If an atom of sulfur (atomic number 16) were allowed to react with atoms of hydrogen (atomic number 1), which of the following molecules would be formed? The lines represent covalent bonds. H-S-H H H-S-H S-H H H-S-H H
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Step 1: Sulfur has 6 valence electrons and needs 2 more to complete its octet. Show more…
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The atomic number of sulfur is $16 .$ Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound. a. $\mathrm{HS}$ b. $\mathrm{HS}_{2}$ c. $\mathrm{H}_{2} \mathrm{S}$ d. $\mathrm{H}_{4} \mathrm{S}$
The atomic number of sulfur (S) is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound. (Explain your answer.) a. $\mathrm{HS}$ b. $\mathrm{H}_{2} \mathrm{S}$ c. $\mathrm{H}_{4} \mathrm{S}_{2}$ d. $\mathrm{H}_{4} \mathrm{S}$
The atomic number of sulfur is $16 .$ Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound. \begin{equation} \begin{array} { l l } { \text { (A) } \mathrm { HS } } & { \text { (C) } \mathrm { H } _ { 2 } \mathrm { S } } \\ { \text { (B) } \mathrm { HS } _ { 2 } } & { \text { (D) } \mathrm { H } _ { 4 } \mathrm { S } } \end{array} \end{equation}
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