1. Answer: For sulfur to attain a noble gas configuration, it must gain TWO ELECTRONS.
EXPLANATION:
The noble gases are the only group of elements that have complete number of electrons in their outermost shells, this make them to be stable hence they don't normally participate in chemical reactions. Other elements participate in chemical reactions in order to form bonds with one another with the aim of attaining noble gas octet structure. The octet structure states that a stable element must have eight (8) electrons in its outermost shell.
The atomic number of sulfur is 16 and its electronic configuration is 2,8,6. The electronic configuration shows that sulfur has 6 electrons in its outermost shell, thus, it needs two more electron in order to have 8 electrons in its outermost shell.
2. Answer: When sulfur gain two electrons it will attain the electronic configuration of ARGON.
EXPLANATION
Sulfur needs two electrons to attain the octet structure. When sulfur gain two electrons, the total number of electrons in its atoms will become 16 + 2, which is equal to 18 and its electronic configuration will be 2, 8, 8. The atomic number of the noble gas argon is also 18, thus, sulfur will attain the electronic structure of argon if it gains two electrons.
Answer:
Explanation:
Sulfur is a non-metal that belongs the group VI on the periodic table. Their general valence shell configuration is ns²np⁴. This group has six electrons in their valence or outermost shell. To attain nobility, the would require eight electrons to complete their octet.
The valence shell of sulfur belongs to the L-orbital and it has a maximum capacity of eight electrons.
To complete the octet of the outermost shell, S would require two electrons from a donating or sharing atom.
If sulfur gains two electrons, it would perfectly resembles Argon(18)
The electronic configuration would be: 1S²2S²2P⁶3S²3P⁶
