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Answer is (C) A and B

We did not know about the Nervous control system in 17^th century. 

(A) Reflex arcs

Some major plant hormones and their action are given in the following table. Major plant hormones and their action.

Answer is (C) Axon

B) Cerebellum

(B) Schwann cells

(B) Glial cells

1. cerebrum 

2. synapse 

3. Auxin 

4. General growth rate and metabolic rate

(D) Glial cells

Synapse is the functional region of contact between two neurons.

1. Definition: Synapse is a functional region between two neurons where information from one neuron is transmitted or relayed to another neuron. 

2. Through synaptic region is with minute gaps it does not have any protoplasmic connection between them. 

3. Information is passed from one nerve cell to the other through these gaps either in the form of chemical or electrical signals or both.

(C) dendrite end of one neuron to axon end of adjacent neuron.

i) Auxin 

ii) Thyroxine.

B) Functional region between two neurons

a) The diagram belongs to T.S. of Spinal cord (peripheral).

b) A – Dorsal Root, B – Ventral Root

c) C – Association neuron It analyse the information – and send the order (function) through motor neuron to muscle.

d) Sensory nerve enters through dorsal horn.

a) Hormones in animals and hormones in plants.

b) Adrenal gland.

c) Abscisic Acid (ABA)

d) Cell elongation and differentiation of shoots and roots.

The inner orbital complexes, low spin complexes (or) Spin paired complexes.

The d orbital involved in dsp³ hybridisation of [Fe(CO)₅] is dx²y² .

(d) [Fe (CO)₅] and [Ni (CN)₄]^2- Others are solvate isomersim.

(b) [CO (en)₂ Cl₂] Cl 

(b) [CO(en)₂Cl₂]Cl 

(b) [Ni (CN)₄]^2-

(c) [Cu(NH₃)₄]²⁺

(a) [CO(CN)₆]^3-

Crystal field stabilization energy for high spin d octahedral complex is 0.

The spin only magnetic moment of tetrachlorido manganate (II) ion is 5.9 BM

C) stimulators of ovaries and testes

(A) Hypothalamus

(D) Thigmotropism

(c) Square planar complex

Isomerism is the phenomenon in which more than one coordination compounds having the same molecular formula have different physical and chemical properties due to different arrangement of ligands around the central metal atom.

1. The ligand field causes the splitting of d orbitals of the central metal atom into two sets (t_2g and eg). 

2. When the white light falls on the complex ion, the central metal ion absorbs visible light corresponding to the crystal field splitting energy and transmits rest of the light which is responsible for the colour of the complex. 

3. This absorption causes excitation of d – electrons of the central metal ion from the lower energy t_2g level to the higher energy eg level which is known as d – d transition

1. [CO(NH₃)₄(H₂O)₂]Cl₃

2. K₂[Ni(CN)₄] 

3. [Cr(en)₃]Cl₃

4. [Pt(NH₃)BrCl(NO₂)]^-

5. [PtCl₂(en)₂](NO₃)₂ 

6. Fe₄[Fe(CN)₆]₃

(d) Crystal field theory

In both the complexes, Fe is in +3 oxidation state with the configuration 3d⁵ . CN^- is a strong field ligand. In its presence, 3d electrons pair up leaving only one unpaired electron. The hybridisation is d² sp³ forming inner orbital complex. H₂O is a weak ligand. In its presence 3d electrons do not pair up. The hybridisation is sp³d² forming an outer orbital complex containing five unpaired electrons, hence it is strongly paramagnetic.

(c) Linus Pauling

Limitations of VB – Theory: 

1. It does not explain the colour of the complex 

2. It considers only the spin only magnetic moments and does not consider the other components of magnetic moments. 

3. It does not provide a quantitative explanation as to why certain complexes are inner orbital complexes and the others are outer orbital complexes for the same metal. For example, [Fe(CN₆)]^4- is diamagnetic (low spin) whereas [Fe(CN₆)]^4- is paramagnetic (high spin).

1. The ligand → metal bond in a coordination complex is covalent in nature. It is formed by the sharing of electrons between the central metal atom and electron donor ligand.

2. Each ligand should have atleast one filled orbital containing a lone pair of electrons.

3. In order to accommodate the electron pairs donated by the ligands, the central metal ion present in a complex provides required number of vacant orbitals.

4. These vacant orbitals of central metal atoms undergo hybridisation, the process of mixing of atomic orbitals of comparable energy to form equal number of new orbitals called hybridised orbitals with same energy.

5. The vacant hybridised orbitals of the central metal ion, linearly overlap with filled orbitals of the ligands to form coordinate covalent sigma bonds between the metal and the ligand. 

6. The hybridised orbitals are directional and their orientation in space gives a definite geometry to the complex ion.

7. In the octahedral complexes, if the (n-l)d orbitals are involved in hybridisation they are called inner orbital complexes or low spin complexes (or) spin paired complexes. If the nd orbitals are involved in hybridisation, such complexes are called outer orbital complexes (or) high spin (or) spin free complexes. Here “n” represents the principal quantum number of the outermost shell.

8. The complexes containing a central metal atom with unpaired electron (s) are paramagnetic. If all the electrons are paired, then the complexes will be diamagnetic. 

9. Ligands such as CO, CN^-, en and NH₃ present in the complexes cause pairing of electrons present in the central metal atom. Such ligands are called strong field ligands. 

10. Greater the overlapping between, the ligand orbitals and the hybridised metal orbital, greater is the bond strength.

EDTA,  Lead is used as a chelating ligand for the separation of lanthanides, in softening of hard water and also in removing poisoning.

(c) (iii) only

EDTA is used for the separation of lanthanides, in softening of hard water and also in removing lead poisoning.

(d) Glycine is an amino acid whereas others are complex salts.

(a) Both A and R are correct and R is the correct explanation of A.

(b)  (iii) only

(a) Both A and R are correct and R Is the correct explanation of A.

Cu⁺ , Zn²⁺ have d configuration and Sc³⁺ , Ti⁴⁺ have d¹⁰ configuration. 

2. d – d transition is not possible in the above complexes. So they are colourless.

Ti in [Ti(H₂O)₆]³⁺ is in +3 oxidation state. Sc in [Sc(H₂O)₆]³⁺ is in +3 oxidation state. The outer electronic configuration of Sc, Ti and their trivalent ions are,

SC: 3d¹ 4S² 

SC³⁺ : 3d⁰

Ti: 3d² 4S²

Ti³⁺ : 3d¹

Ti³⁺ has one unpaired electron in 3d orbital and they undergoes d-d transition. This electron can be promoted to a higher energy level by light absorption. Therefore [Ti(H₂O)₆]³⁺ is coloured. In the case of [Sc(H₂O)₆]³⁺ there is no electron in 3d orbital of Sc³⁺ , hence there is no possibility of light absorbance. Therefore [Sc(H₂O)₆]³⁺ is colourless.

1. In [CuI₄]^2- complex, the size of chloride ion is less hence exist. But in [CuI₄]^2- the bigger iodide ion makes the compound unstable.

2. When copper cation comes in contact with iodide anion, iodide get oxidised to iodine molecule hence the formation of the above complex ion does not take place. 

Hence [CuI₄]^2- exists while [CuI₄]^_2- does not exist.

The brain has three divisions:

1. Forebrain: The forebrain consists of the cerebrum, diencephalon.

2. Midbrain: Midbrain has optic lobes.

3. Hindbrain has cerebellum, medulla oblongata.