1. Access to HE Diploma Pharmacy and Biomedical Science
Introduction to Matter
Lesson 6

2. Hand in homework
Moles, Formulae and Equations workbook.

3. Assessment Criteria 1.1 Define an element giving examples.
1.2 Write the names and symbols of the first 20 elements.
1.3 Describe and explain what some of the general physical properties of metals and non-metals are
1.4 Describe the relative position of metals, non-metals, groups and periods within the periodic table with examples.
2.1 Classify substances as elements or compounds from their names giving examples
2.2 Describe two differences between a compound and a mixture
3.1 Describe protons, neutrons and electrons in terms of their relative charges and relative masses.
3.2 Describe the distribution of mass and charge within an atom.
3.3 Describe the contribution of protons and neutrons to atomic nuclei in terms of atomic number and mass number.
3.4 Deduce the electronic configurations of atoms up to z = 36 and ions, given the atomic number and charge, limited to s and p blocks up to Z= 36.
4.1 Describe ionic bonding as the electrostatic attraction between two oppositely charged ions including dot and cross diagrams.
4.2 Describe a covalent bond as a pair of electrons shared between two atoms
4.3 Write the formulae for some simple and some complex compounds
4.4 Describe and interpret and/or predict physical properties in terms of the types motion and arrangement of particles (atoms, molecules and ions) and the forces between them, and the different types of bonding.
5.1 Describe an acid as a species that can donate a proton.
5.2 Describe a base as a species that can accept a proton
5.3 Describe the reaction of an acid typified by hydrochloric acid with metals, carbonates bases and alkalis and interpret them using ionic equations to emphasise the role of H+(aq)
5.4 Write a balanced equation for the reaction between two elements and between an acid and a base
6.1 Construct balanced chemical equations, full and ionic

4. Review Activity
acid + metal carbonate →

5. Review Activity
Write a balanced equation for the reaction between two elements Write a balanced equation for the reaction between an acid and a base

6. Today’s Aim
Understand that chemical reactions can be represented by chemical equations

7. Week 6
6.1 Construct balanced chemical equations, full and ionic

8. Week 6 Reading Access to Chemistry
Alan Jones, Mike Clement, Avril Higton Elaine Goulding
ISBN
Inside the atom
Pages

9. What happens when you put
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
What happens when you put
AgNO3 and NaCl in water?

10. What really happens when you put
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
What really happens when you put
AgNO3 and NaCl in water?

11. NaCl (aq) Na +1 (aq) + Cl -1 (aq) KEY POINT: really means:
“dissociated ions” or
“ions in solution”

12. What is Dissolving ?
When an ionic compound (eg salt) dissolves in water, the compound disassociates. (breaks apart into cations and anions)
Ex: Ca(NO3)2(s) Ca2+(aq) + 2NO3-(aq)
When a covalent compound (eg sugar) dissolves in water, the molecules simply disperse; they do not disassociate. Molecules of the covalent compounds simply disperse due to attraction with polar water molecules.

13. An Ionic Compound Dissolves: A Covalent Compound Dissolves:

14. Mg(NO3)2 (aq) Mg +2 (aq) + (NO3) -1 (aq) 2 KEY POINT: really means:
“dissociated ions” or
“ions in solution”

15. KEY POINT:
AgCl (s)
really means:
Solid Silver (I) Chloride.

16. What happens when you put
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
What happens when you put
AgNO3 and NaCl in water?

17. AgNO3
NaCl

18. NO3-
Na+
Ag+
Cl-

19. Na+
NO3-
Ag+
Cl-

20. Na+
NO3-
AgCl

21. Na+
NO3-
AgCl(s)
precipitate
AgCl

22. AgCl(s) NO3- Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3-

23. AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
complete ionic equation

24. Na+
NO3-
AgCl
Reaction

25. No Reaction
Na+
NO3-
AgCl

26. These ions do not participate in the reaction. They are called
SPECTATOR IONS
Na+
NO3-
AgCl

27. The net ionic equation is constructed from the complete ionic equation:

28. NO3- and Na+ are not participating in the reaction

29. net ionic equation

30. net ionic equation

31. describes double replacement reaction
Complete molecular equation-
describes double replacement reaction
Complete ionic equation-
more accurately shows the reacting species as ions and the products either as ions or a precipitate
Net ionic equation-
focuses only on the ions REACTING
Spectator ions are those ions that do NOT participate in the reaction

32. PREDICTING THE FORMATION OF A PRECIPITATE
Consider the possibility that a precipitate may form.
Must use the solubility table.
Possible outcomes
No visible reaction (nvr)
Formation of one ppt.
Formation of two ppt. (rare occurrence)

33. Basic Chemical equation AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)
Complete ionic equation shows ions in solution Ag+ (aq) + NO3(aq) + K+ (aq) + Cl-(aq)  AgCl(s) + K+ (aq) + NO3- (aq)
Net ionic equation shows ions in rxn Ag+ (aq) + Cl-(aq)  AgCl(s)
(leave out spectator ions)
link

34. Review Week 6
6.1 Construct balanced chemical equations, full and ionic

35. Workbook
Complete section

36. Next Week
Exam