Which of the following sets represents the collection of isoelectronic species?(a)- $N{{a}^{+}},M{{g}^{2+}}A{{l}^{3+}},C{{l}^{-}}$ (b)- $N{{a}^{+}},C{{a}^{2+}}S{{c}^{3+}},{{F}^{-}}$ (c)- ${{K}^{+}},C{{l}^{-}},C{{a}^{2+}}S{{c}^{3+}}$ (d)- ${{K}^{+}},C{{a}^{2+}},S{{c}^{3+}},{{F}^{-}}$ Show
Answer Verified Hint: Isoelectronic species have the same number of electrons. : In isoelectronic species, as the nuclear charge increases, the force of attraction by the nucleus on the electrons also increases. Complete answer: (b)- $N{{a}^{+}},C{{a}^{2+}}S{{c}^{3+}},{{F}^{-}}$ (c)- ${{K}^{+}},C{{l}^{-}},C{{a}^{2+}}S{{c}^{3+}}$ (d)- ${{K}^{+}},C{{a}^{2+}},S{{c}^{3+}},{{F}^{-}}$
Note: The nuclear charge is calculated by the number of electrons + charge on the ion. `K^(+), Ca^(2+), Sc^(3+)` `Na^(+), F^(-), V^(3+)` `K^(+), Cl^(-), Mg^(2+)` `Cr^(3+), Fe^(2+), Co^(3+)` Answer : A Solution : `K^(+), Ca^(2+), Sc^(3+)` all contain 18 electrons in rest of species are : `Na^(+)(10), F^(-)(10), V^(3+)(20), Cl^(-)(18), Mg^(2+)(10), Cr^(5+)(21), Fe^(2+)(24) and Co^(3+)(24)`. `K^(+),Cl^(-),Mg^(2+),Sc^(3+)``K^(+),Ca^(2+),Sc^(3+),Cl^(-)``Na^(+),Ca^(2+),Sc^(3+),F``Na^(+),Mg^(2+),Al^(3+),Cl` Answer : C Solution : Isoelectronic species are those which have same electrons. <br> `K^(+)=19-1=18, Ca^(+2)=20-2=18` <br> `Sc^(+3)=121-3=18, Cl^(-)=17+1=18` `K^(+), Ca^(2+), Sc^(3+), Cl^(-)``Na^(+), Ca^(2+), Sc^(3+), F^(-)``K^(+), Cl^(-), Mg^(2+), Sc^(3+)``Na^(+), Mg^(2+), Al^(3+), Cl^(-)` Answer : A Solution : Isoelectronic species are those which have same number of electrons. <br> `K^(+) = 19 -1 = 18 , Ca^(2+) = 20 - 2 = 18` <br> `Sc^(3+) = 21 - 3 = 18 , C^(-) = 17 + 1 = 18` `K^(+), Ca^(2+), Sc^(3+)``Na^(+), F^(-), V^(3+)``K^(+), Cl^(-), Mg^(2+)`None of these Answer : A Solution : `K^(+), Ca^(2+), Sc^(3+)` all contain 18 electrons in rest of species are : `Na^(+) (10), F^(-)(10), V^(3+)(20) Cl^(-)(18), Mg^(2+)(10), Cr^(3+)(21), Fe^(2+) (24) and Co^(3+) (24)`. Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses No worries! We‘ve got your back. Try BYJU‘S free classes today! No worries! We‘ve got your back. Try BYJU‘S free classes today! No worries! We‘ve got your back. Try BYJU‘S free classes today! Solution The correct option is A K+,Cl−,Ca2+,Sc3+Isoelectronic species are those species which contains same number of electrons. (a) K+=19−1=18 e− Cl−=17+1=18 e− Ca2+=20−2=18 e− Sc3+=21−3=18 e− Thus, all the species are isoelectronic. (b) Ba2+=56−2=54 e− Sr2+=38−2=36 e− K+=19−1=18e− S2−=16+2=18e− Thus, these species are not isoelectronic. (c) N3−=7+3=10e− O2−=8+2=10e− F−=9+1=10 e− S2−=16+2=18 e− Thus, these species are not isoeletronic. (d) Li+=3−1=2 e− Na+=11−1=10 e− Mg2+=12−2=10 e− Ca2+=20−2=18 e− Thus, these species are not isoeletronic.What are examples of isoelectronic species?Isoelectronic species are elements or ions that have the equal number of electrons. Example: O2−,F−,Mg2+ have 10 electrons.
What are isoelectronic sets?Isoelectronic refers to two atoms, ions or molecules that have the same electronic structure and the same number of valence electrons. This term means "equal electric" or "equal charge". Isoelectronic chemical species typically display similar chemical properties.
How do you find the isoelectronic set?Hint: Isoelectronic pairs are those atoms, ions and molecules that have the same number of electrons in them. To find the isoelectronic pairs, we can just add the number of electrons of each atom and also the charge of the ion (if present) to find which of the molecules have the same number of electrons in them.
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