Practice worksheet for drawing Lewis dot structures of various covalent compounds and ions.
Worksheet for drawing Lewis dot structures of covalent compounds including PF₅, NO, I₃⁻, HCN, BrF₅, CO, BrF₃, CO₂⁻, SCl₄, AlH₃, BF₃, C₂H₄, PH₃, C₂H₆, and NH₄⁺.
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Step-by-step solution for: Free Printable Lewis Dot Structure Worksheets
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Show Answer Key & Explanations
Step-by-step solution for: Free Printable Lewis Dot Structure Worksheets
1. PF₅: Phosphorus (P) is the central atom with 5 valence electrons. Each fluorine (F) atom has 7 valence electrons. P forms single bonds with 5 F atoms, using 10 electrons (5 bonds × 2 electrons). Each F atom completes its octet with 3 lone pairs. Total valence electrons: 5 + 5×7 = 40. Structure: P bonded to 5 F atoms, each F has 3 lone pairs.
2. NO: Nitrogen (N) has 5 valence electrons, oxygen (O) has 6. Total valence electrons: 11. N and O form a double bond (4 electrons), N has one lone pair (2 electrons), O has two lone pairs (4 electrons). N has one unpaired electron. Structure: N=O with 2 lone pairs on O and 1 lone pair on N, and one unpaired electron on N.
3. I₃⁻: Central iodine (I) bonded to two terminal I atoms. Total valence electrons: 3×7 + 1 = 22. Central I forms single bonds with each terminal I (4 electrons). Central I has 3 lone pairs (6 electrons), each terminal I has 3 lone pairs (6 electrons each). Structure: I-I-I with 3 lone pairs on central I and 3 lone pairs on each terminal I.
4. HCN: Hydrogen (H) has 1 valence electron, carbon (C) has 4, nitrogen (N) has 5. Total: 10. H-C≡N triple bond. C has no lone pairs, N has one lone pair. Structure: H-C≡N with a lone pair on N.
5. BrF₅: Bromine (Br) is central with 7 valence electrons. Each F has 7. Total: 7 + 5×7 = 42. Br forms single bonds with 5 F atoms (10 electrons). Br has one lone pair (2 electrons). Each F has 3 lone pairs (6 electrons each). Structure: Br bonded to 5 F atoms, Br has one lone pair.
6. CO: Carbon (C) has 4, oxygen (O) has 6. Total: 10. C≡O triple bond. C has one lone pair, O has one lone pair. Structure: C≡O with a lone pair on C and a lone pair on O.
7. BrF₃: Bromine (Br) is central with 7 valence electrons. Each F has 7. Total: 7 + 3×7 = 28. Br forms single bonds with 3 F atoms (6 electrons). Br has 2 lone pairs (4 electrons). Each F has 3 lone pairs (6 electrons each). Structure: Br bonded to 3 F atoms, Br has 2 lone pairs.
8. CO₂⁻: Carbonate ion. Carbon (C) has 4 valence electrons, each O has 6. Total: 4 + 3×6 + 2 = 24 (due to -2 charge). Resonance structures: C double bonded to two O atoms and single bonded to one O⁻. Each O has 3 lone pairs, the single bonded O has an extra electron (negative charge). Structure: Resonance between three forms where one O is double bonded, two are single bonded with negative charge.
9. SCl₄: Sulfur (S) is central with 6 valence electrons. Each Cl has 7. Total: 6 + 4×7 = 34. S forms single bonds with 4 Cl atoms (8 electrons). S has one lone pair (2 electrons). Each Cl has 3 lone pairs (6 electrons each). Structure: S bonded to 4 Cl atoms, S has one lone pair.
10. AlH₃: Aluminum (Al) has 3 valence electrons, each H has 1. Total: 3 + 3×1 = 6. Al forms single bonds with 3 H atoms (6 electrons). Al has no lone pairs. Structure: Al bonded to 3 H atoms.
11. BF₃: Boron (B) has 3 valence electrons, each F has 7. Total: 3 + 3×7 = 24. B forms single bonds with 3 F atoms (6 electrons). B has no lone pairs. Each F has 3 lone pairs (6 electrons each). Structure: B bonded to 3 F atoms, B has no lone pairs.
12. C₂H₄: Ethene. Each C has 4 valence electrons, each H has 1. Total: 2×4 + 4×1 = 12. C=C double bond. Each C bonded to 2 H atoms. Each C has no lone pairs. Structure: H₂C=CH₂.
13. PH₃: Phosphorus (P) has 5 valence electrons, each H has 1. Total: 5 + 3×1 = 8. P forms single bonds with 3 H atoms (6 electrons). P has one lone pair (2 electrons). Structure: P bonded to 3 H atoms, P has one lone pair.
