CHEM 167 Lecture Notes - Lecture 7: Lewis Structure, Lone Pair, Octet Rule

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tanbear441

14 Oct 2016

School

Iowa State University

Department

Chemistry

Course

CHEM 167

Professor

Gerd Meyer

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Document Summary

Energy needed to go from solid to liquid. For a salt to be soluble in a solvent(water), solvation (hydration) energy has to overcome lattice energy. The covalent bond energy is at a minimum. Bond energy: energy released when isolated atoms form a covalent bond. Bond length: the distance between the nuclei of the bonding atoms when the potential. Based on the sharing of electrons between two atoms. Each pair of electrons contains two electrons and constitutes one bond: Sing bond: two electrons in one molecular orbital. Double bonds: four electrons total, two in each olecular orbital. Triple bond: six electrons total, two in each molecular orbital. The driving force behind bond formation is lowering of overall energy. Electron density distribuiton is different for isolated atoms and covalently bonded atoms. Formed when higher electron density or probability to find electrons to be stable. When atomic orbitals from different atoms overlap to forma a bond, energy ___.

Related Questions

How does the formation of a covalent bond lower the potential energy of the two atoms in the bond? Hints How does the formation of a covalent bond lower the potential energy of the two atoms in the bond?

A)Forming a covalent bond transfers an electron from a metal to a nonmetal, which creates a favorable interaction between the resulting ions.

B)The lowest potential energy occurs when the two nuclei are an optimum distance apart from one another so that they don't repel each other.

C)The potential energy is lower when the valence electrons lie in between the positively charged nuclei than when they are close to only one nucleus.

D)Forming a covalent bond releases electrons from the atoms, which lowers the potential energy of the atoms.

Which of the following statements about Molecular Orbital Theory is FALSE?

A. Electrons placed in antibonding orbitals stabilize the ion/molecule.

B. When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in energy than the separate atomic orbitals.

C. If bond order = 0, then bond is unstable compared to individual atoms and no bond will form.

D. The total number of molecular orbitals formed always equal the number of atomic orbitals in the set.

E. The maximum number of electrons in each molecular orbital is two.

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.

Attached is picture. Please explain/show work, will give 5 stars to correct answer, thank you very much! :)

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 167 Lecture Notes - Lecture 7: Lewis Structure, Lone Pair, Octet Rule

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