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Chemical Reactions Part 3 > Chemical Reactions > Flashcards

Chemical Reactions Flashcards

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Organic Chemistry 101 flashcards
1
Q

Where are the reactants listed in a word equation?

A

The left side

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2
Q

Where are the products in a word equation?

A

The right side

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3
Q

What are reactants?

A

The substances which are present initially in a chemical reaction

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4
Q

What are products?

A

The substances which are present at the end of a chemical reaction

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5
Q

What does the arrow mean in a chemical equation?

A 
Yield
Forms
Produces
Reacts to produce
Decomposes into
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6
Q

What is always present when something burns?

A

Oxygen

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7
Q

What are some diatomic atoms?

A

Nitrogen Hydrogen Florine Oxygen Iodine Carbon

Bromine

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8
Q

What does the law of conservation state?

A

The mass of the reactants must be equal to the mass of the products

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9
Q

What are the 5 basic types of chemical reactions?

A 
Synthesis    A+B=AB
Decomposition   AB= A+B
Single replacement   A+BC=AC+B
Double replacement  AB+XY=AY+XB
Combustion
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10
Q

What’s synthesis?

A

The combination of 2 of more substances to make a compound

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11
Q

What’s decomposition?

A

One substance breaks down to create 2 or more similar substances

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12
Q

What’s single replacement?

A

Occurs when one element is replaced by another

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13
Q

What’s double replacement?

A

Occurs when elements in a solution of compounds exchange places or replace each other

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14
Q

What’s combustion?

A

Involves the burning of a hydrocarbon in the presence of oxygen to form carbon dioxide and water

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15
Q

What are 3 characteristics of acids?

A

Water soluble
Conducts electricity
Reactive

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16
Q

What are 4 characteristics of bases?

A

Conducts electricity
Water soluble
Slippery when in aquas solution
Bitter tasting

17
Q

What are 3 examples of acids?

A

Sulfuric Acid
Vinegar
Citric Acid

18
Q

What are 3 examples of bases?

A

Sodium hydroxide
Bleach
Potassium hydroxide
Aluminum hydroxide

19
Q

What’s an example of a neutral substance?

A

Water

20
Q

How is acidity measured?

A

pH scale

21
Q

What’s is a universal indicator?

A

Is a substance that turns different colours in solution with different pH values

22
Q

What’s the advantage of using universal indicators rather than litmus paper?

A

You immediately know the pH

23
Q

What’s a rate of reaction?

A

The speed of a reaction

24
Q

How to reactions take place?

A

Reactions take place when particles collide with a certain amount of energy

25
Q

What’s activation energy?

A

The minimum amount of energy needed for the particles to react

26
Q

What does the rate of reaction depend on?

A

Frequency and Energy

27
Q

What are factors that affect the rate of reaction?

A 
Increased Temperature 
Increased surface area
Use of a catalyst
Increased concentration of reactants
Increased pressure of gaseous reactants
28
Q

Why does heat speed of the rate of reaction?

A

At higher temperature particles have more energy. This means they move more and are more likely to collide with other particles

29
Q

What do catalysts do?

A

They speed up the rate of reaction. They do this by lowering the activation energy so less energy is needed to start a reaction

30
Q

What are 3 examples of catalysts?

A

Nickel
Iron
Platinum

31
Q

Why are catalysts important for industry?

A

Products can be made more quickly, saving time and money. Catalysts reduce the need for heat saving fuel and reducing pollution.

32
Q

What’s another name for an acid-base reaction?

A

Neutralization reactions

33
Q

What are the products of acid-base reactions?

A

Water and salt

34
Q

Give an example of acid-base reaction

A

Hydrobromic acid+sodium hydroxide = water + salt

35
Q

How can we describe chemical reactions?

A

Word Equation
Skeleton Equation
Balanced Equation

Chemical Reactions Part 3 (1 decks)

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