![]() → Write the electronic configuration of Boron → Complete the electronic configuration of beryllium? → Write the electronic configuration of Lithium (3Li) → Complete the subshell electronic configuration? → How many electrons are present in helium ( 2He)? → What may be the maximum number of electrons to be filled in the ‘p’ subshell? → What is the maximum number of electronics that can be accommodated in the ‘s’? → Which subshell is common to all shells? What will be the number of subshells in the ‘M’ shell and ‘N’ → The ‘K’ shell, which is the first shell, has 1 subshell. → What is the maximum number of electrons that can be accommodated in the M Shell? → How many electrons are present in the M shell, the outermost shell of argon? → Write the electronic configuration of sodium and argon and complete the Table. → Is the group 1 element a metal or a nonmetal? → Atomic number of sodium is 11 Electronic configuration – 2,8,1 → What is the basis of classification of elements in the periodic table? Kerala State Syllabus 10th Standard Chemistry Solutions Chapter 1 Periodic Table and Electronic Configuration Periodic Table and Electronic Configuration Text Book Questions and Answers This behavior is in sharp contrast to that of the p-block elements, where the occurrence of two oxidation states separated by two electrons is common, which makes virtually all compounds of the p-block elements diamagnetic.ĭue to a small increase in successive ionization energies, most of the transition metals have multiple oxidation states separated by a single electron.You can Download Periodic Table and Electronic Configuration Questions and Answers, Summary, Activity, Notes, Kerala Syllabus 10th Standard Chemsitry Solutions Chapter 1 help you to revise complete Syllabus and score more marks in your examinations. The occurrence of multiple oxidation states separated by a single electron causes many, if not most, compounds of the transition metals to be paramagnetic, with one to five unpaired electrons. Because of the slow but steady increase in ionization potentials across a row, high oxidation states become progressively less stable for the elements on the right side of the d block. ![]() ![]() Manganese, for example, forms compounds in every oxidation state between −3 and +7. The relatively small increase in successive ionization energies causes most of the transition metals to exhibit multiple oxidation states separated by a single electron. Thus all the first-row transition metals except Sc form stable compounds that contain the 2+ ion, and, due to the small difference between the second and third ionization energies for these elements, all except Zn also form stable compounds that contain the 3+ ion. This in turn results in extensive horizontal similarities in chemistry, which are most noticeable for the first-row transition metals and for the lanthanides and actinides. The similarity in ionization energies and the relatively small increase in successive ionization energies lead to the formation of metal ions with the same charge for many of the transition metals. Trends in Transition Metal Oxidation States As a result, the metals in the lower right corner of the d block are so unreactive that they are often called the “noble metals.” The electronegativity of the elements increases, and the hydration energies of the metal cations decrease in magnitude from left to right and from top to bottom of the d block. \): Some Trends in Properties of the Transition Metals.
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