This document discusses the different types of chemical bonds: ionic, covalent, coordinate covalent, metallic, and hydrogen bonding. Ionic bonds form between a metal and non-metal via the transfer of electrons from the metal to the non-metal. Covalent bonds form via the sharing of electron pairs between two non-metals. Coordinate covalent bonds involve the donation of an electron pair from one atom to another. Metallic bonds allow for delocalized electrons between metal atoms. Hydrogen bonding is a weaker dipole-dipole interaction between a hydrogen atom and a highly electronegative atom. Each bond type results in compounds with distinct physical and chemical properties.

1. Chemical Bonding & Its Types
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2. Sr.No. C
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1. IntroductiontoChemical Bonding 3
2. IonicBonding 5
3. CovalentBonding 13
4. CoordinateCovalent Bonding 24
5. MetallicBonding 30
6. HydrogenBonding 32
7. Reference 39
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Tableof

3. □ Chemical Bond – the type of force that holds two or more atoms together. It is the
attraction betweenpositive nucleusandtheir negative electrons.
TypesofChemical Bond
□ All the elements differ with each other in their valence shell electronic configuration.
Sothe way in which they combine to form compounds also differs. Hence, there are
different types of chemical bonding possible between atoms which make the
molecules. Depending on the type of bond they show different characteristics or
properties.
□ Thereare3typesof bonds.
▪ Ionic Bond
▪ Metallic Bond
▪ Covalent Bond
ChemicalBonding
3

4. TypesofChemical Bond
4

5. ❖ This is the reaction between a
(anion) where
metal (cation) and non-metal
in the cation
transfers its valence electrons to the
anion due to electrostatic force in
order to makeit stable (octet rule).
❖ Its properties:
□ Hard
□ Highmelting point
□ Highboiling point
□ Brittle
IonicBonding
5

6. Ionic(or)Electrovalent bond
6
❖ An ionic bond is a chemical bond formed by the electrostatic attraction between
positive and negative ions. The bond is formed between two atoms when one or more
electrons are transferred from the valence shell of one atom to the valence shell of the
other atom.
❖ The atom that loses electrons will form a cation (positive ion) and the atom that gains
electronswill formananion(negativeion).
❖ These oppositely charged ions come closer to each other due to electrostatic force of
attraction andthusforman ionic bond.
❖ As the bond is between the ions, it is called Ionic bond and the attractive forces
being electrostatic, the bond is also called Electrostatic bond. Since the valence
concept has been explained in terms of electrons, it is also called as Electrovalent
bond.

7. IonicBonding
(Potassium) (Bromine)
K + Br +
K + Br
OtherExamples
Ktransferits
e
l
e
t
c
h
t
e
r
o
B
n
r
t
o
becominga
positiveion.
Now,Br
gainedan
electron
makingita
negativeion.It
alsoachievethe
octetrule.
Thusthey,formedtheKBrorthe
PotassiumBromide.
7
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8. Formationofionic bond
❖ Let usconsider two atoms Aand B. Let atom Ahasone electron in excessand atom Bhasone
electron lesser than the stable octet electronic configuration. If atom Atransfer one electron
to atom B, then both the atoms will acquire stable octet electronic configuration. Asthe result
of this electron transfer, atom A will become positive ion (cation) and atom B will become
negative ion (anion). ese oppositely charged ions are held together by electrostatic force of
attraction which is called Ionic bond or Electrovalent bond.
❖ In general, ionic bond is formed between a metal and non-metal. The compounds containing
ionic bonds are called ionic compounds. Elements of Group 1 and 2 in periodic table, i.e.
alkali andalkaline earth metalsform ionic compoundswhentheyreact with non-metals.
8

9. Illustration1–FormationofSodiumChloride
(NaCl)
9
❖ Theatomicnumberof Sodiumis 11andits electronic configurationis 2, 8,
1.It hasone electron excessto the nearest stable electronic configuration of anoble gas-
Neon. Sosodiumhasatendency to lose one electron from its outermost shell andacquire
astable electronic configurationforming sodiumcation (Na+
).
❖ Theatomicnumberof chlorine is 17andits electronic configurationis 2,8,
7. It has one electron less to the nearest stable electronic configuration of a noble gas-
Argon. So chlorine has a tendency to gain one electron to acquire a stable electronic
configurationformingchloride anion (Cl−
).

