Question

Explain why nitrogen can form compounds with many different oxidation numbers.

Short answer

Nitrogen can form compounds with many oxidation numbers due to its five valence electrons, which allow it to gain, share, or lose electrons in chemical reactions, resulting in oxidation states from -3 to +5.

Step-by-step solution

Understanding Atomic Structure

The element nitrogen has an atomic number of 7, meaning it has 7 protons and typically 7 electrons. In its outer shell, nitrogen has 5 electrons, which can be gained, shared, or lost in chemical reactions, allowing for different oxidation states.

Recognizing Common Nitrogen Oxidation States

Nitrogen commonly exhibits oxidation states ranging from -3 to +5. This variability is due to its ability to form different numbers of covalent bonds and participation in electron transfer processes.

Identifying the Reason for Multiple Oxidation States

The capacity of nitrogen to achieve multiple oxidation states arises from the electronic configuration and the number of electrons in its outer shell that can participate in bonding. The small size of nitrogen favors the formation of multiple bonds, contributing to its ability to achieve a range of oxidation states.

Examining Electron Configuration

Nitrogen's electron configuration is 1s2 2s2 2p3. The five electrons in the second shell (2s and 2p orbitals) can engage in covalent bonding. By either accepting electrons to fulfill the octet rule (achieving a -3 state) or by losing or sharing its valence electrons, it can present a range of positive oxidation numbers (+1 up to +5).

Key concepts

Atomic Structure of Nitrogen

Diving into the atomic structure of nitrogen unveils why this element is a cornerstone in myriad compounds. With an atomic number of 7, nitrogen sits comfortably in the periodic table among the nonmetals, flanked by carbon and oxygen. Each nitrogen atom holds 7 protons within its nucleus, balanced out by 7 electrons whirling around in orbits.

The significance of nitrogen's atomic structure comes into play when addressing its role in chemistry. Specifically, it is the setup of the outermost electron shell that steals the show. This shell houses 5 valence electrons, poised for chemical interaction. The quintet is distributed in an electron configuration of 1s2 2s2 2p3, giving nitrogen its chemical versatility. Due to the presence of these electrons, nitrogen showcases a remarkable willingness to form bonds, leading to a wide array of chemical compounds.

Nitrogen Oxidation States

Understanding the nitrogen oxidation states is akin to exploring its many facets in the realm of compounds. Oxidation states, or oxidation numbers, indicate the degree of electron transfer nitrogen undergoes during chemical reactions. These states range impressively from -3 to +5.

Delving deeper, at the -3 oxidation state, nitrogen acts like a generous host, having 'accepted' additional electrons to fill its valence shell. On the flip side, when nitrogen demonstrates positive oxidation states, it’s essentially 'sharing' or 'giving away' electrons. This electron generosity enables nitrogen to cultivate a +1, +2, +3, +4, or +5 oxidation state, each implying a different bonding scenario. Hence, nitrogen's capability to sway between various chemical personas makes it a vital player in producing substances from ammonia (NH₃) to nitric acid (HNO₃).

Electron Configuration and Bonding

The electron configuration of nitrogen is a telling script of its bonding narrative. Starting off with a composition of 1s2 2s2 2p3, nitrogen comes equipped with three unpaired electrons in the 2p orbital, a duo in the 2s. This setup is primed for forging covalent linkages, as each unpaired electron can pair up with an electron from another atom.

A closer look reveals nitrogen’s flexibility in bonding. It can form three covalent bonds, as seen in ammonia (NH₃), embracing a -3 oxidation state by gaining three electrons to complete its valence shell. Moreover, nitrogen can also establish triple bonds, an instance being the bond in molecular nitrogen (N₂), where two nitrogen atoms share three pairs of electrons. Alternatively, nitrogen can engage in double bonds, as observed in the nitrogen oxides, or even single bonds that correlate with different positive oxidation states. It is this very ability to adapt its bonding based on the electron arrangements and requirements that underscores nitrogen’s significance in the chemistry arena.