What Are the Chemical Properties of Metals and Nonmetals with Reactions and 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 Explained Clearly
1. What are the chemical properties of metals?
The chemical properties of metals include their tendency to lose electrons, form positive ions, react with oxygen to form basic oxides, and react with acids to release hydrogen gas.
- Metals form cations by losing electrons (e.g., Na → Na+ + e-).
- They react with oxygen to form metal oxides: 2Mg(s) + O2(g) → 2MgO(s).
- They react with dilute acids to produce salt and hydrogen gas: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g).
- Many metals react with water to form hydroxides and hydrogen gas.
2. What are the chemical properties of nonmetals?
The chemical properties of nonmetals include their tendency to gain or share electrons, form negative ions, and produce acidic oxides when reacting with oxygen.
- Nonmetals form anions by gaining electrons (e.g., Cl + e- → Cl-).
- They react with oxygen to form acidic oxides: C(s) + O2(g) → CO2(g).
- Nonmetal oxides react with water to form acids: SO3(g) + H2O(l) → H2SO4(aq).
- They usually form covalent compounds by sharing electrons.
3. How do metals react with oxygen?
Metals react with oxygen to form metal oxides, which are generally basic in nature.
- General reaction: Metal + O2 → Metal oxide.
- Example: 4Al(s) + 3O2(g) → 2Al2O3(s).
- Most metal oxides dissolve in water to form bases: CaO(s) + H2O(l) → Ca(OH)2(aq).
- Some metals like gold and platinum are less reactive and do not easily form oxides.
4. How do nonmetals react with oxygen?
Nonmetals react with oxygen to form nonmetal oxides, which are usually acidic in nature.
- Example: S(s) + O2(g) → SO2(g).
- Nonmetal oxides form acids in water: SO2(g) + H2O(l) → H2SO3(aq).
- Carbon forms CO2, which produces carbonic acid in water.
- These reactions explain why nonmetals are associated with acidic properties.
5. What happens when metals react with water?
When metals react with water, they form metal hydroxides or oxides and release hydrogen gas.
- Highly reactive metals: 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g).
- Moderately reactive metals: Mg(s) + 2H2O(l) → Mg(OH)2(aq) + H2(g).
- Less reactive metals react only with steam: 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g).
6. Why do metals form positive ions and nonmetals form negative ions?
Metals form positive ions because they lose electrons easily, while nonmetals form negative ions because they gain electrons to complete their valence shell.
- Metals have low ionization energy, so they lose electrons (e.g., K → K+ + e-).
- Nonmetals have high electron affinity, so they gain electrons (e.g., O + 2e- → O2-).
- This electron transfer leads to ionic bond formation.
7. What is the difference between metal oxides and nonmetal oxides?
The main difference is that metal oxides are basic, while nonmetal oxides are acidic in nature.
- Metal oxide example: Na2O(s) + H2O(l) → 2NaOH(aq).
- Nonmetal oxide example: CO2(g) + H2O(l) → H2CO3(aq).
- Metal oxides neutralize acids, while nonmetal oxides neutralize bases.
- Some oxides like Al2O3 are amphoteric, showing both acidic and basic behavior.
8. How do metals react with acids?
Metals react with dilute acids to produce a salt and hydrogen gas.
- General reaction: Metal + Acid → Salt + H2.
- Example: Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g).
- Only metals above hydrogen in the reactivity series can displace hydrogen from acids.
- Less reactive metals like copper do not react with dilute HCl.
9. Can nonmetals react with acids?
Nonmetals generally do not react with dilute acids because they cannot displace hydrogen from acids.
- Hydrogen displacement requires a more reactive metal.
- Nonmetals like sulfur and carbon do not produce hydrogen gas with dilute HCl or H2SO4.
- However, some nonmetals can react under special conditions, such as oxidation reactions with concentrated acids.
10. What is the reactivity series of metals and why is it important?
The reactivity series of metals is a list that arranges metals in order of decreasing chemical reactivity.
- Common order: K > Na > Ca > Mg > Al > Zn > Fe > Pb > H > Cu > Hg > Ag > Au.
- It predicts reactions with water and acids.
- A more reactive metal can displace a less reactive metal from its salt: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s).
- It is essential for understanding metal extraction and displacement reactions.
