Mixing of s and p orbitals can lead to some strange effects and very unstable structures that cannot be accurately described using Lewis structures. We can even predict properties of molecules that have never been and may never be made! For each part, name a 2p homonuclear diatomic (e.g. Li2, N2, Ne2, etc.) that each statement represents. Draw an MO diagram supporting your choice.
a) A molecule that has a double bond formed from two π molecular orbitals and zero σ molecular orbitals.
b) A molecule that has two unpaired electrons in antibonding orbitals.
c) A molecule with eight electrons in bonding orbitals but has a bond order of zero.
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Mixing of s and p orbitals can lead to some strange effects and very unstable structures...
13. (14 pts) MO Theory Draw the complete (core and valence) molecular orbital energy level diagram for the homonuclear diatomic molecule Be2. Use standard MO symbols to label the energy levels (That is: o, o, , or n*, as needed, with subscripts indicating which atomic orbitals formed them.) a. Sketch the molecular orbital formed when two 2p orbitals, one each on each Be atom, overlap to form a o antibonding MO b. Using your MO energy level diagram in (a),...
_ and _ bond(s) in the H2C-CH2 molecule. 25) There are A) 3 and 2 B) 3 and 4 C) 4 and 3 D) 2 and 3 E) 5 and 1 is tetrahedral 26) The electron-domain geometry of A) CBr4 B) PH3 C) CCl2Br2 D) XeF4 E) all of the above except XeF4 27) GeF3H is formed from GeH4 and GeF4 in the combination reaction: GeH4 + 3GeF4 + 4GeF3H If the reaction yield is 92.6%, how many moles of...