"A covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms."
Covalent bonds in which electrons are shared unequally, resulting in partial positive and negative charges in the molecule.
Electronegativity: It is the measure of the atom's ability to attract the shared pair of electrons towards itself in a chemical bond. Polar covalent bonds occur between atoms with different electronegativities.
Dipole moment: It is the measure of the separation of charges in a molecule. Polar covalent bonds have a non-zero dipole moment.
Lewis structures: Representation of the arrangement of valence electrons in a molecule using dots or lines. Polar covalent bonds can be identified by the unequal sharing of electrons shown in the Lewis structure.
VSEPR theory: Predicts the molecular geometry and shape of molecules based on the repulsion between electron pairs. Polar covalent bonds can affect the shape of the molecule.
Hybridization: Mixing of atomic orbitals to form new hybrid orbitals that can accommodate valence electrons in a molecular orbital. Polar covalent bonds can affect the type of hybridization of atoms in a molecule.
Bond polarity: Describes the unequal distribution of electrons in a chemical bond. Polar covalent bonds have partially positive and partially negative charges on the atoms involved in the bond.
Intermolecular forces: Forces between molecules that hold them together in a compound. Polar covalent bonds can contribute to the strength of intermolecular forces.
Hydrogen bonding: A type of intermolecular force in which a hydrogen atom bonded to a highly electronegative atom (O, N or F) is attracted to another electronegative atom in a neighboring molecule. Polar covalent bonds can participate in hydrogen bonding.
Solubility: The ability of a substance to dissolve in another substance. Polar covalent bonds can affect the solubility of a molecule in a polar solvent.
Chemical reactions: A process in which atoms rearrange to form new molecules. Polar covalent bonds can determine the reactivity of a molecule in a chemical reaction.
H-F bond: This is a bond between hydrogen and fluorine. Fluorine is the most electronegative element, which makes it the most polar bond with a large dipole moment.
H-O bond: This is a bond between hydrogen and oxygen. It is polar due to oxygen's high electronegativity, which makes it the second most polar bond.
C-O bond: This is a bond between carbon and oxygen. It is polar because of oxygen's high electronegativity and carbon's relatively low electronegativity, resulting in a dipole moment.
N-H bond: This is a bond between nitrogen and hydrogen. Nitrogen is more electronegative than hydrogen, which makes this bond polar.
sulfur-oxygen: This bond between sulfur and oxygen is also polar due to the electronegativity difference between the two elements.
C-Cl bond: This is a bond between carbon and chlorine. It is polar because of chlorine's high electronegativity and carbon's relatively low electronegativity, resulting in a dipole moment.
P-O bond: This is a bond between phosphorus and oxygen. It is polar because of oxygen's high electronegativity and phosphorus's relatively low electronegativity, resulting in a dipole moment.
N-O bond: This is a bond between nitrogen and oxygen. Both elements are electronegative, resulting in a polar covalent bond.
S-H bond: This is a bond between sulfur and hydrogen. It is polar due to sulfur's higher electronegativity compared to hydrogen.
"These electron pairs are known as shared pairs or bonding pairs."
"The stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding."
"For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration."
"In organic chemistry, covalent bonding is much more common than ionic bonding."
"Covalent bonding also includes many kinds of interactions, including σ-bonding, π-bonding, metal-to-metal bonding, agostic interactions, bent bonds, three-center two-electron bonds, and three-center four-electron bonds."
"The prefix co- means jointly, associated in action, partnered to a lesser degree, etc.; thus a 'co-valent bond', in essence, means that the atoms share 'valence', such as is discussed in valence bond theory."
"In the molecule H2, the hydrogen atoms share the two electrons via covalent bonding."
"Covalency is greatest between atoms of similar electronegativities. Thus, covalent bonding does not necessarily require that the two atoms be of the same elements, only that they be of comparable electronegativity."
"Covalent bonding that entails the sharing of electrons over more than two atoms is said to be delocalized."
"Thus a 'co-valent bond', in essence, means that the atoms share 'valence', such as is discussed in valence bond theory."
"For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration."
"The stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding."
"In organic chemistry, covalent bonding is much more common than ionic bonding."
"These electron pairs are known as shared pairs or bonding pairs."
"Covalent bonding does not necessarily require that the two atoms be of the same elements, only that they be of comparable electronegativity."
"Covalent bonding also includes many kinds of interactions, including σ-bonding, π-bonding, metal-to-metal bonding, agostic interactions, bent bonds, three-center two-electron bonds, and three-center four-electron bonds."
"A covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs."
"The term covalent bond dates from 1939."
"The prefix co- means jointly, associated in action, partnered to a lesser degree, etc.; thus a 'co-valent bond', in essence, means that the atoms share 'valence', such as is discussed in valence bond theory."