Chemistry Exam > Chemistry Videos > Inorganic Chemistry > Molecule behavior & electronic configuration - Chemical Bonding
Molecule behavior & electronic configuration - Chemical Bonding Video Lecture | Inorganic Chemistry
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FAQs on Molecule behavior & electronic configuration - Chemical Bonding Video Lecture - Inorganic Chemistry
| 1. What is the role of electron configuration in determining molecule behavior? |  |
Ans. The electron configuration of an atom determines its chemical properties and the way it interacts with other atoms to form molecules. The arrangement of electrons in the atom's energy levels determines the atom's stability, reactivity, and bonding behavior. For example, atoms with incomplete outer energy levels tend to gain, lose, or share electrons to achieve a stable electron configuration, resulting in the formation of chemical bonds.
| 2. How does chemical bonding influence molecule behavior? | |
Ans. Chemical bonding is the process by which atoms combine to form molecules. It determines the physical and chemical properties of substances. The type of chemical bond (ionic, covalent, or metallic) influences the strength and nature of the interactions between atoms in a molecule. These interactions affect the molecule's shape, polarity, stability, and reactivity, ultimately determining its behavior and properties.
| 3. What factors influence the formation of chemical bonds between atoms? | |
Ans. Several factors influence the formation of chemical bonds between atoms. These include the electronegativity difference between atoms, the number of valence electrons, and the stability that can be achieved through electron configuration. Electronegativity difference determines whether an ionic or covalent bond will form, while the number of valence electrons determines how many bonds an atom can form. Additionally, atoms tend to gain, lose, or share electrons to achieve a stable electron configuration, which drives bond formation.
| 4. How does electron configuration determine the shape of a molecule? | |
Ans. The electron configuration of the atoms in a molecule influences its shape. The arrangement of electrons around the central atom(s) determines the repulsion between electron pairs, which affects the bond angles and overall shape of the molecule. For example, in a molecule with a central atom surrounded by two bonding electron pairs and two non-bonding electron pairs (tetrahedral electron geometry), the repulsion between the non-bonding pairs causes a bent molecular shape.
| 5. What is the relationship between molecule behavior and intermolecular forces? | |
Ans. Intermolecular forces are the attractive forces between molecules and play a crucial role in determining the behavior of molecules. These forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding. The strength of intermolecular forces influences properties such as boiling point, melting point, solubility, and viscosity. Molecules with stronger intermolecular forces typically exhibit higher boiling points, lower vapor pressure, and stronger attractions between molecules, affecting their behavior in various chemical and physical processes.
Text Transcript from Video
hello friends this video on chemical
bonding part 30 is brought to you by
exam fear calm no words here from exam
before watching the video please make
sure you have watched part 1 to part
with u9y you must be wondering why did
we do so much electronic infliction what
information we are getting from
electronically so let us say this the
molecule will behavior can be predicted
from electronic computation stability of
molecules the bond order the nature of
bond the bond length magnetic character
all these things we can find using
electronic health officials will explain
this one by one all these things is in
fine if you know the electronic
condition per molecule so if let's
suppose my NB is a number of electrons
in bonding orbitals and na is my
antibonding orbitals then my molecule is
stable if my bonding is number of
electrons in bonding is greater than
number of electrons in any moment so in
my bonding electrons greater then anti
bonding electrons my Bala Quila still
quite reasonable also because I told
that bonding has lower energy and the
bonding has higher energy so if I have
more and more electrons in the bonding
orbitals that means my system is pretty
stable right and if it is it is stable
other way around if my antibonding
electrons calm this modem or the bond
order as I told in case of Lewis
definition the bond order was nothing
but the number of bonds but in this case
the bond order is nothing but 1 by 2 or
half the difference of the number of
