Chemical Bonding and Molecular Structure
Get insights from 189 questions on Chemical Bonding and Molecular Structure, answered by students, alumni, and experts. You may also ask and answer any question you like about Chemical Bonding and Molecular Structure
Follow Ask QuestionQuestions
Discussions
Active Users
Followers
New answer posted
4 months agoContributor-Level 10
4.29 (c) It will not form a sigma bond because taking x-axis as the inter-nuclear axis, there will be lateral overlap between the two 2py orbitals forming a -bond.
New answer posted
4 months agoContributor-Level 10
4.28. (a) Acetylene C2? H2? contains 3? bonds and 2? bonds.
(b) Ethylene C2? H4? contains 5? bonds and 1? bond.
New question posted
4 months agoNew answer posted
4 months agoContributor-Level 10
4.26. In BF3, B atom is sp2 hybridised. In NH3, N is sp3 hybridised.
After the reaction, hybridisation of B changes from sp2 to sp3, while the hybridisation of N remains the same.
New answer posted
4 months agoContributor-Level 10
4.25. Electronic configuration of 13Al in ground state= 1s2 2s2 2p6 3s2 3p1
Electronic configuration of 13Al in excited state = 1s2 2s2 2p6 3s1 3px13py1
Hence, hybridisation will be sp2 and this makes the geometry to be Trigonal planar (in case of AlCl3).
In AlCl–4, the empty 3pz orbital is also involved. So, the hybridisation is sp3 and the shape is tetrahedral
New answer posted
4 months agoContributor-Level 10
4.24. Hybridisation: It is defined as the process of intermixing of atomic orbitals of slightly different energies to give rise to new hybridized orbitals having equivalent energy and identical shapes.
Shapes of Orbitals:
sp hybridisation: When one s-and one p-orbital intermix then it is called sp-hybridisation. For example, in BeF2, Be atom undergoes sp-hybridisation. It has linear shape. Bond angle is 180°.
sp2 hybridisation: One s-and two p-orbitals get hybridised to form three equivalent hybrid orbitals. The three hybrid orbitals directed towards three corners of an equilateral triangle. It is, therefore, kno
New answer posted
4 months agoContributor-Level 10
4.23. The dipole moment of NH3 (1.47D) is higher than the dipole moment of NF3 (0.24D), even though the molecular geometry is pyramidal for both the molecules. In each molecule, N atom has one lone pair. F is more electronegative than H and N? F bond is more polar than N? H bond. Hence, NF3? is expected to have much larger dipole moment than NH3. However, reverse is true. In case of ammonia, the direction of the lone pair dipole moment and the bond pair dipole moment is same whereas in case of NF3, it is opposite. Thus, in ammonia molecule, individual dipole moment vectors add whereas in NF3, they cancel each other.
New answer posted
4 months agoContributor-Level 10
4.22. BeH2is a linear molecular (H—Be—H), the bond angle = 180°. Be—H bonds are polar due to difference in their electronegativity but the bond polarities cancel each other. Thus, molecule has resultant dipole moment of zero
New answer posted
4 months agoContributor-Level 10
4.21. According to VSEPR theory, if CH4 were square planar, the bond angle would be 90°. For tetrahedral structure, the bond angle is 109°28? Therefore, in square planar structure, repulsion between bond pairs would be more and thus the stability will be less.
Moreover, the orbitals of carbon in ground and excited states look as shown below. In the excited state, the electrons from 4 H atoms occupy one 2s orbital and three 2p orbitals. This results in an sp3 hybridisation, which is the hybridisation of a tetrahedral geometry
New question posted
4 months ago
Taking an Exam? Selecting a College?
Get authentic answers from experts, students and alumni that you won't find anywhere else
Sign Up on ShikshaOn Shiksha, get access to
- 65k Colleges
- 1.2k Exams
- 688k Reviews
- 1800k Answers