How to draw Lewis structure of any compound? Easy Trick 

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if h goes above the n put your lone pairs bellw

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Both

H follows duplet rule and cl follows octet rule

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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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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Lewis structure for O3

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