates the bond's polarity. A larger difference in electronegativity leads to a more polar bond, with the more electronegative atom gaining a partial negative charge and the less electronegative atom obtaining a partial positive charge. This concept is crucial for predicting the behavior and properties of molecules.

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00

In a ______ bond, atoms with the same electronegativity share electrons equally, like in the molecule Cl2.

pure covalent

01

Electronegativity Symbol

Denoted by χ, symbol for atom's tendency to attract electrons.

02

Electronegativity and Bond Polarity

Greater electronegativity difference increases bond polarity.

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