11th Grade; How Much Do You Actually Know About Chemistry

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Janyce Wowk, BS, Chemistry |
Chemistry Expert
Review Board Member
Janyce is a chemistry professional with a B.S. in Chemistry from Montclair State University. Her experience as a research assistant and lab technician in a PFAS laboratory has allowed her to develop strong laboratory, data analysis, and research skills. On our review board team, Janyce reviews chemistry quizzes, ensuring accuracy and enhancing the quality of our educational materials. Her chemistry expertise and commitment to precision make her a valuable asset in maintaining high-quality resources for learners.
, BS, Chemistry
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11th Grade; How Much Do You Actually Know About Chemistry - Quiz

Did you know that everything is made out of chemicals? . Chemistry is a scientific discipline involved with elements and compound composed of atoms. Molecules and ions. Chemistry is the study of matter;it's composition, properties and reactivity.
Try out this quiz to test your knowledge of chemistry.


Questions and Answers
  • 1. 

    In a periodic table, elements are organized from left to right and from top to bottom. What is the name given to element moving from left to right?

    • A.

      Group

    • B.

      Period

    • C.

      Isotopes

    • D.

      Reactants

    Correct Answer
    B. Period
    Explanation
    In a periodic table, elements are organized in periods, which are the rows that go from left to right. Each period represents a different energy level or shell in which the electrons of the elements are arranged. Therefore, the correct answer is "Period".

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  • 2. 

    What is the name given to elements moving from top to bottom?

    • A.

      Group

    • B.

      Period

    • C.

      Isotopes

    • D.

      Reactants

    Correct Answer
    A. Group
  • 3. 

    Which of the following is true about an atom radius?

    • A.

      Decreases from top to bottom down a group

    • B.

      Increases bottom to top up a group

    • C.

      Decreases right to left accros a group

    • D.

      Decreases left to right across a period

    Correct Answer
    B. Increases bottom to top up a group
    Explanation
    The atomic radius trend within the periodic table can be summarized as follows: it generally increases from top to bottom within a group as additional electron shells are added, leading to greater distance between the nucleus and the outermost electrons. Conversely, it decreases from left to right across a period due to the increasing nuclear charge pulling the outermost electrons closer to the nucleus. Therefore, the correct statement is B, which accurately describes the trend of increasing atomic radius from bottom to top within a group.

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  • 4. 

    Which of the following is a property of atom radius?

    • A.

      Decreases moving from right to left across a period

    • B.

      Increases moving from from bottom to top up a group

    • C.

      Increases moving from top to bottom

    • D.

      Increases moving from left to right across a period

    Correct Answer
    C. Increases moving from top to bottom
    Explanation
    The correct answer is "Increases moving from top to bottom down a group." This is because as you move down a group in the periodic table, the number of energy levels or shells increases. This results in an increase in the atomic radius because the electrons occupy larger orbitals further away from the nucleus. Therefore, the distance between the nucleus and the outermost electrons increases, leading to an increase in the size of the atom.

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  • 5. 

    What is ionization energy?

    • A.

      Energy needed to accept an electron.

    • B.

      Amount of energy needed to remove an electron from anion in a gas state

    • C.

      Amount of energy needed to remove proton from an anion in a solid state

    • D.

      Amount of energy needes to remove neurons from an anion in a liquid state

    Correct Answer
    B. Amount of energy needed to remove an electron from anion in a gas state
    Explanation
    Ionization energy is the amount of energy required to remove an electron from an atom or ion in the gaseous state, resulting in the formation of a positively charged ion. This process occurs when an external energy source, such as heat or light, is applied to the atom or ion, causing the electron to be released. The ionization energy is a measure of the strength of the attraction between the electron and the nucleus of the atom or ion. Additionally, the trend of ionization energy across the periodic table provides valuable information about the electron configuration and chemical behavior of elements.

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  • 6. 

    Which of the following is a property of ionization energy?

    • A.

      Increases moving from left to right across a period

    • B.

