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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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Show Answer Key & Explanations
Step-by-step solution for: Solved Name PERIODIC TABLE PUZZLE 0 1 2 3 4 5 6 7 8 9 10 11 ...
Here’s the completed Periodic Table Worksheet with clear, accurate answers and explanations for each question:
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1. Where are the most active metals located?
✔ Bottom left (Group 1 and 2, especially Francium and Cesium)
*Explanation:* Metallic character increases down a group and decreases across a period. The most reactive metals (alkali and alkaline earth metals) are in Groups 1 and 2, and reactivity increases going down the group due to easier electron loss.
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2. Where are the most active nonmetals located?
✔ Top right (Group 17 — Halogens, especially Fluorine)
*Explanation:* Nonmetallic character increases up a group and across a period. Fluorine is the most electronegative and reactive nonmetal, found at the top right (excluding noble gases).
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3. As you go from left to right across a period, the atomic size (decreases / increases). Why?
✔ Decreases
*Explanation:* Across a period, protons are added to the nucleus while electrons are added to the same energy level. The increasing nuclear charge pulls electrons closer, shrinking the atom.
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4. As you travel down a group, the atomic size (decreases / increases). Why?
✔ Increases
*Explanation:* Each row adds a new electron shell (energy level), making atoms larger despite more protons. The increased distance from nucleus outweighs the increased nuclear charge.
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5. A negative ion is (larger / smaller) than its parent atom.
✔ Larger
*Explanation:* Adding electrons increases electron-electron repulsion, causing the electron cloud to expand. Example: Cl⁻ is larger than Cl.
---
6. A positive ion is (larger / smaller) than its parent atom.
✔ Smaller
*Explanation:* Removing electrons reduces electron-electron repulsion and often removes an entire shell, making the ion smaller. Example: Na⁺ is smaller than Na.
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7. As you go from left to right across a period, the first ionization energy generally (decreases / increases). Why?
✔ Increases
*Explanation:* Atoms become smaller and have higher effective nuclear charge, making it harder to remove an electron. More energy required = higher ionization energy.
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8. As you go down a group, the first ionization energy generally (decreases / increases). Why?
✔ Decreases
*Explanation:* Outer electrons are farther from the nucleus and shielded by inner shells, so less energy is needed to remove them.
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9. Where is the highest electronegativity found?
✔ Top right (Fluorine, Group 17)
*Explanation:* Electronegativity increases across a period and decreases down a group. Fluorine (EN ≈ 4.0) is the most electronegative element.
---
10. Where is the lowest electronegativity found?
✔ Bottom left (Francium or Cesium, Group 1)
*Explanation:* These elements have the largest atomic radii and weakest pull on bonding electrons, so they have the lowest electronegativity (~0.7–0.8).
---
11. Elements of Group 1 are called
✔ Alkali metals
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12. Elements of Group 2 are called
✔ Alkaline earth metals
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13. Elements of Group 3-12 are called
✔ 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).
✔ Metals → Nonmetals
*Explanation:* Left side = metals; right side = nonmetals; middle = metalloids (e.g., B, Si, Ge, As, Sb, Te).
---
15. Group 17 elements are called
✔ Halogens
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16. The most active element in Group 17 is
✔ Fluorine (F)
*Explanation:* It has the highest electronegativity and strongest tendency to gain electrons.
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17. Group 18 elements are called
✔ Noble gases
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18. What sublevels are filling across the Transition Elements?
✔ d-sublevel
*Explanation:* Transition metals fill the d-orbitals (e.g., Sc to Zn fill 3d; Y to Cd fill 4d, etc.).
---
19. Elements within a group have a similar number of
✔ Valence electrons
*Explanation:* This determines chemical properties. E.g., all Group 1 elements have 1 valence electron.
---
20. Elements across a series have the same number of
✔ Electron shells (principal energy levels)
*Explanation:* All elements in Period 3 (Na to Ar) have electrons in n=1, 2, and 3 shells.
---
21. A colored ion generally indicates a
✔ Transition metal ion
*Explanation:* Transition metals form colored ions due to d-d electron transitions (e.g., Cu²⁺ blue, Fe³⁺ yellow/brown).
---
22. As you go down a group, the elements generally become (more / less) metallic.
✔ More metallic
*Explanation:* Atomic size increases, ionization energy decreases → easier to lose electrons → more metallic character.
---
23. The majority of elements in the periodic table are (metals / nonmetals).
✔ Metals
*Explanation:* ~75% of elements are metals (left and center of table).
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24. Elements in the periodic table are arranged according to their
✔ Atomic number (number of protons)
*Explanation:* Modern periodic law: properties are periodic functions of atomic number.
---
25. An element with both metallic and nonmetallic properties is called a
✔ Metalloid
*Explanation:* Examples: Silicon, Germanium, Arsenic — have intermediate conductivity, brittle but shiny, etc.
---
✔ Final Tip: Use this worksheet to reinforce trends — remember “across = change, down = increase/decrease” depending on property. Always relate to nuclear charge, shielding, and electron configuration!
Let me know if you’d like a printable version or flashcards for these concepts!
