Periodic Table Trends of Non Metals and Their Importance
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What are Non Metals?
Non-metals are elements that accept or gain electrons to generate negative ions. They often have 4, 5, 6, or 7 electrons in their outermost shell. Non-metals are materials that lack all of the characteristics of metals. They are excellent heat and electricity insulators. They are usually gasses, although they can also be liquids. Carbon, sulphur, and phosphorus, for example, are solid at normal temperatures.
In this article, we will learn about non-metals, properties of nonmetals, periodic table metals and nonmetals.
Properties of Non-Metals
High ionization energies and electronegativity are two characteristics of non-metals. Non-metals frequently gain electrons when reacting with other compounds, forming covalent bonds, because of their features. The anionic dopants have a substantial influence on the VB among the non-metals. Carbon, nitrogen, fluorine, sulphur, and iodine are non-metal dopants.
Liquid non metal at room temperature is bromine.
Non-metals have the following properties in general.
Non-metal atoms are often smaller than metal atoms. The atomic sizes of non-metals determine the number of other properties.
Electrical conductivities of non-metals are extremely low. The most important attribute that distinguishes non-metals from metals is their low or non-existent electrical conductivity.
Electronegativities are high in non-metals. This indicates that non-metal atoms have a strong desire to keep the electrons they already have. Metals, on the other hand, readily give up one or more electrons to non-metals, allowing them to form positively charged ions and conduct electricity.
Some non-metals are found as gases, others as solids, and one is found as a liquid under normal temperature and pressure.
Due to the large number of non-metals that exist as liquids or gases, they have low melting and boiling points under typical atmospheric circumstances.
Non-metals have a tendency to be fragile in their solid state. As a result, they lack the malleability and ductility that metals have.
Periodic Table Metals and Nonmetals
The periodic table is shown below:
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In the above table nonmetal elements are H,He,C,N,O,F,Ne,P,S,Cl,Ar,Se,Br,Kr,I,Xe,At and Rn.
Lustrous Non-Metal
Metals with a shiny appearance are referred to as lustrous. Metallic lustre refers to the gleaming appearance of metals.
Examples of Lustrous Non-Metal
Metals, such as gold, silver, and copper, have the ability to reflect light from their surfaces and can be polished. Non-lustrous metals, such as lead, are an example. Non-metals have no shine. They don't have a surface that reflects light. Metals have a gleaming aspect, whereas non-metals have a dreary appearance. Diamond and iodine are two dazzling non-metal outliers.
Most Reactive Non-Metal
The most reactive nonmetals are found in the periodic table's upper right corner. Fluorine is the nonmetal with the highest reactivity. It does not exist in nature as a free element. Fluorine gas interacts explosively with a variety of other elements and compounds, making it one of the most toxic chemicals known. Fluorine is a toxic univalent gaseous halogen that is pale yellow-green in colour and is the most chemically reactive and electronegative of all elements.
Physical Properties of Non Metals
Ductility is a quality of the material that will be stretched into wires; however, non-metals are not ductile, with the exception of carbon, which is used in a range of sectors, including sports and music equipment.
The trait of malleability, which is unique to metals, is missing in non-metals. They can't be drawn into sheets since they're brittle and break when pressure is applied.
When they are hit by another material, they do not produce a sonorous sound or a deep ringing sound. Except for graphite, they are poor heat and electricity conductors.
List of Non-Metals (Complete List)
Chemical Properties of Non-Metals
1. Reaction with Water
Non-metals do not react with water, but they are usually quite reactive in air, which is why some are preserved in water. Phosphorus, for example, is a highly reactive non-metal that ignites when exposed to air, which is why it is stored in water to avoid contact with ambient oxygen.
2. Reaction with Acids
There is no evidence that any of the non-metals react with acids.
3. Reaction with Bases
The interaction of non-metals with bases is quite complicated. When chlorine reacts with bases like sodium hydroxide, it produces sodium hypochlorite, sodium chloride, and water.
4. Reaction with Oxygen
When non-metals react with oxygen, they generate oxides. Non-metal oxides are acidic or neutral in nature.
Sulfur dioxide is formed when sulfur combines with oxygen.
\[ S + O_{2} \rightarrow SO_{2}\]
Sulphur dioxide generates sulphurous acid when it combines with water
\[ SO_{2}+ H_{2}O \rightarrow H_{2}SO_{3} \]
Ferrous and Non-Ferrous Metals
What is Ferrous Metal?
The term ferrous comes from the Latin word Ferrum, which means "iron-containing metal composition." Ferrous metals are those that have only trace amounts of iron in their composition. Ferrous metals are magnetic and have high strength and hardness due to their iron content. Their properties, on the other hand, might vary substantially depending on the diversity of alloying elements that make them up. Due to their high carbon content, ferrous metals are susceptible to rust when exposed to moisture.
Examples of Ferrous Metals Use
These metals are strong and long-lasting, and they have a wide range of applications in building and engineering. Ferrous metals can be found in massive buildings like skyscrapers and bridges. Ferrous metals are also found in shipping containers, industrial pipelines, automobiles, railroad tracks, and household items.
