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Step-by-step solution for: Daniel Davis: Daniel Davis: October 2008 Archives
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Step-by-step solution for: Daniel Davis: Daniel Davis: October 2008 Archives
Here is the completed Periodic Table Worksheet with answers and explanations for each question:
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1. Where are the most active metals located?
Answer: Bottom left (Group 1, especially francium or cesium).
Explanation: The most active metals are found in Group 1 (alkali metals), particularly as you go down the group. Their low ionization energy makes them highly reactive.
2. Where are the most active nonmetals located?
Answer: Top right (Group 17, especially fluorine).
Explanation: The most active nonmetals are halogens (Group 17), especially fluorine, due to high electronegativity and strong tendency to gain electrons.
3. As you go from left to right across a period, the atomic size (decreases / increases). Why?
Answer: Decreases.
Explanation: Across a period, nuclear charge increases, pulling electrons closer to the nucleus. Shielding remains relatively constant, so atomic radius decreases.
4. As you travel down a group, the atomic size (decreases / increases). Why?
Answer: Increases.
Explanation: Down a group, each successive element has an additional electron shell, increasing the atomic radius despite increased nuclear charge.
5. A negative ion is (larger / smaller) than its parent atom.
Answer: Larger
Explanation: Adding electrons increases electron-electron repulsion, causing the electron cloud to expand.
6. A positive ion is (larger / smaller) than its parent atom.
Answer: Smaller
Explanation: Removing electrons reduces electron-electron repulsion and increases effective nuclear charge per electron, pulling remaining electrons closer.
7. As you go from left to right across a period, the first ionization energy generally (decreases / increases). Why?
Answer: Increases
Explanation: Increasing nuclear charge pulls electrons more strongly, making it harder to remove an electron.
8. As you go down a group, the first ionization energy generally (decreases / increases). Why?
Answer: Decreases
Explanation: Electrons are farther from the nucleus and shielded by inner electrons, making them easier to remove.
9. Where is the highest electronegativity found?
Answer: Fluorine (top right corner, Group 17)
Explanation: Fluorine has the highest electronegativity because it strongly attracts bonding electrons.
10. Where is the lowest electronegativity found?
Answer: Francium (bottom left, Group 1)
Explanation: Metals like francium have very low electronegativity because they readily lose electrons.
11. Elements of Group 1 are called
Answer: Alkali metals
Explanation: Highly reactive metals that form +1 ions.
12. Elements of Group 2 are called
Answer: Alkaline earth metals
Explanation: Reactive metals forming +2 ions.
13. Elements of Group 3–12 are called
Answer: Transition metals
Explanation: These elements fill d-orbitals and often form colored compounds and multiple oxidation states.
14. As you go from left to right across the periodic table, the elements go from (metals / nonmetals) to (metals / nonmetals).
Answer: Metals → Nonmetals
Explanation: The periodic table transitions from metallic elements on the left to nonmetallic elements on the right.
15. Group 17 elements are called
Answer: Halogens
Explanation: Highly reactive nonmetals that form -1 ions.
16. The most active element in Group 17 is
Answer: Fluorine
Explanation: Fluorine is the most reactive halogen due to high electronegativity and small atomic size.
17. Group 18 elements are called
Answer: Noble gases
Explanation: Chemically inert due to complete valence shells.
18. What sublevels are filling across the Transition Elements?
Answer: d-sublevels
Explanation: Transition metals involve filling of the d orbitals (e.g., 3d, 4d, 5d).
19. Elements within a group have a similar number of
Answer: Valence electrons
Explanation: Elements in the same group have the same number of outermost electrons, leading to similar chemical behavior.
20. Elements across a series have the same number of
Answer: Electron shells (energy levels)
Explanation: Elements in the same period have electrons in the same principal energy level.
21. A colored ion generally indicates a
Answer: Transition metal
Explanation: Transition metals have partially filled d-orbitals, allowing d-d electronic transitions that absorb visible light.
22. As you go down a group, the elements generally become (more / less) metallic.
Answer: More metallic
Explanation: Metallic character increases down a group due to decreasing ionization energy and increasing atomic size.
23. The majority of elements in the periodic table are (metals / nonmetals).
Answer: Metals
Explanation: Over 80% of the elements are metals.
24. Elements in the periodic table are arranged according to their
Answer: Atomic number
Explanation: Elements are ordered by increasing number of protons (atomic number).
25. An element with both metallic and nonmetallic properties is called a
Answer: Metalloid
Explanation: Metalloids (e.g., silicon, arsenic) lie along the staircase line and exhibit intermediate properties.
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✔ Final Answer Summary:
1. Bottom left (Group 1)
2. Top right (Group 17)
3. Decreases – due to increasing nuclear charge
4. Increases – due to addition of electron shells
5. Larger
6. Smaller
7. Increases – increasing nuclear charge
8. Decreases – increasing shielding and distance
9. Fluorine
10. Francium
11. Alkali metals
12. Alkaline earth metals
13. Transition metals
14. Metals → Nonmetals
15. Halogens
16. Fluorine
17. Noble gases
18. d-sublevels
19. Valence electrons
20. Electron shells
21. Transition metal
22. More metallic
23. Metals
24. Atomic number
25. Metalloid
Let me know if you'd like this formatted as a printable PDF or need help understanding any concept further!
