okay uh
welcome to lecture here
we are continuing on here uh with uh
chapter two i think
we're gonna start here in just a second
and uh
see most you're putting here in the chat
box so thank you very much for the role
there
everybody in
okay so as you uh as you know we are
having a quiz today
and again the plan is i'm going to
lecture here for a little bit
uh we'll stop lecture early you then
could go
on to canvas and through proctorio like
that proctoral practice quiz
uh you could take the quiz and then you
could go off to
either lab our discussion
uh at seven so we're gonna do a little
bit of lecturing here and like i said
we'll stop
early and with should give you plenty of
time to kind of go do that
and then again if you have lab today
obviously you need to go to lab
and if you have a discussion you come
back with me about seven
and for discussion
there's a time limit it's about 25
minutes to quiz so you got about 25
minutes to take quiz
and uh which should be plenty of time i
believe
and uh again we'll stop early enough for
you to do that and everything
it is uh based on uh i gave several
quizzes this week but i believe it's
based on uh
for our class uh it is chapter one
is what it's on for our class
uh basically the significant figures
conversions density
temperature uh i think that was all
chapter ones up
i will be posting monday's lecture it
just um
something happened with the recording so
i just got to fix it and then
i'll get it up there probably sometime
today or tomorrow the latest will be up
there
with that recording
okay uh you do need a calculator uh you
do need
you might need something to write with
uh to work out a couple of the problems
uh but yeah you need a calculator or
something you know a scratch piece of
paper maybe to work out some problems
and uh you'll be given some conversions
and pretty much that's all you need you
don't need a periodic table on this one
so you won't
you won't be given a periodic table
again you need to take it using the
chrome
the webcam and the proctorial
thing as well when you do it
okay we'll talk a little bit about
the quiz and sort of the process that
you need to do when we stop
and um we'll talk about it towards the
end but let's get going on some
lecturing here
uh also because monday's a holiday i
think as well uh so let's do that
okay so we were talking about electrons
and uh we're talking about basically
where electrons are in the atom and sort
of how they are
we're kind of getting into the process
of sort of their order and everything
in terms of their locations and as we
sort of finished up on
they pretty much could be in sort of two
locations or
not two locations but they could be in a
few different locations and these sort
of referred to as orbitals
and they're sometimes referred to as
atomic orbitals
and that is s p d
and f and if remember when we talk about
orbitals these are really the
theoretical places in an atom where
an electron could be housed and
every individual orbital no matter which
one it is so for example represented by
these little lines here
every individual orbital could only hold
a maximum
of two electrons and when we talk about
s
orbitals there's only one type of s
orbital
which means you can max out an s
orbital with two electrons
now that's different than p orbitals
there's actually three different types
of p
orbitals and since there's three
different types of p orbitals
each one could hold two so that is six
electrons if you max them out
d orbitals there's five different types
and each one could hold two electrons
which means you can max it out at 10
electrons
and f orbitals there's seven different
types
and if you max them out that would be 14
electrons in that case
uh when we talk about sort of a couple
of things here
uh this is like our n equals one n
equals
two that's the energy levels three
n equals four and these are sometimes
really referred to
as if you take the whole entire thing
here this is sometimes referred to as a
level
or a shell it's sometimes referred to
and for example on the n equals two
shell or level that's kind of the second
energy level
n equals one is the lowest in energy
closest to the nucleus
and as you
three p orbitals together this is what
is sometimes referred to as a
sub level or a sub shell
just like this here would be the 3d
sub shell
over here this would be the
4p subshell
and that's different again if i was
talking about the n equals 4
or n equals 3 level our shell that would
be
everybody that's contained in there
as you go through here so
one way you could kind of quickly
calculate the maximum number of
electrons
on a shell or level
is to take two times n squared and is
that principal quantum number which is
the energy level
you square it and then times it by two
so for example if we did the
n equals two level two squared
is four
and four times two is eight and what
that means is if we filled up this
entire level
with electrons we would max out at a
grand total of
eight electrons if you filled in the
whole entire row there
would be eight electrons so
it's really important to know that
basically acids could hold two
p sub shells could hold three i have six
electrons total
d sub shells could hold 10 and f
subshells could hold
14 electrons now if you know that
and we're going to talk about sort of
the order that occurs how these
electrons go in electrons pretty much go
in at lowest energy
until that's field goes to the next
energy level next energy level keeps
going
uh higher in energy until pretty much
all the electrons have been distributed
now before i scribble all over this
this is what all the energy levels look
like
in say hydrogen where there's only one
electron
and what you see in here again before i
scribbled all over it
is everything with the three for example
that three represents the
n equals three and that basically tells
you it's on the third energy level
and all the guys that have threes are
exactly equal in energy just like all
the ones that have
