This document provides a tutorial on chemical bonding including ionic bonds, covalent bonds, polarity, hydrogen bonding, and intermolecular forces. It discusses how ionic bonds form through the transfer of electrons between metals and nonmetals, and how covalent bonds form through the sharing of electrons between nonmetals. It also explains how polarity arises from unequal sharing of electrons and differences in electronegativity. Additional concepts covered include London dispersion forces, dipole-dipole interactions, factors that influence boiling points, and the properties of hydrogen bonding.
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
Properties of periodic table by Saliha RaisSaliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
Valence shell electron pair repulsion (VSEPR) theory is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. It is also named the Gillespie-Nyholm theory after its two main developers, Ronald Gillespie and Ronald Nyholm
Organic reactions are chemical reactions involving organic compounds. Organic reactions are used in the construction of new organic molecules. The production of many man-made chemicals such as drugs, plastics, food additives, fabrics depend on organic reactions.
Nature of coordination compounds, coordination sphere, coordination number, oxidation state of central metal atom, lewis acids, types of ligands, types of complex(cationic and anionic), Valance bond theory, crystal field theory, werner theory of coordination compounds, Nomenclature of coordination compounds.Eg and t2g ,CFSE, Degeneracy, Application of coordination compounds, Charge of the coordination sphere.
Spatial arrangements, inner and outer orbital complexes, low and high spin complex, spin pair and spin free complexes, isomerism, types of isomerism.
how to write electronic configuration of an atom
rules of filling electrons in energy levels
aufbau principle. hund's rule, Pauli's Exclusion principle
Valence shell electron pair repulsion (VSEPR) theory is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. It is also named the Gillespie-Nyholm theory after its two main developers, Ronald Gillespie and Ronald Nyholm
Organic reactions are chemical reactions involving organic compounds. Organic reactions are used in the construction of new organic molecules. The production of many man-made chemicals such as drugs, plastics, food additives, fabrics depend on organic reactions.
Nature of coordination compounds, coordination sphere, coordination number, oxidation state of central metal atom, lewis acids, types of ligands, types of complex(cationic and anionic), Valance bond theory, crystal field theory, werner theory of coordination compounds, Nomenclature of coordination compounds.Eg and t2g ,CFSE, Degeneracy, Application of coordination compounds, Charge of the coordination sphere.
Spatial arrangements, inner and outer orbital complexes, low and high spin complex, spin pair and spin free complexes, isomerism, types of isomerism.
how to write electronic configuration of an atom
rules of filling electrons in energy levels
aufbau principle. hund's rule, Pauli's Exclusion principle
In this ppt my aim is to show you that about periodic trend ,periodic laws ,metal nonmetal & metalloids ,periodic table,valence electrons ,vb theory & About atomic radius,size etc and about types of bonds ,types of enthalpy ,formation of electrons,rules and many more
2024.06.01 Introducing a competency framework for languag learning materials ...Sandy Millin
http://sandymillin.wordpress.com/iateflwebinar2024
Published classroom materials form the basis of syllabuses, drive teacher professional development, and have a potentially huge influence on learners, teachers and education systems. All teachers also create their own materials, whether a few sentences on a blackboard, a highly-structured fully-realised online course, or anything in between. Despite this, the knowledge and skills needed to create effective language learning materials are rarely part of teacher training, and are mostly learnt by trial and error.
Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
For more information, visit-www.vavaclasses.com
How to Split Bills in the Odoo 17 POS ModuleCeline George
Bills have a main role in point of sale procedure. It will help to track sales, handling payments and giving receipts to customers. Bill splitting also has an important role in POS. For example, If some friends come together for dinner and if they want to divide the bill then it is possible by POS bill splitting. This slide will show how to split bills in odoo 17 POS.
The Indian economy is classified into different sectors to simplify the analysis and understanding of economic activities. For Class 10, it's essential to grasp the sectors of the Indian economy, understand their characteristics, and recognize their importance. This guide will provide detailed notes on the Sectors of the Indian Economy Class 10, using specific long-tail keywords to enhance comprehension.
For more information, visit-www.vavaclasses.com
The Art Pastor's Guide to Sabbath | Steve ThomasonSteve Thomason
What is the purpose of the Sabbath Law in the Torah. It is interesting to compare how the context of the law shifts from Exodus to Deuteronomy. Who gets to rest, and why?
