Tag: group 17

Questions Related to group 17

The comparatively high boiling point of hydrogen fluoride is due to:

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. high reactivity of fluorine

  2. small size of hydrogen atom

  3. formation of hydrogen bonds

  4. small size of fluorine

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Correct Option: C
Explanation:

$F$ being highly electronegative has the ability to form hydrogen bonds due to which boiling point of $HF$ is high.

Which of the following has highest melting point?

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. $SrF _{ 2 }$

  2. $BeF _{ 2 }$

  3. $BaF _{ 2 }$

  4. $MgF _{ 2 }$

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Correct Option: A
Explanation:

The melting point of a compound depends on Vander walls force of attraction which increases as molecular size increases, in given compounds Sr atom has the largest size, so vanderwalls force of attraction will be greater in $SrF _2$ and it will have the highest melting point.

Which of the following statements is true?

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. $\mathrm{B}\mathrm{r} _{2}$ is more reactive than $\mathrm{Cl} _{2}$

  2. $I _{2}$ is more reactive than $\mathrm{B}\mathrm{r} _{2}$

  3. $\mathrm{C}1 _{2}$ isinsoluble in water

  4. Iodine is a solid

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Correct Option: D
Explanation:

Reactivity oder in halogen is:
$F _2>Cl _2>Br _2>I _2$

So option A and are incorrect.
$Cl _2$ is soluble  in water and $I _2$ is a solid (purple crystals) thus option D is correct.

The element which exists in the liquid state is:

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. bromine

  2. mercury

  3. gallium

  4. all of these

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Correct Option: D
Explanation:

Bromine, mercury and gallium exist in liquid state at room temperature

Which of the following is a solid at room temperature?

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. $\mathrm{Cl} _{2}$

  2. $\mathrm{B}\mathrm{r} _{2}$

  3. $I _{2}$

  4. $\mathrm{F} _{2}$

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Correct Option: C
Explanation:

Halogens

$F _{2}$ gas $Cl _{2}$ gas 


$Br _{2}$ liquid


  $I _{2}$ solid


Option C is correct.

Change in entropy is negative for:

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. $Bromine (I) \rightarrow Bromine (g)$

  2. $C(s)+H _2O(g) \rightarrow CO(g)+H _2(g)$

  3. $N _2(g, 10 \ atm) \rightarrow N _2(g, 1 \ atm)$

  4. $Fe(at \ 400 \ K) \rightarrow Fe(at \ 300 \ K)$

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Correct Option: A
Explanation:

When $Br(I)$ goes to to $Br(g)$ then stability of molecules increase. This leads us to negative entropy.

The halogen which is liquid at room temperature is:

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. Fluorine

  2. Astatine

  3. Bromine

  4. Iodine

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Correct Option: C

Which of the following exists as gas?

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. $Br _{2}$

  2. $I _{2}$

  3. $Cl _{2}$

  4. all of the above

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Correct Option: C
Explanation:

Chlorine is gas, bromine is liquid and iodine is solid.

Which of the following properties of the elements chlorine,bromine and iodine increase with increasing atomic number?

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. Ionization energy.

  2. Ionic radius.

  3. Bond energy of the molecule ${X _2}$.

  4. Enthalpy of vaporization.

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Correct Option: B,D
Explanation:

The ionization energies of halogens decrease on moving down the group.

Similarly the bond dissociation energies decrease from chlorine to bromine to iodine.

With increase in the atomic number, the atomic and ionic radii of hydrogen increases from fluorine to iodine.

Also, the melting points and the boiling points increase in the same order.

Hence, the enthalpy of vaporization also increases in the same order.

Which of the following species has the lowest boiling point?

chemistry group 17 group 17 - physical properties physical properties of group 17 elements group 17 elements: the halogen family

  1. $Cl _2$

  2. $Br _2$

  3. $I _2$

  4. None of these

Show answer
Correct Option: A
Explanation:

Boiling point increases with increasing atomic size. $Cl _2$, thus, has the lowest boiling point.