Mix Examples - Metals and Non-metals Questions in English

(A) Magnalium is an alloy of aluminum $(Al)$ and magnesium $(Mg)$. It is known for its high strength,low density,and resistance to corrosion. Due to these properties,it is widely used in the construction of scientific balances,aircraft parts,and precision instruments.

(B) Bronze is an alloy consisting primarily of copper,usually with tin as the main additive. The composition typically ranges from $88\%$ copper and $12\%$ tin. Therefore,the correct components are copper and tin.

(C) Duralumin is an alloy of aluminum $(95\%)$, copper $(4\%)$, magnesium $(0.5\%)$, and manganese $(0.5\%)$.
It is widely used in the aerospace industry for manufacturing aircraft parts due to its high strength-to-weight ratio and excellent corrosion resistance.

(B) Stainless steel is an alloy of iron,chromium,and nickel. It is highly resistant to corrosion and rust,making it the ideal material for manufacturing surgical instruments that require sterilization and durability.

(D) German silver is an alloy consisting of copper $(Cu)$,zinc $(Zn)$,and nickel $(Ni)$.
It does not contain any silver,despite its name.
Since it is a homogeneous mixture of two or more metals,it is classified as an alloy.

(C) Pure gold is known as $24$ carat gold.
It is very soft and ductile,making it unsuitable for making jewelry in its pure form.
Therefore,it is usually alloyed with small amounts of other metals like silver or copper to make it harder.

(B) Pure gold is $24$ carat,which is very soft and not suitable for making jewelry.
To make it harder and durable,it is alloyed with small amounts of other metals like copper or silver.
Typically,gold jewelry is made using $22$ carat gold,which consists of $22$ parts gold and $2$ parts of other metals.

(B) $24$ carat gold is considered pure gold.
$22$ carat gold means that it contains $22$ parts of pure gold mixed with $2$ parts of either copper or silver to make it hard enough for jewelry making.
Therefore,the correct proportion is $22$ parts pure gold and $2$ parts copper.

(C) Haematite is one of the most important ores of iron.
Its chemical formula is $Fe_{2}O_{3}$.
- $Fe_{3}O_{4}$ is the formula for Magnetite.
- $FeCO_{3}$ is the formula for Siderite.
- $FeS_{2}$ is the formula for Iron Pyrites (Fool's Gold).
Therefore,the correct option is $C$.

(D) In a blast furnace,$Coke$ $(C)$ acts as a reducing agent. It reacts with oxygen to form carbon monoxide $(CO)$,which then reduces iron oxides to molten iron. Furthermore,the presence of $Coke$ and the reducing atmosphere created by $CO$ prevents the re-oxidation of the molten iron produced.

(A) In the extraction of iron from its ore,limestone $(CaCO_{3})$ is added as a flux.
At high temperatures,limestone decomposes to form calcium oxide $(CaO)$ and carbon dioxide $(CO_{2})$.
The calcium oxide $(CaO)$ reacts with the silica $(SiO_{2})$ impurity present in the ore to form calcium silicate $(CaSiO_{3})$,which is known as slag.
The chemical reaction is: $CaO + SiO_{2} \rightarrow CaSiO_{3}$ (slag).
Therefore,the correct molecular formula for calcium silicate is $CaSiO_{3}$.

(D) Let us evaluate each group:
$(1)$ Iron - Magnetite - $Fe_{3}O_{4}$: This is correct. Magnetite is an oxide ore of iron with the formula $Fe_{3}O_{4}$.
$(2)$ Iron - Siderite - $FeS_{2}$: This is incorrect. Siderite is $FeCO_{3}$. $FeS_{2}$ is Iron Pyrites.
$(3)$ Copper - Copper glance - $Cu_{2}S$: This is correct. Copper glance (Chalcocite) is a sulfide ore of copper with the formula $Cu_{2}S$.
$(4)$ Copper - Dolomite - $Al_{2}O_{3}$: This is incorrect. Dolomite is $CaCO_{3} \cdot MgCO_{3}$. $Al_{2}O_{3}$ is Corundum (an ore of Aluminum).
Therefore, only groups $(1)$ and $(3)$ are correct.

(C) The only non-metal that exists in a liquid state at room temperature is $Bromine$ $(Br)$.
$Carbon$, $Hydrogen$, and $Phosphorus$ are typically found as solids or gases under standard conditions.

(D) Carbon is a non-metal.
$1$. Carbon reacts with $O_2$ (dioxygen) to form $CO_2$ or $CO$.
$2$. Carbon reacts with $H_2$ (dihydrogen) at high temperatures to form hydrocarbons like methane $(CH_4)$.
$3$. Carbon reacts with $Cl_2$ (dichlorine) to form carbon tetrachloride $(CCl_4)$.
$4$. Carbon does not react with dilute hydrochloric acid $(HCl)$ because it is a non-metal and cannot displace hydrogen from the acid.

