`NO, CN^(-), N_2, O_2^-``NO^+, C_2^(2-), O_2^(-) , CO``N_2, C_2^(2-) , CO, NO``CO, NO^(+), CN^(-), C_2^(2-)` Show
Answer : D Solution : Species having equal number of electrons ae known as isoelectronic species. <br> Number of electrons , <br> In CO =6+8=14 <br> In `NO^+`=7+8-1=14 <br> In `CN^-`=6+7+1=14 <br> In `C_2^(2-)` =12+2=14 <br> Hence, all have 14 electrons, so they are isoelectronic species. `Na^(+),Ca^(2+),Mg^(2+)``N^(3-),F^(-) , Na^(+)``Be,Al^(3+),Cl^(-)``Ca^(2+),Cs^(+), Br`. Answer : B Solution : Isoelectronic species have same number of electrons , `N^(3-), F^(-)` and `Na^(+)` all have 10 electrons. More Free Tutorials Become a Member Members Log‐in Contact UsWant chemistry games, drills, tests and more? You need to become an AUS-e-TUTE Member! Key Concepts
(c) If two or more species have the same electronic configuration they are said to be isoelectronic. Please do not block ads on this website. Isoelectronic Configurations of Atoms and IonsConsider an atom of the Nobel Gas (Group 18 element) argon,
Ar. First energy level: 2 electrons in the s subshell In its simplest form, we could write the electronic configuration of an atom of argon in terms of shells (energy levels) as 2,8,8 In terms of subshells, the electronic configuration would be represented as 1s22s22p63s23p6 Argon is the ONLY element whose atoms have the ground-state electronic configuration of 1s22s22p63s23p6 But there are ions of other elements that can have the ground-state electronic configuration 1s22s22p63s23p6 Consider an atom of chlorine, Cl. First energy level: 2 electrons in the s subshell In its simplest form, we could write the electronic configuration of chlorine as 2,8,7 In terms of subshells, the electronic configuration would be represented as 1s22s22p63s23p5 Like all Group 17 (halogen) elements, atoms of chlorine can gain an electron to form an anion (negatively charged ion) with a charge of 1-. Now, let's consider what happens if this chlorine atom gains an electron to form the chloride ion.
Where will this "extra" electron go?
The electronic configuration of the chloride ion, Cl-, is 1s22s22p63s23p6. It is also possible for cations, positively charged ions, to be isoelectronic with the argon atom in its ground state. Consider an atom of potassium, K, in its ground state. First energy level: 2 electrons in the s subshell In its simplest form, we could write the electronic configuration of potassium as 2,8,8,1 In terms of subshells, the electronic configuration would be represented as 1s22s22p63s23p64s1 Like all Group 1 (alkali metal) elements, potassium will readily lose an electron to form a cation with a charge of +1.
The electron that is lost will come from the highest energy level, the fourth energy level:
And we can see that the potassium ion, K+, has the same electronic configuration as the chloride ion, Cl-, and the same electronic configuration as an atom of argon, Ar. Similary, we can see that an atom of calcium, Ca, (atomic number = 20) has en electronic configuration of
1s22s22p63s23p64s2 Summary Table of Some Isoelectronic SpeciesIf we consider the possible ions of the first 20 elements of the Periodic Table, we can draw up a table summarising which of the species are isoelectronic with atoms of a Group 18 (Noble Gas) element:
Worked Example: Determining Which Species are IsoelectronicQuestion : Which of the species below is NOT isoelectronic with Al3+ ? Solution: (Based on the StoPGoPS approach to problem solving.)
1. We will assume all species are in their ground-state electronic configuration for the purposes of this discussion. 2. The term "neutral" here means electrically neutral, neither positively nor negatively charged. 3. The term "orbiting" is being used to describe the motion of electrons around the nucleus and should not be taken literally (unless you are describing electrons within the orbits of a Bohr model of the atom). Which of the following contains only isoelectronic species?Solution: The combination contains only isoelectronic series is P3−, S2−, Cl−, Ar. Isoelectronic species are the species having same number of electrons.
Which of the following are isoelectronic species Na+ K+ Mg2+ Ca2+ AR?Hence isoelectronic species are Na+ and Mg2+;K+,Ca2+,S2− and Ar. Was this answer helpful?
Which of the following are examples of isoelectronic species?Some examples of isoelectronic species are carbon monoxide and nitrogen because they have equal numbers of electrons that both contain 10 valence electrons.
Is Na+ and Na isoelectronic?The given species are Na+ and Ne . From the explanation, both Na+ and Ne have the same electronic configuration. As a result, they are isoelectronic.
|