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Lewis dot structures and electronic geometries for various molecules and ions. Students can use this information to understand the bonding patterns and electron arrangements in these compounds. A range of elements, including hydrogen, carbon, nitrogen, oxygen, fluorine, bromine, chlorine, iodine, sulfur, and xenon.
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Use Guides 1-3 to draw the Lewis dot structures for the following: H 2 Cl 2
BCl 3 CH 4
Use Guides 1-4 to draw the Lewis dot structures for the following: H CCH 2 2 CN –
Use Guides 1-5 to draw the Lewis dot structures for the following: CO 3 2 - SO 2
NO 2 - C H 6 6 (6 Cs in a ring)
O 3 (not in a ring!) HOCO 2 -
Give the electronic and molecular geometries about the central atom for the following:
A) CH 4 B) XeF 6 2 +
hybrid = sp 3 hybrid = sp d^3 electronic geometry = tetrahedron electronic geometry = octahedral molecular geometry = tetrahedron molecular geometry = octahedral
C) (Note: check comments on multiple bonds) HCN D) CO 3 2 -
hybrid = sp hybrid = sp^2 electronic geometry = linear electronic geometry = trigonal molecular geometry = linear molecular geometry = trigonal
E) BCl 3 F) PCl 5
hybrid = sp 2 hybrid = sp d^3 electronic geometry = trigonal electronic geometry = trigonal pyramid molecular geometry = trigonal molecular geometry = trigonal pyramid
hybrid = sp 3 hybrid = sp^3 electronic geometry = tetrahedral electronic geometry = tetrahedral molecular geometry = bent 109 molecular geometry = trigonal pyramid I) SO 4 2 - ion J) IF molecule 5
hybrid = sp 3 hybrid = sp d^3 electronic geometry = tetrahedral electronic geometry = trigonal bipyramid molecular geometry = tetrahedral molecular geometry = trigonal bipyramid