Question: 2. What is generally true of atoms with relatively large atomic radii? ○ Large atoms hold their electrons very tightly. ○ Large atoms tend to have a low ionization energy and a low electron affinity. ○ Large atoms tend to be found on the right side of their period on the periodic table. ○ Large atoms are usually found at the top of their group on the periodic table. 3. What is the most accurate statement concerning ionization energy? ○ Metals tend to have lower ionization energies than nonmetals. ○ As you move down a group on the periodic table, ionization energy tends to increase. ○ As you move across a period from left to right on the periodic table, ionization energy tends to decrease. ○ The noble gases tend to have the lowest ionization energies. 4. Which factor would be most likely to shrink the size of an atom’s electron cloud? ○ Forming a positive ion. ○ Removing a proton. ○ Adding an energy level. ○ Adding a valence electron to an existing energy level. 5. Which of the following groups is characterized by both a high ionization energy and an electron affinity that is close to zero? ○ Alkali metals (group 1) ○ Transition metals (groups 3-12) ○ Halogens (group 17) ○ Noble gases (group 18)

1. Problem: Understand the properties of atoms related to atomic radius, ionization energy, and electron affinity. 2. Atomic Radius and Related Properties: - Atoms with relatively large atomic radii tend to have electrons that are less tightly held because the outer electrons are farther from the nucleus. - Large atoms generally have low ionization energy and low electron affinity because it requires less energy to remove an electron and they are less likely to attract additional electrons. - Large atoms are usually found on the left side of their period and towards the bottom of their group on the periodic table, not on the right or top. 3. Ionization Energy Trends: - Metals tend to have lower ionization energies than nonmetals because metals lose electrons more easily. - Ionization energy decreases as you move down a group because electrons are farther from the nucleus and more shielded. - Ionization energy increases as you move from left to right across a period due to increasing nuclear charge. - Noble gases have the highest ionization energies, not the lowest, because their electron shells are full and stable. 4. Factors Affecting Atomic Size: - Forming a positive ion shrinks the electron cloud because electrons are removed, reducing electron-electron repulsion. - Removing a proton would change the element and is not a typical factor. - Adding an energy level increases size. - Adding a valence electron to an existing energy level slightly increases size. 5. Groups with High Ionization Energy and Electron Affinity Close to Zero: - Noble gases (group 18) have high ionization energies and electron affinities close to zero because their outer shells are full and stable. Final Answers: 2. Large atoms tend to have a low ionization energy and a low electron affinity. 3. Metals tend to have lower ionization energies than nonmetals. 4. Forming a positive ion. 5. Noble gases (group 18).