August 26, 2024
Summary
TLDRThis educational video script delves into the concept of ions and ionic bonds. It explains that ions are atoms or molecules with a positive or negative charge resulting from gaining or losing electrons. The script highlights the role of the periodic table in predicting ion formation, with noble gases being stable due to full outer electron layers. Cations are positively charged ions that have lost an electron, while anions are negatively charged ions that have gained an electron. The video further discusses ionic bonding, which typically occurs between metals and non-metals, forming ionic compounds like table salt. These compounds are characterized by their ability to form large crystal structures, dissolve in water, conduct electricity when dissolved, and have high boiling points.
Takeaways
- 📘 Ions are atoms or molecules with a positive or negative charge, created when atoms gain or lose electrons.
- ⚡ Cations are positively charged ions that have lost an electron, while anions are negatively charged ions that have gained an electron.
- 🔋 In an atom's inner shell, there can be up to 2 electrons, while the second and third layers can hold up to 8 electrons each.
- 🧪 Noble gases are stable atoms because they have a full outer electron layer, making them non-reactive.
- 👍 Cations can be remembered by associating the 'T' in cation with a '+' symbol (positive charge), while anions sound like 'negative' (negative charge).
- ⚛️ Atoms want to have full electron rings, as this makes them stable and less reactive.
- 🔄 Ionic bonds are formed between oppositely charged ions (cations and anions) and typically occur between metals and non-metals.
- 🧂 Sodium atoms, for example, can lose an electron to become a sodium ion (Na+), forming an ionic bond with other elements.
- 🔬 The periodic table helps predict how atoms will react, with certain columns forming specific types of ions.
- 💧 Ionic compounds, like table salt (NaCl), form crystal structures, dissolve in water, have high boiling points, and can conduct electricity when dissolved.
Q & A
What is an ion?
-An ion is an atom or molecule with a positive or negative charge, created when atoms gain or lose electrons.
How do cations and anions differ?
-Cations are positively charged ions that have lost one or more electrons, while anions are negatively charged ions that have gained one or more electrons.
What is the significance of a full electron shell in atoms?
-Atoms with a full electron shell, like the noble gases, are very stable and non-reactive because their outer electron layer is complete, making them 'happy' or stable.
How can the periodic table help predict ion formation?
-The periodic table helps predict ion formation by indicating how many electrons an atom needs to gain or lose to achieve a stable, full outer electron shell.
Why do atoms in column 1 of the periodic table typically form cations?
-Atoms in column 1 have only one electron in their outer shell, making it easier for them to lose that electron and form a cation with a positive charge.
What happens when a sodium atom loses an electron?
-When a sodium atom loses an electron, it becomes a sodium ion (Na+) with a positive charge because it now has more protons than electrons.
What is ionic bonding?
-Ionic bonding is the strong attraction between oppositely charged ions, typically between metals and non-metals, where one atom gives away an electron and another atom gains it.
What are some properties of ionic compounds?
-Ionic compounds often form large crystal structures, dissolve easily in water, have high boiling points, and conduct electricity when dissolved in water.
Why are noble gases non-reactive?
-Noble gases are non-reactive because their outer electron shells are fully filled, making them stable and not inclined to gain or lose electrons.
How do sodium chloride and other ionic compounds demonstrate ionic bonding?
-In sodium chloride (table salt), sodium gives up an electron to chlorine, forming a strong ionic bond between the positively charged sodium ion (Na+) and the negatively charged chloride ion (Cl-), creating a stable compound.
Outlines
🔬 Understanding Ions and Ionic Bonds
This paragraph introduces the concepts of ions and ionic bonds, emphasizing the importance of noting the topic 'Understanding Ions and Ionic Bonds' in class notes. It explains that an ion is an atom or molecule with a positive or negative charge, created when atoms gain or lose electrons. The discussion covers how the inner layer of an atom contains up to two electrons, while the second and third layers can hold up to eight electrons each. Noble gases are highlighted for their stability due to having a full outer electron layer. The paragraph also distinguishes between cations (positively charged ions) and anions (negatively charged ions), providing a mnemonic to help remember the charges.
⚛️ Sodium Atom and Ion Formation
This section focuses on the sodium atom and how it forms an ion. Sodium, with 11 protons and 11 electrons, is used as an example to illustrate how electrons are arranged in different layers around the nucleus. The process of an electron being removed from the sodium atom is described, transforming it into a sodium ion with a positive charge due to the imbalance between protons and electrons. The concept of ion formation is further explained by referencing the periodic table, highlighting that atoms in certain columns tend to form ions based on their electron configurations.
🧲 Ionic Bonding Explained
This paragraph delves into ionic bonding, explaining that it occurs between oppositely charged ions, typically between metals and non-metals. The bonding process is compared to the attraction between opposite sides of magnets, where one atom loses an electron and another gains it, resulting in a stable connection. The paragraph also discusses the properties of ionic compounds, such as their tendency to form large crystal structures, dissolve easily in water, have high boiling points, and conduct electricity when dissolved in water. Examples of common ionic compounds are provided, including table salt, baking soda, and bleach.