Instructions for Submissions thorugh G- Classroom.pptxJheel Barad
This presentation provides a briefing on how to upload submissions and documents in Google Classroom. It was prepared as part of an orientation for new Sainik School in-service teacher trainees. As a training officer, my goal is to ensure that you are comfortable and proficient with this essential tool for managing assignments and fostering student engagement.
Operation “Blue Star” is the only event in the history of Independent India where the state went into war with its own people. Even after about 40 years it is not clear if it was culmination of states anger over people of the region, a political game of power or start of dictatorial chapter in the democratic setup.
The people of Punjab felt alienated from main stream due to denial of their just demands during a long democratic struggle since independence. As it happen all over the word, it led to militant struggle with great loss of lives of military, police and civilian personnel. Killing of Indira Gandhi and massacre of innocent Sikhs in Delhi and other India cities was also associated with this movement.
Model Attribute Check Company Auto PropertyCeline George
In Odoo, the multi-company feature allows you to manage multiple companies within a single Odoo database instance. Each company can have its own configurations while still sharing common resources such as products, customers, and suppliers.
The Roman Empire A Historical Colossus.pdfkaushalkr1407
The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
2. Chemical Bonds
Ionic Bonds
Transfer of electron from
metal to non metal
Metal donate e Non Metal accept e
Positive ion
(cation)
Negative ion
(anion)
Ionic compound
+ -electrostatic forces
attraction
3. Chemical Bonds
Ionic Bonds
Transfer of electron from
metal to non metal
Metal donate e Non Metal accept e
Positive ion
(cation)
Negative ion
(anion)
Ionic compound
Covalent Bonds
Sharing of electron
bet non metal atoms
Equal sharing electrons
+ -electrostatic forces
attraction
Polar covalent Bonds Non Polar covalent Bonds
Unequal sharing electrons
Covalent Polar Non polar
4. Chemical Bonds
Ionic Bonds
Transfer of electron from
metal to non metal
Metal donate e Non Metal accept e
Positive ion
(cation)
Negative ion
(anion)
Ionic compound
Covalent Bonds
Sharing of electron
bet non metal atoms
Equal sharing electrons
+ -electrostatic forces
attraction
4 0.4 0
Difference in electronegativity
2
EN - 0.9 EN – 3
Diff = (3 – 3 ) = 0
H
EN – 2.1
Diff = 3 – 0.9 = 2.1
Polar covalent Bonds Non Polar covalent Bonds
Unequal sharing electrons
Covalent Polar Non polar
CI CI
EN – 3
Covalent Non polar
CI
Covalent polarIonic
EN – 3
Diff = (3 – 2.1 ) = 0.9
Na+
CI-
EN – 3
5. Shared electron cloud closer to O
Electronegativity
Electronegativity (EN)
•Tendency of atom to attract/pull shared/bonding electron to itself
•EN value higher – pull/attract electron higher (EN value from 0.7 – 4)
Electronegativity
•EN increase up a Group
•EN increase across a Period
6. Shared electron cloud closer to O
Electronegativity
Electronegativity (EN)
•Tendency of atom to attract/pull shared/bonding electron to itself
•EN value higher – pull/attract electron higher (EN value from 0.7 – 4)
Electronegativity
•EN increase up a Group
•EN increase across a Period
H
2.2
Li Be B C N O F
CI
Br
I
1 1.6 2 2.6 3 3.4 4
Electronegativity values
N, O, F have high EN value
3.2
3
2.7
Molecule Diff in EN Polarity
H - F (4.0 – 2.2) = 1.8 Most polar
H - CI (3.2 – 2.2) = 1
H - Br (3.0 – 2.2) = 0.8
H - I (2.7 – 2.2) = 0.5 Least polar
Polarity
Shape Diff in EN
Symmetrical Asymmetrical
Bond polarity cancel out each other
Polar bonds – molecule NON POLAR
Bond polarity cancel out each other
Polar bonds – molecule POLAR
✓✗
7. Shared electron cloud closer to O
Electronegativity
Electronegativity (EN)
•Tendency of atom to attract/pull shared/bonding electron to itself
•EN value higher – pull/attract electron higher (EN value from 0.7 – 4)
Electronegativity
•EN increase up a Group
•EN increase across a Period
H
2.2
Li Be B C N O F
CI
Br
I
1 1.6 2 2.6 3 3.4 4
Electronegativity values
N, O, F have high EN value
3.2
3
2.7
Molecule Diff in EN Polarity
H - F (4.0 – 2.2) = 1.8 Most polar
H - CI (3.2 – 2.2) = 1
H - Br (3.0 – 2.2) = 0.8
H - I (2.7 – 2.2) = 0.5 Least polar
Polarity
Shape Diff in EN
Symmetrical Asymmetrical
Bond polarity cancel out each other
Polar bonds – molecule NON POLAR
Bond polarity cancel out each other
Polar bonds – molecule POLAR
Lewis structure
VSEPR
Geometry
1
4 ECC
3 bond pair
1 lone pair
..
