Paramagnetic Materials: These are metals that are weakly attracted to magnets. They include aluminum, gold, and copper. The atoms of these substances contain electrons most of which spin in the same direction but not all . This gives the atoms some polarity.

Whenever two electrons are paired together in an orbital, or their total spin is 0, they are diamagnetic electrons. Atoms with all diamagnetic electrons are called diamagnetic atoms. A paramagnetic electron is an unpaired electron. An atom is considered paramagnetic if even one orbital has a net spin.

Diamagnetic materials align their magnetic fields in the opposite direction to the external magnetic fields. Paramagnetic and ferromagnetic materials align their magnetic fields in the same direction as the external magnetic fields.

For some alkali metals and noble metals, conduction electrons are weakly interacting and delocalized in space forming a Fermi gas. For these materials one contribution to the magnetic response comes from the interaction between the electron spins and the magnetic field known as Pauli paramagnetism.

The Pauli-limiting field is expressed as Bp = ΔSC//surd 2 μB, where μB is the Bohr magneton and ΔSC is the superconducting gap energy. The common relation held in LSCO implies that the superconducting energy scale in cuprate superconductors is governed by a universal mechanism.

If the Electronic configuration of a molecule has only paired or spin paired electrons, then that molecule is said to be Diamagnetic. Here the molecule C2 has all paired electrons in its electronic configuration. So C2 is Diamagnetic. Whereas, B2 molecule has unpaired electrons.

Are zinc atoms paramagnetic or diamagnetic? There are no unpaired electrons. Because there are no unpaired electrons, Zn atoms are diamagnetic.

Zinc is diamagnetic. Diamagnetic means it has no unpaired electrons.

Re: C2+ C2- Therefore, the 8 electrons would fill up both outer orbitals, the s and p orbitals, while for C2- it would only fill up the 1s orbital and have 2 electrons in the 2s orbital. Therefore, C2- has a stronger bond as it is more stable and harder to pull an electron away from it.

Answer. B2 has two unpaired electron so it is paramagnetic whereas C2 has only paired electrons so it is diamagnetic.

Their double bonds are made of two π bonds because four electrons need to be accommodated in each bond. In bond formation only valence electrons or outermost electrons participate. Hence, in C2 molecules only 2π are present. So, the correct answer is “Option C”.

These 4 electrons are in the pi orbitals and thus the two bonds in the C2 molecule will be pi bonds only and no sigma bond.

answer: there is no reason why carbon can’t form a quadruple bond: This model satisfies the Octet Rule and leaves no electrons for further bonding. Valence-bond theory predicts two possible bonding states for C2: a double bond with all electrons paired, and a triple bond with two unpaired electrons.

covalent σ bond

Does C2 actually exist ? Diatomic carbon or dicarbon (C2) exists only at very high temperatures in carbon vapour produced, for example, in electric arcs, in comets, stellar atmospheres and the interstellar medium, and in blue hydrocarbon flames.

c2 molecule exist in space as gas, but under normal environment it cannot exist as 4 electron bonding with another 4 electron (quadruple bond) is not stable due to large repulsion between electron (same charge repel) and is very unstable.

1σ and 2π

1π bond

Molecular orbital theory shows that there are two sets of paired electrons in a degenerate pi bonding set of orbitals. This gives a bond order of 2, meaning that there should exist a double bond between the two carbons in a C2 molecule.

Answer. Carbon with 4 single bonds is sp3. This adds up to give a bond order of 2, meaning that there exists a double bond between the two carbons in a C2 molecule.

If we go on to the valence-bond model, in which bonds result from the overlap of atomic orbitals, we see a better explanation: carbon cannot form a quadruple bond because it doesn’t have enough atomic orbitals pointing in the right directions.