Periodic Table - Trends & Families

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| By Lmmurp2
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Lmmurp2
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Quizzes Created: 20 | Total Attempts: 22,051
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  • 1/20 Questions

    Magneiusm is in the __________ family.

    • Alkali metal
    • Alkaline earth metal
    • Transition metal
    • Chalcogen
    • Halogen
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About This Quiz

Elements said to be in the same family if they have similarities and for instance boron and lithium are in the same family because they got the largest atomic sizes. What else do you know about the families in which the different elements exist? Take up the quiz and get to find out.

Periodic Table Quizzes & Trivia

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  • 2. 

    Which family is the least reactive?

    • Alkali metals

    • Chalcogens

    • Transition metalsals

    • Noble gases

    Correct Answer
    A. Noble gases
    Explanation
    Noble gases are the least reactive family because they have a full outer electron shell, making them stable and less likely to form chemical bonds with other elements. This stability is due to their complete electron configuration, which does not require them to gain or lose electrons to achieve a stable state. As a result, noble gases have little tendency to react with other elements, making them the least reactive family on the periodic table.

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  • 3. 

    The alkali metals family has _______ valence electrons.

    • 1

    • 2

    • 6

    • 7

    • 8

    Correct Answer
    A. 1
    Explanation
    The alkali metals family has 1 valence electron.

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  • 4. 

    Which of the following elements is an alkali metal?

    • Hydrogen, H

    • Lithium, Li

    • Beryllium, Be

    • Vanadium, V

    Correct Answer
    A. Lithium, Li
    Explanation
    Lithium is an alkali metal because it belongs to Group 1 of the periodic table. Alkali metals are highly reactive metals that are soft, have low melting points, and readily lose their outermost electron to form a positive ion. Lithium exhibits these characteristics, making it an alkali metal. Hydrogen is not an alkali metal as it is a nonmetal, beryllium is an alkaline earth metal, and vanadium is a transition metal.

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  • 5. 

    Why are halogens so highly reactive?

    • They have 1 valence electron and want to get rid of it

    • They have 1 valence electrons and want 7 more electrons

    • They have 7 valence electrons and want 1 more electron

    • They have 7 valence electrons and want to get rid of all 7 electrons

    Correct Answer
    A. They have 7 valence electrons and want 1 more electron
    Explanation
    Halogens are highly reactive because they have 7 valence electrons and want to gain 1 more electron to achieve a stable octet configuration. This makes them highly reactive and likely to form compounds with other elements in order to gain that additional electron.

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  • 6. 

    Ionization energy refers to

    • The energy needed to excite an electron

    • The energy needed to remove an electron

    • The energy needed to attract an electron

    • The energy needed to release a photon

    Correct Answer
    A. The energy needed to remove an electron
    Explanation
    Ionization energy refers to the energy needed to remove an electron from an atom or molecule. This energy is required to overcome the attractive force between the negatively charged electron and the positively charged nucleus. The higher the ionization energy, the more difficult it is to remove an electron, indicating a stronger hold of the electron by the nucleus.

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  • 7. 

    Electronegativity refers to

    • The energy needed to excite an electron

    • The energy needed to remove an electron

    • The energy needed to attract an electron

    • The energy needed to release a photon

    Correct Answer
    A. The energy needed to attract an electron
    Explanation
    Electronegativity refers to the energy needed to attract an electron. It is a measure of an atom's ability to attract and hold onto electrons when it is bonded to another atom. The higher the electronegativity of an atom, the stronger its attraction for electrons. This property is important in determining the type of bond that will form between atoms, as atoms with higher electronegativity values will tend to attract electrons more strongly and form polar covalent or ionic bonds.

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  • 8. 

    The most electronegative element on the periodic table is

    • Lithium, Li

    • Francium, Fr

    • Astatine, At

    • Fluorine, F

    Correct Answer
    A. Fluorine, F
    Explanation
    Fluorine is the most electronegative element on the periodic table because it has the highest electronegativity value. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Fluorine has a strong attraction for electrons due to its small atomic size and high effective nuclear charge. This makes it highly reactive and capable of forming strong bonds with other elements.

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  • 9. 

    The most electronegative element on the periodic table is

    • Lithium, Li

    • Francium, Fr

    • Astatine, At

    • Fluorine, F

    Correct Answer
    A. Fluorine, F
    Explanation
    Fluorine is the most electronegative element on the periodic table. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Fluorine has the highest electronegativity value of 3.98 on the Pauling scale, indicating its strong ability to attract electrons. This is due to its small atomic size and high effective nuclear charge. Therefore, fluorine has a strong tendency to gain electrons and form negative ions, making it the most electronegative element.

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  • 10. 

    _______ is an example of a chalcogen

    • Lithium, Li

    • Barium, Ba

    • Selenium, Se

    • Neon, Ne

    Correct Answer
    A. Selenium, Se
    Explanation
    Selenium is an example of a chalcogen. Chalcogens are a group of elements in the periodic table that includes oxygen, sulfur, selenium, tellurium, and polonium. These elements have similar chemical properties and are located in Group 16 of the periodic table. Selenium, with atomic number 34, is a nonmetal and is commonly used in various industries, including electronics, glass production, and medical applications.

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  • 11. 

    What is the same within a period?