fours which tells you it's on the fourth
energy level
and one tells you it's on the first
energy level
but all these guys with the fours also
are perfectly equal in terms of energy
what actually happens to those uh shells
and subshells
uh as we put more electrons in
more than one electron is there's
actually a switch that occurs and again
just for reference sake you can kind of
see everything looks equal
when we get more electrons involved in
one
they're no longer equal and what that
affects is basically the
order at which electrons would go in
electrons would start here
at the bottom and they actually do go in
opposite of each other so if each of
these arrows represents an electron
one goes upwards one goes downward the
next one would go
here this is the next lowest in energy
the next one would go here to the p
there's actually three different p
orbitals in this subshell and just for
your you know how it goes they actually
go in
one at a time so they would first go in
one at a time just like this
and then they would come back and pair
up
and there's a rule that we really don't
talk too much about in here but there's
a rule that basically tells you
when there's more than one orbital
basically an electron will go in
one at a time and then come back and
sort of pair up
they would then go here it would then go
here again one at a time filling up
and coming back and pairing off and now
here's really where the change sort of
occurs
we can go from the 3p orbital the next
lows in energy is actually the
4s and that guy would get electrons
then we go back to the 3d and start
filling those guys up if necessary
so there's this sort of change that
occurs once we get more electrons in
and there's a thing that you can make uh
looks like this kind of from your book
or you have a similar one
um you could use this one and or you
could do this
and i'll just show you this is a really
easy thing that you can kind of recreate
what we talked about is on the first
energy level there's s's so you just go
1s
2s 3s 4s 5s
6s and 7s then you start with the ps on
the second
so 2p 3p 4p
5p 6p and 7p
then the ds happen on the third energy
level 3d
4d 5d 60
and the f's don't start until the fourth
energy level four
f and five f so this is something you
could kind of create really easily
and again if you start here and go down
one s two p
three d four f that's where these
orbitals first start
and we always start in terms of electron
configuration
kind of following the arrows and we
zigzag
back and forth and this will give you
the proper
order of how electrons go in when we
write something like electron
configuration
so if you know this which you should
know are how to create it like we just
did right there
and if you know that basically s of
maximum electrons
is 2 p is 6
d sub shell is 10 and 14
for our f's you should be able to write
any electron configuration that you
would need to do
so let us take a look at how to write
electron configuration
electron configuration is essentially
the order
at which the electrons are put into an
atom
and there's a special way that we sort
of write it and we're going to talk
about it here
in just a second but we're really
interested in the electrons so something
we talked about earlier
was that the atomic number is the number
of protons which is our
positive guy and remember that if we
were dealing with something that is
neutral
it would also equal the number of
electrons which are negative
so if we use the atomic number for an
element and it is neutral
the atomic number which is our number of
protons will equal the number of
electrons
so let us talk about how to write
electron configuration
so we're going to start with the easy
one here which is hydrogen and again
i'm just going to kind of recreate that
thing you may want to look at that thing
that we were just looking at just to
kind of show you
you know how it goes
let's recreate some of it here
all right so again we're always going to
start here no matter what you do
whenever you're starting electron
configuration you always want to start
there so here we have a atomic number of
one
which means it has one proton and thus
should also have one electron in this
case
so the electron configuration for
hydrogen would be 1s2
and what this means is this first number
is that principal quantum number which
is again a fancy word for
energy level
and again it's really just the energy
level
the s tells us what orbital
our subshell it's in so if you remember
we sort of talked about
these guys as being like maybe rooms on
a hotel
sort of where electrons could be and the
number on top
which should not be a2 i'm gonna erase
that i'm sorry about that
that should actually be a one thank you
got ahead of myself there it should
actually be one on top which is because
it only has one electron
so it should be one s1 and that is how
many electrons
are in the orbital r subshell
so the electron configuration should be
1s1
for hydrogen then this is how you should
write it
the one here is a big one small s
and the one up here is a superscript
no commas no weird thing people always
like to do
dashes i don't know other things that
people do
so that is how you should write it
continuing on to
number two on the periodic table which
has two protons also would have two
electrons
so again here starting up on top
we would come down to here and this
would be 1s
2 in this case
again energy level is the first number
the orbital that those electrons are in
and now the two electrons in that
particular orbital
which would be two now because that is
an
s orbital if you remember the 1s
pretty much is now filled
so any more electrons has to go to the
next orbital
that's available the next lowest energy
orbital
and that happens when we go to lithium
lithium is three which means it has
three electrons
and again here coming back to our thing
we would start here
it would be 1s 2
and now that we feel that we zigzag back
around
and we come to this guy and it would be
2s1
and so this guy here it would have a
