PART 3: Oxides and chorides of the third period (sodium  argon)

Slides:

Advertisements

Similar presentations

Periodic Trends in Chemical Properties

Advertisements

Periodic Trends in Period 3

AN INTRODUCTION TO PERIOD 3 COMPOUNDS A guide for A level students KNOCKHARDY PUBLISHING.

BONDING AND STRUCTURES

Na-Sodium Na2O- Sodium Oxide and NaCl- Sodium Chloride At standard condition- Solid Bonding and Structure: Ionic lattice Electrical Conductivity: Good.

Chapter 5 Section 2 – Ionic Bonding and Salts

Warm Up Give the formula that will result from reacting the following ions: 1.Na +, O 2- 2.Al 3+, Cl - 3.Mg 2+, N 3- 4.Al 3+, S 2- 5.Ca +, Br - 1.Na 2.

After today, you will be able to… Write formulas for ionic compounds Explain what an empirical formula is List and explain the properties of ionic bonds.

Advanced Higher Chemistry Unit 1 The oxides, chlorides and hydrides.

Third Period elements 1 R.B.Mahajan.  The trend  The diagram shows how the atomic radius changes as you go across Period 3.  The increasing number.

13.1. Period 3: Oxides and Chlorides

Periodicity HL and SL 3.1 The periodic table The periodic table is a list of all the elements in order of increasing atomic number. Elements are placed.

Types of Solids Intra V Inter. Intramolecular Type of bonding within the molecule Covalent Ionic Metallic Covalent Simple molecular solids with different.

Chemical Properties. Syllabus Statements 3.3 Chemical properties Discuss the similarities and differences in the chemical properties of elements.

PART 3: Oxides and chorides of the third period (sodium  argon)

Chapter 2: Sections 3 Ionic Bonds What is an Ion? An atom or group of atoms that has become electrically charged An atom or group of atoms that has become.

Topic 13 Periodicity HL.

Bonding Ionic Covalent (Metallic). How do atoms bond(join) together to form the millions of different compounds that make up the world? It all comes down.

Covalent bonding.

Properties of Oxides Across a Period (when added to water) basicacidic 8.6.

PART 3: Oxides and chorides of the third period (sodium  argon) adapted from Mrs. D. Dogancay.

STRUCTURES BONDING, STRUCTURE & PROPERTIES IONIC COVALENT.

CHAPTER 10: PERIODICITY.  In the periodic table elements are arranged in order of ……  The elements are in a certain group and period  Elements in a.

The Alkali Metals – Li, Na, K, Rb, Cs (Fr is unstable and scarce) -Low density largest atoms in each period with lowest mass in each period -Soft weak.

Chemical periodicity. Periodicity of period 3 elements NaMgAl Si PSCl Ar Sodium, magnesium and aluminium are metals. Silicon has some metalloid traits.

Topic 13 - Periodicity. Ionic properties High melting and boiling point Conduct electricity in molten and aqueous states Crystalline solids Soluble.

Structure and Bonding Ionic bondsCovalent bonds Metallic bonds Chemical bonding involves either transferring or sharing electrons in the highest occupied.

Topic 3.1 The periodic table 1. Assessment Statements Discuss the similarities and differences in the chemical properties of elements in the same.

13.1 REACTIONS OF PERIOD 3 ELEMENTS

Chapter 3: Periodicity Higher level. Period 3 oxides (continued) You need to be able to talk about the structure of the oxides as well as the bonding.

METALLIC AND NON-METALLIC OXIDES

STRUCTURE And bonding.

Bonding The force that holds two or more atoms together.

Aim: What properties do Ionic Compounds have?

PART 3: Oxides and chorides of the third period (sodium  argon)

Bonds NonMusical Chairs Review

Chemical Bonding Why & How Atoms Combine

Introduction to Chemical Bonding

? ? ? ? ? ? Bonding in MgO Bonding in Na2O Ionic Ionic

Chapter 3 Notes: Periodic Trends

Example diagram and detailed description of bonding in substance

Física y química 3º E.S.O. FIRST TERM UNIT 2_4: CHEMICAL SUBSTANCES.

Chemical Bonding.

Unit: Chemical Bonding

HL periodicity.

Bonding Chapters 7-8.

How Atoms Combine (7.3).

Compounds & Molecules Compounds - made of 2 or more elements

A guide for A level students KNOCKHARDY PUBLISHING

How Atoms Combine (7.3).

Chemical Bonds.

Chemical (Intramolecular) Bonding

Unit 3 Bonding & Chemical Rxns

The Structure of Matter

Bonding properties To know that there are 3 types of bonding

PART 3: Oxides and chorides of the third period (sodium  argon)

Reactions of period 3 elements with chlorine, oxygen and water

Chemical bonds and Equations 2.1 and 2.4

STRUCTURES Module C2.

5-1 Notes - Compounds Chapter 5, Lesson 1.

Covalent Bonds When Atoms Share.

