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Chapter 3.6 Periodic Table
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the topic of this video is the periodic table
table
the learning objectives are on your
screen before jumping into the modern
view of the periodic table it's
worthwhile to mention briefly the some
historical aspects of the periodic table
the person shown in the figure on the
left is dimitri mendeleev he is largely credited
credited
for inventing the periodic table
another scientist around the same time
named lothar meyer in germany
is is also credited with independently
recognizing that there
were periodic relationships among
properties of elements
at that time although mendeleev by far
gets the most recognition
um it's it's remarkable to think that
uh at the time this is the late 1800s so
this is before
the likes of of um
einstein and max plunk and
de broy and schrodinger uh before
the the the advent of quantum mechanics and
and
and wave particle duality and
electron configurations before
those um concepts had been crystallized
um scientists such as mendeleev
and both our meyer were able to
categorize elements based off of their properties
properties
to to and it was so successful that they
could actually
predict missing elements that had not
yet been discovered
but again these were the the original
periodic table was created
to list elements by their
similar properties not necessarily by an
atomic number or valence electrons or
anything along those lines
now we can jump forward to the modern
periodic table which is on your screen
and also the periodic law the periodic
law states that the properties of the elements
elements
are periodic functions of their atomic
numbers so this
gives us a more concrete way to organize
elements in the
i should point out here that in an
earlier video
i had mistakenly referred to the vertical
vertical
columns as periods whereas the vertical
columns here
in the periodic table are groups okay so groups
groups
are the columns running up and down the
the periodic table
and then the periods are actually the
rows okay so here we have
seven periods in the modern periodic table
table
and we have 18 groups
okay so i just thought i'd point that
out in the electron configuration video
i was mistakenly calling groups periods
and i guess that's just a good lesson it
can be easy to get these mixed up
so come up with some sort of um
strategy to to make sure that you can
remember which are which
but oftentimes it's it's labeled in a
periodic table so
maybe i don't have an excuse we can also
look at different
element types so down here is a color code
code
for metals metalloids and nonmetals what
you'll notice is that
the vast majority of elements in the
periodic table that i'm circling
now fall within the
metal category so
the vast majority of elements that we know
know
are actually metals this pink
uh region in between i'll maybe change colors
colors
to here this this area here
between metals and non-metals it has
elements that we refer to as metalloids
they have characteristics that are
somewhat metallic but also somewhat non-metallic
non-metallic
um and then in the green we have the
nonmetals and that's
including hydrogen over here
maybe i'll change color one more time
so uh over here we have our
non-metals okay
so yeah one way to to remember
um the the this division between metals
metalloids and nonmetals is to
um memorize the metalloid elements and
you can remember that those elements to
the left
are going to be metals and those to the
right in the main group are going to be nonmetals
nonmetals
um so we can also assign some names
to break down the main group elements a
little bit more
here i'm going to change my color yet
again okay
so uh we have looked at main group
elements before but now group one we're
going to define
as um alkaline metals
okay so group one are alkaline metals
these are things like sodium
and lithium and even hydrogen and these
tend to form
plus one cations because they can
they can readily lose one electron they
have low first ionization
energies they can lose one electron and
they ultimately want to get to that
to this noble gas electron configuration
by losing one electron alkali earth
metals have two electrons in their
valence shell
that's what you unifies their uh uh
chemical characteristics
so they tend to form plus two cations
this is the
these are uh elements like magnesium and
calcium okay so this is group two
alkali earth metals plus two cations
and uh keeping in mind that when they
lose both electrons in their valence
shell they will end up with the noble
gas configuration
if we jump over here to nicotines in group
group
15 this is now going to be things like
nitrogen and phosphorus these can readily
readily
gain electrons and they can
form sort of i'll say
as an example n three minus you know
they can accept up to three electrons
in order to achieve that noble gas configuration
configuration
um calcogens his next and group 16.
uh would be things like sulfur and oxygen
oxygen
so these can gain two electrons they're
only two
groups away from the noble gas
configuration so they tend to gain two electrons
electrons
halogens you might see the the general
theme here halogens something like fluorine
fluorine
or chlorine can accept one electron to
get the noble gas configuration
noble gases are considered noble because
they are relatively inert
we've already covered transition metals
and also
d-block metals and then also lanthanides
and actinides as the inner transition metals
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