Nov 24, 2018 Use information from step 4 and 5 to draw the CH 4 lewis structure. Easy Way – Treat them like Puzzle Pieces Lewis structure of CH 4. Alternatively a dot method can be used to draw the CH 4 Lewis structure. Calculate the total valence electrons in the molecule. Total=8; This unit is part of the Chemistry library. Lewis Dot Structure for Boron Oxide (B2O3) Boron (metal) has 3 valence electrons Oxygen (nonmetal) has 6 valence electrons, needs 2 to be balanced B3↘ ↙O2 B2 O3 Lewis Dot Structure for Sodium Fluoride Na +1 Cl-1 Na has 1 valence electron Fl needs 1 to be balanced Na Cl Covalent Bonds Covalent Bonds are attractions of 2 nonmetals They have low melting/boiling points and aren't a good.

Regents Chemistry Topics Unit 5 Bonding TEDED Bonding Video Bond Polarity Dipole Dipole Forces Types of Bonds Properties of Covalent Compounds Hydrogen Bonding Ionization Energy Network Solids van der Waals Forces Lewis Dot Structures-Covalent Metallic Bonds Like Dissolves Like 70 Lewis Dot Structures Videos (AP) Valence Shell Electron Pair Repulsion VSEPR(Shapes) Lewis Dot Structures -Ionic Molecular polarity Percent Water in a Hydrate Properties of Ionic Compounds Intermolecular Force Advanced Regents Chemistry Topics Unit 5 Bonding TEDED Bonding Video (AP) Bond Energy Hydrogen Bonding Types of Bonds Properties of Ionic Compounds van der Waals Forces Ionization Energy Properties of Covalent Compounds Like Dissolves Like (AP) Electron Affinity Network Solids Lewis Dot Structures-Covalent Metallic Bonds Percent Water in a Hydrate (AP) Formal Charge (AP) Valence Shell Electron Pair Repulsion VSEPR(Shapes) (AP) Bond Angles 70 Lewis Dot Structures Videos (AP) Hybridization of Orbitals (AP) Determining Hybridization in Structures (AP)Valence Bond Theory Lewis Dot Structures -Ionic Molecular polarity (AP)Sigma and Pi Bonds Intermolecular Force Bond Polarity Dipole Dipole Forces My Chemical Demonstration Videos

Every chemistry student has to learn how to draw Lewis Dot Structures. The key is to understand the steps and practice.

Lewis Structures are important to learn because they help us predict:

• the shape of a molecule.
• how the molecule might react with other molecules.
• the physical properties of the molecule (like boiling point, surface tension, etc.).

That helps us understand and predict interactions with things like medicine and our body, materials used to make buildings and airplanes, and all sorts of other substances. Lewis structures don't tell us everything, but along with molecule geometry and polarity they are hugely informative.

Ionic Bonding Lewis Dot Diagram

Ionic Lewis Dot Structure Worksheet

Search 100+ Lewis Structures on our site. (Opens new window.)

