How to draw Lewis structure of any compound? Easy Trick

This lecture is about how to draw Lewis structure easily. In this animated lecture, I will teach you drawing Lewis structure of different compounds.
To learn more about how to draw Lewis structure, watch this lecture till the end.
#lewisstructure
#tricktodrawlewisstructure
#chemistry
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[@fathayabgym8507]

Thanks sir ap na is structure ka dots samjha dia,love from Pakistan 🇵🇰👍🏼

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Really nice video and understanding each and every point

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Thank you 😊❤️❤️ so much sir because of you first time I understand this concept just in 6 minute

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Sir jiiii...... Any trick to remember the priority series of functional groups in GOC?

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Tq sir for the best explanation sir please keep maths also sir please 🥺🥺

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Explanation with animation..... ❤❤

[@PilarEverjai]

Thank you for the explanation, but can you explain how to determine the placement of elements when drawing the lewis structure? Ex: NH3, does the H element have to be placed as you displayed, or can an H go above the N?

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if h goes above the n put your lone pairs bellw

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hlw

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assalamualaikum. thanks for your valuable videos, sir. would you make a structural video on NH4, CO3 HCO3, SO4 PH4 NO2 NO3 SO3 Ion. that means I am requesting a video on Radicals structure

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5:48 arrow position for H2O is incorrect

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It's helpful thankyou ! But atoms ka electron yaad nahi ho raha ha koi to suggestion to learn that

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Make video on copsular nature of mattar

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Sir how to show dot structure of ethane

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1:21 why we have to put dot on the upper side of H we could have put that in the lower or anywhere else...??

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We can put it anywhere

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My guru

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HCL compound is formed by which doblet rule or octet rule?

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Both

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H follows duplet rule and cl follows octet rule

[@jamal_106]

HCL, which stands for hydrogen chloride, is a compound formed by the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight electrons in their outermost energy level (except for hydrogen, which aims for a duet configuration with two electrons). In the case of HCL, hydrogen (H) has one valence electron, and chlorine (Cl) has seven valence electrons. In order to achieve a stable electron configuration, hydrogen needs to gain one electron to achieve a duet configuration, while chlorine needs to gain one electron to achieve an octet configuration. Therefore, chlorine accepts the electron from hydrogen, forming a covalent bond between the two atoms. This satisfies the octet rule for both hydrogen and chlorine. In summary, the formation of HCL follows the octet rule, with hydrogen achieving a duet configuration and chlorine achieving an octet configuration. Thank me later........

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Sir why is Lewis dot structure of H2o. Is not in a straight line

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Because of the interelectronic repulsion of oxygen atom as it has 4 non bonding electrons (2 lone electron pairs).

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Please upload Formal Charge????

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Already uploaded... 👍

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Sir can you make video coordinate covalent bond of O³

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Lewis structure for O3

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What is the difference between covalent bond and non covalent bond

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[@jamal_106]

The main difference between a covalent bond and a non-covalent bond lies in the nature of the chemical bond formed between atoms. Here's a breakdown of their characteristics: Covalent Bond: Sharing of electrons: Covalent bonds occur when atoms share electrons to achieve a stable electron configuration. The shared electrons are typically localized between the bonded atoms. Strong bond: Covalent bonds are strong and require a significant amount of energy to break. Examples: Examples of covalent bonds include the bonds found in molecules like water (H2O), methane (CH4), and oxygen (O2). Non-covalent Bond: Weak attractions: Non-covalent bonds are weaker compared to covalent bonds and involve various types of interactions between atoms or molecules. No electron sharing: Unlike covalent bonds, non-covalent bonds do not involve the sharing of electrons between atoms. Types of non-covalent bonds: There are several types of non-covalent bonds, including hydrogen bonds (electrostatic attraction between a hydrogen atom and an electronegative atom like oxygen or nitrogen), ionic bonds (attraction between oppositely charged ions), van der Waals interactions (weak attractions between temporary or induced dipoles), and hydrophobic interactions (interactions between nonpolar molecules in an aqueous environment). Examples: Non-covalent bonds are commonly found in biological systems and play crucial roles in various processes, such as protein folding, DNA structure, and molecular recognition. In summary, covalent bonds involve the sharing of electrons between atoms and are strong, while non-covalent bonds are weaker interactions that do not involve electron sharing but rely on other forces and attractions. Thank me later..........

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U focus on the video not the spelling mistake 😂