Tag: comparison of lanthanoids and actinoids

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Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

Beryllium resembles Aluminium in properties. This is mainly due to:

  1. equal electro negativity values of elements

  2. equal atomic volumes of the elements

  3. equal electron affinity

  4. equal nuclear charges in their atoms
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

Beryllium resembles Aluminium in properties. This is due to similar electronegativity, similar atomic size and they diagonal relationship.

Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

Amphoteric behaviour is shown by the oxides of :

  1. $Al$ and $Ca$
  2. $Pb$ and $Ba$
  3. $Cr$ and $Mg$
  4. $Sn$ and $Zn$
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

Amphoteric oxides can behave as an acid as well as base. They react with both acids and bases to form salts. Tin oxide although doesn't dissolve in water but it is amphoteric in nature. Zinc oxide is also amphoteric in nature.

$ZnO+HCl \rightarrow ZnCl _2+H _2O$
$ZnO+NaOH \rightarrow Na _2ZnO _2+H _2O$
$SnO _2+HCl \rightarrow SnCl _4+H _2O$
$SnO _2+NaOH+H _2O \rightarrow Na _2[Sn(OH) _6]$

Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

If the IP of hydrogen in its ground state is 2.18 x$10^{-18}$ J/atom, then the electron affinity of $Li^{3+}$ ion is :

  1. $-2.18\times$$10^{-18}$J/atom
  2. $-6.54 \times$$10^{-18}$J/atom
  3. $-3.488 \times$$10^{-18}$J/atom
  4. $-1.962\times$$10^{-17}$ J/atom
Reveal answer Fill a bubble to check yourself
D Correct answer
Explanation

E.A of $Li^{+3} = -$I.P of $Li^{+2}$
I.P of $Li^{+2}  = $I.P of $H \dfrac{Z^2}{n^2}$
Therefore, I.P of $Li^{+2}$=$2.18 \times 10^{-18} J/atom \times 9 $ as Z=3
Thus, E.A of $Li^{+3} =-1.962 \times 10^{-17}$ J/atom

Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

If the seventh period is completed, the atomic number of the last element would be:

  1. $118$
  2. $112$
  3. $107$
  4. $120$
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

As the seventh period will be completely filled its electronic configuration must be in the manner of noble gas configuration i.e., $ns^2,: np^6$ because the last element in every period is noble gas element. Hence, the electronic configuration of last element of seventh period is (Rn) $5f^{14} 6d^{10} 7s^27p^6$ as the electronic configuration contains $118$ electrons, the last element in the seventh period will have the atomic number $118$.

Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

Stable electronic configuration of a transition metal is:

  1. $1s^{2} 2s^{2}2p^{6} 3s^{2} 3p^{6} 3d^{9} 4s^{2}$
  2. $1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{5}$
  3. $1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2}$
  4. $1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{10} 4p^{6}$
Reveal answer Fill a bubble to check yourself
B Correct answer
Explanation

Generally the elements having  half filled and completely filled outer electronic configurations are stable  elements,here in given options the configuration $1s^22s^22p^63s^23p^64s^23d^5$ contains half filled outer electronic configuration $(3d^5)$.


Hence option B is correct.

Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

The element with $Z = 106$ belongs to :

  1. $3^{rd}$ period
  2. $ 5^{th}$ period
  3. $7^{th}$ period
  4. $6^{th}$ period
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

$Z=106$ is seaborgium and its electronic configaration is $(Rn) 5f^{14}6d^{4}7s^{2}$. as the differenting electron enter into $7s$, 7 is the principle quantum number which represents the number of period to which the element belongs hence, the element belongs to 7th period.

Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

An atom of element has $2K, 8L$ and $3M$ electrons. Then the element belongs to :

  1. IA group

  2. IIA group

  3. IIIA group

  4. IVA group
Reveal answer Fill a bubble to check yourself
C Correct answer
Explanation

The total number of electrons present in all the shells are $2+8+3=13$, hence the atomic number of element is $13$ and the electronic configuration would be $1s^22s^22p^63s^23p^1 $. Element belongs to $|||A$ group.

Multiple choice chemistry d- and f-block elements actinoids the actinoids the d-and f-block elements comparison of lanthanoids and actinoids

Most of the man-made synthetic elements occur:

  1. in actinide series

  2. in lanthanide series

  3. in coinage metals

  4. in alkaline earth metals
Reveal answer Fill a bubble to check yourself
A Correct answer
Explanation

Synthetic elements, particularly those with high atomic numbers, are often produced through nuclear reactions and are found within the actinide series and beyond (transuranic elements).