Introduction to Matter

Access to HE DiplomaPharmacy and Biomedical Science

Introduction to Matter

Lesson 6Hand in homeworkMoles, Formulae and Equations workbook.

Assessment Criteria1.1 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 are1.4 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 examples2.2 Describe two differences between a compound and a mixture3.1 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 atoms4.3 Write the formulae for some simple and some complex compounds4.4 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 proton5.3 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 base6.1 Construct balanced chemical equations, full and ionic

Review Activityacid + metal carbonate Review ActivityWrite a balanced equation for the reaction between two elements

Write a balanced equation for the reaction between an acid and a baseTodays AimUnderstand that chemical reactions can be represented by chemical equationsWeek 66.1 Construct balanced chemical equations, full and ionic

Week 6 ReadingAccess to ChemistryAlan Jones, Mike Clement, Avril Higton Elaine GouldingISBN 0 -85404-564-3

Inside the atomPages 83 - 118

AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)What happens when you putAgNO3 and NaCl in water?AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)What really happens when you putAgNO3 and NaCl in water?KEY POINT:

NaCl (aq)

really means:

Na +1 (aq) + Cl -1 (aq) dissociated ionsor ions in solutionWhat 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.An Ionic Compound Dissolves:

A Covalent Compound Dissolves:KEY POINT:

Mg(NO3)2 (aq)

really means:

Mg +2 (aq) + (NO3) -1 (aq) 2dissociated ionsor ions in solutionKEY POINT:

AgCl (s)

really means:

AgCl (s)Solid Silver (I) Chloride.AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)What happens when you putAgNO3 and NaCl in water?AgNO3NaClAg+NO3-Na+Cl-Ag+NO3-Na+Cl-AgClNO3-Na+AgClNO3-Na+AgCl(s)precipitateNO3-Na+NO3-Na+NO3-Na+NO3-Na+Na+NO3-Na+NO3-Na+NO3-Na+NO3-Na+AgCl(s)

AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)complete ionic equationNO3-Na+AgClReactionAgClNO3-Na+No ReactionAgClNO3-Na+These ions do not participatein the reaction. They are calledSPECTATOR IONS

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

NO3- and Na+ are not participating in the reaction

net ionic equation

net ionic equation

Complete molecular equation-describes double replacement reactionComplete ionic equation-more accurately shows the reacting species as ions and the products either as ions or a precipitateNet ionic equation-focuses only on the ions REACTINGSpectator ions are those ions that do NOT participate in the reactionPREDICTING THE FORMATION OF A PRECIPITATEConsider the possibility that a precipitate may form.Must use the solubility table.Possible outcomesNo visible reaction (nvr)Formation of one ppt.Formation of two ppt. (rare occurrence)

32Basic 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)linkReview Week 66.1 Construct balanced chemical equations, full and ionic

WorkbookComplete section35Next Week

ExamAg+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + NO3- (aq) + Na+ (aq)Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + NO3- (aq) + Na+ (aq)Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + NO3- (aq) + Na+ (aq)Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + NO3- (aq) + Na+ (aq)Ag+ (aq) + Cl- (aq) AgCl (s)Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + NO3- (aq) + Na+ (aq)Ag+ (aq) + Cl- (aq) AgCl (s)