If an atom of sulfur (atomic number 16) were allowed to react with atoms of hydrogen (atomic number 1), which of the molecules below would be formed?
a.S-H
b.H-S-H
c.H-S-H
|
H
d.H
|
H-S-H
|
H
e.H=S=H
b
To determine which molecule would be formed when an atom of sulfur reacts with atoms of hydrogen, we need to understand the combining capacities of each element and the rules governing chemical bonding.
First, let's look at the atomic number of sulfur (16) and hydrogen (1). The atomic number represents the number of protons in the nucleus of an atom, which also determines the number of electrons surrounding the nucleus.
Sulfur has 16 protons and 16 electrons, while hydrogen has 1 proton and 1 electron.
Now, let's consider the combining capacities, or valence electrons, of each element. Valence electrons are those electrons in the outermost energy level of an atom and are involved in chemical bonding.
Sulfur is in Group 16 of the periodic table, which means it has 6 valence electrons. Hydrogen is in Group 1, and it has 1 valence electron.
To form stable compounds, atoms tend to gain, lose, or share electrons in order to achieve a full outer electron shell (usually 8 electrons, except for hydrogen and helium).
In this case, sulfur needs 2 more electrons to complete its outer shell, while hydrogen only needs 1 more electron.
Now, let's consider the options provided:
a. S-H: This option represents a simple bond between sulfur and hydrogen. However, sulfur would still be short of 1 electron to complete its outer shell, so this would not be a stable molecule.
b. H-S-H: This option represents two hydrogen atoms bonded to a central sulfur atom. This configuration would allow sulfur to achieve a full outer shell with 2 shared electrons. This is a stable and likely molecule known as hydrogen sulfide (H2S).
c. H-S-H with a single bond and a lone pair on sulfur: This option is similar to option b, but it includes a lone pair of electrons on the sulfur atom. While this configuration is possible, it would be less common for sulfur to have a lone pair in this situation. Hence, option b (H2S) is more likely.
d. H attached to either side of S, forming a chain: This option represents multiple hydrogen atoms bonded to a central sulfur atom, forming a chain. This type of structure is less common for sulfur and hydrogen atoms and is not as stable as option b.
e. H=S=H: This option represents a triple bond between sulfur and hydrogen. However, both sulfur and hydrogen prefer to form single bonds. Triple bonds between sulfur and hydrogen are not commonly observed.
Therefore, the most likely molecule formed by the reaction between sulfur and hydrogen is hydrogen sulfide, represented by option b (H-S-H).
To determine the molecule formed when an atom of sulfur reacts with atoms of hydrogen, we need to consider the valence electrons and the bonding capacity of each atom.
First, we need to determine the number of valence electrons for each atom:
- Sulfur (S) has 16 electrons, and its electron configuration is 2-8-6. Since it is in group 16 of the periodic table, it has 6 valence electrons.
- Hydrogen (H) has 1 electron, and it is in group 1 of the periodic table. Therefore, hydrogen has 1 valence electron.
In order for atoms to bond, a complete valence shell is needed. Sulfur needs 2 additional electrons to complete its valence shell, while hydrogen needs 1 additional electron.
Combining one atom of sulfur with two atoms of hydrogen would satisfy the electron requirements for both elements. Let's examine the options provided:
a. S-H: This option only shows a single bond between sulfur and hydrogen. Since sulfur needs two additional electrons, it cannot complete its valence shell through this molecule. Therefore, this option is incorrect.
b. H-S-H: This option shows two hydrogen atoms bonded to a sulfur atom. This satisfies the electron requirements for both elements. The resulting molecule is hydrogen sulfide (H2S). This option is correct.
c. H-S-H | H: This option also shows two hydrogen atoms bonded to a sulfur atom. However, it includes an extra hydrogen atom attached to one of the hydrogen atoms bonded to sulfur. This option is incorrect as it does not correspond to any known molecule.
d. H | H-S-H | H: This option shows three hydrogen atoms bonded to a sulfur atom. Once again, this satisfies the electron requirements for both elements. The resulting molecule is also hydrogen sulfide (H2S). This option is correct as well.
e. H=S=H: This option represents a double bond between sulfur and hydrogen, with each atom having a single hydrogen atom attached. This would imply that sulfur has a bonding capacity of 4, which is not consistent with its electron configuration or known chemistry. Therefore, this option is incorrect.
In summary, the molecules formed when an atom of sulfur reacts with atoms of hydrogen are hydrogen sulfide (H2S). Hence, options b and d are correct.