configuration of
1s2 2s1
yeah so uh this is the orbital diagram
and we really don't do too much about
orbital diagram in this particular class
but just to kind of show you an orbital
diagram
is uh something looks like this so for
this particular guy
i'll just draw it this way not right in
terms of energy but i'll just do it this
way
and how the electrons would go in for
example is
one arrow would always go up first is
how you do it for the first electron
that goes in there
second arrow goes down and then when we
would go to the next orbital
the next electron would be signaled
upwards so it's always
up down unless you have a choice and as
we can see just from this which again
this is what's sometimes referred to
as the orbital diagram which again we
won't do too much of
in this class but this was referred to
as the orbital diagram we could see that
in the
2s orbital now we do have space for one
more electron to go in there
and that happens when we go to number
four here which is beryllium that means
it has
four electrons so again going
back here we're going to start up on top
again
always start here so it's going to be
1s2
we again now will zigzag back here
and we will now be able to fill in this
guy
with the next electron and we will have
1s2 2s2 in this case
and again just to kind of keep track of
where our electrons are at this point
first one went in here next one went in
here
third one went here and the fourth one
went like this
this is what sometimes referred to when
you have two electrons in an orbital
as those electrons are what are referred
to as being paired
their spins are paired they're basically
heading in opposite directions
that's basically what that means now we
can also see here from this sort of
picture and again you don't have to
worry too much about the picture here
but we can see we absolutely have no
more room in this orbital for any more
electrons
which means if we have more electrons we
need to go to the next
lowest energy orbital or subshell to put
those in
and that happens when we get to number
five so number five would obviously be
boron here
it has five electrons and again here
starting up on top going to our 1s
zigzagging back to our 2s2
and now the next lowest brings us to the
2p orbital in terms of where those
electrons would go
and that means we would have 1s2
2s2 2p1 and if you're not sure how many
electrons you're putting in you pretty
much
count the top numbers 2 4
and 5 electrons and again
what this really means is i'll draw a
little bit better in terms of energy
on the first energy level again we put
one electron in
two electron ends the next electrons go
into our second energy level with our 2s
and now the fifth electron will actually
end
right here and again each of these lines
represents an individual orbital
each one could hold two electrons so if
you're just doing the math here you have
2
four and one more in the first one it
could go
so this is again a subshell that could
hold
six total electrons so we now have
plenty of room to sort of fill
in the rest of these and let's continue
on with that which is number
six is carbon and that again means it
has
six electrons so 1s2
2s2 2p2
and again in terms of if you want to
visually kind of see what's happening
again this is our n equals one level our
lowest in energy
first electron second electron
third electron fourth electron fifth
electron
and now when we get actually a subshell
where there's multiple orbitals
the way it goes in and again outside of
our class in terms of y
but what happens is the actual electron
goes to the orbital
next to it and it does fill up one at a
time like i mentioned earlier
and then comes back and pairs off
we can now see that we actually have two
three
four more spaces for electrons in the
subshell
so we might as well finish this guy out
here going to number seven which is
nitrogen
seven protons also will have seven
electrons
which means it should be 1s2
2s2 2p3 again if you count up the top 2
4 and 3 is 7. again
kind of filling in as we're going
through this
so you can kind of visually see what's
happening
again first one goes there our next one
goes there
third one goes into there fourth one
goes into there
fifth goes there six goes there and
again the seventh one
actually will go here at this point
at this point we have room in each of
these orbitals for one more electron
each
and they will now have no choice but to
come back and start going the other way
and pairing off at this point there's a
rule that basically says it's really
more stable when all the electrons
are going kind of in the same direction
and that's what's sometimes referred to
as
parallel spin so continuing on
z is the atomic number so that's the
number that we find on the periodic
table
and again that is the number of protons
and because we're assuming that these
guys are neutral
that is also the number of electrons
right so if something is neutral
it's got to have the same number of
protons and the same number of electrons
the two-piece sub-level can hold a total
of six electrons
so right this is our two-piece sub-level
or subshell
and at this point it is now has three
electrons
so the next ones are going to come back
in and fill this up until
it maxes out at six so why don't we
continue on with that path there
number eight which is oxygen again
number of protons is eight
which it means it does have eight
electrons
so it should be 1s2 2s2
2p4 in this case
and again just visually what's going on
at this part
so n equals one n equals two
one two three four
five six seven and now the eighth one
will actually come back
and go here that will now fill up this
orbital this orbital individual orbital
is now
full because it has two electrons i am
clearly not drawing this
properly in terms of energy but you get
the idea lowest
lowest next lowest we have room as you
can see here for
two more electrons until that subshell
is filled
so might as well finish it out since
we're close to the first 10.
