Interpretation:
The reason for atomic radii of the
Concept introduction:
When increasing
The 4f electrons very incorrectly shield each other from the increased positive charge of the nucleus, so that the effective nuclear charge attracting each electron steadily increases through the
The lanthanum ion (
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Chemistry & Chemical Reactivity
- What two first-row transition metals have unexpected electron configurations? A statement in the text says that first-row transition metal ions do not have 4s electrons. Why not? Why do transition metal ions often have several oxidation states, whereas representative metals generally have only one?arrow_forwardIdentify a cation of a first series transition metal that is isoelectronic with each of the following. (a) Fe3+ (b) Zn2+ (c) Fe2+ (d) Cr3+arrow_forwardWould you expect salts of the gold(I) ion, Au+, to be colored? Explain.arrow_forward
- Identify, based on the position in the periodic table, the actinide elements among those in the following list: Co, Cm, Cd, Ce, Cf.arrow_forwardAssign a reason for each of the following observations:(i) The transition metals (with the exception of Zn, Cd and Hg) are hard and have high melting and boiling points.(ii) The ionization enthalpies (first and second) in the first series of the transition elements are found to vary irregularly.arrow_forwardExplain, using the electron configurations of the elements and ions, why iron is a transition metal but scandium is not, even though they are both d block elements. Write the electronic configurations of vanadium, chromium, nickel and copper. Explain why copper and chromium have unexpected electronic configurations.arrow_forward
- Explain why copper is paramagnetic, but copper(I) ion is diamagnetic in the ground state.arrow_forwardgive an example of tetradentate ligand.arrow_forwardAssign reason for each of the following :(i) Transition elements exhibit paramagnetic behaviour.(ii) Co2+. is easily oxidised in the presence of a strong ligand.arrow_forward
- Please help me, using knowledge of ionization energy and atomic radii, to predict the reactivity of metals within the same group. Think about what would make a metal reactive. Examples can be added if you want to clarify meaning.arrow_forward<p>Explain why transition metals exhibit multiple oxidation states instead of a single oxidation state (like most of the main-group metals).arrow_forwardDescribe the periodic trends in radii and oxidation states of the transition-metal ions, including the origin and effect of the lanthanide contraction.arrow_forward
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