Lecture 2 Study Guide

2. An example molecule where carbon atoms are sp hybridized, featuring a triple bond and a linear geometry.
5. A representation that shows hydrogen atoms or other groups directly next to the carbon atoms they are attached to.
7. An atom or group (e.g., Halogens, OH, NO₂) that attracts electrons, causing a Negative Inductive Effect (-I).
8. The angle formed between three atoms across at least two bonds.
9. An example molecule where the carbon atom is sp³ hybridized, forming four single bonds in a tetrahedral geometry.
10. A representation where every bond is shown as a line in a zigzag manner.

1. An atom or group (e.g., Alkyl group) that donates electrons, causing a Positive Inductive Effect (+I).
3. The combination of two or more atomic orbitals to create an equal number of new hybrid orbitals with different shapes and energies.
4. A local change in electron density due to electron-withdrawing or -donating groups, resulting in a permanent polarization that is transmitted through sigma bonds.
6. A representation of a compound that shows all bonds using dashes to specify the connection between atoms.
7. An example molecule where carbon atoms are sp² hybridized, featuring a double bond and a planar geometry.