(D) Oxides are generally classified as acidic,basic,amphoteric,or neutral.
$CO_{2}$,$SO_{2}$,and $P_{2}O_{5}$ are non-metallic oxides that react with water to form acids,making them acidic in nature.
$N_{2}O$ (nitrous oxide),$NO$ (nitric oxide),and $CO$ (carbon monoxide) are well-known examples of neutral oxides.
Neutral oxides do not react with either acids or bases to form salts.
Therefore,$N_{2}O$ is the correct answer.

(A) $H_{2}$ (Hydrogen gas) is non-polar and does not form hydrogen bonds with water,making it practically insoluble in water.
$CO_{2}$ (Carbon dioxide) is slightly soluble in water,forming carbonic acid $(H_{2}CO_{3})$.
$NH_{3}$ (Ammonia) and $SO_{2}$ (Sulfur dioxide) are highly soluble in water due to their polar nature and ability to form hydrogen bonds or react with water.

(B) $SO_{2}$ (Sulfur dioxide) is widely used as a food preservative in fruit juices,jams,and squashes.
It acts as an antimicrobial agent,inhibiting the growth of bacteria,yeasts,and molds,thereby extending the shelf life of these products.
It also helps in preventing the browning of fruits due to oxidation.

(B) $H_{2}SO_{4}$ (Sulfuric acid) is known as 'the king of chemicals'.
This is because it is used extensively in various industrial processes,including the manufacturing of fertilizers,dyes,pigments,detergents,and explosives.
It is also a vital component in lead-acid batteries used in automobiles.

(B) Combustible gases are those that can burn in the presence of oxygen to release energy.
$H_{2}$ (Hydrogen gas) is highly combustible and reacts with oxygen to form water,releasing a significant amount of heat.
$CO_{2}$ (Carbon dioxide) is a product of combustion and does not support burning.
$SO_{2}$ (Sulfur dioxide) is not combustible.
$NH_{3}$ (Ammonia) is generally considered non-combustible under normal conditions,although it can burn under specific high-temperature conditions,$H_{2}$ is the most standard example of a highly combustible gas in this context.

(D) The Haber process is used for the industrial production of ammonia $(NH_{3})$ from nitrogen $(N_{2})$ and hydrogen $(H_{2})$ gases.
The chemical equation for the reaction is: $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$.
In this process,finely divided iron $(Fe)$ is used as a catalyst to increase the rate of the reaction.
Additionally,molybdenum $(Mo)$ is often used as a promoter to enhance the efficiency of the iron catalyst.

(B) The correct pairings are as follows:
$1$. Extraction of sulphur is done by the $Frasch$ method $(1-q)$.
$2$. Production of nitric acid is done by $Ostwald's$ method $(2-s)$.
$3$. Production of sulphuric acid is done by the $Contact$ process $(3-p)$.
$4$. Production of ammonia gas is done by $Haber's$ process $(4-r)$.
Therefore,the correct sequence is $(1-q), (2-s), (3-p), (4-r)$.

(D) The correct pairings are as follows:
$1.$ Dehydrating agent: Concentrated sulphuric acid $(H_2SO_4)$ is a well-known dehydrating agent that removes water molecules from compounds. Thus, $(1-q)$.
$2.$ In preparation of firecrackers: Sulphur is commonly used in the manufacturing of gunpowder and firecrackers. Thus, $(2-s)$.
$3.$ Weak bleaching agent: Sulphur dioxide $(SO_2)$ acts as a weak bleaching agent, especially for delicate materials like wool and silk. Thus, $(3-p)$.
$4.$ Lightest gas: Dihydrogen $(H_2)$ is the lightest gas in the periodic table. Thus, $(4-r)$.
Therefore, the correct sequence is $(1-q), (2-s), (3-p), (4-r)$.

(C) The chemical formulas for the given acids are as follows:
$1$. Sulphurous acid is $H_{2}SO_{3}$.
$2$. Sulphuric acid is $H_{2}SO_{4}$.
$3$. Oleum (also known as fuming sulphuric acid) is $H_{2}S_{2}O_{7}$.
$4$. Phosphoric acid is $H_{3}PO_{4}$.
Matching these with the given options:
$1-r, 2-s, 3-q, 4-p$.
Therefore, the correct option is $C$.

