Types of Chemical Reactions
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- Опубліковано 10 чер 2017
- This chemistry video tutorial explains how to classify different types of chemical reactions such as synthesis reactions or combination reactions, decomposition reactions, single replacement reactions, combustion reactions, double replacement reactions, precipitation reactions, acid base neutralization reactions, redox reactions, and gas evolution reactions. This video contains plenty of examples and practice problems.
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Calculating Oxidation Numbers:
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Oxidation and Reduction Reactions:
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Types of Chemical Reactions
1- Combustion Reaction
• in combustion, something is burning and it releases a lot of heat energy.
• if you see CO2 and water in the product then it's a combustion reaction.
• All "Combustion" reactions are "Redox Reactions".
2- Synthesis\Combination reaction
• A + B = AB
• you simply combine the reactants to make the product.
• If two pure elements combine to form a compound then it's a "Redox Reaction".
• If two small compounds combine to form a large compound then it's probably NOT a "Redox Reaction".
3- Decomposition reaction
• AB = A + B
• the opposite of the Synthesis\Combination reaction: simply breaks down reactants to make the product.
• heat and electricity cause decomposition reactions
• If a compound breaks down into pure elements then it's a "Redox Reaction".
• If a large compound breaks into two small compounds then it's probably NOT a "Redox Reaction".
4- Single replacement reaction
• A + BC = AC + B
• Just as the name says, a single molecule from the same equation replaces another.
• For the most part, metals tend to replace metals and nonmetals tend to replace nonmetals.
• All "Single Replacement" reactions are "Redox Reactions".
5- Double Replacement reaction
• AB + CD = AD + BC
similar to the Single replacement reaction; however, this one is double, and completely switches elements' places up.
• Both of the reactants must be aqueous
• When a double replacement happens between two aqueous solutions and the products all remain aqueous then no reaction took place.
• A "Double Replacement" reaction is NEVER a "Redox reaction"
• Double Replacement reaction types:
- if a double replacement of two aqueous products happens and you find a solid in the product then it's called a "Precipitation Reaction".
- If a double replacement happens between a strong acid and a strong base it will produce water and salt and will be called "Acid-Base Neutralisation Reaction".
- if a double replacement of two aqueous products happens and you find a gas in the product then it's called a "Gas Evolution Reaction".
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-Redox Reactions: Also called "oxidation-reduction reaction", is any chemical reaction in which the oxidation number of atoms changes.
-Methane(CH4) is also called: Natural gas.
-Almost all ionic compounds are considered salts.
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Isn't a base-acid neutralization reaction a redox reaction and also a double replacement reaction but you said double replacement reactions are never redox
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Here are some timestamps
Synthesis- 2:10
Decomposition- 4:21
Single Replacement- 9:00
Double replacement- 12:08
Combustion- 0:00
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Synthesis: Putting Together
Decomposition: Breaking Up
Single Replacement: “I’m leaving you for your friend”
Double Replacement: “Wife Swap”
Combustion: “Taylor Swift”
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All Credits to my science teacher
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The Taylor Swift one: does the same thing over and over again. Gets a boy. They break up. She writes a song.
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Hope this helps!
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Would you please tell how we can find out when it is aqueous,liquid or solid?
Solubility rules, H2O will typically be liquid unless it's a combustion reaction
Use a solubility chart
it should say it in the question
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when i read the notes i didn't understand but after watching this tutorial, i clearly understand and can differentiate between different types of reactions. thanks alot
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Professor Organic Chemistry Tutor, thank you for explaining and analyzing different types of Chemical Reactions in AP/General Chemistry. All Chemical Reactions come with different compounds. Breaking down large compounds into small compounds is an excellent way to comprehend Chemical Reactions. This is an error free video/lecture on UA-cam TV with the Organic Chemistry Tutor.
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Save time here:
Synthesis
a+b -> ab
Decomposition
ab -> a+b
Single replacement
A+BC -> AC+B
Double Replacement
AB+CD -> AD + BC
Combustion
using heat and basically anything with O2
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23:50 How do you know when a product is solid vs aqueous/soluble? Just memorize everything?
It's based off of the solubility rules. He has a video on that as well.
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I need help figuring out redox and neutralization reactions
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In 37:37, is it also possible to have a combustion reaction there since it produced water and CO2?
on 28:39 one of the products isn't Na2SO4 but K2SO4.
Yes! Nobody seems to notice
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In the decomposition ex. 1 Why does metal oxide has still oxygen, if all the gases will escape to the air?
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(Decomposition or analysis) vs (combination or synthesis), I believe analysis was missing at decomposition part
I learned so much and you give so much example, that I may be able to learned and to understand the 4 chemical reactions THANK YOU!!!
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In your other video of Predicting the Reaction
You have inverted Synthesis and Decomposition reaction
Pls, I'm confused which one is correct
Just know that synthesis is the coming together of two elements to make a compound or the coming together of two compounds to make a larger compound while decomposition is the breaking down of compound which is the product into elements which is the reactants
With the simple replacement reaction when do you know when to replace A with B or C ?
Always the first one
I get how you do the reactions but not the why
Why does there have to be a reaction in general?
E.g. Na2S + HCl -> NaCl + H2S
Does everything react or do some stay the same?
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Fondamental lecture!!!!
30:13 does k become (k)2 due to the separation from O and H?
22:16 why the reaction takes place since Pb is less reactive than Na?
PLEASE SOMEONE ANSWER ME
Mg + O2 = Mgo...can this be also a combustion reaction? coz a lot of heat and light is given off.
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Why at 8:35 is the top equation not an acid replacement? Doesn’t an acid replacement produce salt and water?
27:12 would that be a complete combustion?
12:00 why doesn't the Br from the 3rd question have the 2 subscript and are we supposed to write all diatomic elements with their subscript in the second half of the equation? i.e., you said sodium iodide which implies it is not in it's natural state, but then you wrote I subscript 2. thanks!
this might be late, but will respond. Br in nature is always in a molecule state. A molecule is a diatomic cuz they always come in pair. did you memorize that chart and the diatomic elements? well here it is when it comes to execute what you learn in that section.. You will not find a Br atom by itself in nature.
Gordon's chem class wya
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