N
H
H
H
Polarity
2
3
4
Polar
✓✗
8. Covalent Bonds
Polar covalent Bonds Non Polar covalent Bond
Equal sharing electronUnequal sharing electron
Sharing of electron
9. Separation of charges
Unequal distribution electron due to diff EN value
shared electron closer to Oshared electron closer to F
Covalent Bonds
Polar covalent Bonds Non Polar covalent Bond
Equal sharing electronUnequal sharing electron
Sharing of electron
Formation electric dipole
Partial +/-
Dipole moment
towards O
Partial + ( δ+)
Partial – (δ−)
Net dipole moment
Net Dipole moment
Polar covalent Bonds
Molecule polar ✓
O
O
10. ✗
In presence of electric field
Separation of charges
Unequal distribution electron due to diff EN value
shared electron closer to Oshared electron closer to F
Covalent Bonds
Polar covalent Bonds Non Polar covalent Bond
Equal sharing electronUnequal sharing electron
Sharing of electron
Formation electric dipole
Partial +/-
Dipole moment
towards O
Partial + ( δ+)
Partial – (δ−)
Net dipole moment
Molecule is polar (dipole)
Net Dipole moment
Measured in Debye
Turning force / Dipole moment = Force x DistancePolar covalent Bonds
+ -
O
III
C δ+
δ-
Turning force – dipole moment
+ -
O
II
C
II
O
δ+
δ-
δ-
No Turning force – No dipole moment
✓
Molecule polar ✓
O
O
12. Polarity
Shape
Asymmetrical
Shape
Symmetrical
Polar bonds
CI
Polar bonds
δ-
δ+ δ+
δ+
δ-
δ-
δ-
δ-
δ-
δ-
Bond polarity
don’t cancel
Bond polarity
cancel
H
Net Dipole moment No Net Dipole moment
✗
Asymmetrical Symmetrical
δ-δ+
Polar bonds
Bond polarity
don’t cancel
Net Dipole moment
C O
δ- δ-
Polar bonds
Bond polarity cancel
No Net Dipole moment
✗ ✗✓
✓
I
13. Polarity
Shape
Asymmetrical
Polar bond
Polarity dont cancel
(ASYMMETRICAL)
Net dipole moment
Molecule POLAR
Polar bond
Polarity cancel
(SYMMETRICAL)
NO net dipole moment
Molecule NON POLAR
Shape
Symmetrical
Polar bonds
CI
Polar bonds
δ-
δ+ δ+
δ+
δ-
δ-
δ-
δ-
δ-
δ-
Bond polarity
don’t cancel
Bond polarity
cancel
H
Net Dipole moment No Net Dipole moment
✗
Asymmetrical Symmetrical
δ-δ+
Polar bonds
Bond polarity
don’t cancel
Net Dipole moment
C O
Polar bond
Polarity dont cancel
(ASYMMETRICAL)
Net dipole moment
Molecule POLAR
δ- δ-
Polar bonds
Bond polarity cancel
No Net Dipole moment
Polar bond
Polarity cancel
(SYMMETRICAL)
NO dipole moment
Molecule NON POLAR
✗ ✗✓
✓
I
14. Bonding Forces
Bonding Forces within molecule Bonding Forces bet molecule
Intermolecular force bet molecule (IMF)Ionic
bond
Covalent
bond
Metallic
bond
Permanent dipole
IonsMolecules/NOT ions
Ion dipole forces
Polar Non Polar
Hydrogen bonding
Temporary dipole
(instantaneously induced dipole)
London dispersion forces
Van Der Waals’ Forces attraction
Polar molecule (dipole – dipole attraction)
_ _ _
Attraction bet ions with polar molecules
Dipole/dipole attraction Dipole/dipole attraction
(involving H atom attach to N,O F)
Hydrogen bonding (dipole – dipole attraction)
Forces bet molecule
15. Permanent dipole
Polar Non Polar
Temporary dipole
(instantaneously induced dipole)
London dispersion forces
Dipole/dipole attraction Dipole/dipole attraction
Intermolecular force bet molecule (IMF)
Non polar molecules
Polar molecules
Polar molecules
Forces bet molecule
Molecules
16. Permanent dipole
Polar Non Polar
Temporary dipole
(instantaneously induced dipole)
London dispersion forces
Van Der Waals’ Forces attraction
Polar molecule (dipole – dipole attraction)
Polar molecules due to diff in EN values
Dipole/dipole interaction
Electrostatic forces attraction bet molecules
Dipole/dipole attraction Dipole/dipole attraction
Hydrogen bonding (dipole – dipole attraction)
H atom bond to electronegative atom, N, O, F
Partial H+
attracted to lone pair electron on N, O, F
