Year 11 Chemistry

Investigating the foundational ideas of atomic theory and the experimental evidence that led to early models.

Examining the experimental evidence that led to the discovery of the atomic nucleus and its implications.

Tracing the history of atomic theory from Dalton to the quantum mechanical model, focusing on the Bohr model.

Introducing the modern quantum mechanical model, electron clouds, and the concept of atomic orbitals.

Learning to write electron configurations and draw orbital diagrams for various elements.

Understanding the structure of the periodic table and the significance of s, p, d, and f blocks.

Investigating how the arrangement of electrons determines the physical and chemical properties of elements.

Exploring the periodic trends of electronegativity and electron affinity and their chemical implications.

Classifying elements based on their properties and position on the periodic table.

Exploring the fundamental reasons why atoms form chemical bonds and the role of valence electrons.

the electrostatic forces of attraction between oppositely charged ions (cations and anions) in an ionic lattice structure.

Relating the strong electrostatic forces in ionic bonds to the characteristic properties of ionic compounds.

Exploring the 'sea of electrons' model and how it explains the unique properties of metals.

Exploring how electron sharing leads to the formation of molecules and complex network solids.

Applying VSEPR theory to predict the three-dimensional shapes of molecules and polyatomic ions.

Analyzing how differences in electronegativity lead to polar bonds and how molecular geometry determines overall molecular polarity.

Investigating the structure and properties of covalent network solids like diamond and silicon dioxide.

Defining chemical reactions, identifying reactants and products, and recognizing evidence of chemical change.

Applying the law of conservation of mass to balance chemical equations.

Classifying chemical reactions into common categories: synthesis, decomposition, single displacement, double displacement, and combustion.

Introducing the mole as a bridge between the atomic scale and the laboratory scale.

Performing calculations to convert between moles, mass, and number of particles.

Determining the simplest whole-number ratio of atoms in a compound and its actual molecular formula.

Using balanced equations to predict the mass and volume of products formed in a reaction, starting with mole-mole ratios.

Performing mass-to-mass calculations using balanced chemical equations and molar masses.

Identifying limiting reactants, calculating theoretical yield, and determining percent yield in chemical reactions.

Defining solutions, identifying their components, and understanding the nature of the dissolution process.

Examining the interaction between solute and solvent particles during the formation of a solution.

Investigating how temperature, pressure, and surface area influence the solubility of solids, liquids, and gases.

Distinguishing between different types of solutions based on their solute concentration relative to solubility limits.

Calculating the amount of solute in a given volume of solution using molarity.

Calculating solution concentrations using percent by mass and percent by volume.

Performing calculations to dilute concentrated solutions to desired concentrations.

Applying stoichiometric principles to reactions involving solutions, using molarity.

Defining energy, heat, and temperature and their relationship in chemical systems.

Distinguishing between exothermic and endothermic reactions through temperature changes and enthalpy diagrams.

Introducing enthalpy as a measure of heat content and calculating enthalpy changes for reactions.

Understanding how calorimetry is used to measure heat changes and applying specific heat capacity calculations.

Defining and applying standard enthalpy of formation to calculate reaction enthalpies.

Applying Hess's Law to calculate enthalpy changes for reactions that cannot be measured directly.

Interpreting energy profile diagrams to understand activation energy and reaction pathways.

Defining organic chemistry, the unique properties of carbon, and the diversity of organic compounds.

Exploring the structure, nomenclature, and properties of saturated hydrocarbons (alkanes).

Investigating the structure, nomenclature, and properties of unsaturated hydrocarbons (alkenes and alkynes).

Introducing the unique structure and stability of aromatic compounds, focusing on benzene.

Exploring the structure, nomenclature, and properties of compounds containing hydroxyl and halogen functional groups.

Investigating the structure, nomenclature, and properties of carbonyl compounds (aldehydes and ketones).

Exploring the structure, nomenclature, and properties of carboxylic acids and their derivatives, esters.

Understanding different types of isomerism, including structural, geometric, and optical isomers.

Defining reversible reactions and the concept of dynamic equilibrium in chemical systems.

Applying Le Chatelier's Principle to predict the shift in equilibrium due to changes in reactant or product concentration.

Investigating the effects of temperature and pressure changes on the position of chemical equilibrium.

Defining the equilibrium constant (Kc) and writing equilibrium expressions for homogeneous and heterogeneous reactions.

Performing calculations to determine equilibrium concentrations or the value of Kc.

Using the reaction quotient (Qc) to predict the direction a system will shift to reach equilibrium.

Introducing the pH and pOH scales as measures of acidity and alkalinity in aqueous solutions.

Defining oxidation and reduction in terms of electron transfer and changes in oxidation states.

Learning to balance redox reactions using the half-reaction method in acidic and basic solutions.

Exploring the components and operation of galvanic (voltaic) cells, which generate electricity from spontaneous redox reactions.

Understanding standard electrode potentials and their use in predicting the spontaneity of redox reactions.