Presentation is loading. Please wait.

Presentation is loading. Please wait.

© www.chemsheets.co.uk A2 034 17-Jul-12. H NaCl (s) Na + (g) + Cl - (g)  H lattice energy of formation Na (s) + ½ Cl 2 (g)  H formation  H atomisation(s)

Published byTheodora Skinner Modified over 8 years ago

Similar presentations

Presentation on theme: "© www.chemsheets.co.uk A2 034 17-Jul-12. H NaCl (s) Na + (g) + Cl - (g)  H lattice energy of formation Na (s) + ½ Cl 2 (g)  H formation  H atomisation(s)"— Presentation transcript:

1 © www.chemsheets.co.uk A2 034 17-Jul-12

2 H NaCl (s) Na + (g) + Cl - (g)  H lattice energy of formation Na (s) + ½ Cl 2 (g)  H formation  H atomisation(s) Na (g) + Cl (g) Na + (g) + e - + Cl (g)  H ionisation energy/ies  H electron affinity/ies NaCl © www.chemsheets.co.uk A2 034 17-Jul-12

3 H Na + (g) + Cl - (g)  H lattice energy of formation Na (s) + ½ Cl 2 (g)  H formation  H atomisation(s) Na (g) + Cl (g) Na + (g) + e - + Cl (g)  H ionisation energy/ies  H electron affinity/ies Ionic compound (s) © www.chemsheets.co.uk A2 034 17-Jul-12

4 H Na + (g) + Cl - (g)  H lattice energy of formation  H formation  H atomisation(s) Na (g) + Cl (g) Na + (g) + e - + Cl (g)  H ionisation energy/ies  H electron affinity/ies Ionic compound (s) Elements (std states) © www.chemsheets.co.uk A2 034 17-Jul-12

5 H Na + (g) + Cl - (g)  H lattice energy of formation  H formation  H atomisation(s) Na + (g) + e - + Cl (g)  H ionisation energy/ies  H electron affinity/ies Ionic compound (s) Elements (std states) Gas atoms (g) © www.chemsheets.co.uk A2 034 17-Jul-12

6 H Na + (g) + Cl - (g)  H lattice energy of formation  H formation  H atomisation(s)  H ionisation energy/ies  H electron affinity/ies Ionic compound (s) Elements (std states) Gas atoms (g) Metal ions, e - ’s, non-metal atoms (g) © www.chemsheets.co.uk A2 034 17-Jul-12

7 H  H lattice energy of formation  H formation  H atomisation(s)  H ionisation energy/ies  H electron affinity/ies Ionic compound (s) Elements (std states) Gas atoms (g) Metal ions, e - ’s, non-metal atoms (g) Gas ions (g) © www.chemsheets.co.uk A2 034 17-Jul-12

8 H Ionic compound (s) Gas ions (g)  H lattice energy of formation Elements (std states)  H formation  H atomisation(s) Gas atoms (g) Metal ions, e - ’s, non-metal atoms (g)  H ionisation energy/ies  H electron affinity/ies  H formation = sum of all other  H’s © www.chemsheets.co.uk A2 034 17-Jul-12

9 H NaCl (s) Na + (g) + Cl - (g)  H lattice energy of formation Na (s) + ½ Cl 2 (g)  H formation  H atomisation(s) Na (g) + Cl (g) Na + (g) + e - + Cl (g)  H ionisation energy/ies  H electron affinity/ies NaCl 109 121 494–364 –771  H formation = 109 + 121 + 494 – 364 – 771 = – 411 kJmol -1 ? © www.chemsheets.co.uk A2 034 17-Jul-12

10 H MgCl 2 (s) Mg 2+ (g) + 2 Cl - (g)  H lattice energy of formation Mg (s) + Cl 2 (g)  H formation  H atomisation(s) Mg (g) + 2 Cl (g) Mg 2+ (g) + 2 e - + 2 Cl (g)  H ionisation energy/ies  H electron affinity/ies MgCl 2 150 2(121) 736 1450 2(–364) ? – 642 = 150 + 2(121) + 736 + 1450 – 2(364) +  H lattice  H lattice = – 642 – 150 – 2(121) – 736 – 1450 + 2 (364) = – 2492 kJ mol -1 –642 © www.chemsheets.co.uk A2 034 17-Jul-12

11 H KCl (s) K + (g) + Cl - (g)  H lattice energy of formation K (s) + ½ Cl 2 (g)  H formation  H atomisation(s) K (g) + Cl (g) K + (g) + e - + Cl (g)  H ionisation energy/ies  H electron affinity/ies KCl 90 121 418–364 – 710  H formation = 90 + 121 + 418 – 364 – 710 = – 445 kJ mol -1 ? © www.chemsheets.co.uk A2 034 17-Jul-12

12 H CaBr 2 (s) Ca 2+ (g) + 2 Br - (g)  H lattice energy of formation Ca (s) + Br 2 (l)  H formation  H atomisation(s) Ca (g) + 2 Br(g) Ca 2+ (g) + 2 e - + 2 Br (g)  H ionisation energy/ies  H electron affinity/ies CaBr 2 193 2(112) 590 1150 2(–342) –2125 ?  H formation = 193 + 2(112) + 590 + 1150 – 2(342) – 2125 = – 652 kJ mol -1 © www.chemsheets.co.uk A2 034 17-Jul-12

13 H Al 2 O 3 (s) 2 Al 3+ (g) + 2 O 2 - (g)  H lattice energy of formation 2 Al (s) + 3 / 2 O 2 (g)  H formation  H atomisation(s) 2 Al (g) + 3 O (g) 2 Al 3+ (g) + 6 e - + 3 O (g)  H ionisation energy/ies  H electron affinity/ies Al 2 O 3 2(314) 3(248) 2(577) 2(1820) 2(2740) 3(–142) 3(844) ? –1669 = 2(314) + 3(248) + 2(577) + 2(1820) + 2(2740) + 3(-142) + 3(844) +  H  H = –1669 – 2(314) – 3(248) – 2(577) – 2(1820) – 2(2740) + 3(142) – 3(844) = – 15421 kJ mol -1 –1669 © www.chemsheets.co.uk A2 034 17-Jul-12

14 H CaO (s) Ca 2+ (g) + O 2 - (g)  H lattice energy of formation Ca (s) + ½ O 2 (g)  H formation  H atomisation(s) Ca (g) + O (g) Ca 2+ (g) + 2 e - + O (g)  H ionisation energy/ies  H electron affinity/ies CaO 193 248 590 1150 –142 +844 ? – 635 = 193 + 248 + 590 + 1150 – 142 + 844 +  H lattice  H lattice = – 635 – 193 – 248 – 590 – 1150 + 142 – 844 = – 3518 kJ mol -1 –635 © www.chemsheets.co.uk A2 034 17-Jul-12

15 H CaI 2 (s) Ca 2+ (g) + 2 I - (g)  H lattice energy of formation Ca (s) + I 2 (s)  H formation  H atomisation(s) Ca (g) + 2 I(g) Ca 2+ (g) + 2 e - + 2 I (g)  H ionisation energy/ies  H electron affinity/ies CaI 2 193 2(107) 590 1150 2X – 2054 – 535 = 193 + 2(107) + 590 + 1150 + 2X – 2054 2X = – 535 – 193 – 2(107) – 590 – 1150 – 2054 2X = - 628 X = – 314 kJ mol -1 –535 © www.chemsheets.co.uk A2 034 17-Jul-12

16 H CuO (s) Cu 2+ (g) + O 2 - (g)  H lattice energy of formation Cu (s) + ½ O 2 (g)  H formation  H atomisation(s) Cu (g) + O (g) Cu 2+ (g) + 2 e - + O (g)  H ionisation energy/ies  H electron affinity/ies CuO X 248 745 1960 –142 +844 – 4149 – 155 = X + 248 + 745 + 1960 – 142 + 844 – 4149 X = – 155 – 248 – 745 – 1960 + 142 – 844 + 4149 = + 339 kJ mol -1 –155 © www.chemsheets.co.uk A2 034 17-Jul-12

17 H CoCl (s) Co + (g) + Cl - (g)  H lattice energy of formation Co (s) + ½ Cl 2 (g)  H formation  H atomisation(s) Co (g) + Cl(g) Co + (g) + e - + Cl (g)  H ionisation energy/ies  H electron affinity/ies CoCl 427 121 757–364 –700 ?  H formation = 427 + 121 + 757 – 364 – 700 = + 241 kJ mol -1 © www.chemsheets.co.uk A2 034 17-Jul-12

18 H CoCl 2 (s) Co 2+ (g) + 2 Cl - (g)  H lattice energy of formation Co (s) + Cl 2 (g)  H formation  H atomisation(s) Co (g) + 2 Cl(g) Co 2+ (g) + 2 e - + 2 Cl (g)  H ionisation energy/ies  H electron affinity/ies CoCl 2 427 2(121) 757 1640 2(–364) –2624 ?  H formation = 427 + 2(121) + 757 + 1640 – 2(364) – 2624 = – 286 kJ mol -1 © www.chemsheets.co.uk A2 034 17-Jul-12

19 H CoCl 3 (s) Co 3+ (g) + 3 Cl - (g)  H lattice energy of formation Co (s) + 3 / 2 Cl 2 (g)  H formation  H atomisation(s) Co (g) + 3 Cl(g) Co 3+ (g) + 3 e - + 2 Cl (g)  H ionisation energy/ies  H electron affinity/ies CoCl 3 427 3(121) 757 1640 3230 3(–364) –5350 ?  H formation = 427 + 3(121) + 757 + 1640 + 3230 – 3(364) – 5350 = – 25 kJ mol -1 © www.chemsheets.co.uk A2 034 17-Jul-12

Download ppt "© www.chemsheets.co.uk A2 034 17-Jul-12. H NaCl (s) Na + (g) + Cl - (g)  H lattice energy of formation Na (s) + ½ Cl 2 (g)  H formation  H atomisation(s)"

Similar presentations

Single Replacement One element replaces a similar element in a compound A + BX AX + B A replaces B if A and B are similar Metals can replace less reactive.

