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Grade 11 Exam  >  Grade 11 Tests  >  Chemistry for Grade 11 (IGCSE)  >  Test: Periodic Trends - Grade 11 MCQ

Test: Periodic Trends - Grade 11 MCQ


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10 Questions MCQ Test Chemistry for Grade 11 (IGCSE) - Test: Periodic Trends

Test: Periodic Trends for Grade 11 2024 is part of Chemistry for Grade 11 (IGCSE) preparation. The Test: Periodic Trends questions and answers have been prepared according to the Grade 11 exam syllabus.The Test: Periodic Trends MCQs are made for Grade 11 2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises, MCQs and online tests for Test: Periodic Trends below.
Solutions of Test: Periodic Trends questions in English are available as part of our Chemistry for Grade 11 (IGCSE) for Grade 11 & Test: Periodic Trends 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: Periodic Trends | 10 questions in 10 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: Periodic Trends - Question 1
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How does the metallic character of elements change as you move across a Period on the Periodic Table from left to right?

Detailed Solution for Test: Periodic Trends - Question 1
The metallic character of elements diminishes as you progress across a Period on the Periodic Table from left to right. This trend occurs because atoms have a greater tendency to accept electrons to achieve a full valence shell rather than losing them to attain a full outer shell. Metals are predominantly situated on the left side of the Periodic Table, while non-metals are more common on the right side. This change in metallic character is a fundamental concept in understanding the properties and behavior of elements in the periodic table.
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What does the electronic configuration of an atom reveal about its position on the Periodic Table?

Detailed Solution for Test: Periodic Trends - Question 2
The electronic configuration of an atom reveals the number of occupied electron shells of the atom, which in turn indicates the period in which the atom is placed on the Periodic Table. Each notation in the electronic configuration represents the arrangement of electrons in different shells, providing insight into the atom's position within the periodic table based on the number of shells that are occupied.
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Test: Periodic Trends - Question 3
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How do elements in the same group on the Periodic Table typically behave chemically?

Detailed Solution for Test: Periodic Trends - Question 3
Elements in the same group on the Periodic Table exhibit similar chemical properties due to having the same number of electrons in their outermost shell. This similarity arises from the way their outermost electrons interact with other elements, leading to comparable behaviors in chemical reactions and bonding characteristics.
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What does the final notation in an element's electronic configuration signify?
Detailed Solution for Test: Periodic Trends - Question 4
The final notation in an element's electronic configuration signifies the number of outer electrons that the atom possesses, which indicates the number of valence electrons. Valence electrons are the electrons in the outermost shell of an atom and play a crucial role in determining the element's chemical properties and reactivity.
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How do elements within the same group on the Periodic Table differ as you move down the group?
Detailed Solution for Test: Periodic Trends - Question 5
As you move down a group on the Periodic Table, each subsequent element adds a full shell of electrons. This results in elements within the same group having different numbers of electron shells, with each lower element adding an additional shell compared to the element above it. The addition of electron shells influences the element's atomic radius and other chemical properties.
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What property trend can be observed as one moves down Group I of the Periodic Table?
Detailed Solution for Test: Periodic Trends - Question 6
As one moves down Group I of the Periodic Table, the melting point of elements in this group decreases. This trend is a result of the increase in atomic size and the weakening of metallic bonds as you move down the group. For example, lithium (Li) has a higher melting point compared to potassium (K) due to the differences in atomic structure and bonding.
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Which group of elements on the Periodic Table is known for its rapid reactivity with water?
Detailed Solution for Test: Periodic Trends - Question 7
Group I elements, also known as alkali metals, are recognized for their rapid reactivity with water. When alkali metals come into contact with water, they vigorously react, producing hydrogen gas and forming alkaline solutions. This reactivity increases as you move down the group, with cesium (Cs) being the most reactive alkali metal.
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What is a notable characteristic of noble gases in terms of their reactivity?
Detailed Solution for Test: Periodic Trends - Question 8
Noble gases are characterized by their inertness, meaning they are generally unreactive under normal conditions. This is due to their stable electron configurations, which result in minimal tendencies to gain, lose, or share electrons to form compounds. Helium, neon, argon, krypton, xenon, and radon are all noble gases found in Group VIII of the Periodic Table.
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Which group of elements typically exhibits higher density compared to Group I elements?
Detailed Solution for Test: Periodic Trends - Question 9
Transition elements, located in the middle section of the Periodic Table, generally have higher densities compared to Group I elements. This is attributed to the presence of greater mass and more complex atomic structures within transition elements. The density of transition elements contributes to their various industrial applications, such as in manufacturing, construction, and technology.
Test: Periodic Trends - Question 10
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What trend is observed in the reactivity of Group I metals as we move down the group?
Detailed Solution for Test: Periodic Trends - Question 10
The trend observed in the reactivity of Group I metals as we move down the group is that reactivity increases. This means that metals like rubidium, caesium, and francium exhibit more vigorous reactions with air and water compared to lithium, sodium, and potassium. Understanding this trend helps predict the behavior of alkali metals within the group.
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