How To Name Ionic Compounds With Transition Metals

Summary

This educational video script focuses on the nomenclature of ionic compounds, including binary compounds, those with polyatomic ions, and those involving transition metals that require Roman numerals. The script explains how to name simple ionic compounds like NaCl (sodium chloride) and MgBr2 (magnesium bromide), and progresses to more complex examples with polyatomic ions such as sulfate and carbonate. It also addresses the naming of compounds with variable charges, using Roman numerals to denote the oxidation state of transition metals. The script serves as a comprehensive guide for students to understand and memorize the naming conventions for ionic compounds in chemistry.

Takeaways

• 🔍 Ionic compounds are named differently from molecular compounds, with the former being composed of metals and non-metals.
• 📚 The naming of ionic compounds does not require prefixes like 'mono-', 'di-', 'tri-', etc., which are used for molecular compounds.
• 🧩 For binary ionic compounds, the metal is named first followed by the non-metal with the suffix '-ide'.
• 🌐 Examples include NaCl being named 'sodium chloride' and MgBr2 as 'magnesium bromide'.
• 🔬 When naming compounds with polyatomic ions, one must memorize the names of these ions as they are not derived from the periodic table.
• 📖 The script suggests referring to a 'polyatomic ion sheet' or a related video for common polyatomic ions.
• 🔋 For compounds with variable charges, like transition metals, roman numerals are used to denote the charge of the metal.
• ⚖️ The total charge of the compound must be neutral, with the sum of the charges balancing out to zero.
• 📐 Roman numerals are used to indicate the charge of metals in compounds, with examples provided for iron, copper, chromium, and tin compounds.
• 📘 The video provides a brief tutorial on roman numerals, which are essential for naming compounds with transition metals.
• 📝 Examples are given for naming compounds with multiple charges, such as 'iron(II) chloride' and 'iron(III) chloride'.

Q & A

What is the difference between naming ionic and molecular compounds?

Ionic compounds are composed of a metal and a non-metal and do not use prefixes like mono, di, tri, etc., whereas molecular compounds typically consist of two nonmetals and use these prefixes to indicate the number of atoms.

How do you name a binary ionic compound like NaCl?

For NaCl, the metal 'Na' is named as 'sodium' and the non-metal 'Cl' is named as 'chloride', resulting in the compound name 'sodium chloride'.

What is the name of the compound MgBr2?

MgBr2 is named 'magnesium bromide', where 'Mg' stands for magnesium and 'Br' is named as 'bromide'.

How do you name a compound with a polyatomic ion like SO4?

For compounds with polyatomic ions, you need to memorize the names of these ions. SO4 is named 'sulfate'.

What is the name of the compound Li2SO4?

Li2SO4 is called 'lithium sulfate', where 'Li' is lithium and 'SO4' is sulfate.

How do you determine the name of a compound with a transition metal and variable charges, such as FeCl2?

For transition metals with variable charges, you use Roman numerals to specify the charge. FeCl2 is named 'iron(II) chloride' because iron has a +2 charge to balance the two chloride ions each with a -1 charge.

What is the significance of Roman numerals in naming ionic compounds with transition metals?

Roman numerals are used to indicate the oxidation state of transition metals in ionic compounds, which helps distinguish between different compounds with the same metal but different charges.

How do you name a compound like CuBr?

CuBr is named 'copper(I) bromide', where 'Cu' is copper with a +1 charge and 'Br' is bromide.

What is the name of the compound Cr2S3?

Cr2S3 is called 'chromium(III) sulfide', where each chromium ion has a +3 charge to balance the three sulfide ions each with a -2 charge.

Can you provide an example of how to name a compound with multiple polyatomic ions, such as PbCO3(2-)?

PbCO3(2-) is named 'lead(II) carbonate', where 'Pb' is lead with a +2 charge to balance the two carbonate ions each with a -2 charge.

Outlines

00:00

🧪 Basic Principles of Naming Ionic Compounds

This paragraph introduces the basics of naming ionic compounds, which are composed of metals and non-metals, as opposed to molecular compounds made of nonmetals. It emphasizes the importance of distinguishing between ionic and molecular compounds due to their different naming conventions. The paragraph explains how to name simple binary ionic compounds like NaCl (sodium chloride), MgBr2 (magnesium bromide), AlF3 (aluminum fluoride), and CaO (calcium oxide) by identifying the metal and non-metal elements and adding appropriate suffixes like '-ide' to the non-metal's name.

