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Quarter 2 Competency 2 | Draw an Atom Step by Step | Atomic Structure | MATATAG Science Grade 8 | LearningWithG | YouTubeToText
YouTube Transcript: Quarter 2 Competency 2 | Draw an Atom Step by Step | Atomic Structure | MATATAG Science Grade 8
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Video Transcript
Architects draw buildings. Engineers
draw machines. But what if you could
draw the very blueprints of matter
itself? You can. And starts with one
shape, the atom. Time to take your
[Music]
To understand atoms better, let's use
the bore or planetary model of the atom.
It shows two important parts. First, the
nucleus, the tiny dense center of the
atom. And second, the electron shells or
orbits that surround the nucleus.
Imagine a mini solar system where the
sun is the nucleus and the planets are
electrons moving around it in rings.
This model helps us visualize how atoms
are structured. The nucleus is what
keeps everything in the atom together.
It's where most of the atoms mass is
found. Inside the nucleus, there are
protons and neutrons.
Protons have a positive charge. Neutrons
have no charge. They are neutral. These
particles are packed tightly in the
center, working together to keep the
atom stable. Surrounding the nucleus are
the electron shells. This is where the
electrons are found. These electrons
move very fast around the nucleus. Kind
of like satellites orbiting a planet.
Each shell or orbit is actually an
energy level. The closer the shell is to
the nucleus, the lower the energy. The
farther it is, the higher the energy. So
electrons in the outer shells have more
energy than those in the inner shells.
These shells are labeled as n= 1, n= 2,
n= 3, and so on. Sometimes they're also
named as the k shell, l shell, m shell,
and so on. In theory, some atoms can
have up to seven shells ending at the Q shell.
shell.
Each shell can only hold a certain
number of electrons.
This is called the electron capacity of
a shell. To find out how many electrons
a shell can hold, we use this formula.
Maximum electrons is equal to 2 n^2
where n is the shell number or the
energy level.
Let's try computing it. For the first
shell, n= 1. 2 * 1^ 2 is equal to 2 electrons.
electrons.
Second shell n = 2. 2 * 2^ 2 is equal to
8 electrons.
For the third shell, n= 3. 2 * 3^ 2 is
equal to 18 electrons.
So as the shell number increases, its
capacity to hold electrons also increases.
increases.
But here's something interesting. For
the first 20 elements in the periodic
table, which are the ones we often start
with, the actual distribution of
electrons tends to follow a simplified
pattern. The 288 rule helps us remember
the electron arrangement for the first
20 elements of the periodic table.
Here's how it works. The first shell
holds two electrons.
The second shell holds eight electrons.
The third shell also eight electrons
even though it can actually hold more.
This isn't a strict rule. It's more like
a shortcut for beginners and it works
well for the lighter elements.
You may also hear it referred to as part
of the octet rule which says atoms tend
to have eight electrons in their
outermost shell. So beyond 20 the
patterns become more complex due to sub
levels but you will learn that in higher grades.
grades.
Let's learn how to draw an atom step by
step. We'll kept it simple and easy to follow.
follow.
Step one, identify the atomic number of
the element. This number tells us how
many protons and electrons the atom has.
Step two, draw a small circle for the
nucleus and inside you can write the
element symbol.
Step three, draw the electron shells or
energy levels around the nucleus.
Step four, distribute the electrons
following the 288 rule. We start from
the innermost shell and move outward.
This process helps us visualize the atom
structure and understand its behavior in reactions.
reactions.
Now let's apply the steps to draw an
actual atom. Let's try with our element
here oxygen. First we find its atomic
number that's eight. So oxygen has eight
protons in the nucleus and eight
electrons to place in the shells.
Step two, we draw a nucleus and label it
with oxygen symbol a capital O. Next, we
draw the electron shells. Let's draw one
shell for now. Let's start with the
first shell. That's the smallest
innermost layer where electrons can go.
It's like a tiny circle with just two
sits. So, we place two electrons there
to fill it completely. One here and one
beside it. That's it. full. No extra
space. Once the first shell has two, we
move on. Now we've got six more
electrons to place in the second shell.
The shell is bigger and it has four
spots where electrons like to sit.
Imagine four sets of chairs is space
around the table. Each pair can hold up
two electrons. But here's the trick. We
don't put both on a chair right away. We
go around the table and place one
electron per chair first. 1 2 3 4. Now
every chair has one electron. Then we go
back and add the last two electrons to
make pairs.
This pattern might feel a bit extra, but
it actually helps us understand how
atoms bond with others later on.
Next, we draw the atom for sodium.
Sodium has an atomic number of 11, which
means it has 11 electrons.
Now, let's write the symbol N in the
center of the nucleus. We currently have
two shells around it.
Let's fill in the electrons.
Two in the first shell,
eight in the second,
and one electron in the third shell. And
that's it.
Now let's try a simpler one. Helium.
Helium has two protons. So it has two electrons.
electrons.
That means it only needs one shell. And
that shell it's like a tiny bench with
just two seats. We place both electrons
there, one on each seat.
Now the bench is full. No more room. And
that's makes helium a very stable atom.
Now let's draw a larger atom. Calcium.
Calcium has an atomic number of 20. So
it has 20 electrons to fill the shells.
We'll need two electrons in the first shell,
shell,
eight in the second.
And although the third shell can
accommodate up to 18 electrons, the
octet rule says the outermost shell
can't have more than eight electrons.
And so we put eight in the third shell
and the last two in the fourth shell.
There are different ways to draw
electrons in atom diagrams. You can draw
them as dots or as X's, whichever is
easier to see. What matters most is
their correct placement in each shell.
Also, instead of drawing each atom, we
can simply write the electron
configuration as numbers.
For example, 281 for sodium and 287 for
chlorine. That means two electrons in
the first shell, 8 in the second, and 1
or 7 in the outermost shell. This method
is faster and just as informative. But
whether you use diagrams or numbers,
both show one powerful truth. Atoms
follow clear patterns. And now you know
how to see them.
Let's wrap things up. Let's take a final
look at what we've learned. The atom is
the smallest unit of matter, but it's
made of even smaller parts.
As its center is the nucleus, a dense
core containing protons and neutrons.
Surrounding the nucleus are the electron
shells where negatively charged
electrons move in specific energy levels.
levels.
We also practice drawing atoms by
showing the nucleus at the center and
placing electrons in their correct
shells based on the atomic number.
This shows us how matter is put
together. Atoms aren't just random dots.
They have parts that make them behave a
certain way. Next time we'll check out
protons, neutrons, and electrons and how
their properties affects an element's
identity and reactivity.
This is Learning with G. Stay tuned for
the next lesson. Please subscribe to my
channel for more science content. [Music]
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