How are meteors formed? what are meteors.
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Metals of high reactivity, such as sodium, calcium, magnesium, aluminium, etc. are extracted from their ores by electrolytic reduction. These metals cannot be reduced using carbon because carbon is less reactive than them. Electrolytic Reduction: Electric current is passed through the molten state of metal ores.
The reactivity series of metals is important when it comes to extracting a metal from its ore. The higher a metal is in the reactivity series the harder it is to extract from its ore. Carbon is not a metal but included within the reactivity series as it affects how the metals can be extracted.
This is called a blast furnace. Very reactive metals are strongly bonded in their ores and cannot be extracted using carbon/carbon monoxide. More energy is needed and this is provided by electrolysis.
Element | Reaction with water |
---|---|
Lithium | Quickly |
Calcium | More slowly |
The less reactive metals are extracted by the reduction of their oxides by heat alone. Example: Mercury (II) sulphide ore is roasted in air when mercury (II) oxide is formed. When this mercury (II) oxide is heated to about 300oC, it decomposes to form mercury metal.
Metals more reactive than carbon, such as aluminium, are extracted by electrolysis, while metals less reactive than carbon, such as iron, may be extracted by reduction with carbon. … However, chemical reactions may be needed to remove other elements that might contaminate the metal.
This metals are highly electropositive in nature so they form strong ionic bonds which corresponding non-metallic elements so that it becomes difficult to minimize the electrostatic force of attraction and hence it becomes harder to extract them from their ores.
Moderately reactive metals are extracted from their metal oxides by the process of reduction. As it’s easier to reduce metal oxides to metal, a metal carbonate is first converted to its oxide by the process of calcination and a metal sulphide is first converted to its oxide by the process of roasting.
If a metal is less reactive than carbon, it can be extracted from its oxide by heating with carbon. The carbon displaces the metal from the compound, and removes the oxygen from the oxide. This leaves the metal.
We can see that among the given elements, zinc (Zn), tin (Sn), and lead (Pb) are less reactive than carbon (C) whereas aluminum (Al) is more reactive than carbon. Therefore option (B) Al metal cannot be extracted by the carbon reduction process.
A compound will always displace a less reactive metal from solutions of its compounds. Another example of ‘competition’ between metals to form compounds is observed in the reaction between metals and metal oxides.
Metal ions are positively charged as they lose negative electrons. Some metals give up their electrons more readily than others and are, therefore, more reactive. Metals can be ranked according to their level of reactivity to form the metal reactivity series.
Silver, gold, and platinum are metals with the least reactivity.
– So, out of given metals, Potassium is the most reactive metal. Therefore, potassium is the most reactive metal among the given options.
The metal which has low reactivity can be extracted by heating the ore alone. … Metals are extracted from these ores by heating them alone. For example, ores of copper can be extracted by reduction with carbon (copper (I) oxide) as well as heating alone (copper (I) sulphide).
In metallurgy, refining consists of purifying an impure metal. It is to be distinguished from other processes such as smelting and calcining in that those two involve a chemical change to the raw material, whereas in refining, the final material is usually identical chemically to the original one, only it is purer.
Extraction of Copper: Copper glance (Cu2S) is roasted in the presence of air. This results in oxidation of copper sulphide to give copper oxide. Roasting turns copper glance (ore of copper) into copper (I) oxide. After that, copper oxide is then heated in the absence of air, so that it can undergo calcination.
The extraction of metals from ores is what allows us to use the minerals in the ground! The ores are very different from the finished metals that we see in buildings and bridges. Ores consist of the desired metal compound and the impurities and earthly substances called Gangue.
Extraction using carbon Metals such as zinc, iron and copper are present in ores as their oxides. Each of these oxides is heated with carbon to obtain the metal. The metal oxide loses oxygen, and is therefore reduced.
Metals can be extracted from ores by reduction – the removal of oxygen or forming a metal element from a compound. Oxidation and reduction have multiple meanings, not just to do with the addition and removal of oxygen. Encourage students to use key terms as often as possible.
Tungsten vs Titanium In terms of tensile strength, tungsten is the strongest out of any natural metal (142,000 psi). But in terms of impact strength, tungsten is weak — it’s a brittle metal that’s known to shatter on impact. Titanium, on the other hand, has a tensile strength of 63,000 psi.
About Extracting Metals by Electrolysis Carbon electrodes are used to pass an Electrical Current through the molten mineral. The metal collects at the cathode which carries a negative charge and the pure metal is removed from the electrolysis cell.
More reactive metals in solution have lower standard reduction potentials (thus are more easily oxidised, and have a greater tendency to lose electrons as oxidation is more feasible) and higher electronegativities (a greater ability to attract a bonding pair of electrons).
The moderately reactive metals are extracted by the reduction of their oxides with carbon, aluminium, sodium or calcium. Example: When zinc sulphide (zinc blende ore) is strongly heated in air (roasted), it forms zinc oxide and sulphur dioxide. This process is called roasting. … This process is termed as reduction.
Extraction of metals which are in the middle of activity series. … A metal is obtained from its ore by the processes of reduction or by electrolysis. In the reduction process, it is the oxide ore that is reduced. It is easier to reduce an oxide ore as compared to its sulphides and carbonates.
As we can see in the series, out of all the given options gold is the least reactive metal.
Metal oxides are converted to usable metals when they react with carbon. The extraction of metals in a blast furnace with coke (carbon from heated charcoal) is called smelting. When electricity is used to recover a metal from a metal oxide it is called electrolysis.
The lead oxide is then heated with coke (carbon) in a blast furnace to cause a displacement reaction which produces lead and carbon dioxide. This works because carbon is more reactive than lead, so carbon can reduce the lead oxide to lead.
Metals are extracted using electrolysis or a displacement reaction.
MetalMethodIronReduction by carbon or carbon monoxideTinReduction by carbon or carbon monoxideLeadReduction by carbon or carbon monoxide(Hydrogen)(Non-metal)
A more reactive metal will displace (replace) a less reactive metal in an activity series. So, yes, a metal can displace (replace) any metal that is below it in an activity series.
In the electrochemical series, the metals which are at a higher position are more reactive and hence they displace less reactive metals( metals present near the bottom of the series) from their salts. Metals present higher in the series readily reacts with oxygen, water and acids and form highly stable compounds.
The displacement of more reactive metal from a less reactive metal is known as the displacement reaction. A chemical reaction wherein the more reactive metal displaces the lest reactive metal from its compound is known as the displacement reaction.
It is because they have different number of valence electrons due to their atomic numbers.
Some elements Have more electronagativity Than hydrogen. So they More reactive than hydrogen in other elements.
Four major factors affect reactivity of metals: nuclear charge, atomic radius, shielding effect and sublevel arrangement (of electrons). Metal reactivity relates to ability to lose electrons (oxidize), form basic hydroxides, form ionic compounds with non-metals.
Cesium is second from the bottom of this group, has 6 shells of electrons, and it matches the features of a reactive atom, making it the most reactive element.
Detailed Solution. The correct answer is Calcium. Calcium (Ca) is the most reactive metal amongst these. An element’s reactivity decreases while going down the reactivity series.
Platinum is the least reactive of all the options. Aluminium, iron are also formed in combined forms in the natural surroundings.