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Concentration is a familiar concept to most of us in our daily lives. We all know that adding too much coffee powder to our coffee can result in a too-strong beverage, while too little may result in a diluted, unimpressive morning coffee. Play with this simulation to visualize the relationship between the solute, solvent and their respective volumes!

concentration simulation

Concentration

Physical Chemistry

## INTRODUCTION

Dissolution is a routine activity. We mix two substances to create a solution every day. For example, imagine your morning tea. You take sugar and put it in a liquid to create a sweet solution. Let’s learn about the science behind it.

### WHAT IS THE DISSOLUTION PROCESS?

To understand dissolution, we must first understand the events that occur at the molecular level during the process. The reason that a solute dissolves entirely in a solvent depends on the nature and characteristics of the solute. Overall, we can find similarities in all the solutes. 

It is a common saying in chemistry that “like dissolves like.” This phrase stems from the fact that a solute and a solvent must have similar intermolecular forces to form a solution. The first step in the dissolving process is introducing a solute to a solvent. The molecules of both these substances start interacting, and as a result, the solute molecules move away from each other and are surrounded by the solvent molecules. 

The interaction between a solvent and a dissolved solute is termed solvation. When water is the solvent, the process is called hydration.

![DISSOLUTION PROCESS](//images.ctfassets.net/4yflszkpcwkt/7oLgecrZJD8KDRBZglzFTE/e71cdf28dbee84bbeeec49fd1daa9312/1-s2.0-S0001868614001924-fx1.jpg)
[Source](https://www.sciencedirect.com/science/article/abs/pii/S0001868614001924)

### WHAT ARE THE DIFFERENT TYPES OF SOLUTES?

There are three types of solutes: molecular, ionic, and covalent. In the case of molecular solutes, when we introduce them to the solvent, the molecules separate and become surrounded by solvent particles. 

When we introduce an ionic solute to the solvent, the independent ions of the molecules separate and are surrounded by the solvent particles in a process called dissociation, as occurs when dissolving a polar substance in water. The dissociation process causes the solution to conduct electricity, a unique property of soluble ionic compounds. Because of this property, ionic compounds are also known as electrolytes. 

Strong electrolytes dissociate completely in a solution. Table salt, or sodium chloride (NaCl), is an example of a strong electrolyte. Weak electrolytes do not dissociate completely in a solution; hence, there are fewer cations and anions in the solution. Acetic acid is a popular example of a weak electrolyte. 

Covalent solutes dissolve as individual molecules and do not dissociate in the solution, which is why they’re called nonelectrolytes. Table sugar is a famous example of a covalent solute. 

Notes on the dissolution of gasses: It is crucial to understand that the solubility of gasses is affected by temperature and pressure conditions, so which methods would increase the solubility of gas? Gasses dissolve better at lower temperatures and high-pressure conditions.

## CONCLUSION: 

- Dissolution is when the soluble solute interacts with the solvent to create a solution.
- When solutes interact with the solvent, they move away from each other. The solvent molecules then surround individual molecules before they enter into a solution.
- Ionic solute compounds break into cations and anions upon contact with a solvent.
- The process of breaking into cations and anions is known as dissociation.
- Ionic solutes that dissociate completely are strong electrolytes. 

### FAQs: 

__1. Which is true about the dissolving process in water polar solutes?__

When introducing ionic soluble compounds to water, they dissociate completely to form cations and anions. For example, sodium chloride breaks into Na and Cl-.

__2. What is the dissolving process?__

Dissolution is when the soluble solute interacts with the solvent to create a solution.

__3. What happens to a substance when dissolving in water?__

When particles of a solute interact with the solvent particle, they move away from each other. Solvent molecules then surround individual solute particles before entering into a solution.

__4. What is the dissolving of water?__

If the solvent used is water, the solvation is referred to as hydration.

*We hope you enjoyed studying this lesson and learned something cool about __Dissolution__! 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. Dissolutions: https://chem.libretexts.org/. Accessed 28 Feb 2022.
2. Dissolving Process: https://www.ck12.org/c/chemistry/dissolving-process/plix/Dissolving-Process-55b6b1d9da2cfe5fb80e288f/. Accessed 28 Feb 2022. 


Dissolution is the process in which soluble solute particles interact with solvent particles to create a solution.


