what reacts with a metal to form a salt
Certain soft and weak elements do not conduct oestrus or electricity, are neither malleable nor ductile, and are brittle. Such metals are called not-metals. But 22 of the 118 known elements are not-metals. Non-metals include carbon, oxygen, nitrogen, and sulphur, to name a few. In this article, we volition learn about various chemical properties of non-metals and their reaction with different elements and compounds.
Chemic Backdrop of Non-metals
A big amount of energy is released when a not-metal accepts one or more electrons. On the other hand, a large corporeality of free energy is needed to remove 1 or more electrons from non-metals. Hence non-metals do not form positively charged ions but readily form negatively charged ions. Thus, the non-metals are electropositive elements. It can be represented in the equation as:
- \(\mathop {{\rm{Cl}}}\limits_{{\rm{Chlorine}}\,{\rm{atom}}} + {{\rm{due east}}^ – } \to \mathop {{\rm{C}}{{\rm{l}}^ – }}\limits_{{\rm{Chloride}}\,{\rm{ion}}} \)
- \(\mathop {\rm{O}}\limits_{{\rm{Oxygen}}\,{\rm{atom}}} + 2{{\rm{east}}^ – } \to \mathop {{{\rm{O}}^{2 – }}}\limits_{{\rm{Oxide}}\,{\rm{ion}}} \)
- \(\mathop {\rm{S}}\limits_{{\rm{Sulphur}}\,{\rm{atom}}} + 2{{\rm{e}}^ – } \to \mathop {{{\rm{Southward}}^{2 – }}}\limits_{{\rm{Sulphide}}\,{\rm{ion}}} \)
- \(\mathop {\rm{N}}\limits_{{\rm{Nitrogen}}\,{\rm{atom}}} + iii{{\rm{e}}^ – } \to \mathop {{{\rm{N}}^{3 – }}}\limits_{{\rm{Nitride}}\,{\rm{ion}}} \)
Reaction of Non-metals with Oxygen
Not-metals react with oxygen on heating to form oxides. These oxides may exist acidic or neutral oxides. But they do not form basic oxides. The acidic oxides of non-metals dissolve in water to form acids.
Let united states illustrate the chemical reactions of a few non-metals with oxygen.
Acidic Oxides
The non-metallic oxides which dissolve in water to form acids are called acidic oxides.
Example one: Reaction of carbon with oxygen
When carbon burns in excess of air, information technology forms carbon dioxide, which is an acidic oxide. This oxide dissolves in water to form carbonic acid. The chemical equation involved is as follows.
\({\rm{C}} + {{\rm{O}}_2} \to {\rm{C}}{{\rm{O}}_2}\)
\({\rm{C}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{C}}{{\rm{O}}_3}\)
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Case two: Reaction of sulphur with oxygen
When sulphur reacts with oxygen, it forms sulphur dioxide, an acidic oxide. It dissolves in h2o to form sulphurous acrid. The chemical equation involved is as follows:
\({\rm{South}}\left( {\rm{s}} \right) + {{\rm{O}}_2}\left( {\rm{g}} \right) \to {\rm{S}}{{\rm{O}}_2}\left( {\rm{g}} \correct)\)
\({\rm{S}}{{\rm{O}}_2}\left( {\rm{m}} \correct) + {{\rm{H}}_2}{\rm{O}}\left( {\rm{l}} \right) \to {{\rm{H}}_2}{\rm{Due south}}{{\rm{O}}_3}\left( {{\rm{aq}}} \correct)\)
Neutral Oxides
The non-metallic oxides that neither reacts with acid nor with bases are called neutral oxides. Let u.s. illustrate this reaction with a few non-metals.
Example ane: Reaction of carbon with oxygen
When carbon burns in a limited supply of oxygen, it forms carbon monoxide.
\(ii{\rm{C}} + {{\rm{O}}_2} \to ii{\rm{CO}}\)
The carbon monoxide thus formed does non produce acid with water.