number nine is fluorine which means it
will have
nine electrons as well so again
1s2 2s2
and 2p5 and again i'm still following
that
zigzag little chart that we had a few
slides back
and i'm still stuck on the 2p because i
have not completely filled it
and we don't move on until we've
completely filled the subshell
we don't move on to the next one and
again here
we look at it one two
three four five six
seven eight nine we have now filled this
guy
and filled this guy we could see we have
room for
one more electron there and that will
happen at number 10
which is neon and neon is number 10
which means it has 10 protons and should
also have
10 electrons so we might as well fill
that guy out
so 10 electrons and again
1s2 2s2
2p6 at this point
and
filling in
field 4
5 6 7 8
9 and 10 electrons you can now see that
all these individual orbitals are filled
we have now
filled our 2p
subshell and at this point if we needed
more electrons we would have to go to
the next guy
in line and again i'll just kind of make
this part of it real quick
2p 4p
so so far we've zigzagged this way we
zigzagged this way we have come through
this guy if we had more electrons at
this point we would continue now
to the 3s and work our way through it
you can write electron configurations
for cations and anions as well things
with charges
and we'll talk about that when we're
kind of towards the end here electron
configuration what happens
in terms of when things do get charges
but
you can write definitely electron
configuration for things with charges
any questions on how to write electron
configuration
you should write electron configuration
like this
i don't know about the newish version of
the lab manual but the
old lab manual she used to write it kind
of weird um
she used to just use numbers like 2 8
and so forth in terms of electron
configuration don't do that
write it like this so if
she still does that in the lab manual
the only place i've ever seen
a person do that is a matlab manual uh
kind of writes the electron
configuration kind of weirdly
just uses numbers and stuff like that
you should definitely write it like this
any questions on that so why don't you
try this one once you try argon which is
18 electrons once you write the electron
configuration
for argon which has 18 electrons
okay so let's take a look i see some
popping in there so i think we're
looking good
so uh we got 18 for the atomic number
which means again it would have
18 electrons again when you do this as
you just saw me do on the paper here
this again is something that you could
recreate yourself very quickly
and again we always start up here so
coming this way
we would need 1s2
zigzagging back this way would give us
2s2 coming this way
we will take 2p6 again if you count the
top we have 2
4 and 6 which is 10 electrons
so we still have 18 more to go so we
will continue
past here we now come to the 3s which
could hold a maximum
of two electrons so we're now up to 12.
