Well , ionic compounds in the solid state do not conduct electricity because their ions are held in fixed positions within a rigid lattice structure. In this solid lattice, the ions are not free to move, which is necessary for the conduction of electricity. Electrical conductivity requires the movement of charged particles, such as electrons or ions; since the ions in a solid ionic compound are not mobile, they cannot carry an electric current. However, when ionic compounds are melted into a liquid state or dissolved in water, the lattice structure breaks down, allowing the ions to move freely. This mobility enables the ions to conduct electricity in the liquid or aqueous state.
@@gameswithalex7447 thanks dear, but i wanted to cover everything with a thought that my viewer who is a student should not suffer due to any topic and hence...
Sir , if hydrogen is a non metal and it loses to form positive ions but we also know that its atomic number is 1 if it loses one electron to gain positive ions on it to gain positive charge on itself then there is no left electron in it then how will the atom of this element even exist
When hydrogen loses its single electron, it becomes a hydrogen ion ((H^+)), which is essentially just a proton. In this state, the hydrogen ion is still a valid entity but it doesn't exist as a neutral atom; instead, it often exists in association with other particles or in solutions where it can interact with other ions or molecules. For example, in aqueous solutions, (H^+) ions commonly associate with water molecules to form hydronium ions ((H_3O^+)). While a bare proton may not appear as a standalone "atom" in the traditional sense due to the lack of electrons, it plays a vital role in many chemical reactions and is a fundamental component of acids.
Yes, there are specific reasons why magnesium does not react with oxygen at room temperature: 1. Thermodynamic Stability: At room temperature, magnesium is relatively stable, which means it does not readily react with oxygen. The reaction between magnesium and oxygen requires a certain amount of energy (activation energy) to initiate. 2. Oxide Layer Formation: When magnesium is exposed to oxygen, it can form a thin layer of magnesium oxide (MgO) on its surface. This oxide layer acts as a protective barrier, preventing further reaction between the magnesium metal and oxygen. This is known as passivation. 3. High Activation Energy: The reaction between magnesium and oxygen requires a significant amount of energy to break the bonds in the magnesium metal and oxygen molecules. At room temperature, this energy is not readily available, so the reaction does not occur spontaneously. 4. Temperature Dependence: Magnesium does react with oxygen when heated. At elevated temperatures, the energy provided allows magnesium to react with oxygen more readily, producing magnesium oxide
@@seemamalhotra8836 free electrons not participating in the bond formatio like oxygen has two loan pairs in water molecule ( H2O). There are two hydrogen atoms and one oxygen atom in one water molecule.Here Oxygen has six valence electrons, it shares one electron with each hydrogen atom amd forms two single covalent bonds. The remaining four electrons of oxygen do not participate in any bond formation and hence oxygen has two loan pairs. Hope this helps!
@@seemamalhotra8836 we need to be careful while saying this as i explained, these are the left over free electrons that do not participate in the bonding
Sir , when nitrogen is present in air it reduces the rate of combustion, sir what is the that exact property of nitrogen that allows it to do so and why being the most abundant gas in the atmosphere it does not participate in combustion rather oxygen being less abundant in atmosphere less than nitrogen and participates in the triangle of fire in the combustion but why not nitrogen
Nitrogen's ability to reduce the rate of combustion is primarily due to its chemical stability and inertness at normal temperatures. Here are a few reasons why nitrogen behaves in this way: Triple Bond Stability: Nitrogen molecules ((N_2)) have a very strong triple bond between the two nitrogen atoms. This makes the molecule highly stable and resistant to breaking apart to form new compounds. As a result, nitrogen does not readily react with other substances at ordinary temperatures, including substances involved in combustion. Endothermic Reaction Requirement: Any reaction involving the breaking of nitrogen's triple bonds requires a significant amount of energy (endothermic process), which slows down the combustion process since it consumes energy rather than releasing it. Role as a Diluent: When nitrogen is present, it acts as a diluent for oxygen, effectively lowering the concentration of oxygen available for combustion. This helps to moderate the rate of combustion because the oxygen concentration is a critical factor in how quickly a fire can sustain itself. Oxygen, on the other hand, is much more reactive than nitrogen. Its role in combustion is due to its ability to accept electrons from other substances (acting as an oxidizer) and facilitate exothermic reactions, which release energy in the form of heat and light, thereby sustaining the combustion process. Despite its lower abundance compared to nitrogen, oxygen's reactivity makes it a key component of the fire triangle, along with heat and fuel.
