pyright The McGraw-Hill Companies, Inc. Permission required for reproduction or displaTable 10.2 Geometry of Simple Molecules and lons in Which the Central Atom Has Oneor More Lone PairsArrangement of Electron Pairs About a Central Atom (A) in aMolecule and Geometry of Some Simple Molecules and lonsin Which the Central Atom Has No Lone PairsTable 10.1Number of Arrangement ofElectron PairsGeometry ofMolecule or lonClass of Total Number ofNumber ofMoleculeElectron PairsBonding Pairs Lone PairsExamplesArrangementof ElectronPairs*Number ofMolecularGeometryElectronAB,E3.BentPairsExamplesTrigonal planarSO,180BeCl,, HgCl2B-A-BTrigonalPyramidalAB,ELinearLinearTetrahedralNH,120BF,AB,EBentTetrahedralTrigonal planarTrigonal planarDistortedletrahedron(or seesaw)109.5AB,ECH4, NH4Trigonal bipyramidalSFTetrahedralTetrahedralAB,EB-T-shapedTrigonal bipyramidalCIF,PCI5AB,E,Linear120°Trigonal bipyramidalTrigonal bipyramidalTrigonal bipyramidalambspyramidalAB,E90OctahedralBF,90-SFABESquare planarOctahedralXeF,OctahedralOctahedral"The cokwed lines are wed o how dhe overall shape, bond 8. Predict the geometries of H,S using the VSSPR method with the following stepsStep 1) Draw the skeletal structure and finish Lewis structure 2) +1o)=8e-4H-S-HStep 2: Write the general form (Abx or ABXEY):Step 3) Table number to use (10.1 or 10.2):Step 4: Predict the geometryStep 5) Determine polarity:

In the given molecule: H2S molecule Total no. Of electron pair = 4 No. Of bonding pair = 2 No. Of…

8. Predict the geometries of H,S using the VSSPR method with the following steps Step 1) Draw the skeletal structure and finish Lewis structure 2(1)+1(6):8e- H-S-H v Step 2: Write the general form (Abx or ABXEY): Step 3) Table number to use (10.1 or 10.2): Step 4: Predict the geometry Step 5) Determine polarity:

8. Predict the geometries of H,S using the VSSPR method with the following steps Step 1) Draw the skeletal structure and finish Lewis structure 2(1)+1(6):8e- H-S-H v Step 2: Write the general form (Abx or ABXEY): Step 3) Table number to use (10.1 or 10.2): Step 4: Predict the geometry Step 5) Determine polarity:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

10. a) What is the difference between electron geometry and molecular geometry? b) What is the electron geometry and molecular geometry of BeF2? c) Why is the bond angle in water less than the bond angle in ammonia? d) Is dichloromethane (CH2CI2) polar? Why or why not? #32/HB e) Show/draw the 3-dimensional representation of silicon tetrafluoride,
1.1 Define electronegativity and explain why electronegativity increases with atomic number within a period of the Periodic Table. 1.2 Describe the type of bonding that exists in F2 (g) molecule. How does this type of bonding differ from that found in the HF (g) molecule? 1.3 Define hydrogen bonding using examples. 1.4 PH3 and NH3 moleculea are the same shape but the molecules are non-polar and polar respectively. Explain why this is so. 1.5 Give an example of molecule that has a coordinate covalent bond. 1.6 Draw a Lewis structure for each of the following molecules of ions: a) HF3 b) CIO3-
= O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting deviations from ideal bond angles = (co-) anion. Consider the carbonate What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the carbon-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the carbon-oxygen bonds to be... 0 7 (choose one) X 5 3/5
Use the molecular model kit to construct the following models, and then fill in the boxes for each molecule. When possible. show a resonance Lewis structure. Use formal charge, when possible to select the best structure. Follow example for CH4 below. Formula #VES CH4 8 NH3 H₂O CO₂ Lewis Structure H H-C-H H Resonance? (Y/N) Show N Electron Group & Bond Angle Tetrahedral 109° Molecular Polar? Geometry (Y/N) tetrahedral N VSPER Sketch H H 1 109.5° H H Hybridization sp³
III. Determine the molecular geometry of the encircled atom in the following organic molecules by giving the required information in the table below: (Type your answers except for the Lewis structure. Draw the Lewis structure in a sheet of paper, scan copy or shot a picture of it and paste it next page.) LEWIS STRUCTURE ELECTRON PAIR MOLECULAR MOLECULE GEOMETRY SHAPE CH3 CH3-CH2-C=C-C-CH3 (1) CH3 (2) CH3 -(CH2), CO-CH(CH3)-CH3 (3) CH3 -(CH2)3-CO-CH(CH3)-CH3 S „WOLV VALENCE NO. OF BONDING PAIRS ON - BONDING PAIRS TOTAL ELECTRON GENERAL FORMULA BOND ANGLE HYBRID ORBITAL
SCH4U e) Draw the Lewis Structure for HS Name of Compound: g) Draw the Lewis Structure for CINO Name of Compound: Name: f) Draw the Lewis Structure for H₂O₂ 4. Indicate whether each of the bonds in the molecules in #3 are lonic, polar covalent or non-polar covalent. RbCl PF₂ Name of Compound: 5. Predict which of the bonds in the following groups is most polar. a) C-H. Si-H. Ge-H b) Sn-Br. Sn-1, Sn-F c) C-O. C-H, CIN 6. Classify the bonding in each of the following as pure covalent, polar covalent, or ionic. Rank the polar covalent bonds in order of increasing polarity. a) S d) SCI₂ b) e) F₂ f) c) SF₂
For the compound CO2 (carbon dioxide), the molecule has a ___ geometry, with a bond angle of ___ degrees. linear; 180 bent; 105 No geometry or bond angle, since CO2 is ionic rather than molecular bent; 120 linear; 105
Complete Table 3 (Remember that the values pertain to the Central atoms only. In this table, you will have more than one central atom so report more than one value, ie. 3 / 3) Table 3 Molecules with Multiple Central Atoms Molecule C2H4 H2O2. CH3OH. CH3NH2 Number of Bond Pairs / / / / Number of Lone Pairs / / / / Number of Electron Domains / / / / Molecular Geometry (Shape) / / / / Bond Angle / / / / Polar or Non-Polar Nonpolar Polar Polar Polar
Use the molecular model kit to construct the following models, and then fill in the boxes for each molecule. When possible. show a resonance Lewis structure. Use formal charge, when possible to select the best structure. Follow example for CH4 below. Formula #VES Lewis Structure H CH4 8 H C H -I H Resonance? (Y/N) Show N Electron Group & Bond Angle Tetrahedral 109° Molecular Geometry Polar? (Y/N) tetrahedral N VSPER Sketch H 1 H 109.5° H H Hybridization sp³
2. Chlorite ion, ClO,, is the conjugate base of chlorous acid and has two resonance structures. Draw both resonance structures below. Include proper resonance notation, lone pairs, and formal charges (10.4). (Hint: this is an example of a hypervalent* compound.)
7) 2 OH- H.
Each molecule listed below is formed by sharing electrons between atoms when the atoms within the molecule are bonded together. Molecule A: Cl 2 Molecule B: CCI 4 · Molecule C: NH 3 34. In the box provided in your answer booklet, draw the electron-dot (Lewis) structure for the NH 3 molecule. [1] 35. Explain why CCI 4 is classified as a nonpolar molecule. (1] 36. Explain why-NIshas stronger-intermolecular forces of attraction than Ct2. f} 37. Explain how the bonding in KCl is different from the bonding in molecules A, B, and C. [1]