05:03

🔬 Naming Compounds with Polyatomic Ions

The second paragraph delves into the naming of ionic compounds that contain polyatomic ions, which cannot be named using the periodic table and must be memorized or referred to a polyatomic ion sheet. Examples given include Li2SO4 (lithium sulfate), Na2CO3 (sodium carbonate), Ba(OH)2 (barium hydroxide), and K2C2H3O2 (potassium acetate). The paragraph advises memorizing common polyatomic ions for ease in naming such compounds and suggests a video resource for learning these names.

10:07

🌟 Naming Compounds with Transition Metals and Variable Charges

The final paragraph addresses the naming of ionic compounds involving transition metals with variable charges, where Roman numerals are used to denote the metal's oxidation state. It explains the process of determining the charge of the metal in compounds like FeCl2 (iron(II) chloride) and FeCl3 (iron(III) chloride) by balancing the total charges of the ions. The paragraph also covers other examples such as CuBr (copper(I) bromide), CuBr2 (copper(II) bromide), Cr2S3 (chromium(III) sulfide), SnO (tin(II) oxide), SnO2 (tin(IV) oxide), PbSO4 (lead(II) sulfate), and PbCO3 (lead(IV) carbonate). It concludes with a brief tutorial on Roman numerals, which are essential for naming such compounds.

Keywords

💡Ionic Compounds

Ionic compounds are formed by the electrostatic attraction between positive and negative ions, typically a metal and a non-metal. They are distinct from molecular compounds, which are composed of molecules held together by covalent bonds. In the video, the focus is on naming these compounds correctly, which is crucial for understanding their composition and properties. Examples from the script include NaCl (sodium chloride) and MgBr2 (magnesium bromide).

💡Binary Ionic Compounds

Binary ionic compounds consist of two different elements, one being a metal and the other a non-metal, forming an ionic bond. The script explains that these compounds are named by combining the name of the metal with the suffix '-ide' for the non-metal, as seen in the examples of NaCl named as sodium chloride and MgBr2 as magnesium bromide.

💡Polyatomic Ions

Polyatomic ions are groups of two or more atoms that have a net charge and act as a single ion. They are an essential part of complex ionic compounds and require memorization as their names are not derived from the periodic table. The script mentions that these ions have specific names, such as sulfate (SO4) and carbonate (CO3), which are crucial for correctly naming compounds containing them.

💡Transition Metals

Transition metals are a group of elements in the periodic table known for their ability to form multiple oxidation states. The video explains that when naming ionic compounds containing transition metals, Roman numerals are used to indicate the metal's charge. This is demonstrated with FeCl2 being named iron(II) chloride and FeCl3 as iron(III) chloride.

💡Roman Numerals

Roman numerals are used in chemistry to denote the oxidation state of elements, particularly in ionic compounds with transition metals. The script provides examples of how to use Roman numerals to distinguish between different compounds of the same metal with varying charges, such as in the case of FeCl2 (iron(II) chloride) and FeCl3 (iron(III) chloride).

💡Oxides

Oxides are a type of compound that consists of oxygen and one other element. The script explains that oxides are named by combining the name of the other element with the suffix '-oxide'. For example, CaO is named calcium oxide, indicating the compound's composition of calcium and oxygen.

💡Hydride

A hydride is a compound formed by the combination of hydrogen with another element. In the context of the video, hydrides are named by adding the suffix '-ide' to the name of the element combined with hydrogen, as seen in the example of Ba(OH)2, which is named barium hydroxide.

💡Nitrides

Nitrides are compounds consisting of nitrogen and another element. The video script uses the example of Sr3N2, which is named strontium nitride, to illustrate the naming convention for nitrides, where the metal's name is followed by 'nitride'.

💡Sulfides

Sulfides are compounds made up of sulfur combined with a metal. The script explains that sulfides are named by adding the suffix '-ide' to 'sulfur', resulting in 'sulfide'. An example given is BaS, which is named barium sulfide, following the naming pattern for sulfides.

💡Perchlorates

Perchlorates are a type of compound containing the perchlorate ion (ClO4-). The video mentions that perchlorates are named by combining the name of the metal with 'perchlorate'. For instance, Zn(ClO4)2 is named zinc perchlorate, reflecting the presence of the perchlorate ion in the compound.

💡Ammonium

Ammonium is a polyatomic ion with the formula NH4+. The video script explains that compounds containing the ammonium ion are named by prefixing the rest of the compound's name with 'ammonium'. An example provided is NH4NO3, which is named ammonium nitrate, indicating the presence of the ammonium ion.

Highlights

Introduction to naming ionic compounds, focusing on binary ionic compounds, those with polyatomic ions, and those with transition metals.

