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Which of these electron configurations would indicate a diamagnetic atom?
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∙ 11y ago
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∙ 14y agoWiki User
∙ 11y agoMg[Ne] 3s-2
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∙ 11y agoMg[Ne] 3s2
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Which of the following outer electron configurations would you expect to belong to a reactive metal?
Francium, Fr.
Which of the following configurations would form a bent molecule?
a molecule with two bound atoms and one lone electron pair -apex
How would the electron configurations for sulfur end?
The atomic number for sulfur is 16. That means that its electron configuration is 1s2 2s2 2p6 3s2 3p4. This can be shortened to [Ne] 3s2 3p4, which shows you that 3s2 3p4 is how sulfur's electron configuration ends.
What element is an alkaline earth metal whose electron configuration ends in 6s2?
All alkaline earth metals have electron configurations ending in s2; 6s2 would be the alkaline earth metal in period 6 of the PTE, which is barium.
How many unpaired electrons are in neon atom?
There are 0 unpaired electrons which would make it diamagnetic
Would baryllium be attracted to a magnet?
No, because it is diamagnetic.
Which of the following outer electron configurations would you expect to belong to a reactive metal?
Francium, Fr.
Is bromine Paramagnetic or diamagnetic?
Bromine is paramagnetic. This is because the 4p subshell has a value of 4p5. 5 electrons in a p subshell (which has space for 6), means the last electron is unpaired. The unpaired electron gives it the property of paramagnetism. Alternatively, Selenium is diamagnetic, as it has the outer subshell 4p4, meaning no electrons are unpaired.
Is fluorine paramagnetic?
Fluorine gas is diamagnetic as there are no unpaired electrons A neutral atom of flurine would be paramagnetic as due to the presence of 1 unpaired electron in a 2p atomic orbital
Which of the following configurations would form a bent molecule?
a molecule with two bound atoms and one lone electron pair -apex
Is chlorine a paramagnetic element?
Yes, Chlorine is a paramagnetic element. The electron configuration of Chlorine is 1s(2)2s(2)2p(6)3s(2)3p(5) which contains an unpaired electron in the 3p orbital. Atoms with unpaired electrons are said to be paramagnetic.
Is Mercury often used in magnets?
Mercury is not a magnetic matertial. Notes indicate that it is weakly diamagnetic, i.e. it is repulsed by magnetic fields. So some mercury alloys would also be weakly diamagnetic. Notes indicate that at very low temperatures (4K), mercury becomes a superconductor and it becomes a much stronger diamagnet (repelled). Apparently this magnetizes the mercury at this low temperature. See links.
How would the electron configurations for sulfur end?
The atomic number for sulfur is 16. That means that its electron configuration is 1s2 2s2 2p6 3s2 3p4. This can be shortened to [Ne] 3s2 3p4, which shows you that 3s2 3p4 is how sulfur's electron configuration ends.
Is phosphorus 3p orbital half full?
Yes. If you would like a periodic table that has electron configurations on it, click on related links to get one that is printable.
Which configurations would form a bent molecule?
A molecule with two bound atoms and one line electron pair
Why nitrogen is diamagnetic while contains unpaired electrons?
If you are going by the electron configuration of nitrogen then the unpaired electrons in the 2p shell would indicate that it is paramagnetic. However experiments show that it is diamagnetic. You must remember that nitrogen is a diatomic element and as such is found as N2. The molecular orbital theory explains how there are no unpaired electrons in the bonds between the two N atoms. The 1s and 2s molecular orbitals are completely filled and all of the bonding 2p orbitals are also filled. There are no electrons in the any of the 2p anti-bonding orbitals. Seeing a molecular orbital diagram for N2 will clarify what i mean.
What element is an alkaline earth metal whose electron configuration ends in 6s2?
All alkaline earth metals have electron configurations ending in s2; 6s2 would be the alkaline earth metal in period 6 of the PTE, which is barium.
