Home
Class 9
CHEMISTRY
overset(24)underset(12)Mg and overset(26...

`overset(24)underset(12)Mg` and `overset(26)underset(12)Mg` are symbols of two isotopes of magnesium. Compare these isotopes with respect to:
(i) composition of the nuclei
(ii) Electronic configuration and valence
(iii) Chemical properites
(iv) Physical properites.

Text Solution

Verified by Experts

(i) The nuclei of the isotops have the same numebr of protons (12) but different numbr of neutrons (12,14 respectively)
(ii) Both the isotopes have same electonic configuration of their atoms i.e 2(K) 8(L) 2(M) .They have same valence (2) as well
(iii) Since the chemical properties are related to the electronic configuration these two isotoes have the same chemical properties
(iv) Since the two isotopes differ in theri mass numbers they have different physical propertisdes .
Promotional Banner

Topper's Solved these Questions

  • STRUCTURE OF ATOM

    DINESH PUBLICATION|Exercise N.C.E.R.T In Text Problems|13 Videos
  • STRUCTURE OF ATOM

    DINESH PUBLICATION|Exercise N.C.E.R.T End Exercise|19 Videos
  • MATTER IN OUR SURROUNDINGS

    DINESH PUBLICATION|Exercise (LAQs) Long Answer Questions|5 Videos

Similar Questions

Explore conceptually related problems

Two elements X and Y belong to group 1 and 2 respectively in the same period of periodic table. Compare these elements with respect to (i) number of electrons in their outermost orbits (ii) their valencies (iii) metallic character (iv) their atomic size (v) formula of their chlorides (vi) formula of their sulphates

(a). Write down the electronic configuration of (i) magnesium atom, and (ii) magnesium ion, (At No. of Mg=12) ,brgt (b). Write down the electronic configuration of (i) sulphur atom, and (ii) sulphide ion. (At. No. of S=16).

You are given a n element overset(16)underset(8)X . Find out (a) Number of protons electrons and neutrons in X. (b) Valency of 'X'. Write the chemical formula of the compound formed when 'X' reacts with(i) hydrogen,(ii) carbon.

The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom is called as first ionization energy (IE_(1)) . Similarly the amount of energies required to knock out second, third etc. electrons from the isolated and IE_(3)gt IE_(2)gt IE_(1) . (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (b) electronic configurations (exactly half filled and completely filled configurations are extra stable) are the important factors which affect the ionisation energies. Similarly, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to from gaseous anion is called electron affinity. (X(g)+e^(-)(g)rarr X^(-)(g)+ energy A positive elecrton affinity idicates that the ion X^(-) has a lower more negative energy than the neutral atom X. The second electron affinity for the addition of a second electron to an initially neutral atom is negative because the electron replusion outweights the nuclear attraction, e.g., O(g)+e^(-)overset("Exothermic")rarr O^(-)(g),E_(a)=+141 kJ mol^(-) ....(i) O^(-)(g)+e^(-)overset("Excothermic")rarr, E_(a)=-780 kJ mol^(-) ...(ii) The electron affinity of an element depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, in a group, ionisation energy and electron affinity decrease as the atomic size increases. The members of third period have some higher (e.g., S and Cl) electron affinity values than the members of second period (e.g., O and F) because second period elements have very small atomic size. Hence, there is tendency of electron-electron repulsion, which resultss in less evolution of energy in the formation of correcsponding anion. The first ionisation energy of Na, Mg,AI and Si are in the order of:

overset((i)Mg//ether(ii)PhCHO)underset((iii)H_(3)O^(+))rarr Products