CFCIBrH (Carbon, Fluorine, Chlorine, Bromine, & Hydrogen) I Lewis Diagram of CFCIBrH I I Molecular Model Picture of CFCIBrH 1 Molecular Shape: CH,O . Lewis Diagram of CH,0 1 I Molecular Model Picture of CH.O I Molecular Shape:
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- Please answer this question, Dont use cursive handwriting, answer in clear step by step solutions, For the following molecules, give the: Lewis diagram, name of shape, bond angles (DON'T use bond angles from vsepr chart), and polarity a) F2O b) SF6 Thank you!In the BEST Lewis structure for the molecule XeF2, how many non-bonding lone pairs (1 pair = 2) of electrons are found on the central atom?Lewis structure for sulfur dioxide S02 Number of electrons set(groups)? Number of bonding electron sets (groups)? Number of non-bonding electron sets (groups) or lone pairs? How many bonds have a dipole ? If so do the dipole cancel each out?
- Draw the Lewis Structure for each covalent system a-e below, and answer the question that follows: Electronegativites: H = 2.1 C = 2.5, B = 2.0N = 3.0, 0 = 3.5 S = 2.5, F = 4.0, Xe = 2.6 a. (OF 2 )Is this molecular POLAR or NONPOLAR? b. (XeF2) What is the geometry of this molecule? c. (SO 3 ^ 2- )What is the polyatomic ion geometry? (Assume "S" obeys octet) d.( CH 2 F 2 )Is this molecular POLAR or NONPOLAR? e.( BF 3 )Is this molecular POLAR NONPOLARUsing BEST Lewis structures and the VSEPR model, match each molecular formula with the molecular geometry that describes it.central atom underlined: NH3O ICl3 XeO3 C4H4 O.R.-Lewis structure: Remember to always: • Show charge, if present. • Draw at least one more equivalent resonance structure (with «) if present, to describe delocalized covalent bonding. count all lone pairs in LS: polar: Y/N?
- Draw the attraction between a water molecule and a molecule of BrCl4F. Br is the central atom in an expanded octet - count your electrons carefully. First, draw one molecule and add the partial charges where needed - use the ΔEN to determine the types of bonds. Then, draw the second molecule so that the δ+ on one molecule lines up across from the δ- on the other. Since we can't draw the molecules here you will answer questions about the drawings that you made on the homework worksheet. BrCl4F has one __________ bond between the Br and F with ΔEN = ____________ , and four ________ bonds between the Br and Cl with a ΔEN = _________ . The central Br has 6 REDs and the molecule is symmetrical/asymmetrical (answer is ___________ ) making it a polar/nonpolar (answer is __________ ) molecule. The central Br has a ___________ charge and the F has a ________ charge. H2O has 2 ____________ bonds with a ΔEN = ___________ . H2O has 4 REDs and is symmetrical/asymmetrical (answer…I need to know how to draw the correct Lewis dot diagram for CH4 with the following image.How do you know when to draw a solid wedge vs a dashed wedge when drawing 3D bond-line structures? I know that solid-wedge means the atom is pointing towards you and dashed wedge means it's in the back, but how do you know which atoms are in the front as opposed to the back? How can you tell what the configuration will look like in space just by looking at the lewis structure or name?
- Draw out the Lewis Structures for OH2 and BeH2The molecule BeH2 has no lone pairs of es while OH2 does. Using VSEPR Theory make models which represent BeH2 and OH2.Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.1) A) Describe a polar covalent bond, and give an example B) Describe a nonpolar covalent bond, and give an example