🔬 Part 1: Periodic Trends

1. As you move from left to right across a period, atomic radius:

increases

decreases

stays the same

varies randomly

2. Which element would have the largest atomic radius?

Lithium (Li)

Sodium (Na)

Potassium (K)

Rubidium (Rb)

3. Ionization energy generally increases as you move:

down a group and left across a period

up a group and right across a period

down a group and right across a period

up a group and left across a period

4. Which properties generally increase from left to right across Period 3? (Check all that apply)

Atomic number

Atomic radius

Electronegativity

Number of electron shells

📊 Part 2: Predicting Properties

5. Based on periodic trends, predict which element in each pair would have the higher electronegativity:

a) Oxygen vs. Sulfur: _______________

b) Fluorine vs. Chlorine: _______________

c) Carbon vs. Silicon: _______________

6. Explain why noble gases have very high ionization energies compared to alkali metals in the same period:

7. An unknown element X is in Group 2, Period 4. Predict its properties relative to magnesium (Mg):

Atomic radius: Element X will be __________ than Mg

Ionization energy: Element X will be __________ than Mg

Metallic character: Element X will be __________ metallic than Mg

🧪 Part 3: Application

8. A scientist needs an element with high electronegativity for a chemical reaction. Based on periodic trends, which area of the periodic table should they focus on?

9. Arrange these elements in order of increasing atomic radius: Al, Cl, Na, P

Smallest → Largest: _______ → _______ → _______ → _______

10. Using your knowledge of periodic trends, explain why it becomes easier to remove an electron from atoms as you move down Group 1 (alkali metals):

Periodic Table Properties Patterns

Periodic Table Properties Patterns

🔬 Part 1: Periodic Trends

📊 Part 2: Predicting Properties

🧪 Part 3: Application

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