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What else can I help you with?
Do you expect Be2 1 to exist in the gas phase?
Yes, Be2-1 exists in the gas phase.
Why B2 is paramagnetic while C2 is not?
B2 is paramagnetic due to the presence of unpaired electrons in its molecular orbital configuration. In B2, the molecular orbitals are filled as follows: σ(1s)², σ(1s)², σ(2s)², σ(2s)², and then σ(2p)², π(2p)², leading to two unpaired electrons in the π(2p) orbitals. In contrast, C2 has all its electrons paired, resulting in a completely filled set of molecular orbitals: σ(1s)², σ(1s)², σ(2s)², σ(2s)², σ(2p)², and π(2p)². Thus, C2 is diamagnetic because it lacks unpaired electrons.
Is cesium positive or negative?
it is paramagnetic (go to wikipedia for more info)
How many numbers BETWEEN 8 and 171?
If you include 8 and 171, there would be 171-8+1 = 164 If you dont include both, it would be2 less -> 162
Is a paper clip paramagnetic?
No, just very weakly ferromagnetic. Unless your paperclip is made out of NH4[Fe(SO4)2]·12H2O.
Is Be2 4- paramagnetic or diamagnetic?
Diamagnetic
Is Be2- paramagnetic or diamagnetic?
It is paramagnetic because it has unpaired electrons.
Is sulfur paramagnetic or diamagnetic?
diamagnetic
Is calcium paramagnetic or diamagnetic?
Calcium is diamagnetic.
Is tungsten paramagnetic or diamagnetic?
Tungsten is diamagnetic.
Is b2 paramagnetic or diamagnetic?
B2 is paramagnetic.
Is vanadium paramagnetic or diamagnetic?
Vanadium is paramagnetic.
Is vanadium (V3) paramagnetic or diamagnetic?
Vanadium (V3) is paramagnetic.
Is argon paramagnetic?
No, argon is not paramagnetic. Paramagnetic materials have unpaired electrons, which argon does not have. Argon is a noble gas with a full electron shell, making it diamagnetic.
Is sodium diamagnetic or paramagnetic?
Sodium is diamagnetic, which means it has no unpaired electrons and is weakly repelled by a magnetic field.
SO3 2- is diamagnetic or paramagnetic?
Diamagnetic. All of the electrons are paired.
How can one determine whether a molecule is paramagnetic or diamagnetic?
Paramagnetic molecules have unpaired electrons, while diamagnetic molecules have all paired electrons. One can determine if a molecule is paramagnetic or diamagnetic by examining its electron configuration and counting the number of unpaired electrons. If there are unpaired electrons, the molecule is paramagnetic; if all electrons are paired, the molecule is diamagnetic.
