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Step-by-step solution for: Solved Name PERIODIC TABLE PUZZLE 0 1 2 3 4 5 6 7 8 9 10 11 ...
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Step-by-step solution for: Solved Name PERIODIC TABLE PUZZLE 0 1 2 3 4 5 6 7 8 9 10 11 ...
Here is the completed Periodic Table Worksheet with answers and explanations for each question:
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Answer: On the left side of the periodic table, specifically in Group 1 (alkali metals) and Group 2 (alkaline earth metals).
Explanation: These metals have low ionization energies and readily lose electrons to form positive ions, making them highly reactive.
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Answer: On the right side of the periodic table, especially in Group 17 (halogens).
Explanation: Halogens have high electronegativity and strongly attract electrons to complete their valence shell, making them very reactive.
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Answer: Decreases
Explanation: Across a period, the number of protons (nuclear charge) increases, pulling electrons closer to the nucleus. Although electrons are added to the same energy level, the increasing nuclear charge outweighs the electron-electron repulsion, resulting in a smaller atomic radius.
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Answer: Increases
Explanation: Moving down a group, each successive element has an additional energy level (electron shell), which increases the distance between the nucleus and the outermost electrons, causing the atom to become larger.
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Answer: Larger
Explanation: When an atom gains electrons to form an anion, electron-electron repulsion increases, causing the electron cloud to expand.
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Answer: Smaller
Explanation: When an atom loses electrons to form a cation, the remaining electrons are pulled closer to the nucleus due to reduced electron-electron repulsion and stronger effective nuclear charge.
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Answer: Increases
Explanation: Nuclear charge increases across a period, so electrons are held more tightly. More energy is required to remove an electron.
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Answer: Decreases
Explanation: Electrons are farther from the nucleus in lower periods, so they are easier to remove. Additionally, shielding by inner electrons reduces the effective nuclear charge felt by valence electrons.
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Answer: In fluorine (F), located in Group 17, Period 2.
Explanation: Fluorine has the highest electronegativity because it is small and has a high effective nuclear charge, strongly attracting bonding electrons.
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Answer: In cesium (Cs) or francium (Fr), located in Group 1, Period 6 or 7.
Explanation: These alkali metals have large atomic sizes and low effective nuclear charge on valence electrons, so they barely attract bonding electrons.
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Answer: Alkali metals
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Answer: Alkaline earth metals
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Answer: Transition metals
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Answer: From metals to nonmetals
Explanation: The periodic table transitions from metallic elements on the left to nonmetallic elements on the right, with metalloids along the zigzag line.
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Answer: Halogens
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Answer: Fluorine (F)
Explanation: Fluorine is the smallest halogen and has the highest electronegativity, making it the most reactive.
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Answer: Noble gases
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Answer: d-sublevels
Explanation: Transition metals fill the (n-1)d orbitals as electrons are added.
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Answer: Valence electrons
Explanation: Elements in the same group have the same number of electrons in their outermost shell, leading to similar chemical properties.
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Answer: Energy levels (electron shells)
Explanation: Elements in the same period (horizontal row) have the same principal energy level being filled.
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Answer: Transition metal
Explanation: Transition metals often form colored ions due to d-d electron transitions that absorb visible light.
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Answer: More metallic
Explanation: Metallic character increases down a group because atoms lose electrons more easily due to increased atomic size and shielding.
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Answer: Metals
Explanation: About 80% of the elements are metals, including alkali metals, alkaline earth metals, transition metals, and post-transition metals.
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Answer: Atomic number (number of protons)
Explanation: The periodic table is ordered by increasing atomic number, which determines the element's identity and position.
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Answer: Metalloid
Examples: Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te)
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✔ All questions answered! Let me know if you'd like this formatted as a printable worksheet or need help with any specific concept.
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1. Where are the most active metals located?
Answer: On the left side of the periodic table, specifically in Group 1 (alkali metals) and Group 2 (alkaline earth metals).
Explanation: These metals have low ionization energies and readily lose electrons to form positive ions, making them highly reactive.
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2. Where are the most active nonmetals located?
Answer: On the right side of the periodic table, especially in Group 17 (halogens).
Explanation: Halogens have high electronegativity and strongly attract electrons to complete their valence shell, making them very reactive.
