Naming Ionic and Molecular Compounds | How to Pass Chemistry

Summary

This educational video script teaches the essential skill of naming ionic and covalent compounds, crucial for chemistry students. It emphasizes the importance of identifying compound types and provides strategies for naming, including memorizing charges for ionic compounds and using prefixes for covalent ones. Examples like aluminum oxide, iron oxide, and copper nitrate illustrate the process, ensuring viewers can apply these techniques in their studies.

Takeaways

• 🧪 Ionic compounds are composed of one metal and one nonmetal, while covalent (molecular) compounds consist of two nonmetals.
• 🔍 To name ionic compounds, first identify if it's without a transition metal, with a transition metal, with polyatomic ions, or a mix of transition metals and polyatomic ions.
• 📚 For ionic compounds without transition metals, the metal's name is followed by the nonmetal's name ending in 'ide', and charges need to be balanced.
• 🌐 Charges of elements are crucial for balancing ionic compounds; common charges should be memorized for elements like aluminum (3+) and oxygen (2-).
• 🔢 Transition metals in ionic compounds are named with a Roman numeral in parentheses indicating their charge, as seen with iron (Fe) having a 3+ charge.
• 📖 Polyatomic ions in ionic compounds are named without ending in 'ide' and have specific charges, such as phosphate (PO4^3-).
• 🧩 Ionic compounds with both transition metals and polyatomic ions require the transition metal's charge to be indicated by a Roman numeral and the polyatomic ion's charge to be balanced.
• 🔤 Covalent compounds are named using prefixes to indicate the number of atoms, and the nonmetal's name ends in 'ide'.
• 📚 Memorizing prefixes from 1 through 10 is essential for naming covalent compounds, as they indicate the quantity of each element without needing charge balance.
• 📝 Practice is key to mastering the naming of both ionic and covalent compounds, and the script encourages students to practice and seek further help if needed.

Q & A

What is the main focus of the video?

The video focuses on teaching the different types of combinations for naming ionic and molecular (covalent) compounds.

Why is it important to learn how to name compounds?

It is important because students will be naming compounds throughout their academic career in chemistry.

What is the strategy suggested for remembering how to name compounds?

The strategy is to identify the type of compound (ionic or molecular) from the very beginning.

What is the difference between ionic and covalent compounds in terms of naming?

Ionic compounds consist of one metal and one nonmetal, while covalent compounds consist of two nonmetals.

How are ionic compounds without a transition metal named?

They are named by stating the name of the metal followed by the nonmetal ending in 'ide'.

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

Roman numerals indicate the charge of the transition metal within the compound.

Why are polyatomic ions important in ionic compound naming?

Polyatomic ions are groups of two or more elements that have a specific charge and do not end in 'ide'.

How do you balance charges in ionic compounds?

You balance charges by placing appropriate subscripts on the metal and nonmetal to ensure the total charges are equal and opposite.

What is the significance of prefixes in naming covalent compounds?

Prefixes in covalent compounds indicate the number of atoms of each element without the need to balance charges.

How do you determine the Roman numeral for a transition metal in a compound?

You determine the Roman numeral by looking at the overall charge balance required by the nonmetal in the compound.

What is the difference between naming ionic compounds with polyatomic ions and those without?

In ionic compounds with polyatomic ions, the polyatomic ion does not end in 'ide' and often ends in 'ate' or 'ite', and parentheses are used to indicate the group's charge.

Outlines

00:00

🧪 Naming Ionic and Covalent Compounds

This paragraph introduces the topic of the video, which is about learning how to name different types of compounds, specifically ionic and covalent (molecular) compounds. The instructor, Melissa Maribel, emphasizes the importance of this lesson for students' current and future studies in chemistry. She outlines a strategy for naming compounds by first identifying whether they are ionic or molecular. Ionic compounds consist of a metal and a nonmetal, while covalent compounds are made up of two nonmetals. The periodic table is referenced to distinguish between metals and nonmetals. The paragraph also covers the naming of ionic compounds without transition metals, using aluminum oxide as an example, and explains the process of balancing charges to ensure the compound is neutral.