🧪 Properties of Ionic Compounds
The final paragraph summarizes the key properties of ionic compounds, reiterating that they are formed by the bonding of cations and anions. It mentions that ionic compounds often form large crystal structures, like salt, which are visible to the naked eye. Additional properties include solubility in water, the ability to conduct electricity when dissolved, and having a high boiling point. The periodic table's role in predicting atom reactivity and ionic bonding behavior is also highlighted, with a note on the non-reactivity of noble gases due to their full electron layers.
Mindmap
Keywords
💡Ion
💡Cation
💡Anion
💡Electron
💡Noble Gases
💡Periodic Table
💡Ionic Bond
💡Sodium Ion (Na+)
💡Electron Shells (Energy Levels)
💡Crystal Structure
Highlights
An ion is an atom or molecule with a positive or negative charge resulting from gaining or losing electrons.
Atoms strive for a full outer electron layer for stability, similar to noble gases.
Cations are positively charged ions formed when an atom loses an electron.
Anions are negatively charged ions formed when an atom gains an electron.
The periodic table can be used to predict ion formation based on an element's position.
Noble gases are typically non-reactive due to their full outer electron layer.
Elements in column 17 of the periodic table tend to form cations by gaining an electron.
Elements in column 1 tend to form cations by losing an electron.
Ionic bonding occurs between two different ions, often a metal and a non-metal, creating a strong attraction.
Ionic compounds form large crystal structures, are soluble in water, and have high boiling points.
Ionic compounds can conduct electricity when dissolved in water.
Examples of ionic compounds include table salt (NaCl), baking soda (NaHCO3), and bleach (NaOCl).
The arrangement of electrons in an atom, such as sodium, is crucial for understanding ion formation.
Electrons repel each other and spread out in an atom's electron shell model.
The loss of an electron from a sodium atom results in a positively charged sodium ion (Na+).
Ionic bonds are the result of oppositely charged ions attracting each other.
Properties of ionic compounds include their ability to form crystals and dissolve in water.
Transcripts
today we are talking about understanding
ions and ionic bonds so make sure at the
top of your page for your notes whether
it's digital or physical make sure you
put biology a understanding ions and
ionic bonds and then your name
underneath all right so let's go ahead
and get started so what is an atom well
an atom is a molecule or sorry let me
back up what is an ion not an atom an i
ion is an atom or a molecule with a
positive or negative charge and it's
created when atoms gain or lose
electrons we'll come back to that
picture in just a moment so um as I just
said it's either gaining or losing
electrons and depending on if it's
gaining or losing it's either going
going to have an overall net positive
charge or a net negative charge so in
the inner
layer of an atom there are up to two
electrons so in the nucleus you have
your protons and your neutrons but on
that inner layer you're going to have up
to two electrons then on the second and
third
layers you're going to have up to eight
electrons each okay the noble gases
which are on the far right hand side of
your periodic table they're really
stable atoms because they have a full
outer electron layer so that outside
ring has eight electrons and so when
they have full rings when atoms have
full rings they're super stable and
happy they like that they like when they
have a full ring okay we're going to
keep going just a little bit and then
we'll take some notes so so cat
ions so ions can be named two different
things we have either cat ions or anion
so cations ions are positively charged
so we're thinking plus um they have
fewer electrons than protons they have
lost an electron okay so now they have a
net positive charge we also have anion
they are negatively charged ions they
have more proton more electrons than
protons their overl charge is negative
so a memory trick might be that the
T in cat ion kind of looks like a plus
sign so that might help you remember
cation positive charge anion sounds
somewhat like a negative so um it's you
can think of it's got a negative charge
all right so let's go ahead and take
some notes on that so we had to start we
were saying we had ion
and
ions let me just get my piece up um are
an
atom or
molecule
with a
positive or Nega
negative
charge right and it happens when
either they gain or lose an electron so
I'm just going to kind of do it a
different color just to pop it out so
ions
happen when they
gain or
lose an electron
so I'm going to pop back over to
Black so in the case of gaining an
electron if it gains an
electron it's going to have an overall
negative charge
and it is a cat sorry not a cat it is an
an ion so it's going to be an overall
negative charge if it loses an electron
it's going to be a cat
ion and this is a let me erase and redo
that real quick because I want it to be
the other order it's going to be an
overall
positive
charge and it's a cat
ion so I'm going to highlight that and
highlight that all
right
and let's just make a little note off to
the
side
that
atoms
want to
have
full
Rings they are happiest that way happy
stable okay we want stable atoms we want
to make sure that they are happy um so
in the case
of this right here in the case of this
sodium
atom um sodium has
11
protons okay so since has 11 protons in
a just sodium atom it's also going to
have 11 electrons and if you add up two
and eight and one you get 11 okay so
let's look at this arrangement of this
sodium atom
here and actually you know we're just
going to go ahead and draw it so we have
in the middle and you can go ahead and
draw it too we have our na in the middle
sodium and then
on that first ring we're going to draw
our
electrons and we have two one two now
electrons are very much like magnets and
if you've ever tried to push the same
side of a magnet together they repel
