Lewis Structure Worksheet | Lecture notes Geometry | Docsity - Free Printable
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Step-by-step solution for: Lewis Structure Worksheet | Lecture notes Geometry | Docsity
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Step-by-step solution for: Lewis Structure Worksheet | Lecture notes Geometry | Docsity
1. CH₄: Carbon is central, bonded to four H atoms with single bonds. No lone pairs on C. Tetrahedral geometry.
2. BF₃: Boron is central, bonded to three F atoms with single bonds. No lone pairs on B. Trigonal planar geometry.
3. HCN: Linear structure. H–C≡N. Triple bond between C and N. Lone pair on N.
4. NH₃: Nitrogen is central, bonded to three H atoms with single bonds. One lone pair on N. Trigonal pyramidal geometry.
5. H₂O: Oxygen is central, bonded to two H atoms with single bonds. Two lone pairs on O. Bent geometry.
6. ClO₃⁻: Chlorine is central, bonded to three O atoms. One double bond and two single bonds (resonance). One lone pair on Cl. Formal charges: Cl = +1, single-bonded O = -1 each. Trigonal pyramidal geometry.
7. H₃O⁺: Oxygen is central, bonded to three H atoms with single bonds. One lone pair on O. Formal charge +1 on O. Trigonal pyramidal geometry.
8. NH₂⁻: Nitrogen is central, bonded to two H atoms with single bonds. Two lone pairs on N. Formal charge -1 on N. Bent geometry.
9. NH₄⁺: Nitrogen is central, bonded to four H atoms with single bonds. No lone pairs on N. Formal charge +1 on N. Tetrahedral geometry.
10. C₂H₄: Two C atoms double-bonded to each other. Each C bonded to two H atoms with single bonds. No lone pairs. Trigonal planar geometry around each C.
11. C₂H₂: Two C atoms triple-bonded to each other. Each C bonded to one H atom with a single bond. No lone pairs. Linear geometry.
12. N₃⁻: Linear structure. [N=N=N]⁻ or resonance hybrids. Central N has +1 formal charge, terminal N atoms have -1 each in major resonance form. Linear geometry.
13. NOF: Nitrogen is central, bonded to O and F. Double bond to O, single bond to F. One lone pair on N. Formal charges: N=+1, O=-1, F=0. Bent geometry.
14. ClF₂⁺: Chlorine is central, bonded to two F atoms with single bonds. Two lone pairs on Cl. Formal charge +1 on Cl. Bent geometry.
15. FNO₂: Nitrogen is central, bonded to F and two O atoms. Double bond to one O, single bond to other O and to F. One lone pair on N. Formal charges: N=+1, single-bonded O=-1. Trigonal planar geometry.
16. XeF₅⁺: Xenon is central, bonded to five F atoms with single bonds. One lone pair on Xe. Formal charge +1 on Xe. Square pyramidal geometry.
17. BrF₅: Bromine is central, bonded to five F atoms with single bonds. One lone pair on Br. Square pyramidal geometry.
18. IF₄⁻: Iodine is central, bonded to four F atoms with single bonds. Two lone pairs on I. Formal charge -1 on I. Square planar geometry.
19. SF₆: Sulfur is central, bonded to six F atoms with single bonds. No lone pairs. Octahedral geometry.
20. N₂O₄: Two N atoms bonded together, each bonded to two O atoms. Resonance structures exist. Common structure: N–N single bond, each N double-bonded to one O and single-bonded to another O. Formal charges vary. Planar geometry around each N.
21. C₂O₄²⁻: Two C atoms bonded together, each bonded to two O atoms. Resonance structures: C=C double bond, each C double-bonded to one O and single-bonded to another O (with negative charge). Formal charges: each single-bonded O = -1. Planar geometry around each C.
22. H₂PO₄⁻: Phosphorus is central, bonded to four O atoms. One double bond to O, two single bonds to OH groups, one single bond to O⁻. Formal charges: P=+1, O⁻=-1. Tetrahedral geometry.
23. XeO₄: Xenon is central, bonded to four O atoms with double bonds. No lone pairs on Xe. Tetrahedral geometry.
24. PO₃⁻: Phosphorus is central, bonded to three O atoms. One double bond, two single bonds (resonance). One lone pair on P. Formal charges: P=+1, single-bonded O=-1 each. Trigonal pyramidal geometry.
