Hi. I need help figuring this out. I am lost. Thanks.
For the molecule, CBr4, determine the following:
Name- Carbon Tetrabromide
Electron-Dot Formula-?
Molecular Shape-?
Polarity of bonds (draw dipoles)-?
Polarity of molecules-?
Type of intermolecular forces-?
Carbon tetrabromide is the trivial name. The IUPAC name is tetrabromomethane.
These structures are almost impossible to draw on the boards because of a spacing problem. I assume you know how to draw them. If you don't let me know and I can tell you how to do it.
   Br
   ..
Br:C:Br
   ..
   Br
The above is about the best I can do. Now add 6 electrons around each Br (left, right, top or bottom unless I have already drawn a pair there).
Here is a site on the web that may help you visualize it.
http://en.wikipedia.org/wiki/Tetrabromomethane
polarity of bonds. Draw arrows from Br to C with +end on C end and arrow end (>) on the Br.
The molecule as a whole has no net dipole although each C-Br bond is a polar bond. It has no net dipole because it is symmetrical in space, shaped like a tetrahedron.
Hello! I'd be happy to help you figure it out. Let's break it down step by step.
Name: The molecule CBr4 is called Carbon Tetrabromide. This is determined by the names of the elements and the prefixes indicating the number of each element in the compound.
Electron-Dot Formula: The electron-dot formula, also known as the Lewis structure, represents the placement of valence electrons in the molecule. To determine it for CBr4, follow these steps:
1. Find the total number of valence electrons: Carbon (C) has 4 valence electrons, and Bromine (Br) has 7 valence electrons each. Since there are four Bromine atoms, we have 4 x 7 = 28 valence electrons. Adding the 4 valence electrons from Carbon, we have a total of 32 valence electrons.
2. Place the carbon atom in the center (central atom) and arrange the bromine atoms around it. Connect each bromine to the carbon atom using a single bond (shared pair of electrons).
3. Distribute the remaining valence electrons among the atoms as lone pairs. Each bromine atom requires 3 lone pairs to complete its octet. Place any remaining electrons on the central carbon atom.
The resulting electron-dot formula for CBr4 should be: C (Br) |Br (C) Br|
Molecular Shape: The molecular shape is determined by the arrangement of atoms and lone pairs around the central atom. In this case, the CBr4 molecule has a tetrahedral shape. The central carbon atom is bonded to four bromine atoms, which are positioned at the corners of a tetrahedron.
Polarity of Bonds: To determine the polarity of the bonds, we need to consider the electronegativity difference between the atoms. Carbon and bromine have different electronegativities. Bromine is more electronegative than carbon, indicating that the bonds between carbon and bromine are polar. You can indicate this by drawing an arrow pointing towards the more electronegative bromine atom in the Lewis structure.
Polarity of Molecules: The overall polarity of a molecule depends on both the polarity of its bonds and the molecular geometry. In the case of CBr4, even though the individual carbon-bromine bonds are polar, the tetrahedral shape of the molecule leads to the cancellation of dipole moments. As a result, CBr4 is a nonpolar molecule.
Type of Intermolecular Forces: The type of intermolecular forces in a molecule depends on its polarity and the types of atoms present. Since CBr4 is nonpolar, the dominant intermolecular forces will be weaker London dispersion forces.
I hope this helps you understand the different aspects of CBr4. Let me know if there's anything else I can assist you with!