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Chapter 3.7 Molecular Ionic Compounds

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the topic of this video is molecular and

ionic compounds

and the learning objectives are on your

screen so before jumping into ionic versus

versus

molecular compounds it's worthwhile to

re-emphasize what exactly an ion

is and we can do that by investigating

sodium atom on the left versus its

uh corresponding cation on the right

the only difference here um in between

the neutral atom

and the cation is the number of

electrons okay 11 electrons for the

neutral atom 10 for the

cation it lost one so that it could

achieve the noble gas configuration

um and we would predict that based off

of sodium's position in the

alkaline metals in uh group one

keeping in mind that the 11 protons and

12 neutrons are unchanged between the

neutral atom and the ion

so in the previous video i went through why

why

group 1 alkali metals and group 2 alkali

earth metals would lose 1 and 2

electrons respectively because they will

yield noble gas electron configurations

similarly elements that will become

anions that in other words they take an electron

electron

we can predict how many electrons

they'll take based off of how far away

they are from the noble gas

group in group 18. so group 17 the

halogens want to take one electron take

it to the noble gas configuration group

16. the calcagens want to take two

electrons then nicktogens in group 15

want to take three electrons

and we could even see some behavior in

group 14 such as carbon

accepting up to four electrons to um

uh to reach a double gas configuration

aluminum here in group 13 will actually

lose three electrons to go this way

back up to a neon noble gas

configuration and then also we have

transition metals that

do adopt positive charges they they will

lose electrons to form

um cations and some of the more common

charges that you'll find on transition

metals and d block metals

are shown in the middle of the screen um

so so really the the main takeaway here

is that um we tend to see

charges between metals and non-metals

we tend to see positive charges on

metals and we tend to see

negative charges on non-metals that's

figure and then also to to

expand our uh uh

ion toolkit we actually have this list

here of common polyatomic ions

now it is um incumbent upon you to

memorize the

the common polyatomic ions some of them

are a little bit

easier to memorize than others um

ammonium for example is a cation

hydronium is a cation but the rest are

going to be

anions here and

they some of them are related in a

series for example

so we can go ahead and look at the

naming convention

for perchlorate chlorate chloride and

so something to help you keep track of

these names

is the fact that

okay and hypo

in a name uh indicates under

or sort of less than eight the the the ending

ending

eight is typically reserved for

um more oxygen atoms

in the polyatomic ion whereas the

ending ite indicates fewer oxygen atoms

in the polyatomic ion and so in this

series you see

that per chlorate is sort of hyper

more oxygen atoms chlorate is just

more oxygen atoms chlorite is

fewer oxygen atoms and then hypo

under fewer oxygen atoms hypochlorite

so that can be useful but keep in mind that

that

chlorate you'll notice here has

a formula of clo3 minus

sometimes it might be tempting to think

that all eight

uh all polyatomic ions with an eight ending

ending

have three oxygens but that's not

necessarily the case

it is the case if you consider nitrate

no3 minus okay so this is nitrate

if you look to and also nitrite

has fewer oxygen atoms it's no

two minus but

this this is clearly not held up when

you look at something

because now we have an eight ending but

four oxygen

atoms so these polyatomic ions

their formulas and charges are going to

be important for you to memorize

at this point you don't need to to memorize

memorize

the uh related acid and its formula although

although

this will definitely be good to know in

the future

so now that we have um a big arsenal of

ions to consider both

um single atom ions

like sodium metal or fluoride

anion and also a big list now of

polyatomic ions

now we can actually define ionic bonds

so ionic bonds are electrostatic forces

of attraction between ions of opposite charge

charge

okay so that's just literally um

uh opposites attracting there and then

covalent bonds are when

electrons are shared between nuclei so

those are very distinct

bonding type interactions and it might

come as no surprise

that um ionic

compounds are composed of

ionic bonds ionic

compounds are

composed of ionic

bonds and

are composed of

covalent bonds

okay so with with that being said

um let's take a look here at a practice

problem and walk through

how we might predict what is an ionic

compound and what is a molecular compound

compound

so the question states uh predict

whether the following compounds are

ionic or molecular

ki h which is potassium iodide

okay uh we also have hydrogen peroxide h2o2

h2o2

we have um chloroform which is chcl3

and then we also have lithium carbonate

okay so when you want to differentiate

between an ionic and a molecular

compound you really want to be identifying

identifying

is the compound predominantly a metal

and non-metal

or predominantly non-metal

okay um so ask yourself

uh is it

non-metal if so it is likely

ionic an ionic compound

if it is a strictly

non-metal sort of main group

elements then it is likely to be

molecular okay so let's see if this

if the simple rule holds um for

option a we have

potassium and we have iodide

that's a metal and a nonmetal this would be

ionic compound b

hydrogen uh peroxide h2o2

hydrogen is a nonmetal oxygen is a nonmetal

nonmetal

this we would predict h

nonmetal o nonmetal this we would

predict as

molecular c

chloroform again carbon hydrogen

are and chlorine are all

nonmetals in that case so again we would

predict here

based off of c h and c l being nonmetals

that this is going to be

molecular and finally

d with lithium carbonate we have lithium

which is a metal and we actually have

carbonate here

co3 two minus which is an example of one

of our polyatomic ions

so we have a metal and we have a

non-metal or

in this particular case a polyatomic ion

and so we have two ions

this we would definitely predict is ionic

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Chapter 3.7 Molecular Ionic Compounds