05:04

🔬 Advanced Ionic Compounds Naming

The second paragraph delves into more complex ionic compounds, including those with transition metals and polyatomic ions. It explains how to name ionic compounds with transition metals by using the metal's name, a Roman numeral in parentheses to indicate its charge, and the nonmetal ending in 'ide'. The paragraph uses iron (III) oxide as an example to demonstrate charge balancing. It also discusses ionic compounds with polyatomic ions, noting that these do not end in 'ide' but rather retain their polyatomic name, with the metal's charge being balanced by the polyatomic ion's charge. The paragraph concludes with an example of a compound containing both a transition metal and a polyatomic ion, copper (II) nitrate, and explains how to determine the charges and write the correct formula.

10:06

📚 Covalent Compounds and Prefixes

The final paragraph shifts focus to covalent or molecular compounds, which are composed of nonmetals and do not require charge balancing. It highlights the importance of knowing prefixes to indicate the number of atoms of each element in the compound. The paragraph provides examples of covalent compounds, such as diphosphorus pentoxide and trinitrogen hexaoxide, and explains how to use prefixes to name these compounds correctly. The instructor encourages practice and offers additional help through online tutoring, reinforcing the message that learning chemistry is achievable with dedication and practice.

Keywords

💡Ionic Compounds

Ionic compounds are formed by the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions). In the video, ionic compounds are distinguished by the presence of a metal and a nonmetal. The script explains how to name these compounds by identifying the metal and nonmetal, and then balancing their charges. For example, aluminum oxide is named by placing the metal 'aluminum' first, followed by the nonmetal 'oxygen' with the suffix 'ide', and then balancing the charges to result in Al2O3.

💡Covalent Compounds

Covalent compounds, also known as molecular compounds, are formed by the sharing of electron pairs between atoms. These compounds are typically made up of nonmetals. The video emphasizes that covalent compounds do not require charge balancing in their naming. The script provides an example of diphosphorus pentoxide, where the prefixes 'di-' and 'penta-' indicate the number of phosphorus and oxygen atoms, respectively.

💡Transition Metals

Transition metals are a group of elements in the periodic table that can have multiple oxidation states. In the context of the video, when naming ionic compounds with transition metals, a Roman numeral in parentheses is used to indicate the specific charge of the metal. For instance, iron in Fe2O3 is a transition metal, and the Roman numeral 'III' indicates its charge, which is necessary for balancing the charges in the compound.

💡Polyatomic Ions

Polyatomic ions are groups of two or more atoms that act as a single ion with a specific charge. The video script mentions that when naming ionic compounds with polyatomic ions, the nonmetal does not end in 'ide' but rather retains the name of the polyatomic ion. An example given is calcium phosphate, where 'phosphate' is the polyatomic ion and does not end in 'ide'.

💡Charge Balancing

Charge balancing is a process described in the video for ensuring that the total positive charge of cations equals the total negative charge of anions in an ionic compound. This is crucial for the compound to be electrically neutral. The script illustrates this with aluminum oxide, where aluminum has a 3+ charge and oxygen has a 2- charge. By placing a subscript of '2' for aluminum and '3' for oxygen, the charges are balanced to result in Al2O3.

💡Roman Numerals

Roman numerals are used in chemistry to denote the oxidation state of a transition metal in a compound. The video explains that these numerals are placed in parentheses after the metal's name to indicate its charge. For example, in the compound Fe2O3, the Roman numeral 'III' after iron (Fe) signifies that iron has a +3 oxidation state.

💡Nonmetals

Nonmetals are elements that are not metals and are typically found on the right side of the periodic table. In the video, nonmetals are distinguished by their role in forming ionic or covalent compounds. In ionic compounds, nonmetals often end in 'ide' (e.g., oxide, sulfide), while in covalent compounds, nonmetals are named with prefixes indicating the number of atoms (e.g., di-, tri-).

💡Prefixes

Prefixes are used in chemistry to denote the number of atoms of an element in a compound. The video script explains that in covalent compounds, prefixes such as 'di-', 'tri-', and 'hexa-' are used to indicate the quantity of each nonmetal. For example, in N3O6, 'tri-' indicates there are three nitrogen atoms, and 'hexa-' indicates there are six oxygen atoms.

💡Metals

Metals are elements that are typically found on the left side of the periodic table and are characterized by their ability to lose electrons and form positive ions (cations). In the video, metals are discussed in the context of forming ionic compounds with nonmetals. The script provides examples of metals such as aluminum and iron, which form ionic bonds with nonmetals like oxygen.

