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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.
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.
What does 76 plus 54 plus 92 plus 88 plus 76 plus 88 plus 75 plus 93 plus 92 plus 68 plus 88 plus 76 plus 76 plus 88 plus 80 plus 70 plus 88 plus 72 equal?
76 plus 54 plus 92 plus 88 plus 76 plus 88 plus 75 plus 93 plus 92 plus 68 plus 88 plus 76 plus 76 plus 88 plus 80 plus 70 plus 88plus 72 equal 1,440
Is Be2 4- paramagnetic or diamagnetic?
Diamagnetic
Is Be2- paramagnetic or diamagnetic?
Be2- ion is diamagnetic because it has a completely filled electron configuration with all paired electrons, resulting in no unpaired electrons to exhibit paramagnetic behavior.
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?
SO3 2- is paramagnetic because it has two unpaired electrons.
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.