electrons in bonding m and
gone out with nothing but 1 by 2 into n
V minus n BN v is nothing but number of
electrons in bonding electrons cb4
bonding a for and the body
- n n that is number of electrons in
antibonding so here was a positive bond
order means molecule stable and the
negative means negative or zero means
the molecule transitive correct because
we told that this passed a that means a
bonding molecule will be number number
of electrons in bonding maalik orbitals
will be there it to that number of
electrons in antibonding
so we talk about nature a bond so
integral bond order of value 1 2 3 is
generally for single double or triple
bond right this is generally something
which we learned the classical concept
but we have seen the resonance and
nominate in resonance we have something
called you get 1.5 as a bond order there
we talk about the resonance correct jv8
bond under is 1 you see it is single
bond to double bond 3 it will 1 plus 1.5
see it something up resonance when you
talk about bond length since till na'vi
I just got the bond or how to get the
bond length so Curie see is that the
bond order
can we take an approximate measure of
bond length that means we say that bond
length is inversely proportional to God
I never bond order higher the border
look at the warning and that is
something we have seen in the earlier
theories also for double bond the bond
length was less or triple bond the bond
length must all the more less and so
same thing here so when the bond or
whether we can have a fair idea of the
bond length also bond or try something
with V and easily find using molecule
orbital magnetic nature is something
which we can easily find and I saw in
this theory or a talked about oxygen
ring paramagnetic and
it's difficult to tell this column
identify the early theories but this
theory helps us to find the magnetic
nature example oxygen molecule rate will
tell you how to find this so it says
that if all the molecule orbitals in the
molecules are doubly occupied this
diamond ending and if one or more
molecular orbitals are singly occupied
it is paramagnetic so in case of its
para magnet is it will be at whatever
magnetic field if it is diamagnetic it
will be repaired by minding see all
right we'll take some examples where
we'll explain all the properties once
again right so we'll start with hydrogen
so hydrogen has hydrogen molecule is
nothing but my 2 hydrogen atom and
hydrogen my electronic configuration is
1 s 1 for hydrogen atom so I have one
atom here one electron here mounted on
it right so if you fill this this is 2
electron here so now if you see hydrogen
everything is filled let's let's find
the bone out of us born order is nothing
but 1 by 2 into number of electron
bonding minus number electron in
anti-bonding
so how are electron in bonding to
anti-bonding 0 so this becomes 1 that
means there is a single bond which you
can see that hydrogen has a single bond
correct also there is no one paid length
on all the electrons are paired so it is
dye money let us say helium so in case
of helium will have this structure so
helium is my helium molecule is nothing
but 1 to helium atom so helium atom my
electronic aggregation is 1s2 so let's
put two electrons here and two electrons
here correct so we'll have four
electrons let's tell for electrons in
this fashion so what is the bond order 1
by 2 into number of electron in bonding
- number
antibonding so this becomes 1 by 2 into
bonding electrons they are two
antibonding the star is 2 that becomes 0
so bond order is 0 that means it is not
stable and doesn't exist
correct listen there is no point finding
magnetic nature let's take barium
so for ve atom for ve atom my electronic
configuration is 1s2 2s2 correct so
let's put 1 s 2 2 s 2 1 st yesterday so
let's fill it for electrons unfilled
electrons all filled let's find the bond
order 1 by 2 number in Antibes our
bonding
- number in antibonding how many
electrons in bonding 2 + 2 4 write this
for antibonding the remaining 1 2 + 2 4
it also gives 0 that means it does not
exist it easy
lithium let's see lithium to exist or
not and if it exists what is the what is
parama into your diamond let's see this
so who are lithium it is 1s2 2s1 this is
my ETM atom electronic integration let
us put this 1 s 2 2 s 1 1 s 2 2 s 1 so
now let's put the value of therefore
electrons the for electron two electrons
both will be here let's write the word
bonding order 1 by 2 into n bonding - 10
Taconic how many bonding
this and this so forth antibonding the
remaining one - you get one that means
it is single one correct it is stable
and what about the magnetism is
paramagnetic or diamagnetic you see
there is no unpaired electron so it is
