Question

question 33 (1 point)
compared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be
o a higher
o b lower
o c unpredictable
o d the same

question 34 (1 point)
as you move from left to right across the second period of the periodic table
o a ionization energy increases.
o b electronegativity decreases.
o c atomic mass decreases.
o d atomic radii increase.

question 35 (1 point)
of the following elements, which one has the smallest first ionization energy?
o a boron
o b silicon
o c aluminum
o d carbon

Explanation:

• Question 33:
• In a period of the periodic table, as we move from left to right, the nuclear charge increases while the number of electron shells remains the same. This leads to a greater attraction for electrons, so electronegativity increases.
• Question 34:
• When moving from left to right across a period (e.g., the second period), the nuclear charge increases. This stronger nuclear - electron attraction makes it more difficult to remove an electron, so ionization energy increases.
• Question 35:
• Ionization energy generally increases across a period and decreases down a group. Boron (\(B\)), carbon (\(C\)) are in the second period (\(B\) is to the left of \(C\)), and aluminum (\(Al\)) and silicon (\(Si\)) are in the third period. Aluminum has a lower ionization energy than silicon (across - period trend). Also, aluminum has a lower ionization energy than boron (down - group trend as \(Al\) is below \(B\) in the group of boron family).

Answer:

• Question 33: a. higher
• Question 34: a. ionization energy increases.
• Question 35: c. aluminum