Chemical Bonding: Covalent Bonding Lewis Dot Diagrams
Summary
TLDRIn this video, Miss Martins explains the concept of covalent bonding, focusing on how atoms share electrons to form stable molecules. She distinguishes covalent bonds from ionic bonds, emphasizing that covalent bonding occurs between non-metals. Miss Martins also demonstrates how to identify valence electrons using the periodic table and introduces Lewis Dot diagrams to visually represent bonding. The video covers examples like hydrogen, chlorine, and water molecules, showing how atoms share electrons to achieve stability. Viewers are encouraged to comment if they wish to see more content on double and triple bonds.
Takeaways
- đ§Ș Covalent bonding is defined as the sharing of electrons between atoms to form molecules or compounds.
- đŹ Covalent bonds occur between two non-metals, while ionic bonds occur between a metal and a non-metal.
- đ A quick way to identify covalent bonds in Lewis Dot Diagrams is the absence of brackets and charges, unlike ionic bonds.
- âïž Lewis Dot Diagrams visually represent how atoms bond, showing how they share or transfer electrons, especially focusing on valence electrons.
- 𧟠Valence electrons are the electrons in the outer energy levels of atoms and are involved in bonding.
- đ The number of valence electrons can be easily identified by looking at the group numbers on the periodic table.
- đ In covalent bonding, atoms share electrons to become stable and achieve a noble gas configuration (8 electrons in the outer shell, or 2 for hydrogen).
- đĄ Oxygen, with six valence electrons, needs two more to become stable, while hydrogen needs one more to fill its valence shell.
- đ Covalent bonds in molecules like H2 (hydrogen gas), Cl2 (chlorine gas), and H2O (water) involve sharing of electrons to make both atoms stable.
- â ïž Lone pairs refer to pairs of electrons that are not involved in bonding, which are present in molecules like water.
Q & A
What is covalent bonding?
-Covalent bonding is the sharing of electrons between atoms to form molecules or compounds.
Between what types of atoms does covalent bonding occur?
-Covalent bonding occurs between non-metal atoms.
How can you visually distinguish between covalent and ionic bonds in Lewis Dot diagrams?
-Covalent bonds do not show brackets or charges in Lewis Dot diagrams, while ionic bonds do.
What are valence electrons, and why are they important in bonding?
-Valence electrons are the electrons in the outermost energy level of an atom. They are important because they participate in chemical bonding.
How can you determine the number of valence electrons for an element using the periodic table?
-The number of valence electrons for an element can be determined by looking at the Roman group numerals on the periodic table.
Why do atoms in covalent bonds share electrons?
-Atoms share electrons in covalent bonds to achieve stability, aiming for a full outer energy level, similar to a noble gas configuration.
How many valence electrons does oxygen have, and how does this affect its bonding?
-Oxygen has six valence electrons, meaning it needs two more electrons to achieve a stable configuration. This leads oxygen to form bonds by sharing electrons with other atoms.
What is the significance of lone pairs in a Lewis Dot diagram?
-Lone pairs are pairs of electrons that are not shared in bonding. They remain on the atom and affect the shape and reactivity of the molecule.
How do hydrogen atoms achieve stability in a covalent bond?
-Hydrogen atoms achieve stability by sharing one electron with another hydrogen atom, resulting in each hydrogen having two electrons in total.
What is the difference between a single bond, double bond, and triple bond in covalent bonding?
-A single bond involves one pair of shared electrons, a double bond involves two pairs of shared electrons, and a triple bond involves three pairs of shared electrons.
Outlines
đ§Ș Covalent Bonding Basics
In this segment, Miss Martins introduces the concept of covalent bonding, emphasizing that it occurs between non-metal atoms. She explains how to identify metals and non-metals on the periodic table and how to distinguish between covalent and ionic bonds using Lewis Dot diagrams. The absence of brackets and charges in Lewis diagrams indicates covalent bonds, while the presence signifies ionic bonds. She also discusses the role of valence electrons in bonding, explaining how they are represented in Lewis Dot diagrams and how to determine the number of valence electrons using the periodic table or Aufbau diagrams. The segment ends with an example of how to draw Lewis Dot diagrams for elements like oxygen, sodium, and chlorine.
đ Drawing Lewis Dot Diagrams for Covalent Bonds
This paragraph delves into the process of creating Lewis Dot diagrams for covalent bonds, using hydrogen (H2), chlorine (Cl2), and hydrochloric acid (HCl) as examples. Miss Martins explains how to determine the type of bond by considering the elements involved and their positions on the periodic table. She then demonstrates how to represent the valence electrons of each atom and how they share electrons to achieve stability. The process involves counting the valence electrons, identifying the need for additional electrons to reach a stable configuration, and then showing how these electrons are shared between atoms to form single bonds. The segment also includes a brief overview of how to represent lone pairs in Lewis diagrams.