What is Non-ferrous Metal?
Non-ferrous metals do not contain much iron and are therefore more desirable due to their conductive, non-magnetic, and lightweight qualities. Non-ferrous metals are often more expensive than ferrous metals due to their increased demand.
The malleability of non-ferrous metals is also a distinguishing feature. This implies they can be reshaped and reused multiple times without losing their value. This makes them suitable for a wide range of commercial applications.
Examples of Non-ferrous Metals Use
Copper and bronze have been credited with progressing civilization from the stone age through 1700 BCE when mankind learned to mine copper and tin to produce bronze weapons. Non-ferrous metals are being employed in building, tool manufacturing, electrical cable manufacturing, car engines, pipelines, containers, and even cutlery.
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Conclusion
From above we can conclude that non-metals are generally poor conductors of heat and electricity. Depending on the element, non-metals can be solid, liquid, or gas at room temperature. We should note that Bromine is only non-metal which is liquid at room temperature. We have learned about the physical as well chemical properties of non-metals.
FAQs on Non Metals: Definition, Properties & Examples
1. What is a non-metal and what are some common examples?
A non-metal is a chemical element that generally lacks the properties of a metal. They are typically located on the upper right side of the periodic table. Non-metals are characterized by their tendency to gain or share electrons when reacting with other elements. Common examples include Oxygen (O), Nitrogen (N), Carbon (C), Sulphur (S), Phosphorus (P), and all the halogens like Chlorine (Cl) and Iodine (I).
2. What are the key physical properties that define non-metals?
The main physical properties of non-metals are quite distinct from metals. They are typically:
Non-lustrous: They have a dull appearance and do not shine, with the exception of iodine and graphite.
Brittle: They cannot be hammered into sheets (non-malleable) or drawn into wires (non-ductile). They break or shatter when force is applied.
Poor Conductors: They are poor conductors of both heat and electricity. Graphite, an allotrope of carbon, is a notable exception.
State at Room Temperature: They can exist as solids (like Carbon, Sulphur), a liquid (Bromine), or gases (like Oxygen, Nitrogen).
Low Density and Melting Points: Most non-metals have low densities and low melting/boiling points compared to metals.
3. How are non-metals different from metals in terms of their properties?
The primary differences between metals and non-metals lie in their physical and chemical properties:
Conductivity: Metals are good conductors of heat and electricity, while non-metals are poor conductors (insulators).
Malleability & Ductility: Metals are malleable and ductile, whereas non-metals are brittle.
Oxides: Metals form basic or amphoteric oxides, while non-metals form acidic or neutral oxides.
Electron Behavior: Metals tend to lose electrons to form positive ions (cations), while non-metals tend to gain or share electrons to form negative ions (anions) or covalent bonds.
Lustre: Metals are lustrous (shiny), whereas non-metals are generally dull.
4. What are some important everyday uses of non-metals?
Non-metals are essential for life and technology. Some key uses include:
Oxygen: Crucial for respiration in all living organisms and for combustion processes.
Nitrogen: Used in the production of ammonia and fertilisers, which are vital for agriculture. It's also used in liquid form as a coolant.
Chlorine: Widely used as a disinfectant to purify drinking water and in swimming pools.
Carbon: Found in all organic life. Its allotrope, graphite, is used in pencils and as a lubricant, while diamond is used in jewellery and cutting tools.
Sulphur: Used in the manufacture of sulphuric acid, insecticides, and in the vulcanization of rubber.
5. Why do non-metals generally not conduct electricity?
The inability of most non-metals to conduct electricity is due to their atomic structure. Electrical conductivity requires the presence of free-moving charged particles, typically electrons. Non-metals have high ionisation energies and high electronegativity, meaning they hold onto their valence electrons tightly. Instead of losing electrons to become mobile, they tend to gain or share them to form covalent bonds. As a result, there are no delocalised electrons available to move and carry an electric current. The exception is graphite, where the layered structure allows for some electron mobility.
6. What happens when a non-metal reacts with oxygen? Give an example.
When a non-metal reacts with oxygen, it forms a non-metallic oxide. These oxides are typically either acidic or neutral in nature. An acidic oxide will react with water to form an acid. For example, when carbon (a non-metal) is burned in oxygen, it forms carbon dioxide (CO₂). When CO₂ dissolves in water, it forms carbonic acid (H₂CO₃), demonstrating its acidic nature.
Reaction: C (s) + O₂ (g) → CO₂ (g)
7. Why is hydrogen considered a non-metal even though it is placed in Group 1 of the periodic table with alkali metals?
Hydrogen's placement is a unique case in the periodic table. It is placed in Group 1 because, like alkali metals, it has only one valence electron (1s¹). However, its properties are overwhelmingly non-metallic. Unlike metals, hydrogen is a gas at room temperature, it forms a diatomic molecule (H₂), and it can gain an electron to form a hydride ion (H⁻), similar to halogens. Its chemical behaviour of sharing or gaining an electron is more characteristic of a non-metal than losing an electron like a typical metal.
