1. Complete the following table:
Substance | Lewis Structure | Predicted Molecular geometry | Bond Angles | Polar Bonds | Molecular Polarity | Resonance (if any) |
SO2 | ||||||
BF3 | ||||||
NF3 |
2. Complete the following table:
pH | pOH | [H3O+] | Acidic or Basic |
6.88 | |||
8.4 x 10-14 | |||
3.11 | |||
1.0 x 10-7 |
Ans 1 :
The molecular geometry of the molecules can be determined on the basis of VSEPR theory. The bonds are polar if they have considerable difference in their electrnegativity values.
If the dipole moment of all the bonds do not cancel out , the molecule becomes polar.
So here :
Substance |
predicted molecular geometry |
Bond angles |
Polar bonds |
Molecular polarity |
Resonance (if any) |
SO2 | bent | 120o | polar | polar | 2 resonance structures |
BF3 | trigonal planar | 120o | polar | non-polar | 2 resonance structures |
NF3 | trigonal pyramidal | 102.1o | polar | polar | no |
Lewis structures of the molecules are shown below ...
1. Complete the following table: Substance Lewis Structure Predicted Molecular geometry Bond Angles Polar Bonds Molec...
molecule lewis structure electron geometry molecular geometry bond angles polar or non polar #valenceelectrons I3^- SO2 IF4^- ICl4^- CO3^2- AsF5 PF6^- IF3 XeCl2
Compound Lewis Structure Total Valence Electrons Electron Pair SO Molecular Geometry Approximate Polar? Geometry Bond Angles 24 trigona! planar trigonal planar HCN H-CEN SO2 CS2 1- C-H tethredral tethredral -
Complete the following table: # of valence Molecule Lewis Structure Electronic geometry Polar or Nonpolar # of Lone Pairs Shape of the molecule (name) (Por NP) SiH, PH HS H Se CHO BF3
Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles NF3 2Le -NIF TrigonalPlanar 120 SCI2 20 CI-S-CI Linear HCIO CClA -C-ciTetre hudra 32 CH3NH2 (Both C and N) H-N-H H2CO
Compound Total Valence Lewis Structure Electron Pair Molecular Approximate Polar? Electrons Geometry Geometry Bond Angles
Substance H202 NF: CS Lewis structures Number of bonding groups Complete the following table for the twenty molecules and polyatomic ions listed. Results should be checked with other students in the class or the appropriate Chapters in the text. Number of lone pairs Number of electron groups about the central atom Electron geometry Molecular geometry Approximate bond angles Polarity of molecule or ion Number of resonance structures Hybridization state about the central atom
180 No. of Molecule or Polyatomie lon Valence Electrons Lewis Structure Molecular Geometry Bond Angles Bond Polarity Molecular Dipole or Nonpolar Te amedral C.H.CI, H: 2 a = 14 109.5 lete polar S: triangular 107 S- SO, 410 nonpolar Botter Dobar 3270317 27 est (= 4 I ITO CHO Ic=0 bent 119 polar - 157 F-O-Ect 0= 6 bent 104.5 OF, F = 14 TOT polar 20 N=5 NO; Linear 180 polar |0=12 anion Unear 1800 Nonpolar 1 - 0...
Substance Lewis Structure Electronic Geometry Bond Angle Molecular Geometry BeBrz Polar/Nonpolar Hybridization BP + LP OF tetrahedral bent BP + LP IF BP + LP AICI: BP + LP XeFz BP + LP
Complete the following table for Sulfur Hexafluoride!
Electron Geometry: 1 Molecular Geometry: bi tudod Sulfur hexafluoride Lewis Structure VSEPR Drawing mollo Brusos AEN: Around Central Atom (DIO HISTS Single Bonds: og e-groups = Double Bonds: =BUOTE Overall Polarity: ity:bro slanti Polar Non Polar Triple Bonds: Angles: sebno slain Lone Pairs: aneleno
Substance SO, Lewis Structure Electronic Geometry Hybridization Molecular Geometry Bond Angle Polar/Nonpolar BP + LP NO, AP H.CO ТААР REF Treat as the centralatom BP CHCI BP + LP Ich ВР. + LP 5