Types of Chemical Bonds - AP Chemistry

Hydrogen and Helium achieve stability with 2 valence electrons. Applies because they only need to fill the 1s orbital.

Nonpolar covalent bond. Both oxygen atoms have identical electronegativity.

Triple covalent bond. More electron pairs shared means stronger attraction.

Single covalent bond. Fewer electron pairs allow atoms to be farther apart.

Atoms tend to form bonds until they are surrounded by 8 valence electrons. Applies to most main group elements except hydrogen and helium.

To maximize attraction and minimize repulsion between ions. Optimizes electrostatic interactions in three dimensions.

Larger differences typically lead to ionic bonds; smaller to covalent. Generally, differences $>1.7$ are ionic, $<0.4$ are nonpolar covalent.

Ionic bond. Dissociated ions can move and conduct electricity in solution.

The average distance between nuclei of two bonded atoms. Represents the equilibrium distance between attractive and repulsive forces.

Metallic bond. Iron atoms share electrons in a metallic lattice.

Nonpolar covalent bond. Two identical chlorine atoms share electrons equally.

$109.5^\circ$. Four atoms arranged around a central atom in 3D space.

A covalent bond with unequal sharing of electrons between atoms. Results from electronegativity differences between bonded atoms.

Covalent bond. Carbon and oxygen share electrons in double bonds.

A bond involving the sharing of electron pairs between atoms. Occurs when atoms have similar electronegativity values.

Ionic bond. $Mg^{2+}$ and $O^{2-}$ ions form an ionic compound.

Ionic bond. Strong electrostatic forces require more energy to break.

Covalent bond. Carbon shares electrons equally with four hydrogen atoms.

Metallic bond. Allows metals to conduct electricity and be malleable.

A bond formed by the electrostatic attraction between oppositely charged ions. Forms between metals and nonmetals with large electronegativity differences.

Covalent bond. Oxygen and hydrogen share electrons to form the molecule.

Electrostatic attraction. Opposite charges attract according to Coulomb's law.

A covalent bond with equal sharing of electrons between atoms. Occurs when atoms have identical or very similar electronegativity.

Ionic bond. $Na^+$ and $Cl^-$ ions are held together by electrostatic forces.

Sharing of electron pairs. Allows atoms to achieve stable electron configurations.

Attraction between free electrons and metal ions. Enables electrical conductivity in metals.

The energy required to break one mole of bonds in gaseous molecules. Also called bond dissociation energy.

Water (H₂O). Oxygen is more electronegative than hydrogen.

A covalent bond where both electrons come from the same atom. Also called a dative bond, common in complex ions.