CHEM 1A Study Guide - Midterm Guide: Pauli Exclusion Principle, Effective Nuclear Charge, Atomic Number

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cyansardine547

23 Dec 2020

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A neutral atom other than a hydrogen atom has more than one electron orbital energies. Nucleus of mea is more highly charged attracts electrons more lower e ( than hydrogen) energy e. Also repels each other , opposing nuclear attraction raise orbitals energies potential energy. 2e r l attraction of electron 1 to the nucleus. 2e " r l attraction of electron 2 to the nucleus e r. , z t = increase in v l pe) as electrons approach each other , r decreases attraction between the 2 electrons remember that hydrogen has only 1 electron ! All the orbitals of a given shell of a hydrogen atom are degenerate ( having the same energy ) so different calculations e - E - repulsions cause the energy of a in mea , Each electron is said to be shielded from the full attraction of the nucleus by the other to be higher than that of 25.

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Chemistry Multiple Choice Questions (1,2,3)

Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one ? bond with another carbon atom and one ? and one ? bond with another carbon atom. Each carbon atom also forms one ? bond with a hydrogen atom. Identify which types of orbitals overlap to form the bonds between the atoms in a benzene molecule. Drag the appropriate labels to their respective targets.

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Chemical bonds are formed by linear combinations of atomic orbital's. These atomic orbital's should have compatible energies. An axial overlap of these orbitals results in the formation of a sigma bond, whereas a lateral overlap results in the formation of a pi bond. When two atomic orbitai's on different atoms approach each other, two molecular orbital's are formed: one bonding molecular orbital and one antibonding molecular orbital. The bonding molecular orbital has a lower energy than the corresponding atomic orbital's: antibonding orbital's have higher energies than the corresponding atomic orbital's. An example using the hydrogen molecule is shown here. However, the same rule applies to systems with multiple atomic orbital's. For each atomic orbital that overlaps, one molecular orbital must form. In the diagram below. 1s orbitais from two hydrogen atoms combine to form one bonding sigma1 orbital and one antibonding orbital. The total number of bonding and antibonding orbital's is always equal to the number of orbital's that overlap. Similarly, molecular orbital's can also be formed by the overlapping of hybrid orbital's. The hybrid orbital's are formed by the linear combination of different atomic orbital's of nearly equal energy on the same atom. The atomic orbital's of nearly equal energy undergo a process of mixing and reorientation to form new orbital's of lower energy. This process is called hybridization For example, hybridization of one s and two p orbital's on an atom forms three sp2 hybrid orbital's. Benzene is an organic chemical compound with the molecular formula C6H6. In the benzene molecule, carbon atoms form a ring with alternating single and double bonds connecting them. Thus, each individual carbon atom forms one sigma bond with another carbon atom and one sigma and one pi bond with another carbon atom. Each carbon atom also forms one sigma bond with a hydrogen atom. Identify which types of orbital's overlap to form the bonds between the atoms in a benzene molecule.

CHEM 1A Study Guide - Midterm Guide: Pauli Exclusion Principle, Effective Nuclear Charge, Atomic Number

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