Tag: group 17 elements: the halogen family

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

Statement I : The physical state of halogen molecules may be solids, liquids or gases at room temperature.
Statement 2 : The halogen molecules are considered as nonpolar and by increasing mass the dispersion forces between them increases.

  1. true, true, correct explanation

  2. true, true, not correct explanation

  3. true, false

  4. false, true
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

Statement I : The physical state of halogen molecules may be solids, liquids or gases at room temperature.
Statement 2 : The halogen molecules are considered as nonpolar and by increasing mass the dispersion forces between them increases. With increase in the dispersion forces, the state changes from gas (fluorine and chlorine) to liquid (bromine) to solid (iodine).

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

The bond energies of $F _{2}, Cl _{2}, Br _{2}$, and $I _{2}$ are 155 kJ $mol^{-1}, \ $244 kJ $mol^{-1}$, 193 kJ $mol^{-1}$ and 151 kJ $mol^{-1}$ respectively. The weakest bond will be in:

  1. $Br _{2}$
  2. $Cl _{2}$
  3. $F _{2}$
  4. $I _{2}$
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Since the bond energy of $I _2$ is least, it's bond will be weakest.

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

Which of the following family exist as diatomic molecules at room temperature?

  1. Alkali metals

  2. Alkaline earth metals

  3. Noble gases

  4. Halogens

  5. Transition metals
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Halogens exist as diatomic molecules at room temperature. The valence shell electronic configuration of halogens is  $\displaystyle ns^2 np^5$.  Two halogen atoms share one electron each to form diatomic molecule in which each halogen atom has completed its octet.

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

The compound IF$ 7$ is named as ________.

  1. iodine heptafluorine

  2. iodine septafluoride

  3. iodine fluoride

  4. none of these
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

$IF _7$ is named as Iodine (VII) Flouride. Because the halogen of larger size give electron pair and the halogen of small size which has high electronegativity accepts a lone pair of electrons. So suffix '-ide' is added to halogen of small size.

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

Statement 1 : Elemental iodine has a higher boiling point than elemental bromine.
Statement 2 : Iodine forms stronger covalent bonds than bromine.

  1. <p>Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.</p>

  2. <p>Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.</p>

  3. <p>Statement 1 is correct but Statement 2 is not correct.</p>

  4. <p>Statement 1 is not correct but Statement 2 is correct.</p>

  5. <p>Both the Statement 1 and Statement 2 are not correct. </p>
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

Statement 1: Elemental iodine has a higher boiling point than the elemental bromine because of the higher molecular mass of $I _2$ than the $Br _2$.
Statement 2: Iodine does not form stronger covalent bonds than $Br$ because size of iodine is larger due to which the bond becomes longer in length and longer bond is weaker, hence, forms weaker covalent bond.

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

Statement 1 : Bromine has a higher boiling point than chlorine.
Statement 2 : Bromine has stronger dispersion forces than chlorine.

  1. <p>Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.</p>

  2. <p>Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.</p>

  3. <p>Statement 1 is correct but Statement 2 is not correct.</p>

  4. <p>Statement 1 is not correct but Statement 2 is correct.</p>

  5. <p>Both the Statement 1 and Statement 2 are not correct. </p>
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

Statement 1 : Bromine has a higher boiling point than chlorine. This is due to the fact that the Bromine has higher , molar mass than the Chlorine.
Statement 2:
Dispersion forces are present between all molecules, whether they are polar or nonpolar.
Larger and heavier atoms and molecules $(Br)$ exhibit stronger dispersion forces than smaller and lighter ones $ (Cl)$
In a larger atom or molecule, the valence electrons are, on average, farther from the nuclei than in a smaller atom or molecule. They are less tightly held and can more easily form temporary dipoles.
The ease with which the electron distribution around an atom or molecule can be distorted is called the polarizability.
London dispersion forces tend to be:
1. stronger between molecules that are easily polarized.
2. weaker between molecules that are not easily polarized.

In short "The more electrons a molecule has, the stronger the London dispersion forcesare. For example, bromine, Br2, has more electrons than chlorine, Cl2, sobromine will have stronger London dispersion forces than chlorine, resulting in a higher boiling point for bromine, 59 oC, compared to chlorine, –35 oC."

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

The solubility of $KCl$ is relatively more in (where D in dielectric constant):

  1. $C _6II _6 (D = 0)$
  2. $(CH _3) _2CO (D = 2)$
  3. $CH _3OH(D= 32)$
  4. $CCl _4 (D = 0)$
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

KCl is an ionic salt that dissolves well in polar solvents with high dielectric constants. Methanol (CH3OH, D=32) has the highest dielectric constant among the options, making it the best solvent for KCl. Benzene (C6H6), acetone ((CH3)2CO, D=2 is incorrect - should be ~21), and carbon tetrachloride (CCl4) all have very low or zero dielectric constants and are poor solvents for ionic compounds.