💡Naming Conventions

Naming conventions in chemistry are systematic rules for naming chemical compounds. The video script outlines the naming conventions for both ionic and covalent compounds. For ionic compounds, the convention involves identifying the metal and nonmetal, using Roman numerals for transition metals, and balancing charges. For covalent compounds, prefixes are used to indicate the number of atoms, and charges do not need to be balanced.

Highlights

Learn the different types of combinations for naming ionic and molecular compounds.

Understanding compounds is crucial for ongoing chemistry studies.

A simple strategy to remember how to name compounds correctly is introduced.

Identifying the type of compound (ionic or molecular) is the first step.

Ionic compounds consist of one metal and one nonmetal.

Covalent compounds consist of two nonmetals.

Highlighted nonmetals on the periodic table are crucial for naming compounds.

Naming ionic compounds without a transition metal involves using the metal name and nonmetal ending in 'ide'.

Balancing charges is essential for ionic compounds.

Transition metals in compounds are named with a Roman numeral in parentheses.

Polyatomic atoms are groups of two or more elements and have specific charges.

Ionic compounds with polyatomic atoms do not end in 'ide'.

Transition metals and polyatomic atoms in compounds are named with Roman numerals and specific polyatomic names.

Covalent compounds are named using prefixes and do not require charge balancing.

Prefixes in covalent compounds indicate the number of atoms of each element.

Diphosphorus pentoxide and trinitrogen hexaoxide are examples of covalent compound naming.

Practice is encouraged to solidify understanding of compound naming.

Online tutoring is offered for further assistance.

Transcripts

In this video you're gonna learn all the different types of combinations of

naming ionic compounds and molecular, also known as covalent compounds. Alright,

let's do this!

Hello hello Melissa Maribel here and I help students like you

understand what you just learned in class. So you stress less and you graduate

faster. All right guys, this is a very VERY important lesson today, because you

will be naming compounds until the end of the semester and if you decide to

continue with chemistry, you'll be naming compounds forever.

So if you need to pause replay or write anything down, please please do so. I will

be letting you know what you need to understand versus what you need to

memorize. Okay, here is a simple strategy that has helped my students remember how

to name compounds correctly. The strategy is to identify the type of compound from

the very beginning. Whether it's ionic or molecular. Molecular refers to covalent

compounds. An ionic compound consists of one metal and one nonmetal. A covalent

compound consists of two nonmetals. Looking at your periodic table the

highlighted portion shows you all the different types of nonmetals. Everything

there after then is a metal. We'll start with the different types of naming

for ionic compounds. The first one, ionic compounds without a transition metal.

Aluminum Oxide shows you the name of the metal, our aluminum, and oxygen, or our

nonmetal, ending in "ide." Looking at the periodic table we need to identify our

charges, so if you have to pause the video and write these down, these are the

charges that you need to have memorized. For ionic compounds you will always have

to balance out your charges. For this example aluminum oxide, let's identify

the charges for aluminum and oxygen. Aluminum's charge is a

3+ charge and oxygen has a 2- charge. Aluminum had that 3+ charge

and oxygen had the 2-. Let's balance these charges out by multiplying our

aluminum or, really, placing a subscript of 2, that 2 then multiplies with our

3+ charge and it becomes a 6+ charge. We want these charges to be the

exact same. So I'll also then place a 3 subscript, that would then turn this 2-

to a 6- charge and our charges are balanced. Another way of looking at

this is to really "lasso," I've heard that term before, our charges where our

aluminum gets that 2 and oxygen then gets the 3. They get the opposite charges

of each other just so they can make the same exact charge. They would then cancel

out the charges and be neutral. And our final balanced compound is aluminum

oxide having that subscript of 2 and 3. The second one is ionic compounds with a

transition metal. This consists of the name of our transition metal, a Roman

numeral in parentheses, and a nonmetal ending in "ide." Our transition metal is

iron and our Roman numeral is 3. Your Roman numeral actually tells you the

charge of your transition metal. A lot of times transition metals have different

types of charges. Iron sometimes has a 2+ or a 3+ charge, so our Roman

numeral actually tells us the charge of what iron is, within this compound. Your

nonmetal is the oxygen and once again that ends in "ide." So we need to balance

out our charges. Your iron as we saw was a 3+ charge, your oxygen was a

2- charge. Balancing out these charges we'll place a 2 subscript for our iron

and a 3 subscript for the oxygen. We now have these sixes canceling out, which is

what we wanted, and your final compound is Fe2O3.

Polyatomic atoms just means that there are two or more elements within that

atom. Know these polyatomic atoms. Write some flashcards.

