Question 1: Which element has the highest electronegativity in the periodic table?

Answer: Fluorine

Question 2: What is the trend in atomic radius as you move down Group 1?

Answer: It increases

Question 3: What happens to ionization energy as you move across a period from left to right?

Answer: It increases

Question 4: True or False: Noble gases have the highest electron affinity.

Answer: False

Question 5: True or False: Alkali metals become more reactive as you move down the group.

Answer: True

Question 6: Explain why the atomic radius decreases across a period.

Answer: The atomic radius decreases due to increased nuclear charge attracting the electrons more strongly.

Question 7: Describe the trend in metallic character as you move across a period.

Answer: Metallic character decreases as you move across a period due to increased nuclear charge and electron affinity.

Question 8: Why do halogens have high electron affinities?

Answer: Halogens have high electron affinities because they are one electron short of a full outer shell.

Question 9: Calculate the first ionization energy given the following data: Use the formula E = hν - φ, where h is Planck's constant, ν is the frequency, and φ is the work function.

Answer: Calculation based on provided data

Question 10: Match the following elements with their correct group in the periodic table:

Answer: See full answer key

Question 11: Order the following elements by increasing atomic number: Oxygen, Carbon, Neon, Helium.

Answer: See full answer key

Question 12: Fill in the blank: The element with the highest ionization energy in the second period is ______.

Answer: Neon

Question 13: Discuss the factors affecting ionization energy and how they vary across a period and down a group.

Answer: Detailed discussion on nuclear charge, electron shielding, and their effect on ionization energy trends across periods and groups.