Key Differences in Metal and Nonmetal Reactions with Examples
The elements are classified into metals and non-metals depending on their varying chemical and physical properties. Both metals and nonmetals are an essential part of our lives. We cannot imagine surviving without the nonmetals such as oxygen. Also, our survival would be complicated without the existence of the metals as well. Well, there is certainly a chemical science behind all these substances. However, in this article today, we will be dealing with only the topic of metals and what are the chemical properties of metals and nonmetals for class 8. So, here is a physical and chemical property of metals and nonmetals PDF that would help you learn about the properties of the metals.
What are Metals
Metals are known as the electropositive element wherein they tend to donate the electrons and form positively charged ions and become stable. Consider, for example,
Na ➝ Na+ + e-
Metals usually tend to possess certain distinguishing physical properties which make them easier for us to identify and classify.
The chemical properties of metals and nonmetals class 10 are as follows.
Physical Properties of Metals
Some of the primary physical properties of metals are as follows.
The metals tend to possess lustre and a shiny or metallic appearance.
They are generally in the form of solids when present at room temperature.
Metals are generally very good conductors of both heat and electricity.
They are ductile and malleable.
Metals mostly tend to possess very high melting points.
Chemical Properties of Metals
Let us now take a look at the chemical properties of metals.
Reaction of Metal With Oxygen
Let us first discuss the chemical properties of metals react with oxygen.
Metals tend to react with oxygen and form the metal oxides. Metals tend to donate the electrons to oxygen to form these metal oxides. Consider, for example,
4K + O2 ➝ 2K2O
These metal oxides are usually basic, however, they can also turn out to be amphoteric. Amphoteric oxides refer that they are both acidic as well as basic in nature. Some metals such as sodium and potassium tend to react vigorously with the oxygen. When sodium or potassium gets exposed to air it tends to catch fire easily. Therefore, they are kept safe in kerosene.
Reaction of Metal With Water
Some metals also react with water and form a metal hydroxide while others do not react at all. The reactivity of metals with water differs from one metal to the other.
Metals such as sodium and potassium are highly reactive when they come in contact with the water. They react with water and form alkalis like the sodium hydroxide and the potassium hydroxide.
2Na + 2H2O ➝ Na(OH)2 + H2
Calcium also tends to react with water for forming calcium hydroxide compounds and hydrogen.
2Ca + 2H2O ➝ Ca(OH)2 + H2
On the other hand, magnesium and zinc do not tend to react with cold water. They, however, form their respective oxides when they are reacted with only hot water.
Mg + H2O ➝ MgO + H2
Iron is comparatively less reactive than elements like calcium, sodium, magnesium, potassium, and zinc. It does not react with hot and cold water, but reacts with steam and forms magnetic oxides.
3Fe + 4H2O ➝ Fe3O4 + 4H2
Reaction with Dilute Acids
Metals such as potassium, sodium, calcium and lithium tend to react vigorously with the diluted HCl and H2SO4 and form hydrogen and their respective metal salt
However, zinc, iron, magnesium, lead and tin do not vigorously react with the acids.
Mg + HCl ➝ MgCl2 + H2
Fe + H2SO4 ➝ FeSO4 + H2
Metals that fall below the hydrogen element in the reactivity series do not tend to react with the dilute acids. They do not displace hydrogen atom to form a bond with the non-metallic anion.
Reaction of Metal with Other Metal Salts
Metals that are relatively more reactive will readily tend to react with the less reactive metals. The more reactive metals tend to displace the less reactive metals from either their oxides, sulphides, or chlorides.
Zn + CuSO4 ➝ ZnSO4 + Cu
Metals are arranged in the periodic table according to their electrode potential. This is known as an electrochemical series which is as follows.
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FAQs on Chemical Properties of Metals and Nonmetals: A Complete Guide
1. What are the primary chemical properties of metals?
Metals are defined by several key chemical properties related to their tendency to lose electrons. Key properties include:
- Reaction with Oxygen: Metals react with oxygen to form metal oxides, which are typically basic in nature. For example, magnesium burns in air to form magnesium oxide (MgO).
- Reaction with Water: Reactive metals like sodium and potassium react vigorously with cold water to produce metal hydroxides and hydrogen gas. Less reactive metals like iron react only with steam.
- Reaction with Dilute Acids: Most metals react with dilute acids (like HCl or H₂SO₄) to form a metal salt and release hydrogen gas. For example, zinc reacts with hydrochloric acid to form zinc chloride and hydrogen (Zn + 2HCl → ZnCl₂ + H₂).