Dissolving Process Study Guide

## INTRODUCTION

Depending on whether chemical compounds conduct electricity through their aqueous solution, they can be divided into two distinct parts, including electrolytes and non-electrolytes. Chemistry definition of electrolyte states that it is a chemical compound that could easily dissolve in an aqueous solution (water), creating ions. 

The formed ions are the prime source behind conducting electricity through the solution. Non-electrolytes do not conduct any electricity when dissolved in water because they cannot form any ions. 

### ELECTROLYTE IN CHEMISTRY

When dissolved in water, electrolytes are those chemical compounds that could break down into ions and conduct electricity throughout the aqueous solution. However, the compound should be an ionic compound made of anions and cations to break down into ions. The ions break down when you dissolve electrolyte compounds in the aqueous solution, forming aqueous cations and anions dispersed uniformly. 

The solution is neutral due to the uniform distribution of ions. You must have seen this experiment where an electric current is introduced into the aqueous solution, and the ions start moving to the two ends. This experiment helps prove electrolytes conduct electricity. 

However, electrolytes can again be divided into weak and strong electrolytes. You would not find any neutral molecules in the aqueous solution of a strong electrolyte as it completely ionizes. Although, with weak electrolytes, the ions do not get completely ionized; therefore, you might find some neutral molecules there. 

### EXAMPLES OF ELECTROLYTES

Strong bases and acids are great examples of electrolytes as they get completely ionized in water. However, some compounds only dissolve partially but are still considered strong electrolytes like strontium hydroxide. 

There are some weak electrolytes as well, like mostly nitrogen-containing compounds. Water is a strong example of a weak electrolyte. 

![Sugar](//images.ctfassets.net/4yflszkpcwkt/1Pku45980SxCMFhApfao0T/a54ea8c6164dae0769ade03fe34328de/Difference-Between-Electrolytes-and-Nonelectrolytes-2.jpg)
[Source](https://pediaa.com/difference-between-electrolytes-and-nonelectrolytes/#:~:text=Electrolytes%20are%20chemical%20compounds%20that,ions%20when%20dissolved%20in%20water)

### NON-ELECTROLYTE COMPOUNDS 

These chemical compounds cannot conduct electricity. Most non-electrolyte compounds are covalent compounds; they do not form any ion. Hydrocarbons are primary examples of non-electrolytes because they cannot dissolve in water. 

![Non electrolytes](//images.ctfassets.net/4yflszkpcwkt/7g4e3Us3OzdnQ2gWydgdDD/e5ff313948997edd208f38c7a225639e/Nonelectrolyte.jpg)
[Source](https://studiousguy.com/nonelectrolyte-examples/)

## CONCLUSION

- Electrolytes could break into ions and can conduct electricity 
- Non-electrolytes do not get dissolved in water; therefore, they cannot conduct electricity 
- Strong acids alongside bases are good examples of electrolytes. 
- Hydrocarbons are examples of non-electrolytes.

### FAQs: 

__1. What are electrolytes and their types?__

Electrolytes are chemical compounds that can conduct electricity. The two types are strong electrolytes and weak electrolytes. 

__2. How do you identify an electrolyte in chemistry?__

If a chemical compound dissolves in water and then separates into cations and anions, it is an electrolyte, and if it fails to do so, it is a non-electrolyte. 

*We hope you enjoyed studying this lesson and learned something cool about __Electrolytes and Non-electrolytes__! 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. Difference between Electrolytes and Non-electrolytes: https://pediaa.com/difference-between-electrolytes-and-nonelectrolytes/#:~:text=Electrolytes%20are%20chemical%20compounds%20that,ions%20when%20dissolved%20in%20water. Accessed 28 Feb 2022.
2. Non-electrolyte: https://byjus.com/chemistry/nonelectrolyte/#:~:text=Examples%20of%20Nonelectrolytes&text=Glucose%2C%20a%20sugar%20with%20the,it%20is%20considered%20a%20nonelectrolyte. Accessed 28 Feb 2022.


Electrolyte Chemistry helps us understand the basics of electrolytes and non-electrolytes, the benefits, and their significant differences.


Electrolytes And Non-Electrolytes Study Guide

## INTRODUCTION

Do you know that cleaning of wounds can also be done by saline solution? Saline solution is a solution of common salt and water. 
But what is a solution in chemistry?
Let’s understand!

