Structure 2.1 The ionic model
Structure 2.1.1
Understandings:
Understandings:
- When metal atoms lose electrons, they form positive ions called cations. When non-metal atoms gain electrons, they form negative ions called anions.
- Predict the charge of an ion from the electron configuration of the atom.
- The formation of ions with different charges from a transition element should be included.
- Structure 3.1 How does the position of an element in the periodic table relate to the charge of its ion(s)
- Structure 1.3 (HL) How does the trend in successive ionisation energies of transition elements explain their variable oxidation states?
Structure 2.1.2
Understandings:
Understandings:
- 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”.
- Deduce the formula and name of an ionic compound from its component ions, including polyatomic ions.
- Interconvert names and formulas of binary ionic compounds.
- The following polyatomic ions should be known by name and formula: ammonium, hydroxide, nitrate, hydrogencarbonate, carbonate, sulfate and phosphate.
- Reactivity 3.2 Why is the formation of an ionic compound from its elements a redox reaction?
- HL Structure 2.2 How is formal charge used to predict the preferred structure of sulfate?
- HL 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?
Structure 2.1.3
Understandings:
Understandings:
- Ionic compounds exist as three-dimensional lattice structures, represented by empirical formulas.
- Explain the physical properties of ionic compounds to include volatility, electrical conductivity and solubility.
- Include lattice enthalpy as a measure of the strength of the ionic bond in different compounds, influenced by ion radius and charge.
- Structure 3.1 How can lattice enthalpies and the bonding continuum explain the trend in melting points of metal chlorides across period 3?
This video covers the factors that affect lattice enthalpy.
Factors that affect lattice enthalpy
Factors that affect lattice enthalpy
- There are two factors that affect the value of the lattice enthalpy, the charge on the ions and the ionic radius of the ions.
- Ions with a higher charge have a stronger force of attraction, therefore a higher lattice enthalpy.
- Smaller ions have a stronger force of attraction, therefore a higher lattice enthalpy.