In a redox reaction, the substance that accepts electrons is said to be

Among the substances listed, ammonia (NH3) is a compound. The option D (ammonia) is the correct option.

Compound Substance

• A compound substance refers to a type of substance that is composed of two or more different elements chemically combined in fixed proportions. In other words, it is a substance formed when atoms of different elements bond together to form molecules. The elements in a compound substance are chemically bonded, meaning they are held together by chemical forces such as covalent bonds, ionic bonds, or metallic bonds.

Compounds can have various physical forms, such as solids, liquids, or gases, depending on the specific elements and the nature of their chemical bonds. They can also exhibit a wide range of chemical and physical properties, such as melting point, boiling point, density, solubility, and reactivity.

Chemical formulas are used to represent compound substances, indicating the types and numbers of atoms present in a molecule of the compound. For example, the chemical formula for water is H2O, representing two hydrogen (H) atoms bonded to one oxygen (O) atom. Ammonia is composed of nitrogen (N) and hydrogen (H) atoms bonded together. Carbon (C), chlorine (Cl), and uranium (U) are elements rather than compounds.

Therefore, Ammonia which is option D is the correct option.

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Answer:

Ammonia

Explanation:

Ammonia is a inorganic compound that is made up of single nitrogen atom.

Answer:

                  Option-1 (O²⁻) is the correct answer.

Explanation:

                       All given anions contains same charge. So, we can ignore the effect of charge on these anions.

As we know all given compounds belongs to same group (Group 6) in periodic table. And from top to bottom along the group the elements are placed as,

                                                          Oxygen O

                                                          Sulfur S

                                                          Selenium Se

                                                          Tellurium Te

Hence, moving from top to bottom along the group the number of shells increases. And with increase in number of shell the atomic or ionic radii increases. As Oxygen is present at the top of the group, therefore, it has the smallest radius due to less number of shells.

O²⁻ ion has the smallest radius

Further explanation

In an atom there are levels of energy in the shell and sub shell.

This energy level is expressed in the form of electron configurations.

Writing electron configurations starts from the lowest to the highest sub-shell energy level. There are 4 sub-shells in the shell of an atom, namely s, p, d and f. The maximum number of electrons for each sub shell is

• s: 2 electrons
• p: 6 electrons
• d: 10 electrons and
• f: 14 electrons

Charging electrons in the sub shell uses the following sequence:

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.

Each sub-shell also has an orbital shown in the form of a square in which there are electrons symbolized by half arrows

The atomic radius shows the distance of the atomic nucleus to the electrons in the outer shell

From left to right in the period system the atomic radius gets smaller, while from one group from top to bottom the atomic radius gets longer

The more the number of shells the atom has, the radius of the atom getting longer, but if the number of shells is the same, the larger atomic number has shorter radius because the core charge is greater so that the attraction of the nucleus to the electrons is stronger

In the ions

(1) O²⁻

(2) S²⁻

(3) Se²⁻

(4) Te²⁻

All of these ions are ions from the elements of the VIA group in the periodic system. This group consists of oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and polonium (Po).

The periodic system is arranged in the order of atomic numbers, whereas in this VIA group from top to bottom, the atomic number gets bigger

• Element O

Atomic Number: 8

Electron configuration: 1s² 2s² 2s⁴ (number of shells 2)

• Element S

Atomic Number: 16

Electron configuration: [Ne] 3s² 3p⁴ (number of shells 3)

• Element Se

Atomic Number: 34

Electron configuration: [Ar] 3d¹⁰ 4s²4p⁴ (number of shells 4)

• Element Te

Atomic Number: 52

Electron configuration: [Cr] 4d10 5s² 5p⁴ (number of shells 5)

From the configuration of the electron shows that the lower the shell owned by the elements of the VIA group the greater (from 2 to 5) so that the radius is also getting longer/bigger

Because what is being asked is the radius of the ion, the electron configuration of each element is equally reduced by 2 electrons, but the number of shells remains the same

(1)O²⁻

Electron configuration: 1s² 2s² 2s²

(2) S²⁻

Electron configuration: [Ne] 3s² 3p²

(3) Se²⁻

Electron configuration: [Ar] 3d¹⁰ 4s²4p²

(4) Te²⁻

Electron configuration: [Cr] 4d¹⁰ 5s² 5p²

Because the amount of shell from the Oxygen ion is the smallest, the radius of the O²⁻ is also the smallest

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Keywords: element, group 6A, the smallest radius