Periodic Trends

What is a "trend" in the context of the periodic table?

• A repeating pattern of properties.

• A random distribution of elements.

• The physical state of an element.

• The atomic mass of an element.

What happens to the atomic radius as you move down a group in the periodic table?

• It decreases due to increased nuclear charge.

• It increases due to the addition of more electron shells.

• It remains constant.

• It fluctuates unpredictably.

Why does the atomic radius generally decrease as you move from left to right across a period in the periodic table?

• The number of electron shells increases.

• The nuclear charge increases, pulling electrons closer to the nucleus.

• The number of valence electrons decreases.

• Shielding effect becomes more prominent.

What is the relationship between an atom's size and its ionization energy?

• Larger atoms have higher ionization energy.

• Smaller atoms have lower ionization energy.

• Smaller atoms have higher ionization energy.

• Atomic size has no effect on ionization energy.

How does ionization energy generally change as you move from left to right across a period in the periodic table?

• It decreases.

• It increases.

• It remains constant.

• It first decreases then increases.

What happens to the ionization energy of elements as you move down a group in the periodic table?

• It increases.

• It decreases.

• It remains constant.

• It first increases then decreases.

What does electronegativity measure?

• The energy required to remove an electron from an atom.

• The size of an atom's nucleus.

• An atom's attraction to electrons.

• The number of valence electrons in an atom.

Which statement accurately describes the trend of electronegativity across a period in the periodic table?

• Electronegativity decreases from left to right.

• Electronegativity increases from left to right.

• Electronegativity remains constant from left to right.

• Electronegativity first increases then decreases from left to right.