Molecular Orbitals of Oxygen
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- O−2
- O2−2
- Both are paramagnetic
- Both are diamagnetic
(Round off to the Nearest Integer).
- CO, NO
- O2, NO+
- CN−, CO
- N2, O−2
- Zero
- 1
- 2
- 3
According to molecular orbital theory, the species among the following that do not exist are:
N2, N+2, N−2, N2+2
Which is more covalent ?
- 0
- 2
- 1
- 3
- σ− orbital
- π− orbital
- π∗− orbital
- σ∗− orbital
In O−2, O2 and O2−2 molecular species, the total number of anti-bonding electrons respectively are:
7, 6, 8
1, 0, 2
6, 6, 6
8, 6, 8
- 3
- 2
- 5
- 4
- −0.75, 1.25
- - 0.75, 1.0
- - 0.75, 0.6
- - 3, 1.25
- π∗ orbitals
- σ∗ orbitals
- σ orbitals
- π orbitals
What are the different rules for filling up the orbitals? Explain each rule in detail.
Calculate EAN of cobalt (Z=27) in [CO(NH3)6]+3 and of zinc (Z=30) in [Zn(NH3)4]SO4
(I) VCl3 (II) VOSO4 (III) Na3VO4 (IV)
[V(H2O)6]SO4.H2O
- III < II < I < IV
- III < IV < III < I
- II < III < I < IV
- IV < I < II < III
Name an element that has two shells, each one of which is completely filled with electrons.
- 1
- 6
- 8
- 10
Carbon forms million of compounds because of its tetravalent and capacity of _ ?
In O−2, O2 and O2−2 molecular species, the total number of anti-bonding electrons respectively are:
1, 0, 2
7, 6, 8
6, 6, 6
8, 6, 8
According to type of overlapping covalent bonds can be classified as: (a) σ bond (b) π bond (c) δ bond.
Which of the following set of orbitals does not produce nodal plane in xz–plane?
- dyz+dyz
- dxy+dxy
- py+dxy
- None of these
- −0.75, 1.25
- - 0.75, 1.0
- - 0.75, 0.6
- - 3, 1.25
- Zero
- 1
- 2
- 3
- 0
- +1
- −1
- −2
6s, 5d, 6p, 7s, 5f
- 6s<6d<5d<5f<7s
- 6s<5d<6p<7s<5f
- 6s<7s<5d<5f<6p
- 6d<5f<6s<6p<7s
- t22ge2g
- t42ge0g
- t32ge1g
- t02gt4g
b. p−CH3O−C6H4−+CH2
c. p−Cl−C6H4−+CH2
d. C6H5−+CH2
Correct order of stability of above species is:
- b > a > c > d
- b > d > c > a
- c > d > a > b
- a > b > c > d
Give reasons for the following:
A molecule of Carbon tetrachloride has four single covalent bonds.