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- It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how many valence electrons would such a neutral NH4 molecule have ifit could exist? a. The +1 cation, NH4+ , does exist. How many valence electrons does one NH4+ ion have? b. Draw the Lewis structure for NH4+Describe the shapes and compare the polarities of HF and HBr molecules. In each case, identify the end of the molecule that is more positive.Identify the molecular and electron geometries around each carbon (left and right). S: H H:C : C:H .. H Left Carbon Right Carbon Mol. Geo.: Mol. Geo.: Electron Geo. Electron Geo: 5.] Use electronegativity values to identify whether the following molecules are polar or nonpolar (explain why?). Indicate the polarity of each bond (towards, or from the central atom) using arrows. The molecular geometry is given in parentheses. (2 points) CH2B12 (tetrahedral geometry with C in the center) Br becavse H- Br Home Seos (trigonal planar with Se in the center) 11 4.
- 9. Determining Molecular Polarity NH, H,O CH, CH,F HCI Br BeF, BH, BHF, BEHF Struc. Form.. Н-C Molecule Linear Shape Bond 8+. 8- Polarity H-CI 2.1 3.0 Polar Molec. 8- H-Cl Polarity. Polar Polar Bond-a bond between 2 elements with UNEQUAL electron distribution. Polar Molecnle-a molecule that has UNEQUAL electron distribution over the whole molecnle3. Determine whether the following molecules are polar or nonpolar. Briefly explain how you can tell. d. е. F F .F F FWhich statement A-D about VSEPR theory is not correct? Select one: a. The steric number has five values from 2 to 6. b. Statements A-D are all correct. c. In VSEPR theory, the shape or geometry of a molecule is determined by electron-electron repulsion. d. The steric number of a central atom is the sum of the number of bonds and lone pairs around the atom. e. The molecular shape or geometry can differ from the electron-pair geometry.
- :Cl: .. : C- :Cl: .. Will this molecule be polar or nonpolar? CCI4 nonpolar polarGiven the Lewis structures below, determine whether each molecule is polar or nonpolar. (NOTE: Lewis structure drawings may not accurately represent the molecular geometry). (A) :F : (B). (C) •. As. C :F : :F: .0. Molecule A V [ Choose ] polar nonpolar Molecule B [ Choose Molecule C [ Choose ] :ü: i:See the attached lewis structure and answer the following: 1.Predict the molecular shape of methane. a. tetrahedral b. trigonal planar (120°) c. bent d. trigonal pyramidal e. linear 2. Predict the molecular shape of the carbonate ion. a. tetrahedral b. trigonal planar (120°) c. bent d. linear e. trigonal pyramidal 3. Predict the molecular shape of carbon dioxide. a. linear b. bent c. trigonal pyramidal d. trigonal planar (120°) e. tetrahedral 4. Predict the molecular shape of the sulfite ion. a. bent b. trigonal planar (120°) c. tetrahedral e. linear f. trigonal pyramidal
- bstances below. and pasting in a picture or adding an attachment of a photo to alence electrons, Lewis structure, and molecular geometry) 4. O, (double bond needed) a. Valence Electrons: b. Lewis Structure: c. Molecular Geometry:Match the bond angle(s). A) D) ****] B) [K] A. NH3 B. SF3 C. CIF4 D. PF E. 13 H-N-H H : F: ::. C) F-C-E Can't see image? Draw the best Lewis dot structures for the following molecules/ions to address the question.PART B. LEWIS STRUCTURES, VSEPR, AND MODELS IBr, Phosphorus trichloride Name or Formula NO Lewis Structure :Br: :Br: # of Electron Domains around Central Atom Name of E.D. Geometry