10. ❖ When an atom of sodium combines with an atom of chlorine, an electron is transferred
from sodiumatomto chlorine atomforming sodiumchloride molecule thusboth the atoms
achievestable octet electronic configuration.
10

11. Illustration2–FormationofMagnesiumChloride
(MgCl2
)
❖ The atomic number of Magnesium is 12 and the electronic configuration is 2, 8, 2. It
has two electron excess to the nearest stable electronic configuration of a noble gas-
Neon. Somagnesiumhasatendency to lose two electrons from its outermost shell and
acquire astable electronic configurationformingmagnesiumcation (Mg2+
).
❖ Asexplainedearlier two chlorine atomswill gaintwo electronslost bythe
magnesiumatomformingmagnesiumchloride molecule(MgCl2) 11

12. The nature of bonding between the atoms of a molecule is the primary factor that determine the properties of
compounds. By this way, in ionic compounds the atoms are held together by a strong electrostatic force that makes
the compoundsto haveits characteristic features as follows:
a.Physical state – ese compounds are formed because of the strong electrostatic force between cations and anions
which are arranged in a well-de ned geometrical pattern. us Ionic compounds are crystalline solids at room
temperature.
b.Electrical conductivity–Ionic compoundsare crystalline solids and sotheir ions are tightly held together. The ions,
therefore, cannot move freely, so they do not conduct electricity in solid state. However, in molten state and their
aqueous solutions conduct electricity.
c.Melting point–the strong electrostatic force between the cations and anions hold the ions tightly together, so very
highenergyis required to separatethem. Henceionic compoundshave highmelting andboiling points.
d.Solubility – Ionic compounds are soluble in polar solvents like water. ey are insoluble in non- polar solvents like
benzene(C6H6), carbontetra chloride (CCl4).
e. Density,hardnessandbrittleness–Ioniccompoundshavehighdensity andtheyare quite hard
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rapid and
because of the strong electrostatic force between the ions. But they are highly brittle.
f. Reactions– Ionic compounds undergo ionic reactions which are practically
instantaneous.
CharacteristicsofIonic compounds

13. ❖ Atomscancombinewith eachother bysharingthe unpaired electrons in their outermost
shell. Each of the two combining atoms contributes one electron to the electron pair
whichis neededfor the bondformationand hasequalclaim onthe sharedelectron pair.
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❖ According to Lewis concept when two atoms between
them, each of the atoms attains configuration of the
nearestnoble gas.
form a covalent bond
the stable electronic
❖ Since the covalent bond is formed because of the sharing of electrons which become
commonto boththe atoms,it is alsocalled asatomic bond.
❖ Covalentbondsareformedby:
a. Overlapof hybridorbitals with atomic orbitals
b. Overlapof hybridorbitals with other hybrid orbitals
Covalentbond

14. Threetypesof Covalent Bonds…
❖ SingleBond:Asingle covalent bondis formed whentwo atoms bondand share asingle
pair of electron.
❖ DoubleBonds:Atype of covalent bondin which two electron pairs are sharedbetween
two atoms.Eachatomcontributestwo electronsto the bond.
❖ Triple Bonds: A covalent bond in which three electron pairs are shared between two
atoms.(their valenceelectronsareassociatedwith how manypairstheycancreate)
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CovalentBonding

