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Down the group the principal quantum number (n) increases and the valence electrons are farther from the nucleus. Give reason.ī) What is meant by isoelectronic speciesĬ) Select the isoelectronic species from the follow-ing n, O 2, F, Mg 2+, Al 2+, Na +Ī) Atomic radii of alkali metals increases down the group with increase in atomic number. (Say – 2011)Ĭomment on the variation of atomic radius with increase in atomic number in a group.
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With addition of electrons, effective nuclear charge decreases and size increases.Ĭ) Ionisation enthalpy decreases with increase in size of the atom.Ī) A graph showing the variation of atomic Radius with atomic number for alkali metals is given below. of shells, effective nuclear charge increases and hence size of the atom decreases, ie, the size of a cation is less than that of the atom. From the position of the elements their properties can be understood.ī) The physical and chemical properties of the elements are periodic functions of their atomic number.Ī graph of atomic radius versus atomic number is given below: (March – 2011)Ī) What do you understand from this graph?ī) Account for the observation that cations are always smaller than the parent atom while anions are always larger than the parent atom.Ĭ) Using the above graph, how will you account for the variation of ionization enthalpy in a period?Ī) Atomic size decreases with increase in atomic number.ī) With loss of electrons or decrease in no. He left vacant spaces in the original table for elementsto be discovered. (Say – 2010)Ī) Discuss about the main features of Mendeleev’s periodic table.Ĭ) Give the name for the element with atomic number 112.Ī) Mendeleev’s periodic table made the study of chemistry of elements easier and systematic. Hence electron gain enthalpy of F is less negative that of Cl.ĭevelopment of Periodic Table have made the study of elements and their compounds easier. However, adding an electron to the 2p orbital leads to greater repulsion than adding an electron to the larger 3p or bital.
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So, atomic radius decreases from left to right.Ĭ) Within a group electron gain enthalpy becomes less negative down a group. It is because within the period the outer electrons are in the same valence shell and the effective nuclear charge increases as the atomic number resulting in the increased attraction of the electrons to the nucleus. Consequently, it is easier to remove the fourth 2p electrons from oxygen than it is, to remove one of the three 2p electrons from nitrogen.ī) The atomic size generally decreases across a period. (Hund’s rule) whereas in the oxygen atom, two of the four2p electrons must occupy the same 2p orbitals resulting in an increased electron repulsion. This arises because in nitrogen atom, three 2p electrons reside in different atomic orbitals. (March – 2009)ī) State the modern periodic law of elements.Ī) Mendeleev’s Periodic law : The physical and chemical properties of elements are periodic functions of their atomic mass.ī) Modern Periodic law: The physical and chemical properties of elements are a periodic function of their atomic numbers.Īccount for the following: (March – 2010)Ī) Ionization enthalpy of nitrogen is greater than that of oxygen.ī) Atomic radius decreases from left to right in a period.Ĭ) Electron gain enthalpy of F is less negative than that of Cl.Ī) Ionisation enthalpy of nitrogen is greater than that of oxygen.
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Kerala Plus One Chemistry Chapter Wise Previous Questions Chapter 3 Classification of Elements and Periodicity in PropertiesĪ) Who introduced the periodic law of elements for the first time? State the law. Here we have given Plus One Chemistry Previous Questions Chapter 3 Classification of Elements and Periodicity in Properties.
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