In: Chemistry
What is the number of individual atomic orbitals in each of the following sets? A) 7s B) 5d C) 3p D) 1s Enter your answer with integers separated by commas and with no spaces (for example, 4,4,1).
Are the following statements true or false?
True False Two sigma bonds comprise a double bond.
True False A double bond consists of two pairs of
electrons.
True False Bonds formed from atomic p orbitals are
always sigma bonds.
True False A pi bond restricts rotation about the sigma
bond axis.
True False A triple bond consists of one pi bond and two
sigma bonds.
True False Side-to-side overlap results in a bond with
electron density above and below the bond axis.
Answer-
Number of individual atomic orbitals in each of the following sets-
A) 7s , 7 denotes no of shell means 7th shell and s orbital which has only 1 orbital
B) 5d , 5 denotes no of shell means 5th shell and d orbital which has 5 orbital (dxy,dyz,dzx,dx2-dy2,dz2)
C) 3p ,3 denotes no of shell means 3rd shell and p orbital which has 3 orbital (px,py,pz )
D) 1s , 1denotes no of shell means 1st shell and s orbital which has only 1 orbital.
Number of individual atomic orbitals in each of the given sets (1,5,3,1)
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Reason- since a double bond comprises of one sigma and one pi bond
Reason - since single bond consist of one pair i.e. 2 electrons hence a double bond consist of 2 pairs of electrons.
Reason-because sigma and pi bonds are formation depend on -
a) sigma bonds are formed by head to head overlap like s-s, s-p, s-d or p-d
b)pi bonds are formed by lateral overlap like p-p
Reason-since rotation need comparatively more energy and can deform the bond.
Reason- since A triple bond consists of 2 pi bond and 1 sigma bond.
Reason-since axis involved in the overlap are not along the horizontal axis.