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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bro your explanation kinda kills my fear for my exam , litterally wtf is this , you are amazinggggg❤‍🔥

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Really nice video and understanding each and every point

[@user-uk7ob4ti6u]

Much appreciated goes to Najam Academic ,so that you always do great thing to everyone in the world.

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this explanation was too good thank you soo much sir

[@i-mathgicnayan9944]

Thank you so much sir Najam! Your videos are really helpful for students starting to learn chemistry like me 🥰🥰 will surely recommend your channel to my colleagues!

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❤

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[@YTLittleWorld]

Thanks for this video.
Its help a lot..❤

[@fathayabgym8507]

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

[@ARVINDKUMAR-uw9od]

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

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Nice explain

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Omg finally i understood it thanks a lot!

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Excellent explanation

[@khizarhayat31]

Please Make video on rutherford atomic model,Experiment,conclusion,defects almost everything about this.please .........
Also about Bohr model.you are best teacher.I am your regular viewer.please .....

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Great explain thank you ❤

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Hi,your all lectures are fantastic and easy to understand you have cleared my all concept,Thankyou very Much ...Sir how you make this video from which app or software and also thumbnail Pls tell Sir.

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Ur technique to teach is amazing

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Explanation with animation..... ❤❤

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Sir please make video on molecular formula

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

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Keep practicing questions , at a time it'll be at the tip of your tongue.

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Sir plz do a video for resonance structures

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amazing

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Thank You Sir❤

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Sir make video on main branches of chemistry

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

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Your videos are amazing and easy to understand.

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Bro Hybridization Is So Easy..

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[@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?

[@deloader]

if h goes above the n put your lone pairs bellw

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5:48 arrow position for H2O is incorrect

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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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Explain about acidic nature please

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Sir how to show dot structure of ethane

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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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Brother who can me conclube that who many electrons in the hydrogen etc
Can u please explain

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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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1:22 -It❌ Ate✅

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U focus on the video not the spelling mistake 😂

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sir amazing lecture but in ka faida hi nahi howa we need to know different and some difficult for better because We never gonna have easy in exams always tough so I hope that you will give some difficult examples

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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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Please upload Formal Charge????

[@NAJAMACADEMY]

Already uploaded...
👍

[@muraliullamparthi8012]

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

[@sayudhsarkar9158]

Both

[@yusrafaruqi2934]

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........

[@simplyspace4624]

Sir can you make video coordinate covalent bond of O³

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th-cam.com/video/O9D4wt_CQjo/w-d-xo.html

[@nikhilthapa6840]

Lewis structure for O3

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@@nikhilthapa6840 yes

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@@simplyspace4624 did you found that helpful?

[@simplyspace4624]

@@nikhilthapa6840 there was never 0³ structure explained

[@makingmathseasy807]

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

[@yusrafaruqi2934]

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

[@aimankhan7680]

Sir what is duplet rule ???

[@aimankhan7680]

Also octate rule

[@yusrafaruqi2934]

Duplet rule: atom should have atleast 2 electrons in its valence shell to get stable.
Octet rule: atom should have atleast 8 electrons in its valence shell to get stable.

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The ending of your every sentence 😂