Understanding Periodic Trends: Atomic Radius and Reactivity
This worksheet guides you through key periodic trends, including atomic radius, ionization energy, and electronegativity, enhancing your analytical and problem-solving skills.
1. What is the general trend for atomic radius across a period in the periodic table? (1 choice)
2. Which of the following factors affect the atomic radius of an element? (Select all that apply) (multiple choice)
3. Define ionization energy and explain why it generally increases across a period.
4. List the periodic trends that typically increase from left to right across a period.
Electronegativity
Ionization energy
Electron affinity
5. Which element is likely to have the highest electronegativity? (1 choice)
6. Predict which element would have a larger atomic radius: Sodium (Na) or Potassium (K)? Explain your reasoning. (multiple choice)
7. Given the elements Oxygen (O), Sulfur (S), and Selenium (Se), arrange them in order of increasing electronegativity and justify your arrangement.
8. Analyze the following statement: "The reactivity of nonmetals increases across a period." Which factors contribute to this trend? (Select all that apply) (multiple choice)
9. Compare and contrast the trends in electron affinity and ionization energy across a period. Provide examples to support your analysis.
10. Evaluate the following elements: Fluorine (F), Chlorine (Cl), and Bromine (Br). Which element would you expect to have the highest reactivity and why? (Select all that apply) (multiple choice)
11. Design an experiment to demonstrate the trend in metallic character across a period. Describe the materials, procedure, and expected results.
12. Based on periodic trends, which element would you predict to be the most reactive metal? (1 choice)
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