Predict the electron pair geometry and molecular geometry for the following substances by drawing their Lewis structures. Also state if each substance is polar or nonpolar. a) BH3. i) Lewis Structure: b) H₂O ii) Electron pair Geometry: iii) Molecular Geometry: iv) Polar or Nonpolar:
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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!20) For carbon disulfide (toxic, malodorous, flammable liquid) and selenium disulfide (solid, melting point 111oC, over-the-counter drug used to treat certain types of dermatitis) a) compile their Lewis electron dot formulas b) identify their electron pair geometry according to the VSEPR theory, c) determine which of these two molecules is polar and which is non-polar and shortly explain whyWhich of the following statements is/are true about the Lewis bond theory? (a) It explains the stability of the molecule. (b) It explains why one covalent bond might differ from another. (c) It ignores the energy changes in chemical bond formation. (d) It treats all covalent bond in the same manner. a and b O b and c O c and d a and d
- 10. Each ball-and-stick model below shows the electron-pair and molecular geometry of a generic molecule. Explain what is wrong with each molecular geometry and provide the correct molecular geometry based on the number of lone and bonding pairs around the central atom. (a) (b) (c) 11. Draw the Lewis structure for acetamide (CH3CONH2) and determine the geometry about each interior atom. Experiments show that the geometry about the N atom in acetamide is nearly planar. Draw a resonance structure that can account for the planar geometry about the N atom.Hyrbridi- Molecular polarity Formula Lewis structure Total # of Electron group Molecular Valence geometry geometry zatiom Electrons BF3 CO32- CH4 SCl,Determine the electron and molecular geometries of each molecule. For molecules with two central atoms, indicate the geometry about each central atom.(a) N2(b) N2H2 (skeletal structure HNNH)(c) N2H4 (skeletal structure H2NNH2)
- 2. Consider the following molecules or ions: CIOF5, NOBr, NH2F, and XeO2F3+. Answer the following questions based on the Lewis structures and VSEPR theory prediction of their molecular shapes. (a) Which one has only bond angles of 109.5°? (b) Which one has only bond angles of 120°? (c) Which one has bond angles of 90 and 180°? (d) Which one has bond angles of 90, 120, and 180°?For each molecule or ion, determine the preferred Lewis structure and use it to predict the molecular shape and bond angles. a) H3O+ b) XeF2 c) I3- d) SNF3 (S central atom) e) POCl3 f) PF34. What will be the geometry about each central atom in the following molecules? Draw a sketch of the molecule. The skeletal structure for each molecule is listed in parentheses. a) C₂H₂ (HCCH) c) CH,NH, (H,CNH,) b) N₂H (H₂NNH₂) d) CF,COOH (both O atoms are attached to the second C, H atom is attached to O)
- Determine the approximate bond angles in the following ions and molecules approx. 180 аpprox. 120 No Answers Chosen No Answers Chosen approx. 109.5 аpprax, 90 No Answers Chosen No Answers Chosen mix of 120 and 9o No Answers Chosen Possible answers | (SCNJ- (C: central atom) I (NO3)- (N: central atom) I (PO3]3- (P: central atom) I SF4 (S: central atom)Part A) Draw the following lewis structures and give the formal charges for the atoms as well as the number of valence electrons I2 Part B)According to VSEPR theory, why are bonds and lone pairs spaced as far apart as possible? Part C)Why can we ignore the disposition of the lone pairs on terminal atoms? Part D)What are the bond angles for a molecule having an octahedral electronic geometry with two lone pairs and four bonds on the central atom?1) A) In the Lewis structure for IF2–, how many lone pairs of electrons are around the central iodine atom?a) 0b) 1c) 2d) 3e) 4B) The Cl–Xe–Cl bond angle in XeCl4 is closest toa) 90°b) 120°c) 150°d) 360°e) 109°C) Which of the following atoms cannot exceed the octet rule in a molecule?a) Bb) Snc) Pdd) Ie) All atoms exceed the octet rule