If chemistry workbook ch099 a | PDF - Free Printable
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Step-by-step solution for: If chemistry workbook ch099 a | PDF
It looks like you've uploaded a Periodic Table Worksheet with 25 questions related to the periodic table, but the image itself isn't visible here. However, I can help you solve and explain each of these questions based on standard chemistry knowledge.
Here is a complete solution and explanation for each question:
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1. Where are the most active metals located?
✔ Answer: On the left side of the periodic table (especially Group 1 and Group 2).
🔍 Explanation: The most active metals are the alkali metals (Group 1) and alkaline earth metals (Group 2). They lose electrons easily due to low ionization energy.
2. Where are the most active nonmetals located?
✔ Answer: On the right side of the periodic table (especially Group 17 – halogens).
🔍 Explanation: Halogens (like fluorine and chlorine) are highly reactive because they need just one electron to complete their outer shell.
3. As you go from left to right across a period, the atomic size (decreases / increases). Why?
✔ Answer: Decreases
🔍 Explanation: As you move left to right across a period, the number of protons (nuclear charge) increases, pulling electrons closer to the nucleus. This reduces atomic radius.
4. As you travel down a group, the atomic size (decreases / increases). Why?
✔ Answer: Increases
🔍 Explanation: Moving down a group adds more electron shells (energy levels), increasing the distance between the nucleus and outermost electrons.
5. A negative ion is (larger / smaller) than its parent atom. Why?
✔ Answer: Larger
🔍 Explanation: A negative ion (anion) forms when an atom gains electrons. The added electrons increase electron-electron repulsion, causing the electron cloud to expand.
6. A positive ion is (larger / smaller) than its parent atom. Why?
✔ Answer: Smaller
🔍 Explanation: A positive ion (cation) forms when an atom loses electrons. With fewer electrons, the remaining electrons are pulled closer by the nucleus, reducing size.
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 across a period makes it harder to remove an electron, so more energy is needed.
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 and are shielded by inner electrons, making them easier to remove.
9. Where is the highest electronegativity found?
✔ Answer: In the top right corner (fluorine).
🔍 Explanation: Fluorine has the highest electronegativity because it strongly attracts bonding electrons due to high effective nuclear charge and small atomic size.
10. Where is the lowest electronegativity found?
✔ Answer: In the bottom left corner (cesium or francium).
🔍 Explanation: These metals have very low electronegativity because they tend to lose electrons rather than attract them.
11. Elements of Group 1 are called
✔ Answer: Alkali metals
🔍 Explanation: Group 1 includes lithium, sodium, potassium, etc., known for being highly reactive metals.
12. Elements of Group 2 are called
✔ Answer: Alkaline earth metals
🔍 Explanation: Includes magnesium, calcium, etc., slightly less reactive than alkali metals.
13. Elements of Group 17 are called
✔ Answer: Halogens
🔍 Explanation: Highly reactive nonmetals that form salts (e.g., chlorine, bromine).
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: Left side = metals; right side = nonmetals; middle = metalloids.
15. Group 17 elements are called
✔ Answer: Halogens (same as #13)
16. The most reactive element is
✔ Answer: Francium (Fr) — though often considered Cesium (Cs) due to Francium's radioactivity.
🔍 Explanation: Alkali metals become more reactive down the group due to decreasing ionization energy.
17. Group 18 elements are called
✔ Answer: Noble gases
🔍 Explanation: Very stable and unreactive due to full valence shells.
18. What sublevels are filling across the transition elements?
✔ Answer: d-sublevels
🔍 Explanation: Transition metals fill the (n-1)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 outer-shell electrons, leading to similar chemical properties.
20. Elements across a series have the same number of ___
✔ Answer: Energy levels (electron shells)
🔍 Explanation: All elements in a period have the same principal energy level (e.g., Period 3 has n=3).
21. A colored ion generally indicates a ___
✔ Answer: Transition metal
🔍 Explanation: Transition metals form colored ions due to d-d electron transitions.
22. As you go down a group, the elements generally become (more / less) metallic.
✔ Answer: More metallic
🔍 Explanation: Down a group, atoms lose electrons more easily, increasing metallic character.
23. The majority of elements in the periodic table are (metals / nonmetals).
✔ Answer: Metals
🔍 Explanation: About 80% of 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: Examples: silicon, germanium, arsenic. They lie along the zigzag line between metals and nonmetals.
