Answer:
Differences between Orbit and Orbitals
Orbit
An orbit is the simple planar representation of an electron.
It can be simply defined as the path that gets established in a circular motion by revolving the electron around the nucleus
The shape of molecules cannot be explained by an orbit as they are non-directional by nature.
An orbit that is well-defined goes against the Heisenberg principle.
Orbital
An orbital refers to the dimensional motion of an electron around the nucleus in a three-dimensional motion.
An orbital can simply be defined as the space or the region where the electron is likely to be found the most.
The shapes of the molecules can be found out as they are directional by nature.
An ideal orbital agrees with the theory of Heisenberg’s Principles.
The vapor pressure of a solution will decrease and the freezing point will decrease with an <span>increasing</span> in the amount of dissolved solute. So the answer is third option.
Answer:
C: Mg
Explanation:
Hybridization of atomic orbitals is a fundamental concept introduced by Pauling that describes the mixing of orbitals at an atom which adds a definite direction to the Lewis - shared electron pair or electron chemical - bond concept.
Carbon(C) can hybridized on sp, sp2 and sp3 simply because it's valence shell gives room for it.
For silicon(si), when forming covalent bonds with other atoms, it's 3s and 3p orbitals are mixed with each other to form new hybrid orbitals.
Magnesium in itself doesn't hybridized except in magnesium hydrides.
Boron orbitals(B): when boron forms bonds with three other atoms like borazine, they are hybridized to either the sp2 or hybridized to the sp3 which occurs when boron forms bonds with four atoms just as is in metal borohydrides.