(D) In the periodic table,elements are broadly classified into metals,non-metals,and metalloids.
Out of the $114$ elements discovered,$22$ elements are classified as non-metals.
These elements do not exhibit metallic properties such as luster,malleability,ductility,or high electrical conductivity.
Therefore,the correct answer is $22$.

(A) At room temperature,most non-metals are either solids or gases.
Among the given options,$Chlorine$ $(Cl_2)$ is a non-metal that exists as a gas.
$Sulfur$ and $Phosphorus$ are solids at room temperature.
$Bromine$ is a non-metal that exists as a liquid at room temperature.
Therefore,the correct option is $A$.

(C) Non-metals can exist in solid,liquid,or gaseous states at room temperature.
$1$. Bromine $(Br_2)$ is the only non-metal that exists in a liquid state at room temperature.
$2$. Chlorine $(Cl_2)$ and Hydrogen $(H_2)$ exist in a gaseous state at room temperature.
$3$. Sulfur $(S_8)$ is a non-metal that exists in a solid state at room temperature.
Therefore,the correct option is $C$.

(A) Phosphorus is a non-metal that exists in a solid state at room temperature. It is commonly found in different allotropic forms such as white phosphorus and red phosphorus,both of which are solids.

(A) Carbon is the fundamental element that forms the backbone of all organic molecules,including vitamins,proteins,and carbohydrates. These compounds are known as organic compounds because they are primarily composed of carbon atoms bonded to hydrogen,oxygen,nitrogen,and other elements. Carbon's unique ability to form stable covalent bonds with itself and other atoms allows for the complex structures required for life.

(D) Generally,non-metals are non-lustrous and appear dull. However,$Iodine$ is an exception among non-metals as it possesses a characteristic metallic luster. Therefore,the correct option is $D$.

(B) Most non-metals are poor conductors of electricity because they lack free electrons.
However,$Graphite$,an allotrope of carbon,contains free electrons in its structure due to its hexagonal layered arrangement.
These free electrons allow $Graphite$ to conduct electricity,making it an exception among non-metals.

(C) Ammonia $(NH_3)$ is a chemical substance composed of nitrogen and hydrogen atoms in a fixed ratio of $1:3$.
Since it is formed by the chemical combination of two different elements,it is classified as a compound.
Elements are pure substances consisting of only one type of atom,whereas mixtures are physical combinations of substances without fixed proportions.
Therefore,ammonia is a compound.

(B) Non-metals react with oxygen to form non-metallic oxides.
These oxides are generally acidic in nature because they dissolve in water to form acids (e.g.,$SO_2 + H_2O \rightarrow H_2SO_3$).
Some non-metallic oxides,such as carbon monoxide $(CO)$,water $(H_2O)$,and nitrous oxide $(N_2O)$,are neutral in nature.
Therefore,non-metal oxides are typically acidic or neutral.

(C) Non-metals react with oxygen to form oxides that are generally acidic in nature.
$CO_{2}$ (Carbon dioxide) is an oxide of a non-metal (Carbon).
When $CO_{2}$ dissolves in water,it forms carbonic acid $(H_{2}CO_{3})$,which confirms its acidic nature.
Therefore,$CO_{2}$ is an acidic oxide.

(D) $H_{2}O$ (water) is a neutral oxide. It does not change the color of red or blue litmus paper,indicating that it is neither acidic nor basic in nature. It acts as a solvent and can react with both acids and bases depending on the conditions,but it is classified as a neutral oxide.

(B) Neutral oxides are those that do not react with either acids or bases. Common examples of neutral oxides include $N_{2}O$,$NO$,and $CO$.
$SO_{2}$ is an acidic oxide because it reacts with water to form sulfurous acid $(H_{2}SO_{3})$ and reacts with bases to form salts.
Therefore,$SO_{2}$ is not a neutral oxide.

(A) When sulfur dioxide $(SO_{2})$ reacts with water $(H_{2}O)$,it forms sulfurous acid $(H_{2}SO_{3})$.
The chemical equation for this reaction is: $SO_{2} + H_{2}O \rightarrow H_{2}SO_{3}$.
Sulfurous acid is a weak acid formed by the dissolution of sulfur dioxide in water.

(C) Phosphorus pentoxide is a chemical compound with the empirical formula $P_{2}O_{5}$.
However,in its solid state,it exists as a dimer with the molecular formula $P_{4}O_{10}$.
While $P_{2}O_{5}$ is often used to represent the empirical formula,$P_{4}O_{10}$ is the correct molecular formula for the substance as it exists in nature.