      Decreases moving from left to right across a period

    • C.

      All.of the above

    • D.

      Non of the above

    Correct Answer
    A. Increases moving from left to right across a period
    Explanation
    The ionization energy is the energy required to remove an electron from an atom or ion. As we move from left to right across a period, the atomic radius decreases, resulting in a stronger attraction between the positively charged nucleus and the negatively charged electrons. This increased attraction requires more energy to remove an electron, thus increasing the ionization energy. Therefore, the correct answer is "Increases moving from left to right across a period."

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  • 7. 

    Which of the following is a feature of Ionization energy?

    • A.

      Increases moving from top to bottom down a group

    • B.

      Decreases moving from bottom to top up a group

    • C.

      Decreases moving from top to bottom down a group

    • D.

      Non of the above

    Correct Answer
    C. Decreases moving from top to bottom down a group
    Explanation
    Ionization energy refers to the energy required to remove an electron from an atom or ion. As you move from top to bottom down a group in the periodic table, the ionization energy generally decreases. This is because the atomic size increases, resulting in a greater distance between the nucleus and the outermost electrons. As a result, the attraction between the nucleus and the electrons weakens, making it easier to remove an electron and lowering the ionization energy.

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  • 8. 

    What is electron affinity?

    • A.

      Reflection of how readily an atom will accept an electron

    • B.

      Flexibility of cations

    • C.

      Ability of anions to become positively charged

    • D.

      Non of the above

    Correct Answer
    A. Reflection of how readily an atom will accept an electron
    Explanation
    Electron affinity refers to the reflection of how readily an atom will accept an electron. It is a measure of the attraction an atom has for an additional electron. A higher electron affinity indicates a stronger attraction for electrons, while a lower electron affinity suggests a weaker attraction. Therefore, the correct answer accurately defines electron affinity as the reflection of an atom's willingness to accept an electron.

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  • 9. 

    Which of the following is true about electronegativity?

    • A.

      The higher the electronegativity, the lower the attraction for bonding an electron

    • B.

      The higher the electronegativity, the lesser the beauty of the proton

    • C.

      The lower the electronegativity, the higher the attraction for bonding an electron

    • D.

      The higher the electronegativity, the higher the attraction for bonding an electron

    Correct Answer
    D. The higher the electronegativity, the higher the attraction for bonding an electron
    Explanation
    Electronegativity refers to the ability of an atom to attract electrons towards itself in a chemical bond. The answer states that the higher the electronegativity, the higher the attraction for bonding an electron. This means that atoms with high electronegativity have a strong pull on electrons, making them more likely to form bonds by attracting electrons from other atoms. Therefore, the answer correctly explains the relationship between electronegativity and the attraction for bonding electrons.

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  • 10. 

    Which of the following is true?

    • A.

      Electronegativity increases down an element group.

    • B.

      Electronegativity decreases across the period.

    • C.

      Electronegativity decreases down the group.

    • D.

      Non of the above

    Correct Answer
    C. Electronegativity decreases down the group.
    Explanation
    Electronegativity is the measure of an atom's ability to attract electrons in a chemical bond. In general, electronegativity tends to decrease as you move down a group in the periodic table. This is because the atomic size increases down a group, resulting in a greater distance between the nucleus and the outermost electrons. As a result, the positive charge of the nucleus has less influence on the outer electrons, leading to a decrease in electronegativity. Therefore, the statement "Electronegativity decreases down the group" is true.

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Janyce Wowk |BS, Chemistry |
Chemistry Expert
Janyce is a chemistry professional with a B.S. in Chemistry from Montclair State University. Her experience as a research assistant and lab technician in a PFAS laboratory has allowed her to develop strong laboratory, data analysis, and research skills. On our review board team, Janyce reviews chemistry quizzes, ensuring accuracy and enhancing the quality of our educational materials. Her chemistry expertise and commitment to precision make her a valuable asset in maintaining high-quality resources for learners.

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