CHEM 110 Lecture Notes - Atomic Orbital, Lewis Structure

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11. 1 what a bonding theory should do. As the two h atoms approach each other, three types of interactions occur: each electron is attracted to the other nucleus, the electrons repel each other, the two nuclei repel each other. ~ the potential energy corresponds to the negative of the bond-dissociation energy. The strength of the lewis structure is its ability to be written with ease, however it is unable to demonstrate the molecular shape of the molecule. Covalent bonding: the sharing of electrons between atoms to achieve greater stability. Nucleus has a positive point charge; electron cloud is present (determined by the. If h atoms are far apart, there are no interactions: As two lone h atoms move closer together, there are interactions: Attraction from the electron cloud, results in an repulsion between the two atoms. The energy of attraction exceeds the energy of repulsion when the two atoms are 74 pm apart (maximum stabilization)

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 statement best explains the difference between the electrondistributions of a bonding orbital (e.g., H2?) and an anti-bondingorbital (e.g., He2?)?

A)The electrons in the bonding orbital tend to be distributedbetween the two atoms. This is because of their tendency to beshared among the two nuclei.
B)The electrons in an anti-bonding orbital situation tend to be asfar apart as possible. The involved nuclei repel each other.
C)In a bonding orbital situation, the electron distribution isbetween the nuclei, because both nuclei want to share theelectrons. In an anti- bonding circumstance, the electrondistribution is around each atom. There is a void between thenuclei and the nuclei repel each other.
D)Anti-bonding orbitals and bonding orbitals have similardistributions. The difference is in the overall electron densitybetween atoms.

orchidcamel629

the alignment of the rings of two interacting phenylalanines prefers to be in what configuration if no other interactions come into play but just electrostatic interaction?

A. stacked on top of each other

B. edge to edge.

C. edge to plane.

D there is no preferred orientation.

E. hydrophobic interactions cause them to repel each other.

CHEM 110 Lecture Notes - Atomic Orbital, Lewis Structure

CHEM 110 Full Course Notes

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