Question

The characteristics of elements X, Y, and Z with atomic numbers, respectively $33$, $53$ and $83$ are

• A. X and Z are non-metals and Y is a metalloid
• B. X and Y are metalloids and Z is a metal.
• C. X, Y and Z are metals.
• D. X is a metalloid, Y is a non-metal and Z is a metal

Answer 1

The correct option is D

X is a metalloid, Y is a non-metal and Z is a metal

The explanation for the correct option:

Option (D): X is a metalloid, Y is a non-metal and Z is a metal

1. The element X with atomic number$=33$, its electronic configuration of the atomic number will be$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}4{\mathrm{s}}^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^3$ So, its configuration is similar to 15th group and it has $5$ valence electrons.
2. This group consists of nitrogen, phosphorus, arsenic, antimony, and bismuth. The first two elements of this group are non-metallic in nature, arsenic and antimony are metalloids and bismuth is a metal.
3. The element Y with atomic number=$=53$ has an electronic configuration $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^{2}4{\mathrm{p}}^{6}4{\mathrm{d}}^{10}5{\mathrm{s}}^{2}5{\mathrm{p}}^5$ which represents iodine.
4. Iodine is a Group $17$ element as it contains $7$ valence electrons in its outermost shell. It lies in the halogen period hence it is a non-metal.
5. The element Z with atomic number$=$$83$ has a configuration $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}4{\mathrm{s}}^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^{6}5{\mathrm{s}}^{2}4{\mathrm{d}}^{10}5{\mathrm{p}}^{6}6{\mathrm{s}}^{2}4{\mathrm{f}}^{14}5{\mathrm{d}}^{10}6{\mathrm{p}}^3.$
6. It lies in the p-block as its last electron lies in the p orbital.
7. It is the only metal in the group$15$.

The explanation for the incorrect options:

Option (A): X and Z are non-metals and Y is a metalloid

1. The element Y with atomic number=$=53$ has an electronic configuration $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^{2}4{\mathrm{p}}^{6}4{\mathrm{d}}^{10}5{\mathrm{s}}^{2}5{\mathrm{p}}^5$ that represents iodine.
2. Iodine is a group $17$ element as it contains $7$ valence electrons in its outermost shell. It lies in the halogen period hence it is a non-metal.
3. Hence, it is an incorrect option.

Option (B): X and Y are metalloids and Z is a metal.

1. The element X with atomic number$=33$, its electronic configuration of the atomic number will be$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}4{\mathrm{s}}^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^3$ So, its configuration is similar to $15\mathrm{th}$ group and it has $5$ valence electrons.
2. This group consists of nitrogen, phosphorus, arsenic, antimony, and bismuth. The first two elements of this group are non-metallic in nature, arsenic and antimony are metalloids and bismuth is a metal.
3. Hence, it is an incorrect option.

Option (C): X, Y, and Z are metals.

1. The element Z with atomic number$=$$83$ has a configuration $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}4{\mathrm{s}}^{2}3{\mathrm{d}}^{10}4{\mathrm{p}}^{6}5{\mathrm{s}}^{2}4{\mathrm{d}}^{10}5{\mathrm{p}}^{6}6{\mathrm{s}}^{2}4{\mathrm{f}}^{14}5{\mathrm{d}}^{10}6{\mathrm{p}}^3.$
2. It lies in the p-block as its last electron lies in the p orbital.
3. It is the only metal in the group$15$.
4. Hence, it is an incorrect option.

Therefore, X is a metalloid, Y is a non-metal and Z is a metal.