đ§ Covalent Bonding in Water
The final paragraph focuses on the covalent bonding in water (H2O). Miss Martins explains that water is a covalent compound because it involves non-metals (hydrogen and oxygen). She details the process of drawing the Lewis Dot diagram for water, starting with the representation of valence electrons for each hydrogen and the oxygen atom. She then illustrates how hydrogen shares its single electron with oxygen, which in turn shares two of its six electrons with the hydrogen atoms, forming two single bonds. The remaining four electrons on oxygen form two lone pairs. This explanation highlights the concept of single bonds and lone pairs in Lewis Dot diagrams, providing a clear visual of how the water molecule's structure is represented.
đ Further Exploration of Chemical Bonds
In the concluding remarks, Miss Martins invites viewers to engage with the content by liking, subscribing, and commenting if they are interested in learning more about double and triple bonds. She summarizes the key points covered in the video and encourages viewers to continue their exploration of chemical bonding.
Mindmap
Keywords
đĄCovalent bonding
đĄNon-metals
đĄPeriodic table
đĄValence electrons
đĄLewis Dot Diagrams
đĄSingle bond
đĄDiatomic molecules
đĄLone pairs
đĄNoble gas structure
đĄHydrogen molecule (H2)
Highlights
Introduction to covalent bonding: the sharing of electrons between atoms to form molecules or compounds.
Covalent bonding occurs between two non-metal atoms.
Key difference between covalent and ionic bonds: covalent bonds do not show brackets or charges in Lewis Dot diagrams.
Visualizing bonds: Lewis Dot diagrams help represent how atoms share or transfer electrons.
Valence electrons: the electrons in the outer energy levels of an atom involved in bonding.
Periodic table hack: the group number helps determine the number of valence electrons an atom has.
Drawing Lewis Dot diagrams: each valence electron is represented as a dot or cross around the atomic symbol.
Hydrogen only needs 2 electrons to be stable due to its single orbital, unlike most atoms that need 8.
Single bond formation: when two atoms share one pair of electrons.
Hydrogen molecule (H2) example: two hydrogen atoms share electrons to complete their outer shells.
Chlorine molecule (Cl2) example: each chlorine atom shares one electron to form a covalent bond.
Hydrochloric acid (HCl) example: hydrogen shares its electron with chlorine to stabilize both atoms.
Water molecule (H2O) example: oxygen shares electrons with two hydrogen atoms, forming two single bonds.
Lone pairs: unshared pairs of electrons that remain on the oxygen atom in water.
Call to action: Thumbs up and comments for more videos on double and triple bonds.
Transcripts
hello everyone and welcome to another
video with me Miss Martins and today
we're going to continue with chemical
bonding we're going to be focusing on
covalent bonding in the last lesson we
introduced chemical bonding and we
looked at the three different types if
you missed that lesson I'm going to link
it over here so you want to watch that
one first but today we're going to focus
on covalent bonding which we defined as
the shearing of electrons between atoms
to form molecules or compounds
it's very important to take note that
covalent bonding takes place between a
non-metal and a non-metal now how do I
know which atoms are metals or
non-metals
remember there's a dividing line on the
periodic table that separates Metals
which can be seen over here on this side
of the periodic table with non-metals
which can be seen on this side of the
periodic table just remember that little
hydrogen over here is actually a
non-metal if you get the Lewis Dot
diagrams of different molecules or
compounds the quickest way to see if
it's representing a covalent bond or an
ionic bond is with the absence or the
presence of brackets so what I mean by
that is you can see here in covalent
bonding this is water the hydrogen and
the oxygen are bonded covalently which
means they share electrons you do not
see brackets there you do not see
charges there over here ionic bonds you
can see brackets we can see charges this
is different this is ionic bonding we'll
get to ionic bonding in another video if
you want to see it just let me know down
below but that's just a quick visual way
to tell the difference between a Lewis
Dot Diagram that is representing
covalent bonding versus a Lewis Dot
Diagram that is representing ionic
bonding I keep going on about Lewis Dot
diagrams but what the heck are those
basically Lewis Dot diagrams are a
visual representation of how atoms bond
with one another it shows how they share
electrons if they have a covalent bond
or how electrons are transferred if we
are talking about an ionic bond and
Lewis Dot diagrams always works with the
valence electrons valence electrons are
the electrons found in the outer energy
levels of an atom a very quick way to
tell the number of valence electrons
that an atom has if you look at your
periodic table is to look at the Roman
group numerals that is located here on
your periodic table so for example you
can see here to my right boron has three
valence electrons remember we can also
look at an awful diagram in order to
tell how many valence electrons an atom
has so if you draw the off-bar diagram
for oxygen again if you don't know how
to do this or if you're looking for a
recap on off-bar diagrams I'll link my
video on Alpha diagrams over here we
will see that the outer energy level
which is energy level 2 is not full
energy level 2 has 1 2 3 4 5 6 electrons
because these are the electrons in the
outer energy level we also call them
valence electrons and those are the
electrons that are going to be involved
in bonding so it's the valence electrons
that we draw in our Lewis Dot diagrams
so if I ask you to draw the Lewis Dot
diagrams for the following elements so
not compounds just elements this is how
it works for oxygen what we'll do is
we'll either use an off-bar diagram or
we'll look at our periodic table in
order to see that oxygen has six valence
electrons we draw six dots or six
crosses around oxygen we draw one on
each side so what I mean by that is we
go one two three four let me start at