Nitrogen is the most abundant gas in Earth's atmosphere primarily due to several factors related to its chemical properties and the history of Earth's formation and development: Chemical Stability: Nitrogen N2 (triple bond) is a very stable molecule due to its strong triple bond. This stability means that it does not easily react with other elements or compounds, allowing it to persist in the atmosphere over geological time scales without being easily removed or transformed into other compounds. Geological and Biological Processes: The nitrogen in our atmosphere is a result of volcanic emissions and the breakdown of ammonia (NH3) from primordial Earth's atmosphere. Over time, nitrogen was released and accumulated. It is not easily taken up in large quantities by surface processes when compared to other gases. Inertness: Nitrogen's inertness reduces its reactivity compared to oxygen or other gases. While oxygen readily participates in combustion and various chemical reactions, nitrogen remains mostly unreactive under ambient conditions, allowing it to accumulate to high levels. Life and Biological Nitrogen Cycle: While biological processes, such as those in the nitrogen cycle, continuously circulate nitrogen through various forms (organic and inorganic), these processes generally return nitrogen to the atmosphere in its gaseous form, thanks to the action of denitrifying bacteria. These factors, combined over billions of years, have resulted in nitrogen becoming the dominant component of Earth's atmosphere, comprising about 78% of the air by volume.
Non-metals can't push hydrogen out of acids because they don't give up electrons easily. To displace hydrogen, a substance usually needs to provide electrons so that the hydrogen ions in the acid can gain these electrons and can turn into hydrogen gas. Metals do this well because they easily lose electrons. Non-metals, on the other hand, prefer to gain or share electrons, so they don't help hydrogen ions change into hydrogen gas.
Aqueous solutions of ionic compounds can conduct electricity because the ionic compounds dissociate into their constituent ions when dissolved in water. This process allows the solution to carry electric current. Here's how it works: Dissociation in Water: When an ionic compound, like sodium chloride ((NaCl)), is dissolved in water, it separates into its positive ions ((Na+)) and negative ions ((Cl-)). Movement of Ions: These free-moving ions are able to carry charge through the solution. The positive ions move towards the negative electrode (cathode), and the negative ions move towards the positive electrode (anode) when an electric field is applied. Conductivity: The movement of these charged particles within the solution constitutes an electric current, allowing the solution to conduct electricity. In summary, it is the presence of free ions in aqueous solutions that enables the conduction of electrical current. Pure water, on the other hand, contains very few ions and is a poor conductor of electricity.
The reactivity of metals depends on a few key things, mainly how they are built at the atomic level and how easily they can give up electrons to become positive ions. Here’s why some metals are more reactive than others: Electron Setup: Metals that need to lose fewer electrons to become stable are more reactive. For example, metals like lithium and sodium, which belong to the alkali group, have only one electron to lose and do this easily. Energy to Remove Electrons: Metals that need less energy to lose an electron are more reactive. Alkali metals require less energy to do this compared to other metals, making them more reactive. Size of Atoms: Bigger metal atoms have outer electrons that are further from the nucleus, making them easier to remove. Because of this, bigger atoms like cesium or potassium react more readily. Strength of Metallic Bonds: Metals with weaker connections between their atoms tend to be more reactive. Alkali metals have weaker bonds compared to others, which makes them react more. Spot on the Periodic Table: Metals on the left and towards the bottom part of the periodic table are more reactive. They have bigger atoms and need less energy to lose electrons. Reactivity Order: Metals are ranked in a series that shows how likely they are to react, like forming compounds or displacing hydrogen in reactions. This helps predict and compare how different metals behave. In short, a metal's reactivity is about how easily it can give away electrons, how stable it is afterward, and the energy changes during this process. All these factors together explain how a metal reacts with other substances like water or acids.
Nice sir
@@ShreeyanshSharma1221 thank you dear, watch full video it will help you
Yes sir
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@@RekhaChaudhary-r1t thank you for your support
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@@aayushikoshal2542 👍
Best Explanation ❤
thank you dear
Thank you sir
@@sujalanejaxa8722 thank you dear
Amazingly explained sir
But plz do share the notes in the description
It would be easy for us to revise again ...
@@anandgiri5257 let me check the possibilities
Why ionic compounds in the solid state do not conduct electricity
Well , ionic compounds in the solid state do not conduct electricity because their ions are held in fixed positions within a rigid lattice structure. In this solid lattice, the ions are not free to move, which is necessary for the conduction of electricity. Electrical conductivity requires the movement of charged particles, such as electrons or ions; since the ions in a solid ionic compound are not mobile, they cannot carry an electric current.
