Group 17 Elements General Introduction – Electronic configuration and general trends in physical and: NEET MCQs with Answers

9 free questions on Group 17 Elements General Introduction – Electronic configuration and general trends in physical and for NEET (UG), starting with previous-year NEET and AIPMT questions. Try each one, then tap Show answer for the answer and a short explanation.

Syllabus covered: Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group.

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Question 1

Previous-year question
Identify the incorrect statement among the following. [Re-NEET 2024]
  1. The acidic strength of HX (X = F, Cl, Br and I) follows the order: HF > HCl > HBr > HI
  2. Fluorine exhibits −1 oxidation state whereas other halogens exhibit +1, +3, +5 and +7 oxidation states also.
  3. The enthalpy of dissociation of F₂ is smaller than that of Cl₂
  4. Fluorine is a stronger oxidising agent than chlorine.
Show answer
Answer: (A) The acidic strength of HX (X = F, Cl, Br and I) follows the order: HF > HCl > HBr > HI
Explanation: The acidic strength of hydrogen halides increases down the group as the H–X bond dissociation enthalpy decreases: HF HCl > HBr > HI is incorrect. Fluorine shows only −1 while the other halogens also show +1, +3, +5 and +7; the F–F bond enthalpy is lower than Cl–Cl due to lone-pair repulsion; and F₂ is the strongest oxidising agent.

Question 2

Previous-year question
Which of the following statements is not true for halogens? [NEET 2018]
  1. All form monobasic oxyacids
  2. All are oxidising agents
  3. Chlorine has the highest electron-gain enthalpy
  4. All but fluorine show positive oxidation states
Show answer
Answer: (A) All form monobasic oxyacids
Explanation: Most halogen oxyacids (HOX, HXO₂, HXO₃, HXO₄) are monobasic, but iodine also forms periodic acid H₅IO₆, which is not monobasic, so "all form monobasic oxyacids" is not true. All halogens are oxidising agents and chlorine has the most negative electron-gain enthalpy.

Question 3

Previous-year question
Match the interhalogen compounds of column-I with the geometry in column-II: 1. XX′, 2. XX′₃, 3. XX′₅, 4. XX′₇ with (i) T-shape, (ii) pentagonal bipyramidal, (iii) linear, (iv) square pyramidal, (v) tetrahedral. [NEET 2017]
  1. 1–(iii), 2–(i), 3–(iv), 4–(ii)
  2. 1–(v), 2–(iv), 3–(iii), 4–(ii)
  3. 1–(iv), 2–(iii), 3–(ii), 4–(i)
  4. 1–(iii), 2–(iv), 3–(i), 4–(ii)
Show answer
Answer: (A) 1–(iii), 2–(i), 3–(iv), 4–(ii)
Explanation: Diatomic interhalogens are linear, XX′₃ is T-shaped, XX′₅ is square pyramidal and XX′₇ is pentagonal bipyramidal.

Question 4

Previous-year question
Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules? [NEET 2016]
  1. I₂ > Br₂ > Cl₂ > F₂
  2. Cl₂ > Br₂ > F₂ > I₂
  3. Br₂ > I₂ > F₂ > Cl₂
  4. F₂ > Cl₂ > Br₂ > I₂
Show answer
Answer: (B) Cl₂ > Br₂ > F₂ > I₂
Explanation: F₂ has an anomalously low bond enthalpy because of lone-pair repulsion in the small molecule, giving Cl₂ > Br₂ > F₂ > I₂.

Question 5

Previous-year question
The variation of the boiling point of the hydrogen halides is in the order HF > HI > HBr > HCl. What explains the higher boiling point of hydrogen fluoride? [AIPMT 2015]
  1. The electronegativity of fluorine is much higher than for other elements in the group.
  2. There is strong hydrogen bonding between HF molecules.
  3. The bond energy of HF molecules is greater than in other hydrogen halides.
  4. The effect of nuclear shielding is much reduced in fluorine which polarises the HF molecule.
Show answer
Answer: (B) There is strong hydrogen bonding between HF molecules.
Explanation: Association of HF molecules through strong hydrogen bonds requires extra energy to break, raising the boiling point.

Question 6

Previous-year question
Which order is correct for the bond dissociation enthalpy of halogen molecules? [AIPMT, 2016]
  1. I₂ > Br₂ > Cl₂ > F₂
  2. Cl₂ > Br₂ > F₂ > I₂
  3. Br₂ > I₂ > F₂ > Cl₂
  4. F₂ > Cl₂ > Br₂ > I₂
Show answer
Answer: (B) Cl₂ > Br₂ > F₂ > I₂
Explanation: Cl₂ has the highest bond enthalpy; F₂ is anomalously low due to lone-pair repulsion, giving Cl₂ > Br₂ > F₂ > I₂.

Question 7

Previous-year question
Among the following the correct order of acidity is: [AIPMT, 2016]
  1. HClO₃ < HClO₄ < HClO₂ < HClO
  2. HClO < HClO₂ < HClO₃ < HClO₄
  3. HClO₃ < HClO₂ < HClO < HClO₄
  4. HClO₄ < HClO₂ < HClO < HClO₃
Show answer
Answer: (B) HClO < HClO₂ < HClO₃ < HClO₄
Explanation: Acidity of the oxoacids of chlorine increases with oxidation state: HClO < HClO₂ < HClO₃ < HClO₄.
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Question 8

The white precipitate of AgCl dissolves in aqueous ammonia to give a soluble complex. Which silver halide is the least soluble in aqueous ammonia?
  1. AgI
  2. AgF
  3. AgCl
  4. AgBr
Show answer
Answer: (A) AgI
Explanation: AgCl dissolves because Ag⁺ forms the soluble complex [Ag(NH₃)₂]⁺. AgI has by far the smallest solubility product among these halides, so it supplies too little Ag⁺ for complex formation to dissolve it. AgF, in contrast, is freely soluble in water, so AgI is the one that remains undissolved.

Question 9

HOCl, HOBr and HOI all contain the halogen in the +1 oxidation state. How do their acid strength and oxidising power compare?
  1. Acid strength: HOI > HOBr > HOCl; Oxidising power: HOI > HOBr > HOCl
  2. Acid strength: HOCl > HOBr > HOI; Oxidising power: HOI > HOBr > HOCl
  3. Acid strength: HOCl > HOBr > HOI; Oxidising power: HOCl > HOBr > HOI
  4. Acid strength: HOI > HOBr > HOCl; Oxidising power: HOCl > HOBr > HOI
Show answer
Answer: (C) Acid strength: HOCl > HOBr > HOI; Oxidising power: HOCl > HOBr > HOI
Explanation: With the oxidation state fixed, the electronegativity of the halogen decides the acid strength. Chlorine, the most electronegative of the three, withdraws electron density from the O–H bond most strongly, so HOCl releases H⁺ most easily. Oxidising power falls in the same direction, giving HOCl > HOBr > HOI for both properties.

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