by my memory let's take with a carbon so
carbon is a six electron in the carbon
atom so 1s2 2s2 2p2 right this is the
carbon atom so let us put here 1s2 2s2
2p2 here of the same thing
correct so let's fill this for electron
more electrons now we have again four
electrons here right so one two three
correct
so let's find the Bohr model 1 by 2
integral ting - wanting one is
antibonding how many gardening gardening
this is bonding who is borning - 4 h 8 -
anti bonding is to this tree correct so
that means it is a carbon-carbon triple
bond so this is a mistake here 2 + 2 4
it is 4 here so 8 minus 4 by 4 is 2 that
is double bond also it is stable because
it is greater than 0 and there is no
unpaired electrons it is die - correct
let's take oxygen sick oxygen oxygen
atom has a polyfill
publication on 1s2 2s2 2p4 just when
this 1s2 2s2 2p4 one two three four
similarly here we'll say let's say
enhanced right now let's try this for
will this work for till this for now we
have eight one two three four five six
seven eighty right let's say the bonnet
over this one by two and bonding - inti
bonding
how many bonding two four six and four
ten ten
when's ND morning harmony two four six
right so you get that means there's a
double bond what about the magnetic
character I can see the unpaired
electron right so it is Fahrenheit since
unpaired electron unpaired electron over
there so it is tough correct
thank you visit exam viacom to watch
free education videos try free online
tests get the best quality study
materials study from the best tutors and
mentors and much more thanks and screen
bonding part 30 is brought to you by
exam fear calm no words here from exam
before watching the video please make
sure you have watched part 1 to part
with u9y you must be wondering why did
we do so much electronic infliction what
information we are getting from
electronically so let us say this the
molecule will behavior can be predicted
from electronic computation stability of
molecules the bond order the nature of
bond the bond length magnetic character
all these things we can find using
electronic health officials will explain
this one by one all these things is in
fine if you know the electronic
condition per molecule so if let's
suppose my NB is a number of electrons
in bonding orbitals and na is my
antibonding orbitals then my molecule is
stable if my bonding is number of
electrons in bonding is greater than
number of electrons in any moment so in
my bonding electrons greater then anti
bonding electrons my Bala Quila still
quite reasonable also because I told
that bonding has lower energy and the
bonding has higher energy so if I have
more and more electrons in the bonding
orbitals that means my system is pretty
stable right and if it is it is stable
other way around if my antibonding
electrons calm this modem or the bond
order as I told in case of Lewis
definition the bond order was nothing
but the number of bonds but in this case
the bond order is nothing but 1 by 2 or
half the difference of the number of
electrons in bonding m and
gone out with nothing but 1 by 2 into n
V minus n BN v is nothing but number of
electrons in bonding electrons cb4
bonding a for and the body
- n n that is number of electrons in
antibonding so here was a positive bond
order means molecule stable and the
negative means negative or zero means
the molecule transitive correct because
we told that this passed a that means a
bonding molecule will be number number
of electrons in bonding maalik orbitals
will be there it to that number of
electrons in antibonding
so we talk about nature a bond so
integral bond order of value 1 2 3 is
generally for single double or triple
bond right this is generally something
which we learned the classical concept
but we have seen the resonance and
nominate in resonance we have something
called you get 1.5 as a bond order there
we talk about the resonance correct jv8
bond under is 1 you see it is single
bond to double bond 3 it will 1 plus 1.5
see it something up resonance when you
talk about bond length since till na'vi
I just got the bond or how to get the
bond length so Curie see is that the
bond order
can we take an approximate measure of
bond length that means we say that bond
length is inversely proportional to God
I never bond order higher the border
look at the warning and that is
something we have seen in the earlier
theories also for double bond the bond
length was less or triple bond the bond
length must all the more less and so
same thing here so when the bond or
whether we can have a fair idea of the
bond length also bond or try something
with V and easily find using molecule
orbital magnetic nature is something
which we can easily find and I saw in
this theory or a talked about oxygen