Click the Chemical Formula to see the Lewis Structure Acetone (C3H6O) AsCl3 (Arsenic Trichloride) AsF3 (Arsenic Trifluoride) AsF5 (Arsenic Pentafluoride) AsF6- (AsF6-) AsH3 (Arsenic Trihydride) AsO33- (Arsenite Ion) BBr3 (Boron Tribromide) BCl3 (Boron Trichloride) BF3 (Boron Trichloride) BF4- (Tetrafluoroborate Ion) BH3 (Boron Hydride) BH4- (BH4-) B(OH)3 (B(OH)3) BeCl2 (Beryllium Chloride) BeF2 (Beryllium Fluoride) BeH2 (Beryllium Hydride) Br2 (Bromine Gas or Elemental Bromine) Br3- (Tribromide Ion) BrF (Bromine Monofluoride) BrF2 (Bromine Difluoride) BrCl3 (Bromine Trichloride) BrF3 (Bromine Trifluoride) BrF5 (Bromine Pentafluoride) BrO- (Hypobromite Ion) BrO2- (Bromite Ion) BrO3- (Bromate Ion) C22- (Dicarbide Ion) CBr4 (Carbon Tetabromide) CCl4 (Carbon Tetachloride) ClF (Chlorine Monofluoride) CF2Cl2 (Dichlorodifluoromethane) CH2Cl2 (CH2Cl2) CH3- (CH3-) CH3Br (CH3Br) CH3Cl (Chloromethane or Methyl Chloride) CH3CN (Acetonitril or Methyl Cyanide) CH3COO- CH3COO- CH3COOH (Acetic Acid) CH3F (CH3F) CH3NH2 (Methylamine) CH3NO2 (CH3NO2) CH3OCH3 (Dimethyl Ether or Methoxymethane) CH3OH (Methanol or Methyl Alcohol) CH4 (Methane) C2F4 (C2F4) C2H2 (Ethyne or Acetylene) C2H2Br2 (C2H2Br2) C2H2Cl2 (C2H2Cl2) C2H4 (Ethene) C2H6 (Ethane) C2H6O C2H6O C3H6 (C3H6) C3H8 (Propane) C4H10 (Butane) C6H6 (Isomers - including Benzene) C6H12 (C6H12) CHCl3 (Chloromethane) CH2F2 (Difluoromethane) CH2O (Methanal or Formaldehyde) CH4O (CH4O) Cl2 (Chlorine Gas or Elemental Chlorine) Cl2CO (Cl2CO) Cl2O (Dichlorine Monoxide) Cl3PO (Phosphoryl Trichloride) ClF3 (Chlorine Trifluoride) ClF5 (Chlorine Tetrafluoride) ClO- (Hypochlorite Ion) ClO2 (Chlorine Dioxide) ClO2- (Chlorite Ion) ClO3- (Chlorate Ion) ClO4- (Perchlorate Ion) CO (Carbon monoxide) CO2 (Carbon Dioxide) CO32- (Carbonate Ion) COCl2 (COCl2) COF2 (COF2) COH2 (COH2) CN- (Cyanide Anion) CS2 (Carbon Disulfide) F2 (Fluorine Gas, Difluorine) H2 (Hydrogen Gas or Elemental Hydrogen) H2CO (Formaldehyde or Methanal) H2CO3 (Carbonic Acid) H2O (Water or Dihydrogen monoxide) H3O+ (Hydronium Ion) H2O2 (Hydrogen Peroxide or Dihydrogen Dioxide) HBr (Hydrogen Bromide or Hydrobromic Acid) HF (Hydrogen Fluoride or Hydrofluoric Acid) HCCH (Ethyne) HCl (Hydrogen Chloride or Hydrochloric Acid) HCO2- (Formate Ion) HCO3- (Hydrogen Carbonate Ion or Bicarbonate Ion) HCOOH (Methanoic Acid or Formic Acid) HI (Hydrogen Iodide or Hydroiodic Acid) HClO3 (Chloric Acid) HCN (Hydrogen Cyanide) HNO2 (Nitrous Acid) HNO3 (Nitric Acid) H2S (Dihydrogen Sulfide) HOCl (Hypochlorous Acid) H2Se (Dihydrogen Selenide) HSO3- (Bisulfite Ion) HSO4- (Bisulfate Ion) H2SO3 (Sulfurous Acid) H2SO4 (Sulfuric Acid) H3PO4 (Phosphoric Acid) I2 (Iodine Gas or Elemental Iodine) I3- (I3-) IBr2- (IBr2-) ICl (Iodine Chloride) ICl2- (ICl2-) ICl3 (ICl3) ICl4- (ICl4-) ICl5 (Iodine Pentachloride) IF2- (IF2-) IF3 (Iodine Trifluoride) IF4- (IF4-) IF5 (Iodine Pentafluoride) IO3- (Iodate Ion) IO4- (Perioiodate Ion) N2 (Nitrogen Gas, also called Elemental Nitrogen) N3- (Azide Ion) N2F2 (Dinitrogen Difluoride) N2H2 (Dinitrogen Dihydride) N2H4 (Dinitrogen Tetrahydride or Hydrazine or Diamine) N2O3 (Dinitrogen Trioxide) N2O4 (Dinitrogen Tetroxide) N2O5 (Dinitrogen Pentoxide) NCl3 (Nitrogen Trichloride) NF3 (Nitrogen Trifluoride) NH2- (NH2-) NH2Cl (Chloroamine) NH2OH (Hydroxylamine) NH3 (Ammonium or Nitrogen Trihydride) NH4+ (Ammonium Ion) NI3 (Nitrogen Triiodide) NO+ (Nitrosonium Ion) NO (Nitric Oxide or Nitrogen Monoxide) N2O (Nitrous Oxide or Dinitrogen Monoxide) NO2 (Nitrogen Dioxide) NO2- (Nitrite Ion) NO2Cl (NO2Cl) NO2F (NO2F) NO3- (Nitrate Ion) NOBr (Nitrosyl Bromide) NOCl (Nitrosyl Chloride) NOF (Nitrosyl Fluoride) O2 (Oxygen Gas, also called Elemental Oxygen) O22- (Perioxide Ion) O3 (Ozone) O3 O3 Resonance Structures OCl2 (OCl2) OCN- (Cyanate Ion) OCS (OCS) OF2 (Oxygen Difluoride) OH- (Hydroxide Ion) PBr3 Phosphorus Tribromide PBr5 Phosphorus Pentabromide PCl3 Phosphorus Trichloride PCl4- PCl4- PCl5 Phosphorus Pentachloride PF3 Phosphorus Trifluoride PF5 Phosphorus Pentafluoride PF6- Hexafluorophosphate Ion PH3 Phosphorus Trihydride POCl3 Phosphoryl Chloride or Phosphorus Oxychloride PO33- (Phosphite Ion) PO43- (Phosphate Ion) SBr2 (Sulfur Dibromide) SCl2 (Sulfur Dichloride) SCl4 (Sulfur Tetrachloride) SCN- (Thiocyanate) SeF4 (Selenium Tetrafluoride) SeF6 (Selenium Hexafluoride) SeO2 (Selenium Dioxide) SF2 (Sulfur Difluoride) SF4 (Sulfur Tetrafluoride) SF6 (Sulfur Hexafluoride) S2Cl2 (Diulfur Dichloride) SiCl4 (Silicon Tetrachloride) SiF4 (Silicon Tetrafluoride) SiF62- (Silicon Hexafluoride Ion) SiH4 (Silicon Tetrahydride) SiO2 (Silicon Dioxide) SnCl2 (Tin (II) Chloride) SOCl2 (SOCl2) SO2 (Sulfur Dioxide) SO3 (Sulfur Dioxide) SO32- (Sulfite Ion) SO42- (Sulfate Ion) Water (H2O) XeCl4 Xenon Tetrachloride XeF2 XeF2 XeF4 Xenon Tetrafluoride XeF6 Xenon Hexafluoride XeH4 XeO4 XeO3 XeO3 XeO2F2 XeO2F2

Steps for Writing Lewis Structures Find the total valence electrons for the molecule. Explain How Examples: H2S, NCl3, OH- Put the least electronegative atom in the center. Note: H always goes outside. Examples: NOCl, CF2Cl2, HCN Put two electrons between atoms to form a chemical bond. Examples: CH4, NH3, I2 Complete octets on outside atoms. Note: H only needs two valence electrons. If central atom does not have an octet, move electrons from outer atoms to form double or triple bonds. Examples: O2, N2, C2H4 Advanced Steps If you have extra electrons after the above steps add them to the central atom. Note: elements in the Period Three (usually S, P, or Xe) can have more than eight valence electrons. Examples: ClF3, SF4,XeH4 Check the Formal Charges to make sure you have the best Lewis Structure. Explain How Examples: SO42-, N2O, XeO3 Notable Exceptions to the Octet Rule H only needs 2 valence electrons. Be and B don’t need 8 valence electrons. S and P sometimes have more than 8 val. Electrons. Elements in Period Three, Four, etc (on the periodic table) can hold more than 8 valence electrons.

Ionic Lewis Structure Practice