### What is  Solute?

Something that dissolves in a solution is called a solute. The amount of solvent in a fluid solution is always greater than the amount of solute. Salt and water are two of the solutes we encounter most frequently on a daily basis. Because salt dissolves in water, it serves as the solute. An object that a solvent may dissolve into a solution is referred to as a solute. A solution can take on several forms. It may exist in the forms of a solid, liquid, or gas.

### What is Solvent?

The most plentiful component in a solution is referred to as the solvent. It is the substance that the solute has dissolved in. Typically, a solvent is a liquid. The most potent solvent, according to general information on the internet and descriptions in certain publications, is water. Because it can dissolve practically any material more effectively than any other liquid, it is also referred to as the "universal solvent." Water is a great solvent due to its polarity as well.

### SOLUTION
A homogenous mixture of two or more substances is called a solution. 

![Solution](//images.ctfassets.net/4yflszkpcwkt/57e6kte9NJMs0XnQUP9iF6/986bbc6d7b5b44671c59d6c40bd4ea45/2.svg)

### COMPONENTS OF A SOLUTION
A solution is formed by mixing a solute and solvent. So what are solute and solvent? A solute is a substance that is dissolved in a dissolving medium called a solvent.

For example, when we make a salt solution, salt is being dissolved in a dissolving medium that is water. Here, salt is solute as it is dissolved in dissolving medium water, which is solvent.

The same applies to a sugar solution. Sugar is solute, and water is solvent. 
Another thing to keep in mind is that solute is in limited quantity while the solvent is in excess. 

### Important Difference between Solute and Solvent

The fundamental distinction between a solute and a solvent is that one dissolves, while the other acts as a dissolving medium. Solutes are substances that are added to solvents to create solutions, which is the major distinction between them. During the creation of a solution, a solvent is a material that disperses the solute particles.

| Parameter | Solute  | Solvent     |
| ---------- | ---------- | ---------- |
| Meaning       | a substance that dissolves       | It is a dissolving medium      |
| Boiling point| Higher than solvent       | Lower than solute       |
| Dependability| Solubility depends on the properties of the solute       | Solubility depends on the properties of the solvent     |
| Physical state | Found in solid, liquid, or gaseous state       | Found mainly in the liquid state, but can be gaseous as well       |

### THE AQUEOUS SOLUTIONS

When the solvent used to make a solution is water, the solution is called aqueous. The saltwater solution is an aqueous solution. The dissolved part that is solute can be in any state: solid, liquid, or gas. For example, acid solutions are acids dissolved in water like vinegar, seawater is a solution of many salts in water, and cough syrup is a solution of many drugs dissolved in water.

But is a solution only formed when the solvent is liquid?
NO!

### Types of Solvents

There are two categories of solvents based on polarity: polar and non-polar. A solvent's polarity determines whether it can dissolve any solute.

When water molecules are drawn to electrically charged solute molecules, the solute is said to be dissolved if the force of attraction is strong enough to break the solute molecules and distribute them uniformly throughout the solvent. Fats, oils, and greases are non-polar solutes that do not dissolve in water. They combine to generate an emulsion when combined. The same kinds of big non-polar solute molecules are drawn to non-polar solvents by the grouping of electrons on one side of the molecule. All non-polar solutes dissolve in non-polar liquids using this process.

### Examples of Solution

• When we combine salt (often table salt) and water, we create salt water. The solvent in this instance is water, while the solute is salt.
• By combining sugar and water, sugar water is created.
• Mouthwash is made up of several chemicals that have been dissolved in water.
• Iodine crystals are dissolved in alcohol to create an iodine tincture.
• Sugar, carbon dioxide, colour, and other ingredients are found in soda.

### A TRUE SOLUTION

A true solution is a homogenous mixture of two or more substances in which the particle size of solute dissolved is less than 1 nm.
When we mix salt into the water, what happens after some time?
Does the salt start setting at the bottom of the beaker?
No, that doesn’t happen because it is a true solution. So, a true solution is one in which the solute doesn’t get separated out if it is kept for an indefinite time. Other examples of true solutions are sugar and water solution, air, etc.

