Explore the characteristics and properties of ionic and metallic bonds in an entirely new way using study guides, practice problems, and 3D, interactive simulations.

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Osmium

## INTRODUCTION 

Crystals can be discovered in chemical deposits all over the world. The ruby crystal seen here is incredibly precious, both for its aesthetic value and application in lasers. Crystals are thought to have magical properties by some individuals 😮. Others believe the "magic" lies in the crystal's structural form, in which the cations and anions stack up in a predictable pattern 🤓 These crystals are made up of ionic compounds. Let’s learn about these compounds and crystals in detail.

![Ruby Crystal](//images.ctfassets.net/4yflszkpcwkt/76AR40TuwM3b5NI8tLlOiw/d986ea951e6d00b9706379e78e52e560/f-d_2ede1738d80d09cf6ef84f97af3aa042f4ab4f1856e1c30f12eff3c6_IMAGE_THUMB_POSTCARD_TINY_IMAGE_THUMB_POSTCARD_TINY.1)
[Source](https://www.ck12.org/chemistry/ionic-crystal-structure/lesson/Ionic-Crystal-Structure-CHEM/) 

### WHAT ARE IONIC COMPOUNDS? 

Ionic compounds are compounds made up entirely of ions. Ions are molecules that lose or gain electrons, and they will also have an opposite charge. Nonmetals acquire negative charge by losing electrons and forming anions, whereas metals gain positive charge by losing electrons and forming cations. Cations tend to get a positive charge, whereas anions have a negative charge. Metals and non-metals commonly form ionic connections. 

### CRYSTALS

![Crystalline Solids](//images.ctfassets.net/4yflszkpcwkt/6ndWQFttIMrG5WOLr1Y3gJ/9481299c76f1d44b556879881048f58e/halite1.jpg)
[Source](https://study.com/academy/lesson/how-crystalline-solids-amorphous-solids-differ.html)

Instead of amorphous solids, ionic compounds produce crystal lattices. Though molecular substances may form crystals, they generally do so in different shapes than ionic compounds, and molecular crystals are generally smoother than crystalline materials. An ionic crystal is a regular pattern at the atomic scale, with the cation and anion cycling and generating a three-dimensional framework based on the smaller ion uniformly filling up the spaces between the bigger ions. 

### PROPERTIES 

- They have very high melting and boiling points. High temperatures are demanded to counteract the affinity between oppositely charged ions in ionic compounds. 
- They're brittle and rigid. 
- Ionic crystals are difficult to distinguish because the positive and negative ions are firmly attached. 
- When mixed with water, they conduct electricity. 
- The dispersed ions in ionic compounds mixed with water can carry electric current through the mixture. 

### USES OF IONIC COMPOUNDS

Table salt, often known as sodium chloride, is an ionic substance, and the melting point of salt is very high. While a salt crystal is an electrical insulator, saline fluids (salt mixed in water) do not. 

Other common uses of ionic compounds are shown below: 

![Examples-of-Ionic-Compounds](//images.ctfassets.net/4yflszkpcwkt/so3SA3kQ5pX9i1EB67v2T/c288d123a43b1f246a456680bd98b783/Examples-of-Ionic-Compounds.jpg)
[Source](https://sciencenotes.org/examples-of-ionic-compounds-in-everyday-life/)

## CONCLUSION:

- Ionic compounds are made up of ions with opposing charges kept together by ionic bonds.  
- Ionic compounds have a total net neutral charge because the opposite charges balance each other out.  
- Metals transmit valence electrons to non-metals to generate ionic compounds. 
- Crystals of ionic compounds have high melting and boiling points. 

### FAQs:  

__1. Do ionic compounds make crystals?__

Ionic chemicals form crystals rather than molecules. Many consecutive positive and negative ions are linked in a matrix to form a crystal. 

__2. Why do ionic compounds form hard crystals?__

Crystal lattices having oppositely charged ions make up the crystals of electrovalent substances. A certain number of anions encircle each cation and vice versa. Because of the strong electrostatic interaction between these oppositely charged ions, ionic compounds form rigid crystals. 

__3.  Why are ionic compounds conductive?__

Since their ions can travel from point A to point B, ionic substances conduct electricity when molten (fluid) or in an aqueous phase (dispersed in water). Because their ions are maintained in fixed places and cannot migrate, ionic substances never conduct electricity when solidified. 

__4. Why are ionic compounds more conductive than covalent?__

Compared to covalent compounds, ionic compounds are generated by intense electrostatic attraction between ions, resulting in greater melting temperatures and high conductivity. 

*We hope you enjoyed studying this lesson and learned something cool about the __Physical Properties of Ionic Compounds__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎  

## SOURCES: 
1. Ionic Compound. https://www.ck12.org/c/chemistry/physical-properties-of-ionic-compounds/lesson/Ionic-Compounds-MS-PS/ Accessed 18 February 2022 
2. Ionic Compound Properties, Explained. https://www.thoughtco.com/ionic-compound-properties-608497 Accessed 18 February 2022
3. Ionic Compounds. https://www.toppr.com/guides/chemistry/metals-and-nonmetals/ionic-compounds/ Accessed 18 February 2022

Whenever metals react with non-metals, ionic compounds are created. 


Physical Properties of Ionic Compounds Study Guide

## INTRODUCTION 
Oxygen forms H2O, carbon forms CH4, while boron forms BH3. The question is, how are different compounds formed? Is there an easy way to analyze how many bonds are going to be formed of an element with another one?
Yes, with the help of electron dot diagrams. In this lesson, we will discuss the electron dot structure of C (Carbon) and other elements.

### WHAT ARE ELECTRON DOT DIAGRAMS?

When valence electrons are arranged around an atomic symbol, then it is called an electron dot diagram or Lewis dot structure.
Valence electrons are electrons present in the outermost shell or highest occupied principal energy level and can be found out easily by the electronic configuration of an element. 

For example, Li has a 1S² 2S¹ configuration. Here, the outermost shell contains 1 electron that is 2S¹. 
For Be, the configuration is 1S² 2S², and the number of valence electrons is 2. Valence electrons remain the same when we move from top to bottom in a periodic table. 

For example, valence electrons for alkali metals that are group 1: Li, Na, K, Rb, Cs is 1, while for alkaline earth metals (group 2) such as Be, Mg, Ca, Sr, and Ba is 2. 
For group 13, valence electrons are 13-10 = 3, and the same pattern is followed till group 18. But valence electrons increase by 1 when we move left to the right in a periodic table. 

For example, valence electrons for Li are 1, and it increases by 1 and reaches a maximum value of 8 when we move from Li to Ne in period 2. 

Valence electrons are arranged because those electrons take part in chemical reactions.

Electron dot diagram for Li is:     Li•  
Lewis dot diagram for Be:         •Be•
Electrons are evenly distributed around an atom because they repel each other till carbon, electrons are arranged on 4 sides of the atomic symbol.

![Valence Electrons](//images.ctfassets.net/4yflszkpcwkt/3vn2btTcnbqbA5sJP8P731/d4883c3dc801270e8f82aace318c28bd/asset-v1_LabXchange_100_2019_type_asset_block_Ls1A_Ch_1_fig_10.png)
[Source](https://www.labxchange.org/library/pathway/lx-pathway:21e1bc06-6002-4b02-addb-759cf78bc15b/items/lx-pb:21e1bc06-6002-4b02-addb-759cf78bc15b:html:a1d4bda3)

After carbon, electrons are paired up.

![Covalent Bond](//images.ctfassets.net/4yflszkpcwkt/7tTVmvxPQbRUs22TKTBE4y/2da9d44dfa5b27419b648a5ce95083dd/faf00d095edb4bc3f9cd59296f0b75c6.jpg)
[Source](https://saylordotorg.github.io/text_introductory-chemistry/s13-03-covalent-bonds.html)

And the same pattern is followed throughout:

![lewis dot table](//images.ctfassets.net/4yflszkpcwkt/264NLxibcdRIAwIRoGwNWZ/43ef3dc823157c6d467b9778b835c373/lewis_dot_table.jpg)
[Source](https://www.middleschoolchemistry.com/multimedia/chapter4/lesson6)

## CONCLUSION:

- When valence electrons are arranged around an atomic symbol, then it is called an electron dot diagram. 
- Valence electrons are electrons present in the outermost shell.
- Electron dot diagrams are used to show bonding by depicting valence electrons are these electrons are responsible for bonding.

### FAQs:

__1. What is an electron dot diagram?__

When valence electrons are arranged around an atomic symbol, then it is called an electron dot diagram.

__2. Write down the electronic configuration of Be and its electron dot diagram.__

For Be, the electronic configuration is 1S² 2S², and the number of valence electrons is 2. So, the electron dot diagram for Be is:  •Be•

__3. Why are valence electrons shown in the electron dot diagram?__

Because valence electrons take part in a reaction, or they are the ones that make bonds.

*We hope you enjoyed studying this lesson and learned something cool about __Electron Dot Diagrams__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎.

## SOURCES:
1. Electron Dot Diagram: https://www.ck12.org/c/chemistry/electron-dot-diagrams/lesson/Electron-Dot-Diagrams-CHEM/?referrer=concept_details. Accessed 5th March 2022.
2. Lewis Electron Dot Diagram: https://www.brightstorm.com/science/chemistry/chemical-bonds/lewis-electron-dot-diagram/#:~:text=Lewis%20Electron%20Dot%20Diagrams%20are,orbital%20and%203%20p%20orbitals). Accessed 5th March 2022.


Electron dot diagrams are used to show bonding with the help of valence electrons expressed as dots around the symbol of an atom.


Electron Dot Diagrams Study Guide

## INTRODUCTION

Do solid objects like iron nails and gold jewelry come to mind when you think about metals? If that's the case, you might be surprised to hear that the gleaming liquid dripping from the beaker in the image below is also a  metal. It's called mercury, and this is the only metal that occurs as a liquid on Earth. What exactly are metals, and what are their characteristics? We will find that out in this article.

![Metals](//images.ctfassets.net/4yflszkpcwkt/3z00UcgeSu2ubA1JNpPDbW/11f2b47991a314cdb676608332477026/f-d_a58929a56d1a52d394f2aed3b80419218d78acd7934ffb728bf2ebbe_IMAGE_THUMB_POSTCARD_TINY_IMAGE_THUMB_POSTCARD_TINY.1)
[Source](https://www.ck12.org/chemistry/metals/lesson/Metals-MS-PS/)

The answer to why metals show certain properties lies in the arrangement of electrons in an atom and metallic bonding.

### WHAT IS METALLIC BONDING?

- Metallic bonding is the exchange of free electrons between positively charged metal ions in a lattice. 
- Metallic bonds have a substantially different structure than covalent and ionic ones. 
- Metallic bonds connect metal atoms, while ionic bonds connect metals to nonmetals, and covalent bonds connect nonmetals to nonmetals.
- The valence electrons from the interacting metal atoms' s and p orbitals delocalize in metallic bonding. 
- That is, rather than circling their individual metal atoms, the interacting metal ions form a "sea" of electrons that encompasses the positively charged atomic nuclei. 
- The electrons are then free to travel around between the nucleus.
- This is the reason why this type of bonding is also termed as "electron sea model".

![Metallic Bonding](//images.ctfassets.net/4yflszkpcwkt/1LQS7Q9pNyDibT0ykeVsbN/e05897d3266796b0da2edaf2de10070a/imageedit_42_3617246218.gif)
[Source](https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Chemical_Bonding/Fundamentals_of_Chemical_Bonding/Metallic_Bonding)

The peculiarities of metallic bonds explain a variety of distinctive qualities of metals.

### PROPERTIES OF METALS

- Since the electrons in the electron sea can move freely and transport electric current, metals are good conductors of electricity.
- Metals are lustrous. Photons just bounce off the metal surface since light cannot permeate it. However, the frequency of light upon which photons are reflected has an upper limit.
- When a force is given to a metal, free-flowing electrons can slide between the immobile cations, preventing them from colliding just like the motion of oil-coated ball bearings gliding past one another. Metals are, as a result, extremely malleable and ductile. They can be shaped by hammering, rolling into thin sheets, or pulling into thin wires.

![aluminium-cooking-foil](//images.ctfassets.net/4yflszkpcwkt/7dQtthlfRqXEPvPigGrXCZ/e2f7fac8c5c01bad871a2569db570054/aluminium-cooking-foil.jpeg)
[Source](https://courses.lumenlearning.com/introchem/chapter/bonding-in-metals-the-electron-sea-model/)

## CONCLUSION:

- The electron sea model is a metallic bonding model in which cations are stationary points inside a mobile "sea" of electrons.
- The peculiarities of metallic bonds explain a variety of distinctive qualities of metals.

### FAQs:

__1. What is the sea of electrons model?__

The electron sea model is a metallic bonding model in which cations are stationary points inside a mobile "sea" of electrons.

__2. What does the electron sea model explain?__

Many of the physical features of metals are explained by the electron sea model. Since electrons move readily in them, they make good conductors of electricity. Due to the general drifting electrons and the ease with which the cations slide past each other, they are flexible. Because of the unbound electrons, they reflect light.

__3. What are mobile electrons?__

In metallic bonding, the terminology "mobile electron" is employed. Because the valence electrons in metals are weakly linked and free to travel throughout the metallic lattice, they are referred to as mobile electrons.

*We hope you enjoyed studying this lesson and learned something cool about the __Sea of Mobile Electrons__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎 

## SOURCES:
1. Bonding in Metals: https://courses.lumenlearning.com/introchem/chapter/bonding-in-metals-the-electron-sea-model/ Accessed 27 Feb 2022.
2. Metallic bonding: https://study.com/academy/lesson/metallic-bonding-the-electron-sea-model-why-metals-are-good-electrical-conductors.html Accessed 27 Feb 2022.
3. Metallic Bond: https://www.ck12.org/c/chemistry/metallic-bond/lesson/Metallic-Bonding-CHEM/ Accessed 27 Feb 2022.


 Metal characteristics are determined by the metallic bond (described by the electron sea model).



Metallic Bond Study Guide

## INTRODUCTION 

Have you ever wondered how chemical reactions occur? How does the bonding between two atoms become strong? Or what is the mechanism behind covalent bonding? All the question has one answer, the atoms want to stabilize their structure; hence, they follow the octet rule. Now, what is the octet rule in chemistry? Let's find out the meaning of the octet rule together! 

![NaCl Octet Rule](//images.ctfassets.net/4yflszkpcwkt/67yaOL4CM4pOwfuX0uvJFx/51fdb933e274ec5d46452b837190218f/Ionic_bonding_animation.gif)
[Source](https://en.wikipedia.org/wiki/Octet_rule)

### OCTET RULE CHEMISTRY DEFINITION 

Every atom wants to attain stability by either losing its lone electron or gaining a new electron to attain the configuration of the nearest noble gas. This phenomenon is known as the octet rule. 

Noble gases do not like to share their electrons as they are chemically inert. They have attained the octet rule and are hence stable. The molecules like halogens, oxygen, etc., attain the octet rule. Besides, the s-block elements, as well as p-block elements that follow the octet rule, will obey to reach the stability of their atoms. 

![Octet-Rule](//images.ctfassets.net/4yflszkpcwkt/7wdj9su4xOxPCMaojBAzf4/2a16b1f88a0c655d1d23c1b8e2bc1949/Octet-Rule.jpg)
[Source](https://www.chemistrylearner.com/octet-rule.html)

### EXCEPTION OF THE OCTET RULE

Not every element follows the octet rule; there are some exceptions to this rule. They are as follows:

- An atom, ion, or molecule with an unpaired valence electron known as a free radical does not follow this rule. Although, these elements or atoms or ions are very unstable and break down easily. 
- Some elements like helium, lithium, and hydrogen obey the duet rule as the first shells only contain 2 atoms. Hence, if they achieve 2 atoms in their valence shell, they are stable. 
- The transition elements do not obey the octet rule as they have a d-orbital present. The valence shells can hold 18 electrons. 
- The aromatic compounds follow Heckle’s Law due to their delocalization of pi-electrons. They do not follow the octet rule. 

### FAQs

__1. What is the simple definition of the octet rule?__

The octet rule states that atoms gain or lose electrons to achieve an outer shell electron structure nearest that of a noble gas. The attractive force between atoms is informally calculated with this rule.

__2. What is the octet rule, and what is its importance?__

The octet rule is a rule which states the behavior of an atom to attain stability. The atoms try to gain or lose electrons to attain an outer shell electron configuration nearest that of a noble gas. 

The octet rule is crucial in covalent bonding simply because both atoms get a full valence shell due to the sharing electrons. All atoms seek to reach a full valence shell, like those present in noble gases. Wondering why? This is considered the most stable electron structure.

__3. What is the octet rule?__

The octet rule states that atoms are most stable when their valence shells are loaded with eight electrons. The atoms want to have an outer shell configuration of noble gas so that they can attain stability. 

*We hope you enjoyed studying this lesson and learned something cool about the __Importance of the Octet Rule__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎 

## SOURCES:

1. The Octet Rule: https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Electronic_Structure_of_Atoms_and_Molecules/Electronic_Configurations/The_Octet_Rule. Accessed 7th March 2022.
2. The Octet Rule: https://www.ck12.org/c/chemistry/octet-rule/lecture/The-Octet-Rule:-Help-Definition-and-Exceptions/.Accessed 7th March 2022. 


The octet rule indicates that atoms try to gain or lose electrons to attain the outer shell electron configuration to reach the nearest noble gas configuration. 


Octet Rule Study Guide

## INTRODUCTION

Atoms are the primary building blocks of matter. Because atoms were formerly supposed to be the smallest particles in the universe and couldn't be separated, the term "atom" derives from the Greek word "indivisible." Charged atoms or molecules are called ions. Before discussing the differences between the two, we need to know about them in detail.

![Atoms vs Ions](//images.ctfassets.net/4yflszkpcwkt/1n3dDBL4pn5ccwA16J0GsW/0bc333fc9aa0d3d241457fbf79cdd2b4/ions.gif)
[Source](https://www.qrg.northwestern.edu/projects/vss/docs/propulsion/1-what-is-an-ion.html)

### A BRIEF IDEA ABOUT THE ATOM

All matter is made up of atoms, the smallest units of matter. According to contemporary atomic theory, an atom is made up of two parts- the nucleus and the atomic orbital surrounding it. Positively charged particles constitute the nucleus, also known as protons, and neutrally charged particles or neutrons. A proton has a charge of 1, while the neutrons do not carry any charge. 

There is an electron cloud surrounding the nucleus, in which the atom's negatively charged electrons are moving along imaginary orbitals. The electrical charge of an electron is -1. All the atoms of a certain element are similar to each other, i.e., the number of protons, neutrons, and electrons is the same for all the atoms of a particular element.

### OVERVIEW OF IONS

Molecules and compounds are formed when atoms are joined together by chemical bonds. Covalent, ionic, coordinate, and metallic bonds are examples of these types of bonds through which electrons are generally exchanged. A net electrically charged atom or molecule is known as an ion. An atom or a molecule gives up or receives electrons, forming ions. Ions can be either positively charged or negatively charged. When an atom loses electrons, the number of protons in the atom becomes more than the number of electrons. 

Therefore, it becomes a positively charged ion or a cation. Similarly, when an atom receives an electron from any other atom, the number of electrons becomes more than that of protons. Hence, it turns into a negatively charged ion or an anion.

An electric field can attract since they are electrically charged entities. Cations are attracted towards the negative pole, whereas anions toward the positive pole.

![Ions](//images.ctfassets.net/4yflszkpcwkt/5V0q75obNyYYs1G28a6xoO/518acb4ceb4e0be006c2ca3ee9f0bd30/Difference-Between-Atom-and-Ion-2.png)
[Source](https://pediaa.com/difference-between-atom-and-ion/)

## FAQs

__1. How do atoms and ions differ?__

The difference between atoms and ions is as follows –

The basic component of all matter is the atom, whereas ions are electrically charged particles. Since the number of electrons and protons remain equal in an atom, the charge remains neutral. On the other hand, an ion is formed every time an atom gains or loses an electron, negatively or positively charged, respectively. 

This implies that the number of electrons and protons do not remain the same in ions. Due to this, an ion is attracted to an electric field with an opposite charge, while an atom remains neutral in any electric field.

__2. What do ions and atoms have in common?__

The similarities between them are that both contain electrons that can be exchanged.

__3. Are atoms or ions more stable? Why?__

Since ions are electrically charged particles and are more prone to react with other elements, atoms are more stable.

__4. Where can we find negative ions?__

Negative ions are abundant in nature, especially near waterfalls, while surfing the ocean, on the beach, and in the highlands.

*We hope you enjoyed studying this lesson and learned something cool about __Atoms vs. Ions__! Join our Discord community to get any questions you may have answered and engage with other students like you! Don't forget to download our App to experience our fun VR classrooms - we promise, it makes studying much more fun!* 😎 

## SOURCES
1. Atoms vs. Ions: https://chemed.chem.purdue.edu/genchem/topicreview/bp/ch2/atom_ion.html.Accessed 9th March 2022.
2. Atoms vs. Ions: https://www.ck12.org/c/chemistry/ions-and-ion-formation/lecture/Atoms-vs.-Ions/.Accessed 9th March 2022.


This article provides a detailed analysis of the ion vs. atom topic and aims to clarify some doubts. 


Atoms vs Ions Study Guide

# Introduction

There are several different types of bonds and forces that are known to bind different molecules together. The two most common chemical bonds we come across are __covalent and ionic bonding__, where atoms easily transfer their electrons to each other. 

Well, what exactly is ionic bonding? Keep reading to find out!

## WHAT IS TYLER DEWITT IONIC BONDING? 

- Ionic bonding can be defined as the __electrostatic force__ of attraction which tightly holds the two very oppositely charged ions together. 
- A chemical bond is formed between two known atoms through the complete transfer of one or even more electrons from one significant atom to another; this results in the atoms attaining the nearest __inert gas configuration__. 

![ionic ](//images.ctfassets.net/4yflszkpcwkt/561D3P8lJ3lAbHAdGV0vbD/41b11a2172c226572929686db560396c/Ionic-Bond.jpg)
[Source](https://byjus.com/chemistry/ionic-bond-or-electrovalent-bond/)

Mainly, there are three ways by which atoms could attain stability:

- Sharing of electrons, that results in creating a __covalent bond__ between the atoms.
- Sharing of electrons by one atom only and not by both atoms.
- Transfer of electrons and completing the __octet configuration__. The bond that is then formed is termed an electrovalent bond or __ionic bond__. 
- This bond signifies one atom losing electrons while the other atom gains electrons in its outermost shell. 

- __Electrovalent bonds__ result in the formation of positive and negative ions. 
- Electrovalent bonds are only observed between metals and non-metals. 
- They cannot form between two nonmetals. 
- More simply, through electrovalent bonding, a certain number of electrons from one atom move towards a different atom so that both can attain a stable inert gas configuration. 

## WHAT ARE THE MAJOR PROPERTIES OF IONIC BONDING?

You would witness the following properties in ionic bonding because of a strong force that tightly holds the cations and anions in ionic bonding molecules.

- The ionic bonds are considered to be the __strongest__ among all other chemical bonds.
- Under the proper medium, these bonds are the __most reactive__ as they have charge separation.
- Ionic bonding molecules have __high boiling and melting points__.
- The molecules that showcase ionic bonding, in their aqueous solution or even in their molten state, are __good electricity conductors__. This phenomenon happens as the ions are charge carriers. 

![ionic](//images.ctfassets.net/4yflszkpcwkt/1xLvj5mgdGZeQtTSDjPE43/725ee84c05c791be99b0ce45c85a0851/5.jpg)
[Source](https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Supplemental_Modules_(Organic_Chemistry)/Fundamentals/Ionic_and_Covalent_Bonds)

## WHAT IS TYLER DEWITT COVALENT BONDING?
- Covalent bonding can be termed as __sharing of electrons__ between atoms. 
- This type of bonding happens between two atoms of the __same elements__ or atoms of elements that are very close to each other in the periodic table. 
- Covalent bonding can be primarily observed between __nonmetals__; however, in some cases, it can also be observed between metals and nonmetals. 
- The Tyler Dewitt covalent bond occurs when the difference between the __electronegativities__ of two atoms is way too small for an electron transfer to occur.

# SUMMARY 
- Ionic bonding is defined as the electrostatic force of attraction that holds the two oppositely charged ions together strongly.
- Electrovalent bonds result in negative and positive ions. 
- Covalent bonding can be termed as sharing of electrons between atoms.

## FAQs
__1. What is a covalent bond Tyler Dewitt?__

A covalent bond can be defined as an interatomic linkage that results in the sharing of an electron pair between two atoms.

__2. How do you explain ionic bonding?__

Ionic bonding can be defined as the electrostatic force of attraction which tightly holds the two very oppositely charged ions together.

*We hope you enjoyed studying this lesson and learned something cool about __Ionic Bonding!__ Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise, it makes studying much more fun!😎*

## Sources
1. Ionic Bond: https://byjus.com/chemistry/ionic-bond-or-electrovalent-bond/.Accessed 10th March 2022.
2. Ionic and Covalent Bonds: https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Supplemental_Modules_(Organic_Chemistry)/Fundamentals/Ionic_and_Covalent_Bonds.Accessed 10th March 2022.
3. The Ionic Bond: https://courses.lumenlearning.com/boundless-chemistry/chapter/the-ionic-bond/.Accessed 10th March 2022.

Tyler Dewitt's ionic bonding is defined as the complete moving of valence electrons between atoms. This type of bond generates two different types of ions, known as cations and anions.


Ionic Bonding Study Guide

## INTRODUCTION
Look at the image shown below. Do you know that all of those items have something in common? They are all made up of ions! What are these ions? Let’s find out!

![Examples-of-Ionic-Compounds](//images.ctfassets.net/4yflszkpcwkt/1ceeqiAVTd6UwwvKviGgyn/63b5da785bec22fcc515e697d6278605/Examples-of-Ionic-Compounds.jpg)
[Source](https://sciencenotes.org/examples-of-ionic-compounds-in-everyday-life/)

### What are IONS?
Ions are generated when electrons are added to, or removed from, neutral atoms (containing the same number of protons as electrons), molecules, or other ions. 

