B. Carbon and Silicon
C. Argon and Chlorine
D. Potassium and Calcium
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Answer:
Option-B (Carbon and Silicon)
Explanation:
Among the given pairs only carbon and silicon have the most similar properties. This is because,
Sodium and Magnesium belong to different groups. Sodium present in Group I has one electron in its valence shell and capable of transferring only one electron while, Magnesium present in Group II have two electrons in its valence shell and is capable of donating two electrons. Hence, both show different properties.
Example:
2 Na + Cl₂ → NaCl
Mg + Cl₂ → MgCl₂
As shown in reactions when Sodium and Magnesium are treated with Cl₂ they give a products with different proportions.
Carbon and Silicon show almost same properties because both belong to Group IV hence both are capable of forming four bonds. Also, they share the same property of self linkage in making a long chains.
Argon and Chlorine also belong to two different groups. Argon is present in Group VIII (Noble Gases) and Chlorine is present in Group VII (Halogens). Hence, Argon is an inert specie which is non reactive while Chlorine gives different reaction easily.
Potassium and Calcium belong to different groups. Potassium present in Group I has one electron in its valence shell and capable of transferring only one electron while, Calcium present in Group II have two electrons in its valence shell and is capable of donating two electrons. Hence, both show different properties.
Example:
2 K + Cl₂ → KCl
Ca + Cl₂ → CaCl₂
As shown in reactions when Potassium and Calcium are treated with Cl₂ they give a products with different proportions.
Mg(s) + N2(g) --> Mg3N2(s)
51 Balance the equation in your answer booklet for the reaction between magnesium and nitrogen, using the smallest whole-number coefficients. [1]
52 In the ground state, which noble gas has atoms with the same electron configuration as a magnesium ion? [1]
53 Explain, in terms of electrons, why an atom of the metal in this reaction forms an ion that has a smaller radius than its atom. [1]
51)
Mg(s) + N₂(g) --> Mg₃N₂(s)
There is one Mg atom on the reactant side and three Mg atoms on the product side. So to balance the number of Mg on both side of the equation a coefficient 3 is placed before Mg on the reactant side. The number of N atoms are two on both side of the reaction. Therefore the balanced chemical equation is,
2Mg(s) + N₂(g) --> Mg₃N₂(s)
52)
The electron configuration of Mg is 1s²2s²2p⁶3s² or [Ne]3s²
The electron configuration of Mg²⁺ is 1s²2s²2p⁶ or [Ne]
The electron configuration of Ne is 1s²2s²2p⁶
Ne he same electron configuration as a Mg²⁺ ion.
53)
Mg has its valence electron in the 3s shell, but Mg²⁺ has no electron in the 3s shell, the valence electron in Mg²⁺is in the 2p orbital. The size of the 2 shell is smaller than the 3 shell. Hence, Mg²⁺ is smaller than Mg.
The balanced equation for the reaction between magnesium and nitrogen is 3Mg(s) + N2(g) -> Mg3N2(s). Neon has atoms with the same electron configuration as a magnesium ion. When an atom of a metal forms an ion, it loses electrons and has a smaller radius.
51. The balanced equation for the reaction between magnesium and nitrogen is:
3Mg(s) + N2(g) → Mg3N2(s)
52. The magnesium ion has the same electron configuration as a neon atom because both have the electron configuration of 2,8. Therefore, neon is the noble gas with atoms having the same electron configuration as a magnesium ion.
53. When an atom of a metal forms an ion, it loses one or more electrons to achieve a stable electron configuration. This results in a decrease in the size of the ion compared to the neutral atom. The loss of electrons reduces the repulsion between the remaining electrons, causing the ion to have a smaller radius.
Learn more about Magnesium here:
#SPJ6
The correct answer for above statement:
chromium is in group 6 d-block
Explanation:
The d-block elements are designated transition metals and have valence electrons in d orbital's. The f-block elements, observed in the two rows at the ground of the periodic table, are called inner transition metals and have valence electrons in the f-orbital's.
Chromium is a synthetic element with symbol Cr and atomic number 24. It is the first component in group 6. It is a steely-gray, glistening, dense and brittle metal which takes a high polish, resists smudging, and has a great melting point.