Advertisements
Advertisements
प्रश्न
Compare the ionization enthalpies of the first series of the transition elements.
Advertisements
उत्तर
Ionization enthalpies of first transition series:
- Ionization energy of the transition element is intermediate between those of s and p block elements.
- As we move from left to right in a transition metal series, the ionization enthalpy increases as expected. This is due to an increase in nuclear charge corresponding to the filling of d electrons.
- The increase in first ionisation enthalpy with increase in atomic number along a particular series is not regular. The added electron enters (n-1) d-orbital and the inner electrons act as a shield and decrease the effect of nuclear charge on valence ‘ns’ electrons. Therefore, it leads to variation in the ionization energy values.
APPEARS IN
संबंधित प्रश्न
Which one of the following ions has the same number of unpaired electrons as present in V3+?
The catalytic behaviour of transition metals and their compounds is ascribed mainly due to ____________.
The correct order of increasing oxidizing power in the series
What are interstitial compounds?
Explain briefly how +2 states become more and more stable in the first half of the first-row transition elements with increasing atomic numbers.
Explain the variation in `"E"_ ("M"^(3+)//"M"^(2+))^0` 3d series.
The `"E"_("M"^(2+)//"M")^0` value for copper is positive. Suggest a possible reason for this.
Which metal in the 3d series exhibits +1 oxidation state most frequently and why?
Why first ionization enthalpy of chromium is lower than that of zinc?
Transition metals show high melting points why?
