Draw Lewis structures of the following molecules and ions: $H_2S$,$SiCl_4$,$BeF_2$,$CO_3^{2-}$,$HCOOH$.
(N/A) The Lewis structures represent the valence electrons of atoms in a molecule or ion. The structures are as follows:
| Name / Formula | Lewis Structure |
|---|---|
| Hydrogen sulphide $(H_2S)$ | $H:\ddot{S}:H$ |
| Silicon tetrachloride $(SiCl_4)$ | $\ddot{Cl}:\ddot{Si}:\ddot{Cl}$ (with $Cl$ atoms at four corners) |
| Beryllium fluoride $(BeF_2)$ | $:\ddot{F}:Be:\ddot{F}:$ |
| Carbonate ion $(CO_3^{2-})$ | $[ :\ddot{O}:\ddot{C}:\ddot{O}: ]^{2-}$ (with one double bond to $O$) |
| Formic acid $(HCOOH)$ | $H:\ddot{C}:\ddot{O}:H$ (with a double bonded $O$ on $C$) |
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$B$. Bond length of $N_2$ is shorter than $O_2$.
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$B$. Bond length of $N_2$ is shorter than $O_2$.
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$D$. Dipole moment of $H_2S$ is higher than that of water molecule.
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