15. S
ingle
Bond
Double
Bond
E
15
X
A
M
TripleBond
P
L
E
S
:
ExamplesofThreeTypesofCovalent
Bonds

16. ❖ Let usconsidertwo atomsAandB. Let atomAhasonevalence electron andatomB
has seven valence electrons. As these atoms approach nearer to each other, each
atom contributes one electron andthe resulting electron pair fills the outer shell of
both the atoms. Thus both the atoms acquire a completely filled valence shell
electronic configurationwhichleadsto stability.
FormationofCovalent bond
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17. Illustration1–Formationofhydrogen molecule
(H2)
❖ Hydrogenmolecule is formed bytwo hydrogenatoms.Eachhavingone valence electron
(1s1
), it is contributed to the sharedpair andboth atoms acquire stable completelyfilled
electronic configuration.
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18. Illustration2–Formationofchlorine
molecule(Cl2)
❖ Chlorine molecule is formed by two chlorine atoms. Each chlorine atom has seven
valence electrons (2,8,7). These two atoms achieve a stable completely filled
electronic configuration(octet) bysharingapair of electrons.
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19. Illustration3–Formationofmethane molecule
(CH4)
❖ Methane molecule is formed by the combination of one carbon and four hydrogen
atoms. The carbon atom has four valence electrons (2, 4). ese four electrons are
shared with four atoms of hydrogen to achieve a stable electronic configuration
(octet) by sharing a pair of electrons.
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20. Illustration4–Formationofoxygen molecule(O2)
❖ Oxygenmolecule is formed bytwo oxygenatoms. Each oxygenatom hassix valence
electrons (2,6). These two atoms achieve a stable electronic configuration (octet)
by sharing two pair of electrons. Hence a double bond is formed in between the
two atoms.
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21. Illustration5–Formationofnitrogen molecule
(N2)
❖ Nitrogen molecule is formed by two nitrogen atoms. Each nitrogen atom has five
valence electrons (2, 5). These two atoms achieve a stable completely filled
electronic configuration (octet) by sharing three pair of electrons. Hence a triple
bondis formedin betweenthe two atoms.
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22. Sigmav/sPiBond
❖ Sigma (σ) bonds are the strongest type of
bonds in the covalent bonding. They are
formedbyhead- on overlapping
between
valence
atomic
atomic
orbitals. The
orbitals of the two atoms which
share the electrons overlap or
merge end to end.
❖ Pi(π) bonds, on the other hand, are
weaker bonds and they are formed
when parallel orbitals overlapped
to share the electrons.
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23. CharacteristicsofCovalent compounds
a.Physicalstate–Dependingon force of attraction between covalent molecule the bond may
be weaker or stronger. Thus covalent compounds exists in gaseous, liquid and solid form.
E.g. Oxygen-gas;Water-liquid: Diamond-solid.
b.Electrical conductivity – Covalent compounds do not contain charged particles (ions), so
theyarebadconductorsof electricity.
c. Meltingpoint–Exceptfew covalentcompounds(Diamond,Silicon carbide),
they have relatively low melting points compared to Ionic compounds.
d.Solubility – Covalent compounds are readily soluble in non-polar solvents like benzene
(C6H6), carbontetra chloride (CCl4). eyareinsoluble in polar solventslike water.
e. Hardnessandbrittleness–Covalentcompoundsareneither hard nor
brittle. Buttheyaresoft andwaxy.
f.Reactions – Covalent compounds undergo molecular reactions in solutions and these
reactions are slow.
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24. ❖ In the formation of normal covalent bond each of the two bonded atoms contribute one
electron to form the bond. However, in some compounds the formation of a covalent bond
between two atoms takes place by the sharing of two electrons, both of which comes from
only one of the combining atoms is bondis called Coordinate covalent bond or Dative
bond.
❖ Mostly the lone pair of electrons from an atom in a molecule may be involved in the dative
bonding.
❖ The atom which provides the electron pair is called donor atom while the other atom which
accepts the electron pair is called acceptor atom. The Coordinate covalent bond is
represented byanarrow (→ ) which points from
the donorto the acceptor atom.
CoordinateCovalent Bond
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25. ❖ Let usconsidertwo atomsAandB. Let atomAhasanunsharedlone pair of electrons
and atom Bis in short of two electrons than the octet in its valence shell. Now atom
A donates its lone pair while atom B accepts it. Thus the lone pair of electrons
originally belongedto atom Aare nowsharedbyboth the atomsandthe bondformed
bythis mutualsharingis called Coordinatecovalentbond. (A→B)
FormationofCoordinateCovalent Bond
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26. Illustration1–Formationofcoordinate covalent
bondbetweenNH3 → BF3 molecules
❖ In some cases, the donated pair of electrons comes from a molecule as a whole which is already
formed to another acceptor molecule. Here the molecule ammonia (NH3) gives a lone pair of
electrons to Boron trifluoride (BF3) molecule which is electron deficient. Thus a Coordinate
covalent bond is formed between NH3 (donor molecule) and BF3 (acceptor molecule) and is
represented byNH3→ BF3.
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27. Characteristicsofcoordinatecovalent compounds
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Thecompoundscontainingcoordinate covalentbondsarecalled coordinate compounds.
a. Physicalstate–Thesecompoundsexist asgases,liquids orsolids.
b.Electricalconductivity–Like covalentcompounds,coordinate compoundsalsodonot contain charged
particles (ions), sotheyarebadconductorsof electricity.
c.Meltingpoint–Thesecompoundshavemelting andboiling pointshigherthanthoseof purely covalent
compoundsbut lower than those of purely Ionic compounds.
d.Solubility–Insoluble in polar solventslike water but aresoluble in non-polar solvents like benzene,CCl4,
and toluene.
e.Reactions– Coordinate covalent compounds undergo molecular reactions which are
slow.

28. BondinginElectronDeficientMolecules
❖ Theclassof compoundswhich havestrongtendencyto acceptelectrons becausethey
havetoo few electrons to provide atotal count of electrons required for nextinert gas
configurationarecalled electron deficient molecules.
❖ Examples :
BF3,AlCl3, Diborane (BH3)2.
❖ BF3is electron-deficient compound. In BF3, due to pπ−pπ bonding form filled 2p
orbital of F to vacant 2p orbital of B, electron deficiency is reduced, thereby
increasingthe stability of BF3molecule. Dative covalentbondis presentin BF3.
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29. ❖ Aluminium chloride exists as Al2Cl6 and this dimeric structure is held through
chlorine bridges. Chlorine atoms donate a pair of electrons to electron deficient
aluminium atoms.
❖ Therearedative covalentbondsbetween2AlCl3
❖ m
D
o
a
t
l
e
i
v
c
e
u
l
c
e
o
s
v
.
a
l
e
n
t bonds form when 2 distinct atoms with a difference of
electronegativity below 1.7 (i.e either able to form covalent bondsor polar covalent
bonds) share anelectron pair that only comesfrom one of the atoms. In this case, 2
atomsof chlorine sharetheir lone pairsof electronsto 2other aluminium atoms.
BondinginElectronDeficientMolecules
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30. MetallicBonding
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❖ The kind of bonding between metallic elements in which the valence electrons can
move freely from one atom to another. Since they can move freely they are called
delocalized electrons. They do not share, lose or gain electrons. Their valence
electronsforma"sea”of electrons.
Properties:
❖ Highmeltingandboiling points
❖ Electrical andheat conductor
Examplesofmetalelements:
❖ Lithium, Magnesium,Sodium etc.