Explanation of how to write the name of NaCl, emphasizing the distinction between ionic and molecular compounds.

Guidelines for naming ionic compounds without using prefixes like mono, di, tri, etc.

Naming MgBr2 as magnesium bromide, illustrating the process for compounds with a single metal and non-metal.

AlF3 is named aluminum fluoride, demonstrating the naming of compounds with polyatomic ions.

CaO is named calcium oxide, showing the naming of compounds with oxygen.

Naming Sr3N2 as strontium nitride, explaining the process for compounds with transition metals.

BaS is named barium sulfide, another example of naming compounds with transition metals.

The importance of memorizing polyatomic ions for chemistry courses.

Li2SO4 is named lithium sulfate, highlighting the naming of compounds with polyatomic ions.

Na2CO3 is named sodium carbonate, further illustrating the naming of compounds with polyatomic ions.

Ba(OH)2 is named barium hydroxide, demonstrating the naming of hydroxides.

KC2H3O2 is named potassium acetate, showing the naming of compounds with organic polyatomic ions.

Zn(ClO4)2 is named zinc perchlorate, discussing the naming of perchlorates.

NH4NO3 is named ammonium nitrate, explaining the naming of ammonium compounds.

FeCl2 is named iron(II) chloride, using Roman numerals to specify the charge of transition metals.

FeCl3 is named iron(III) chloride, further demonstrating the use of Roman numerals for variable charges.

CuBr and CuBr2 are named copper(I) bromide and copper(II) bromide, respectively, showing the naming of copper compounds.

CrS and Cr2S3 are named chromium(II) sulfide and chromium(III) sulfide, respectively, illustrating the naming of chromium compounds.

SnO and SnO2 are named tin(II) oxide and tin(IV) oxide, respectively, discussing the naming of tin compounds.

Basic tutorial on Roman numerals for chemistry, including how to write numbers one through seven.

PbSO4 is named lead(II) sulfate, showing the naming of lead compounds with sulfate ions.

PbCO3 is named lead(II) carbonate, demonstrating the naming of lead compounds with carbonate ions.

Conclusion of the video, summarizing the method for naming ionic compounds.

