When a white coloured compound of a precious metal is exposed to sunlight, a change in colour is observed .
a. What is the change you observe?
b. Identify the metal
c. Also mention the type of chemical reaction
d. Give one application of this reaction
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The lure of gold has been the downfall of many, from those worshipping the biblical golden calf to those unsuccessfully staking their claims during the 19th century gold rushes. Nevertheless, this lustrous metal continues to connote the pinnacle of achievement, as evidenced by Nobel Prize medals, Olympic medals, and Academy Award statuettes. Would our fascination with gold be lessened if we knew that its shiny allure was the result of excited electrons?
Silver, iron, platinum, gold, and copper are all metals, which generally are malleable and ductile, conduct electricity and heat, and have a metallic luster. Some of their properties can be attributed to the way electrons are arranged in the material.
This piece of jewelry is framed in yellow gold, with purple gold detail on the right border.
This illustrated manuscript from the Book of Hours is decorated with gold leaf, beaten to an extremely thin foil.
In this hypothesis, each metal atom contributes its outer electrons to a shared pool. The electrons are free to move throughout the metal, which explains its high electrical and thermal conductivities and luster.
The bonding of metals
When two atoms combine, different types of bonding can occur: covalent, ionic, and metallic. Silver, iron, platinum, gold, and copper all form metallic bonds. Unlike covalent bonding, metallic bonding is non-directional. The strong bond consists of positively charged metal atoms in fixed positions, surrounded by delocalized electrons. These delocalized electrons are often referred to as "a sea of electrons," and can help explain why copper and gold are yellow and orange, while most other metals are silver.
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