each other they're both negatives and
they both repel each other same thing
here with electrons they like to really
push each other apart so they're going
to spread themselves out when you draw
your picture you want to draw it that
way that they're spreading out as far as
they
can then on our next one we have eight
so we're going to do the same thing
we're going to spread them really far
apart so they're going to be in
different like quadrants of this
model okay so now we're at 10 electrons
and remember in the sodium
atom it had
11 so that last one's just kind of
hanging out right over here somewhere
off to the side all right so this right
here that we just drew is our
sodium not sa a s o d IU M sodium atom
sometimes my brain goes faster than my
hand and I'm already on the second word
in
my while I'm writing the first word um
so this is our sodium atom but if this
electron over here if it were to get
kicked
off so this electron gets booted it's
like
goodbye so if this
electron kicked
out now it is actually going to be
instead of a sodium atom it's a
sodium ion and it is n a and then think
for a moment if you took an electron off
would that be plus or
minus it would be
plus because now there are only 10
electrons so we had 11
protons which are a plus and when we
kicked that guy off now we have 10
electrons and 11 - 10 is 1 that means we
have A+ one charge so this now is the
sodium cat
I because it lost an electron so you
don't really need to know super super in
depth but that is what's going on with
ions all
right then let's just talk a few more
pieces the last couple pieces we're
going to talk about is just that we can
really predict the ion formation based
on where something is in the periodic
table and so for example we have our
noble gases which are right over here in
that out column 18 their outer layer
layer is completely full so that means
it's super stable and these ones are
typically not reactive over here on that
um column 18 they're not going to react
they don't want to take in any electrons
they don't want to lose any electrons
they just are like we're cool we're good
how we are this column right here column
17 they typically form an ions because
they only have seven electrons in their
outside shell so they want to gain one
electron it's easier for them to take
one in then it would be to kick seven
out okay and then column one right over
here um they
also I think I just said something wrong
on the last one I think I said cat but I
meant anion um so column one
forms anion
or cat I sorry column one forms cat ions
because they're losing an electron over
here okay um so like for example we have
our hydrogen it's got one in that shell
and so it's going to lose that one
lithium has three so that means that it
would have had Li is the inside one and
then then that first shell it's going to
have two but then on that third shell it
would have just one so it wants to kick
that guy off because it's just sitting
there so it's going to be a cat ion all
right so it's going to have an overall
positive
charge um so ionic bonding usually when
you're bonding between oppositely
charart not usually let me back up so
ionic bonding is when you have two
different
elements that are both ions that are
being connected together so it's like a
um two magnets and you have the same
side or sorry you have opposite sides
and they're pushing together and they
suction together that is going to be
like an ionic bond so it usually occurs
between metals and non-metals and so one
atom gives away an electron and then one
atom gains an electron and they kind of
are like sharing those parts okay so
then they're connected so an example it
would be table salt actually NAC
and I don't know what happened to this
one this one got
crazy
but what it should say is um ionic
compounds form large Crystal type
structures often um they also easily
dissolve in water and then they also
have really high boiling points and
they're able to conduct electricity when
dissolved in water so there's just some
properties about them here's some
examples of other ionic compounds so we
have things like sodium chloride chide
which is table salt sodium bicarbonate
which is baking soda um sodium hydroxide
some drain cleaner um magnesium sulfate
which is Epsom salt and sodium
hypochlorite which is bleach so those
are all things that are ionic compounds
meaning that they're sharing something
across all right so just a quick
overview and then we'll take a few last
notes um ions are charged particles
formed by gaining or losing electrons we
have cat ions which have overall
positive charge they have lost an
electron we have annion they have an
overall negative charge they have gained
an electron so then we have ionic bonds
there're strong attractions between
oppos oppositely charged ions so we have
a positive ion and a negative ion coming
together and if we look at the periodic
table that can help us predict some of
that information so let's pop over here
and just make that note
that periodic
table that's the key part um it
helps
predict um how
things not things let's be more specific
how
atoms will
react
okay and then maybe we put a little note
that noble gas
Es are very
non-reactive because they have a full
ring um do I want to call it a ring
full
layer okay and then our last little
piece that we're going to put is just
ionic bonding
so it's a cat ion and an ion bonded
together I'm going to put another little
note
often
um Crystal or large Crystal
structures like salt which we say large
I mean salt crystals are not very big
but in relation to how small an atom is
a little grain of salt is very large
right so that is what we mean by a large
crystal structure is that right there
that ass salt crystal you can actually
see one of those with your eyes right
but that's a bunch of
um sodium and chloride together NaCl
together bonded
ionically um they're off also
soluble which means they can be
dissolved in water um and then they are
conductive in
water and then high boiling point
all right
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