Quantum Numbers and Electron Configuration Quiz

Orbitals and Quantum Numbers

• Each orbital is described by three sets of quantum numbers: principal (n), azimuthal (l), and magnetic (M), and spin quantum number.
• The principal quantum number (n) determines the main energy level and size of orbitals.
• The azimuthal quantum number (l) defines the shape of the orbitals.
• The magnetic quantum number (M) specifies the spatial orientation of orbitals.
• The spin quantum number describes the spin of electrons in orbitals.

Rules of Electron Arrangement

• The Aufbau principle, Pauli exclusion principle, and Hund's rule govern electron arrangement.
• Electrons fill orbitals starting with the lowest energy level.
• No orbital can contain more than two electrons with opposite spins.

Electron Arrangement in Carbon

• Carbon's electron arrangement follows the Aufbau principle, Pauli exclusion principle, and Hund's rule.
• Electrons are distributed among 1s and 2s orbitals, and the three 2p orbitals.

Orbital Hybridization

• Hybridization is the formation of new orbitals by combining two or more orbitals with different energy, shape, and size.
• Carbon atoms typically bond with other atoms using their orbitals and unpaired electrons.

sp3 Hybridization and Bond Formation in Alkanes

• sp3 hybridization involves mixing the 2s orbital and all three 2p orbitals of carbon to form four new hybrid orbitals.
• The sp3 orbitals have a tetrahedral shape and are arranged at 109.5° to each other in the excited state.
• sp3 hybridization is used in the formation of bonds in alkanes, such as methane.

sp Hybridization and Bond Formation in Alkynes

• sp hybridization involves promoting one electron from the 2s orbital to the empty 2p orbital, resulting in two hybrid orbitals of equal energy.
• The hybrid orbitals are linear and oriented at 180° to each other.
• Two of the 2p orbitals remain unhybridized and are oriented perpendicular to the plane of the linear sp orbitals and to each other.
• sp hybridization is used in the formation of bonds in alkynes, such as ethyne.

sp2 Hybridization and Bond Formation in Alkenes

• sp2 hybridization involves promoting one electron from the 2s orbital to the 2p orbital, resulting in three new hybrid orbitals.
• The sp2 hybrid orbitals are of equivalent energy and are displayed along the apex of a triangle with an angle of 120° between them.
• sp2 hybridization is used in the formation of bonds in alkenes, such as ethene.

Electronic Theory of Valency and Molecular Orbital Theory

• The electronic theory of valency suggests that chemical bonding involves the electrons in the outer shells of atoms.
• The octet rule applies to elements in the second period, including carbon, which exhibits a valency of four.
• The sp3 orbitals have higher energy than 2s but lower than 2p orbitals and contain one unpaired electron each.