what kind of e-pair geometry, molecular geometry, and bond angles does C4H10 exhibit? I'm confused.
What are you confused about? There are no unpaired electrons. C4H10 is a saturated hydrocarbon, and the s and p orbitals are hybridized to form sp3 type bonds. These are all tetrahedral at 109.5 degrees.
Ohhhh that's right you have to look at each C separately, that's where I got mixed up, thanx.
Звдь
To determine the electron pair geometry, molecular geometry, and bond angles of C4H10, first we need to draw the Lewis structure of the molecule.
C4H10 is the formula for butane, which is an alkane. Alkanes are made up of carbon (C) and hydrogen (H) atoms connected by single bonds. Butane has 4 carbon atoms and 10 hydrogen atoms.
The Lewis structure can be drawn as follows:
H H H H
| | | |
H - C - C - C - C - H
| | | |
H H H H
In butane, each carbon atom is connected to four other atoms.
Now we can determine the electron pair geometry.
The 4 atoms around each carbon atom create a tetrahedral electron pair geometry. This is because there are no lone pairs of electrons on the carbon atoms and the molecular formula is C4H10.
Next, we can determine the molecular geometry by looking only at the arrangement of atoms, not the lone pairs of electrons.
In butane, each carbon atom is bonded to three other atoms. Therefore, the molecular geometry is also tetrahedral for each carbon atom.
Lastly, let's determine the bond angles in butane.
In a tetrahedral arrangement, the bond angles are approximately 109.5 degrees. This is because the tetrahedral arrangement maximizes the distance between the bond pairs, resulting in the most stable shape.
So, in summary, C4H10 (butane) exhibits a tetrahedral electron pair geometry, tetrahedral molecular geometry, and approximately 109.5-degree bond angles.