Chemical Bonding and Orbital Theory Quiz

Hybrid Orbitals and Bonding

• Orbital shapes (s, p, d) are conserved when hybrid orbitals form
• Hybrid orbitals can be formed from s and d orbitals, creating a bow-tie shape
• Hybrid orbitals contain electrons in constant motion and allow for bonding with other elements
• Hybrid orbitals create a three-dimensional shape due to repulsion between electrons
• The sp3 orbital has four hybrid orbitals and forms a 3D tetrahedron shape with 109.5° bond angles
• Understanding hybridization allows visualization of covalent bond formation
• Ethane (CH3CH3) consists of two carbon atoms and six hydrogen atoms forming single covalent bonds
• Determining hybridization (sp3, sp2, or sp) depends on the number of atoms bound and the type of bond
• Single, double, and triple bonds are formed based on the number of atoms bound and the type of hybridization
• A sigma bond occurs with two hybrid orbitals overlapping, while a pi bond involves unhybridized p orbitals
• In a triple bond, sp hybridization results in two sp orbitals and two p orbitals forming pi bonds
• Acetylene demonstrates the triple bond and sp hybridization, resulting in two pi bonds and a stronger, shorter bond.

Molecular Orbital Theory and Metallic Bonding

• Electrons are assigned from lower to higher energy orbitals, and similar energy orbitals create stronger bonding orbitals
• Molecular Orbital (MO) theory provides a comprehensive understanding of how atoms bond, including bond strength and bond order
• Valence bond theory does not explain the strength difference between single and double bonds or the occurrence of bond structures with a bond order of 1.5
• Bond order, describing the type of bond between atoms, is calculated by adding electrons in bonding molecular orbitals and subtracting anti-bonding orbitals, then dividing by two
• MO theory differentiates between the strength of sigma and pi bonds, explaining why double and triple bonds are locked in place and not twice or thrice as strong as single bonds
• Bond strength is related to bond order and the energy gaps between bonding and anti-bonding orbitals, influencing the energy required to break a bond
• MO diagrams visualize orbitals, relative bond strength, and bond characteristics, demonstrating the impact of different electronegativities on bond character
• Metallic bonding involves the overlapping of outermost electron orbitals of metal atoms, allowing for the free movement of electrons, and is unique to metals
• Ionic bonds form between a metal and a non-metal, while covalent bonding occurs between non-metal atoms through the sharing of electron pairs
• Metals constitute over 80% of the periodic table, and metallic characteristics decrease somewhat from right to left toward the metalloids
• The sea of electrons bonding model, unique to metallic bonding, allows the free movement of electrons, contributing to properties vital to human survival such as the crystalline lattice configuration
• Metal atoms arrange their structure in a crystalline lattice configuration, enabling orbital overlap and providing a solid structure for electrons to travel along, with low intermolecular energy