sulfide ion ground state electron configuration

The sulphide ion S2− has ground state electronic configuration of 1s22s22p63s23p6.

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What would be the electron configuration of a sulfur ion S − 2?

The electronic configuration of Sulfur is 1 s 2 2 s 2 2 p 6 3 s 2 3 p 4 .

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Which element has the ground state electron configuration 1s 2 2s 2 2p 6 3s 2?

The electron configuration of Mg (atomic number 12) is 1s2 2s2 2p6 3s2. Thus, this option is the correct choice.

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How many electrons are in a sulfide ion S2?

Hence, S2− ion has 16 protons, 16 neutrons and 18 electrons.

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How many electrons are in a sulfur anion S2 −?

Sulfur is a member of the oxygen family and has the atomic number 16. It gains two electrons to form S2− . Therefore the number of electrons and protons in S2− are 18 and 16 respectively.

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What does sulfur anion S2 -) contain?

Now, the sulfide anion, S2− , is formed when two electrons are added to a neutral sulfur atom. As you can see in the configuration of the neutral atom, these two electrons will be added to the 3p-orbitals, which can hold a maximum of six electrons between them.

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What is the electron configuration for sulfur a 1s2 2s2 2p6 3s2 3p4?

The p orbital can hold up to six electrons. We’ll put six in the 2p orbital and then put the next two electrons in the 3s. Since the 3s if now full we’ll move to the 3p where we’ll place the remaining four electrons. Therefore the sulfur electron configuration will be 1s22s22p63s23p4.

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What is the total number of electrons in a S² ⁻ ion?

The total number of electrons in the sulfur anion (S²⁻) will be 2 more than the number of electrons in the sulfur atom because of the -2 charge. The number of electrons in a sulfur atom is 16 then the S²⁻ ion will have 18 electrons.