the top again five and six in total an
atom has space for eight okay which
means that oxygen has an open space over
here and an open space over here it
needs eight electrons in its outer
orbital in its outer energy level in
order to be full but it doesn't have it
it only has six so if I want to do
sodium
we look at sodium on the periodic table
sodium is in group one it's over here we
know that that means that it has one
valence electron it'll have one dot or
cross it doesn't matter where you draw
it I'm just going to do it on the right
hand side so one dot or one cross let's
look at chlorine
chlorine is over here
and as we can see chlorine has seven
valence electrons that you start this
time one two three four five six seven
remember it has space for eight so he
has an open little Gap over here but
chlorine only has seven the reason they
share the electrons is to be stable they
want to reach that noble gas structure
they want to be stable and this is very
important you need to know this hydrogen
needs two in total to be full or stable
hydrogen and helium they only have a 1s
orbital so then they need two electrons
in total to be full or stable
everything else needs eight so if I ask
you to draw a Lewis Dot Diagram for the
hydrogen molecule or H2 or hydrogen gas
this is how you do it you first decide
whether it is an ionic or a covalent
bond it's very obvious that it is a
covalent bond because hydrogen is a
non-metal so a hydrogen and a hydrogen
will be two non-metals then what we do
is we think about the valence electrons
that each hydrogen atom has so one eye
this hydrogen atom has one electron
this hydrogen atom has one electron
because I have two hydrogen atoms I'm
going to use an X to represent the
electron in the first hydrogen atom and
adopt to represent the one valence
electron in the second then we think
about the following we said hydrogen
needs two in order to be full
each hydrogen only has one so what they
do is these hydrogen atoms share those
electrons with each other so we add
these together and my final compound you
draw them closer to each other and you
draw the shared electrons in the middle
now each hydrogen has two electrons so
this hydrogen on the left has two
electrons this hydrogen on the right has
two electrons and remember hydrogen only
needs two to be stable to fill its outer
energy levels so that is a single Bond
because they share one pair of electrons
this is why hydrogen is diatomic if we
look at chlorine or the chlorine
molecule cl2 again we know that this is
covalent bonding because chlorine is a
non-metal so we have a chlorine atom
with a chlorine atom two non-metals each
chlorine look at the number of valence
electrons each chlorine has seven
valence electrons so it has space for
one more remember it needs eight to be
stable
the second chlorine molecule also has
seven so one two three four five six
seven again another space it needs one
more electron to be full so think about
it they each have seven
they each need one more to be full so
these electrons over here these two over
here can be shared with one another
green electrons that are highlighted
they're going to pull to the middle
because they're going to be shared and
then you just fill in the other
electrons as normal this pair of
electrons over here you see it's a pair
which means it's a single Bond if they
share one pair of electrons they form a
single Bond and again here's a little
quick summary of the chlorine molecule
look at HCL or hydrochloric acid we know
that it is a covalent bond because
hydrogen is a non-metal I know it's on
the left hand side of the periodic table
but remember
hydrogen is an exception it's a
non-metal and chlorine is also a
non-metal hydrogen has one valence
electron you can see there by the Roman
group numeral
chlorine has seven
think about it hydrogen needs two to be
stable chlorine needs eight so hydrogen
needs one more chlorine needs one more
then they think oh cool we can just
share these with each other so you draw
them closer to each other and then the
things that they share
they go to the middle and that becomes
the shared pair of electrons so yeah you
can see one pair of electrons are shared
single Bond here is a nice summary for
you to understand them and then finally
let's do H2O or water again it's
covalent because hydrogen and oxygen are
non-metal so non-metal in a non-metal if
you think about this compound now we've
got one oxygen and two hydrogens so
this hydrogen has one valence electron
the second hydrogen also has one valence
electron plus our oxygen atom let's look
at oxygen oxygen has six valence
electrons now remember hydrogen needs
two to be stable so it has six
it needs two more it needs two more and
isn't it just perfect because it needs
two more it can share this one with that
hydrogen and this one with that hydrogen
and think about it that will also make
the hydrogens full and stable so I'm
going to draw the final molecule
molecule here oxygen will go in the
middle and it makes sense because oxygen
needs to share with this hydrogen and
this hydrogen so I'm going to fill in
everything else as is with oxygen just
like I had it initially
now you see over here I have an open
space that's where the first Hydrogen is
going to come closer and share that
electron in this open space the other
hydrogen is going to come closer and
share that electron now you have to
count the number of electrons around
oxygen you'll get eight and each
hydrogen has two it's basically like
this a single Bond over there and a
single Bond over there how do I know
it's two single bonds because this is a
single pair of electrons that's shared
over there which creates a single Bond
and a single pair of electrons that is
shared over there that creates a single
Bond these two electrons here that is
called a lone pair and we have another
two electrons over there which is
another lone pair another summary for
you and if you would like to see me do
double bonds and triple bonds please
give this video a thumbs up so that I
know you want to see more and comment
down below please don't forget to like
this video And subscribe to my channel
so that I know you want to see more of
this content
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