Electrostatic force attraction bet molecules involve H
Intermolecular force bet molecule (IMF)
Non Polar molecule (Induced dipole attraction)
Random movement /distribution of electron
Instantaneous negative charge on atom
Induced a temporary dipole separation
Electrostatic forces attraction bet molecules
Non polar molecules
Polar molecules
Polar molecules
Forces bet molecule
Molecules
17. Permanent dipole
Polar Non Polar
Temporary dipole
(instantaneously induced dipole)
London dispersion forces
Dipole/dipole attraction Dipole/dipole attraction
Molecules
Non polar molecules
Polar molecules
Polar molecules
18. Hydrogen bonding (dipole – dipole attraction)
H atom bond to electronegative atom, N, O, F
Partial H+
attracted to lone pair electron on N, O, F
Electrostatic force attraction bet molecules involve H
Permanent dipole
Polar Non Polar
Temporary dipole
(instantaneously induced dipole)
London dispersion forces
Polar molecule
Polar molecules due to diff in EN values
Dipole/dipole interaction
Electrostatic forces attraction bet molecules
Dipole/dipole attraction Dipole/dipole attraction
Molecules
Non Polar molecule (Induced dipole attraction)
Random movement /distribution of electron
Instantaneous negative charge on atom
Induced a temporary dipole separation
Instantaneous dipole in one atom
induce a dipole in its neighbor
Electrostatic forces attraction bet molecules
Non polar molecules
Polar molecules
Polar molecules
Requirement for H bonding
•H atom bonded to N, O, F
•N, O, F - highly electronegative/ small size
•Attract electron close to itself – Polarised H+
•N---H, O—H, F—H bonds VERY POLAR
•Very polar H+
attract closely to lone pair on N, O, F
N ---- H O ---- H F ---- H
δ- δ- δ-δ+ δ-+ δ+
19. Hydrogen bonding (dipole – dipole attraction)
H atom bond to electronegative atom, N, O, F
Partial H+
attracted to lone pair electron on N, O, F
Electrostatic force attraction bet molecules involve H
Permanent dipole
Polar Non Polar
Temporary dipole
(instantaneously induced dipole)
London dispersion forces
Van Der Waals’ Forces attraction
Polar molecule
Polar molecules due to diff in EN values
Dipole/dipole interaction
Electrostatic forces attraction bet molecules
Dipole/dipole attraction Dipole/dipole attraction
Molecules
Non Polar molecule (Induced dipole attraction)
Random movement /distribution of electron
Instantaneous negative charge on atom
Induced a temporary dipole separation
Instantaneous dipole in one atom
induce a dipole in its neighbor
Electrostatic forces attraction bet molecules
Non polar molecules
Polar molecules
Polar molecules
Requirement for H bonding
•H atom bonded to N, O, F
•N, O, F - highly electronegative/ small size
•Attract electron close to itself – Polarised H+
•N---H, O—H, F—H bonds VERY POLAR
•Very polar H+
attract closely to lone pair on N, O, F
N ---- H O ---- H F ---- H
δ- δ- δ-δ+ δ-+ δ+
20. Intermolecular force bet molecule (IMF)
Dipole – dipole attraction Induced – dipole attraction
London dispersion forces
Polar Non Polar
All molecules have London dispersion forces due to uneven distribution of electron cloud
-
-
-
-
-
-
-
-
-
-
-
-
-
-
-
δ+δ-
London dispersion forces
London dispersion forces
Van Der Waals’ Forces attraction
21. Intermolecular force bet molecule (IMF)
Dipole – dipole attraction Induced – dipole attraction
London dispersion forces
Polar Non Polar
All molecules have London dispersion forces due to uneven distribution of electron cloud
-
-
-
-
-
-
-
-
-
-
-
-
-
-
-
δ+δ-
London dispersion forces
London dispersion forces
Van Der Waals’ Forces attraction
Factor affecting b/p of molecules
Temporary dipole attraction
London dispersion force
Permanent dipole attraction