## CONCLUSION

- Solution: A homogenous mixture of two or more substances is called a solution. 
- It is formed by mixing solute (smaller quantity) and a solvent (larger quantity). Solute and solvent can be in any state.

### FAQs:

__1. Do sand and water, when mixed, make a solution?__

No, sand and water do not mix to make a homogenous mixture. So, they do not make a solution.

__2. Is air an aqueous solution?__

No, the air is not an aqueous solution; as for aqueous solutions, the solvent should be water. But the air is a mixture of gasses.

__3. A solvent is the component of a solution that is present in a larger quantity. Is this statement right?__

Yes, the solvent is present in larger quantities while the solute is present in
smaller quantities.

*We hope you enjoyed studying this lesson and learned something cool about __Solute and Solvent__! 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!* 😎

A homogenous mixture of two or more substances is called a solution, and it is made by mixing solute and solvent.


Solute and Solvent Study Guide

## INTRODUCTION

A solution is defined as a homogeneous mixture of two or more different substances. The major portion of a solution is the solvent, and the minor portion is the solute. 

When a solute is dissolved in a solvent, the solvent particles surround and separate the solute particles in a process called dissolution. The interaction between these particles is known as solvation. Solvents and solutes with similar intermolecular forces have a stronger attraction than those with dissimilar forces. The stronger the attraction, the stronger the solubility of the solute in the solvent.

Unlike covalent molecules, ionic compounds break into positively and negatively charged ions when dissolved in a solvent. This process is called dissociation, and such solutes are known as electrolytes. 

Now that you have some background, let’s dive deeper into the details of dissociation, solvation, and electrolytes below.

### DISSOCIATION

Sodium chloride or table salt is an ionic compound formed by one sodium (Na) and one chlorine (Cl) atom. Due to its ionic nature, NaCl breaks into a positively charged cation (Na+) and a negatively charged anion (Cl-) when dissolved in a solvent. When atoms or molecules gain a positive or negative charge, it is called ionization. 

Dissociation is the process by which a larger molecule like NaCl breaks into smaller particles, and compounds that dissociate in a solution are called electrolytes. Some examples of electrolytes include sodium chloride (NaCl), hydrochloric acid (HCl), and sodium hydroxide (NaOH).

### SOLVATION

As we mentioned before, dissolution is the process in which solute particles are surrounded by solvent particles to form a solution. Dissolution signifies the kinetic process in which molecules move away from each other, which can be quantified in terms of rate. Solvation, on the other hand, is used to quantify the equilibrium state in which the rate of dissolution becomes equal to the rate of precipitation. Alterations to a solvent’s quantity can affect the rate of solvation within a solution.

### ELECTROLYTES

![Electrolytes](//images.ctfassets.net/4yflszkpcwkt/2n9BPJzgE8fp5EZvfLiows/ee99a97e833d465d1c6feec7738ee7e9/CNX_Chem_11_02_electrolyt1-1024x509.jpg)
[Source](https://courses.lumenlearning.com/chemistryformajors/chapter/electrolytes/)

Electrolytes are substances that undergo dissociation when dissolved in water and have a general electrolyte chemical formula of A+ B-.. The process of dissociation leads to the formation of charged particles known as ions. The positively charged ions are known as cations, and the negatively charged ions are known as anions. 

A unique property of an electrolyte is that it can conduct electricity when melted or dissolved in water. NaCl is a prime example of an electrolyte’s chemical formula because it breaks into Na+ and Cl- when dissolved in water.

## CONCLUSION
- Dissolution occurs when solute particles are surrounded by solvent particles to form a solution.
- Ionic solute compounds break into cations and anions when they come into contact with a solvent in a process known as dissociation.
- Solvation is a process by which solute particles interact and associate themselves with solvent particles. It is used to quantify the equilibrium state in which the rate of dissolution becomes equal to the rate of precipitation.
- Electrolytes are substances that undergo dissociation when dissolved in water to form ions. Dissolved electrolytes have the unique property of being able to conduct electricity.

### FAQs

__1. What are some examples of electrolytes?__

NaCl is a strong ionic compound, which is an example of an electrolyte. Other examples of electrolytes include KCl, NaCl, and HCl. 

__2. How can you identify an electrolyte?__

When in a dilemma regarding the question of which compounds are electrolytes, check if they break into strong ions when dissolved.

