91影视

Many monatomic ions are found in seawater, including the ions formed from the following list of elements. Write the Lewis symbols for the monatomic ions formed from the following elements: (a)\({\rm{CI}}\)(b)\({\rm{Na}}\)(c)\({\rm{Mg}}\)(d)\({\rm{Ca}}\)(e)\({\rm{K}}\)(f)\({\rm{Br}}\)(g)\({\rm{Sr}}\)(h)\({\rm{F}}\).

Write the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols of the atom from which they are formed: (a) \({\rm{MgS}}\) (b) \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\) (c) \({\rm{GaC}}{{\rm{l}}_{\rm{3}}}\) (d) \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) (e) \({\rm{L}}{{\rm{i}}_{\rm{3}}}{\rm{N}}\) (f) \({\rm{KF}}\) .

In the Lewis structures listed here, M and X represent various elements in the third period of the periodic table. Write the formula of each compound using the chemical symbols of each element:

Write the Lewis structure for the diatomic molecule \({{\rm{P}}_{\rm{2}}}\), an unstable form of phosphorus found in high temperature phosphorus vapor.

Write Lewis structures for the following: (a)\({{\rm{O}}_{\rm{2}}}\)(b)\({{\rm{H}}_{\rm{2}}}{\rm{CO}}\)(c)\({\rm{As}}{{\rm{F}}_{\rm{3}}}\)(d)\({\rm{ClNO}}\)(e)\({\rm{SiC}}{{\rm{l}}_{\rm{4}}}\)(f)\({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\)(g)\({\rm{N}}{{\rm{H}}_{\rm{4}}}^{\rm{ + }}\)(h)\({\rm{B}}{{\rm{F}}_{\rm{4}}}^{\rm{ - }}\)(i)\({\rm{HCCH}}\)(j)\({\rm{CICN}}\)(k)\({{\rm{C}}_{\rm{2}}}^{{\rm{2 + }}}\).

Iron(\({\rm{III}}\)) sulfate (\({\rm{F}}{{\rm{e}}_{\rm{2}}}{{\rm{(S}}{{\rm{O}}_{\rm{4}}}{\rm{)}}_{\rm{3}}}\)) is composed of \({\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}\) and \({\rm{S}}{{\rm{O}}_{\rm{4}}}^{{\rm{2 - }}}\) ions. Explain why a sample of iron(\({\rm{III}}\)) sulfate is uncharged.

Write Lewis structures for the following: (a) \({\rm{CI}}{{\rm{F}}_{\rm{3}}}\) (b) \({\rm{PC}}{{\rm{I}}_{\rm{5}}}\) (c) \({\rm{B}}{{\rm{F}}_{\rm{3}}}\) (d) \({\rm{P}}{{\rm{F}}_{\rm{6}}}^{\rm{ - }}\) .

Write Lewis structures for the following: (a)\({\rm{Se}}{{\rm{F}}_{\rm{6}}}\)(b)\({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\)(c)\({\rm{SeC}}{{\rm{l}}_{\rm{3}}}^{\rm{ + }}\)(d)\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\)(contains a\({\rm{B - B}}\)bond).

Write Lewis structures for: (a) \({\rm{P}}{{\rm{O}}_{\rm{4}}}^{{\rm{3 - }}}\) (b) \({\rm{IC}}{{\rm{I}}_{\rm{4}}}^{\rm{ - }}\) (c) \({\rm{S}}{{\rm{O}}_{\rm{3}}}^{{\rm{2 - }}}\) (d) \({\rm{HONO}}\) .

Correct the following statement: 鈥淭he bonds in solid\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are ionic; the bond in a\({\text{HCl}}\)molecule is covalent. Thus, all of the valence electrons in\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are located on the\({\text{C}}{{\text{I}}^{\text{ - }}}\)ions, and all of the valence electrons in a\({\text{HCl}}\)molecule are shared between the\({\text{H}}\)and\({\text{CI}}\)atoms.鈥