Which of the following molecules are polar? XeCl2 COF2 PCl4F SF6 PCl3
Solution:
Following compounds are polar:
COF2 - COF2: C has four valence electrons uses two to bind the F atoms and two to bind O (satisfy the octet of O). The molecule is AX3 trigonal planar the C-F→ δ- vectors do not cancel (despite partial offset by O) so molecule is polar.
PCl4F- This is an AX5 system trigonal bipyramid with the F atom axial (you would not be expected to know but get same result if it goes equatorial). The P:F → δ- vector is not cancelled so the molecule is polar.
PCl3 - Chlorine is more elctronegative than phosphorus . P has a lone pair of electrons , every Cl atom has three pairs of electrons . The molecule is not symmetrical . Shared electrons tend to go nearer towards the chlorine side the chlorine atoms are shifted towards one side of the center of the molecule , and a net dipole effect is created So this molecule is polar .
Which of the following molecules are polar? XeCl2 COF2 PCl4F SF6 PCl3
How many of the following molecules are polar? xeCl2 COF2 PC4F SF6
Which of the following molecules are polar? a)BF3 b)PCl5 c)SF6 d)BeBr2 E)PCl3
of the following, XeF2, XeF4, SF6, which of these are polar molecules? a)XeF2 b) XeF4 c) SF6 d) non are polar e) all are polar please explain one by one. a typed answer is prefered.
Which of these molecules are polar? Check all that apply. PCl3 SO2 CO2 CH2Cl2
Match the following molecules with the correct molecular geometry. (some might be used more than once, and others may not be used at all)Answer..... XeCl2..... COF2..... PCl4F..... SF6..... C2Br2..... SiF4..... SF4Answers:A. See-SawB. LinearC. TetrahedralD. BentE. Trigonal BipyramidalF. Trigonal PyramidalG. Trigonal PlanarH. Octahedral
which molecules on the image are polar? chack all that apply -CH2Cl2 -SO2 -CO2 -PCl3 O Which molecules on the image are polar? Check all that apply. CH,C1, so, CO2 PCI about us Careers terms of use contact us
Arrange the following molecules by increasing bond polarity. ( least polar to most polar) 1. PCl3 2. CCl4 3. CaCl2 4. CsCl 5. Cl2
Consider the molecule below Determine the electron geometry at each of the 3 labeled atoms. 1=trigonal planar. 2=tetrahedral. 3=tetrahedral 1=trigonal planar. 2=trigonal pyramidal. 3=trigonal pyramidal 1=tetrahedral. 2=tetrahedral, 3=trigonal planar 1 =tetrahedral. 2=tetrahedral, 3=tetrahedral 1=bent. 2=tetrahedral. 3=trigonal pyramidal Which is expected to have the largest London forces? F2 CnHx BeCb C3H5 How many of the following molecules are polar? XeCl2 COF2 PCl4F SF6 3 2 1 0 4
What is the electronic and molecular geometry of the following molecules? (i) PCl3 electron domain: molecular domain: (ii) CCl4 electron domain: molecular domain: (iii) XeF4 electron domain: molecular domain: (iv) SF6 electron domain: molecular domain:
Which of the following contains polar covalent bonds? Select one: N2 PCl3 Na2O MgO