14. C₂H₆: Ethane. Each C has 4 valence electrons, each H has 1. Total: 2×4 + 6×1 = 14. C-C single bond. Each C bonded to 3 H atoms. Each C has no lone pairs. Structure: H₃C-CH₃.
15. NH₄⁺: Nitrogen (N) has 5 valence electrons, each H has 1. Total: 5 + 4×1 - 1 = 8 (due to +1 charge). N forms single bonds with 4 H atoms (8 electrons). N has no lone pairs. Structure: N bonded to 4 H atoms, positive charge on N.
2. NO: Nitrogen (N) has 5 valence electrons, oxygen (O) has 6. Total valence electrons: 11. N and O form a double bond (4 electrons), N has one lone pair (2 electrons), O has two lone pairs (4 electrons). N has one unpaired electron. Structure: N=O with 2 lone pairs on O and 1 lone pair on N, and one unpaired electron on N.
3. I₃⁻: Central iodine (I) bonded to two terminal I atoms. Total valence electrons: 3×7 + 1 = 22. Central I forms single bonds with each terminal I (4 electrons). Central I has 3 lone pairs (6 electrons), each terminal I has 3 lone pairs (6 electrons each). Structure: I-I-I with 3 lone pairs on central I and 3 lone pairs on each terminal I.
4. HCN: Hydrogen (H) has 1 valence electron, carbon (C) has 4, nitrogen (N) has 5. Total: 10. H-C≡N triple bond. C has no lone pairs, N has one lone pair. Structure: H-C≡N with a lone pair on N.
5. BrF₅: Bromine (Br) is central with 7 valence electrons. Each F has 7. Total: 7 + 5×7 = 42. Br forms single bonds with 5 F atoms (10 electrons). Br has one lone pair (2 electrons). Each F has 3 lone pairs (6 electrons each). Structure: Br bonded to 5 F atoms, Br has one lone pair.
6. CO: Carbon (C) has 4, oxygen (O) has 6. Total: 10. C≡O triple bond. C has one lone pair, O has one lone pair. Structure: C≡O with a lone pair on C and a lone pair on O.
7. BrF₃: Bromine (Br) is central with 7 valence electrons. Each F has 7. Total: 7 + 3×7 = 28. Br forms single bonds with 3 F atoms (6 electrons). Br has 2 lone pairs (4 electrons). Each F has 3 lone pairs (6 electrons each). Structure: Br bonded to 3 F atoms, Br has 2 lone pairs.
8. CO₂⁻: Carbonate ion. Carbon (C) has 4 valence electrons, each O has 6. Total: 4 + 3×6 + 2 = 24 (due to -2 charge). Resonance structures: C double bonded to two O atoms and single bonded to one O⁻. Each O has 3 lone pairs, the single bonded O has an extra electron (negative charge). Structure: Resonance between three forms where one O is double bonded, two are single bonded with negative charge.
9. SCl₄: Sulfur (S) is central with 6 valence electrons. Each Cl has 7. Total: 6 + 4×7 = 34. S forms single bonds with 4 Cl atoms (8 electrons). S has one lone pair (2 electrons). Each Cl has 3 lone pairs (6 electrons each). Structure: S bonded to 4 Cl atoms, S has one lone pair.
10. AlH₃: Aluminum (Al) has 3 valence electrons, each H has 1. Total: 3 + 3×1 = 6. Al forms single bonds with 3 H atoms (6 electrons). Al has no lone pairs. Structure: Al bonded to 3 H atoms.
11. BF₃: Boron (B) has 3 valence electrons, each F has 7. Total: 3 + 3×7 = 24. B forms single bonds with 3 F atoms (6 electrons). B has no lone pairs. Each F has 3 lone pairs (6 electrons each). Structure: B bonded to 3 F atoms, B has no lone pairs.
12. C₂H₄: Ethene. Each C has 4 valence electrons, each H has 1. Total: 2×4 + 4×1 = 12. C=C double bond. Each C bonded to 2 H atoms. Each C has no lone pairs. Structure: H₂C=CH₂.
13. PH₃: Phosphorus (P) has 5 valence electrons, each H has 1. Total: 5 + 3×1 = 8. P forms single bonds with 3 H atoms (6 electrons). P has one lone pair (2 electrons). Structure: P bonded to 3 H atoms, P has one lone pair.
14. C₂H₆: Ethane. Each C has 4 valence electrons, each H has 1. Total: 2×4 + 6×1 = 14. C-C single bond. Each C bonded to 3 H atoms. Each C has no lone pairs. Structure: H₃C-CH₃.
15. NH₄⁺: Nitrogen (N) has 5 valence electrons, each H has 1. Total: 5 + 4×1 - 1 = 8 (due to +1 charge). N forms single bonds with 4 H atoms (8 electrons). N has no lone pairs. Structure: N bonded to 4 H atoms, positive charge on N.
Parent Tip: Review the logic above to help your child master the concept of lewis dot structure covalent bond worksheet.