STRUCTURES Module C2.

Simple Molecular Covalent

Chemical Bonds.

A guide for A level students KNOCKHARDY PUBLISHING

Chemical Bonding.

Metals & non-metals - a comparison of properties.

Presentation transcript:

PART 3: Oxides and chorides of the third period (sodium  argon)

Oxides of Period 3 Elements

Formula Na2O MgO Al2O3 SiO2 P4O10 (P4O6) SO3 (SO2) Cl2O7 (Cl2O) State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of oxide

solid liquid liquid solid solid solid solid (solid) (gas) (gas) 1275 Formula Na2O MgO Al2O3 SiO2 P4O10 (P4O6) SO3 (SO2) Cl2O7 (Cl2O) State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of oxide solid liquid liquid solid solid solid solid (solid) (gas) (gas) 1275 2852 2027 1610 24 17 -92 - 3600 2980 2230 175 45 80

solid liquid liquid solid solid solid solid (solid) (gas) (gas) 1275 Formula Na2O MgO Al2O3 SiO2 P4O10 (P4O6) SO3 (SO2) Cl2O7 (Cl2O) State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of oxide solid liquid liquid solid solid solid solid (solid) (gas) (gas) 1275 2852 2027 1610 24 17 -92 - 3600 2980 2230 175 45 80 very poor good none

simple covalent molecular Formula Na2O MgO Al2O3 SiO2 P4O10 (P4O6) SO3 (SO2) Cl2O7 (Cl2O) State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of oxide solid liquid liquid solid solid solid solid (solid) (gas) (gas) 1275 2852 2027 1610 24 17 -92 - 3600 2980 2230 175 45 80 very poor good none covalent macromolecular simple covalent molecular ionic

Left side of PT: oxides of Na, Mg and Al Physical properties - melting points, boiling points & conductivity: (from left  right) Left side of PT: oxides of Na, Mg and Al ionic (metal + nonmetal… large difference in electronegativity) Ionic solids have high melting points Ionic solids are capable of conducting electricity in molten state (moving charge = electricity)

Middle of PT: oxide of Si (silicon dioxide) Physical properties - melting points, boiling points & conductivity: (from left  right) Middle of PT: oxide of Si (silicon dioxide) macromolecular structure Strong diamond-like structure (covalently bonded network) accounts for high boiling point diamond SiO2

Right side of PT: oxides of P, S and Cl Physical properties - melting points, boiling points & conductivity: (from left  right) Right side of PT: oxides of P, S and Cl simple covalent molecules difference in electronegativities between element and oxygen is small low melting and boiling points

simple covalent molecular Formula Na2O MgO Al2O3 SiO2 P4O10 (P4O6) SO3 (SO2) Cl2O7 (Cl2O) State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of oxide solid liquid liquid solid solid solid solid (solid) (gas) (gas) 1275 2852 2027 1610 24 17 -92 - 3600 2980 2230 175 45 80 very poor good none covalent macromolecular simple covalent molecular ionic Forms MgOH2(aq), Weakly alkaline Forms NaOH(aq), alkaline does not react P4O10 forms H3PO4(aq), a weak acid SO3 forms H2SO4(aq), a strong acid does not react Cl2O7 forms HClO4(aq), a strong acid

simple covalent molecular Formula Na2O MgO Al2O3 SiO2 P4O10 (P4O6) SO3 (SO2) Cl2O7 (Cl2O) State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of oxide solid liquid liquid solid solid solid solid (solid) (gas) (gas) 1275 2852 2027 1610 24 17 -92 - 3600 2980 2230 175 45 80 very poor good none covalent macromolecular simple covalent molecular ionic Forms MgOH2(aq), Weakly alkaline Forms NaOH(aq), alkaline does not react P4O10 forms H3PO4(aq), a weak acid SO3 forms H2SO4(aq), a strong acid does not react Cl2O7 forms HClO4(aq), a strong acid basic amphoteric acidic

Chemical properties - Acid-base nature of oxides: (from left  right) Oxides of electropositive (opposite of electronegative) elements are very basic and form alkaline solutions. Na2O(s) + H2O(l)  MgO(s) + H2O(l)  2 NaOH(aq) Mg(OH)2(aq)

Chemical properties - Acid-base nature of oxides: (from left  right) The amphoteric nature of aluminum oxide can be seen from its rxns w/ hydrochloric acid (a strong acid) and sodium hydroxide (a strong base) Acting as a base: Acting as an acid: Al2O3(aq) + 6HCl(aq)  2AlCl3(aq) + 3H2O(l) Al2O3(aq) + 2NaOH(aq) + 3H2O(l)  2NaAl(OH)3(aq) sodium aluminate

Chemical properties - Acid-base nature of oxides: (from left  right) Silicon dioxide behaves as a weak acid. It does not react with water (that would be weird… SiO2 is sand, so if sand chemically reacted with water then our beaches would be very different places). Imagine beach erosion rates if water chemically reacted with sand!!!

