Given these electronegativities, predict which type of bond will form between the 2 atoms listed: H. He 2.20 Li Be N Ne 0.98 1.57 2.04 2.55 3.04 3.44 3.98 Na Mg Al Si CI Ar 0.93 1.31 1.61 1.90 2.19 2.58 3.16 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 0.82 1.00 1.36 1.54 1.63 1.66 1.55 1.83 1.88 1.91 1.90 1.65 1.81 2.01 2.18 2.55 2.96 3.00 To H-CI A. Polar Covalent В. H-H Nonpolar covalent C. Jonic O-0 Li - CI
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- Give approximate values for the indicated bond angles in thefollowing molecules:Using BEST Lewis structures and the VSEPR model, match each molecular formula with the molecular geometry that describes it.The structure of borazine, B3N3H6, is a six-membered ringof alternating B and N atoms. There is one H atom bondedto each B and to each N atom. The molecule is planar.(a) Write a Lewis structure for borazine in which the formalcharge on every atom is zero. (b) Write a Lewis structurefor borazine in which the octet rule is satisfied forevery atom. (c) What are the formal charges on the atomsin the Lewis structure from part (b)? Given the electronegativitiesof B and N, do the formal charges seem favorableor unfavorable? (d) Do either of the Lewis structuresin parts (a) and (b) have multiple resonance structures?(e) What are the hybridizations at the B and N atoms inthe Lewis structures from parts (a) and (b)? Would you expectthe molecule to be planar for both Lewis structures?(f) The six B¬N bonds in the borazine molecule are allidentical in length at 1.44 Å. Typical values for the bondlengths of B¬N single and double bonds are 1.51 Å and1.31 A°, respectively. Does the value of the B¬N…
- Which statement best captures the fundamental idea behind VSEPR theory? Explain what is wrong with the statements you do not choose. a. The angle between two or more bonds is determined primarily by the repulsions between the electrons within those bonds and other (lone pair) electrons on the central atom of a molecule. Each of these electron groups (bonding electrons or lone pair electrons) lowers its potential energy by maximizing its separation from other electron groups, thus determining the geometry of the molecule. b. The angle between two or more bonds is determined primarily by the repulsions between the electrons within those bonds. Each of these bonding electrons lowers its potential energy by maximizing its separation from other electron groups, thus determining the geometry of the molecule. c. The geometry of a molecule is determined by the shapes of the overlapping orbitals that form the chemical bonds. Therefore, to determine the geometry of a molecule, you must determine…Calculate the number of shared electrons(S), using the formulaS = N –AWhere N= total no of valence electrons needed by all atoms in the moleculeA= total no of valence electrons available in each atom (remember to add electronsfor negatively charged ions and subtract electrons for positively charged ion, Draw the Lewis Dot formula, Determine the electronic geometry of the central atom, Sketch the geometry around the central atom AND Describe the geometry for the following: NH3 NH4+ PCl6-Which of the following electron configuration pairs would most likely result in covalent bonding? A. 1s2 2s2 2p5 and 1s2 2s2 2p6 B. 1s2 2s2 2p5 and 1s2 2s2 2p5 C. 1s2 2s2 and [Ar] 4s1 D. [Ne] 3s1 and [Ne] 3s1
- Determine the magnitude of the positive and negative charges on each atom for the following. OF2: bond angle 103.1 degrees, bond length 1.405 A, dipole moment 0.297 D SF2: bond angle 98.1 degrees, bond length 1.587 A, dipole moment 1.050 D Rationalize your answers above using concepts of electronegativity.Find the molecule that does not follow octet principle. PF3 NF3 NH3 BCl3Represent the bonding in SF2 (F-S-F) with Lewis diagrams. Include the formal charges on all atoms. The dimerof this compound has the formula S2F4. It was isolated in1980 and shown to have the structure F3S-SF. Draw apossible Lewis diagram to represent the bonding in thedimer, indicating the formal charges on all atoms. Is it possible to draw a Lewis diagram for S2F4 in which all atomshave valence octets? Explain why or why not
- Write Lewis structures that obey the octet rule for each of the following molecules and ions. (In each case the first atom listed is the central atom.) a. POCl3, SO42-, XeO4, PO43-, ClO4- b. NF3, SO32-, PO33-.Cl3- c. ClO2-, SCl2, PCl2- d. Considering your answers to part a, b, and c, what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons?Draw out Lewis Structures for CO2 and H2O.Using VSEPR Theory make models to represent the two molecules [you do not have to showdouble bonds in your model].From your answer predict the shape of CS2 and H2S. Looking at the Periodic Table predict which of the following molecules will have the sameshape. Using VSEPR theory determine what that shape will be.NCl3 PF3 AlCl3 BrF3Explain lectronegativity and Bond Polarity?