Dipole/dipole attraction
Hydrogen bonding
22. Types of forces/Bonding
Factors affecting VDF forcesIntermolecular force bet molecule (IMF)
Interaction Strength Boiling
Point/C
Covalent Strongest High
Ionic Strong High
Ion dipole Strong HIgh
Dipole- dipole
(H bond)
Moderate High
Dipole – dipole Weak Low
Temporary induce dipole
(London dispersion)
Weakest Low
Dipole – dipole attraction Induced – dipole attraction
London dispersion forces
Polar Non Polar
All molecules have London dispersion forces due to uneven distribution of electron cloud
-
-
-
-
-
-
-
-
-
-
-
-
-
-
-
δ+δ-
London dispersion forces
RMM/Size Surface Area
London dispersion forces
Van Der Waals’ Forces attraction
N N
F F RMM – 38
RMM – 28
Size/ RMM increase
Number electrons increase
Temporary induced dipole increase
Van Der Waals bet molecule increase
RMM same
Surface area increase
Temporary induced dipole increase
Van Der Waals bet molecules increase
RMM – 72
RMM – 72
Pentane (C5H12)
Factor affecting b/p of molecules
Temporary dipole attraction
London dispersion force
Permanent dipole attraction
Dipole/dipole attraction
Hydrogen bonding
23. Factors affecting VDF forcesFactor affecting b/p of molecules
RMM/Size Surface Area
N N
F F RMM – 38
RMM – 28
Size/ RMM increase
Number electrons increase
Temporary induced dipole increase
Van Der Waals bet molecule increase
RMM same
Surface area increase
Temporary induced dipole increase
Van Der Waals bet molecules increase
RMM – 72
RMM – 72
Pentane (C5H12)
Temporary dipole attraction
London dispersion force
Permanent dipole attraction
Dipole/dipole attraction
Hydrogen bonding
24. Factors affecting VDF forcesFactor affecting b/p of molecules
RMM/Size Surface Area
N N
F F RMM – 38
RMM – 28
Size/ RMM increase
Number electrons increase
Temporary induced dipole increase
Van Der Waals bet molecule increase
RMM same
Surface area increase
Temporary induced dipole increase
Van Der Waals bet molecules increase
RMM – 72
RMM – 72
Pentane (C5H12)
Temporary dipole attraction
London dispersion force
Permanent dipole attraction
Dipole/dipole attraction
Hydrogen bonding
H2 N2 CI2 H2O
RMM 2 28 71 18
Boiling
Point/C
-252 -196 -34 100
Forces London
force
London
force
London
force
London force
Dipole/dipole
Hydrogen bonding
-
-
--
--
H2
London forces
N2
London forces
CI2
London forces
H2O
London forces
Dipole/dipole
Hydrogen bond
RMM increase - London force/VDF increase – boiling point increase
-
-
-
-
--
-
-
--
-
-
-
-
-
-
25. Factors affecting VDF forcesFactor affecting b/p of molecules
RMM/Size Surface Area
N N
F F RMM – 38
RMM – 28
Size/ RMM increase
Number electrons increase
Temporary induced dipole increase
Van Der Waals bet molecule increase
RMM same
Surface area increase
Temporary induced dipole increase
Van Der Waals bet molecules increase
RMM – 72
RMM – 72
Pentane (C5H12)
Temporary dipole attraction
London dispersion force
Permanent dipole attraction
Dipole/dipole attraction
Hydrogen bonding
H2 N2 CI2 H2O
RMM 2 28 71 18
Boiling
Point/C
-252 -196 -34 100
Forces London
force
London
force
London
force
London force
Dipole/dipole
Hydrogen bonding
-
-
--
--
H2
London forces
N2
London forces
CI2
London forces
H2O
London forces
Dipole/dipole
Hydrogen bond
RMM increase - London force/VDF increase – boiling point increase
-
-
-
-
--
-
-
--
-
-
-
-
-
-
Hydrogen bondingHydrogen bonding
RMM lowest - boiling point highest - due to hydrogen bonding
26. HCI HBr HI HF
RMM 36.5 81 128 20
Boiling
Point/C
-85 -66 -35 19.5
Forces London
force/VDF
London
force/VDF
London
force/VDF
London
force/VDF
Dipole/dipole
Hydrogen bond
RMM increase - London force/VDF increase – boiling point increase
Which liquid has higher boiling point?