Transcripts

in this video we're going to focus on

naming ionic compounds

this is going to be binary ionic

compounds

those with polyatomic ions

and those with transition metals where

you have to incorporate the roman

numerals

so let's begin

let's start with the basics how can we

write the name of nacl so if we're given

the chemical formula how can we write

the name of this compound

so it's an ionic compound

and ionic compounds are composed of a

metal and a non-metal you need to

distinguish it from molecular compounds

because the naming system is different

for molecular compounds typically not

all the time but most of the time it's

consistent of two nonmetals and you have

to use rules like monodye triad tetra

and things like that but when you have

an ionic compound you don't need to use

the prefixes mono diatrite tetra so keep

that in mind

so what you need to do is name the first

element

n a is called sodium

now the second element instead of

calling it chlorine you're going to add

the end in chloride

so it's called

sodium

chloride

let's try another example

so let's say if we want to write the

name of mgbr2

so first use the periodic table to

identify mg

mg

is called magnesium

and then you look at the second element

on a periodic table it's called bromine

but

instead of saying bromine we're going to

add the suffix eyed so it's going to be

bromide

so to name it it's simply called

magnesium

bromide

let's try some more examples

alf 3

and cao

so al stands for aluminum

f represents fluorine

but we're going to say fluoride so alf 3

is called

aluminum

fluoride

now what about cao what is the name for

that

ca stands for calcium

and the o represents oxygen

but we're going to say oxide so this is

called calcium

oxide

now let's try two more examples

write the chemical names of

sr3 n2 and bas

so sr stands for strontium

n

represents nitrogen

so this is going to be called strontium

nitride

now what about the last one bas

the a is associated with the element

barium

s is sulfur but we're going to change it

to sulfide

so barium sulfide

so that's how you can name binary ionic

compounds

now sometimes

you might be given an ionic compound

that contains a polyatomic ion

and the periodic table won't help you

much in this case at least for the

polyatomic ion you simply have to commit

it to memory if you're fortunate your

teacher is going to give you the

polyatomic ion sheet and so you could

just use that look it up

if not you have to commit it to memory

so

you're going to need it for the rest of

your chemistry course i would advise you

just to memorize it and it's just going

to make life easier

so let's start with li2 so4

and na2

co3

so how can we name this substance

li you could look that up in a periodic

table that's a lithium

now so4 is a polyatomic ion it has a

single name

the periodic table won't help you with

that you need to look it up in your

polyatomic ion sheet

so4 is simply called sulfate

and that is something you just have to

know

now there's a video

in which i made that goes over the

common polyatomic ions that you need to

look for just look it up on youtube you

should be able to find it

and it's just

it'll help you to like understand

how to name certain polyatomic ions so

it's easier for you to memorize it it

helps you to get a better understanding

of the naming system

na2co3 na represents sodium

co3 is called carbonate

so combined it's sodium carbonate

here's another one

name this one baoh2

and kc2h3oh2

or just o2

ba

is barium

and oh when you see it

it's known as hydroxide so this is going

to be called barium

hydroxide

now what about the next example

what does k stand for

k

is called potassium

and

c2h3o2 that's a single polyatomic ion

known as acetate

so combine this is potassium

acetate

now i'm going to give you two more

examples with polyatomic ions

go ahead and name this one

and also

nh4

no3

zn stands for zinc

clo4 is known as perchlorate

so collectively

this is zinc per chlorine

now the last one

it's ionic compound even though it

doesn't have a metal inside of it

nh4

that's known as ammonium that's a

polyatomic ion

no3

is another polyatomic ion which is

called nitrate so combined

this is ammonium nitrate

consider these two compounds

fecl2

and fecl3

how can we name

these two compounds

fe

stands for iron

and cl

is going to be chloride instead of

chlorine

but now how is this going to be

different from the other one because the

other one is also iron chloride

so we need a way

to distinguish

fecl2

from fecl3

it turns out that certain transition

metals have multiple charges

and so you need to use roman numerals to

specify

the charge of the transition metal

there are certain metals that are not

transition metals that also have

multiple charges and you would still use

the roman numeral system for it

so what we need to do is figure out the

charge of fe and fecl2

now the charge of a single chloride ion

is negative one

and in this example

there are two of them

so the total negative charge is negative

two

therefore fe

has to have a positive two charge to

neutralize

the negative two charge from the two

chloride ions

so therefore since the charge in fe is

positive two

this is called

iron two chloride

now in the next example

we have three chloride ions so the total

charge is negative three

which means the total charge from fe has

to be positive three

the net charge has to add up to zero

because there's no charge on fecl3

so therefore this is going to be called

iron

3

chloride

and that's how you can name

ionic compounds that

have metals with variable charges

let's look at another example

cubr

and

cubr2

go ahead and name these two compounds

now let's start with cubr

bromide has a negative one charge and

there's only one of them

so copper has to balance that negative

one charge so it must have a plus one

charge

so therefore this is going to be called

copper

one

bromide because it has a plus one charge

now what about the second example

what's the name for it

well in this case we have two

bromide ions so the total charge is

negative two so therefore copper has to

have a plus two charge

to balance the two negative charges so

it's going to be copper

two

bromide now what about crs

and cr2 s3

go ahead and try those two examples

so let's find the charge on sulfur

sulfur has a negative two charge

which means in this example chromium has

to have a plus two charge

so this is going to be called

chromium

two sulfide

now for the second example

there's three sulfide ions

so the total negative charge is negative

six

which means the total positive charge

has to be positive six

now there's two chromium ions

so for the total charge to add up to

plus six each of these chromium ions

have to have a plus three charge so

therefore this is going to be called

chromium

sulfide

so hopefully these examples are helping

to get a good idea of how to name these

types of ionic compounds

try this sno and sno2

oxygen has a minus two charge

so tin

has to have a plus two charge

so the first one is called

tin

ii

oxide

now let's move on to our next example

so this time there's two oxide ions with

a total negative charge of negative four

but there's only one tin atom

so therefore it has to have a plus four

charge

so this is going to be called tin

four

oxide

now for those of you who need to review

the roman numeral system here's some

basics

this is one

this is two

this represents three

now this is five

now if you put the i symbol to the left

of the five

it really means subtraction like five

minus one so this is four

if you put it to the right of the five

it means addition five plus one is six

so if you want to write seven put two

eyes to the right of the v

so that represents seven

so just a basic tutorial of roman

numerals in the course of

this class

you don't really need to go past seven i

haven't seen any examples beyond that so

if you know these numbers you should be

good

now let's try this one pbso4

and pb

co3 2.

so4 is sulfate and it has a negative two

charge which means pb has to have a

positive two charge so this is going to

be called

lead

to

sulfate

now for the last example

carbonate

has a minus two charge

but there's two carbonate ions in that

compound so the total negative charge is

negative four

and there's only one pb atom so it has

to bear the entire positive 4 charge

so this is going to be called

lead

4

carbonate

and that is it for this video

so now you know how to name

ionic compounds

you