Reactions Of Metals With Water | Reactions | Chemistry | FuseSchool
TLDRThis script explores the reactivity of metals with water, highlighting the differences between alkali metals and alkaline earth metals. Group 1 metals like lithium and potassium react vigorously, displacing hydrogen to form metal hydroxides and hydrogen gas. Potassium's reaction is notably violent, igniting hydrogen gas. Group 2 metals, such as beryllium and magnesium, show varied reactivity, with calcium, strontium, and barium forming less soluble hydroxides. The script also touches on the industrial uses of metal hydroxides and the process of creating them from salts rather than direct metal-water reactions. It concludes with a note on transition metals' inertness and aluminum's unique protective oxide layer.
Takeaways
- 🔥 Alkali metals from Group 1 react vigorously with cold water, displacing hydrogen to form metal hydroxides and hydrogen gas.
- 🌀 Lithium, as an alkali metal, floats and reacts gently with water, forming Li+ and OH- ions, making the solution basic.
- 💥 Potassium, also an alkali metal, reacts more violently with water, releasing enough heat to ignite hydrogen gas and the metal itself.
- 🛑 Alkaline earth metals from Group 2 show varied reactivity with water; beryllium is inert, while magnesium reacts slightly.
- 📉 The reactivity of alkaline earth metals increases as you go down the group, with elements like strontium reacting more vigorously than calcium.
- 💧 Strontium reacts with water to form strontium hydroxide, which can be seen as a white precipitate and is only partially soluble in water.
- 🛡 The solid hydroxide formed by Group 2 metals can create a protective layer on the metal surface, slowing the reaction.
- 🏭 Metal hydroxides have industrial uses, such as lithium hydroxide in water-repellent grease and strontium hydroxide in sugar production.
- 🧪 Industrial production of metal hydroxides does not involve adding pure metal to water due to cost and efficiency; salts and strong bases are used instead.
- 🌌 Transition metals generally do not react with water due to the high energy required to release electrons and form soluble ions.
- 🛡️ Elements like tin and lead, near the metal-nonmetal border, are inert in water, with molten tin used to coat iron cans to prevent water reactions.
- 🤔 Aluminum is unique; it reacts with water to form a protective aluminum oxide layer, which then prevents further reaction.
Q & A
How do alkali metals from Group 1 react with cold water?
-Alkali metals from Group 1 react vigorously with cold water, displacing hydrogen from the water molecule to form a metal hydroxide and hydrogen gas. The metal atom floats on the surface and fizzes gently until it disappears, forming metal ions and hydroxide ions that make the solution basic.
What happens when lithium reacts with water?
-Lithium, an alkali metal, floats on the surface of water and reacts to form lithium hydroxide and hydrogen gas. It forms Li+ and OH- ions, which dissolve in the solution, making it basic and turning universal indicator paper blue to purple depending on concentration.
What is the difference in the reaction between lithium and potassium with water?
-While lithium's reaction with water is gentle, potassium's reaction is much more violent due to its higher reactivity. The reaction with potassium is exothermic enough to ignite the hydrogen gas and can even ignite the metal itself.
How do alkaline earth metals from Group 2 react with water?
-Alkaline earth metals from Group 2, such as magnesium, react with water less vigorously than Group 1 metals. Elements below calcium, like strontium and barium, form their hydroxides with water, but the reaction is less vigorous than their Group 1 counterparts.
Why does the reaction of strontium with water produce a white precipitate?
-The white precipitate observed during the reaction of strontium with water is solid strontium hydroxide. Unlike Group 1 hydroxides, those formed by Group 2 metals are only partially water-soluble and can often be seen in solid form.
What is the role of metal hydroxides in industry?
-Metal hydroxides have various industrial uses. For example, lithium hydroxide is used to make a highly water-repellent grease, and strontium hydroxide is involved in the manufacture of table sugar from the sugar beet crop.
How is strontium hydroxide typically produced in industry?
