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- 1.) Use the VSEPR model to determine the three-dimensional shapes ofcarbon tetraiodide, CI4, and phosphine, PH3. Circle the correct answer! Choose only 1. CI4: Linear trigonal planar bent tetrahedral trigonal pyramidal trigonal bipyramidal seesaw T-shaped Octahedral square pyramidal square planar Circle the correct answer! Choose only 1. PH3: Linear trigonal planar bent tetrahedral trigonal pyramidal trigonal bipyramidal seesaw T-shaped Octahedral square pyramidal square planar 2.) Identify the polarity of carbon dioxide (CO2) and water (H2O) based upon its geometry and the dipole moments of the individual bonds. Circle the correct answer! Choose only 1. carbon dioxide: Polar nonpolar Circle the correct answer! Choose only 1.water: polar nonpolarPlatinum hexafluoride is an extremely strong oxidizing agent. It can even oxidize oxygen, its reaction with O2 giving O2+PtF6−.a. Sketch the molecular orbital energy level diagram for the O2+ ion.b. How many net σ and π bonds does the ion have?c. What is the O-O bond order?d. How has the bond order changed on taking away electrons from O2 to obtain O2+?e. Is the O2+ ion paramagnetic?Explain why BrF4¯ geometry is square planar while BF4¯ geometry is tetrahedral.
- The molecular geometry of the BrO 3- ion is A) trigonal planar bent c) tetrahedral T-shaped E) trigonal pyramidalConsider the following molecule: H2NCH=CH2. Which atomic orbitals overlap to form the nitrogen-carbon sigma bonding orbitals of this molecule? (Best to use my easy method to draw the structure.) skeleton H H N C C H H O Csp and Nsp O Csp? and C2p Csp? and Csp? O Csp and N2p O Csp and Csp O C2p and C2p O Csp? and Csp O Nsp and Csp2Arrange the following radicals in order of increasing stability, unut OHi, How would I find the number of unpaired electrons for O2+ from the molecular orbital diagram?In Which of the following Componds would lonic bonds be encountered ? that apply) (Circle or underline all NH 3 PC 3 co2 M gO NH y NO 3Which statements accurately describe sigma bonds? Sigma bonds can only result from the overlap of two p orbitals. Sigma bonds only form when regions of orbitals with different signs overlap. Sigma bonds are symmetric about the internuclear axis. Sigma bonds result from the overlap of orbitals in only one region of space. Sigma bonds result from the overlap of orbitals in two regions of space. Sigma bonds cannot rotate without interfering with orbital overlap. A sigma bond could result from the sideways (as opposed to head-on) overlap of two p orbitals. Sigma bonds only form when regions of orbitals with the same sign overlap.Order the following electronic orbitals from lowest (1) to highest (5) energy level. < < Pi anti-bonding Non-bonding Sigma bonding Sigma anti-bonding Pi bondingAll the following statements are true about sigma bond EXCEPT The electron density is high in the region between the two nuclei. The electron density is concentrated above and below the bond axis. The electron density is symmetrical to the bond axis. Overlapping of two s orbitals forms a sigma bond.s it possible to draw a resonance structure with the lone pair? What is the hybridization of the heteroatom? Draw a valence bond orbital diagram to show the location of the lone pair (you do not need to draw any orbitals to show s bonds). In what orbital are the electron pairs located?SEE MORE QUESTIONS