Example ii: Reaction of hydrogen with oxygen
When hydrogen combines with oxygen, it forms water. This reaction takes identify only when an electrical spark is introduced.
\(2{{\rm{H}}_2} + {{\rm{O}}_2} \to 2{{\rm{H}}_2}{\rm{O}}\)
Example 3: Reaction of nitrogen with oxygen
Nitrogen and oxygen react at a high temperature of nearly 2700°C-3000℃ to produce a depression yield of nitric oxide.
\({{\rm{N}}_2}\left( {\rm{grand}} \correct) + {{\rm{O}}_2}\left( {\rm{g}} \right) \to 2{\rm{NO}}\)
In all of the in a higher place reactions, all the non-metallic oxides are formed by sharing electrons, and then are covalent compounds. Hence, non-metallic oxides do non contain any oxide ions.
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Reactions of Non-metals with H2o
Usually, non-metals practise not react with water to produce hydrogen gas. This is because non-metals cannot reduce hydrogen ions of water to hydrogen gas. Only a few highly reactive not-metals such as fluorine react with water to grade oxygen or ozone \(\left( {{{\rm{O}}_3}} \correct)\) molecules. The reactions involved are as follows.
\(2{{\rm{F}}_2}\left( {\rm{g}} \right) + 2{{\rm{H}}_2}{\rm{O}}\left( {\rm{l}} \right) \to four{\rm{HF}}\left( {{\rm{aq}}} \right) + {{\rm{O}}_2}\left( {\rm{g}} \right)\)
\({\rm{3}}{{\rm{F}}_2}\left( {\rm{g}} \right) + iii{{\rm{H}}_2}{\rm{O}}\left( {\rm{l}} \correct) \to 6{\rm{HF}}\left( {{\rm{aq}}} \correct) + {{\rm{O}}_3}\left( {\rm{k}} \correct)\)
Reaction of Not-metals with Dilute Acids
Non-metals do not react with dilute acids. In other words, not-metals do not displace hydrogen from acids. For case, the non-metals similar carbon, sulphur and phosphorus practise not react with dilute hydrochloric acid or dilute sulphuric acid to produce hydrogen gas. Permit us run into why not-metals are not able to displace hydrogen from acids.
In order to displace hydrogen ions \(\left( {{{\rm{H}}^ + }} \right)\) of an acid and convert them into hydrogen gas, electrons should exist supplied to the hydrogen ions of the acrid. Now, a not-metallic, beingness itself, an acceptor of electrons, cannot give electrons to the hydrogen ions of the acrid to reduce them to hydrogen gas.
And hence the not-metals are non able to displace hydrogen ions from acids to class hydrogen gas. Thus, if non-metals similar carbon, sulphur, phosphorus are put into a test tube containing dilute sulphuric acid (or dilute hydrochloric acid), then no hydrogen gas is evolved.
Reaction of Non-metals with Salt Solutions
Generally, a more than reactive non-metal displaces less reactive non-metal from its salt solution. We can illustrate this with a few examples.
Instance one: Reaction of chlorine with sodium bromide
\({\rm{C}}{{\rm{l}}_2}\left( {\rm{1000}} \right) + 2{\rm{NaBr}}\left( {{\rm{aq}}} \right) \to 2{\rm{NaCl}}\left( {{\rm{aq}}} \right) + {\rm{B}}{{\rm{r}}_2}\left( {\rm{g}} \right)\)
When chlorine gas is passed through a solution of sodium bromide, sodium chloride, along with bromine gas, is formed. In this reaction, more than reactive non-metal chlorine displaces less reactive non-metallic bromine from its salt solution sodium bromide.
Example 2: Reaction of chlorine with potassium iodide
When chlorine gas is passed through a solution of potassium iodide, potassium chloride, along with iodine gas, is formed.
