Question 1:

Which of the following periodic trends refers to the ability of an atom to attract electrons in a chemical bond?

Explanation: The correct answer is A) Electronegativity. Electronegativity is a periodic trend that describes an atom's ability to attract electrons towards itself in a chemical bond. It increases from left to right across a period and decreases from top to bottom within a group in the periodic table.

Question 2:

Which of the following periodic trends represents the energy required to remove an electron from an atom?

Explanation: The correct answer is B) Ionization Energy. Ionization energy is the energy required to remove an electron from an atom, resulting in the formation of a positive ion. It generally increases from left to right across a period and decreases from top to bottom within a group in the periodic table.

Question 3:

Which of the following periodic trends describes the size of an atom?

Explanation: The correct answer is C) Atomic Radius. Atomic radius refers to the size of an atom. It is a periodic trend that generally decreases from left to right across a period and increases from top to bottom within a group in the periodic table.

Question 4:

Which of the following elements is expected to have the highest electronegativity?

Explanation: The correct answer is B) Chlorine (Cl). Chlorine is expected to have the highest electronegativity among the given elements. Electronegativity generally increases from left to right across a period, and chlorine, being closer to the right side of the periodic table, has a higher electronegativity than sodium and potassium.

Question 5:

Which of the following elements is expected to have the largest atomic radius?

Explanation: The correct answer is C) Helium (He). Helium is expected to have the largest atomic radius among the given elements. Atomic radius generally increases from top to bottom within a group, and helium, being located at the top of Group 18 (noble gases), has a larger atomic radius than oxygen and fluorine.