Determine the geometry about each interior atom in each molecule and draw the molecule. (Skeletal structure is indicated in parentheses.) a. CH3NH2 (H3CNH2) b. CH3CO2CH3 (H3CCOOCH3 both O atoms attached to second C) c. NH2CO2H (H2NCOOH both O atoms attached to C)

Understanding molecular geometry is crucial when studying chemical structures, as it impacts both physical and chemical properties of substances. It refers to the three-dimensional arrangement of atoms within a molecule. VSEPR (Valence Shell Electron Pair Repulsion) theory is a model used to predict molecular geometry. This theory states that electron pairs around a central atom will arrange themselves as far apart as possible to minimize repulsion. There are several types of molecular geometries, such as linear, bent, trigonal planar, tetrahedral, and others. For example, in CH3NH2, the geometry around the carbon atom is trigonal planar due to the three hydrogen atoms bonded to it, while the nitrogen atom has a bent geometry due to the presence of one lone pair along with two hydrogen atoms. Each molecular geometry is associated with a certain spatial arrangement that minimizes the repulsion between electron pairs, leading to a stable structure.

To enhance a student's learning, incorporating models or visual aids can greatly help in conceptualizing the spatial arrangement. Additionally, interactive tools or simulations that allow manipulation of the molecular structures could provide a more immersive learning experience.

Electron geometry, sometimes called electronic geometry, considers both the bonding and the nonbonding electron pairs surrounding the central atom. Unlike molecular geometry, which only takes into account the placement of atoms, electron geometry accounts for all electron pairs, giving a complete picture of what's happening around the central atom. Using VSEPR theory, we can determine that the electron geometry can be trigonal planar, tetrahedral, octahedral, among others, irrespective of whether the electron pairs are involved in chemical bonds. For instance, in the case of NH2CO2H, the nitrogen has a tetrahedral electron geometry including one lone pair and two hydrogen atoms, while the molecular geometry is bent. In simplifying the concept, the similarity to a classroom arrangement can be noted, where desks (electron pairs) are positioned as far apart as possible (to minimize repulsion) in the available space. Encouraging students to use molecular modeling kits can also provide a hands-on approach to understand the different electron geometries.

Chemical bonding is a fundamental concept in chemistry that explains how atoms combine to form compounds. Atoms bond to achieve greater stability, which usually involves attaining a noble gas electron configuration. There are three primary types of chemical bonds: ionic, covalent, and metallic. In our molecules CH3NH2, CH3CO2CH3, and NH2CO2H, we focus on covalent bonding, where atoms share electron pairs. For instance, in CH3CO2CH3, the carbon atoms are bonded covalently to hydrogen and oxygen atoms, with the oxygen also forming a double bond, indicating the sharing of two pairs of electrons with carbon.Explaining chemical bonding using real-life examples, such as the sharing or transferring of items among friends to create a balance, can make this abstract concept more relatable. Further, teaching students about electronegativity and how it affects bond polarity can deepen their understanding of molecular interactions and properties.