"The average osmotic pressure of human blood is \(7.8\ atm\) at \(27\ degree C\).
 The concentration of aqueous \(NaCl\) solution that can be used in the bloodstream is:
(Given \(R = 0.082\ L\ atm\ K^{-1}\ mol^{-1}\))"

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In the formation of coordination complexes, if the inner \(d\) orbital \((n-1) d\) is used in hybridisation, the complex, is called an inner orbital or low spin or spin paired complex. And if it uses outer \(d\) orbital ( \(n d\) ) in hybridisation (like \(s p^3 d^2\) ), it is called outer orbital or high spin or spin free complex. The degeneracy of the \(d\) orbitals has been removed due to ligand electron-metal electron repulsions in the complex. This splitting of the degenerate levels due to the presence of ligands in a definite geometry is termed as crystal field splitting. For coordination complexes, the magnetic moment is determined by the number of unpaired electrons and is calculated by using the 'spin-only' formula, \(\mu=\sqrt{n(n+2)}\) where \(n\) is the number of unpaired electrons and \(\mu\) is the magnetic moment in units of Bohr magneton (BM). The coordination compounds are of great importance. These compounds are widely present in the mineral, plant and animal worlds and are known to play many important functions in the area of analytical chemistry, metallurgy, biological systems, industry and medicine.
Which of the following complex has the highest magnetic moment?

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One of the notable features of the transition element is the great variety of oxidation states it may show in its compounds. The elements which give the greatest number of oxidation states occur in or near the middle of the series. Manganese, for example exhibits all the oxidation states from +2 to +7. The lesser number of oxidation states at the extreme ends is either due to losing or sharing of few electrons (Sc, Ti) or too many d electrons of higher valence. Early in the first series scandium (II) is virtually unknown and titanium (IV) which is more stable than Ti (III) or Ti (II). On the other end, the only oxidation state of zinc is \(+ 2\).
Cris reducing but Mn is oxidising in nature although both have \(d ^{ 1 }\) configuration. It is due to the reason that Cr configuration changes from

Extraction of gold and silver involves leaching the metal with \(CN^-\text{}\) ion. This is also a:

\(\text{R-Br} \xrightarrow{\text{Mg, dry Ether}} \text{P} \xrightarrow{\text{EtOH}} \text{Q}\)
What is Q?

Identify the essential amino acids from the following.
(A) Threonine
(B) Serine
(C) Histidine
(D) Lysine
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Which of the following does not belong to the first transition series ?

Observe the figure and answer the following:

The given diagram represents stages (A-E) of development of the embryo sac in angiosperms. Which of the following correctly identifies the structure labelled (ii), (iii), (iv), (v), and (vi) in figure E?

Which of the following statements are correct?
A. Some hormones are steroids.
B. Hyper thyroidism is due to increased level of thyroxine
C. Hypothyroidism can be controlled by reducing ""lodised"" salt intake.
D. Glucagon tends to increase the glucose level in blood.
E. Insulin is released in response to rapid rise in blood glucose level.
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In zwitter ionic form, amino acids show amphoteric behaviour as they react both with acids and bases.
Except glycine, all other naturally occurring \(\alpha\) - amino acids are optically active, since the \(\alpha\) -carbon atom is asymmetric. These exist both in 'D' and 'L' forms. Most naturally occurring amino acids have L-configuration. L-Aminoacids are represented by writing the \(-NH_2\) group on left hand side.
Which of the following amino acid is essential?

Which of the following statement is/are correct for complex \([NiCl_4]^{2-}\) ?
(A) Ni has oxidation state +2
(B) Cl is a weak field ligand
(C) Compound is paramagnetic
(D) \(d s p^2\) hybridisation
(E) Low spin complex
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Evaluate \(: 3^{15} \bmod (7)\)

Periodic abstinence is an example of: