Periodic Table

Summary

This educational video delves into the periodic table's structure, highlighting the significance of groups and periods. It explains how elements within the same group share similar chemical properties, exemplified by alkali metals' reactivity with water. The video also covers the periodic table's metallic, non-metallic, and metalloid elements, their conductive properties, and how they form ions. It touches on the unique characteristics of noble gases and the importance of atomic numbers and weights. The script concludes with a focus on common elements, their symbols, and their uses in everyday life.

Takeaways

• 📚 The periodic table is organized into groups (vertical columns) and periods (horizontal rows), with groups sharing similar chemical properties.
• 🔍 Group 1, the alkali metals, are highly reactive and include lithium, sodium, potassium, rubidium, cesium, and francium; hydrogen is not an alkali metal.
• 🌊 Alkali metals react violently with water, with reactivity increasing down the group, and have lower melting points compared to other metals.
• 📉 The density of alkali metals is lower than water, allowing them to float, unlike metals like iron which are denser and sink.
• 🚀 Group 2 consists of alkaline earth metals, which are reactive but less so than alkali metals, including beryllium, magnesium, calcium, strontium, barium, and radium.
• 🔄 Transition metals have multiple oxidation states and can form ions with variable charges, unlike alkali and alkaline earth metals.
• 🌐 The periodic table also includes halogens (Group 17), chalcogens (Group 16), and noble gases, which are chemically inert and do not readily participate in reactions.
• 🔢 The number of valence electrons corresponds to the group number for main group elements and influences their reactivity and ion formation.
• 🌟 Metals are typically found on the left side of the periodic table and are good conductors of electricity and heat, while non-metals are found on the right and tend to form anions.
• 💎 Metalloids, like silicon and germanium, have properties between metals and non-metals and are used as semiconductors, with conductivity increasing with temperature.
• ⚛️ The atomic number represents the number of protons and identifies the element, while the atomic mass represents the average mass of the element's isotopes.
• 🌱 Common elements and their uses were discussed, such as hydrogen in stars, helium in balloons, lithium in batteries, and carbon in various forms like graphite and diamond.

Q & A

What are the two main features of the periodic table?

The two main features of the periodic table are the columns called 'groups' and the rows called 'periods'.

Why do elements in the same group share similar chemical properties?

Elements in the same group share similar chemical properties because they have the same number of valence electrons, which determines their chemical behavior.

What is the name of the elements in Group 1 and what are their characteristics?

Group 1 elements are known as alkali metals. They are very reactive, and their reactivity increases as you go down the group.

How does the reactivity of alkali metals change as you move down the group?

The reactivity of alkali metals increases as you move down the group due to factors such as a lower melting point and increased ease of giving up electrons.

What is the difference between alkali metals and alkaline earth metals in terms of reactivity?

Alkali metals are more reactive than alkaline earth metals. Alkaline earth metals, found in Group 2, are reactive but not as reactive as the alkali metals.

What are the characteristics of transition metals in the periodic table?

Transition metals have multiple oxidation states, meaning they can form ions with variable charges, unlike alkali and alkaline earth metals which form ions with a single charge.

What are the noble gases and why are they called 'noble'?

Noble gases are elements in Group 18, including helium, neon, argon, krypton, xenon, and radon. They are called 'noble' because they are chemically inert and do not readily participate in chemical reactions.

How does the density of alkali metals compare to water and why do they float?

Alkali metals, such as lithium and sodium, have a lower density than water, which is why they float on water.

What is the significance of the atomic number and how does it relate to the number of protons?

The atomic number is the number of protons in the nucleus of an atom and it uniquely identifies an element. Each element has a specific atomic number that corresponds to the number of protons it has.

Why is the average atomic mass of an element not always a whole number?

The average atomic mass of an element is not always a whole number because it represents the weighted average of all the isotopes of that element found in nature, taking into account their relative abundance.

What are metalloids and how do they differ from metals and non-metals?

Metalloids, also known as semiconductors, are elements that have properties intermediate between metals and non-metals. They can conduct electricity better than non-metals but not as well as metals, and their conductivity increases with temperature.

