Nitrogen and sulfur · ⁨חנקן וסולפיד⁩

Nitrogen gas, $\text{N}_2$, makes up most of the air but reacts with very little. There are two reasons:

• the two nitrogen atoms are joined by a triple bond 三键, which has a very high bond energy 键能. A lot of energy is needed to break it.
• the molecule has no polarity 极性 — it is perfectly symmetrical, so nothing pulls other molecules towards it.

Basicity of ammonia

The basicity 碱性 of ammonia (its ability to act as a base) comes from the lone pair 孤对电子 of electrons on the nitrogen atom. Using the Brønsted–Lowry theory, ammonia is a base because this lone pair can accept a proton 质子 ($\text{H}^+$):

The ammonium ion

When the lone pair forms a bond to $\text{H}^+$, it makes the ammonium ion 铵离子, $\text{NH}_4^+$. Because both shared electrons came from the nitrogen, this new bond is a coordinate bond 配位键. The ion has four identical N–H bonds and a tetrahedral shape.

Displacement of ammonia from its salts

If you warm an ammonium salt with a base (such as sodium hydroxide), you push out ammonia gas. This is an acid–base displacement 置换:

The sharp smell of ammonia, and damp red litmus turning blue, is a test for an ammonium salt.

Where they come from

Oxides of nitrogen ($\text{NO}$ and $\text{NO}_2$, together called $\text{NO}_x$) come from two sources:

• natural: lightning gives enough energy for nitrogen and oxygen in the air to combine.
• man-made: the high temperature inside an internal combustion engine 内燃机 makes nitrogen and oxygen react:

Removing them from car exhaust

A catalytic converter 催化转化器 cleans the exhaust gases 尾气. It lets the harmful gases react together to form harmless ones:

Photochemical smog

In sunlight, $\text{NO}$ and $\text{NO}_2$ react with unburned hydrocarbons to form peroxyacetyl nitrate (PAN). PAN is a harmful part of photochemical smog 光化学烟雾, the brown haze seen over busy cities.

Acid rain

The oxides of nitrogen also help make acid rain 酸雨 in two ways:

• directly: $\text{NO}_2$ dissolves in rain to form nitric acid.
• as a catalyst: $\text{NO}_2$ speeds up the oxidation of atmospheric sulfur dioxide 二氧化硫 ($\text{SO}_2$) into $\text{SO}_3$, which then forms sulfuric acid in the rain.

Worked example. A white solid is warmed with aqueous $\text{NaOH}$, and a gas is released that turns damp red litmus blue. Identify the gas and the ion in the solid, and explain the reaction. The only common gas that turns damp red litmus blue is ammonia, $\text{NH}_3$, so the solid contains the ammonium ion, $\text{NH}_4^{+}$. The hydroxide ion is the stronger base, so it takes the proton back from the ammonium ion:

This is the standard test for $\text{NH}_4^{+}$. Always say the litmus is damp: the ammonia must dissolve in the water before it can show its basicity, so dry litmus would give no colour change at all.

• $\text{N}_2$ is unreactive because of its strong triple bond (very high bond energy) — state this exactly.
• Ammonia is a base and a ligand because of its lone pair; the ammonium ion forms by a dative bond.
• Explain how oxides of nitrogen form (high temperature in engines) and their link to acid rain and photochemical smog.
• Give balanced equations and correct observations for reactions of ammonia and the ammonium ion.