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3. As you go from left to right across a period, the atomic size (decreases / increases). Why?
Answer: Decreases
Explanation: Across a period, the number of protons (nuclear charge) increases, pulling electrons closer to the nucleus. Although electrons are added to the same energy level, the increasing nuclear charge outweighs the electron-electron repulsion, resulting in a smaller atomic radius.
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4. As you travel down a group, the atomic size (decreases / increases). Why?
Answer: Increases
Explanation: Moving down a group, each successive element has an additional energy level (electron shell), which increases the distance between the nucleus and the outermost electrons, causing the atom to become larger.
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5. A negative ion is (larger / smaller) than its parent atom.
Answer: Larger
Explanation: When an atom gains electrons to form an anion, electron-electron repulsion increases, causing the electron cloud to expand.
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6. A positive ion is (larger / smaller) than its parent atom.
Answer: Smaller
Explanation: When an atom loses electrons to form a cation, the remaining electrons are pulled closer to the nucleus due to reduced electron-electron repulsion and stronger effective nuclear charge.
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7. As you go from left to right across a period, the first ionization energy generally (decreases / increases). Why?
Answer: Increases
Explanation: Nuclear charge increases across a period, so electrons are held more tightly. More energy is required to remove an electron.
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8. As you go down a group, the first ionization energy generally (decreases / increases). Why?
Answer: Decreases
Explanation: Electrons are farther from the nucleus in lower periods, so they are easier to remove. Additionally, shielding by inner electrons reduces the effective nuclear charge felt by valence electrons.
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9. Where is the highest electronegativity found?
Answer: In fluorine (F), located in Group 17, Period 2.
Explanation: Fluorine has the highest electronegativity because it is small and has a high effective nuclear charge, strongly attracting bonding electrons.
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10. Where is the lowest electronegativity found?
Answer: In cesium (Cs) or francium (Fr), located in Group 1, Period 6 or 7.
Explanation: These alkali metals have large atomic sizes and low effective nuclear charge on valence electrons, so they barely attract bonding electrons.
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11. Elements of Group 1 are called
Answer: Alkali metals
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12. Elements of Group 2 are called
Answer: Alkaline earth metals
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13. Elements of Group 3–12 are called
Answer: Transition metals
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14. As you go from left to right across the periodic table, the elements go from (metals / nonmetals) to (metals / nonmetals).
Answer: From metals to nonmetals
Explanation: The periodic table transitions from metallic elements on the left to nonmetallic elements on the right, with metalloids along the zigzag line.
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15. Group 17 elements are called
Answer: Halogens
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16. The most active element in Group 17 is
Answer: Fluorine (F)
Explanation: Fluorine is the smallest halogen and has the highest electronegativity, making it the most reactive.
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17. Group 18 elements are called
Answer: Noble gases
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18. What sublevels are filling across the Transition Elements?
Answer: d-sublevels
Explanation: Transition metals fill the (n-1)d orbitals as electrons are added.
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19. Elements within a group have a similar number of
Answer: Valence electrons
Explanation: Elements in the same group have the same number of electrons in their outermost shell, leading to similar chemical properties.
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20. Elements across a series have the same number of
Answer: Energy levels (electron shells)
Explanation: Elements in the same period (horizontal row) have the same principal energy level being filled.
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21. A colored ion generally indicates a
Answer: Transition metal
Explanation: Transition metals often form colored ions due to d-d electron transitions that absorb visible light.
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22. As you go down a group, the elements generally become (more / less) metallic.
Answer: More metallic
Explanation: Metallic character increases down a group because atoms lose electrons more easily due to increased atomic size and shielding.
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23. The majority of elements in the periodic table are (metals / nonmetals).
Answer: Metals
Explanation: About 80% of the elements are metals, including alkali metals, alkaline earth metals, transition metals, and post-transition metals.
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24. Elements in the periodic table are arranged according to their
Answer: Atomic number (number of protons)
Explanation: The periodic table is ordered by increasing atomic number, which determines the element's identity and position.
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25. An element with both metallic and nonmetallic properties is called a
Answer: Metalloid
Examples: Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te)
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✔ All questions answered! Let me know if you'd like this formatted as a printable worksheet or need help with any specific concept.
Parent Tip: Review the logic above to help your child master the concept of periodic table worksheet instructional fair.