- Reaction with Salt Solutions: A more reactive metal will displace a less reactive metal from its salt solution. This is based on the reactivity series.
- Nature of Ions: Metals are electropositive, meaning they readily lose electrons from their valence shell to form positive ions (cations).
2. What are the main chemical properties of non-metals?
Non-metals exhibit chemical properties that are generally opposite to those of metals, primarily driven by their tendency to gain or share electrons. Their main properties are:
- Reaction with Oxygen: Non-metals react with oxygen to form non-metal oxides, which are typically acidic or neutral in nature. For example, carbon burns to form carbon dioxide (CO₂), which is an acidic oxide.
- Reaction with Water: Non-metals generally do not react with water or steam to produce hydrogen gas.
- Reaction with Dilute Acids: Non-metals do not react with dilute acids to displace hydrogen.
- Reaction with Salt Solutions: Similar to metals, a more reactive non-metal can displace a less reactive non-metal from its salt solution. For instance, chlorine can displace bromine from a potassium bromide solution.
- Nature of Ions: Non-metals are electronegative; they tend to gain electrons to form negative ions (anions) or share electrons to form covalent bonds.
3. Why are most metal oxides basic, while non-metal oxides are acidic in nature?
This fundamental difference arises from how their oxides react with water. When a basic metal oxide, like sodium oxide (Na₂O), dissolves in water, it forms a metal hydroxide (an alkali or base), such as sodium hydroxide (NaOH). This hydroxide releases OH⁻ ions in the solution, making it basic. In contrast, when an acidic non-metal oxide, like sulphur dioxide (SO₂), dissolves in water, it forms an acid, such as sulphurous acid (H₂SO₃). This acid releases H⁺ ions, making the solution acidic.
4. What are amphoteric oxides? Provide examples of metals that form them.
Amphoteric oxides are a special class of metal oxides that can exhibit both acidic and basic properties. They react with both acids and bases to form salt and water. This dual nature is a key exception to the general rule that metal oxides are basic. Two common examples of metals that form amphoteric oxides are:
- Aluminium (Al): Forms Aluminium Oxide (Al₂O₃). It reacts with HCl (an acid) and NaOH (a base).
- Zinc (Zn): Forms Zinc Oxide (ZnO). It also reacts with both acids and strong bases.
5. How does an element's position in the reactivity series affect its chemical properties?
The reactivity series is a ranking of metals from highest to lowest reactivity. An element's position dictates its chemical behaviour in several ways:
- Reaction with Water/Acids: Metals at the top (e.g., potassium, sodium) are highly reactive and react vigorously with cold water and acids. Metals in the middle (e.g., zinc, iron) react with steam or acids but less vigorously. Metals at the bottom (e.g., gold, platinum) are unreactive and do not react with either.
- Displacement Reactions: Any metal can displace another metal that is positioned below it in the series from its salt solution. For example, iron (Fe) can displace copper (Cu) from a copper sulphate solution because iron is more reactive than copper.
- Method of Extraction: The reactivity series also determines how a metal is extracted from its ore. Highly reactive metals require electrolysis, while less reactive metals can be extracted by reduction with carbon.
6. What happens when a metal reacts with a solution of another metal salt?
When a metal is added to a solution of another metal's salt, a displacement reaction occurs, but only if the added metal is more reactive than the metal in the salt. The more reactive metal displaces the less reactive one from its compound. For example, if you place an iron nail (Fe) in a blue solution of copper sulphate (CuSO₄), the iron, being more reactive, will displace the copper. The solution will gradually turn light green as iron sulphate (FeSO₄) is formed, and a reddish-brown layer of copper will deposit on the nail.
7. What is the core chemical difference between how metals and non-metals form chlorides?
The core difference lies in the type of chemical bond formed. Metals react with chlorine by transferring electrons, forming ionic bonds. For instance, sodium (a metal) donates one electron to chlorine, forming sodium chloride (NaCl), which consists of Na⁺ and Cl⁻ ions. These ionic chlorides are typically crystalline solids with high melting points and conduct electricity when molten or dissolved in water. In contrast, non-metals react with chlorine by sharing electrons, forming covalent bonds. For example, hydrogen (a non-metal) shares electrons with chlorine to form hydrogen chloride (HCl), a covalent molecule. These covalent chlorides are often gases, liquids, or low-melting-point solids and do not conduct electricity.
