Answer:
The orbital shapes are actually representation of (Ψ)2 all over the orbit simplified ... ψnlml(r,θ,ϕ)=Rnl(r)Ymll(θ,ϕ) , ... and thus it is directly linked to the angular and radial nodes. ... for different quantum values(which can be assigned to different orbitals are ) .... The two types of nodes are angular and radial.
Explanation:
hope it helps
A) 120 mm
B) 127 mm
C) 914.4 mm
D) 1000 mm
E) 3048 mm
Answer:
B.) Trigonal planar
Explanation:
This molecule has 3 bonds and no lone pairs. The angles are all 120° and the bonds are within the same plane. These molecules have the molecular shape of trigonal planar.
Rounded to 1 significant figure, 25 m would go to 30. This is because 0 isn't significant, so the 3 is the only significant figure.
Answer:
Explanation:
is insufficient to overcome intermolecular forces.