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Chapter 9: Problem 30

Explain how an activity series of metals is organized.

Short Answer

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An activity series of metals is a list of metals arranged in descending order of their reactivity, which is mainly determined by their ease of losing electrons to form positive ions. Metals with lower ionization energies are more reactive. The series is influenced by factors like ionization energy, atomic size, and shielding effect. General trends within the series include higher reactivity for Group 1 and Group 2 metals (alkali and alkaline earth metals) and lower reactivity for transition metals and noble metals. This organization helps predict metal reactivity and is crucial for applications like corrosion prevention, electrochemistry, and metallurgy.

Step by step solution

01

1. Define Activity Series of Metals

An activity series of metals is a list of metals arranged in descending order of their reactivity. This reactivity is mainly determined by the metals鈥� ease of losing electrons to form positive ions. The more reactive a metal is, the greater its ability to lose electrons, and the higher it will be placed in the activity series.
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2. Factors Influencing Metal Reactivity

Reactivity of a metal depends on several factors, such as the ionization energy (the energy required to remove an electron from an atom), the atomic size, and the shielding effect (the ability of inner electron shells to shield the positive charge of the nucleus from the outermost electrons). In general, metals with lower ionization energies are more reactive because they can lose their electrons more easily.
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3. Example of an Activity Series

Below is a common example of an activity series of metals, ordered from most reactive to least reactive: 1. Potassium (K) 2. Sodium (Na) 3. Calcium (Ca) 4. Magnesium (Mg) 5. Aluminum (Al) 6. Zinc (Zn) 7. Iron (Fe) 8. Nickel (Ni) 9. Tin (Sn) 10. Lead (Pb) 11. Hydrogen (H) 12. Copper (Cu) 13. Silver (Ag) 14. Gold (Au) As seen in the example above, metal reactivity decreases as we move down the list.
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4. General Trends in Activity Series

There are some general trends that can be observed in an activity series of metals: - Metals from Group 1 (alkali metals) and Group 2 (alkaline earth metals) in the periodic table, such as potassium, sodium, calcium, and magnesium, tend to be more reactive because they have low ionization energies. - Transition metals (in the middle of the periodic table) are generally less reactive than the alkali and alkaline earth metals. For example, iron, nickel, and copper have lower reactivity compared to sodium or magnesium. - Metals in the bottom-right of the activity series, such as silver and gold, are known as noble metals. They have high ionization energies and are quite unreactive. An activity series of metals helps us predict which metals will react more readily with other elements and which metals can displace others in a chemical reaction depending on their relative reactivities. Understanding and organizing metals according to their reactivity is essential in various applications, such as corrosion prevention, electrochemistry, and metallurgical processes.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

metal reactivity
Metal reactivity refers to how easily a metal can participate in a chemical reaction. This mainly involves a metal's ability to lose electrons and form positive ions.
The ease with which a metal can lose its electrons determines its reactivity and its position in the activity series.
This is why potassium and sodium are at the top of the list鈥攖hey lose electrons very easily. Factors such as ionization energy and atomic size play a crucial role in determining how reactive a metal is. Understanding metal reactivity is essential in predicting how metals interact in various chemical reactions, including displacements and replacements in compounds.
ionization energy
Ionization energy is the energy required to remove an electron from an atom. It is a key factor in determining a metal's reactivity.
Metals with lower ionization energies lose electrons more easily and are therefore more reactive. This is particularly true for alkali metals, which readily lose an electron to stabilize themselves.
This property is why they are so reactive and are often at the top of the activity series. Conversely, metals with high ionization energy, like gold or silver, are less likely to lose electrons and are much less reactive.
In essence, the lower the ionization energy, the higher the metal sits in the activity series, reflecting its higher reactivity in chemical reactions.
alkali metals
Alkali metals are found in Group 1 of the periodic table and include metals like lithium, sodium, and potassium.
They are characterized by their single electron in the outermost shell, which they are eager to lose in order to achieve a stable, noble gas configuration.
This makes them extremely reactive, particularly with water and halogens. Their low ionization energies contribute significantly to their placement high in the activity series.
This group of metals is highly important in various industries and technologies, thanks to their reactivity and ease of forming compounds with other elements.
transition metals
Transition metals occupy the central block of the periodic table and include elements like iron, copper, and nickel. These metals are generally less reactive than alkali metals because they have higher ionization energies and electrons in d-subshells that don't lose electrons as easily.
However, they exhibit a wide range of oxidation states, which allows them to form colorful compounds and participate in a variety of chemical reactions, including acting as catalysts.
Despite being less reactive, transition metals are crucial in many processes, from industrial manufacturing to biological systems, thanks to their ability to complex with other atoms and ions.
noble metals
Noble metals, like gold, silver, and platinum, are found at the bottom of the activity series due to their very low reactivity.
These precious metals have high ionization energies, meaning they do not easily lose electrons, making them resistant to corrosion and tarnish.
Their resistance to reacting with other substances makes them ideal for use in jewelry, electronics, and as catalysts in chemical reactions. Understanding their low reactivity helps in utilizing them effectively in applications where durability and longevity without the need for frequent replacement or maintenance are critical.

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Most popular questions from this chapter

A reaction occurs when hydrosulfuric acid \(\left(\mathrm{H}_{2} \mathrm{S}\right)\) is mixed with an aqueous solution of iron(III) bromide. The reaction produces solid iron(III) sulfide and aqueous hydrogen bromide. Write the chemical and net ionic equations for the reaction.

Photosynthesis Identify the products in the following reaction that occurs in plants: Carbon dioxide and water react to produce glucose and oxygen

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When carbon monoxide and oxygen react, carbon dioxide forms. $$ \text { carbon monoxide } (\mathrm {g})+ \text { oxygen }(\mathrm {g}) \rightarrow \text { carbon dioxide } (\mathrm {g})$$

Mixing nitric acid (HNO \(_{3} )\) and aqueous ammonium hydroxide produces water and aqueous ammonium nitrate.
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