BONDING
Electronegativity
Electronegativity
•
• Atomic propAtomic property : how tightly an erty : how tightly an atom holds onto itatom holds onto it electrons
electrons •
• An atom with An atom with higher electronehigher electronegativity has stronger pullgativity has stronger pull on electrons than an atom
Electronegativity
• If two atoms come together to form a bond the atom with higherelectronegativity will attract the electrons away from the atom with lower electronegativity
• !he degree to which the electrons are attracted to the more
Electronegativity
• $eriodic table %the $auling electronegativity of the
elements&
• $eriodic table %the $auling electronegativity of the
$rimary Bonds
• )aterial are not made of individual atoms they are made of
groups of atoms#
• Groups of all *ind of atom %a piece of iron&
• Groups of di"erent *inds of atoms %polyethylene made of carbon
and hydrogen&
• !he bonds that form between the atoms have signi+cant
in,uence on the material-s properties#
• Eg# )elting point sti"ness thermal e.pansion : directly related to
the strength of bonds
• relationship between structure / properties : understadnig
$rimary Bonds
• One way to de+ne chemical compounds is that they are
groups of atoms held together by primary bonds#
• !hree basic types of primary bonds: each of them
formed by di"erent ways of sharing the electrons to
satisfy the octet rule %atoms are most stable when they have +lled valence shell which for many atoms means 0 electrons e.ception is hydrogen&
$rimary Bonds
• Ionic bond: Bond form when electron is transferred from
one atom to another to satisfy the octet rule for each of them resulting in positive and negative ions#
• !hese ions are then attracted to each other through
electrostatic interactions
• Ionic bonds are the strongest bonds and melting
temperatures of ionic compounds are the highest of any materials
$rimary Bonds
• 1ovalent bond: Bond formed when two atoms have
share electron e2ually#
• !hese atoms are then bound together because the
octet rule is satis+ed only while share electrons are considered to be in the valence shell of both atoms#
• 1ovalent bonds are considered strong but generally
$rimary Bonds
• )etallic bond: Bond formed when a group of atoms
contribute their valence electrons to form 3sea of electrons4 around the atoms#
• !he octet rule is satis+ed on average for all the atoms# • )etallic bonds are considered to be the wea*est of the
primary bonds although some metals can form bonds that are stronger than covalent bonds#
$rimary Bonds
• 5se you *nowledge of electronegativity to predict the
types of bonds that will form between atoms#
$rimary Bonds
• 6hat *ind of primary bonds in the compounds 1a78 and
GaN(
• 3'ow big of a di"erence in electronegativity is needed for a bond to be ionic(4 • In reality electron are not shared e.actly e2ually between two atoms
because one will have a higher electronegativity than the other %e.cept diatomic molecules with the same atoms eg# N8&
• !his means always some ionic character to a covalent bond# • !he 9 ionic character of a bond:
• 9ionic character ;<< = %;>e.p%><#8?%ENA @ ENB&8&& where ENA and ENB :
electronegativity of the two atoms limitation: only compares the ionic and covalent characters of the bonds#
$rimary Bonds
• Another way to loo* at the type of bonding is through
the bond>type triangle#
• 1onsiders both the electronegativity di"erence between
the two atoms and the average value of the
electronegativities of the two atoms to determine the bonding type#
$rimary Bonds
Bond-type triangle, showing the regions for metallic (M), semimetallic (SM), covalent (C), and ionic (I) bonding as a function of the average electronegativity and electronegativity difference for the
'ow to use this triangle( Bond character
Interaction
• Nonbonding interactions 3secondary bonds4
• econdary bonds not actually bond confusing# term
3nonbonding interactions4
• 5nli*e primary bond nonbonding interactions do not result
from sharing of electrons#
• !hey occurs because of attraction between partial charges
that are present in the molecules and much wea*er than primary bonds
Interaction
• !ypes of nonbonding interactions and strength of the
Interaction
• 'ydrogen bond: Occurs between o.ygen nitrogen or
,uorine on one molecule and hydrogen atoms on
another molecule that are bound to o.ygen nitrogen or ,uorine#
• !his is the strongest nonbonding interaction# • Cemember commonly called 3bond4 it is not a
primary bond it is a nonbonding interaction#
Schematic diagram of hydrogen bonds
Interaction
• $ermanent dipole: Occurs when a very electronegative atoms forms a covalent bond with a less electronegative atom resulting in partial positive and negative charges in the molecule#
• !he partial charges on the this molecule can then interact with the partial charges on another molecule forming a permanent dipole interaction#
Interaction
• Induced dipole: !his type of
interaction is formed by random ,uctuations in the electron
distribution in atoms#
• A random ,uctuation results in
partial positive and negative regions on an atom#
• !he charges that are randomly
crated on this atom can attract or repel electrons on a nearby atom resulting in a wea* attraction
between the atom#
Interaction
• !he di"erence between primary bonds and nonbonding
interaction(
• Bonds vs# Nonbonding Interactions#
• 6hat *inds of primary and nonbonding interactions are present
Interaction
• 'ow primary bonds and nonbonding interactions a"ect
properties(
• 'ow their structure a"ect their boiling points( • Bonding and $roperties#
ummary
• 7undamental atomic properties of electronegativity has an important
in,uence on materials properties#
• !he way in which atoms interact as de+ned by electronegativity
a"ects both primary bonds and nonbonding interactions which in turn a"ect the properties#
• 'ere we discuss about only boiling point as a properties#
• Ne.t we will discuss how bonding can also be used to e.plain
engineering properties such as sti"ness and thermal e.pansion#
• 1onnection among electronegativity bonding and properties that we
discussed illustrates an important aspect of materials science and engineering properties#
• 5nderstanding this connection allows us to predict and control the
1rystalline defects
• ;: Fist and describe in your own words three types of point
defect in crystals#
• 8 : Fist and describe in your own words three types of line
defect in crystals#
• : Fist and describe in your own words three types of planar
defects in crystals#
• Individual Assignment ( Material Science Group 1 : Submit
on 29 Sept during class, Material Science Group 2: Submit on 30 Sept during class