\({\rm{C}}{{\rm{l}}_2}\left( {\rm{g}} \right) + 2{\rm{KI}}\left( {{\rm{aq}}} \right) \to two{\rm{KCl}}\left( {{\rm{aq}}} \right) + {{\rm{I}}_2}\left( {\rm{S}} \correct)\)
In this reaction, more reactive not-metal chlorine displaces less reactive not-metal iodine from its table salt solution potassium iodide.
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Reaction of Non-metals with Chlorine
Generally, not-metals react with chlorine to class covalent chlorides. This is because these chlorides are formed past sharing of electrons betwixt the atoms of non-metals and the chlorine. Hence, these chlorides are covalent compounds. These chlorides are non-electrolytes as they do not bear electricity. These chlorides are as well volatile liquids or gases.
Let us illustrate the reaction betwixt non-metals and chlorine with a few examples.
Example 1: Reaction of hydrogen and chlorine
When hydrogen reacts with chlorine in the presence of diffused sunlight, it forms hydrogen chloride gas.
\({\rm{C}}{{\rm{l}}_2} + {{\rm{H}}_2} \to ii{\rm{HCl}}\)
Instance 2: Reaction of phosphorus and chlorine
When phosphorus reacts with chlorine, it forms phosphorus trichloride.
\(half dozen{\rm{C}}{{\rm{50}}_2} + {{\rm{P}}_4} \to iv{\rm{PC}}{{\rm{l}}_3}\)
Sometimes phosphorus reacts with excess chlorine to class phosphorus pentachloride \(\left( {{\rm{PC}}{{\rm{l}}_5}} \right).\)
Example 3: Reaction of carbon with chlorine
When carbon reacts with chlorine, it forms carbon tetrachloride \(\left( {{\rm{CC}}{{\rm{l}}_4}} \correct).\)
\(2{\rm{C}}{{\rm{l}}_2}\left( {\rm{g}} \right) + {\rm{C}}\left( {\rm{s}} \correct) \to {\rm{CC}}{{\rm{l}}_4}\left( {\rm{l}} \right)\)
\({\rm{CC}}{{\rm{50}}_4}\) does not carry electricity as it contains a covalent bond and has no ions for bonding.
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Reaction with Hydrogen
Non-metals react with hydrogen to form covalent hydrides. The sharing of electrons forms the non-metal hydrides. That is, non-metal hydrides are formed by covalent bonding. Here are some examples.
- Sulphur is a non-metallic which combines with hydrogen to form a covalent hydride called hydrogen sulphide, \({{\rm{H}}_2}{\rm{S}}{\rm{.}}\)
- \(\mathop {{\rm{Southward}}\left( {\rm{south}} \correct)}\limits_{{\rm{Sulphur}}} + \mathop {{{\rm{H}}_2}\left( {\rm{g}} \right)}\limits_{{\rm{Hydrogen}}} \to \mathop {{{\rm{H}}_2}{\rm{S}}\left( {\rm{g}} \right)}\limits_{{\rm{Hydrogen}}\,{\rm{sulphide}}} \)
- The hydrogen sulphide gas has the characteristic smell resembling the smell of rotten eggs.
- Nitrogen is a non-metal that combines with hydrogen in the presence of an iron catalyst to course a covalent hydride called ammonia.
- \(\mathop {{{\rm{N}}_2}\left( {\rm{g}} \right)}\limits_{{\rm{Nitrogen}}} + \mathop {{\rm{three}}{{\rm{H}}_2}\left( {\rm{thousand}} \right)}\limits_{{\rm{Hydrogen}}} \to \mathop {{\rm{2N}}{{\rm{H}}_3}\left( {\rm{g}} \correct)}\limits_{{\rm{Ammonia}}} \)
Oxygen is also a non-metal which combines with hydrogen to form a hydride called h2o. Similarly, the hydride of carbon in methane and the hydride of chlorine is \({\rm{HCl}}.\) The not-metal hydrides are covalent compounds formed by the sharing of electrons. Not-metals form covalent hydrides because non-metal atoms cannot give electrons to hydrogen atoms to form hydride ions. Non-metal hydrides are liquids or gases. Not-metal hydrides do not contain ions, and hence they do not conduct electricity. Non-metallic hydrides are stable compounds.