(B) Phosphorus pentoxide $(P_4O_{10})$ is an oxide of a non-metal.
Non-metallic oxides are generally acidic in nature.
When phosphorus pentoxide reacts with water,it forms phosphoric acid $(H_3PO_4)$,which confirms its acidic character:
$P_4O_{10} + 6H_2O \rightarrow 4H_3PO_4$.
Therefore,the correct option is $B$.

(C) Sulphurous acid is an inorganic compound with the chemical formula $H_{2}SO_{3}$.
It is formed when sulphur dioxide $(SO_{2})$ is dissolved in water $(H_{2}O)$.
The reaction is: $SO_{2} + H_{2}O \rightarrow H_{2}SO_{3}$.
In contrast,$H_{2}SO_{4}$ is sulphuric acid,$H_{2}S_{2}O_{7}$ is oleum,and $H_{2}SO_{2}$ is sulphoxylic acid.

(D) Phosphoric acid,also known as orthophosphoric acid,is a mineral acid with the chemical formula $H_{3}PO_{4}$.
It consists of one phosphorus atom,four oxygen atoms,and three hydrogen atoms.
Therefore,the correct option is $D$.

$(A)$ The reaction between dinitrogen $(N_2)$ and dihydrogen $(H_2)$ is known as the Haber process.
In this process, one mole of nitrogen gas reacts with three moles of hydrogen gas to produce two moles of ammonia $(NH_3)$ gas.
The balanced chemical equation for this reaction is:
$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$
Therefore, the correct compound formed is ammonia.

(C) Henry Cavendish is credited with the discovery of hydrogen gas in $1766$. He identified it as a distinct substance by reacting metals with strong acids and called it 'inflammable air'.

(C) compound is a substance formed when two or more chemical elements are chemically bonded together.
Water is a chemical compound with the molecular formula $H_2O$.
It consists of two hydrogen atoms covalently bonded to one oxygen atom.
Ammonia $(NH_3)$ contains nitrogen and hydrogen.
Methane $(CH_4)$ contains carbon and hydrogen.
Hydrochloric acid $(HCl)$ contains hydrogen and chlorine.
Therefore,the correct option is $C$.

(B) When zinc $(Zn)$ reacts with diluted hydrochloric acid $(HCl)$,it undergoes a displacement reaction.
In this reaction,zinc displaces hydrogen from the acid to form zinc chloride $(ZnCl_{2})$ and releases hydrogen gas $(H_{2})$.
The chemical equation for this reaction is: $Zn(s) + 2HCl(aq) \rightarrow ZnCl_{2}(aq) + H_{2}(g)$.

(A) The weight of a gas is determined by its molar mass.
$1$. The molar mass of $H_2$ (Dihydrogen) is approximately $2.016 \ g/mol$.
$2$. The molar mass of $NH_3$ (Ammonia) is approximately $17.03 \ g/mol$.
$3$. The molar mass of $SO_2$ (Sulfur dioxide) is approximately $64.06 \ g/mol$.
$4$. The molar mass of $O_2$ (Dioxygen) is approximately $32.00 \ g/mol$.
Since $H_2$ has the lowest molar mass among the given options,it is the lightest gas.

(B) $H_2$ gas is insoluble in water and is lighter than air. Therefore,it is collected by the downward displacement of water. In this method,the gas jar is filled with water and inverted over the delivery tube in a water trough. As the $H_2$ gas enters the jar,it displaces the water downwards,filling the jar with the gas.

(D) Water gas is a mixture of carbon monoxide $(CO)$ and dihydrogen $(H_2)$.
It is produced by passing steam over red-hot coke at high temperatures.
The chemical reaction is: $C(s) + H_2O(g) \xrightarrow{1273 K} CO(g) + H_2(g)$.

(A) In the industrial production of hydrogen gas, specifically through the Bosch process (reaction of water gas with steam), $Iron$ $(Fe)$ is used as a catalyst. The reaction is: $CO(g) + H_2O(g) \xrightarrow{Fe} CO_2(g) + H_2(g)$. This is known as the water-gas shift reaction, where $Iron$ oxide (promoted with chromium oxide) acts as the catalyst to increase the yield of hydrogen.

(A) Natural gas is a fossil fuel energy source that formed deep beneath the earth's surface.
It is primarily composed of $CH_4$ (Methane), which typically accounts for $70\%$ to $90\%$ of its composition.
Other components include small amounts of ethane, propane, butane, and non-hydrocarbon gases.
Therefore, the correct option is $A$.

(C) The process of adsorption of $H_2$ gas on the surface of transition metals like $Pd$,$Pt$,or $Ni$ is known as occlusion.
$H_2$ gas can be adsorbed on these metals and can be released later when required,for example,in hydrogenation reactions.
Therefore,$H_2$ (dihydrogen) is the correct answer.