The tendency to exhibit – 3 oxidation state, decreased down the group in group 15 elements. Explain.
The tendency to exhibit – 3 oxidation state, decreased down the group in group 15 elements. Explain.
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Elements of group 14 (a) exhibit oxidation state of +4 only (b) exhibit oxidation state of +2 and +4
(b)The elements of group 14 have 4 valence electrons. Therefore, the oxidation state of the group is +4. However, as a result of the inert pair effect, the lower oxidation...
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In group 16, the stability of + 6 oxidation state decreases and that of + 4 oxidation state increases down the group. Why
[Hint : Due to inert pair effect.]
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Fluorine exhibit only - 1 oxidation state whereas other halogens exhibit +ve oxidation
[Hint : Due to absence of vacant d-orbitals in the octet of F.]
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Assign a possible reason for the following : (a) Stability of + 5 oxidation state decreased and that of + 3 oxidation
[Hint : (a) Due to inert pair effect. (b) Due to more bond dissociation enthalpy of O H as compared to S H bond. (c) Due to more steric hindrance...
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Which element among 3d series exhibit highest oxidation state ?
The correct answer is Ans. Mn
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Sc, the first member of first transition series does not exhibit variable oxidation state. Why ?
Due to noble gas electronic configuration in + 3 oxidation state no other oxidation state is stable.
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Name the members of the lanthanoid series which exhibit +4 oxidation state and those which exhibit +2 oxidation state.
The lanthanides that exhibit +2 and +4 states are shown in the given table. The atomic numbers of the elements are given in the parenthesis. +2 +4 Nd (60) Ce (58) Sm (62) Pr (59) Eu (63) Nd...
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How would the tendency to lose electrons change as you go (i) from left to right across a period? (ii) down a group?
(a) (i) Tendency to lose electrons decreases. (ii) Increases. (b) The three compounds are X(NO3)2, XSO4 and X3(PO4)2. Valence electrons of element X is 2. Therefore, element X belongs to group 2. It will form...
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Which of the following halogen does not exhibit positive oxidation state in its compounds?
(d) Fluorine exhibit -ve oxidation state
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Explain the following observations: (i) Fluorine does not exhibit any positive oxidation state.
(i) Fluorine does not exhibit any positive oxidation state as it is the most electro-negative element and does not have d orbitals in its valance shell. (ii) This is due to...
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