a. b. C. :0: d.

Use the References to access important values if needed for this ques Hybrid orbitals are formed by combining the valence orbitals on an atom. A molecule has sp³ d hybridization with 3 lone pairs. The electron pair geometry of this molecule is: The geometry of this molecule is: This molecule will have an approximate bond angle of (Choose all that apply.): 90° 109.5° 120° 180°

Use the References to access important values if needed for this question. A π bond arises from "sideways" overlap of two parallel p orbitals. The electron density lies above and below a plane containing the 2 nuclei that is perpendicular to the orbitals. Submit Answer p-orbital p-orbital atom 1 atom 2 What atomic or hybrid orbitals make up the bond between N and O in nitrosyl bromide, NOBr? sp² orbital on N + sp³ 3 orbital on O How many bonds does N have in NOBr? How many bonds does N have? + Retry Entire Group л bond 9 more group attempts remaining

Draw the following molecule and answer the questions below. H3CCHCHC(O)CH2CCH What is the hybridization/bonding orbital of the bolded atom? What is the hybridization of the bonded atom?

Draw partial orbital diagrams to describe how mixing of atomic orbital of the center atom lead to hybrid orbital in each of the following ; a. PCl3

2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew. b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.