-In industry, strontium hydroxide is not made by adding pure strontium to water. Instead, it is produced by starting with the salt strontium nitrate and adding a strong base.
Do transition metals react with water in their pure form?
-Generally, transition metals in their pure form do not react with water. They usually need to give up at least two electrons to become soluble ions, and the energy required for this process is too high.
Why are elements like tin and lead inert in water?
-Elements near the border between metals and non-metals, such as tin and lead, are inert in water. For example, molten tin is sprayed onto iron cans to prevent them from reacting with any water inside the can.
How does aluminum react with water, and what forms on the metal surface?
-Pure aluminum initially reacts with water by forming aluminum oxide (Al2O3). This oxide forms a protective layer on the metal surface, which stops further reactions from occurring.
What is the significance of the protective layer formed by aluminum oxide on aluminum metal?
-The protective layer of aluminum oxide prevents further reactions from occurring on the aluminum surface. This self-protecting property is important in many applications where aluminum is used due to its resistance to corrosion.
Outlines
🔬 Reactivity of Metals with Water
This paragraph discusses the reactivity of different groups of metals with water, focusing on alkali metals from Group 1 and alkaline earth metals from Group 2. Alkali metals react vigorously with cold water, displacing hydrogen to form metal hydroxides and hydrogen gas. The example of lithium is given, where it floats and reacts gently, forming ions that make the solution basic. Potassium, another alkali metal, reacts more violently, igniting the hydrogen gas. Alkaline earth metals, starting with beryllium, show a decrease in reactivity with water as you move down the group, with elements like strontium and barium reacting less vigorously than their alkali counterparts. The reaction of strontium with water is described, where it sinks, produces hydrogen gas, and forms a white precipitate of strontium hydroxide, which is only partially soluble in water and can form a protective layer on the metal surface.
Mindmap
Keywords
💡Alkali Metals
💡Reactivity Trend
💡Metal Hydride
💡Universal Indicator Paper
💡Alkaline Earth Metals
💡Hydroxide
💡Protective Layer
💡Transition Metals
💡Inert Elements
💡Aluminium Oxide (Al2O3)
💡Strontium Nitrate
Highlights
Alkali metals from Group 1 react vigorously with cold water, displacing hydrogen to form metal hydroxide and hydrogen gas.
Lithium metal floats on water and reacts gently, forming Li+ and OH- ions, making the solution basic.
The reaction of potassium with water is more violent, igniting the hydrogen gas and metal itself due to its higher reactivity.
Group 2 alkaline earth metals show varied reactivity with water, with beryllium being inert and magnesium reacting slightly.
Elements like strontium, barium, and calcium below calcium in Group 2 react with water to form less vigorous hydroxides than Group 1.
Strontium metal sinks in water, producing hydrogen gas and a white precipitate of solid strontium hydroxide.
Group 2 metal hydroxides are partially water-soluble and can form a protective layer, slowing the reaction.
Metal hydroxides have industrial uses, such as lithium hydroxide in water-repellent grease and strontium hydroxide in sugar manufacturing.
Industrial production of metal hydroxides typically starts with metal salts and a strong base, not direct metal and water reactions.
Transition metals generally do not react with water due to the high energy required to form soluble ions.
Elements near the metal-nonmetal border, like tin and lead, are inert in water, with molten tin used to coat iron cans to prevent water reactions.
Aluminum initially reacts with water by forming a protective layer of aluminum oxide, which stops further reactions.
The protective oxide layer on aluminum prevents further reaction with water, highlighting its unique reactivity.
Universal indicator paper can be used to test the basicity of solutions formed by metal reactions with water.
The reactivity trend within a group shows an increase in reactivity as you move down the group in the periodic table.
The chemical equation for metal reactions with water remains similar across metals, but the vigor of the reaction varies.
Metal hydroxides formed by Group 2 metals can be seen in solid form during the reaction, indicating partial solubility.
Transcripts
Browse More Related Video
5.0 / 5 (0 votes)
Thanks for rating: