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Ionization Enthalpy

Consider the ...

Question

Consider the following statements and arrange in the order of true/false as given in the codes.
$S_{1} : N a_{2} O_{2} < M g O < Z n O < P_{4} O_{10} :$ Acidic property.
$S_{2} : N a < M g > A l < S i :$ First ionisation energy.
$S_{3} : F > C l > B r :$ Electron affinity.

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Solution

The correct option is C TTF
$S_{1} : N a_{2} O_{2} < M g O < Z n O < P_{4} O_{10} :$ as non-metallic character increases the acidic character increases. $M g O, N a_{2} O$ are basic, $Z n O$ amphoteric and $P_{4} O_{10}$ acidic.
$S_{2} : N a < M g > A l < S i$ , $M g$ has higher first ionisation energy than $N a$ due to small size and high electron penetration power of s-subshell electrons) and $S i$ has higher ionization energy than $A l a n d M g$ because of higher nuclear charge and small size. $I E_{1} : N a = 496, A l = 577, M g = 737 a n d S i = 786 k J / m o l e$
$S_{3} :$ There is more inter-electronic repulsion in 2p-subshell of fluorine than chlorine (3p). So extra electron will be added easily in 3p-subshell of chlorine as compared to 2p-subshell of fluorine.. Down the group electron affinity values generally decrease with increase in atomic number due to increase in atomic size. So $C l > F > B r .$

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Similar questions

Q. Consider the following statements and arrange in the order of true/ false as given in the codes.

S_{1} : N a_{2} O_{2} < M g O < Z n O < P_{4} O_{10}

: Acidic property.

S_{2}

: Na < Si < Mg < Al: First ionisation energy.

S_{3}

: F > Cl > Br : Electron affinity.

Question 17
Arrange the following elements in the order of their decreasing metallic character
Na, Si, Cl, Mg, Al

(a) Cl > Si >Al > Mg >Na
(b) Na >Mg >Al >Si > Cl
(c) Na > Al > Mg > Cl > Si
(d) Al > Na> Si > Ca> Mg

Arrange the following as per instructions given in the brackets.

(a) Mg. Cl, Na, S, Si (decreasing order of atomic size)

(b) Cs, Na, Li, K, Rb (increasing metallic character)

(d) Cl, F, Br, I (increasing electron affinity)

(e) Cs, Na, Li, K, Rb (decreasing electronegativity)

Q. Consider the following orderings:

I

A l > S i > P > C l

I I

B e < M g < C a < S r

I I I

I < B r < C l < F

I V

{N a}^{+} < {M g}^{2 +} < {A l}^{3 +} < {S i}^{4 +}

Which of these give(s) a correct trend in ionization energy?

Q. Arrange the following in the order given below : Increasing order of ionization potential of

N a, A l, M g, S i

is :

N a < A l < M g < S i

. if true enter 1 ,else enter 0.

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Ionization Enthalpy

Standard XII Chemistry

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Consider the following statements and arrange in the order of true/false as given in the codes. S1:Na2O2<MgO<ZnO<P4O10: Acidic property. S2:Na<Mg>Al<Si: First ionisation energy. S3:F>Cl>Br: Electron affinity.

Consider the following statements and arrange in the order of true/false as given in the codes.
$S_{1} : N a_{2} O_{2} < M g O < Z n O < P_{4} O_{10} :$ Acidic property.
$S_{2} : N a < M g > A l < S i :$ First ionisation energy.
$S_{3} : F > C l > B r :$ Electron affinity.