S2.1 The Ionic Model

• When metal atoms lose electrons, they form positive ions called cations. When non-metal atoms gain electrons, they form negative ions called anions.

• The ionic bond is formed by electrostatic attractions between oppositely charged ions.

• Binary ionic compounds are named with the cation first, followed by the anion. The anion adopts the suffix “ide”.

• Ionic compounds exist as three-dimensional lattie structures, represented by empirical formulas

Structure 3.1—How does the position of an element in the periodic table relate to the charge of its ion(s)?

AHL Structure 1.3—How does the trend in successive ionization energies of transition elements explain their variable oxidation states?

Reactivity 3.2—Why is the formation of an ionic compound from its elements a redox reaction?

AHL Structure 2.2—How is formal charge used to predict the preferred structure of sulfate?

AHL Reactivity 3.1—Polyatomic anions are conjugate bases of common acids. What is the relationship between their stability and the conjugate acid’s dissociation constant, Ka?

Tool 1, Inquiry 2—What experimental data demonstrate the physical properties of ionic compounds?

Structure 3.1—How can lattice enthalpies and the bonding continuum explain the trend in melting points of metal chlorides across period 3?