Differences Between Metals and Non-metals
| Metal | Not-metal |
| Metals form positive ions. Examples: \({\rm{Northward}}{{\rm{a}}^ + },\,{{\rm{G}}^ + },\,{\rm{C}}{{\rm{a}}^{ii + }},\,{\rm{M}}{{\rm{grand}}^{two + }},\,{\rm{F}}{{\rm{e}}^{2 + }},\) etc.. | Non-metals form negative ions. Examples: \({\rm{C}}{{\rm{l}}^ – },\,{{\rm{South}}^{2 – }},\,{{\rm{N}}^{3 – }},\) etc.. |
| Oxides of metals are basic in nature, i.east., the oxides of metals react with water to give bases or alkalis. \({\rm{Due north}}{{\rm{a}}_2}{\rm{O}} + {{\rm{H}}_2}{\rm{O}} \to 2{\rm{NaOH}}\) \({\rm{CaO}} + {{\rm{H}}_2}{\rm{O}} \to {\rm{Ca}}{\left( {{\rm{OH}}} \right)_2}\) | Oxides of non-metals are acidic in nature, i.e., the oxides of non-metals react with water to give acids. \({\rm{C}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{C}}{{\rm{O}}_3}\) \({\rm{Due south}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{S}}{{\rm{O}}_3}\) \({\rm{S}}{{\rm{O}}_3} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\) |
| Metals dissolve in dilute acids to produce hydrogen gas. \({\rm{Zn}} + {{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4} \to {\rm{ZnS}}{{\rm{O}}_4} + {{\rm{H}}_2}\) Exceptions Some metals do not produce hydrogen when treated with an acid nether ordinary circumstances. | Non-metals generally practise non dissolve in dilute acids. |
| Metals, in general do not combine with hydrogen. Exceptions Some metals (\({\rm{Na}},\,{\rm{Ca}},\,{\rm{Li}},\,{\rm{Be}}\) etc.) combine with hydrogen to course non-volatile unstable hydrides. | Non-metals combine with hydrogen to class stable compounds. |
| Metallic chlorides are generally non hydrolyzed by water or are simply partially hydrolyzed. \({\rm{NaCl}} + {{\rm{H}}_2}{\rm{O}} \to {\rm{No}}\,{\rm{hydrolysis}}\) \({\rm{AlC}}{{\rm{l}}_3} + three{{\rm{H}}_2}{\rm{O}} \to {\rm{Al}}{\left( {{\rm{OH}}} \correct)_3} + 3{\rm{HCl}}\) | Chlorides of not-metals are usually hydrolyzed by water. \({\rm{PC}}{{\rm{I}}_3} + three{{\rm{H}}_2}{\rm{O}} \to 3{\rm{HCl}} + {{\rm{H}}_3}{\rm{P}}{{\rm{O}}_3}\) \({\rm{SiC}}{{\rm{l}}_4} + 4{{\rm{H}}_2}{\rm{O}} \to {\rm{Si}}{\left( {{\rm{OH}}} \right)_4} + 4{\rm{HCl}}\) |
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Summary
There are simply \(22\) non-metal elements, of which \(11\) are gases, 1 is a liquid, and the rest \(x\) are solids. Oxygen is a non-metal which is essential for our survival. Non- metal course anions past gaining electrons to complete their octet. In this article, we learn about how the non-metals react with water, oxygen, dilute acids, salt solutions, chlorine and hydrogen.
FAQs
Q.1. What are the chemic properties of non-metallic?
Ans:
(a) At room temperature, almost not-metals do not react with air.