Outlines

00:00

🔍 Introduction to the Periodic Table

This paragraph introduces the periodic table of elements, emphasizing the significance of groups and periods. Groups are columns that categorize elements with similar chemical properties, while periods are rows. The paragraph details the properties of alkali metals in Group 1, including their reactivity with water and the trend of increasing reactivity down the group. It also discusses the melting points of alkali metals, comparing them to other metals like iron, and mentions the density of alkali metals, noting that some, like lithium and sodium, float on water. The paragraph further explores other groups, such as alkaline earth metals in Group 2, transition metals with variable oxidation states, and noble gases in Group 18, which are chemically inert.

05:04

📚 Understanding Groups and Valence Electrons

The second paragraph delves into the naming conventions of groups, with Group 1 also known as Group 1A, and the pattern continuing for other groups, correlating with the number of valence electrons. It explains the concept of valence electrons and how they influence an element's reactivity and the type of ions they form. Metals, typically found on the left side of the periodic table, tend to lose electrons and form cations, while non-metals on the right side gain electrons to form anions. The paragraph also distinguishes between metals, non-metals, and metalloids, highlighting the unique properties of metalloids as semiconductors. Additionally, it introduces the terms 'lanthanides' and 'actinides,' which are separate rows for elements with similar properties to the lanthanide and actinide series, respectively.

10:07

🌟 Atomic Structure and Element Notation

This paragraph focuses on the atomic structure, explaining the significance of the element symbol, atomic number, and atomic weight. The atomic number corresponds to the number of protons and identifies the element, while the atomic weight represents the average mass of an element's isotopes. It clarifies that isotopes are variants of an element with different numbers of neutrons, using carbon as an example with its isotopes carbon-12, carbon-13, and carbon-14. The paragraph also discusses the abundance of isotopes and how it affects the average atomic mass, with carbon-12 being the most prevalent.

15:08

🌐 Common Elements and Their Applications

The fourth paragraph provides an overview of common elements, their symbols, and their uses. It covers elements like hydrogen, helium, lithium, sodium, magnesium, calcium, potassium, iron, copper, cobalt, nickel, cadmium, and others, highlighting their relevance in various applications, such as hydrogen in stars, helium in balloons, lithium in batteries, sodium in table salt, and calcium in bones. The paragraph also touches on the importance of knowing the symbols and names of elements for quizzes and academic purposes.

20:09

💎 Allotropes and Diatomic Elements

The final paragraph discusses allotropes, which are different structural forms of the same element, using carbon as an example with graphite and diamond. It explains that while graphite conducts electricity, diamond does not, despite both being pure carbon. The paragraph also covers elements found in the air, such as nitrogen and oxygen, and their diatomic forms, including ozone. It mentions the uses of fluorine in toothpaste, chlorine in pool disinfection, and bromine and iodine in various compounds. The discussion extends to noble gases like neon, argon, krypton, xenon, and radon, with a warning about the dangers of radon gas accumulation in poorly ventilated homes. The paragraph concludes with a brief mention of rare and expensive elements like silver, gold, palladium, platinum, and uranium.

Keywords

💡Periodic Table

The Periodic Table is a tabular arrangement of chemical elements, ordered by their atomic number, electron configuration, and recurring chemical properties. It is the central theme of the video, providing a framework to discuss the properties and behaviors of elements. The script explains that the table is divided into rows called 'periods' and columns called 'groups', which categorize elements with similar properties.

💡Groups

In the context of the Periodic Table, 'Groups' are the vertical columns that categorize elements with similar chemical properties. The video script mentions specific groups such as Group 1 (alkali metals) and Group 2 (alkaline earth metals), emphasizing that elements within the same group exhibit similar behaviors, which is a key concept in understanding periodicity.

💡Periods

Referring to the horizontal rows of the Periodic Table, 'Periods' are a way to organize elements so that those in the same row have the same number of atomic orbitals. The script explains that periods are related to the electron shell structure of the elements and introduces terms like 'lanthanides' and 'actinides', which are series of elements placed separately within the table.

💡Alkali Metals

Alkali metals, which belong to Group 1, are a class of elements that are highly reactive due to their single valence electron, which they readily give up to form positive ions or cations. The script uses lithium, sodium, and cesium as examples, noting their reactivity increases down the group, with cesium being more reactive than sodium.

💡Valence Electrons

Valence electrons are the electrons located in the outermost shell of an atom and play a key role in determining an element's chemical properties. The video script explains how the number of valence electrons corresponds to the group number, influencing the element's reactivity and the charge of the ions they form.

💡Metalloids

Metalloids, also known as semiconductors, are elements that have properties intermediate between metals and non-metals. They are mentioned in the script as elements that do not conduct electricity as well as metals but are not insulators like non-metals. Silicon and germanium are given as examples, and their conductivity is noted to increase with temperature, unlike metals.

💡Nonmetals

Nonmetals are elements that tend to gain electrons to achieve a stable electron configuration, often forming negative ions or anions. The script distinguishes between nonmetals that acquire electrons and noble gases, which are nonmetals but do not actively participate in chemical reactions due to already having a complete set of valence electrons.

💡Noble Gases

Noble gases, found in Group 18 of the Periodic Table, are characterized by their chemical inertness. The script explains that these elements, such as helium, neon, and argon, have a full complement of valence electrons, making them very stable and unlikely to engage in chemical reactions.

💡Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. The script discusses carbon as an example, mentioning carbon-12, carbon-13, and carbon-14, and how the abundance of an isotope affects the average atomic mass of an element.

💡Atomic Number

The atomic number of an element, as mentioned in the script, is a unique identifier that represents the number of protons in the nucleus of an atom. It is a fundamental property that defines the element and its position in the Periodic Table. For instance, hydrogen has an atomic number of 1, indicating it has one proton.

💡Allotropes

Allotropes are different structural forms of the same element in the same physical state. The script uses carbon as an example, contrasting graphite, which can conduct electricity, and diamond, which cannot, despite both being pure forms of carbon. This concept illustrates how the arrangement of atoms can significantly alter the properties of an element.

Highlights

The periodic table is organized into groups (columns) and periods (rows).

Elements in the same group share similar chemical properties.

Group 1, the alkali metals, includes lithium, sodium, potassium, rubidium, cesium, and francium.

Alkali metals are highly reactive, especially with water, and their reactivity increases down the group.

Cesium is more reactive than sodium, potentially explosive when reacting with water.

Melting points of alkali metals decrease as you go down the group, with cesium having a melting point of around 29°C.

Group 16 elements are called calcagens, sharing similar chemical properties.

Group 17 elements, the halogens, are non-metals with similar chemical reactivity.

Alkali metals have low density, with lithium and sodium floating on water.

Group 2, the alkaline earth metals, are less reactive than the alkali metals.

Transition metals have multiple oxidation states, unlike alkali and alkaline earth metals.

The noble gases are chemically inert and do not readily participate in chemical reactions.

Groups are also named with letters (e.g., Group 1A for Group 1), corresponding to the number of valence electrons.

Valence electrons determine the type of ions an element will form, with metals forming cations and non-metals forming anions.

Metals are conductors of electricity and heat, and are malleable and ductile.

Non-metals are insulators, brittle, and tend to form anions by gaining electrons.

Metalloids, like silicon and germanium, have semiconductor properties with increased conductivity at higher temperatures.

The periodic table includes the lanthanides and actinides, which are series of elements with similar properties.

Each element's symbol represents its identity, with the atomic number indicating the number of protons.

The average atomic mass accounts for the presence of isotopes, which have different numbers of neutrons.

Common elements and their uses are highlighted, such as hydrogen in stars, helium in balloons, and lithium in batteries.

Rare and expensive elements like gold, platinum, and uranium are mentioned for their unique properties and applications.

The importance of knowing element names and symbols is emphasized for quizzes and practical knowledge.

Transcripts

in this video we're going to talk about

the periodic table of the elements

now there's two important things you

need to know about this

the columns are called groups the rows

are called periods

so this is group 1 group 2

3

4

5 6

7 8

9 10 11 12.

and so forth

now the elements in a group

share similar chemical properties for

instance group one

is known as the alkali metals

the alkali metals include lithium sodium

potassium rubidium cesium and francium

hydrogen is not considered to be an

alkali metal

the alkali metals they're very reactive

all of these metals they

react violently with water some of them

blow up with water

in fact their reactivity increases as

you go down a group which means that

cesium

is much more reactive than sodium

in fact if you put cesium in water it

can blow up

there's a lot of youtube videos that

demonstrate this reaction whereas if you

put sodium in water it'll react

vigorously but

it may not blow up as quickly as cesium

would

one of the reasons for this is that

cesium has a much lower melting point

than sodium in fact the melting point of

the alkali metals

decreases as you go down the group

alkali metals have a much lower melting

point compared to other metals the

melting point of cesium is around 29

degrees celsius whereas the melting

point of iron

is around 1500 degrees celsius

so we need to understand is that

elements in a given column

they share

similar chemical properties

compared to elements that are not in the

same column

so for instance group 16 these elements

are known as the calcagens

they share chemical similar chemical

properties

these elements here

group 17 are known as the halogens

they're non-metals and they have a

similar chemical reactivity

so elements in the same group

share similar chemical properties

the alkali metals also have low density

values

the density of lithium and sodium

is less than water in fact those

elements will float on water

whereas if you were to put iron metal in

water it will sink to the bottom because

iron metal

is

much more dense

than water

now the next column

group two

this group is known as the alkaline

earth metals

they include beryllium magnesium calcium

strontium barium and radium

the alkaline earth metals are reactive

but they're not as reactive as the

alkali metals the alkali metals are much

more reactive than the alkaline earth

metals

next we have the transition metals

the transition metals have multiple

oxidation states

now just to compare and contrast

when the alkali metals when they give up

their electrons they form ions with a

positive one charge

so think of sodium plus or potassium

plus

when the alkaline earth metals give up

their electrons

they form

cations with a two plus charge

so think of magnesium two plus

calcium two plus

strontium two plus

now the transition metals they can form

ions with

variable charges

iron for instance

it can form the two plus ion or the

three plus ion

copper

there's copper plus one there's copper

two plus

so the oxidation states the charges that

the transition metals can have

can vary widely

now let's move on to the next group

so we discussed the calculus

and we also talked about the halogens

the halogens include fluorine chlorine

bromine and iodine the calcagens include

oxygen sulfur selenium

tellurium and polonium

next we have the noble gases

the noble gases they're chemically inert

they're not reactive

for the most part they don't participate

in chemical reactions it's extremely

hard to get them to react with other

elements

so we have elements like helium neon

argon krypton xenon and radon those are

the noble gases they're chemically inner

now there are other

ways of naming the groups so group one

is also called group 1a

group 2 is group 2a

group 13 that's group 3a

14 is 4a this is 5a

6a

7a

and 8a

now those values also correspond to the

number of valence electrons found in the

elements of that group

so let's talk about that next

so group 1 or group

1a this group has one

valence electron

group 2 has 2 valence electrons group 3a

has 3 valence electrons group 4a 4

valence electrons and then five six

seven

eight

helium is an exception to this

helium has two valence electrons

but the elements below that the other

noble gases like neon argon krypton

they have eight valence electrons

a valence electron is the electrons that

are in the outermost energy level

or the last energy level of an atom

now the number of electrons

gives us an idea

of

the type of charges that these elements

will form

but before we talk about that let's talk

about metals

non-metals and metalloids

on the left side of the periodic table

we have the metals

metals are electrical conductors

they allow electricity to flow through

them they can also conduct heat

they're malleable

they can be hammered into sheets they're

ductile they can be pulled into wires

copper and silver

they're commonly used to form wires in

electrical circuits

metals they also like to give away

electrons and as they do so they become

positively charged

ions known as cations

on the right side of the periodic table

we have nonmetals

the halogens are considered to be

non-metals

but the other non-metals which i

highlighted in blue

that is in this group

these nonmetals

they like to take electrons metals like

to give away electrons and non-metals

like to take electrons

whenever a nonmetal takes an electron it

becomes negatively charged

negatively charged ions

are known as

anions

positively charged ions are known as

cations

metals like to form cations

non-metals like to form anions

so the elements in group one the alkali

metals

they like to form

positively charged cations with a plus

one charge because they only have

one valence electron to give away

the alkaline earth metals they have two

valence electrons

when they give up those two valence

electrons

they will form

a cation with a positive two charge

so thus we have ions like mg2 plus

aluminum which is in group 3a or group

13

it's going to form an ion

a positively charged ion with a three

plus charge

so as you can see metals form cations

ions with a positive charge

and the charge is based on the number of

electrons that they can give away

non-metals like to form

anions

ions with negative charges

fluorine

is a halogen

that has 7 valence electrons it's

in group 7a or group 17.

now the nonmetals they like to take

electrons so that they can have a

complete octet they want to have eight

valence electrons fluorine has seven

it needs to acquire one electron

to have eight

so fluorine will form an ion with a

negatively one or negative one charge

the calcagens

have six valence electrons

they're part of group six a

and they need two more to get to eight

so they like to form ions with a

negative two charge

so we have oxide

which is o2 minus

nitrogen and phosphorus they have five

valence electrons

they're both nonmetals and so they like

to acquire electrons

so they need three more to get to eight

so when they acquire the three electrons

that they desire

they will have a three minus charge or

negative three charge

so that's how you could determine

the type of ions that these elements

will form

metals like to give away electrons to

form positively charged ions and

non-metals like to

take electrons to form

negatively charged anions

now keep this in mind the noble gases

are non-metals

they are not metallic

but even though they're not metals they

don't behave the same way as the other

nonmetals these nonmetals here

between

groups 4a and group 7a

those nonmetals they like to acquire

electrons

the noble gases

they're nonmetals but they don't like to

acquire electrons nor do they want to

give away their electrons they are

already complete they're happy they're

satisfied they don't want to do anything

they just want to chill

so make it make sure you understand the

distinction between those two types of

nonmetals

the nonmetals

they don't conduct electricity

unlike metals

metals are malleable and ductile but the

nonmetals they're brittle

between the metals and the nonmetals we

have

a group called the metalloids

the metalloids

they don't conduct electricity as well

as metals do

but they're not insulators like the

non-metals

they can conduct a small amount of

electricity so they're called

semiconductors

two common semiconductors that you'll

encounter are silicon and germanium

the electrical conductivity of

semiconductors

increases with temperature

so if you were to heat up silicon

or shine light upon it

it's going to conduct electricity better

compared to if you didn't do those

things

so metals

they actually become less conductive if

you increase the temperature

in fact if you can cool a metal down to

absolute zero

it can behave as a superconductor

metalloids or semiconductors they behave

differently their conductivity increases

with increase in temperature

now we talked about the vertical columns

being called groups

one thing i didn't mention yet are the

rows

the rows are called periods so this is

period one

period two

period three

and so forth

over here you have the lanthanides and

the actinides

the lanthanides

they should be after barium so starting

with element 57 you have the lanthanides

after 88 you have the actinides which

starts at 89.

so those are some other terms you need

to be familiar with the lanthanides and

ancinites

now the next thing we need to talk about

is the stuff

that's found next to the element

so the letter represents the symbol of

the element

h stands for hydrogen

the top number

is the atomic number the atomic number

is the same as the number of protons the

atomic number identifies the element so

hydrogen always has one proton

helium always have

two protons in its nucleus beryllium

will always have four protons in its

nucleus

the number on the bottom which is

usually not a whole number it's a

decimal value

it represents the atomic weight but more

specifically the average atomic mass

of that element

in its natural state on earth

now for instance if you look at carbon

you'll see that the average atomic mass

is 12.01

the reason why it's not exactly 12 is

because

there are different forms of elemental

carbon known as isotopes

there's carbon 12

which can be written that way when it's

written that way

the six is the atomic number

the top number is the mass number

there's other isotopes of carbon there's

carbon 13

and is also carbon 14.

the mass number is the sum of the number

of protons and neutrons so carbon-12 has

six protons six neutrons

carbon 13 has six protons seven neutrons

carbon 14 has six protons eight neutrons

but all forms of carbon

have six protons which is the atomic

number which identifies the element

now notice that the average is close to

12. 12.01 what that tells you is that

this particular form of carbon

is the most abundant isotope of carbon

on earth

carbon 13 and carbon 14

they're pretty rare

so more than 99

of all the carbon atoms on earth will be

in the form of carbon 12.

less than one percent

is carbon 13 and carbon 14.

so if you have

let's say

a hundred atoms of carbon

probably one of them will be carbon 13

and most likely the other 99 will be

carbon 12.

now since you're watching this video

it's likely that you're going to be quiz

on the names of the elements

so for instance if you're given the

chemical symbol of the element

li you need to know that this refers to

lithium

if you see the symbol be on your quiz

you need to know that this is beryllium

so let's talk about the common elements

that you're most likely to be quizzed on

first we have h

hydrogen hydrogen is the fuel that

powers the stars of the universe the sun

converts hydrogen

into helium

in a process known as nuclear fusion

helium he

it's found in hot air balloons well

not hot air balloons but balloons that

tend to rise

if you put helium in a balloon because

helium is less than air those are the

balloons that will go up they won't fall

to the ground but they'll float high

into the sky unless you hold them

lithium is found in lithium-ion

batteries

sodium is found in table salt table salt

is sodium chloride it contains sodium

and chlorine

in its ionic form

magnesium is found in water

calcium

is found in your bones

potassium in its ionic form k plus

is found in bananas

bananas are high in potassium

know this one iron metal

fv doesn't sound like iron but

fe is known as ferrous or ferric

which is associated with iron

when you see

see you think of cuprus or kubrick

that's associated with copper

c-o is cobalt

and i is nickel

the nickel five sense actually contains

copper and zinc

but think of nickel cadmium batteries

that's where you'll find nickel cd is

cadmium

copper is found in wires the same thing

as silver

gold is the storage for wealth pt is

platinum ir is iridium

those are also rare metals

pd palladium

aluminum think of aluminum foil

and gallium

that's a metal that can actually melt in

your hand

mercury

is already a liquid at room temperature

so

think of liquid metal that's mercury

carbon

there's many forms of carbon perhaps you

heard of carbon dioxide

that's the stuff that we breathe out

perhaps you heard of graphite

in inside your pencil

graphite can actually conduct

electricity it's an elemental form of

carbon

diamond is another form of carbon

diamond is pure carbon the same as

graphite is fear carbon

but diamond doesn't conduct electricity

it does conduct heat graphite can

conduct electricity

so graphite and diamond they're

allotropes of carbon

they're both pure elemental forms of

carbon but

they have different structures

silicon

is found in solar cells

germanium

can also

be used to make solar cells as well

when you see ascendus represents tin

think of a tin can

pb is

lead think of lead acid batteries found

inside your car

nitrogen is found in the air

almost 80 percent of air is composed of

nitrogen

or 79 actually about 20 of air is

composed of oxygen

then we have phosphorus

sulfur

selenium

te telerum

now you need to be familiar with the

diatomic elements

nitrogen is diatomic

it's a molecule composed of two atoms of

nitrogen

oxygen gas is diatomic

oxygen has two forms oxygen gas the air

that we breathe in and ozone o3 which

is found in the upper atmosphere

so these are

allotropes or two different forms

of the element oxygen

next we have fluorine

fluorine is found in toothpaste in the

form fluoride

next chlorine that's also diatomic

chlorine is typically used to disinfect

pools

and then you have bromine

and then iodine

iodine is found in table salt in the

form iodide

next we have neon think of

neon lights

there's argon argon is found in the air

krypton

i think of superman's kryptonite and

then we have xenon

and then radon now radon's interesting

because

radon can be formed from the

decomposition of uranium thorium or

radium

and because it's a gas it can actually

come from the ground

and

go up into your house

so if your home doesn't have good

ventilation if you don't open the

windows

over time

radon can build and this is a

radioactive gas that can be hazardous to

your health

so it's good to open the windows of your

house to prevent the buildup of radon in

your home

these elements which i kind of

touched on some of them

these elements are very rare and they're

expensive

silver gold palladium platinum

the price of these metals are very high

we talked about uranium a little uranium

is radioactive that's found in uh

it's used for nuclear fission

it's used in different nuclear reactors

as well

and there's other elements to talk about

but

we've covered the common ones

so that's basically it for this video so

make sure you know

the names of the elements and the

symbols that correspond to them

and

that's that thanks for watching