Chemical properties - Acid-base nature of oxides: (from left  right) Silicon dioxide behaves as a weak acid. It does not react with water (that would be weird… SiO2 is sand, so if sand chemically reacted with water then our beaches would be very different places). However, silicon dioxide will form sodium silicate with sodium hydroxide (meaning it reacts with a base). SiO2(s) + 2NaOH(aq)  Na2SiO3(aq) + H2O(l)

Chemical properties - Acid-base nature of oxides: (from left  right) The oxides of phosphorus, sulfur and chlorine are all strongly acidic (all form strong acids when added to water). SO2(s) + H2O(l)  P4O10(s) + H2O(l)  Cl2O7(l) + H2O(l)  H2SO3(aq) sulfurous acid 6 4 H3PO4(aq) phosphoric acid 2 HClO4(aq) perchloric acid

Chemical properties - Acid-base nature of oxides: (from left  right)

Chlorides of Period 3 Elements

Formula NaCl MgCl2 Al2Cl6 SiCl4 PCl3 (PCl5) S2Cl2 Cl2 State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of solution

liquid solid solid solid liquid liquid gas (solid) 178 801 714 -70 Formula NaCl MgCl2 Al2Cl6 SiCl4 PCl3 (PCl5) S2Cl2 Cl2 State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of solution liquid solid solid solid liquid liquid gas (solid) 178 801 714 -70 -112 -80 -101 (sublimes) 1413 1412 - 58 76 136 -35

liquid solid solid solid liquid liquid gas (solid) 178 801 714 -70 Formula NaCl MgCl2 Al2Cl6 SiCl4 PCl3 (PCl5) S2Cl2 Cl2 State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of solution liquid solid solid solid liquid liquid gas (solid) 178 801 714 -70 -112 -80 -101 (sublimes) 1413 1412 - 58 76 136 -35 good poor none

simple covalent molecule Formula NaCl MgCl2 Al2Cl6 SiCl4 PCl3 (PCl5) S2Cl2 Cl2 State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of solution liquid solid solid solid liquid liquid gas (solid) 178 801 714 -70 -112 -80 -101 (sublimes) 1413 1412 - 58 76 136 -35 good poor none ionic simple covalent molecule

Physical properties - melting points, boiling points & conductivity: (from left  right) Structure affects physical properties of chlorides in the same way it did for oxides. NaCl and MgCl2 are ionic – conduct electricity in molten state – high melting points

Physical properties - melting points, boiling points & conductivity: (from left  right) AlCl3 is covalent – poor conductor

Physical properties - melting points, boiling points & conductivity: (from left  right) Unlike SiO2, SiCl4 has a simple molecular structure (not a macromolecular network) SiO2 network SiCl4 molecules

Physical properties - melting points, boiling points & conductivity: (from left  right) PCl3, PCl5, S2Cl2, Cl2 – all have simple molecular structures (covalently bonded molecules) held together by weak van der Waals’ forces, resulting in low melting and boiling points. S2Cl2 Cl2 molecules

simple covalent molecule Formula NaCl MgCl2 Al2Cl6 SiCl4 PCl3 (PCl5) S2Cl2 Cl2 State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of solution liquid solid solid solid liquid liquid gas (solid) 178 801 714 -70 -112 -80 -101 (sublimes) 1413 1412 - 58 76 136 -35 good poor none ionic simple covalent molecule dissolves easily Fumes of HCl produced Some rxn w/ H2O

simple covalent molecule Formula NaCl MgCl2 Al2Cl6 SiCl4 PCl3 (PCl5) S2Cl2 Cl2 State at 25°C Melting pt. (°C) Boiling pt. (°C) Electrical conductivity in molten state Structure Rxn w/ H2O Nature of solution liquid solid solid solid liquid liquid gas (solid) 178 801 714 -70 -112 -80 -101 (sublimes) 1413 1412 - 58 76 136 -35 good poor none ionic simple covalent molecule dissolves easily Fumes of HCl produced Some rxn w/ H2O weakly acidic neutral acidic

Chemical properties - Acid-base nature of chlorides: (from left  right) NaCl dissolves in H2O to give a neutral solution (more on why when we get to the acid/base unit). MgCl2 gives a slightly acidic solution with water (again, more on this later).

Chemical properties - Acid-base nature of chlorides: (from left  right) All other chlorides including AlCl3 react vigorously with water to produce acidic solutions of hydrochloric acid together with fumes of hydrogen chloride. AlCl3(s) + H2O(l)  SiCl4(l) + H2O(l)  PCl3(l) + H2O(l)  2 3 Al2O3(s) + HCl(aq) 6 4 Si(OH)4(aq) + HCl(aq) 4 3 H3PO3(aq) + HCl(aq) 3

Chemical properties - Acid-base nature of chlorides: (from left  right) Chlorine itself reacts with water to some extent to form acidic solution. Cl2(g) + H2O(l)  HCl(aq) + HClO(aq)