I will also place a link in the description box of more polyatomic atoms

that you should also know. Moving on to ionic compounds with a polyatomic atom.

They consist of the name of our metal and our polyatomic atom. Notice that you

do not have your nonmetal ending in "ide." A lot of times polyatomic atoms end in

"ate" or "ite" with the exception of hydroxide and cyanide. We have calcium

phosphate. Calcium is the name of our metal and phosphate is our type of

polyatomic atom. Polyatomic atoms do have specific charges, so that is once

again something you do have to know. Calcium has a 2+ charge, phosphate

has a 3- charge. Our phosphate started off with having four oxygen. So

to balance out our charges we need to place this in parentheses to isolate

that phosphate group.

Doing so, we'll place our three with our calcium, that'll once again give us

a 6+ charge. We'll place our 2 on the outside of parentheses. Polyatomic

atoms tend to have parentheses whenever we place a subscript. These are now

balanced and your final compound is calcium phosphate. This is how it's

properly balanced. Our last ionic compound mixes transition metals and

polyatomic atoms. It consists of the name of the transition metal, a Roman numeral,

and the polyatomic atom. Here we'll see Copper (II), once again that (II) tells us the charge

of copper, which is our transition metal, and our polyatomic atom of nitrate.

Nitrate is NO3 and has a -1 charge. We saw that copper had that

2+ charge so all we need to do is just have a 2 for our nitrate since copper is

already 2. Balancing out our charges we'll place this in parentheses and place our

2 subscript outside and we'll have these twos cancel. Your final compound is

copper nitrate with a 2 subscript only on the nitrate. Let's start with

going backwards now. So instead of having the compound name

we're given the formula and asked to actually write the name of the compound.

FeBr2, Fe is known as iron and Br is known as bromine. Iron is a type of

transition metal, bromine is a nonmetal. So our nonmetal will end in "ide" and we

know that a transition metal will have a Roman numeral. To figure out what your

Roman numeral is, let's go back to the overall charges. So bromine is a type of

halogen, just meaning that it has a -1 charge. So since this had

a -1 charge, Fe or iron, must have had a 2+ charge. Another way

of identifying this, is if we were to go backwards, this 2 would go back on to

the iron, since bromine needed 2 to balance out the charges altogether. So

we'll have iron (II) bromide. Let's try another example like that.

Cu3(PO4)2. Cu is known as copper. It is a type of transition metal

so we have to have a Roman numeral. PO4 is a type of polyatomic atom.

We had to know that polyatomic atoms charge was a 3- because this then

allows us to figure out that copper had a 2+ charge. Another way of

looking at this is, this 2 goes back to the previous element. So that 2 belongs

to the copper and this 3 then belongs to our phosphate group. That's a trick that

you can use whenever you're using your formula and you're trying to go back to

the actual name of the compound. So our name of our compound would then be

copper (II) phosphate. Those are all the different types of combinations for

ionic compounds. Moving on to covalent or molecular compounds. Something that we

have to know are the prefixes. Know 1 through 10 because you do not have to

balance any of the charges, I repeat for covalent compounds do not balance

charges. Covalent compounds consists of two nonmetals as we mentioned before.

The setup will be that there is a prefix plus the name of your nonmetal, next

another prefix plus the name of your nonmetal ending in "ide."

Diphosphorus Pentoxide. You will also hear this as Penta oxide. The most common form is

pentoxide. Our subscript is that "Di" and the "Pent." "Di" meaning two and "Pent"

meaning five. Once again we do not have to balance any charges. All you have to

notice is the "Di" means two, so there are two phosphorus. The "Pent" means five so

there is five oxygen. That's it, you're done no balancing charges. Your prefixes

literally tell you how much of that element there is. We have N3O6. We'll look

at the different subscripts and figure out what prefix they need. So our three

meaning "tri" and six means "hexa." So we'll put "tri"

and then the name of our nonmetal which was nitrogen, then we'll put "hexa" and the

name of our other nonmetal ending in "ide." So we have Trinitrogen hexaoxide. Now I

hope you don't plan on leaving here without practicing what you just learned.

(Music)

If you need more help, I will be doing online tutoring every now and then, so

sign up I'll place a link in the description box. Now don't forget you, can

learn absolutely anything. You want to be a doctor, you can do it. You want to be a

dentist, you can do it. And the secret to learning anything is