*We hope you enjoyed studying this lesson and learned something cool about __Solvation, Dissociation, and Electrolytes__! 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. Electrolytes:https://byjus.com/chemistry/electrolytes/.Accessed 8th March 2022. 
2. Solvation, Dissociation, and Electrolytes: https://www.ck12.org/c/chemistry/electrolytes-and-nonelectrolytes/enrichment/Solvation-Dissociation-and-Electrolytes-Example-1/.Accessed 8th March 2022. 


What compounds are electrolytes? Electrolytes are substances that undergo dissociation when dissolved in water. The process of dissociation leads to the formation of charged particles known as ions.


Solvation, Dissociation, and Electrolytes Study Guide

## INTRODUCTION: 
Where do we use electrolytes in daily life? Take a guess. Don't we use salt in our food? That's an electrolyte. Those special sports drinks offered to athletes are also electrolytes. The detergent we use for washing our clothes is once again an electrolyte. These are a few instances wherein electrolytes play an important role in our day-to-day lives. 

![Electrolytes in Energy Drinks](//images.ctfassets.net/4yflszkpcwkt/7FM5oZysmD51kYQO3wKuUu/d745682494d35c6e0c055549919ef0c7/5643472.png)
[Source](http://msgallagherlhs.weebly.com/electrolytes-in-energy-drinks.html)

### BUT THE QUESTION ARISES: WHAT IS AN ELECTROLYTE?

Electrolytes are substances that become ions (an atom or molecule with a net electrical charge) when they get dissolved in water and acquire the capacity to conduct electricity. A positively charged ion is called a cation, whereas a negatively charged ion is called an anion.

Based on ionization (dissociation into constituent ions) in an aqueous solution, electrolytes are of 2 types: strong and weak.

![Electrolytes](//images.ctfassets.net/4yflszkpcwkt/5bt8GIEaALG9FXxxnxmnFB/1a1fd70e208f28bfe198ab75291249e3/Electrolytes.png)
[Source](https://sciencenotes.org/electrolytes-strong-weak-and-non-electrolytes/)

### STRONG ELECTROLYTE:

Strong acids, bases, and salts are examples of strong electrolytes. In an aqueous solution, these compounds dissociate into ions.

__EXAMPLES:__

- HCl - Hydrochloric acid
- HBr - Hydrobromic acid
- HI - Hydroiodic acid
- NaOH - Sodium hydroxide
- NaCl - Sodium chloride

### WEAK ELECTROLYTE:

In water, weak electrolytes only partially disintegrate into ions. Weak acids, bases, and a range of other substances are examples of weak electrolytes. The majority of nitrogen-containing substances are weak electrolytes.

__EXAMPLES:__

- HF - Hydrofluoric acid
- CH₃CO₂H - Acetic acid
- NH₃ - Ammonia
- H₂O - Water

![WEAK ELECTROLYTE](//images.ctfassets.net/4yflszkpcwkt/2a9LDOXjHBq2iZcFGnqbyA/b8b02f0a9493abdf1979b378b2f0d38b/elec2.gif)
[Source](https://www.stolaf.edu/depts/chemistry/courses/toolkits/121/js/naming/elec.htm)

## CONCLUSION: 

- An electrolyte is a substance that dissolves in water and acquires the capacity to conduct electricity.
- There are two types of electrolytes- strong and weak electrolytes.
- A strong electrolyte is an electrolyte that dissolves almost completely in water. An example of a strong electrolyte is Hydrogen Chloride (HCl).
- A weak electrolyte is an electrolyte that doesn't dissolve completely in water.

### FAQs: 

__1. Is HCl acid a strong electrolyte?__

Yes, hydrogen chloride is a strong electrolyte, and it dissolves in water completely to form Hydrogen ions and chlorine ions.

__2. Why is HCl an electrolyte?__

HCl is an electrolyte because it completely dissolves to form hydrogen ions and chloride ions when mixed with water. These together conduct electricity. Hence, it's an electrolyte.

__3. When does HCl act as a non-electrolyte?__

In its pure form, HCl gas is a non-electrolyte. Electrolytes are formed once it's dissolved in water. Since hydrogen chloride gas is not dissolved in water, it's a non-electrolyte.

