List of top Chemistry Questions on Periodic properties

In which of the following, elements are arranged in the correct order of their first electron gain enthalpy values?
Identify the correct order of the given compounds against the given property:
Which of the following orders is not correct for the given property?
Which of the following is not a periodic property?
The correct order of C, N, O and F in terms of second ionisation potential is
Given below are two statements:
Statement I: $\mathrm{K>Mg>Al>B}$ is the correct order in terms of metallic character.
Statement II: Atomic radius is always greater than the ionic radius for any element.
In the light of the above statements, choose the correct answer from the options given below:
Given below are two statements:
Statement I: The first ionization enthalpy of Cr is lower than that of Mn.
Statement II: The second and third ionization enthalpies of Cr are higher than those of Mn.
In the light of the above statements, choose the correct answer from the options given below:
The correct polarity order among the following is?
Which of the following has the highest melting point?
Out of \( \mathrm{N, P, S, Cl, F} \), number of valence electrons in the {least metallic element and most metallic element respectively is: }
The correct order of electron gain enthalpy (magnitude only) for group 16 elements is:
Correct order of 2$^{nd}$ ionisation energy is:
The correct order of ionization energy of Cl, S, P, Al, Si is:
Consider the following statements about group 13 elements of the periodic table. (A) Electronegativity decreases down the group.
(B) Size increases down the group.
(C) Ionization energy decreases down the group.
(D) Boiling point of Boron is maximum.
(E) Melting point of Boron is maximum.
Correct order of ionisation enthalpy is:
The correct order of ionisation energy of Cl, S, P, Al, Si is:
In period 4 of the periodic table which elements have the lowest and highest atomic radii respectively?
Given below are two statements: Statement I: The correct order for radius is \( \text{Al}>\text{Mg}>\text{Mg}^{2+}>\text{Al}^{3+} \). Statement II: Atomic size always depends on electronegativity. In the light of the above statements, choose the correct option.
Electronegativity difference between a group 15 element and $\text{P}$ is less than electronegativity difference between another group 15 element and $\text{P}$. Those group 15 elements respectively are :
Which of the following is the correct order with respect to the property indicated?
$K_2Cr_2O_7 + KI \xrightarrow{H^+} I_2 + Cr^{3+}$
Statement-I : Size of $O^{2-}$ is smaller than $F^-$.
Statement-II: Second ionization energy of $\text{Na}$ is greater than second ionization energy of $\text{Mg}$.
Four elements from the second period Boron to Oxygen can have the following IE$_1$ values (in kJ mol$^{-1}$): 1086.5, 800.6, 1313.9, 1402.3. The value of IE$_1$ for Nitrogen is:
Given below are two statements: Statement-I: The correct order for radius is \[ \mathrm{Al > Mg> Mg^{2+} > Al^{3+}} \] Statement-II: Atomic size always depends on electronegativity. In the light of the above statements, choose the correct option.
Which element releases electrons most easily (lowest ionization enthalpy)?
Rank elements Li, Be, B, C in increasing first ionization energy: