How to Name Chemicals Made Easy

Summary

This educational video by Katz Book teaches viewers how to name binary compounds, which are made of two different elements. It covers the basics of naming simple ionic and covalent compounds, explaining the difference in the naming process due to their composition. The video also delves into the octet rule and how it helps determine the formula of ionic compounds, as well as the use of Roman numerals for multivalent ionic compounds. The script includes examples and encourages practice to solidify understanding.

Takeaways

• 📚 The video is an educational resource on how to name binary compounds, which are chemical substances made of two different elements.
• 🔍 It covers the naming of simple ionic compounds, multivalent ionic compounds, and simple covalent compounds, but excludes polyatomic ions and organic compounds.
• 📝 In naming binary compounds, the more metallic or less electronegative element is written first, followed by the less metallic or more electronegative element.
• 🧩 The periodic table helps determine the metallic nature of elements, with metals typically being more metallic as you move down and to the left.
• 🔑 For covalent compounds, prefixes are used to indicate the number of atoms, while for ionic compounds, prefixes are generally not used.
• 🌐 The 'mono' prefix is not used for the first element in covalent compounds, but it is used for the second element if applicable.
• ⚖️ Ionic compounds are differentiated from covalent compounds by the use of Roman numerals to indicate the charge of the metal ion in the compound's name.
• 🔢 The octet rule is fundamental in determining the formula of ionic compounds, where elements tend to gain or lose electrons to achieve a stable electron configuration similar to the nearest noble gas.
• 🧲 To find the formula of an ionic compound from its name, the charges of the ions are balanced to ensure the compound is electrically neutral.
• 🌟 Multivalent metals can form more than one stable ion, and their compounds are named using Roman numerals to denote the metal's charge.
• 📉 The script provides practice examples for viewers to apply the concepts learned, emphasizing the importance of practice in mastering the naming of chemical compounds.

Q & A

What is the main focus of the video 'How to Name Chemicals Made Easy'?

The video focuses on teaching the process of naming binary compounds, which are chemicals made of two different elements. It covers the naming of simple ionic compounds, multivalent ionic compounds, and simple covalent compounds.

Why is it important to determine whether a compound is ionic or covalent when naming it?

It is important because ionic and covalent compounds are named differently. Ionic compounds typically do not use prefixes, while covalent compounds do use prefixes to indicate the numbers in the formula.

What is the general rule for writing the chemical formula and name of binary compounds?

The more metallic or less electronegative element is written first, and the less metallic or more electronegative element is written second, both in the chemical name and formula.

How does one determine the metallic nature of an element for naming purposes?

The metallic nature of an element can be determined by looking at its position in the periodic table. Metals are generally found on the left and bottom of the table and are more metallic as you move down and to the left.

What is the significance of the prefixes used in naming covalent compounds?

The prefixes in covalent compound names indicate the number of atoms of each element in the compound. For example, 'di-' indicates two atoms, 'tri-' indicates three atoms, and so on.

Why does the 'mono' prefix not apply to the first element in a covalent compound?

The 'mono' prefix is not used for the first element in a covalent compound because it is assumed to be present in a quantity of one, so it is not necessary to specify it.

What is the octet rule, and how does it relate to the formation of ionic compounds?

The octet rule states that main group elements tend to gain or lose electrons to achieve a stable electron configuration, typically having the same number of valence electrons as the nearest noble gas, which is usually eight. This principle helps determine the charges of ions in ionic compounds.

How can one deduce the formula of an ionic compound from its name?

By knowing the charges of the ions involved, one can balance the charges to deduce the formula. The magnitude of one ion's charge becomes the subscript of the other element in the formula.

What is the difference between naming simple ionic compounds and multivalent ionic compounds?

Simple ionic compounds follow the octet rule and do not use prefixes or Roman numerals in their names. Multivalent ionic compounds, which involve metals that can form more than one ion, are named using Roman numerals to indicate the charge of the metal ion.

How are the charges of ions in a compound related to the subscripts in the chemical formula?

The charges of ions in a compound determine the subscripts in the chemical formula. For example, if an ion has a charge of +2, it will have a subscript of 2 in the formula to balance the charges of the other ions.

What is the purpose of practicing naming binary compounds after learning the rules?

Practicing helps to reinforce the understanding of the rules and to apply them effectively in different scenarios, ensuring that the learner can accurately name and understand the composition of various binary compounds.

Outlines

00:00

🧪 Basics of Naming Binary Chemical Compounds

This paragraph introduces the topic of naming binary chemical compounds, which are composed of two different elements. It explains that the process starts with identifying the compound as either ionic or covalent, with metals typically written before nonmetals. The video will cover simple ionic and covalent compounds but not polyatomic ions or organic compounds. Examples given are calcium chloride (CaCl2) and carbon dioxide (CO2), highlighting the importance of electronegativity and metallic character in determining the order of elements in a compound's name and formula. The paragraph also explains the use of prefixes in covalent compounds and the significance of the periodic table in identifying an element's metallic nature.

05:02

🔍 Understanding Ionic and Covalent Compound Nomenclature

This paragraph delves into the specifics of naming ionic and covalent compounds. Ionic compounds, such as calcium chloride, do not use prefixes, whereas covalent compounds, like carbon dioxide, do. It emphasizes the importance of prefixes and the dropping of 'a' or 'o' from prefixes when followed by oxygen. The paragraph also explains the octet rule, which is fundamental in determining the charge of ions in ionic compounds. Examples are provided to illustrate how to balance charges to derive the correct chemical formula, such as magnesium fluoride (MgF2) and aluminum oxide (Al2O3). The concept of multivalent ions is introduced, with iron as an example, showing how Roman numerals are used to denote the charge of the metal ion in the compound's name.

10:05

📚 Applying Chemical Nomenclature to Practice

The final paragraph focuses on applying the knowledge of chemical nomenclature to practice. It provides examples of how to determine the formula and name of various compounds, including lithium nitride (Li3N), carbon tetrachloride (CCl4), manganese dioxide (MnO2), and barium iodide (BaI2). The paragraph explains the process of identifying the type of compound, calculating the total charge of anions to determine the charge of the metal ion in multivalent ionic compounds, and correctly writing the formula with the cation first. It encourages viewers to practice naming chemicals using the provided periodic table and offers a resource for further learning at Katsbook.com.

Keywords

💡Binary Compounds

Binary compounds are chemical substances composed of two different elements. They are fundamental in chemistry and serve as the starting point for understanding more complex chemical nomenclature. In the video, binary compounds are categorized into ionic and covalent, with examples like calcium chloride (CaCl2) and carbon dioxide (CO2) illustrating the naming conventions.

💡Metallic Nature

The metallic nature of an element refers to its tendency to lose electrons and form positive ions. It can be determined by its position in the periodic table, where metals are typically found on the left and tend to be more reactive. The video explains that in binary compounds, the more metallic element is written first in both the chemical name and formula, as seen with calcium in calcium chloride.

💡Electronegativity

Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. Elements with higher electronegativity are more nonmetallic and are written second in a compound's formula. The video uses carbon dioxide as an example, where carbon, being more to the left in the periodic table, is considered more metallic (less electronegative) than oxygen and is thus written first.

💡Chemical Formula

A chemical formula represents the composition of a compound, indicating the elements present and their proportions. The video script emphasizes the importance of the order in chemical formulas, with metallic or less electronegative elements first, and the use of prefixes to indicate the number of atoms, as in CO2 where 'di-' indicates two oxygen atoms.

💡Ionic Compounds

Ionic compounds are formed by the electrostatic attraction between oppositely charged ions, typically a metal and a nonmetal. They are named without prefixes, as explained in the video with calcium chloride being simply 'calcium chloride', reflecting the ionic nature of the bond.

💡Covalent Compounds

Covalent compounds consist of nonmetals or metalloids sharing electrons to achieve a stable electron configuration. They are named using prefixes to indicate the number of atoms, as shown in the video with carbon dioxide being 'carbon dioxide' with no prefix for 'mono' carbon.

💡Prefixes

In covalent compounds, prefixes are used to denote the number of atoms of each element. The video provides a list of common prefixes and explains their usage, such as 'di-' for two, 'tri-' for three, and the omission of 'mono' for the first element, as in 'carbon dioxide' instead of 'mono carbon dioxide'.

💡Octet Rule

The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration, typically resembling that of a noble gas with eight valence electrons. The video uses the octet rule to explain how to determine the charges of ions in ionic compounds, such as magnesium in magnesium fluoride.

💡Charge Balancing

In chemical compounds, the total positive charge must balance the total negative charge to result in a neutral compound. The video demonstrates this principle in determining the formula of ionic compounds, like needing two fluoride ions to balance one magnesium ion in magnesium fluoride (MgF2).

💡Multivalent Ions

Multivalent ions are ions that can exist with more than one positive charge. The video discusses how metals in the middle of the periodic table can form ions with different charges, such as iron forming both Fe2+ and Fe3+ ions, and the importance of using Roman numerals to denote these charges in compound names, like 'iron(II) chloride' and 'iron(III) chloride'.

💡Roman Numerals

Roman numerals are used in chemistry to indicate the charge of multivalent ions in ionic compounds. The video explains their use in naming compounds like 'chromium(III) bromide', where the numeral 'III' represents the +3 charge of the chromium ion.

Highlights

Introduction to the basics of naming binary compounds, which are essential for understanding chemical nomenclature.

Explanation of binary compounds as those made of two different elements, emphasizing the foundational nature of their naming.

The rule of writing the more metallic or less electronegative element first in both chemical names and formulas.

Use of the periodic table to determine the metallic nature of elements, with metals becoming more metallic as you move down and to the left.

The naming convention where the first element's name remains unchanged, while the second element's ending changes to 'ide'.

Difference in naming ionic and covalent compounds, with ionic compounds not using prefixes and covalent compounds using prefixes to indicate numbers.

Memorization of common prefixes for covalent compounds, with the 'mono' prefix not used for the first element.

The principle that the 'a' or 'o' at the end of a prefix is dropped if followed by oxygen, as in P2O4 being named diphosphorus tetroxide.

How to name binary covalent compounds using the learned prefixes, with examples provided.

Distinguishing between ionic and covalent compounds for proper naming, with ionic compounds typically made of a metal and a nonmetal.

The octet rule and its application in determining the charges of ions in ionic compounds, leading to the correct chemical formula.

The relationship between the charges of ions and the subscripts in the chemical formula, with examples provided.

Handling multivalent ions, such as iron forming both Fe2+ and Fe3+ ions, and their naming using Roman numerals.

The importance of calculating the total charge of anions to determine the charge and formula of cations in ionic compounds.

Practical examples of naming and formulating binary compounds, including lithium nitride, carbon tetrachloride, manganese dioxide, and barium iodide.

Encouragement to practice naming binary compounds with the aid of the periodic table to solidify understanding.

Conclusion summarizing the importance of learning to name binary compounds and the steps involved in the process.

Transcripts

how to name chemicals made easy brought

to you by Katz book welcome back and

thanks to all my subscribers and patrons

out there for making this video possible

in this video we're going to learn how

to name binary compounds binary compound

is a chemical that is made of two

different elements so naming binary

compounds is really the first step in

learning how to name any chemical this

video will cover how to name simple

ionic compounds multivalent ionic

compounds and simple covalent compounds

however it will not cover polyatomic

ions or organic compounds I'll cover

those topics in subsequent videos let's

start out by looking at two common

examples cacl2

which is calcium chloride and co2 which

is carbon dioxide in these examples and

in general the more metallic or less

electronegative element is written first

and the less metallic or more

electronegative element is written

second this is true for both the

chemical name and the chemical formula

you can determine the metallic nature of

an element by looking at the periodic

table in this periodic table metals are

red nonmetals blue and metal alloys are

purple as you move toward the metals

that is as you move down and to the left

the elements become more metallic in the

case of calcium chloride calcium is a

metal and chlorine is a nonmetal so

calcium is written first however in the

case of carbon dioxide both carbon and

oxygen are nonmetals but because carbon

is to the left of oxygen it is more

metallic than oxygen remember as you

move down and to the left

elements become more metallic so carbon

is written first and then oxygen there

are a few other things that we should

learn from our examples first of all the

first elements name remains unchanged

while the ending of the second element

changes to IDE this is true for both

ionic and covalent compounds we can see

that calcium and carbon are the same but

chlorine changed into chloride and

oxygen change into oxide also we notice

that there is a dye prefix in front of

oxide which corresponds to the two in

co2

however calcium chloride which also has

a two in the formula does not have a dye

prefix why is that because calcium

chloride is ionic and carbon dioxide is

covalent ionic and covalent compounds

are named differently so the first thing

you need to do

and naming compounds is to figure out

whether the compound is ionic or

covalent ionic compounds are typically

made of a metal and a nonmetal just like

calcium chloride while covalent

compounds are composed of only nonmetals

or metalloids just like carbon dioxide

ionic compounds do not use prefixes but

covalent compounds do use prefixes to

indicate the numbers in the formula

let's focus on covalent compounds for a

minute

the most common prefixes for covalent

compounds are written here if they are

unfamiliar to you you should memorize

them before we look at any more examples

we should notice that the mono prefix

for one is not used for the first

element co2 is not mono carbon dioxide

but simply carbon dioxide in the same

way bf3 is boron trifluoride the mono

prefix is not used for the first element

however mono is used for the second

elements for example n 2o is dinitrogen

monoxide in that case there is a prefix

for both elements notice also that the

mono lost its last oh it is not die

nitrogen mono oxide in general an a or o

at the end of a prefix will be dropped

if followed by oxygen so P 2 O 4 is die

phosphorus tetroxide not die phosphorus

tetra oxide because the a is dropped

let's try a couple more

how would you name B 2 s 3 yes die boron

trisulfide

and what is the formula of arsenic

pentachloride that's right ASCO five as

long as you know the prefixes you can

name any binary covalent compound but

what about ionic compounds

remember that cacl2 is simply calcium

chloride in general ionic compounds do

not use prefixes that means that Li 3 n

is simply lithium nitride and al 2 s 3

is simply aluminum sulfide but how can

you figure out the formula from the name

without prefixes we can use the octet

rule the octet rule basically states

that main group elements tend to gain or

lose electrons in order to have the same

number of electrons as the nearest noble

gas which is typically eight valence

electrons so in forming ionic compounds

elements with one two or three valence

electrons will lose all their valence

electrons give

elements in column one a positive one

charge elements in column two a positive

two charge and then skipping the

transition elements aluminium forms ions

with a positive three charge carbon has

four valence electrons and generally

does not form single atom ions so we

will skip the carbon column nitrogen has

five valence electrons who'll gain three

electrons to become like neon and have

eight valence electrons because

electrons are negatively charged

those three electrons will give nitrogen

a negative three charge

similarly oxide has a negative two

charge and fluoride has a negative one

charge in general all elements within a

column will form the same charged ions

unless you cross the metalloids

staircase let's try some examples what

is the formula of magnesium fluoride

magnesium in column two typically forms

positive two ions and when you write the

formula of the ion it should be mg 2

plus not mg plus two fluoride is in the

next-to-last column so it should have a

negative one charge which we write as

simply f- not as F minus 1 or F 1 minus

so how do the charges lead us to the

formula well all compounds need to be

neutral so we need to balance the

charges of the ions in this case

magnesium has a positive 2 charge but

fluoride is only negative 1 so we need

to fluorides for every one magnesium in

order to have an overall charge of zero

that means that the formula of magnesium

fluoride is mg f2 no subscript after mg

means that there is only one magnesium

in the formula and the 2 after the F

means that there are 2 fluorides in the

formula now let's pause and think about

how the formula of the compound is

related to the charges of the ions

notice how the 2 charge of magnesium

becomes the subscript of fluorine and

notice how the 1 charge of fluoride

becomes the implied 1 subscript of

magnesium this is a general principle

the magnitude of one ions charge becomes

a subscript of the other element let's

try a couple examples what is the

formula of aluminum oxide aluminum ions

have a positive 3 charge and oxide ions

have a negative 2 charge that means the

formula of aluminum oxide is al to the 2

comes from the oxides charge o 3 and 3

comes from aluminum charge

let's try one more what is the formula

of calcium sulfide calcium ions have a

positive 2 charge and sulfide just like

oxide has a negative 2 charge that means

the formula of calcium sulfide should be

ca 2's 2 however keep in mind that those

subscripts tell you the ratio of the

ions so this formula means that calcium

and sulfur are in a 2 to 2 ratio a 2 to

2 ratio of course is the same as a 1 to

1 ratio and for ionic compounds and only

ionic compounds we should reduce the

ratio to the smallest whole numbers so

the formula of calcium sulfide is simply

CAS okay we're almost done with how to

name binary compounds but what about all

those metals in the middle of the

periodic table it turns out that they do

not follow the octet rule and most of

them can form more than one different

stable ion therefore we will call them

multivalent ions for example iron can

form positive 2 or positive 3 ions when

combined with chloride for example the

iron 2 ions make Fe cl2 and the iron 3

ions make fe co 3 so what do you call

those compounds they cannot both be

called iron chloride you might be

tempted to name them with covalent

prefixes like iron dichloride but that

would be wrong instead multivalent ionic

compounds are named using Roman numerals

for the charge of the metal so Fe CL 2

is called iron 2 chloride and fecl3 is

called iron 3 chloride remember that the

Roman numerals indicate the positive

charge of the metal ion not any number

in the formula just in case you're not

familiar with Roman numerals here's a

list of the ones you need for naming

chemicals let's try a few examples what

is the formula of copper 1 phosphide

first we write down the ions from his

name we know that copper one has a

positive one charge so that's Cu plus

phosphorus has five valence electrons so

we'll gain 3 electrons to make phosphide

which is P 3 minus next we can just

switch the 3 and the 1 so the formula is

Cu 3 P going from the formula to the

name is a little harder what is the name

of CR BR 3 because we don't know the

charge of chromium in this compound is

important to first calculate the total

negative charge of the ana

bromine is a halogen in the next-to-last

column of the periodic table so bromide

has a negative one charge the three

after br means that there are three

bromides in the formula so the total

charge of the anions is negative three

that means that the total charge of the

cations must be positive three in order

to balance the charge since there is

only one chromium in the formula its

charge is positive three that means that

the name of CRB r3 is chromium 3 bromide

remember that the Roman numeral 3 refers

to the charge of chromium not the number

of bromides in the formula now anytime

you learn something new you really need

to practice it to make it your own so

I'm going to give you three chemicals

and I want you to try to name them I

also want you to determine the formula

of a binary compound of iodine and

barium I'll even give you the periodic

table to help you out please pause the

video now and solve these problems using

everything you learned in this video all

right now for the answers before you

begin you first need to determine what

type of compound each one is the first

compound is an alkali metal and a

nonmetal so it is a simple ionic

compound that obeys the octet rule keep

in mind that the metals which obey the

octet rule are primarily the ones in the

first two columns and aluminum nearly

all the other metals are multivalent

since Li 3n is a simple ionic compound

that obeys the octet rule it should not

have any prefixes or Roman numerals its

name is simply lithium nitride the

second compound is composed of two

nonmetals

so it's a covalent compound that means

its name uses prefixes for subscripts so

it's name is carbon tetrachloride

remember that the mono prefix is not

used for the first element the third

compound is a transition metal and a

nonmetal so it is a multivalent ionic

compound in order to figure out the

charge of the manganese we need to

calculate the total charge of the anions

oxygen with six valence electrons gains

two electrons to form co2 - and there

are two oxides in the formula remember

the subscript - in MN O 2 means there

are two oxides for every one manganese

if we add up the charges of the anions

we get negative 2 plus negative 2 equals

negative 4 and to balance that the

cations must have

positive for charge since there is only

one manganese is charge must be positive

for therefore its name is manganese for

oxide the last compound is a nonmetal

and an alkaline earth metal so it's

another simple ionic compound iodide

like all halides as a negative one

charge and barium in the second column

as a positive 2 charge you may at first

think that the formula would be I to be

a but that is incorrect because the

cation or the more metallic element

should be written first so the formula

is Bai 2 and the name of the compound is

barium iodide thanks so much for

watching the entire video if you found

it helpful please like subscribe or

check me out at Kats book com if you

have any questions or comments be sure

to share them below and have a wonderful

day