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Oct 17
- When water reacts with metals, a chemical reaction occurs that can result in the formation of metal oxides or hydroxides.
- The reactivity of a metal with water depends on its position in the reactivity series. Metals higher in the reactivity series, such as alkali metals and alkaline earth metals, react more readily with water.
- The reaction between water and metals can release hydrogen gas, which can be observed as bubbles forming on the surface of the metal.
- Some metals, such as iron and aluminum, can form a protective oxide layer on their surface when they react with water, which can prevent further reaction.
- The reaction between water and metals can be accelerated by the presence of acids or other reactive substances in the water.
- The reaction between water and metals can be used in various industrial processes, such as the production of hydrogen gas or the extraction of metals from ores.
- The reactivity of a metal with water depends on its position in the reactivity series. Metals higher in the reactivity series, such as alkali metals and alkaline earth metals, react more readily with water.
- The reaction between water and metals can release hydrogen gas, which can be observed as bubbles forming on the surface of the metal.
- Some metals, such as iron and aluminum, can form a protective oxide layer on their surface when they react with water, which can prevent further reaction.
- The reaction between water and metals can be accelerated by the presence of acids or other reactive substances in the water.
- The reaction between water and metals can be used in various industrial processes, such as the production of hydrogen gas or the extraction of metals from ores.
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Google Gemini AI
Oct 17
Reactivity of Metals with Water
Group 1 Metals (Alkali Metals)
- React vigorously with water at room temperature.
- Release hydrogen gas (H2) and form hydroxides (MOH).
- Example: 2Na + 2H2O → 2NaOH + H2
Group 2 Metals (Alkaline Earth Metals)
- React less vigorously than Group 1 metals.
- Release hydrogen gas and form hydroxides.
- Example: Mg + 2H2O → Mg(OH)2 + H2
Magnesium
- Reacts slowly with cold water but vigorously with hot water.
- Releases hydrogen gas and forms magnesium hydroxide.
- Example: Mg + 2H2O → Mg(OH)2 + H2
Aluminum
- Does not react with water at room temperature due to a protective oxide layer.
- Reacts with boiling water or in the presence of an acid.
- Releases hydrogen gas and forms aluminum hydroxide.
- Example: 2Al + 6H2O → 2Al(OH)3 + 3H2
Iron
- Does not react with dry water.
- Reacts slowly with moist air or water to form iron oxide (rust).
- Release of hydrogen gas is negligible.
Zinc
- Reacts slowly with water, especially in the presence of an acid.
- Releases hydrogen gas and forms zinc hydroxide.
- Example: Zn + 2H2O → Zn(OH)2 + H2
Factors Affecting Reactivity:
- Metal's reactivity: More reactive metals react more vigorously with water.
- Surface area: Increased surface area allows for more contact between the metal and water, increasing reaction rate.
- Temperature: Elevated temperature increases reaction rate.
- Presence of acids or bases: Acids and bases can accelerate or inhibit reactions, respectively.
Group 1 Metals (Alkali Metals)
- React vigorously with water at room temperature.
- Release hydrogen gas (H2) and form hydroxides (MOH).
- Example: 2Na + 2H2O → 2NaOH + H2
Group 2 Metals (Alkaline Earth Metals)
- React less vigorously than Group 1 metals.
- Release hydrogen gas and form hydroxides.
- Example: Mg + 2H2O → Mg(OH)2 + H2
Magnesium
- Reacts slowly with cold water but vigorously with hot water.
- Releases hydrogen gas and forms magnesium hydroxide.
- Example: Mg + 2H2O → Mg(OH)2 + H2
Aluminum
- Does not react with water at room temperature due to a protective oxide layer.
- Reacts with boiling water or in the presence of an acid.
- Releases hydrogen gas and forms aluminum hydroxide.
- Example: 2Al + 6H2O → 2Al(OH)3 + 3H2
Iron
- Does not react with dry water.
- Reacts slowly with moist air or water to form iron oxide (rust).
- Release of hydrogen gas is negligible.
Zinc
- Reacts slowly with water, especially in the presence of an acid.
- Releases hydrogen gas and forms zinc hydroxide.
- Example: Zn + 2H2O → Zn(OH)2 + H2
Factors Affecting Reactivity:
- Metal's reactivity: More reactive metals react more vigorously with water.
- Surface area: Increased surface area allows for more contact between the metal and water, increasing reaction rate.
- Temperature: Elevated temperature increases reaction rate.
- Presence of acids or bases: Acids and bases can accelerate or inhibit reactions, respectively.
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