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- Consider the following flat drawing of methane (CH4) . a. What is HCH bond angle implied by this drawing if you assume it is flat? b. Are the electron domains of this flat CH4 spread out as much as possible? c. Use model materials to make a model of CH4 (methane). If you assembled it correctly, thefour bonds (bonding electron domains) of your model will be 109.5° apart. d. In which representation, the drawing above or the model in your hand (circle one) are theH’s of CH4 more spread out around the central carbon? e. Confirm that your model looks like the following drawing. The wedgebond represents a bond coming out of the page, and the dash bondrepresents a bond going into the page f. You will often see methane drawn as if it were flat (like on the previous page). Why is thismisleading, and what is left to the viewer’s imagination when looking at such a drawing?1. Complete the following table. Molecular Formula Atom a b C C₂H4O 2. Use the Lewis structure below to complete the following table. d H b Lewis Structure H a H H-C-C C-H H-C-O: H Electron Geometry Line-Angle Structure H H :O: H C ||||-- H H C CC H d Hybridization to 3. Identify the functional groups in the Lewis structure from question #2. Approx. Bond AngleNumber of lone pairs of electrons associated with central atom (LP) Lewis Structure Diagram Number of electron groups associated with the central atom (EG) Molecular shape (MS) Bond angle(s) Hybridization Number of sigma bonds (0) -- Single Bond Number of bonds (π) -- Double bonds/Triple bonds Overall dipole (yes/no ---- if yes, include below) 3D drawing (VSEPR SHAPE) XeF4 PCI, SO₂
- 3. Predict (a) the approximate bond angle, (b) the hybridization around the indicated atoms (the atoms to which the arrows are drawn in the structures below). Write your answers near the corresponding labels (1 to 5) in the drawings. (Note: the lone pairs on the F atoms are omitted for clarity.) H. 1 F 2 4 F Br -F С -о-н F F 'N : 1: 2: 3: 4: 5:1. Ethanol, C,H,0 (CH,CH,OH) Lewis structure using dots to represent bonding electrons: Lewis structure using lines to represent pairs of bonding electrons: Label the carbon bonded to only hydrogen and other carbon atom as carbon A, and the other carbon atom as carbon B. Carbon atom A: Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Carbon atom B: Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Oxygen atom Total number of electron groups: Number of lone pairs: Number of bonding groups/pairs: Bond angles: Electron geometry: Molecular geometry: Hybridization: Number of hybrid orbitals: Is this molecule polar? (Y/N) Can this molecule hydrogen bond with itself? Number of sigma bonds: Number of pi bonds: MacBook Pro2. Complete the table for the indicated compounds Molecule C2H2 SF5- NO3- Lewis structure include lone pairs & formal charges on each atom Resonance structures don't have to include lone pairs; write N/A if there are none Electron Geometry Hybridization on central atom Overlapping orbitals include value of n in the orbital name (e.g. 1s, not s). Write N/A if that kind of bond is not present in the molecule T: Molecular Geometry Bond angle(s) include < as necessary 3D structure and polarity don't have to include lone pairs; draw the |dipole arrow on the molecule or write "non- polar"
- Answer the following questions regarding the Lewis structure of P002. Blank #1: The polonium atom uses a oxygen atoms. Blank #2: The oxygen atoms use a polonium atom. Blank #3: The arrangement of electron groups around the selenium atom is Blank #4: There is a delocalized pi-bond between the polonium atom and both oxygen atoms formed by the overlap of on all three atoms. Blank # 1 Blank # 2 Blank # 3 hybrid orbitals to make a sigma bond with the hybrid orbital to make a sigma bond with the Blank # 4 A/ A P AComplete the data table shown below. Fill in the table as you draw your molecules as in the following example. Molecule Lewis Structure Electron Molecular Hybridization Molecular Or ion Geometry Geometry of Central atom polarity H20 H---O---H Tetrahedral bent sp3 polar CHA BH3 CH2B12 NH3 H30* H2O2 CHẠO [CIO3] Na2SO4 SO2 CO2 C2H4 NH4* PCISONDING Counting sigma and pi bonds in a small molecule Answer the questions below about the highlighted atom in this Lewis structure: H H | | + H- | | H H •C-C-C=N: In how many sigma bonds does the highlighted atom participate? In how many pi bonds does the highlighted atom participate? What is the orbital hybridization of the highlighted atom? 0 0 0 X 1/5
- 11. Arrange the following compounds in order of increasing bolling polnt. CHO -CHCHO -CHCH CHCHLCH CHo A D hinh >_>_lowest 12. Arrange the following compounds in order of increasing melting point. .. HO CH OH A highest>_>_>_>_lowest 13. For the following molecule: Draw the Lewis Structure, show the molecular geometry around the central atoms, hybridizations, and approximate bond angles Molecular Geometry around Central Atom hybridi- zation bond angle F,CHNCO KFCN = CNC =Table 2: Complete this table with your partner. You may ask the instructor to check your work. Formula Lewis structure Molecular geometry around central atoms(s) and name Polar or nonpolar, Draw dipole arrow Hybridization of each atom Orbitals involved in each bond XeCl2 CIF CH;CN SEF3 SF,Cl2 of each atom y dipole arrowNumber of Molecule valence electrons Formal Charge Electron-Group Geometry Molecular Geometry Resonance IBR3 I: Select one .. I: Select one .. No Where are the lone-pair electrons on the central atom located? O axial O equatorial O there are no lone pairs PFA P: Trigonal Bipyramidal v P: Distorted tetrahedral (see-saw) P: -1 No Where are the lone-pair electrons on the central atom located? O axial O equatorial O there are no lone pairs AtCl3 At: 0 At: Select one ... At: Select one .. No Where are the lone-pair electrons on the central atom located? O axial O equatorial O there are no lone pairs AtO2Br At: 0 At: Select one . At: Select one .. No What is the O-At-O bond angle? O 90SEE MORE QUESTIONSRecommended textbooks for youOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage LearningOrganic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage LearningOrganic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning