Electron Configuration and Bonding Theories

Electron Configuration

• The Lewis dot structure is based on the electron configuration of atoms
• Electron configuration: the arrangement of electrons in an atom's energy levels
• Valence electrons: outermost energy level electrons, involved in bonding
• Lewis structures show the valence electrons of an atom

Bonding Theories

• Lewis dot structure is based on the valence bond theory (VBT)
• VBT: atoms share electrons to form bonds
• Electron pairs: shared electrons in a bond
• Octet rule: atoms tend to gain or lose electrons to achieve a full outer energy level (8 electrons)

Valence Shell

• Valence shell: outermost energy level of an atom
• Valence shell electrons: electrons involved in bonding
• Lewis structures show the valence shell electrons of an atom
• Valence shell expansion: atoms can expand their valence shell to accommodate more electrons

Formal Charge

• Formal charge: a way to calculate the charge on an atom in a molecule
• Formal charge = (number of valence electrons) - (number of bonds) - (number of non-bonding electrons)
• Formal charge is used to determine the stability of a molecule
• A formal charge of 0 is ideal, but it's not always possible

Hybridization

• Hybridization: the mixing of atomic orbitals to form hybrid orbitals
• Hybrid orbitals: used to describe the bonding in a molecule
• Hybridization occurs in response to the formation of bonds
• Common hybridizations: sp, sp2, sp3, which correspond to different bond angles and shapes

Electron Configuration

• Electron configuration refers to the arrangement of electrons in an atom's energy levels, with valence electrons being the outermost energy level electrons involved in bonding.
• Lewis structures are based on electron configuration, showing the valence electrons of an atom.

Bonding Theories

• The Lewis dot structure is founded on the valence bond theory (VBT), which states that atoms share electrons to form bonds.
• Electron pairs are shared electrons in a bond, and the octet rule dictates that atoms tend to gain or lose electrons to achieve a full outer energy level of 8 electrons.

Valence Shell

• The valence shell is the outermost energy level of an atom, containing valence shell electrons that are involved in bonding.
• Lewis structures depict the valence shell electrons of an atom, and valence shell expansion allows atoms to accommodate more electrons.

Formal Charge

• Formal charge is a calculation method for determining the charge on an atom in a molecule, using the formula: (number of valence electrons) - (number of bonds) - (number of non-bonding electrons).
• The goal of formal charge is to achieve a stable molecule, with a formal charge of 0 being ideal, although not always possible.

Hybridization

• Hybridization involves the mixing of atomic orbitals to form hybrid orbitals, which describe the bonding in a molecule.
• Hybridization occurs in response to bond formation, with common hybridizations including sp, sp2, and sp3, corresponding to different bond angles and shapes.