Big Idea 1. All matter is composed of atoms.

Section 7.1: Development of the Periodic Table

Section 7.2: Effective Nuclear Charge

o Explain the meaning of effective nuclear charge, Z_eff, and how Z_eff depends on nuclear charge and electron configuration.

Section 7.3: Sizes of Atoms and Ions

o Explain how the radius of an atom changes upon losing electrons to form a cation or gaining electrons to form an anion.

o Use the periodic table to determine the electron configurations of ions.

Section 7.4: Ionization Energy

o Predict the trends in ionization energy as successive electrons are removed, including the discontinuous increase that occurs when the ionization corresponds to removing a core electron.

Section 7.5: Electron Affinity

o Explain how electron affinity and ionization energy are related, and how irregularities in the periodic trends for electron affinity can be related to electron configuration.

Section 7.6: Metals, Nonmetals, and Metalloids

o Explain the differences in chemical and physical properties of metals and nonmetals, including the basicity of metal oxides and the acidity of non-metal oxides.

Section 7.7: Trends for Groups 1A and 2A Metals

o Explain how atomic properties, such as ionization energy and electron affinity, relate to the chemical reactivity and physical properties of the alkali and alkaline earth metals (Groups 1A and 2A).

o List and explain the unique characteristics of hydrogen.

Section 7.8: Trends for Selected Nonmetals

o Right balanced equations for the reactions of the group 1A and 2A metals with water, oxygen, hydrogen, and the halogens.

o Explain how the atomic properties, such as ionization energy and electron affinity, of group 6A, 7A, and 8A elements relate to their chemical reactivity and physical properties.

Section 7.9 Electron Configurations and the Periodic Table

o Use the periodic table to write condensed electron configurations and determine the number of unpaired electrons in an atom.