An element ‘E’ has the ionisation enthalpy value of 374 kJ mol⁻¹. ‘E’ reacts with elements A, B, C and D with electron gain enthalpy values of −328, −349, −325 and −295 kJ mol⁻¹, respectively. The correct order of the products EA, EB, EC and ED in terms of ionic character is :

Given below are two statements :Statement (I) : The radii of isoelectronic species increases in the order. Mg2+ F > Br > IIn the light of the above statements, choose the most appropriate answer from the options given below :

Match List-I with List-II. .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-baqh{text-align:center;vertical-align:top} .tg .tg-amwm{font-weight:bold;text-align:center;vertical-align:top} .tg .tg-0lax{text-align:left;vertical-align:top} List - I List - II (A) ${\mathrm{Al}}^{3+}<{\mathrm{Mg}}^{2+}<{\mathrm{Na}}^{+}<{\mathrm{F}}^{-}$ (I) Ionisation Enthalpy (B) $\mathrm{B}<\mathrm{C}<\mathrm{O}<\mathrm{N}$ (II) Metallic character (C) $\mathrm{B}<\mathrm{Al}<\mathrm{Mg}<\mathrm{K}$ (III) Electronegativity (D) $\mathrm{Si}<\mathrm{P}<\mathrm{S}<\mathrm{Cl}$ (IV) Ionic radii Choose the correct answer from the options given below :

Which of the following electronegativity order is incorrect?

Given below are two statements :Statement I : According to the Law of Octaves, the elements were arranged in the increasing order of their atomic number.Statement II : Meyer observed a periodically repeated pattern upon plotting physical properties of certain elements against their respective atomic numbers.In the light of the above statements, choose the correct answer from the options given below :

Given below are two statements : Statement (I) : An element in the extreme left of the periodic table forms acidic oxides. Statement (II) : Acid is formed during the reaction between water and oxide of a reactive element present in the extreme right of the periodic table. In the light of the above statements, choose the correct answer from the options given below :

The element that does not belong to the same period of the remaining elements (modern periodic table) is:

Given below are the atomic numbers of some group 14 elements. The atomic number of the element with lowest melting point is :

Which of the following statements are NOT true about the periodic table? A. The properties of elements are function of atomic weights. B. The properties of elements are function of atomic numbers. C. Elements having similar outer electronic configurations are arranged in same period. D. An element's location reflects the quantum numbers of the last filled orbital. E. The number of elements in a period is same as the number of atomic orbitals available in energy level that is being filled. Choose the correct answer from the options given below:

The successive 5 ionisation energies of an element are $800,2427,3658,25024$ and $32824\mathrm{kJ}/\mathrm{mol}$, respectively. By using the above values predict the group in which the above element is present :

Given below are two statements : Statement (I) : The first ionization energy of Pb is greater than that of Sn . Statement (II) : The first ionization energy of Ge is greater than that of Si . In the light of the above statements, choose the correct answer from the options given below :

The incorrect decreasing order of atomic radii is

Consider the following elements $\mathrm{In},\mathrm{Tl},\mathrm{Al},\mathrm{Pb},\mathrm{Sn}$ and Ge . The most stable oxidation states of elements with highest and lowest first ionisation enthalpies, respectively, are

The atomic number of the element from the following with lowest 1st ionisation enthalpy is :

Given below are two statements:Statement I: H2Se is more acidic than H2TeStatement II: H2Se has higher bond enthalpy for dissociation than H2TeIn the light of the above statements, choose the correct answer from the options given below:

Given below are two statements : Statement (I) : The metallic radius of Al is less than that of Ga . Statement (II) : The ionic radius of ${\mathrm{Al}}^{3+}$ is less than that of ${\mathrm{Ga}}^{3+}$. In the light of the above statements, choose the most appropriate answer from the options given below :

The property/properties that show irregularity in first four elements of group-17 is/are (A) Covalent radius (B) Electron affinity (C) Ionic radius (D) First ionization energy Choose the correct answer from the options given below :

The number of valence electrons present in the metal among $\mathrm{Cr},\mathrm{Co},\mathrm{Fe}$ and Ni which has the lowest enthalpy of atomisation is :

The group 14 elements $A$ and $B$ have the first ionisation enthalpy values of 708 and $715\mathrm{kJ}{\mathrm{mol}}^{-1}$ respectively. The above values are lowest among their group members. The nature of their ions ${\mathrm{A}}^{2+}$ and ${\mathrm{B}}^{4+}$ respectively is

Electronic configuration of four elements A, B, C and D are given below : (A) $1s^{2}2s^{2}2p^3$ (B) $1s^{2}2s^{2}2p^4$ (C) $1s^{2}2s^{2}2p^5$ (D) $1s^{2}2s^{2}2p^2$ Which of the following is the correct order of increasing electronegativity (Pauling's scale)?