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Zn(s)

Cu(s)

HCl(aq)

Reactions of Copper

HNO3

H2 SO4 (aq)

Group members: Sanjana Punjabi, Juaquin Coc, Janivi Quiroz, Julian Cute Jr. , Jaydan Moguel

NaOH(aq)

Heat

The Formation of Copper (II) Nitrate

Cu(NO3)2 (aq)

Mechanisms

Formation of Copper (II) Nitrate

Balanced Equation:

  • 3Cu(s) + 8HNO 3(aq) 3Cu(NO3)2(aq) + 2NO2(g) + 4H2O(l)

Type of Reaction:

  • Oxidation-Reduction (Redox)reaction/ Acid-base reaction

  • Cu oxidizing agent
  • HNO3 Reducing agent

Oxidation:

  • 3Cu0 Cu2+ + 6e-

Reduction:

  • HNO3 NO+ H2O

  • 6e- +4H++ 2NO3- 2NO +4H2O

[Cu(OH2)6]2+- complex compound

Formation of Copper (II) Hydroxide

Cu(OH) (s)

Mechanisms

Formation of Copper (II) Hydroxide

Balanced Equation:

· Cu(NO3)2(aq) + 2Na(OH)2(aq) Cu(OH)2(s) + 2NaNO3(aq)

Type of Reaction:

Double displacement reaction

Precipitation Reaction

Cu(OH)2 Is formed, a blue insoluble solid that precipitates out of solution

Complete ionic equation

· Cu2+(aq) + 2NaO3-(aq)+2Na+(aq)+2OH-(aq)

Cu(OH)2(s) +2Na+(aq) + 2NO3-(aq)

to get the net ionic equation, you must eliminate spectator ions, i.e. ions that are present on both sides of the equation

· Cu2+(aq) + 2OH3-(aq) Cu(OH)2(s)

[Cu(OH2)6]2+

complex compound

The Formation of Copper (II) Oxide

CuO (s)

Mechanisms

Formation of Copper (II) Oxide

Balanced Equation:

Cu(OH)2(s) CuO(s) + H2O(l)

Decomposition Reaction

· CuO(s) + H2SO4(aq) CuSO4(aq) + H2O(l)

Double displacement reaction

Acid-base reaction 2H+ acid)+ O-(a base) H2O

Precipitation reaction

Oxide ion is replaced with sulfate ion

And a light blue solution forms.

The Formation of Copper (II) Sulphate

CuSO (aq)

Formation of Copper (II) Sulphate

Mechanisms

Balanced Equation:

CuSO4(aq) + Zn(s) Cu(s) + ZnSO4(aq)

Single displacement (synthesis) reaction

Oxidation-Reduction (redox) reaction

Oxidation:

· Zn(s) Zn2+ +2e-

Reduction:

· Cu2+(aq) + 2e- Cu(s)

Copper Metal

What is the Copper Cycle?

Introduction

  • Some of the most commonly found forms of copper are the sulphides of copper such as covellite (CuS, which is also called cupric sulphide or copper(II) sulphide), chalcocite (Cu2S, which is also called cuprous sulphide or copper (I) sulphide), and chalcopyrite (CuFeS2)

  • Copper is a reddish-gold colored metal that is ductile, malleable, and an effective conductor of heat and electricity.Copper was widely used to make cookware like pans and kettles, but are less common now as there are cheaper cookware made of aluminum or stainless steel. High-quality pots and pans are made with copper bottoms, which distributes the heat from the stovetop quickly and evenly throughout the pan. Copper can resists corrosion by water, air, and most acids (except for concentrated nitric and sulfuric acids), for this reason it is ideal in making coin.

  • Copper does not oxidize(lose electrons) readily in air and has a very low reactivity with dilute mineral acids such as sulfuric acid (H2SO4) and hydrochloric acid (HCl). However nitric acid (HNO3) has a high reactivity with copper and will readily dissolve copper metal producing the copper(II) ion of copper metal in nitric acid is an oxidative process where electrons are transferred from copper metal to the nitrogen of the acid.
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