H H
H
H
H
H
DNA
Br Br
Br
I I
I
Hydrogen bonding
RMM lowest - boiling point highest - due to hydrogen bonding
Hydrogen Bond bet
nitrogenous base
27. HCI HBr HI HF
RMM 36.5 81 128 20
Boiling
Point/C
-85 -66 -35 19.5
Forces London
force/VDF
London
force/VDF
London
force/VDF
London
force/VDF
Dipole/dipole
Hydrogen bond
RMM increase - London force/VDF increase – boiling point increase
Which liquid has higher boiling point?
H H
H
H
H
H
DNA
Br Br
Br
I I
I
Hydrogen bonding
RMM lowest - boiling point highest - due to hydrogen bonding
Br2 ICI
RMM 162 162
B/p/C 58 97
Forces London
force/VDF
London
force/VDF
Dipole/dipole
Which liquid has higher boiling point?
-
-
-
-
-
-
Br2
London forces bet molecules
Br Br Br Br I I ICI CI CI
+ + +- - -
ICI
London forces + Dipole –dipole attraction
Hydrogen Bond bet
nitrogenous base
28. CH3CH2OH CH3CH2CH2OH CH3COOH C2H5-O-C2H5
RMM 46 60 60 74
Boiling
Point/C
78 97 118 34
Forces London
H2 bond
London
H2 bond
London
H2 bond
London
RMM - London force – boiling point
Which liquid has higher boiling point?
Stronger Hydrogen bond – boiling point
....
.......
....
Hydrogen
bond
Hydrogen
bond
....
✕
C3H8 CH3CHO CH3CH2OH
RMM 44 44 46
Boiling
Point/C
-42 20.2 118
Forces London London
Dipole/dipole
London
Dipole/dipole
H2 bond
Which liquid has higher boiling point?
…...
....
…..…..
.......
..........
…...
London forces London forces
+
Dipole/dipole
London forces
+
Dipole/dipole
+
Hydrogen Bond
Hydrogen
bond
29. CH3CH2OH CH3CH2CH2OH CH3COOH C2H5-O-C2H5
RMM 46 60 60 74
Boiling
Point/C
78 97 118 34
Forces London
H2 bond
London
H2 bond
London
H2 bond
London
RMM - London force – boiling point
Which liquid has higher boiling point?
Stronger Hydrogen bond – boiling point
....
.......
....
Hydrogen
bond
Hydrogen
bond
....
✕
C3H8 CH3CHO CH3CH2OH
RMM 44 44 46
Boiling
Point/C
-42 20.2 118
Forces London London
Dipole/dipole
London
Dipole/dipole
H2 bond
RMM highest
No Hydrogen Bond
Which liquid has higher boiling point?
…...
....
…..…..
.......
..........
…...
London forces London forces
+
Dipole/dipole
London forces
+
Dipole/dipole
+
Hydrogen Bond
✕
Hydrogen
bond
30. CH3CH2OH CH3CH2CH2OH CH3COOH C2H5-O-C2H5
RMM 46 60 60 74
Boiling
Point/C
78 97 118 34
Forces London
H2 bond
London
H2 bond
London
H2 bond
London
RMM - London force – boiling point
Which liquid has higher boiling point?
Stronger Hydrogen bond – boiling point
CH3COOH boiling point higher
C=O (carbonyl) – electron withdrawing gp
withdraw electron from OH gp
O-H gp more polarised
stronger H2 bond
....
.......
....
Hydrogen
bond
Hydrogen
bond
....
