SCH3U - Chemical Trends - Atomic Properties

Which of the following best describes the trend in atomic radius across a period in the periodic table?

• It increases

• It decreases

• It remains constant

• It fluctuates randomly

What is the main reason atomic radius increases down a group?

• Increase in effective nuclear charge

• Addition of inner shell electrons

• Decrease in ionization energy

• Increase in electronegativity

Which of the following elements has the largest atomic radius?

• Oxygen

• Fluorine

• Sodium

• Neon

What does effective nuclear charge (Zeff) represent?

• Total number of electrons in an atom

• Attraction between protons and neutrons

• Net attraction between the nucleus and valence electrons

• Atomic mass of an atom

Which element experiences the highest effective nuclear charge?

• Helium

• Lithium

• Fluorine

• Neon

Which element has the highest first ionization energy?

• Hydrogen

• Lithium

• Helium

• Fluorine

Ionization energy is defined as:

• Energy released when an atom gains an electron

• Energy needed to remove an electron from a gaseous atom

• Energy required to split a compound

• Energy emitted during radioactive decay

Why does ionization energy generally increase across a period?

• More electron shells

• Decrease in nuclear charge

• Increase in effective nuclear charge

• Electrons are further from the nucleus

What is electronegativity?

• The energy to remove an electron

• The ability of an atom to attract electrons in a bond

• The size of an atom

• The number of valence electrons

According to the Pauling scale, which element is the most electronegative?

• Chlorine

• Oxygen

• Fluorine

• Nitrogen