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Grade 11 Exam  >  Grade 11 Tests  >  Chemistry for Grade 11 (IGCSE)  >  Test: Periodic Table and Electronic Configuration - Grade 11 MCQ

Test: Periodic Table and Electronic Configuration - Grade 11 MCQ


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10 Questions MCQ Test Chemistry for Grade 11 (IGCSE) - Test: Periodic Table and Electronic Configuration

Test: Periodic Table and Electronic Configuration for Grade 11 2024 is part of Chemistry for Grade 11 (IGCSE) preparation. The Test: Periodic Table and Electronic Configuration questions and answers have been prepared according to the Grade 11 exam syllabus.The Test: Periodic Table and Electronic Configuration MCQs are made for Grade 11 2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises, MCQs and online tests for Test: Periodic Table and Electronic Configuration below.
Solutions of Test: Periodic Table and Electronic Configuration questions in English are available as part of our Chemistry for Grade 11 (IGCSE) for Grade 11 & Test: Periodic Table and Electronic Configuration 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 Table and Electronic Configuration | 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 Table and Electronic Configuration - Question 1
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According to the electronic configuration concept, which shell of an atom plays a crucial role in determining the atom's stability?

Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 1
In the electronic configuration of an atom, the outermost shell, known as the valence shell, is vital in determining the atom's stability. When this shell is filled with the maximum number of electrons it can hold, the atom is most stable. This stability is crucial for chemical reactions and interactions with other atoms.
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How many electrons can the first shell of an atom accommodate according to the simplified introductory model?

Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 2
In a simplified model used for introductory purposes, the first shell of an atom can hold a maximum of 2 electrons. This shell is the closest to the nucleus and is filled before electrons start occupying the subsequent shells.
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Test: Periodic Table and Electronic Configuration - Question 3
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How many electrons does carbon possess?

Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 3
Carbon possesses 6 electrons. Two of these electrons occupy the first shell, while the remaining four electrons reside in the second shell. This distribution gives carbon an electronic configuration of 2,4. Understanding the electron configuration of elements is crucial in predicting their chemical properties and behavior.
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What happens to the electronic configuration of sodium when it becomes a sodium ion by losing one electron?
Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 4
When sodium loses one electron to become a sodium ion, it retains 10 electrons. In its ionized state, sodium has 2 electrons in the first shell and 8 in the second shell, resulting in an electronic configuration of 2,8. This change in electron configuration is essential in understanding the formation of ions and their stability.
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Why is the electronic configuration of an atom important in chemistry?
Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 5
The electronic configuration of an atom is crucial in chemistry as it helps predict the chemical reactivity of the element. By understanding how electrons are arranged in the electron shells, chemists can anticipate how atoms will interact with other atoms to form compounds. The electron configuration provides valuable insights into an element's behavior in chemical reactions.
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How does the filling of electron shells change after potassium and calcium in the Periodic Table?
Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 6
Following potassium and calcium in the Periodic Table, the filling of electron shells becomes more complex. While the third shell can hold up to 18 electrons, these elements initially fill 8 electrons in the third shell. The remaining electrons then start filling the fourth shell for stability reasons before completing the third shell. This deviation from the standard filling pattern showcases the unique electronic structure of elements beyond potassium and calcium.
Test: Periodic Table and Electronic Configuration - Question 7
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What does the electronic configuration 2,8 of a sodium ion signify?
Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 7
The electronic configuration 2,8 of a sodium ion indicates that it has 8 electrons in its outermost shell. This configuration reflects that sodium belongs to Group 1 of the Periodic Table and possesses a single electron in its outer shell, making it highly reactive. The number of electrons in the outer shell determines an element's chemical properties and its tendency to form bonds with other elements.
Test: Periodic Table and Electronic Configuration - Question 8
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What does the notation '7' in the electron configuration of chlorine signify?
Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 8
The notation '7' in the electron configuration of chlorine signifies that chlorine has 7 outer electrons. This indicates that chlorine belongs to Group VII of the Periodic Table, also known as the halogens. Elements within the same group share similar chemical properties due to having the same number of outer shell electrons, which influences their reactivity and bonding characteristics.
Test: Periodic Table and Electronic Configuration - Question 9
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Why do noble gases exhibit unreactivity compared to other elements?
Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 9
Noble gases demonstrate unreactivity because they possess a full outer shell of electrons. This full electron shell makes them highly stable and minimizes the tendency to gain, lose, or share electrons with other atoms. As a result, noble gases are less likely to form chemical bonds with other elements, leading to their classification as inert or unreactive.
Test: Periodic Table and Electronic Configuration - Question 10
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What is the significance of the outermost shell of electrons in atoms?
Detailed Solution for Test: Periodic Table and Electronic Configuration - Question 10
The outermost shell of electrons in atoms plays a crucial role in influencing the chemical properties of the element. This outer shell is involved in interactions with other atoms, determining how elements will react and form chemical compounds. The number and arrangement of electrons in the outermost shell are key factors in understanding an element's reactivity and chemical behavior.
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