31. MetallicBonding
31

32. ❖ Hydrogen bonding refers to the formation of Hydrogen bonds, which are a special
class of attractive intermolecular forces that arise dueto the dipole-dipole interaction
between ahydrogenatomthat is bondedto a highly electronegative atomandanother
highlyelectronegative atom while lies in the vicinity of the hydrogenatom.
❖ For example, in water molecules (H2O), hydrogen is covalently bonded to the more
electronegative oxygen atom. Therefore, hydrogen bonding arises in water molecules
due to the dipole-dipole interactions between the hydrogen atom of one water
molecule andthe oxygenatomof anotherH2O molecule.
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HydrogenBonding

33. ExamplesofHydrogen Bonding
❖ HydrogenBondinginHydrogen fluoride
Fluorine having the highest value of
electronegativity forms the strongest
hydrogen bond.
❖ HydrogenBondingin Water
A water molecule contains a highly
electronegative oxygen atom linked to the
hydrogen atom. Oxygen atom attracts the
shared pair of electrons more and this end of
the molecule becomes negative whereas the
hydrogenatomsbecome positive.
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34. ❖ HydrogenBondingin Ammonia
It contains highly electronegative atom nitrogen
linked to hydrogen atoms
❖ HydrogenBondinginAlcoholsand Carboxylic
acid
Alcohol is a type of an organic molecule which
contains an -OH group. Normally, if any
molecule which contains the hydrogen atom is
connected to either oxygen or nitrogen directly,
then hydrogenbondingis easily formed.
HydrogenBondingin Alcohols
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HydrogenBondinginCarboxylic acid
HydrogenBondingin Ammonia
ExamplesofHydrogen Bonding

35. There are two typesof Hbonds,andit is classified asthe following:
❖ Intermolecular Hydrogen Bonding
❖ Intramolecular Hydrogen Bonding
IntermolecularHydrogenBonding
❖ When hydrogen bonding takes place between different molecules of the same or
different compounds, it is called intermolecularhydrogen bonding.
❖ For example –hydrogenbondingin water, alcohol, ammonia etc.
IntramolecularHydrogen Bonding
❖ The hydrogenbonding which takes place within amolecule itself is called intramolecular
hydrogen bonding.
❖ It takes place in compounds containing two groups such that one group contains
hydrogen atom linked to an electronegative atom and the other group contains a highly
electronegative atomlinked to alesser electronegative atomof the other group.
❖ The bond is formed between the hydrogen atoms of one group with the more
electronegative atomof the othergroup
TypesofHydrogen Bonding
35

36. ExampleofIntermolecular&Intramolecular Hydrogen
Bonding
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37. StrengthoftheHydrogenbond
37
❖ The hydrogen bond is a weak bond. The strength of hydrogen bond is in-between
the weakvander Waalsforces andthe strongcovalent bonds.
❖ The dissociation energy of the hydrogen bond depends upon the attraction of the
sharedpair of electronsandhenceonthe electronegativity of the atom.

38. PropertiesofHydrogen Bonding
❖ Solubility: Lower alcohols are soluble in water because of the hydrogen bonding which can take place
between water andalcohol molecule.
❖ Volatility: As the compounds involving hydrogen bonding between different molecules have a higher boiling
point, sotheyare less volatile.
❖ Viscosity and surface tension: The substances which contain hydrogen bonding exists as an associated
molecule. So their flow becomes comparatively difficult. They have higher viscosity and high surface
tension.
❖ The lower density of ice than water: In the case of solid ice, the hydrogen bonding gives rise to a cage-like
structure of water molecules. As a matter of fact, each water molecule is linked tetrahedral to four water
molecules. The molecules are not as closely packed as they are in a liquid state. When ice melts, this case
like structure collapses and the molecules come closer to each other. Thus for the same massof water, the
volume decreasesanddensityincreases.Therefore, ice hasalower densitythan water at 273K.
That is whyice floats.
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39. Reference
❖ Iqbal, M. Z. (1995). Inorganic Chemistry (for B.Sc
Students),Ilmi Kitab Khana.
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