*We hope you enjoyed studying this lesson and learned something cool about __Strong and Weak Electrolytes__! 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. Strong and Weak Electrolytes. https://www.ck12.org/c/chemistry/strong-and-weak-electrolytes/lesson/Strong-and-Weak-Electrolytes-CHEM/ accessed 17 Feb 2022
2. Chemistry Examples: Strong and Weak Electrolytes. https://www.thoughtco.com/strong-and-weak-electrolytes-609437 accessed 17 Feb 2022


Electrolytes are substances that become ions when they get dissolved in water.


Strong and Weak Electrolytes Study Guide

TL;DR A Complete Guide to the Dissolution Process

TL;DR Electrolytes and Non-Electrolytes

TL;DR Structure Of Water

## INTRODUCTION

Water is one of the most precious resources on the earth. Though 71% of our planet’s surface is covered by water, only 3% is freshwater, and of that 3%, only 1.2% is safe for human consumption. Water is necessary for a multitude of life-sustaining activities, such as drinking and household needs, recreation, agriculture, industry, and thermoelectricity. Its unusual properties make it integral not only for human activities, but also the biological processes that keep every other living being on the planet alive. Let’s learn about its structure to gain a better understanding of why it’s so important.

## WHAT IS THE STRUCTURE OF WATER?

![Structure of Water](//images.ctfassets.net/4yflszkpcwkt/2Uz4hFdjYYpslpNbON48Hf/5f660fae2b7377252dcfcfa6c1cd2a3e/f-d_f45c7d78874201970958daf29d7bd7b304d46aedfdc403ae9231b788_IMAGE_THUMB_POSTCARD_TINY_IMAGE_THUMB_POSTCARD_TINY.1)
[Source](https://www.ck12.org/c/chemistry/structure-of-water/lesson/Structure-of-Water-CHEM/) 

A water molecule consists of one oxygen atom bound to two hydrogens by covalent bonds. A covalent bond is characterized by the sharing of one or more electron pairs between two atoms. When a covalent bond is formed between atoms of significantly different electronegativities, it is classified as a polar bond. Because oxygen has a higher electronegativity than hydrogen, water is considered a polar molecule.

Polar bonds result in an unequal sharing of electrons. The oxygen atom in a water molecule attracts the shared electron pairs to a greater degree and thus acquires a partial negative charge (δ−), while each hydrogen acquires a partial positive charge (δ+). As a result, the H-O-H bond is bent at a 105o angle.

Polar water molecules attract each other by dipole-dipole forces, where the positive end of a molecule is attracted to the negative end of another. Each hydrogen atom on a molecule strongly attracts a lone pair of electrons on an adjacent water molecule. This results in the formation of a hydrogen-hydrogen bond, which is stronger than a dipolar one.

## CONCLUSION

- The chemical formula of water is H₂O.
- In a water molecule, two atoms of hydrogen and one atom of oxygen are bound together by covalent bonds.
- The shared electrons of each covalent bond are attracted to the oxygen atom to a greater degree because of its stronger electronegative force.
- The tilt of the shared electron results in hydrogen acquiring a positive charge and oxygen acquiring a partial negative charge.
- The partial charges result in a bent shape of the molecule, arranged at a 105° angle. This is the bond angle of water.  
- Polar water molecules attract each other by dipole-dipole forces, where one end of the positive molecule is attracted by the negative end of another polar molecule.
- Each hydrogen atom on a molecule strongly attracts a lone pair of electrons on an adjacent water molecule. This results in the formation of a hydrogen-hydrogen bond.

### FAQs

__1. What kind of bond joins hydrogen to oxygen in a water molecule?__

A polar covalent bond.

__2. Does water have a bond angle of 180°?__

No, a Water molecule is a bond arranged at an angle of 105°.

__3. What is the bond shape of water?__

The bond shape of the water is a bent structure.

*We hope you enjoyed studying this lesson and learned something cool about the __Structure Of Water__! 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. Structure of water: https://www.ck12.org/c/chemistry/structure-of-water/lesson/Structure-of-Water-CHEM/. Accessed 8th March 2022.
2. Structure of Water: https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/15%3A_Water/15.01%3A_Structure_of_Water. Accessed 8th March 2022.

The structure of the water molecule is a covalent bond formed at a 105o water bond angle. 


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