To figure out the answer to this question, it is important to determine and compare the electronegativity values of all the participating atoms. This does not lead to separation of charges and the molecule remains in a stable state with no intention to bond with other nearby atoms, under normal conditions. On the other hand, non-polar molecules are those where the electronegativity difference between the participating molecules is not much and almost negligible. Polar molecules are those where the electronegativity difference between the two participating atoms is huge which leads to the separation of charges.ĭue to this, one end withholds a positive charge whereas the other one acquires a negative charge. Is Chloromethane (CH3Cl) Polar or Non-Polar? Moreover, no distortion in the structure occurs as there is no lone pair in the CH3Cl molecule because of which each bond is of equal angle and present at equal distance from one another as all the single bonds are contributing to equal repulsion.īelow is the 3D representation of the CH3Cl molecule. The molecular geometry of a molecule can be studied with the help of the Valence Shell Electron Pair Repulsion (VSEPR) theory which says chloromethane (CH3Cl) has a tetrahedral shape as the bond angle is 109.5° with the Carbon (C), always as the central atom. The CH3Cl is a Penta atomic molecule with a bond angle of 109.5° which gives the molecule a bent shape. Step 5: Now draw the Lewis diagram assembling the aforementioned steps. Step 4: Look for the number and type of bond-forming in a CH3Cl molecule: In the case of Ch3Cl, only single covalent bonds are forming between the participating atoms. Step 3: Figure out how many more electrons are required to stabilize one CH3Cl molecule: One CH3Cl molecule needs 8 more electrons to stabilize its structure completely. In the case of CH3Cl, the total number of valence electrons will be 14. Step 2: Figure out the total number of participating valence electrons: This will be figured by adding up the valence electrons of all the atoms. As the Carbon (C) atom has a lower value, so it will be the central atom. In the case of CH3Cl, there are only two single atoms C and Cl, where their electronegativity values are 2.6 and 3.2. Step 1: Find the central atom: Usually, single-atom with the least electronegativity becomes the central atom. Now, let us study the step-by-step method for drawing the Lewis structure of Chloromethane (CH3Cl). So, the number of valence electrons in the outermost shell for Chlorine (Cl) is 7. Lastly for Chlorine (Cl), the atomic number is 17 where its electronic configuration is 1s2 2s2 2p6 3s2 3p5. This makes the number of valence electrons in one Carbon (C) 4. In the case of Carbon (C), its atomic number is 6, so the electronic configuration is 1s2 2s2 2p2. As the s shell needs two electrons, there is a vacancy of one electron, so the number of valence electrons in one Hydrogen (H) atom is 1. The atomic number of Hydrogen (H) is 1, so its electronic configuration is 1s1. To begin with the Lewis structure of CH3Cl, first, we need to determine the electronic configuration of each participating atom. In addition to this, the Lewis structure also determines whether a single, double or triple bond is formed between the interacting atoms. If you realize, these valence electrons are always written in pair at each side of the symbol to show if all paired electrons exist or not.
Within the diagram, the ‘dots’ nearby the symbol of an element represents the valence electrons. The diagram is drawn to determine how the valence electrons of different atoms participate in the bond formation to form a molecule. The Lewis structure is a pictorial representation showing the electrons present in the valence shell in an atom. Conclusion Lewis Structure of Chloromethane (CH3Cl)
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