Difference Between Metals and Non-Metals: Properties, Location & Examples
Metals and Non-Metals is essential in chemistry and helps students understand various practical and theoretical applications related to this topic. Knowing the core differences between metals, non-metals, and metalloids makes studying the periodic table and chemical reactions easier.
This is fundamental from class 8 onwards and supports building concepts for higher-level chemistry.
What is Metals and Non-Metals in Chemistry?
A metal is an element that is generally hard, shiny, malleable, ductile, and a good conductor of heat and electricity, such as iron, copper, aluminium, or gold. In contrast, a non-metal is an element (like oxygen, sulfur, or carbon) that lacks these properties—typically being dull, non-conductive, brittle, and can be solid, liquid, or gas at room temperature.
This concept appears in chapters related to the periodic table, properties of matter, and chemical bonding, making it a foundational part of your chemistry syllabus.
Molecular Formula and Composition
Metals and non-metals are elements, so they do not have a fixed molecular formula. However, they can form compounds. For example, sodium (metal) reacts with chlorine (non-metal) to form sodium chloride (NaCl).
In the periodic table, most elements are metals, followed by fewer non-metals, and a small category of metalloids having mixed properties.
Preparation and Synthesis Methods
Metals are mainly extracted from ores using physical and chemical processes like mining, roasting, smelting, and electrolysis. Non-metals are generally found in nature in their elemental form, in minerals, or as gases in the atmosphere.
For example, oxygen is separated from air through fractional distillation, while carbon is obtained from coal. These methods are explained further in concepts related to extraction of metals and separation techniques.
Physical Properties of Metals and Non-Metals
Metals and non-metals possess clearly distinct physical properties. Below is a comparison to help you remember:
| Property | Metals | Non-Metals |
|---|---|---|
| Appearance | Shiny (lustrous) | Usually dull |
| State at Room Temperature | Mostly solid (except Mercury) | Solid, liquid, or gas |
| Malleability | Malleable (can be beaten into sheets) | Non-malleable (brittle) |
| Ductility | Ductile (drawn into wires) | Non-ductile |
| Conductivity | Good conductor of heat & electricity | Poor conductor (except graphite) |
| Density | Usually high | Usually low |
| Sonority | Sonorous (make ringing sound) | Non-sonorous |
Chemical Properties and Reactions
Metals tend to lose electrons to form positive ions (cations) and react with oxygen to form basic oxides. Non-metals tend to gain electrons (form anions) and usually form acidic oxides.
Metals often react vigorously with water and acid, while non-metals generally do not. The differences in reactivity help in understanding chemical bonding and compounds formed by metals and non-metals.
Frequent Related Errors
- Confusing metalloids (like silicon) as metals or non-metals.
- Thinking all metals are hard; sodium and potassium are soft and cut with a knife.
- Believing all non-metals are gases (most, like sulfur, are solids).
- Not recognizing graphite (a non-metal) conducts electricity.
- Assuming metals are always silver; copper and gold have different colors.
Uses of Metals and Non-Metals in Real Life
Metals like iron, aluminium, and copper are used for making wires, machinery, transport, and utensils due to their high strength and conductivity. Gold and silver are common in jewelry.
Non-metals like oxygen are vital for breathing, nitrogen is important in fertilizers, and sulfur is used in medicines and firecrackers. Everyday life relies on both groups in multiple ways for survival, comfort, and technology.
Relation with Other Chemistry Concepts
Metals and non-metals are critical for understanding classification of elements, reactivity series, and bonding types such as ionic and covalent bonds. The unique behavior of metals and non-metals in chemical reactions ties directly into periodic trends and their respective properties.
Step-by-Step Reaction Example
1. Consider the reaction between a metal and a non-metal.2. For example: Sodium (Na) reacts with chlorine (Cl2) to form sodium chloride (NaCl).
3. Balanced equation: 2Na (s) + Cl2 (g) → 2NaCl (s)
4. Sodium loses an electron (oxidized) and chlorine gains (reduced): Na → Na+ + e-; Cl2 + 2e- → 2Cl-.
5. The product, NaCl, is an ionic compound due to the transfer of electrons.
Lab or Experimental Tips
Remember: Metals usually have a shiny "metallic lustre" and ring when tapped, while non-metals do not. In class, Vedantu educators suggest using a simple scratch or hammer test to distinguish between soft metals (like sodium) and others safely, always under proper guidance.
Try This Yourself
- Name two elements that are metalloids.