They are also formed when ions combine with other particles; or when a covalent connection between two atoms is ruptured, leaving both of the bond's electrons associated with one of the formerly connected atoms. Now that we have learned what ions are, let’s discuss how they are formed.

![Ions transfer](//images.ctfassets.net/4yflszkpcwkt/6FVITPQkhvGhep5h10YzIs/81a5af2b44e16c20bdd73c5e28ae4d55/Ions_transfer.png)
[Source](https://docs.google.com/document/d/1HBu8aTnZ-ULqZydkE5iFejLYMlZnxqU1hkOj7BLhdps/edit#)   

### FORMATION OF IONS: 
Ionization is the phenomenon of a neutral atom shedding or acquiring electrons, resulting in ions' formation. Ions are formed when the number of protons in an atom does not equal the number of electrons. An ion therefore is an atom that has gained or lost one or more electrons and therefore has a negative or positive charge.

Ionization is the process of exchanging electrons among atoms or molecules. The procedure is motivated by the desire to obtain more stable electronic configurations, such as the octet rule, which stipulates that the outermost (valence) shell of most stable atoms and ions has eight electrons. 

If an atom or molecule gains an electron, it becomes negatively charged (an anion), and if it loses an electron, it becomes positively charged (a cation).

Sodium (Na) is a prominent example of an ion. Because sodium possesses eleven electrons, it has a positive charge. On the other hand, Sodium would be more stable with 10 electrons, according to the octet rule (2 in its innermost shell, 8 in its outermost shell). As a result, sodium loses one electron to become much more stable. 

![Electron Transfer](//images.ctfassets.net/4yflszkpcwkt/6JQR0pINJ6yy2EFT4wJI1g/f8dc80cc695a94d22ac729400ea06448/621fa5542b64b86957ef1260e9286d55.jpg) 
[Source](https://courses.lumenlearning.com/suny-orgbiochemistry/chapter/ions/)

### GENERAL PROPERTIES OF IONS: 
Ions, especially as gases, are extremely reactive. They normally generate neutral compounds when they interact with ions of the opposite charge. The same-charged ions repel each other. A magnetic field may also deflect ions, as shown in the first photograph of the northern lights. 

If an atom or molecule gains an electron, it becomes negatively charged (an anion), and if it loses an electron, it becomes positively charged (a cation).

## CONCLUSION:

- Atoms may receive or lose electrons and therefore become ions, atoms with an uneven number of protons and electrons and hence have a positive or negative charge. 
- Ionization is the transformation of an atom into an ion. 
- Ions are reactive particles attracted or repelled by other charged particles and are diverted by a magnetic field. 

### FAQs: 

__1. What is the purpose of ion formation?__

When atoms lose or gain electrons to meet the octet rule and have entire outer valence electron shells, ions are created. 

__2.  What is the rule for forming ions?__

Metal atoms drop their highest energy level electron, or electrons, and produce positively charged ions. Nonmetal atoms gain one electron or multiple electrons to form negatively charged ions. 

__3. Why is knowing about ions important?__

Body fluid contains electrolytes, which form charged ions when dissolved in water. These ions allow electrical messages to flow freely throughout the body. Electrolytes perform a critical role in the body, regulating osmotic pressure in cells and assisting muscle and nerve cell activity. 

*We hope you enjoyed studying this lesson and learned something cool about __Ions and Ion Formation__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun, VR classrooms - we promise, it makes studying much more fun!* 😎  

## SOURCES: 
1. Ions. https://www.ck12.org/c/chemistry/ions-and-ion-formation/lesson/Ions-MS-PS/. Accessed 26 Jan 2022.
2. Formation of ions. https://www.britannica.com/science/ion-physics. Accessed 26 Jan 2022.
3. Properties of ions. https://courses.lumenlearning.com/introchem/chapter/ions/. Accessed 26 Jan 2022.


Any atom or group of atoms with one or more positive or negative electrical charges is called an ion. 