we still are not there so we need to
zigzag back this way to our three
p and three p
six because it can hold six and if we
count the top there
two four six is ten plus two more is
twelve and six more
is eighteen so this would be the
electron configuration
for argon question on that looks like
everybody's getting it in there in the
chat box so that's good
any questions on how to do that again no
commas no dashes no weird things you
know don't
just kind of write it like that like you
see it on the screen and
that should be the correct way
now when we look at the periodic table
there actually is uh blocks on the
periodic table
and when you look at the first two
groups
that is the s block
and if you remember s could hold two
electrons and if you look here
this is s1 and
s2 over here groups three
through eight is the p block
and if you remember p subshell could
hold a maximum of
six electrons so if you look at say the
top box here p1
p2 p3 p4
p5 and p6 the transition metals in here
transition metals in here is the d block
and it could hold 10. so first box is d1
d2 all the way to d10
and those two guys on the bottom
is the f block which called 14 again if
you count all the boxes on the bottom of
the periodic table
it actually is 14. you could actually
use the periods
this goes like one two three four very
badly drawn five
six and seven and as you go this way and
you can literally count off the electron
configuration
uh by doing that so for example
if we wanted say lithium which is right
about here
we would start here this is hydrogen
hydrogen would be 1s1
to helium which is here would be 1s2
coming down here to lithium would be
1s2 2s1 you could actually count it off
all the way across over here this would
be oxygen that we did
somewhere in this ballpark uh this would
be 2p1
2p2 2p3 and 2p4
you could actually count it off using
the
period number and also the block there
are some exceptions though this is the
fourth period here
about here and this is
sc and this is
4s1 4s2
but remember that the d orbitals don't
begin until the third energy level
so this row right here is actually 3d
and then
4d 5d 60 and so forth coming down
and remember that f's actually start at
4f
so the ds are one behind the period
number
and the f's are actually too behind the
period number
i personally would uh probably not count
it off the periodic table unless you
really know what you're doing
um i would probably use the zigzag thing
and you'd probably be in pretty good
shape
because if you really are not sure you
will get into some trouble
now when we look at something like
potassium for example
which is 19 again it would be 1s2
2s2 2p6
that is 10. 3s2
3p6 which is 18
and potassium is 19. so then we would go
to
4s1 so again if where's that
thing i was zigzagging so 1s2
2s2 2p6
3s2 3p and then
we go to our 4s next
and as i see in here
when we look at this part of the
configuration
and we count up how many electrons there
are that is 2
4 10 12
6 is 18 electrons if you look on the
periodic table
for number 18 it is our good friend
argon and you can write electron
configuration
by putting argon in brackets
and then continuing on with the
configuration
this stands for the electron
configuration
for argon and this way of writing it
which i saw somebody write it i think in
the
in the notes there or the chat with the
neon
this way you're writing in it is what is
sometimes referred to as the noble
gas configuration
and because it's a noble gas
configuration
you do need to know the order yes so you
do need to know that's the exact thing
and again it's something that you could
kind of
recreate pretty quickly on a paper and
stuff like that so
you do need to know how to memorize it
or how to recreate it pretty quickly
this is what it's sometimes referred to
as the noble gas configuration
which means what goes in the brackets
needs to be a noble gas noble gas is
group number
eight on the periodic table so for
example
if we look at sodium which is 11
and we write its electron configuration
1s2 2s2
2p6 3s1
if we take this part of the
configuration through
here that is 10 electrons
again if you go to the periodic table
look at number 10 number 10
is neon so a way we could write this
is neon in brackets and continue on with
3s1
so again that would be the noble gas
configuration so it is always the noble
gas that comes
right before whatever you're trying to
write in terms of its electron
configuration
questions on that are right in noble gas
configuration
now somebody asked about things with
charges
so when we look at the periodic table
i'm approaching it right right there i
don't think
i tried my spot actually here's
let me do this
there we go so when you look at a
periodic table remember this is a group
one this group two
group three group four group five six
seven
and eight and when things gain charges
there are certain things on the periodic
table that will always make a fixed
charge no matter what the situation is
everybody in group one no matter what
the situation is we'll always make a
plus one charge
when it does make a charge everybody in
group two will make a plus
two charge everybody in group three
which is pretty much aluminum
will make a plus three charge
when you go to group five they actually
become negative these are the non-metals
so minus three
minus two and group six and minus one
remember you got that staircase kind of
coming down here
and above the right of it is non-metals
and the transition metals can have
multiple types of charges
except for a kind of a three pack here
uh zinc and cadmium there will always be
plus
two and if you hang a left there silver
will always be
plus one no matter what the situation is
so when things gain charges um as we
talked about when we talked about
electrons protons and neutrons
it is just the electrons that are
affected and you do have to take that
into account if you're writing an
