![]() Hence, it is s p 3 d hybridised and has trigonal bipyramidal shape. ![]() It has two types of dipole moment vectors which cannot cancel out each other and hence it is polar in nature i.e. Hence, it is s p 3 hybridised and has trigonal pyramidal shape. (c) In P F 3, P has three σ bonds and one lone pair. The resultant of the two dipole moment vectors cancel out with the third dipole moment vector as the bond angle is 120 ∘. All the dipole moment vectors cancel out each other. Due to this lone pair, the shape of the molecule comes out to be square pyramidal and the dipole moment does not get canceled out. Therefore, S i F 4 is s p 3 hybridised and has a tetrahedral shape. JEE Main 2022 Question Paper Live Discussion.Difference Between Selling And Marketing.TS Grewal Solutions Class 11 Accountancy.TS Grewal Solutions Class 12 Accountancy.CBSE Previous Year Question Papers Class 12.CBSE Previous Year Question Papers Class 10.NCERT Solutions For Class 6 Social Science.NCERT Solutions for Class 7 Social Science.NCERT Solutions for Class 8 Social Science.Can you explain this answer? tests, examples and also practice Chemistry tests. Can you explain this answer? theory, EduRev gives you anĪmple number of questions to practice Which of the following molecules will have a permanent dipole moment?a)SiF4b)XeF4c)SF4d)BF3Correct answer is option 'C'. Can you explain this answer? has been provided alongside types of Which of the following molecules will have a permanent dipole moment?a)SiF4b)XeF4c)SF4d)BF3Correct answer is option 'C'. Can you explain this answer?, a detailed solution for Which of the following molecules will have a permanent dipole moment?a)SiF4b)XeF4c)SF4d)BF3Correct answer is option 'C'. Which of the following molecules will have a permanent dipole moment?a)SiF4b)XeF4c)SF4d)BF3Correct answer is option 'C'. Can you explain this answer? defined & explained in the simplest way possible. Here you can find the meaning of Which of the following molecules will have a permanent dipole moment?a)SiF4b)XeF4c)SF4d)BF3Correct answer is option 'C'. Hence, the correct answer is option 'C' SF4. ![]() However, the molecule is symmetrical and the dipole moments of the bonds cancel out each other, resulting in no net dipole moment. The lone pair creates an asymmetric distribution of electron density and breaks the symmetry of the molecule, resulting in a net dipole moment.ĭ) BF3 - Boron trifluoride has a trigonal planar geometry with three polar B-F bonds. Hence, XeF4 has no net dipole moment.Ĭ) SF4 - Sulfur tetrafluoride has a trigonal bipyramidal geometry with four polar S-F bonds and one lone pair of electrons on sulfur. Similar to SiF4, the dipole moments of these bonds cancel out each other due to the symmetry of the molecule. Hence, SiF4 has no net dipole moment.ī) XeF4 - Xenon tetrafluoride has a square planar geometry with four polar Xe-F bonds. However, the dipole moments of these bonds cancel out each other due to the symmetry of the molecule. The magnitude of the dipole moment depends on the electronegativity difference and the bond length.Ī) SiF4 - Silicon tetrafluoride has a tetrahedral geometry with four polar Si-F bonds. ![]() Due to the difference in electronegativity, the electron density in the bond shifts towards the more electronegative atom, making it partially negative and the other atom partially positive. A polar bond is formed when two atoms of different electronegativity are bonded together. Permanent dipole moment arises due to the presence of polar bonds in a molecule. ![]()
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