However, when ionic compounds are melted into a liquid state or dissolved in water, the lattice structure breaks down, allowing the ions to move freely. This mobility enables the ions to conduct electricity in the liquid or aqueous state.
Is there any particular reason why aluminium does not react with oxygen at room temperature?
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@@riyakoshal4172 thank you
Maza agya sir ❤❤
Magar video bohot lambi hai😂😂
@@gameswithalex7447 thanks dear, but i wanted to cover everything with a thought that my viewer who is a student should not suffer due to any topic and hence...
Sir , if hydrogen is a non metal and it loses to form positive ions but we also know that its atomic number is 1 if it loses one electron to gain positive ions on it to gain positive charge on itself then there is no left electron in it then how will the atom of this element even exist
When hydrogen loses its single electron, it becomes a hydrogen ion ((H^+)), which is essentially just a proton. In this state, the hydrogen ion is still a valid entity but it doesn't exist as a neutral atom; instead, it often exists in association with other particles or in solutions where it can interact with other ions or molecules. For example, in aqueous solutions, (H^+) ions commonly associate with water molecules to form hydronium ions ((H_3O^+)). While a bare proton may not appear as a standalone "atom" in the traditional sense due to the lack of electrons, it plays a vital role in many chemical reactions and is a fundamental component of acids.
@@Vijyanguru ok sir
Thanks a lot
Very nice sir
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@@DurvaanshSingh thanks
Is there any particular reason why magnesium does not react with oxygen at room temperature?
Yes, there are specific reasons why magnesium does not react with oxygen at room temperature:
1. Thermodynamic Stability:
At room temperature, magnesium is relatively stable, which means it does not readily react with oxygen. The reaction between magnesium and oxygen requires a certain amount of energy (activation energy) to initiate.
2. Oxide Layer Formation:
When magnesium is exposed to oxygen, it can form a thin layer of magnesium oxide (MgO) on its surface. This oxide layer acts as a protective barrier, preventing further reaction between the magnesium metal and oxygen. This is known as passivation.
3. High Activation Energy:
The reaction between magnesium and oxygen requires a significant amount of energy to break the bonds in the magnesium metal and oxygen molecules. At room temperature, this energy is not readily available, so the reaction does not occur spontaneously.
4. Temperature Dependence:
Magnesium does react with oxygen when heated. At elevated temperatures, the energy provided allows magnesium to react with oxygen more readily, producing magnesium oxide
@@Vijyanguru thanks a lot sir
Sir kisi compound ke loan pairs uske free electrones hote h??
@@seemamalhotra8836 free electrons not participating in the bond formatio like oxygen has two loan pairs in water molecule ( H2O). There are two hydrogen atoms and one oxygen atom in one water molecule.Here Oxygen has six valence electrons, it shares one electron with each hydrogen atom amd forms two single covalent bonds. The remaining four electrons of oxygen do not participate in any bond formation and hence oxygen has two loan pairs.
Hope this helps!
Sir that means loan pairs and free electrons is same thing
@@seemamalhotra8836 we need to be careful while saying this as i explained, these are the left over free electrons that do not participate in the bonding
Ok sir
amazing explanation sir , but pls do another Favour of sharing the notes in description............
@@divyanshSiwach great idea let me check in future
Sir , when nitrogen is present in air it reduces the rate of combustion, sir what is the that exact property of nitrogen that allows it to do so and why being the most abundant gas in the atmosphere it does not participate in combustion rather oxygen being less abundant in atmosphere less than nitrogen and participates in the triangle of fire in the combustion but why not nitrogen
Nitrogen's ability to reduce the rate of combustion is primarily due to its chemical stability and inertness at normal temperatures. Here are a few reasons why nitrogen behaves in this way:
Triple Bond Stability: Nitrogen molecules ((N_2)) have a very strong triple bond between the two nitrogen atoms. This makes the molecule highly stable and resistant to breaking apart to form new compounds. As a result, nitrogen does not readily react with other substances at ordinary temperatures, including substances involved in combustion.
Endothermic Reaction Requirement: Any reaction involving the breaking of nitrogen's triple bonds requires a significant amount of energy (endothermic process), which slows down the combustion process since it consumes energy rather than releasing it.
Role as a Diluent: When nitrogen is present, it acts as a diluent for oxygen, effectively lowering the concentration of oxygen available for combustion. This helps to moderate the rate of combustion because the oxygen concentration is a critical factor in how quickly a fire can sustain itself.
