CO in high concentration is fatal in less than 5 mins !! The worst part is that this is an odorless and colorless gas and

CO in high concentration is fatal in less than 5 mins !! The worst part is that this is an odorless and colorless gas and
From this post onwards, we shall study some examples and learn how bonds are formed between two different atoms. Hydrogen fluoride (HF) – We
With this post we start discussing MOT theory for diatomic heteronuclear molecules – molecules formed by two different atoms. The MO diagrams for heteronuclear atoms
Fluorine molecule (F2) – F (9) 1s2 2s2 2p5 Two fluorine atoms bring 7 electrons each to the table and thus the 10 electrons get arranged
Nitrogen molecule (N3) – N (7) 1s2 2s2 2p3 When we construct the MO diagram for nitrogen , we will only draw the valence 2s and
Helium molecule (He2) – He (2) – 1s2. Helium has two electrons in the 1s orbital. Thus, when we draw the MO diagram, two electrons
Pi Symmetry Orbitals with pi symmetry are NOT symmetric w.r.t to the internuclear axis. When rotated around the axis, they produce a phase change (which
Overlaps & Symmetry Based on how the bonds are formed, the interaction between two AOs can have following symmetry- i) Sigma (σ) ii) Pi (π
SYMMETRY OF MOLECULAR ORBITALS. Based on symmetry ,the orbitals can be classified as – GERADE MOs and UNGERADE MOs. Gerade MOs ⇒ Gerade = Even
In this post we shall begin by constructing MO diagrams. We shall begin with the simplest of all homonuclear diatomic molecules – The H2 molecule.
We have seen in the periodic table series , that the electronic configuration tells us where exactly the electron is. Configuration means order… so
LINEAR COMBINATION OF ATOMIC ORBITALS (LCAO approximation) MOT is incorporated in quantum mechanics. As we have already discussed that classical physics (physics
Molecular orbital theory (MOT). This theory assumes that the electrons ,shared between the atoms, are spread throughout the molecule i.e they are NOT
Molecular orbital theory(MOT) is a quantum mechanical approach to bonding.Thus, this theory considers an orbital as a wave function(ψ).In order to understand MOT , it
Q: Which of the following statements for bond angles (θ) in CH4 and CH2F2 molecules is true – A] θ CH4 > θ CH2F2 B] θ CH4 < θ CH2F2 C] θ
Q: Why does PCl5 exists but NCl5 does not? A. Ionization energy of N is very high B.N does not have vacant d- orbitals C.It does not
THE DRAGO RULE. Drago rule states that , if – the central atom has at least one lone pair of electron on it the central
In this post, we will study yet another rule ,which is important while studying hybridization in molecules. This rule was stated to explain certain observations
How compounds exist in solid state ? Compounds exist as ions in solid state. Consider the following example – PCl5 molecule – This molecule has
Example 3 – PCl3F2 molecule . This molecule has TBP geometry with two F atoms and three Cl atoms as substituents.According to Bent’s rule –
After having learnt the statement of Bent’s rule in the earlier post , let us now study the rule with some examples. We know that bond angle(θ) ∝
In this post we are going to learn a comparatively new rule, proposed by Henry Bent.Henry Bent (1926-2015) was an American physical chemist who
We have already studied that the angle between the central and terminal atoms of a molecule is called as a bond angle.In this post we
In the last post, we have seen that the bond angles (θ) , hybridization index (i) and the fraction of s and p character in
Molecules with hybrid orbitals can be of two types – A] Symmetric molecules where all bonds are same.e.g.- CH4 molecule , where all bonds are C-H
After studying all types of hybridizations, we now delve deeper into this theory and learn various cardinal concepts related to it in detail. It
Sp3d3 hybridization The process of mixing of one s- orbital ,three p- orbitals and three d-orbitals in an atom to form seven sp3 d3 hybrid orbitals of equivalent
sp3d2 hybridization. The process of mixing of one s- orbital ,three p- orbitals and two d-orbital in an atom to form six sp3 d2 hybrid orbitals of equivalent energy is called sp3 d2 hybridization. EXAMPLE – SULPHUR HEXACHLORIDE (SF6) In the last post we studied the hybridization in SF4 molecule. The central sulphur atom was sp3d hybridized. It had a lone pair of electrons. […]
In the last few posts we studied about the most common types of hybridization namely –sp3, sp2 and sp hybridization. These are exhibited predominantly by
The Valence bond theory (VBT) is one of the theories which explains the formation of the covalent bond. It is based on the assumption that