Question

The oxygen and nitrogen families have some obvious similarities and differences. (a) State two general physical similarities between Group \(5 \mathrm{~A}(15)\) and \(6 \mathrm{~A}(16)\) elements. (b) State two general chemical similarities between Group \(5 \mathrm{~A}(15)\) and \(6 \mathrm{~A}(16)\) elements. (c) State two chemical similarities between \(\mathrm{P}\) and \(\mathrm{S}\). (d) State two physical similarities between \(\mathrm{N}\) and \(\mathrm{O}\). (e) State two chemical differences between \(\mathrm{N}\) and \(\mathrm{O}\).

Short answer

Both groups contain nonmetals and metalloids, show variable oxidation states, \(\text{P}\) and \(\text{S}\) are multivalent, \(\text{N}\) and \(\text{O}\) are diatomic gases, \(\text{N}\) usually forms triple bonds, \(\text{O}\) forms double bonds.

Step-by-step solution

Physical similarities between Group 5A (15) and 6A (16)

Both groups are made up of nonmetals, metalloids, and poor metals. Additionally, they often have similar atomic and ionic radii trends down their groups.

Chemical similarities between Group 5A (15) and 6A (16)

Elements in both groups have multiple oxidation states. Also, both groups form covalent bonds with other nonmetals.

Chemical similarities between \(\text{P}\) and \(\text{S}\)

Phosphorus (\( \text{P} \)) and Sulfur (\( \text{S} \)) can both exhibit multiple oxidation states. They both form oxoacids and can form bonds with oxygen.

Physical similarities between \(\text{N}\) and \(\text{O}\)

Nitrogen (\( \text{N} \)) and Oxygen (\( \text{O} \)) are both diatomic molecules in their most stable form (\( \text{N}_2 \) and \( \text{O}_2 \)). They are both colorless and odorless gases at room temperature.

Chemical differences between \(\text{N}\) and \(\text{O}\)

Nitrogen (\( \text{N} \)) forms predominantly triple bonds, while Oxygen (\( \text{O} \)) typically forms double bonds in its molecules. Also, Nitrogen is less electronegative compared to Oxygen, influencing their reactivity.

Key concepts

Physical Similarities

The physical characteristics of Group 5A (15) and Group 6A (16) elements exhibit fascinating parallels. Both groups include a mix of nonmetals, metalloids, and poor metals. This diversified composition means that elements share physical states ranging from gases to solids at room temperature. Moreover, these elements display analogous trends in their atomic and ionic radii across the groups. As you move down each group, the radii increase progressively due to the addition of electron shells which adds to the similarities in their physical behavior.

Chemical Similarities

Group 5A (15) and Group 6A (16) elements exhibit several chemical parallels. One prominent similarity is their ability to demonstrate multiple oxidation states. For instance, nitrogen (Group 5A) can show oxidation states from -3 to +5, while sulfur (Group 6A) ranges from -2 to +6. Another significant similarity is their propensity to form covalent bonds with other nonmetals. Both groups often establish strong covalent bonds, which play a crucial role in the formation of various compounds, including organic and inorganic molecules.

Oxidation States

Oxidation states are vital in understanding chemical reactivity. Phosphorus (P) and Sulfur (S), which belong to Group 5A and Group 6A respectively, can exhibit a range of oxidation states. Phosphorus can have oxidation states from -3 to +5, while sulfur can range from -2 to +6. These variable oxidation states allow these elements to participate in a variety of chemical reactions, forming numerous compounds. For example, phosphoric acid (H₃PO₄) and sulfuric acid (H₂SO₄) are both examples of compounds formed due to the versatility in oxidation states of P and S.

Covalent Bonds

The ability to form covalent bonds is a shared characteristic of Group 5A and Group 6A elements. These bonds are established when atoms share electrons, creating a strong and stable connection. Nonmetals in these groups, such as nitrogen (N) and sulfur (S), commonly form covalent bonds with other nonmetals. For instance, nitrogen forms covalent bonds in ammonia (NH₃), and sulfur does so in hydrogen sulfide (H₂S). Covalent bonding not only stabilizes molecules but also influences their properties, such as melting and boiling points.

Diatomic Molecules

In their most stable forms, both nitrogen (N) and oxygen (O) occur as diatomic molecules. Diatomic molecules are composed of two atoms of the same element. Nitrogen exists as N₂, and oxygen exists as O₂ in nature. These molecules are colorless and odorless gases at room temperature, making them physically similar. Being diatomic also contributes to their distinct chemical properties, such as their reactivity and the types of bonds they can form. For example, nitrogen typically forms triple bonds in N₂, whereas oxygen forms double bonds in O₂.