ring paramagnetic and
it's difficult to tell this column
identify the early theories but this
theory helps us to find the magnetic
nature example oxygen molecule rate will
tell you how to find this so it says
that if all the molecule orbitals in the
molecules are doubly occupied this
diamond ending and if one or more
molecular orbitals are singly occupied
it is paramagnetic so in case of its
para magnet is it will be at whatever
magnetic field if it is diamagnetic it
will be repaired by minding see all
right we'll take some examples where
we'll explain all the properties once
again right so we'll start with hydrogen
so hydrogen has hydrogen molecule is
nothing but my 2 hydrogen atom and
hydrogen my electronic configuration is
1 s 1 for hydrogen atom so I have one
atom here one electron here mounted on
it right so if you fill this this is 2
electron here so now if you see hydrogen
everything is filled let's let's find
the bone out of us born order is nothing
but 1 by 2 into number of electron
bonding minus number electron in
anti-bonding
so how are electron in bonding to
anti-bonding 0 so this becomes 1 that
means there is a single bond which you
can see that hydrogen has a single bond
correct also there is no one paid length
on all the electrons are paired so it is
dye money let us say helium so in case
of helium will have this structure so
helium is my helium molecule is nothing
but 1 to helium atom so helium atom my
electronic aggregation is 1s2 so let's
put two electrons here and two electrons
here correct so we'll have four
electrons let's tell for electrons in
this fashion so what is the bond order 1
by 2 into number of electron in bonding
- number
antibonding so this becomes 1 by 2 into
bonding electrons they are two
antibonding the star is 2 that becomes 0
so bond order is 0 that means it is not
stable and doesn't exist
correct listen there is no point finding
magnetic nature let's take barium
so for ve atom for ve atom my electronic
configuration is 1s2 2s2 correct so
let's put 1 s 2 2 s 2 1 st yesterday so
let's fill it for electrons unfilled
electrons all filled let's find the bond
order 1 by 2 number in Antibes our
bonding
- number in antibonding how many
electrons in bonding 2 + 2 4 write this
for antibonding the remaining 1 2 + 2 4
it also gives 0 that means it does not
exist it easy
lithium let's see lithium to exist or
not and if it exists what is the what is
parama into your diamond let's see this
so who are lithium it is 1s2 2s1 this is
my ETM atom electronic integration let
us put this 1 s 2 2 s 1 1 s 2 2 s 1 so
now let's put the value of therefore
electrons the for electron two electrons
both will be here let's write the word
bonding order 1 by 2 into n bonding - 10
Taconic how many bonding
this and this so forth antibonding the
remaining one - you get one that means
it is single one correct it is stable
and what about the magnetism is
paramagnetic or diamagnetic you see
there is no unpaired electron so it is
by my memory let's take with a carbon so
carbon is a six electron in the carbon
atom so 1s2 2s2 2p2 right this is the
carbon atom so let us put here 1s2 2s2
2p2 here of the same thing
correct so let's fill this for electron
more electrons now we have again four
electrons here right so one two three
correct
so let's find the Bohr model 1 by 2
integral ting - wanting one is
antibonding how many gardening gardening
this is bonding who is borning - 4 h 8 -
anti bonding is to this tree correct so
that means it is a carbon-carbon triple
bond so this is a mistake here 2 + 2 4
it is 4 here so 8 minus 4 by 4 is 2 that
is double bond also it is stable because
it is greater than 0 and there is no
unpaired electrons it is die - correct
let's take oxygen sick oxygen oxygen
atom has a polyfill
publication on 1s2 2s2 2p4 just when
this 1s2 2s2 2p4 one two three four
similarly here we'll say let's say
enhanced right now let's try this for
will this work for till this for now we
have eight one two three four five six
seven eighty right let's say the bonnet
over this one by two and bonding - inti
bonding
how many bonding two four six and four
ten ten
when's ND morning harmony two four six
right so you get that means there's a
double bond what about the magnetic
character I can see the unpaired
electron right so it is Fahrenheit since
unpaired electron unpaired electron over
there so it is tough correct
thank you visit exam viacom to watch
free education videos try free online
tests get the best quality study
materials study from the best tutors and
mentors and much more thanks and screen
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Nov 16, 2024 Last updated |
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