✕
C - O - H
=
o
C3H8 CH3CHO CH3CH2OH
RMM 44 44 46
Boiling
Point/C
-42 20.2 118
Forces London London
Dipole/dipole
London
Dipole/dipole
H2 bond
RMM highest
No Hydrogen Bond
Which liquid has higher boiling point?
…...
....
…..…..
.......
..........
…...
London forces London forces
+
Dipole/dipole
London forces
+
Dipole/dipole
+
Hydrogen Bond
✕
Hydrogen
bond
31. Why 2 Nitrophenol has lower b/p than 4 nitrophenol?
C6H5NO3
( 2 nitrophenol)
C6H5NO3
( 4 nitrophenol)
RMM 139 139
Boiling
Point/C
216 279
Forces London
Intramolecular
H2 bond
London
Intermolecular
H2 bond
Which NCI3 is polar but BCI3 non polar?
...
…
Intramolecular
H2 bond Non polar
……
✕ Intermolecular
H2 bond
✓
✓
BCI3 NCI3
RMM 117 120
Boiling
Point/C
13 71
Forces London London
Dipole/dipole
…...
Non polar
...
δ-
δ-
δ-
δ-+
polar
polar
….....
✓Dipole dipole
32. Why 2 Nitrophenol has lower b/p than 4 nitrophenol?
Molecule symmetrical
Bond polarity cancel
No net dipole moment
Molecule NON POLAR
C6H5NO3
( 2 nitrophenol)
C6H5NO3
( 4 nitrophenol)
RMM 139 139
Boiling
Point/C
216 279
Forces London
Intramolecular
H2 bond
London
Intermolecular
H2 bond
Which NCI3 is polar but BCI3 non polar?
...
…
Intramolecular
H2 bond Non polar
……
✕
More intramolecular H2 bond
Lack intermolecular H2 bond
Intermolecular
H2 bond
✓
✓
More intermolecular H2 bond
Lack intramolecular H2 bond
BCI3 NCI3
RMM 117 120
Boiling
Point/C
13 71
Forces London London
Dipole/dipole
…...
Non polar
...
δ-
δ-
δ-
δ-+
polar
polar
….....
Molecule asymmetrical
Bond polarity does not cancel
NET dipole moment
Molecule POLAR
✓Dipole dipole
33. Polarity for Cis/Trans Geometrical Isomers
Cis
dichloroethene
Trans
dichloroethene
RMM 96 96
Melting
Point/C
-80 -50
Boiling
Point/C
60 48
...
δ-
Cis
Dipole dipole
Trans
...
...
...
Cis
dichloroethene
Trans
dichloroethene
Melting
Point/C
-80 -50
Kink/ bend shape
Cis
dichloroethene
Trans
dichloroethene
Boiling
Point/C
60 48
Greater attraction
δ+ δ+
δ-
δ- δ-
...
...
Cis Trans
Non polar
Non polar
Polar
Polar
Cis Trans
…......
…......
✓ ✓
34. Trans isomer – CI opposite side
Bond polarity cancel
NO Net dipole moment / NON POLAR
Intermolecular forces weaker
Molecule in linear shape
Able to pack closely together
Greater surface area for interaction
Intermolecular forces stronger
Polarity for Cis/Trans Geometrical Isomers
Molecule in kink/bend shape
Unable to pack closely together
Less surface area for interaction
Intermolecular forces weaker
Cis
dichloroethene
Trans
dichloroethene
RMM 96 96
Melting
Point/C
-80 -50
Boiling
Point/C
60 48
...
δ-
Cis
Dipole dipole
Trans
...
...
...
Cis
dichloroethene
Trans
dichloroethene
Melting
Point/C
-80 -50
Kink/ bend shape
Cis
dichloroethene
Trans
dichloroethene
Boiling
Point/C
60 48
Greater attraction
Cis isomer – CI same side
Bond polarity does not cancel
Net dipole moment /POLAR
Intermolecular forces stronger
δ+ δ+
δ-
δ- δ-
...
...
Cis Trans
Non polar
Non polar
Polar
Polar
Cis Trans
…......
…......
✓ ✓
35. Trans isomer – CI opposite side
Bond polarity cancel
NO Net dipole moment / NON POLAR
Intermolecular forces weaker
Molecule in linear shape
Able to pack closely together
Greater surface area for interaction
Intermolecular forces stronger
Polarity for Cis/Trans Geometrical Isomers
Molecule in kink/bend shape
Unable to pack closely together
Less surface area for interaction
Intermolecular forces weaker
Cis
dichloroethene
Trans
dichloroethene
RMM 96 96
Melting
Point/C
-80 -50
Boiling
Point/C
60 48
...
