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Among the following isostructural compounds, which one has highest lattice energy ?
Smaller is the size of ion, higher is the lattice energy.
A sbonded molecule MX3 is T-shaped. The number of non-bonding pairs of electrons is :
For a T-shaped molecule like MX3, the central atom M has 3 bonding pairs and 2 non-bonding pairs of electrons. The presence of 2 non-bonding electron pairs gives the molecule a T-shaped geometry, as the bonding pairs occupy more space and push the non-bonding pairs towards the corners.
In a chemical change from the hybrid state of P changes from:
In PCl3, the hybridised state of P is sp3 while in PCl5, the hybridised state of P is sp3d
The geometrical arrangement and shape of are respectively
which is the incorrect about bond angles ?
NH3 - 107 ,
NF3 ,102,
PH3 - 93,
PF3- 97
H2O- 104.5
Which molecules/ions are most paramagnetic?
Use MOT
B2 is most paramagnetic due to presence of two unpaired electrons.
Which has linear shape but not sp hibridisation ?
In & , the hibridisation state of central atom is sp3d but shape is linear.
Which of the following structure is most expected for the molecule XeOF4 ?
XeOF4 is an oxyfluoride of xenon, with xenon in the +6 oxidation state. The molecule has a square pyramidal shape, with the xenon atom at the center, surrounded by 4 fluorine atoms in a square planar arrangement and 1 oxygen atom at the apex.
Which has highest bond energy ?
CO is not a homo-nuclear atom like C2, N2 or even O3, O3 (both these categories are different: with and without 2s-2p mixing). So there is a large discrepancy in the atomic energy levels of 2s, 2p e- of C and O.As a result, 2p(pi)x, 2p(pi)y and 2p(sigma)z have lower energy than 2s(sigma)*. So the e- lost is from 2s(sigma)*2 and not 2p(sigma)z. And hence the bond order increases from 3 to 3.5 and not decreases to 2.5 . (The typical school textbook formula doesn't work for species like CO,CO+ and even NO,NO+ in many situations)
Which has highest bond angle ?
Fact, 2nd period element having min lone pair ,is having max bond angle
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