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PERIODIC TABLE WORKSHEET
1. Where are the most active metals located?
Answer: Bottom left (Group 1, especially francium or cesium).
Explanation: The most active metals are found in Group 1 (alkali metals), particularly as you go down the group. Their low ionization energy makes them highly reactive.
2. Where are the most active nonmetals located?
Answer: Top right (Group 17, especially fluorine).
Explanation: The most active nonmetals are halogens (Group 17), especially fluorine, due to high electronegativity and strong tendency to gain electrons.
3. As you go from left to right across a period, the atomic size (decreases / increases). Why?
Answer: Decreases.
Explanation: Across a period, nuclear charge increases, pulling electrons closer to the nucleus. Shielding remains relatively constant, so atomic radius decreases.
4. As you travel down a group, the atomic size (decreases / increases). Why?
Answer: Increases.
Explanation: Down a group, each successive element has an additional electron shell, increasing the atomic radius despite increased nuclear charge.
5. A negative ion is (larger / smaller) than its parent atom.
Answer: Larger
Explanation: Adding electrons increases electron-electron repulsion, causing the electron cloud to expand.
6. A positive ion is (larger / smaller) than its parent atom.
Answer: Smaller
Explanation: Removing electrons reduces electron-electron repulsion and increases effective nuclear charge per electron, pulling remaining electrons closer.
7. As you go from left to right across a period, the first ionization energy generally (decreases / increases). Why?
Answer: Increases
Explanation: Increasing nuclear charge pulls electrons more strongly, making it harder to remove an electron.
8. As you go down a group, the first ionization energy generally (decreases / increases). Why?
Answer: Decreases
Explanation: Electrons are farther from the nucleus and shielded by inner electrons, making them easier to remove.
9. Where is the highest electronegativity found?
Answer: Fluorine (top right corner, Group 17)
Explanation: Fluorine has the highest electronegativity because it strongly attracts bonding electrons.
10. Where is the lowest electronegativity found?
Answer: Francium (bottom left, Group 1)
Explanation: Metals like francium have very low electronegativity because they readily lose electrons.
11. Elements of Group 1 are called
Answer: Alkali metals
Explanation: Highly reactive metals that form +1 ions.
12. Elements of Group 2 are called
Answer: Alkaline earth metals
Explanation: Reactive metals forming +2 ions.
13. Elements of Group 3–12 are called
Answer: Transition metals
Explanation: These elements fill d-orbitals and often form colored compounds and multiple oxidation states.
14. As you go from left to right across the periodic table, the elements go from (metals / nonmetals) to (metals / nonmetals).
Answer: Metals → Nonmetals
Explanation: The periodic table transitions from metallic elements on the left to nonmetallic elements on the right.
15. Group 17 elements are called
Answer: Halogens
Explanation: Highly reactive nonmetals that form -1 ions.
16. The most active element in Group 17 is
Answer: Fluorine
Explanation: Fluorine is the most reactive halogen due to high electronegativity and small atomic size.
17. Group 18 elements are called
Answer: Noble gases
Explanation: Chemically inert due to complete valence shells.
18. What sublevels are filling across the Transition Elements?
Answer: d-sublevels
Explanation: Transition metals involve filling of the d orbitals (e.g., 3d, 4d, 5d).
19. Elements within a group have a similar number of
Answer: Valence electrons
Explanation: Elements in the same group have the same number of outermost electrons, leading to similar chemical behavior.
20. Elements across a series have the same number of
Answer: Electron shells (energy levels)
Explanation: Elements in the same period have electrons in the same principal energy level.
21. A colored ion generally indicates a
Answer: Transition metal
Explanation: Transition metals have partially filled d-orbitals, allowing d-d electronic transitions that absorb visible light.
22. As you go down a group, the elements generally become (more / less) metallic.
Answer: More metallic
Explanation: Metallic character increases down a group due to decreasing ionization energy and increasing atomic size.
23. The majority of elements in the periodic table are (metals / nonmetals).
Answer: Metals
Explanation: Over 80% of the elements are metals.
24. Elements in the periodic table are arranged according to their
Answer: Atomic number
Explanation: Elements are ordered by increasing number of protons (atomic number).
25. An element with both metallic and nonmetallic properties is called a
Answer: Metalloid
Explanation: Metalloids (e.g., silicon, arsenic) lie along the staircase line and exhibit intermediate properties.
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✔ Final Answer Summary:
1. Bottom left (Group 1)
2. Top right (Group 17)
3. Decreases – due to increasing nuclear charge
4. Increases – due to addition of electron shells
5. Larger
6. Smaller
7. Increases – increasing nuclear charge
8. Decreases – increasing shielding and distance
9. Fluorine
10. Francium
11. Alkali metals
12. Alkaline earth metals
13. Transition metals
14. Metals → Nonmetals
15. Halogens
16. Fluorine
17. Noble gases
18. d-sublevels
19. Valence electrons
20. Electron shells
21. Transition metal
22. More metallic
23. Metals
24. Atomic number
25. Metalloid
Let me know if you'd like this formatted as a printable PDF or need help understanding any concept further!
Parent Tip: Review the logic above to help your child master the concept of periodic table worksheet instructional fair.