Oxygen, on the other hand, is much more reactive than nitrogen. Its role in combustion is due to its ability to accept electrons from other substances (acting as an oxidizer) and facilitate exothermic reactions, which release energy in the form of heat and light, thereby sustaining the combustion process. Despite its lower abundance compared to nitrogen, oxygen's reactivity makes it a key component of the fire triangle, along with heat and fuel.
@@Vijyanguru alright sir thanks a lot
Sir why nitrogen is most abundant gas in the earth atmosphere?
Nitrogen is the most abundant gas in Earth's atmosphere primarily due to several factors related to its chemical properties and the history of Earth's formation and development:
Chemical Stability: Nitrogen N2 (triple bond) is a very stable molecule due to its strong triple bond. This stability means that it does not easily react with other elements or compounds, allowing it to persist in the atmosphere over geological time scales without being easily removed or transformed into other compounds.
Geological and Biological Processes: The nitrogen in our atmosphere is a result of volcanic emissions and the breakdown of ammonia (NH3) from primordial Earth's atmosphere. Over time, nitrogen was released and accumulated. It is not easily taken up in large quantities by surface processes when compared to other gases.
Inertness: Nitrogen's inertness reduces its reactivity compared to oxygen or other gases. While oxygen readily participates in combustion and various chemical reactions, nitrogen remains mostly unreactive under ambient conditions, allowing it to accumulate to high levels.
Life and Biological Nitrogen Cycle: While biological processes, such as those in the nitrogen cycle, continuously circulate nitrogen through various forms (organic and inorganic), these processes generally return nitrogen to the atmosphere in its gaseous form, thanks to the action of denitrifying bacteria.
These factors, combined over billions of years, have resulted in nitrogen becoming the dominant component of Earth's atmosphere, comprising about 78% of the air by volume.
Sir, why non metal are not able to displace hydrogen from acid
Non-metals can't push hydrogen out of acids because they don't give up electrons easily. To displace hydrogen, a substance usually needs to provide electrons so that the hydrogen ions in the acid can gain these electrons and can turn into hydrogen gas. Metals do this well because they easily lose electrons. Non-metals, on the other hand, prefer to gain or share electrons, so they don't help hydrogen ions change into hydrogen gas.
and hydrogen is displaced from a compound in the form of hydrogen gas
Sir,why are aqueous solution of ionic compounds able to conduct electricity?
Aqueous solutions of ionic compounds can conduct electricity because the ionic compounds dissociate into their constituent ions when dissolved in water. This process allows the solution to carry electric current. Here's how it works:
Dissociation in Water:
When an ionic compound, like sodium chloride ((NaCl)), is dissolved in water, it separates into its positive ions ((Na+)) and negative ions ((Cl-)).
Movement of Ions:
These free-moving ions are able to carry charge through the solution. The positive ions move towards the negative electrode (cathode), and the negative ions move towards the positive electrode (anode) when an electric field is applied.
Conductivity:
The movement of these charged particles within the solution constitutes an electric current, allowing the solution to conduct electricity.
In summary, it is the presence of free ions in aqueous solutions that enables the conduction of electrical current. Pure water, on the other hand, contains very few ions and is a poor conductor of electricity.
Sir, why some metal are more reactive and others are less reactive
The reactivity of metals depends on a few key things, mainly how they are built at the atomic level and how easily they can give up electrons to become positive ions. Here’s why some metals are more reactive than others:
Electron Setup:
Metals that need to lose fewer electrons to become stable are more reactive. For example, metals like lithium and sodium, which belong to the alkali group, have only one electron to lose and do this easily.
Energy to Remove Electrons:
Metals that need less energy to lose an electron are more reactive. Alkali metals require less energy to do this compared to other metals, making them more reactive.
Size of Atoms:
Bigger metal atoms have outer electrons that are further from the nucleus, making them easier to remove. Because of this, bigger atoms like cesium or potassium react more readily.
Strength of Metallic Bonds:
Metals with weaker connections between their atoms tend to be more reactive. Alkali metals have weaker bonds compared to others, which makes them react more.
Spot on the Periodic Table:
Metals on the left and towards the bottom part of the periodic table are more reactive. They have bigger atoms and need less energy to lose electrons.
Reactivity Order:
Metals are ranked in a series that shows how likely they are to react, like forming compounds or displacing hydrogen in reactions. This helps predict and compare how different metals behave.
In short, a metal's reactivity is about how easily it can give away electrons, how stable it is afterward, and the energy changes during this process. All these factors together explain how a metal reacts with other substances like water or acids.
Nice sir
@@GrowwithGaurav-369 thank you dear