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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?Sigma Bonding Ao bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH4 1s orbital What atomic or hybrid orbitals make up the sigma bond between C, and C, in propyne, CHCCH3 ? (C, is the second carbon in the structure as written.) orbital on C2 + orbital on C What is the approximate C,-C2-C, bond angle ?4. Valence Bond Theory. Consider formaldehyde, H₂CO. ( a) Draw a Lewis structure of formaldehyde. b) Draw a picture using valence bond theory showing the bonding of formaldehyde using appropriate hybrid orbitals. (Include electrons) c) Describe the bonding of the C-O bond and C-H bond by listing the bond type (σ, π) and the orbitals contributing to the bonding. C-O: C-H:
- ar moiecuie 2. CHCI, Steric Number= 3-D Sketch (use wedges and dashes as appropriate) BALPA= :ci-c-CI: Bond angle(s) | Shape = Hybridization #o bonds = #n bonds = Y Polar molecule? Circle one:3. For each of the following compounds, indicate the total number of valence electrons - VE, draw the Lewis structure(s), calculate the bond order - BO- of the central ion, calculate the formal charge of each atom in the molecule, and determine the hybridization of the central ion. Show the formal charges in () to the upper right of each atom, then put the bond order and central atom hybridization (CAH - Ex. sp) on the lines provided. Under the structure (resonance structures if the molecule has them), name the general and specific shapes of the molecule. a) BF3 in novaw VE = b) XeF4 c) SO3 General Shape (Electron Domain Geometry) = Specific Shape (Molecular Geometry) = d) SO3²- (latot) 9V General Shape (Electron Domain Geometry) = Specific Shape (Molecular Geometry) = noi General Shape (Electron Domain Geometry)=niku (1) Specific Shape (Molecular Geometry) = Syriw bo sidodong pnom srit ai esutaunta General Shape (Electron Domain Geometry) = Specific Shape (Molecular Geometry) = BO =…Draw the following molecule and answer the questions below. H3CCHCHC(O)CH2CCH What is the hybridization/bonding orbital of each bolded atom? What is the hybridization of each bonded atom?
- Sigma Bonding AG bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH4 1s orbital What atomic or hybrid orbitals make up the sigma bond between C, and O, in acetic acid, CH3COOH ? (C, is the second carbon in the structure as written.) orbital on C, + orbital on O1 What is the approximate C1-C2-O1 bond angle ?Determine the hybridization of the marked N atom in tofacitinib, a drug used to treat rheumatoid arthritis. In what type of orbital does the lone pair on this N atom reside? (Lone pairs have been omitted in this structure.) N. N, NEC. N tofacitinib N' sp hybridized; sp orbital sp hybridized; sp° orbital 3. sp° hybridized; p orbital sp hybridized; sp² orbital sp hybridized; p orbital 3DSigma Bonding Ao bond arises from the straight-on overlap of two atomic orbitals. The electron density lies along the axis of the two bonded nuclei. sp3 hybrid orbital Example: Sigma Bonding in methane, CH4 1s orbital What atomic or hybrid orbitals make up the sigma bond between C, and O in acetaldehyde, CH3CHO ? (C, is the second carbon in the structure as written.) orbital on C, + orbital on O What is the approximate C,-C2-O bond angle ?
- Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. Determine the hybridization around C1, C2 and oxygen atoms. What is the expected bond angle around C1, and C2 atoms? Identify the type of bonds (σ or π) and the overlapping orbitals that form bonds A, B, and C.Number 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 904. Silicon is an interesting atom because it behaves similarly to carbon. There is speculation in the scientific field that aliens could be made of silicon structures rather than carbon. The following structures are silicon versions of important carbon signaling molecules in our body. 1.) What is the electron geometry and hybridization for each of these structures? H-Si-H H-H Silane Silanone Silicon Dioxide e geometry: e geometry: hybridization: e geometry: hybridization: hybridization: 2.) Based on what you have described above, match the orbital diagram below with the correct molecule above:SEE MORE QUESTIONS