---
1. Where are the most active metals located?
✔ Bottom left (Group 1 and 2, especially Francium and Cesium)
*Explanation:* Metallic character increases down a group and decreases across a period. The most reactive metals (alkali and alkaline earth metals) are in Groups 1 and 2, and reactivity increases going down the group due to easier electron loss.
---
2. Where are the most active nonmetals located?
✔ Top right (Group 17 — Halogens, especially Fluorine)
*Explanation:* Nonmetallic character increases up a group and across a period. Fluorine is the most electronegative and reactive nonmetal, found at the top right (excluding noble gases).
---
3. As you go from left to right across a period, the atomic size (decreases / increases). Why?
✔ Decreases
*Explanation:* Across a period, protons are added to the nucleus while electrons are added to the same energy level. The increasing nuclear charge pulls electrons closer, shrinking the atom.
---
4. As you travel down a group, the atomic size (decreases / increases). Why?
✔ Increases
*Explanation:* Each row adds a new electron shell (energy level), making atoms larger despite more protons. The increased distance from nucleus outweighs the increased nuclear charge.
---
5. A negative ion is (larger / smaller) than its parent atom.
✔ Larger
*Explanation:* Adding electrons increases electron-electron repulsion, causing the electron cloud to expand. Example: Cl⁻ is larger than Cl.
---
6. A positive ion is (larger / smaller) than its parent atom.
✔ Smaller
*Explanation:* Removing electrons reduces electron-electron repulsion and often removes an entire shell, making the ion smaller. Example: Na⁺ is smaller than Na.
---
7. As you go from left to right across a period, the first ionization energy generally (decreases / increases). Why?
✔ Increases
*Explanation:* Atoms become smaller and have higher effective nuclear charge, making it harder to remove an electron. More energy required = higher ionization energy.
---
8. As you go down a group, the first ionization energy generally (decreases / increases). Why?
✔ Decreases
*Explanation:* Outer electrons are farther from the nucleus and shielded by inner shells, so less energy is needed to remove them.
---
9. Where is the highest electronegativity found?
✔ Top right (Fluorine, Group 17)
*Explanation:* Electronegativity increases across a period and decreases down a group. Fluorine (EN ≈ 4.0) is the most electronegative element.
---
10. Where is the lowest electronegativity found?
✔ Bottom left (Francium or Cesium, Group 1)
*Explanation:* These elements have the largest atomic radii and weakest pull on bonding electrons, so they have the lowest electronegativity (~0.7–0.8).
---
11. Elements of Group 1 are called
✔ Alkali metals
---
12. Elements of Group 2 are called
✔ Alkaline earth metals
---
13. Elements of Group 3-12 are called
✔ Transition metals
---
14. As you go from left to right across the periodic table, the elements go from (metals / nonmetals) to (metals / nonmetals).
✔ Metals → Nonmetals
*Explanation:* Left side = metals; right side = nonmetals; middle = metalloids (e.g., B, Si, Ge, As, Sb, Te).
---
15. Group 17 elements are called
✔ Halogens
---
16. The most active element in Group 17 is
✔ Fluorine (F)
*Explanation:* It has the highest electronegativity and strongest tendency to gain electrons.
---
17. Group 18 elements are called
✔ Noble gases
---
18. What sublevels are filling across the Transition Elements?
✔ d-sublevel
*Explanation:* Transition metals fill the d-orbitals (e.g., Sc to Zn fill 3d; Y to Cd fill 4d, etc.).
---
19. Elements within a group have a similar number of
✔ Valence electrons
*Explanation:* This determines chemical properties. E.g., all Group 1 elements have 1 valence electron.
---
20. Elements across a series have the same number of
✔ Electron shells (principal energy levels)
*Explanation:* All elements in Period 3 (Na to Ar) have electrons in n=1, 2, and 3 shells.
---
21. A colored ion generally indicates a
✔ Transition metal ion
*Explanation:* Transition metals form colored ions due to d-d electron transitions (e.g., Cu²⁺ blue, Fe³⁺ yellow/brown).
---
22. As you go down a group, the elements generally become (more / less) metallic.
✔ More metallic
*Explanation:* Atomic size increases, ionization energy decreases → easier to lose electrons → more metallic character.
---
23. The majority of elements in the periodic table are (metals / nonmetals).
✔ Metals
*Explanation:* ~75% of elements are metals (left and center of table).
---
24. Elements in the periodic table are arranged according to their
✔ Atomic number (number of protons)
*Explanation:* Modern periodic law: properties are periodic functions of atomic number.
---
25. An element with both metallic and nonmetallic properties is called a
✔ Metalloid
*Explanation:* Examples: Silicon, Germanium, Arsenic — have intermediate conductivity, brittle but shiny, etc.
---
✔ Final Tip: Use this worksheet to reinforce trends — remember “across = change, down = increase/decrease” depending on property. Always relate to nuclear charge, shielding, and electron configuration!
Let me know if you’d like a printable version or flashcards for these concepts!
Parent Tip: Review the logic above to help your child master the concept of chemistry periodic table worksheet answer key.