electron configuration
so for example if you take something
like oxygen with a minus two charge
the minus means that it gained electrons
and the two means that it gained
two electrons so oxygen's atomic number
is eight which means it also gained
2 electrons to become negative 2 it has
10 electrons
which means if we wrote the electron
configuration for oxygen with a minus 2
charge
it would be 1s2 2s2
2p6 would be its electron configuration
now if something gains a positive charge
let's take our friends sodium there
sodium which is group number one
on the periodic table we'll make a plus
one charge
sodium normally has 11 electrons
the positive means it lost electrons and
plus one means it lost
one electron which means this guy would
also have
10 electrons and its configuration would
be
1s2 2s2
2p6 and you may recognize as we were
just talking about
this has 10 electrons the oxygen with
minus two
sodium with plus one has ten electrons
and the guy on the periodic table that
has ten electrons
is neon right
so oxygen with a minus two charge has
the same configuration as neon
sodium with a plus one charge also has
the same configuration as neon
things that have the same electron
configuration these are what are
referred to as being
isoelectronic with each other
isoelectronic means they have the same
electron configuration
and if you look at the periodic table
sodium is here
oxygen is like here and neon
is here and what happens is as we'll
talk about in bonding in the next
chapter
metals tend to lose electrons to
end up just like the noble gas that came
right before
them so when sodium loses his electron
it's able to back up and become just
like neon in terms of electrons
while oxygen when it gains two electrons
able to move two places
forward and also end up with the same
electron configuration
as neon the whole purpose of bonding is
to end up with the exact
same electron configuration as a noble
gas
noble gases are extremely stable and
that's why that happens basically
any questions on that okay we're going
to
lay it up here so you have plenty of
time to take your quiz and all that good
stuff
so a couple things before you sign off
here for lecture
monday is a holiday i believe so we'll
be back on
wednesday for lecture with everybody
uh so have a good week if you're out for
the week a couple things about the quiz
you do need again
the computer the webcam the proctorial
just like that proctor
practice quiz it should not ask you for
a code that means you are not using
the chrome browser with the proctorial
installed
you will be given on the quiz some
conversions to use
is perfectly fine you can use a
calculator perfectly fine
you could use a scrap piece of paper to
work out things
you should not have notes out yes so i
should not see notes or anything like
that
it is closed book closed notes and all
that kind of stuff
um it will be okay it's not an issue i'm
going to assume that you are looking
down to work out things on your
calculator stuff like that
if you can arrange the camera view to
get a little bit of a shot of you and
your work area
that would be best yes if you can do
that
um so the goal here is you know try to
do the right thing
a reminder that um there are different
versions so don't have the right answers
on the wrong version or anything like
that
you do not have any work that you need
to upload here it's just kind of all or
nothing yeah so
pick the right answer enter the right
answer for this quiz
on exams you'll be able to upload work
but for this one you don't have to
upload any work
or anything like that there is an entire
module that you need to go through
so you will be first asked to look at
there's an academic honesty agreement to
look at
there's an electronic version of that
where you can sign it electronically
just put your
name and your initials then that will
open up the quiz for you to take
and then you can take the quiz and
submit it again you'll be able to see
all the questions at once
there's one submit button at the end do
not hit the submit button until you're
completely done with the quiz
otherwise it will submit it and you will
not be reopened for you
you will also pop up there and go you
sure you want to submit this you didn't
answer anything
so hopefully that warning will stop you
as well there is discussion after this
there is lab
after this as well if you have lab today
so we'll do some discussion and stuff
like that
i don't remember i think there's maybe
uh seven ish or so
or eight questions i think on it and
again uh
you could work it on scratch paper you
and sort of your work area in the view
any questions on any of that so
uh let me let you go so you can go do
that is not
up there right now give me about a
minute or so
and uh there will be an announcement
that will come out
for through canvas with a link to it but
just in case you could find in the
module section
just give me about a minute or so here
right now and i'll go do that for you
otherwise have a good week if you're out
and off the lab after this
and if you have discussion we'll start
about seven ish maybe 705 something like
that
and we'll have some discussion if you
have questions and all that kind of
stuff
any other questions make sure you type
here in the chat box if you didn't do so
and good luck on your quiz and i will
see some of you in a bit
where's the quiz found out it's gonna be
in the canvas section i'm doing it right
now to give me like one minute
you should be able to see it okay so
there'll be an announcement that'll come
out as well
and if you are on the uh module page you
may have to refresh the page
and then you'll be able to see it half
of you it should be there and the other
half give me one
second here
okay so it should be up there i'm going
to close this meeting you don't need to
be in the meeting
so i'll see you in a bit or have a nice
week if you are off the lab after this
