Unit 1 - Redox Flashcards

1
Q

How do metal displacement reactions occur?

A

When a metal higher up in the electrochemical series displaces a metal in solution which is lower than itself.

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2
Q

What is reduction?

A

A gain of electrons by something

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3
Q

What is oxidation?

A

A loss of electrons by something

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4
Q

What is a reducing agent?

A

Something that allows reduction to take place

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5
Q

What is an oxidising agent?

A

Something that allows oxidation to take place

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6
Q

What happens to a reducing agent?

A

It is oxidised

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7
Q

What happens to an oxidising agent?

A

It is reduced

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8
Q

In a redox reaction what takes place at the same time?

A

Oxidation and reduction

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9
Q

What are good oxidising agents?

A

Things with high electronegativity

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10
Q

What are good reducing agents?

A

Things with low electronegativity

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11
Q

How do elements with low electronegativities tend to form ions?

A

By losing electrons (oxidation)

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12
Q

How do elements with high electronegativities tend to form ions?

A

By gaining electrons (reduction)

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13
Q

When combining reduction and oxidation equations to form a redox equation what MUST be the same number?

A

The electrons must be equal, equations can be multiplied to make this happen

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14
Q

Where are the oxidising agents in the electrochemical series?

A

The top - they will be reduced so things with high electronegativity will do this well

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15
Q

Where are the reducing agents in the electrochemical series?

A

The bottom - they will be oxidised so things with low electronegativity will do this well

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16
Q

In redox equations what can we add to balance charges?

A

electrons and H+ ions

17
Q
A