δ-
Cis
Dipole dipole
Trans
...
...
...
Cis
dichloroethene
Trans
dichloroethene
Melting
Point/C
-80 -50
Kink/ bend shape
Cis
dichloroethene
Trans
dichloroethene
Boiling
Point/C
60 48
Greater attraction
Cis isomer – CI same side
Bond polarity does not cancel
Net dipole moment /POLAR
Intermolecular forces stronger
δ+ δ+
δ-
δ- δ-
...
...
Cis Trans
Non polar
Non polar
Polar
Polar
Cis Trans
…......
…......
✓ ✓
36. RMM increases
Number electron
VDF increases
Evidence for Hydrogen Bonding
Boiling Point group 4 Hydrides
Group 4, 5, 6, 7 Hydrides
Group 4 – SiH4, GeH4, SnH4
Group 5 – PH3, AsH3, SbH3
Group 6 – H2S, H2Se, H2Te
Group 7 – HCI, HBr, HI
37. RMM increases
Number electron
VDF increases
H2O
•2 hydrogen atoms
•2 lone pairs on oxygen
4 Hydrogen bonding available
Evidence for Hydrogen Bonding
Boiling Point group 4 Hydrides
Group 4, 5, 6, 7 Hydrides
Group 4 – SiH4, GeH4, SnH4
Group 5 – PH3, AsH3, SbH3
Group 6 – H2S, H2Se, H2Te
Group 7 – HCI, HBr, HI
High boiling point for
NH3, HF, H2O due to hydrogen bonding
H2O HF
HF
•1 hydrogen atom
•3 lone pairs on fluorine
Lack hydrogen atoms for hydrogen bond
NH3
NH3
•3 hydrogen atoms
•1 lone pairs on ammonia
Lack lone pairs for hydrogen bond
38. CH3-C=O CH3-C-CH3 CH3C-O-H CH3-O-CH3 CH3-N-H CH3-C-N-H
I II II I II
H O O H O
Which of the following molecules are polar/non polar?
ICI BCI3 CH2CI2 SF6 NF3
CO2
δ+ δ- δ+
δ-
δ-
δ-
δ+
δ+
δ+ δ+
δ-
δ-
δ-
δ-
δ-
δ-
δ-
δ- δ-
δ-
δ-
δ- δ-
Which of the following molecules have hydrogen bonding?
CH3CHO CH3COCH3 CH3COOH CH3OCH3 CH3NH2 CH3CONH2
39. CH3-C=O CH3-C-CH3 CH3C-O-H CH3-O-CH3 CH3-N-H CH3-C-N-H
I II II I II
H O O H O
Which of the following molecules are polar/non polar?
ICI BCI3 CH2CI2 SF6 NF3
CO2
δ+ δ- δ+
δ-
δ-
δ-
δ+
δ+
δ+ δ+
δ-
δ-
δ-
δ-
δ-
δ-
δ-
δ- δ-
δ-
δ-
δ- δ-
Polar bond Polar Bond Polar Bond Polar Bond Polar Bond Polar Bond
Bond Polarity Bond Polarity Bond Polarity Bond Polarity Bond Polarity Bond Polarity
exist cancel exist cancel exist cancel
(Asymmetric) (Symmetrical) (Asymmetrical) (Symmetrical) (Asymmetrical) (Symmetrical)
✓✓✓
Which of the following molecules have hydrogen bonding?
CH3CHO CH3COCH3 CH3COOH CH3OCH3 CH3NH2 CH3CONH2
Hydrogen NOT No Hydrogen Bond Hydrogen attach No Hydrogen Bond Hydrogen attach Hydrogen attach
attach to N,O,F to N, O, F to N, O, F to N, O, F
✕ ✕✓ ✓ ✓✕
✕ ✕ ✕
40. Acknowledgements
Thanks to source of pictures and video used in this presentation
Thanks to Creative Commons for excellent contribution on licenses
http://creativecommons.org/licenses/
Prepared by Lawrence Kok
Check out more video tutorials from my site and hope you enjoy this tutorial
http://lawrencekok.blogspot.com