Single Replacement One element replaces a similar element in a compound A + BX AX + B A replaces B if A and B are similar Metals can replace less reactive.
BORN-HABER CYCLES A guide for A level students KNOCKHARDY PUBLISHING 2008 SPECIFICATIONS.

BORN-HABER CYCLES A guide for A level students KNOCKHARDY PUBLISHING 2008 SPECIFICATIONS.
Oxidation-reduction reactions

Oxidation-reduction reactions
Title: Lesson 6 Born-Haber Cycles and Lattice Enthalpies Learning Objectives: – Understand the term lattice enthalpy – Use Born-Haber cycles to calculate.

Title: Lesson 6 Born-Haber Cycles and Lattice Enthalpies Learning Objectives: – Understand the term lattice enthalpy – Use Born-Haber cycles to calculate.
Formation of Binary Ionic Compounds Binary Ionic Compound n Binary- two n Ionic- ions n Compound- joined together.

Formation of Binary Ionic Compounds Binary Ionic Compound n Binary- two n Ionic- ions n Compound- joined together.
2.2 Ionic Compounds 2.2.1 Atomic Ions LO:I understand how ions are formed from neutral atoms.

2.2 Ionic Compounds Atomic Ions LO:I understand how ions are formed from neutral atoms.
Metal atoms with low ionization energies and non-metal atoms with high electron affinity form cations (+) and anions (-) Oppositely charged ions attract.

Metal atoms with low ionization energies and non-metal atoms with high electron affinity form cations (+) and anions (-) Oppositely charged ions attract.
Activity Directions: Use the worksheet to guide you as you create the formulas. You will be matching the blue and yellow elements according to their valance.

Activity Directions: Use the worksheet to guide you as you create the formulas. You will be matching the blue and yellow elements according to their valance.
Ionic Bonding. CA Standards  Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons.

Ionic Bonding. CA Standards  Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons.
Ionic Bonding  Electrons are transferred  Electronegativity differences are generally greater than 1.7  The formation of ionic bonds is always exothermic!

Ionic Bonding  Electrons are transferred  Electronegativity differences are generally greater than 1.7  The formation of ionic bonds is always exothermic!
For an ionic compound the lattice enthalpy is the heat energy released when one mole of solid in its standard state is formed from its ions in the gaseous.

For an ionic compound the lattice enthalpy is the heat energy released when one mole of solid in its standard state is formed from its ions in the gaseous.
Lecture 2711/07/05. Ionic bond Ionic compounds Valence electrons are transferred from one atom to another Metal + non-metal NaCl Bonding.

Lecture 2711/07/05. Ionic bond Ionic compounds Valence electrons are transferred from one atom to another Metal + non-metal NaCl Bonding.
Topic: Lewis Dot Diagrams for Ionic Compounds

Topic: Lewis Dot Diagrams for Ionic Compounds
Chemical Bonding: The Ionic Bond Model. Chemical Bonds Forces that hold atoms to each other within a molecule or compound.

Chemical Bonding: The Ionic Bond Model. Chemical Bonds Forces that hold atoms to each other within a molecule or compound.
Ionic Bonding  Electrons are transferred  Electronegativity differences are generally greater than 1.7  The formation of ionic bonds is always exothermic!

Ionic Bonding  Electrons are transferred  Electronegativity differences are generally greater than 1.7  The formation of ionic bonds is always exothermic!
Ionic Compounds Formed from positive and negative ions. Almost always have a metal and a nonmetal.

Ionic Compounds Formed from positive and negative ions. Almost always have a metal and a nonmetal.
1 Born-Haber Cycles enthalpy H magnesium chloride MgCl 2 (s) Mg 2+ (g) + 2Cl - (g) H lattice Mg (s) + Cl 2 (g) H formation H atomisation Mg (g) + Cl.

1 Born-Haber Cycles enthalpy H magnesium chloride MgCl 2 (s) Mg 2+ (g) + 2Cl - (g) H lattice Mg (s) + Cl 2 (g) H formation H atomisation Mg (g) + Cl.
1 For an ionic compound the lattice enthalpy is the heat energy released when one mole of solid in its standard state is formed from its ions in the gaseous.

1 For an ionic compound the lattice enthalpy is the heat energy released when one mole of solid in its standard state is formed from its ions in the gaseous.
27/08/2015 Ionic bonding This is where a metal bonds with a non-metal. The metal atom donates one or more electrons to the non-metal. For example, consider.

27/08/2015 Ionic bonding This is where a metal bonds with a non-metal. The metal atom donates one or more electrons to the non-metal. For example, consider.
Chemical Names and Formulas Molecules and Molecular Compounds 1.Molecule- the smallest electrically neutral unit of a substance that still has the properties.

Chemical Names and Formulas Molecules and Molecular Compounds 1.Molecule- the smallest electrically neutral unit of a substance that still has the properties.

Similar presentations

Ads by Google