    • The number of valence electrons

    • The number of orbits/shells

    • The reactivity characteristics

    • The physical properties (color, melting point, boiling point)

    Correct Answer
    A. The number of orbits/shells
    Explanation
    The correct answer is the number of orbits/shells. Within a period, the elements have the same number of orbits or shells in their atomic structure. This is because elements in the same period have the same number of energy levels or electron shells. The number of valence electrons, reactivity characteristics, and physical properties may vary within a period depending on the specific element.

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  • 12. 

    Electronegativity __________ as you go down a column because the electrons are ________ to/from the nucleus.

    • Increases, closer

    • Decreases, closer

    • Increases, farther

    • Decreases, farther

    Correct Answer
    A. Decreases, farther
    Explanation
    As you go down a column, electronegativity decreases because the electrons are farther from the nucleus. Electronegativity is the measure of an atom's ability to attract electrons towards itself in a chemical bond. As you move down a column, the number of energy levels or shells increases, causing the outermost electrons to be farther from the nucleus. This decrease in attraction between the nucleus and the outermost electrons results in a decrease in electronegativity.

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  • 13. 

    How many valence electrons does Helium (He) have?

    • 1

    • 2

    • 7

    • 8

    Correct Answer
    A. 2
    Explanation
    Helium (He) has 2 valence electrons. Valence electrons are the electrons in the outermost energy level of an atom. Helium is in the second period of the periodic table, so it has 2 energy levels. The first energy level is filled with 2 electrons, so the 2 remaining electrons in the second energy level are the valence electrons.

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  • 14. 

    Which element in period 5 has the largest atomic radii?

    • Rubidium, Rb

    • Xenon, Xe

    • Vanadium, V

    • Duborium, Db

    Correct Answer
    A. Rubidium, Rb
    Explanation
    Rubidium, Rb, has the largest atomic radii among the given elements in period 5. Atomic radii generally increase from top to bottom within a group or period. Since Rubidium is located towards the bottom of period 5, it has more energy levels and electron shielding, causing its atomic radius to be larger compared to the other elements in the same period.

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  • 15. 

    The element with the lowest ionization energy  periodic table is

    • Lithium, Li

    • Francium, Fr

    • Astatine, At

    • Fluorine, F

    Correct Answer
    A. Francium, Fr
    Explanation
    Francium, Fr, has the lowest ionization energy among the given elements. Ionization energy refers to the energy required to remove an electron from an atom. The trend of ionization energy in the periodic table is that it generally decreases from top to bottom and increases from left to right. Since Francium is located at the bottom and leftmost position in the periodic table, it has the lowest ionization energy. This means that Francium is the easiest to remove an electron from, making it the element with the lowest ionization energy.

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  • 16. 

    Transition metals have _________ valence electrons.

    • 1

    • 2

    • 6

    • 8

    Correct Answer
    A. 2
    Explanation
    Transition metals have 2 valence electrons. This is because transition metals are located in the d-block of the periodic table, and the d sublevel can hold a maximum of 10 electrons. However, in transition metals, the outermost s sublevel is usually filled with 2 electrons, giving them a total of 2 valence electrons.

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  • 17. 

    Iron, Fe is smaller than Hassium (Hs), primarily because

    • Iron has fewer neutrons

    • Iron has a smaller mass

    • Iron has a smaller atomic number

    • Iron has fewer orbits

    Correct Answer
    A. Iron has fewer orbits
    Explanation
    Iron, Fe, is smaller than Hassium, Hs, primarily because iron has fewer orbits. The size of an atom is determined by the number of electrons and the energy levels or orbits in which they are located. Iron has fewer orbits compared to Hassium, which means that the electrons in iron are closer to the nucleus and the atomic radius is smaller. This results in a smaller atom size for iron compared to Hassium.

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  • 18. 

    Atomic radius __________ as you go across a period because ________

    • Increases, there are more orbits

    • Increases, the nucleus pulls less on the electrons

    • Decreases, there are less orbits

    • Decreases, the nucleus pulls more on the electrons

    Correct Answer
    A. Decreases, the nucleus pulls more on the electrons
    Explanation
    As you go across a period, the atomic radius decreases because the nucleus pulls more on the electrons. This is due to the increase in the number of protons in the nucleus, which increases the positive charge. The increased positive charge attracts the negatively charged electrons more strongly, causing them to be pulled closer to the nucleus and resulting in a smaller atomic radius.

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  • 19. 

    Which family consists primarily of large, radioactive, man-made elements?

    • Alkali metals

    • Transition metals

    • Lanthanides

    • Actinides

    Correct Answer
    A. Actinides
    Explanation
    The actinides family consists primarily of large, radioactive, man-made elements. These elements are located in the bottom row of the periodic table and have atomic numbers ranging from 89 to 103. They are all radioactive and are primarily produced through nuclear reactions. Examples of actinides include uranium, plutonium, and americium.

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  • 20. 

    Which element in group 16 has the largest atomic radius?

    • Oxygen, O

    • Sulfur, S

    • Selenium, Se

    • Tellurium, Te

    • Polonium, Po

    • Ununhexium, Uuh

    Correct Answer
    A. Ununhexium, Uuh
    Explanation
    Ununhexium, also known as element 116, has the largest atomic radius among the elements in group 16. This is because as you move down a group in the periodic table, the atomic radius generally increases. Ununhexium is located at the bottom of group 16, so it has the largest atomic radius compared to Oxygen, Sulfur, Selenium, Tellurium, and Polonium.

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  • Current Version
  • Mar 21, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Apr 07, 2011
    Quiz Created by
    Lmmurp2
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