Given below are two statements:
Statement I: The electronegativity of group 14 elements from Si to Pb gradually decreases.
Statement II: Group 14 contains non-metallic, metallic, as well as metalloid elements.
In the light of the above statements, choose the most appropriate from the options given below:
Statement I: The electronegativity of group 14 elements from Si to Pb gradually decreases.
Statement II: Group 14 contains non-metallic, metallic, as well as metalloid elements.
In the light of the above statements, choose the most appropriate from the options given below:
Both Statement I and Statement II are false
Both Statement I and Statement II are true
Statement I is true but Statement II is false
Statement I is false but Statement II is true
The Correct Option is D
Approach Solution - 1
To evaluate the given statements about group 14 elements in the periodic table, let's consider each statement individually:
- Statement I: The electronegativity of group 14 elements from Si to Pb gradually decreases.
This statement is incorrect. In the periodic table, the electronegativity generally decreases as you move down a group due to the increasing atomic radius and shielding effect, which reduces the attraction between the nucleus and valence electrons. Thus, for Group 14 elements such as Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb), the electronegativity decreases from Si to Pb. However, if disregards the hint that the decrease is not 'gradual,' given the variance in metallic properties and atomic structure influence. Nonetheless, in principle, Si is more electronegative than Pb.
- Statement II: Group 14 contains non-metallic, metallic, as well as metalloid elements.
This statement is true. Group 14 elements showcase a variety of properties: Carbon (C) is a non-metal, Silicon (Si) and Germanium (Ge) are metalloids, while Tin (Sn) and Lead (Pb) are metals. This variety arises due to the increase in atomic size and metallic character down the group.
In conclusion, Statement I is false but Statement II is true. Therefore, the correct option is:
- Statement I is false but Statement II is true.
Approach Solution -2
The electronegativity values for Group 14 elements from Si to Pb are almost the same, with values approximately as follows:
Therefore, Statement I is false as there is no gradual decrease in electronegativity from Si to Pb.- Statement II is true because Group 14 does indeed contain non-metallic (C), metalloid (Si, Ge), and metallic (Sn, Pb) elements.
So, the correct answer is : Statement I is false but Statement II is true
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(E) Carbon can exhibit negative oxidation states.
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Concepts Used:
Group 14 Elements
The group 14 elements are also known as the carbon group. Sometimes it is also called crystallogens. The group 14 elements can be found on the right side of the periodic table. The elements of the carbon group are:
- Carbon - C
- Silicon - Si
- Germanium - Ge
- Tin - Sn
- Lead - Pb
- Flerovium - FI
The group 14 elements or the carbon family belongs to the p-block of the periodic table. The carbon group is also the second group in the p-block.
Electronic Configuration:
The arrangement of electrons in the orbitals of a molecule or atom is known as electronic configuration. The general electronic configuration of the group 14 elements is ns2np2.
All group 14 elements have 4 electrons in the outer shell. Hence, the valency of the carbon family or group 14 elements is 4.
Properties of Group 14 Elements:
- Covalent Radii
- Ionization Enthalpy
- Electronegativity
- Metallic Character
- Density
- Four Covalent Compounds
- The Melting and Boiling Points