Presentation on theme: "WITHOUT using the text book give me your definition (word and picture) of these; 1.Oxidation 2.Reduction 3.Oxidation agent 4.Reducing agent."— Presentation transcript:
WITHOUT using the text book give me your definition (word and picture) of these; 1.Oxidation 2.Reduction 3.Oxidation agent 4.Reducing agent
Different explanations of oxidation/reduction; Reducing agents give away e- (e- donors) Oxidising agents accept e- (are reduced) Use different models to fit situation ModelReductionOxidation OxygenLoss of oxygenGain of oxygen HydrogenGain of hydrogenLoss of hydrogen ElectronGain of e-Loss of e- Oxidation State (numbers)DecreasesIncreases Well explore this today
Atoms and Ions Ions in solution Halogens Manufacturing Dipoles Bonding Halogenoalkanes Elements of the sea Ionic Formulae Redox
Why certain compounds are formed? How the periodic table is arranged? What are the differences between solid and liquid solutions for ionic compounds? How can we predict compounds being formed?
Ionic Formulae Generally - Metals are positive (ca+ions), lose e- Non-metals are negative (anions), gain e- (when non-metal becomes an ion – name from chlorine to chloride If O contained as well as another non- metal ate indicates presence of O Overall neutral (charges balance out) Complete ES2.1 and make some other rules for ionic formulae rules
CI 9.1 Oxidation states (numbers) Occur in both ionic and covalent compounds Total of a compound MUST be 0 (neutral) Elements (Mg, or O 2 ) are 0 Fl always -1 Cl usually -1 (Cl changes if with F or O) O usually -2 (unless with Fl or H) H +1 with non metals or -1 in metals
Oxidation States (numbers) Other metals usually follow ionic charge (i.e. Gp1 always +1, Gp 2 always +2, Al 3+) Some transition metals can vary – shown by (roman numerals) in-between i.e. Fe(II)O or Fe 2 (III)O 3.
ES 2.2 Be OBSERVANT – skill which is usually tested in your year 12 practical examination Write this experiment up – adding in things to be aware of. Answer questions
Work out the individual oxidation states 1.NaOH 2.HNO 3 3.CuSO 4 4.OF 2 5.H 2 O 6.H 2 O 2
Can we answer our key questions? 1.Why certain compounds are formed? 2.How the periodic table is arranged? 3.What are the differences between solid and liquid solutions for ionic compounds? 4.How can we predict compounds being formed?
Can we answer our key questions? 1.ES 2.2 write up 2.Complete CS assignment 3 Extension Read ahead CI9.1