Question

A solid element \(\mathrm{Y}\) conducts electricity and forms two chlorides YCln a colourless volatile liquid and \(\mathrm{YCl}_{\mathrm{n}-2}\) a colourless solid. Then Y belongs to which of the following groups of periodic table? (a) 16 (b) 15 (c) 14 (d) 13

Short answer

The element \( \mathrm{Y} \) belongs to group 14 of the periodic table.

Step-by-step solution

Analyze Electrical Conductivity

Element \( \mathrm{Y} \) conducts electricity, indicating that \( \mathrm{Y} \) is likely a metal or a metalloid, since non-metals do not conduct electricity.

Examine Formation of Chlorides

\( \mathrm{Y} \) forms a chloride \( \mathrm{YCl}_n \) which is a colourless volatile liquid, and another chloride \( \mathrm{YCl}_{n-2} \) which is a colourless solid. This suggests that \( \mathrm{Y} \) can have multiple oxidation states, which is characteristic of elements in groups 13 or 14 of the periodic table.

Determine Possible Group From Clue

Since \( \mathrm{Y} \) has a chloride that is a volatile liquid, the higher oxidation state of \( \mathrm{Y} \) likely corresponds to group 14 because group 13 typically do not have volatile chlorides like \( \mathrm{YCl}_n \).

Identify Group 14 Characteristics

Elements in group 14 can exhibit oxidation states of +4 and +2, which match the pattern \( \mathrm{YCl}_n \) (volatile liquid) and \( \mathrm{YCl}_{n-2} \) (solid). In group 13, the typical oxidation change does not suit the behavior as described.

Conclude Based on Findings

By assessing the characteristics of both the chloride states and the element's ability to conduct electricity, it is most consistent with Group 14 elements like Si, Ge, or Sn, known for forming such chlorides.

Key concepts

Electrical Conductivity

Electrical conductivity is a key property that helps determine what type of element we're dealing with. Elements are categorized based on their ability to conduct electricity into metals, non-metals, and metalloids. Metals are excellent conductors due to their free-moving electrons.
Metalloids have intermediate conductivity, which increases under certain conditions, while most non-metals do not conduct electricity at all.
Therefore, if element \( \mathrm{Y} \) conducts electricity, it suggests that \( \mathrm{Y} \) is likely to be a metal or a metalloid.

Oxidation States

Oxidation states are indicators of the degree of oxidation (loss of electrons) an atom has undergone. They tell us which form of chloride an element can create based on its ability to donate or receive electrons.
Elements can exist in more than one oxidation state. For example, elements in Group 14 show variable oxidation states, typically +4 and +2. This flexibility helps them form multiple types of chlorides, indicating different oxidation levels.
In our example, \( \mathrm{Y} \) forming both \( \mathrm{YCl}_n \) and \( \mathrm{YCl}_{n-2} \) shows that it exhibits at least two different oxidation states, further pointing towards it being a Group 14 element.

Chloride Formation

The formation of chlorides is a common trait used to understand an element's chemical behavior. Chlorides form when elements react with chlorine, and the type of chloride formed depends on the element's oxidation state.
Elements that exhibit multiple oxidation states often form more than one type of chloride. In our example, \( \mathrm{Y} \) forms two types of chlorides: \( \mathrm{YCl}_n \), a volatile liquid, and \( \mathrm{YCl}_{n-2} \), a solid. This behavior suggests the flexibility of oxidation states common in Group 14 elements, known for such chemical patterns.

Metals and Metalloids

Metals and metalloids can often be distinguished by their electrical and structural properties. Metals are characterized by high electrical conductivity, malleability, luster, and often form positive ions by losing electrons. Metalloids share properties with metals and non-metals and can exhibit varying degrees of conductivity.
Next to metals, metalloids stand out due to their semi-conductive nature, making them important in electronics. In the context of Group 14, elements like silicon (Si) and germanium (Ge) are key examples of metalloids displaying intermediate electrical conductivity, aligning with \( \mathrm{Y} \)'s properties.

Group 14 Elements

Group 14 of the periodic table consists of elements carbon (C), silicon (Si), germanium (Ge), tin (Sn), and lead (Pb). They are known for exhibiting both metallic and non-metallic characteristics.
The elements in this group can form two common oxidation states: +4 and +2, which supports their ability to form chlorides like those observed in element \( \mathrm{Y} \).
While carbon behaves more as a non-metal, the other Group 14 elements like Si and Sn show properties of metals and metalloids, making them capable of electrical conduction and chloride formation.