BeF2 exists as a linear molecule. Which kind of hybrid orbitals does Be use in this compound?Use Orbital Diagrams to show how the orbitals are formed. (6)

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Answered: BeF2 exists as a linear molecule. Which…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.59PAE: 7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three...

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7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?
Use valence bond theory to explain the bonding in F2, HF, and CIBr. Sketch the overlap of the atomic orbitals involved in the bonds.
7.57 What observation about molecules compels us to consider the hybridization of atomic orbitals?
Lets look more closely at the process of hybridization. (a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them? (b) Do hybrid atomic orbitals form between different p orbitals without involving 5 orbitals? (c) What is the relationship between the energy of hybrid atomic orbitals and the atomic orbitals from which they are formed?
7. Nitrogen is the central atom in each of the species given. (a) Draw the Lewis electron-dot structure for each of the species. + NO₂ NO₂ NO₂ (b) List the species in order of increasing bond angle. Justify your answer. (c) For NO₂ and NO₂, give the hybridization of the nitrogen atom in it. (d) Identify the only one of the species that dimerizes and explain what causes it to do so.
9.17 (a) An AB6 molecule has no lone pairs of electrons on the Aatom. What is its molecular geometry? (b) An AB4 moleculehas two lone pairs of electrons on the A atom (in additionto the four B atoms). What is the electron-domain geometryaround the A atom? (c) For the AB4 molecule in part (b), predictthe molecular geometry.
For each of the following molecules, draw the Lewis structure, predict the molecular shape using VSEPR method, and propose the orbital hybridization on the central atom of each molecule. (a) BeF2 (b) GeF2 (c) AsCl3 (d) BrCl3 (e) GeCl4 (f) SeCl4 (g) AsCls (h) BrF5 (i) SF, (j) XeF4
(a) Determine the molecular geometry of SeF4using the VSEPR model. The molecular geometry of SeF4 is (___________________) linear or trigonal planar or bent tetrahedral or trigonal pyramidal or trigonal bipyramidal or seesaw or T-shaped or octahedral or square pyramidal or square planar . (b) Explain why the molecular geometry of SeF4 is different from that of IBr3, although they have similar electron-domain geometries. Although both SeF4 and IBr3 have the electron-domain geometry of (_________________) linear or trigonal planar or bent tetrahedral or trigonal pyramidal or trigonal bipyramidal or seesaw or T-shaped or octahedral or square pyramidal or square planar, IBr3 has _____ lone pair(s) of electrons whereas SeF4 has only ________ lone electron pair(s) in the (______________) axial or equatorial positions. Accordingly, the molecular geometry of SeF4 is (________________) linear or trigonal planar or bent tetrahedral or trigonal pyramidal or trigonal bipyramidal or seesaw or…
Give the number and type of hybrid orbital that forms when each set of atomic orbitals mixes:(a) two d, one s, and three p(b) three p and one s
Please answer these questions on your Page 3 (11) What is the hybridization of the central N atom in NO₂? N and O are in groups 5 and 6 and their atomic numbers are and 8. (12) What is the hybridization of the central I atom in IF? I and F are both in group 7 and their atomic numbers are 53 and 9. (13) What is the hybridization of the central Xe atom in XeO3? Xe and O are in groups 8 and 6 and their atomic numbers are 54 and 8. (14) There are how many o bonds and how many bonds in N3 (N.B. the molecule is not cyclic)? You must give the two correct values to get your point. N is in group 5 and its atomic number is 7. (15) Who proposed that energy is quantized?
9.8 The drawing below shows the overlap of two hybrid orbitalsto form a bond in a hydrocarbon. (a) Which of the followingtypes of bonds is being formed: (i) C¬C s, (ii) C¬C p,or (iii) C¬H s? (b) Which of the following could be theidentity of the hydrocarbon: (i) CH4, (ii) C2H6, (iii) C2H4, or(iv) C2H2? [Section 9.6]
1. For each molecular geometry, give the number of total electron pairs, the number of bonding pairs and the number of lone pairs on the central atom. (a) (b) (c) 2. For the following species provide the Lewis structure and make a 3D sketch showing estimated bond angles. Determine the polarity of each molecular and draw the dipole. a) SF4 b) KrF4 3. Determine the 3D structure of the molecule of formula C2H4O (H3CCHO). Indicate the geometry around each "central" atom and estimate bond angles. Representing Molecular Geometries on Paper X-A-X XX Linear Trigonal planar Bent Tetrahedral Trigonal pyramidal Trigonal bipyramidal Seesaw Octahedral Square planar

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BeF2 exists as a linear molecule. Which kind of hybrid orbitals does Be use in this compound? Use Orbital Diagrams to show how the orbitals are formed. (6)