Work through the list without notes. If you cannot do a statement, follow its link, then come back. Guide = study guide; Practice = practice questions.
Understanding
- I can define electronegativity and say how it differs from electron affinity. (Guide: “Electronegativity and its trends” and “Common misconceptions”)
- I can explain why electronegativity increases across a period and decreases down a group, using shielding, distance and Coulomb’s law. (Guide; Practice Q5)
- I can explain why C–H bonds are treated as nonpolar even though carbon is slightly more electronegative. (Guide: “Nonpolar covalent bonds”)
- I can describe metallic bonding as cations surrounded by delocalized valence electrons. (Guide: Figure 2; Practice Q3)
- I can explain why ionic and covalent bonding form a continuum, and why every polar bond has some ionic character. (Guide: Figure 1; Practice Q7)
Skills
- I can put δ+ and δ− on the correct atoms of a polar bond, including unusual cases such as O–F. (Practice Q2)
- I can rank single bonds by bond dipole from electronegativity values or from periodic-table position. (Guide: Worked example 1; Practice Q1, Q5)
- I can classify a bond as nonpolar covalent, polar covalent, ionic or metallic. (Guide: Worked example 3; Practice Q4)
- I can use the metal/nonmetal rule of thumb alongside the electronegativity difference. (Guide: “Ionic bonds: more than a number”)
Reasoning
- I can make a claim about the bonding in an unknown solid from its melting point, conductivity and response to hammering, and justify it. (Guide: Worked example 2; Practice Q6)
- I can explain why a fixed cut-off value of electronegativity difference cannot decide bond type. (Practice Q7)
- I can explain at the particle level why a metal conducts electricity as a solid. (Practice Q6(c))
All ticked? Move on to Topic 2.2, Intramolecular Force and Potential Energy, or return to the course roadmap.