CHEM 127 Lecture Notes - Lecture 8: Sulfur, Triple Bond, Chemical Formula

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silverelk210

23 Oct 2016

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The change in energy as the hydrogen atoms are moved closer and closer together. The energy decreases as they get closer together because they are sharing their electrons lling their valence shells. Then as they get even closer, the protons of the atoms are going to repel and you have to put in more and more energy to get them closer and closer together. Carbon can make four bonds and oxygen can make two bonds. Each line represent one pair of shared electrons. Must have same numbers and types of atoms as molecular formula. If you have an odd number of electrons in an atom. These molecules as a whole tend to be very reactive. Tend to be from group 2 or 13. Most commonly, beryllium from group 2 and boron from group 13. These atoms do not bring very many atoms to bond so they often times will not get lled to satisfy the octet.

Related Questions

How do you know when to draw a single/double/triple bond whendrawing Lewis Structures? I need a good answer because I stilldon't understand Lewis Strucctures.

2.BOND MATH!
-Used to determine the total number of bonds in amolecule or ion
-Forumula: Number of Bonds = (number of octet electrons - numberof valance electrons)/(2)
-Example of Bond math: PCl3. There are 4 atoms so4 times 8 (octet) = 32. And P (5 valance)
plus 7 times 3 (three Cl atoms in the molecule andCl has 7 valence electrons) equals 26. So,
(32-26)/(2)= 3 Bonds.

How do you get the number of octet electrons? Idon't see how they got 4 atoms????

rosepig378

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 127 Lecture Notes - Lecture 8: Sulfur, Triple Bond, Chemical Formula

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