(b) The simply non-metallic is white phosphorus, which burns to generate its oxide afterward reacting with air.
(c) Not-metals exist in all states of matter at room temperature.
(d) Alloys do not form with non-metals. Some elements, such as carbon, silicon, and phosphorus, can class.
(e) Not-metals do not react with dilute acids.
Q.2. What are 4 chemical properties?
Ans: The 4 chemical properties are:
(a) Non-metals are electronegative elements.
(b) Non-metals form acidic or neutral oxides.
(c) Non-metals grade covalent chlorides.
(d) Non-metals carry equally oxidizing agents.
Q.three. What are the chemical differences betwixt metals and non-metals?
Ans: The chemical differences between metals and non-metals are:
| Reaction with | Metals | Not-metals |
| Oxygen | Metallic oxides are formed, which are by and large basic in nature. | Non-metal oxides are formed, which are more often than not acidic in nature. |
| H2o | Metallic hydroxides are formed. | Generally, do not react. |
| Dilute acid | Metals more reactive than hydrogen displace hydrogen from dilute acids to course metal salts and hydrogen gas. | Practise not react with dilute acids. |
| Salt solution | More than reactive metallic displaces less reactive metal from its table salt solution. | Not-metal that is more than reactive displaces less reactive non-metallic from its salt solution. |
| Chlorine | Metal chlorides are formed, which are ionic in nature. | Non-metallic chlorides are formed, which are covalent in nature. |
| Hydrogen | Ionic metal hydrides are formed by reactive metals. | Covalent hydrides are formed. |
Q.4. What happens when the non-metal oxide is dissolved in water?
Ans: Some oxides of not-metals are acidic in nature and form acids when dissolved in water. For example, when sulphur dioxide is dissolved in water, the product obtained is sulphurous acrid. This reaction is as follows:
\({\rm{Due south}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{S}}{{\rm{O}}_3}\)
Q.5. Why are non-metals called electronegative elements?
Ans: Non-metals are chosen electronegative elements as they have the trend to accept electrons to obtain a stable electronic configuration. Thus, by accepting electrons, non-metals form negatively charged ions. Hence, non-metals are called electronegative elements.
Q.6. What is the nature of oxides of non-metals? How volition you justify their nature?
Ans: The oxides formed by most of the non-metals are acidic in nature. For instance, \({\rm{C}}{{\rm{O}}_2}\) and \({\rm{S}}{{\rm{O}}_2}\) are acidic in nature. Their reaction shows the acidic nature of these oxides to h2o.
Carbon dioxide dissolves in water to class carbonic acid. Thus, it is acidic in nature.
\(\mathop {{\rm{C}}{{\rm{O}}_2}\left( {\rm{g}} \correct)}\limits_{{\rm{Carbon}}\,{\rm{dioxide}}} + \mathop {{{\rm{H}}_2}{\rm{O}}\left( {\rm{50}} \correct)}\limits_{{\rm{Water}}} \to \mathop {{{\rm{H}}_2}{\rm{C}}{{\rm{O}}_3}\left( {{\rm{aq}}} \right)}\limits_{{\rm{Carbon}}\,{\rm{acrid}}} \)
Sulphur dioxide also dissolves in water to form an acid called sulphurous acid. Thus, information technology is too acidic in nature.
\(\mathop {{\rm{Due south}}{{\rm{O}}_2}\left( {\rm{grand}} \correct)}\limits_{{\rm{Sulphur}}\,{\rm{dioxide}}} + \mathop {{{\rm{H}}_2}{\rm{O}}\left( {\rm{l}} \right)}\limits_{{\rm{Water}}} \to \mathop {{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_3}\left( {{\rm{aq}}} \right)}\limits_{{\rm{Sulphurous}}\,{\rm{acrid}}} \)
Nosotros hope this article on the chemical properties of non-metals has helped you. If you have any queries, drop a comment below, and we will become dorsum to you.
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