Question

Write the following chemical properties of of metals on :

(i) Action of acids
(ii) Action of bases
(iii)Displacement reactions​

Answer 1

Answer:

1. When a metal reacts with an acid, it generally displaces hydrogen from the acids. This leads to the evolution of hydrogen gas. The metals combine with remaining part of acids to form a salt. For example reaction of sulphuric acid with zinc.

H2SO4 + Zn → ZnSO4 + H2

2.Alkalis (bases that are soluble in water) react with the metal to produce salt and hydrogen gas. For example reaction of zinc with sodium hydroxide.

2 NaOH + Zn → Na2ZnO2 + H2

3.Displacement reactions involve a metal and a compound of a different metal. In a displacement reaction:

a more reactive metal will displace a less reactive metal from its compounds

Displacement reactions are easily seen when a salt of the less reactive metal is in the solution. During the reaction:

the more reactive metal gradually disappears as it forms a solution

the less reactive metal coats the surface of the more reactive metal

For example, magnesium is more reactive than copper. When a piece of magnesium is dipped into blue copper sulfate solution:

the blue colour fades as colourless magnesium sulfate solution forms

brown copper coats the surface of the magnesium

Magnesium powder is added to blue copper sulfate solution and when stirred, they change into a colourless magnesium sulfate solution and copper powder.

Here are the equations for the reaction:

magnesium + copper sulfate → magnesium sulfate + copper

Mg + CuSO4 → MgSO4 + Cu

No reaction is seen if you do things the other way round – in other words, if you put copper powder into magnesium sulfate solution. This is because copper is not reactive enough to displace magnesium from magnesium sulfate.

Explanation:

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Answer 2

${ \large{ \underline{ \pmb{ \frak{Required \: Answers : }}}}}$

$\: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \star{ \underline{ \underline{ \textsf{ \textbf{Basic terms : }}}}}$

Metals are the substances or elements which lose electrons and obtain positively charged ions. is called a metal

Example

$\leadsto \sf Na \rightarrow1 {e}^{ - } \rightarrow {Na}^{ + } \\ \\ \leadsto \sf Al \rightarrow3 {e}^{ - } \rightarrow {Al}^{ +3 } \\ \\ \leadsto \sf K \rightarrow1 {e}^{ - } \rightarrow {K}^{ + } \: \: \\ \\ \leadsto \sf Ca \rightarrow2 {e}^{ - } \rightarrow {Ca}^{ + 2} \\ \\ \leadsto \sf Mg \rightarrow2 {e}^{ - } \rightarrow {Mg}^{ +2 }$

${ \red{ \boxed{ \bf{Solution \: (i)}}}}$

• When an Metal reacts with an Acid!

★ When a metal reacts with an acid,effervescence or bubbles of hydrogen gas are formed with the evolution of heat energy and in further salts are fromed ( main compounds)

$\circ \rm \: Metal + Acid \: \: \longrightarrow \: Salt + Hydrogen \: gas + Heat \: enegry$

★ Now the reaction of metals like Magnesium, Aluminum, Zinc and Iron are as follows!

• With Magnesium

$\circ \: \: \sf \: Mg + 2HCl \longrightarrow \: \: MgCl_{2} + H_{2}$

• With Aluminum

$\circ \sf \: 2Al + 6HCl\longrightarrow \: 2AlCl_{3} + 3H_{2}$

• With Zinc

$\circ \sf \: Zn + H2SO_{4}\longrightarrow \: ZnSO_{4} +H_{2}$

• With Iron

$\circ \sf \: Fe + 2HCl\longrightarrow \: FeCl_{2} + H_{2}$

Remember:

• Metals like copper, silver, gold don't release hydrogen from dilute acids

${ \red{ \boxed{ \bf{Solution \: (ii)}}}}$

• When an Bases reacts with metal

Most metals don't react with bases,

★Metals like Aluminum , Lead and Zinc with strong bases and form compounds with the evolution of hydrogen gas

• Reaction with Aluminum

$\circ \sf \: 2Al + 2NaOH + 2H_{2}O\longrightarrow \: 2NaAlO_{4} + 3H_{2}$

★ Metals don't react with weak bases

${ \red{ \boxed{ \bf{Solution \: (iii)}}}}$

• Displacement reactions

★A more reactive metal can displace a less reactive metal from its salt solution. This reaction is also termed as displacement reaction.

★ Here are some of them!

$\circ \sf \: Fe + CuSO_{4}\longrightarrow \: FeSO_{4} +Cu \: \: \: \\ \\ \\ \circ \sf \:Mg + CuSO_{4}\longrightarrow \: MgSO_{4} +Cu \\ \\ \\ \circ \sf \: Zn+ CuSO_{4}\longrightarrow \: ZnSO_{4} +Cu$

${ \large{ \underline{ \pmb{ \frak{Additional \: Info : }}}}}$

$\: \: \: \: \: \: \: \: \:\: \: \: \: \: \: \star{ \underline{ \underline{ \textsf{ \textbf{Metal\: Reactivity\: Series: }}}}}$

Table :

$\begin{gathered}\begin{gathered} \tiny\boxed{\begin{array}{ c |c} \frak{ \pmb{symbol}}& \rm{ \pmb{metal}}\\ \dfrac{\qquad\qquad}{ \sf K}&\dfrac{\qquad\qquad}{ \sf 80 \: cm}& \\ \dfrac{\qquad\qquad}{ \sf Na}& \dfrac{\qquad\qquad}{ \sf sodium}& \\ \dfrac{\qquad\qquad}{ \sf Ca}&\dfrac{\qquad\qquad}{ \sf calcium }& \\ \dfrac{\qquad\qquad}{ \sf Mg}&\dfrac{\qquad\qquad}{ \sf magnesium }& \\ \dfrac{\qquad\qquad}{ \sf \: Al }&\dfrac{\qquad\qquad}{ \sf aluminium }& \\ \dfrac{\qquad\qquad}{ \sf Zn}&\dfrac{\qquad\qquad}{ \sf zinc }& \\ \dfrac{\qquad\qquad}{ \sf Fe}&\dfrac{\qquad\qquad}{ \sf iron }& \\ \dfrac{\qquad\qquad}{ \sf Pb}&\dfrac{\qquad\qquad}{ \sf lead }& \\ \dfrac{\qquad\qquad}{ \sf H}&\dfrac{\qquad\qquad}{ \sf hydrogen}& \\ \dfrac{\qquad\qquad}{ \sf Cu}&\dfrac{\qquad\qquad}{ \sf copper }& \\ \dfrac{\qquad\qquad}{ \sf Ag}&\dfrac{\qquad\qquad}{ \sf silver}& \\ \dfrac{\qquad\qquad}{ \sf Au}&\dfrac{\qquad\qquad}{ \sf gold}& \\ \dfrac{\qquad\qquad}{ \sf Pt}&\dfrac{\qquad\qquad}{ \sf platinum }&\end{array}}\end{gathered}& \\ \end{gathered}$