Respuesta :
Answer : The electron configuration for the monatomic ions are shown below.
Explanation :
For the neutral atom, the number of protons and electrons are equal. But, they are unequal when the atoms present in the form of ions or the atom has some charges.
When an unequal number of electrons and protons then it leads to the formation of ionic species.
Ion : An ion is formed when an atom looses or gains electron.
When an atom looses electrons, it will form a positive ion known as cation.
When an atom gains electrons, it will form a negative ion known as anion.
(a) The given element is, Cl (Chlorine)
As we know that the rubidium element belongs to group 17 and the atomic number is, 17
The ground-state electron configuration of Cl is:
[tex]1s^22s^22p^63s^23p^5[/tex]
This element will easily gain 1 electron and form [tex]Cl^-[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Cl ion is:
[tex]1s^22s^22p^63s^23p^6[/tex]
(b) The given element is, Na (Sodium)
As we know that the sodium element belongs to group 1 and the atomic number is, 11
The ground-state electron configuration of Na is:
[tex]1s^22s^22p^63s^1[/tex]
This element will easily lose 1 electron and form [tex]Na^{+}[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Na ion is:
[tex]1s^22s^22p^6[/tex]
(c) The given element is, Mg (Magnesium)
As we know that the magnesium element belongs to group 2 and the atomic number is, 12
The ground-state electron configuration of Mg is:
[tex]1s^22s^22p^63s^2[/tex]
This element will easily lose 2 electrons and form [tex]Mg^{2+}[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Mg ion is:
[tex]1s^22s^22p^6[/tex]
(d) The given element is, Ca (Calcium)
As we know that the calcium element belongs to group 2 and the atomic number is, 20
The ground-state electron configuration of Ca is:
[tex]1s^22s^22p^63s^23p^64s^2[/tex]
This element will easily lose 2 electrons and form [tex]Ca^{2+}[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Ca ion is:
[tex]1s^22s^22p^63s^23p^6[/tex]
(e) The given element is, K (Potassium)
As we know that the potassium element belongs to group 1 and the atomic number is, 19
The ground-state electron configuration of K is:
[tex]1s^22s^22p^63s^23p^64s^1[/tex]
This element will easily lose 1 electron and form [tex]K^{+}[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of K ion is:
[tex]1s^22s^22p^63s^23p^6[/tex]
(f) The given element is, Br (Bromine)
As we know that the bromine element belongs to group 17 and the atomic number is, 35
The ground-state electron configuration of Rb is:
[tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^5[/tex]
This element will easily gain 1 electron and form [tex]Br^-[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Br ion is:
[tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^6[/tex]
(g) The given element is, Sr (Strontium)
As we know that the strontium element belongs to group 2 and the atomic number is, 38
The ground-state electron configuration of Rb is:
[tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^2[/tex]
This element will easily lose 2 electrons and form [tex]Sr^{2+}[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of Sr ion is:
[tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^6[/tex]
(h) The given element is, F (Fluorine)
As we know that the fluorine element belongs to group 17 and the atomic number is, 9
The ground-state electron configuration of F is:
[tex]1s^22s^22p^5[/tex]
This element will easily gain 1 electron and form [tex]F^{-}[/tex] ion which attain stable noble gas electronic configuration.
The full ground-state electron configuration of F ion is:
[tex]1s^22s^22p^6[/tex]
An ion having only one atom is called a mono-atomic ion and is represented as the symbol of the element with mass and charge in subscript and superscript.
The ion that loses an electron is called a cation while the ion that acquires an electron is called an anion.
The electronic configuration of the following ions are:
a. Cl (Chlorine):
- Chlorine belongs to group 17 in the periodic table and has an atomic number of 17.
- The ground state electronic distribution of chlorine ion:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}[/tex]
- To attain noble gas configuration Cl will gain one electron to form [tex]Cl^{-}[/tex].
- The full ground-state electron distribution of Cl ion is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}[/tex]
b. Na (Sodium):
- The sodium element has the atomic number 11 and belongs to group 1.
- Ground-state electron arrangement of Na is:
[tex]1s^{2}2s^{2}2p^{6}3s^{1}[/tex]
- It loses an electron to attain noble gas configuration and forms [tex]Na^{+}[/tex].
- The full ground-state electron arrangement of Na ion is:
[tex]1s^{2}2s^{2}2p^{6}[/tex]
c. Mg (Magnesium):
- It has atomic number 12 and belongs in the 2nd group.
- Ground-state electron distribution of Mg is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}[/tex]
- To attain noble gas configuration it loses two electrons and forms
[tex]Mg^{2+}[/tex].
- The full ground-state electron distribution of Mg ion is:
[tex]1s^{2}2s^{2}2p^{6}[/tex]
d. Ca (Calcium):
- The atomic number is 20 and belongs to group 2.
- The ground-state electron arrangement of Ca is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}[/tex]
- It loses two electrons to attain a noble gas configuration and forms [tex]Ca^{2+}[/tex].
- The full ground-state electron arrangement of Ca ion is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}[/tex]
e. K (Potassium):
- The atomic number is 19 and belongs to group 1.
- The ground-state electron distribution of K is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}[/tex]
- To attain noble gas configuration it loses one electron and forms [tex]K^{+}[/tex].
- The full ground-state electron distribution of K ion is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}[/tex]
f. Br (Bromine):
- The bromine element has the atomic number 35 and belongs to group 17.
- The ground-state electron arrangement of Br ion is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}[/tex]
- It gains one electron to attain noble gas configuration and forms [tex]Br^{-}[/tex].
- The full ground-state electron arrangement of Br ion is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}[/tex]
g. Sr (Strontium):
- It belongs to the 2nd group and has atomic number 38.
- The ground-state electron arrangement of Sr ion is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}[/tex]
- It loses two-electron to attain noble gas configuration and forms [tex]Sr^{2+}[/tex].
- The full ground-state electron arrangement of Sr ion is:
[tex]1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}[/tex]
h. F (Fluorine):
- It belongs to group 17 and has the atomic number 9.
- The ground-state electron distribution of F ion is:
[tex]1s^{2}2s^{2}2p^{5}[/tex]
- It gains one electron to form [tex]F^{-}[/tex] to attain the noble gas configuration.
- The full ground-state electron distribution of F ion is:
[tex]1s^{2}2s^{2}2p^{6}[/tex]
To learn more about electronic configuration of elements follow the link:
https://brainly.com/question/9616334