- Classify the following as metal or non-metal: carbon, aluminium, sulfur, iron.
- Describe one chemical property that distinguishes metals from non-metals.
- List any three uses of non-metals in daily life.
Final Wrap-Up
We explored metals and non-metals—their defining properties, differences, common examples, extraction, and uses in real life. Understanding this topic provides a stronger foundation for more complex concepts in chemistry. To revise and expand your knowledge, check out live classes, summaries, and more detailed resources on Vedantu.
Recommended for further learning: Periodic Table, Metalloids, Properties of Metals and Nonmetals
FAQs on Metals and Non-Metals Explained with Easy Examples
1. What is the basic definition of metals and non-metals?
Metals are elements that are typically shiny, hard, and excellent conductors of heat and electricity. Examples include iron and copper. Non-metals are elements that generally lack these properties; they are often dull, brittle, and poor conductors. Examples include oxygen and carbon.
2. What are the main physical differences between metals and non-metals?
The key physical differences are:
- Lustre: Metals are shiny (lustrous), while non-metals are dull.
- Hardness: Metals are generally hard and strong, while non-metals are typically soft or brittle.
- Malleability & Ductility: Metals can be beaten into sheets (malleable) and drawn into wires (ductile). Non-metals are not.
- Conductivity: Metals are good conductors of heat and electricity, while non-metals are poor conductors (insulators).
3. What are some common examples of metals and non-metals found in everyday life?
Common examples include:
- Metals: Iron (for construction), Aluminium (in foil and cans), Copper (in electrical wires), and Gold (in jewellery).
- Non-metals: Oxygen (for breathing), Carbon (in pencil lead and diamonds), Sulphur (in matches), and Nitrogen (in fertilizers).
4. Where can I find metals, non-metals, and metalloids on the periodic table?
On the periodic table, metals are found on the left side and in the center. Non-metals are located on the upper right side. Metalloids form a diagonal 'staircase' line that separates the metals from the non-metals.
5. What are the key chemical properties that distinguish metals from non-metals?
The main chemical differences are how they react:
- Electron behavior: Metals tend to lose electrons to form positive ions (cations). Non-metals tend to gain or share electrons.
- Oxides: Metals react with oxygen to form basic oxides (e.g., magnesium oxide), while non-metals form acidic oxides (e.g., sulphur dioxide).
6. What are metalloids and why are they unique?
Metalloids are elements that have properties intermediate between those of metals and non-metals. They are unique because they aren't quite metals or non-metals. For example, they can be shiny like metals but brittle like non-metals. Their most important property is being semiconductors, which is vital for electronics. Examples include Silicon (Si) and Germanium (Ge).
7. How do metals and non-metals form different types of chemical bonds?
They form different bonds based on electron behaviour. When a metal reacts with a non-metal, the metal transfers electrons to the non-metal, forming an ionic bond. When two non-metals react, they share electrons, forming a covalent bond.
8. Why are most metals good conductors of heat and electricity?
Metals are good conductors because their atoms are packed together in a structure that allows their outer electrons to move freely. This 'sea' of delocalised electrons can easily flow to carry an electric current or transfer heat energy from one part of the metal to another.
9. If most metals are solid, why is mercury a liquid at room temperature?
Mercury is a fascinating exception. The forces holding its atoms together, known as metallic bonds, are unusually weak compared to other metals. Because these bonds are weak, it takes very little heat energy to break them, causing mercury to have a very low melting point and exist as a liquid at room temperature.
10. How can a non-metal like graphite conduct electricity when others cannot?
Graphite, a form of carbon, has a unique layered structure. Within each layer, every carbon atom is bonded to three other atoms, leaving one free electron per atom. These free electrons can move along the layers, allowing graphite to conduct electricity, much like the free electrons in metals do.
11. Why are metalloids like silicon so important for making electronics?
Metalloids like silicon are crucial because they are semiconductors. This means their ability to conduct electricity can be precisely controlled. By adding tiny amounts of impurities (a process called doping), we can turn them into the on/off switches, known as transistors, that form the building blocks of all modern electronic devices like smartphones and computers.
12. Why do metals generally form basic oxides while non-metals form acidic oxides?
This happens because of what their oxides do in water. When a metal oxide (like sodium oxide) dissolves in water, it forms a metal hydroxide, which is a base. When a non-metal oxide (like sulphur dioxide) dissolves in water, it forms an acid (like sulphurous acid). This fundamental difference in chemical behaviour is a key distinction between the two groups.
