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Grade 11 Exam  >  Grade 11 Tests  >  Chemistry for Grade 11 (IGCSE)  >  Test: Reactivity Series & Explaining Reactivity - Grade 11 MCQ

Test: Reactivity Series & Explaining Reactivity - Grade 11 MCQ


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15 Questions MCQ Test Chemistry for Grade 11 (IGCSE) - Test: Reactivity Series & Explaining Reactivity

Test: Reactivity Series & Explaining Reactivity for Grade 11 2024 is part of Chemistry for Grade 11 (IGCSE) preparation. The Test: Reactivity Series & Explaining Reactivity questions and answers have been prepared according to the Grade 11 exam syllabus.The Test: Reactivity Series & Explaining Reactivity MCQs are made for Grade 11 2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises, MCQs and online tests for Test: Reactivity Series & Explaining Reactivity below.
Solutions of Test: Reactivity Series & Explaining Reactivity questions in English are available as part of our Chemistry for Grade 11 (IGCSE) for Grade 11 & Test: Reactivity Series & Explaining Reactivity solutions in Hindi for Chemistry for Grade 11 (IGCSE) course. Download more important topics, notes, lectures and mock test series for Grade 11 Exam by signing up for free. Attempt Test: Reactivity Series & Explaining Reactivity | 15 questions in 15 minutes | Mock test for Grade 11 preparation | Free important questions MCQ to study Chemistry for Grade 11 (IGCSE) for Grade 11 Exam | Download free PDF with solutions
Test: Reactivity Series & Explaining Reactivity - Question 1
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According to the reactivity series of metals, which metal is the most reactive?

Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 1
In the reactivity series of metals, potassium is considered the most reactive metal. This means that potassium can easily lose electrons and form positive ions in chemical reactions. An interesting fact is that due to its high reactivity, potassium is stored under oil to prevent it from reacting with moisture or oxygen in the air.
Test: Reactivity Series & Explaining Reactivity - Question 2
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How does the reactivity series of metals help in understanding their behavior in reactions with water and acids?

Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 2
The reactivity series of metals helps in understanding their behavior in reactions with water and acids by ordering metals based on their reactivity levels. This arrangement allows us to predict how metals will react with water and acids, with the most reactive metals reacting more vigorously compared to less reactive metals.
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Test: Reactivity Series & Explaining Reactivity - Question 3
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Why are non-metals like hydrogen and carbon included in the reactivity series of metals?

Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 3
Non-metals like hydrogen and carbon are included in the reactivity series of metals because of their role in extracting metals from their oxides. Despite being non-metals, hydrogen and carbon play crucial roles in metallurgy by participating in reactions that help in the extraction of metals from their ores.
Test: Reactivity Series & Explaining Reactivity - Question 4
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How does the reactivity series assist in identifying the relative reactivity of metals with water and acids?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 4
The reactivity series assists in identifying the relative reactivity of metals with water and acids by ordering metals based on their reactivity levels. This ordering helps in predicting and understanding how different metals will react with water and acids, providing valuable insights into their chemical properties and behavior in various reactions.
Test: Reactivity Series & Explaining Reactivity - Question 5
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What type of reaction occurs when more reactive metals such as potassium, sodium, and calcium react with cold water?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 5
When highly reactive metals like potassium, sodium, and calcium react with cold water, they produce metal hydroxide along with hydrogen gas. This reaction is a characteristic feature of metals high in the reactivity series and showcases their vigorous reactivity with water.
Test: Reactivity Series & Explaining Reactivity - Question 6
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Which metal is known for its vigorous reaction with water, producing hydrogen gas and a strong alkaline solution of sodium hydroxide?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 6
Sodium (Na) is recognized for its vigorous reaction with water, resulting in the production of hydrogen gas and a strong alkaline solution of sodium hydroxide. This reaction is a clear demonstration of sodium's high reactivity. The reaction of sodium with water is quite exothermic and showcases the intensity with which highly reactive metals can interact with water.
Test: Reactivity Series & Explaining Reactivity - Question 7
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Which metal is considered unreactive and does not readily react with oxygen under normal conditions?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 7
Gold (Au) is a noble metal known for its unreactive nature, particularly with oxygen under normal conditions. Unlike reactive metals like alkali metals, gold does not undergo oxidation reactions with oxygen. This property is one of the reasons why gold is highly valued for its resistance to tarnishing and corrosion, making it a sought-after material in various industries.
Test: Reactivity Series & Explaining Reactivity - Question 8
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What determines the reactivity of a metal in relation to electron loss?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 8
The reactivity of a metal is determined by its propensity to lose electrons. Metals that are positioned higher in the reactivity series easily shed electrons, showcasing higher reactivity compared to metals lower in the series. This tendency to lose electrons plays a crucial role in various chemical reactions involving metals.
Test: Reactivity Series & Explaining Reactivity - Question 9
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In a displacement reaction between metals and aqueous solutions of metal salts, what happens when a more reactive metal encounters a less reactive metal?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 9
In a displacement reaction, when a more reactive metal encounters a less reactive metal in a solution of one of its salts, the more reactive metal displaces the less reactive metal. This phenomenon occurs because more reactive metals have a higher tendency to lose electrons and form ions compared to less reactive metals, showcasing the reactivity trend in action.
Test: Reactivity Series & Explaining Reactivity - Question 10
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What chemical process involves the gain of electrons according to the mnemonic OIL-RIG?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 10
According to the mnemonic OIL-RIG, reduction involves the gain of electrons. In chemical reactions, reduction refers to the process where a species gains electrons, leading to a decrease in its oxidation state. This mnemonic helps in remembering the key concept of reduction as it relates to electron transfer in reactions.
Test: Reactivity Series & Explaining Reactivity - Question 11
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How does the displacement of copper by magnesium in a copper sulfate solution visually manifest?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 11
When magnesium displaces copper in a copper sulfate solution, the displacement reaction visually manifests as copper forming a layer on magnesium. This process showcases the reactivity of magnesium as it displaces copper from the solution, leading to the formation of elemental copper and magnesium sulfate. This visual observation provides evidence of the displacement reaction and the relative reactivity of the metals involved.
Test: Reactivity Series & Explaining Reactivity - Question 12
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What is the primary reason why aluminium appears to be unreactive with water and dilute acids despite being high in the reactivity series?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 12
Aluminium, despite its position high in the reactivity series, seems unreactive with water and dilute acids due to its rapid reaction with oxygen. This reaction results in the formation of a thin layer of aluminium oxide, which acts as a protective barrier. This oxide layer prevents further reactions with water and dilute acids, giving the appearance of unreactivity. This unique property of aluminium highlights the significance of surface chemistry in determining the reactivity of metals with various substances.
Test: Reactivity Series & Explaining Reactivity - Question 13
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Which characteristic of aluminium contributes to its behavior as if it is unreactive with water and dilute acids?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 13
The formation of a protective layer of aluminium oxide on the surface of aluminium is the key characteristic that contributes to its behavior as if it is unreactive with water and dilute acids. This thin layer effectively shields the underlying aluminium from further reactions by preventing direct contact with these substances. Understanding this unique property of aluminium sheds light on how surface reactions can significantly influence the overall reactivity of a metal.
Test: Reactivity Series & Explaining Reactivity - Question 14
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Why does aluminium not react with water despite its high reactivity in the series?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 14
Aluminium's reactivity with water is mitigated by the formation of a protective layer of aluminium oxide when it comes into contact with water. This oxide layer acts as a barrier, preventing further reaction of aluminium with water molecules. As a result, despite its high reactivity in the series, aluminium displays limited reactivity with water due to the presence of this protective oxide layer.
Test: Reactivity Series & Explaining Reactivity - Question 15
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How does the formation of a protective layer of aluminium oxide affect its reactivity with dilute acids?
Detailed Solution for Test: Reactivity Series & Explaining Reactivity - Question 15
The formation of a protective layer of aluminium oxide plays a crucial role in inhibiting the reaction of aluminium with dilute acids. This oxide layer acts as a barrier that prevents direct contact between the underlying aluminium metal and the acidic solution. As a result, the reactivity of aluminium with dilute acids is significantly reduced, showcasing how surface chemistry can influence the overall chemical behavior of a metal in different environments.
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