Ncert Solutions Chemistry Class 11th
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3.11. What do you understand by isoelectronic species? Name a species that will be iso electronic with each of the following atoms or ions.
(i) F–(ii) Ar (iii) Mg2+(iv) Rb+
3.11. What do you understand by isoelectronic species? Name a species that will be iso electronic with each of the following atoms or ions.
(i) F–(ii) Ar (iii) Mg2+(iv) Rb+
3.11. Species (atoms/ions) which have same number of electrons are called isoelectronic species. The isoelectronic species out of the given atoms/ions are:
(i) Na+ is isoelectronic to F-
(ii) K+ is isoelectronic to Ar
(iii) Na+ is isoelectronic to Mg2+
(iv) Sr2+ is isoelectronic to Rb+
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3.10. How do atomic radii vary in a period and in a group? How do you explain the variation?
3.10. How do atomic radii vary in a period and in a group? How do you explain the variation?
3.10. Across a period, the atomic radii decrease from left to right due to increase in effective nuclear charge from left to right across a period
Within a group, atomic radius increases down the group due to continuous increases in the number of electronic shells or orbit numbers in the structu
Upvote 3.9. What does atomic radius and ionic radius really mean to you?
3.9. What does atomic radius and ionic radius really mean to you?
3.9. Atomic radius: It is the distance from the centre of nucleus to the outer most shell of electrons in the atom of any element. It incorporates both the covalent, metallic radius or van there Waal's radius depending on whether the element is a non-metal or a metal.
Ionic radius: It is the distance
Upvote 3.8. Why do elements in the same group have similar physical and chemical properties?
3.8. Why do elements in the same group have similar physical and chemical properties?
3.8. The elements in a group have same number of valence electrons and hence have similar physical and chemical properties.
Upvote 3.7. Which element do you think would have been named by
(i) Lawrence Berkeley Laboratory
(ii) Seaborg’s group?
3.7. Which element do you think would have been named by
(i) Lawrence Berkeley Laboratory
(ii) Seaborg’s group?
3.7. (i) Lawrencium (Lr) with atomic number (z) = 103
(ii) Seaborgium (Sg) with atomic number (z) = 106.
Upvote 3.6. Write the atomic number of the element present in the third period and seventeenth group of the periodic table.
3.6. Write the atomic number of the element present in the third period and seventeenth group of the periodic table.
3.6. The element is chlorine (Cl) with atomic number (Z) = 17.
Upvote 3.5. In terms of period and group where will you locate the element with z = 114?
3.5. In terms of period and group where will you locate the element with z = 114?
3.5. Elements with atomic numbers from Z = 87 to Z = 114 are present in the 7th period of the periodic table. So, this elements lies in the Period – 7 and Group -14 of Block-p.
Upvote 3.4. On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.
3.4. On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.
3.4. The sixth period means that the highest principal quantum number = 6. The subsequent periods comprise of 8, 18, 18 and 32 elements in the same order. The sixth period comprises of 32 elements where electrons enter the 6s, 4f, 5d and 6p orbitals. Number of orbitals present in 6s=1. 4f=
Upvote 3.3. What is the basic difference in approach between Mendeleev’s Periodic Law and the Modern Periodic Law?
3.3. What is the basic difference in approach between Mendeleev’s Periodic Law and the Modern Periodic Law?
3.3. Mendeleev's periodic law classifies the elements based on their atomic weight. Modern periodic law classifies the elements based on their atomic number.
Upvote 3.2. Which important property did Mendeleev use to classify the elements in this periodic table and did he stick to that?
3.2. Which important property did Mendeleev use to classify the elements in this periodic table and did he stick to that?
3.2. Mendeleev arranged the elements horizontally, in periods and vertically, in groups in the increasing order of their atomic masses. This classification was done in such a way that the elements with similar properties fall in the same group.
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