Chemical Properties of Metals
Metals have distinct chemical properties that set them apart from other elements. These properties are mainly due to their tendency to lose electrons and form positive ions (cations). Here are the major chemical properties of metals explained in simple terms:
1. Reaction of Metals with Oxygen
When metals react with oxygen, they form metallic oxides. Most of these oxides are basic in nature, meaning they react with water to form bases (alkalis).
Example:
2Mg + O₂ → 2MgO
(Magnesium reacts with oxygen to form magnesium oxide.)
Some metals like aluminum and zinc form amphoteric oxides, which can react with both acids and bases.
2. Reaction of Metals with Water
Some metals react with water to form metal hydroxides and hydrogen gas.
Example:
2Na + 2H₂O → 2NaOH + H₂
(Sodium reacts vigorously with water to form sodium hydroxide and hydrogen gas.)
Not all metals react the same way — for instance, sodium and potassium react explosively with water, while iron and copper react very slowly or not at all.
3. Reaction of Metals with Acids
Metals generally react with dilute acids to produce hydrogen gas and a salt.
Example:
Zn + 2HCl → ZnCl₂ + H₂
(Zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas.)
However, some metals like copper, silver, and gold do not react with dilute acids because they are less reactive.
4. Reaction of Metals with Other Metal Salts
A more reactive metal can displace a less reactive metal from its salt solution. This is known as a displacement reaction.
Example:
Fe + CuSO₄ → FeSO₄ + Cu
(Iron displaces copper from its copper sulfate solution.)
This property is often used to determine the reactivity series of metals.
5. Formation of Ionic Compounds
Metals readily lose electrons to form positive ions (cations). These ions then combine with non-metal ions (anions) to form ionic compounds.
Example:
2Na + Cl₂ → 2NaCl
(Sodium reacts with chlorine to form sodium chloride — a stable ionic compound.)
These chemical behaviors show that metals are strong reducing agents, meaning they easily give up electrons. This property makes them valuable in chemical industries, electrochemistry, and materials science.
Chemical Properties of Non-Metals
Non-metals show chemical behaviors that are quite the opposite of metals. Instead of losing electrons, non-metals usually gain or share electrons during chemical reactions. This gives them unique characteristics that are essential for forming compounds vital to life and industry. Let’s explore their main chemical properties in a simple and human way.
1. Reaction of Non-Metals with Oxygen
Non-metals react with oxygen to form non-metallic oxides. These oxides are generally acidic in nature. When dissolved in water, they form acids.
Example:
C + O₂ → CO₂
(Carbon reacts with oxygen to form carbon dioxide.)
Carbon dioxide dissolves in water to produce carbonic acid:
CO₂ + H₂O → H₂CO₃
Some non-metal oxides like carbon monoxide (CO) are neutral and neither acidic nor basic.
2. Reaction of Non-Metals with Water
Most non-metals do not react directly with water. Elements like sulfur, phosphorus, and carbon remain unaffected by water under normal conditions. However, some of their oxides dissolve in water to form acids.
Example:
SO₂ + H₂O → H₂SO₃
(Sulfur dioxide reacts with water to form sulfurous acid.)
3. Reaction of Non-Metals with Acids
Non-metals generally do not react with acids because they are poor reducing agents. Acids contain hydrogen ions (H⁺) that can be reduced only by elements that easily donate electrons — something non-metals typically don’t do. For example, sulfur, carbon, or phosphorus show no visible reaction with hydrochloric acid.
4. Reaction of Non-Metals with Bases
Some non-metals can react with strong bases under specific conditions, forming salts and water.
Example:
Cl₂ + 2NaOH → NaCl + NaClO + H₂O
(Chlorine reacts with sodium hydroxide to form sodium chloride, sodium hypochlorite, and water.)
This kind of reaction is used in making disinfectants like bleach.
5. Formation of Covalent Compounds
Non-metals usually form covalent compounds by sharing electrons with other non-metals. These compounds are made up of molecules rather than ions and often have low melting and boiling points.
Example:
H₂ + Cl₂ → 2HCl
(Hydrogen and chlorine share electrons to form hydrogen chloride.)
Similarly, water (H₂O), ammonia (NH₃), and methane (CH₄) are all covalent compounds formed by non-metals.
Non-metals are generally oxidizing agents, meaning they gain electrons during reactions. Their chemistry plays a major role in forming acids, gases, and essential organic compounds that make up our environment and even our own bodies. From oxygen that supports life to nitrogen that nourishes plants — non-metals truly define the balance of nature.