25. NO: Nitrogen and oxygen connected by a double bond. Nitrogen has one unpaired electron, oxygen has two lone pairs. Formal charges: N=+1, O=-1. Linear geometry.
2. BF₃: Boron is central, bonded to three F atoms with single bonds. No lone pairs on B. Trigonal planar geometry.
3. HCN: Linear structure. H–C≡N. Triple bond between C and N. Lone pair on N.
4. NH₃: Nitrogen is central, bonded to three H atoms with single bonds. One lone pair on N. Trigonal pyramidal geometry.
5. H₂O: Oxygen is central, bonded to two H atoms with single bonds. Two lone pairs on O. Bent geometry.
6. ClO₃⁻: Chlorine is central, bonded to three O atoms. One double bond and two single bonds (resonance). One lone pair on Cl. Formal charges: Cl = +1, single-bonded O = -1 each. Trigonal pyramidal geometry.
7. H₃O⁺: Oxygen is central, bonded to three H atoms with single bonds. One lone pair on O. Formal charge +1 on O. Trigonal pyramidal geometry.
8. NH₂⁻: Nitrogen is central, bonded to two H atoms with single bonds. Two lone pairs on N. Formal charge -1 on N. Bent geometry.
9. NH₄⁺: Nitrogen is central, bonded to four H atoms with single bonds. No lone pairs on N. Formal charge +1 on N. Tetrahedral geometry.
10. C₂H₄: Two C atoms double-bonded to each other. Each C bonded to two H atoms with single bonds. No lone pairs. Trigonal planar geometry around each C.
11. C₂H₂: Two C atoms triple-bonded to each other. Each C bonded to one H atom with a single bond. No lone pairs. Linear geometry.
12. N₃⁻: Linear structure. [N=N=N]⁻ or resonance hybrids. Central N has +1 formal charge, terminal N atoms have -1 each in major resonance form. Linear geometry.
13. NOF: Nitrogen is central, bonded to O and F. Double bond to O, single bond to F. One lone pair on N. Formal charges: N=+1, O=-1, F=0. Bent geometry.
14. ClF₂⁺: Chlorine is central, bonded to two F atoms with single bonds. Two lone pairs on Cl. Formal charge +1 on Cl. Bent geometry.
15. FNO₂: Nitrogen is central, bonded to F and two O atoms. Double bond to one O, single bond to other O and to F. One lone pair on N. Formal charges: N=+1, single-bonded O=-1. Trigonal planar geometry.
16. XeF₅⁺: Xenon is central, bonded to five F atoms with single bonds. One lone pair on Xe. Formal charge +1 on Xe. Square pyramidal geometry.
17. BrF₅: Bromine is central, bonded to five F atoms with single bonds. One lone pair on Br. Square pyramidal geometry.
18. IF₄⁻: Iodine is central, bonded to four F atoms with single bonds. Two lone pairs on I. Formal charge -1 on I. Square planar geometry.
19. SF₆: Sulfur is central, bonded to six F atoms with single bonds. No lone pairs. Octahedral geometry.
20. N₂O₄: Two N atoms bonded together, each bonded to two O atoms. Resonance structures exist. Common structure: N–N single bond, each N double-bonded to one O and single-bonded to another O. Formal charges vary. Planar geometry around each N.
21. C₂O₄²⁻: Two C atoms bonded together, each bonded to two O atoms. Resonance structures: C=C double bond, each C double-bonded to one O and single-bonded to another O (with negative charge). Formal charges: each single-bonded O = -1. Planar geometry around each C.
22. H₂PO₄⁻: Phosphorus is central, bonded to four O atoms. One double bond to O, two single bonds to OH groups, one single bond to O⁻. Formal charges: P=+1, O⁻=-1. Tetrahedral geometry.
23. XeO₄: Xenon is central, bonded to four O atoms with double bonds. No lone pairs on Xe. Tetrahedral geometry.
24. PO₃⁻: Phosphorus is central, bonded to three O atoms. One double bond, two single bonds (resonance). One lone pair on P. Formal charges: P=+1, single-bonded O=-1 each. Trigonal pyramidal geometry.
25. NO: Nitrogen and oxygen connected by a double bond. Nitrogen has one unpaired electron, oxygen has two lone pairs. Formal charges: N=+1, O=-1. Linear geometry.
Parent Tip: Review the logic above to help your child master the concept of lewis dot structures worksheet.