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Let me know if you'd like this formatted as a printable PDF, or if you want diagrams or visual aids!
Here is a complete solution and explanation for each question:
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PERIODIC TABLE WORKSHEET – Answers & Explanations
1. Where are the most active metals located?
✔ Answer: On the left side of the periodic table (especially Group 1 and Group 2).
🔍 Explanation: The most active metals are the alkali metals (Group 1) and alkaline earth metals (Group 2). They lose electrons easily due to low ionization energy.
2. Where are the most active nonmetals located?
✔ Answer: On the right side of the periodic table (especially Group 17 – halogens).
🔍 Explanation: Halogens (like fluorine and chlorine) are highly reactive because they need just one electron to complete their outer shell.
3. As you go from left to right across a period, the atomic size (decreases / increases). Why?
✔ Answer: Decreases
🔍 Explanation: As you move left to right across a period, the number of protons (nuclear charge) increases, pulling electrons closer to the nucleus. This reduces atomic radius.
4. As you travel down a group, the atomic size (decreases / increases). Why?
✔ Answer: Increases
🔍 Explanation: Moving down a group adds more electron shells (energy levels), increasing the distance between the nucleus and outermost electrons.
5. A negative ion is (larger / smaller) than its parent atom. Why?
✔ Answer: Larger
🔍 Explanation: A negative ion (anion) forms when an atom gains electrons. The added electrons increase electron-electron repulsion, causing the electron cloud to expand.
6. A positive ion is (larger / smaller) than its parent atom. Why?
✔ Answer: Smaller
🔍 Explanation: A positive ion (cation) forms when an atom loses electrons. With fewer electrons, the remaining electrons are pulled closer by the nucleus, reducing size.
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 across a period makes it harder to remove an electron, so more energy is needed.
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 and are shielded by inner electrons, making them easier to remove.
9. Where is the highest electronegativity found?
✔ Answer: In the top right corner (fluorine).
🔍 Explanation: Fluorine has the highest electronegativity because it strongly attracts bonding electrons due to high effective nuclear charge and small atomic size.
10. Where is the lowest electronegativity found?
✔ Answer: In the bottom left corner (cesium or francium).
🔍 Explanation: These metals have very low electronegativity because they tend to lose electrons rather than attract them.
11. Elements of Group 1 are called
✔ Answer: Alkali metals
🔍 Explanation: Group 1 includes lithium, sodium, potassium, etc., known for being highly reactive metals.
12. Elements of Group 2 are called
✔ Answer: Alkaline earth metals
🔍 Explanation: Includes magnesium, calcium, etc., slightly less reactive than alkali metals.
13. Elements of Group 17 are called
✔ Answer: Halogens
🔍 Explanation: Highly reactive nonmetals that form salts (e.g., chlorine, bromine).
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: Left side = metals; right side = nonmetals; middle = metalloids.
15. Group 17 elements are called
✔ Answer: Halogens (same as #13)
16. The most reactive element is
✔ Answer: Francium (Fr) — though often considered Cesium (Cs) due to Francium's radioactivity.
🔍 Explanation: Alkali metals become more reactive down the group due to decreasing ionization energy.
17. Group 18 elements are called
✔ Answer: Noble gases
🔍 Explanation: Very stable and unreactive due to full valence shells.
18. What sublevels are filling across the transition elements?
✔ Answer: d-sublevels
🔍 Explanation: Transition metals fill the (n-1)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 outer-shell electrons, leading to similar chemical properties.
20. Elements across a series have the same number of ___
✔ Answer: Energy levels (electron shells)
🔍 Explanation: All elements in a period have the same principal energy level (e.g., Period 3 has n=3).
21. A colored ion generally indicates a ___
✔ Answer: Transition metal
🔍 Explanation: Transition metals form colored ions due to d-d electron transitions.
22. As you go down a group, the elements generally become (more / less) metallic.
✔ Answer: More metallic
🔍 Explanation: Down a group, atoms lose electrons more easily, increasing metallic character.
23. The majority of elements in the periodic table are (metals / nonmetals).
✔ Answer: Metals
🔍 Explanation: About 80% of 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: Examples: silicon, germanium, arsenic. They lie along the zigzag line between metals and nonmetals.
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Let me know if you'd like this formatted as a printable PDF, or if you want diagrams or visual aids!
Parent Tip: Review the logic above to help your child master the concept of periodic table worksheet instructional fair.
