![]() ![]() Elements a, b, c and d have the following electronic configurations:īelong to the same group of periodic tableģ6. No of electrons in 9 orbitals = 9×2 = 18 = 18 elementsģ5. Justify that the fifth period of the periodic table should have 18 elements on the basis of quantum numbers. Therefore, this elementīelongs to period No.7 and group No.18 along with inert gases.ģ4. In what period and group will an element with Z = 118 will be present?Įlectronic configuration is (1s 2 2s 2 2p 6 3s 2Ħd 10 7s 2 7p 6 ). (ns 2,np 6), and therefore in each period the halogen has Readily accept an electron to get the stable noble gas electronic configuration Having the general electronic configuration of ns 2, np 5 Noble gases have stable ns 2, np 6 configuration, and theĪddition of further electron is unfavourable and requires energy. Will disturb their stable electronic configuration and they have almost zero (1s 2, 2s 2, 2p 3) the addition of extra electron In case of elements such as beryllium (1s 2,2s 2), nitrogen Stable than partially filled valence shell electronic configuration of boron. It is due to the fact that beryllium with completely filled 2s orbital, is more KJ mol −1 respectively contrary to the expectation. However, the actual ionisation energies of beryllium and boron are 899 and 800 It is expected that boron(B) has higher ionisation energy than beryllium since The electronic configuration of atom is one of the important factor which affects the value of ionisation potential and electron gain enthalpy. Ionisation enthalpy of atomic hydrogen = E ∞ − E 1Įnthalpy of atomic hydrogen in terms of kJ mol −1 = 1.686 × 10 3ģ2. Of an electron in the ground state of the hydrogen atom (E 1) = −2.8 × Calculate the ionisation enthalpy of atomic hydrogen in terms of kJ mol -1. Energy of an electron in the ground state of the hydrogen atom is -2.8 x 10 -18 J. Because the electron must be removed against net positiveģ1. Thus the successive ionisation energies, always increases in the Which step will have the highest ionisation energy and why?Įffective nuclear charge of the cation is higher than the corresponding neutralĪtom. Magnesium loses electrons successively to form Mg +, Mg 2+ and Mg 3+ ions. IE 1 represents the first ionisation energy.Ģ8. Neutral gaseous atom in its ground state. Remove the most loosely bound electron from the valence shell of the isolated Ionisation enthalpy is defined as the minimum amount of energy required to "Ionisation enthalpy is defined as the energy required to remove the most loosely bound electron from the valence shell of an atom" Is the definition given below for ionisation enthalpy is correct? It is approximated by the below mentionedĢ7. Net nuclear charge experienced by valence electrons in the outermost shell isĬalled the effective nuclear charge. With same number of electrons are called isoelectronic ions. What are isoelectronic ions? Give examples. Modern periodic law was developed which states that "the physical andĬhemical properties of the elements are periodic functions of their atomicĢ5. Periodic Classification of Elements | Chemistry ![]()
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