1.7 Redox Flashcards

1
Q

What is oxidation

A

The loss of electrons

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2
Q

What is reduction

A

The gain of electrons

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3
Q

What is a redox reaction

A

Transfer of e-
e- lost must equal e- gained

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4
Q

What is a half equation

A

Separate equations showing the oxidation and reduction process
Must be balanced in terms of atoms and charge

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5
Q

What is an oxidation state

A

OS of an element is the number of electrons involved when at atom forms a bond
OS state refers to one atom of the element in a compound or ion
OS has a number and a sign

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6
Q

What are the rules for assigning OS

A

-An uncombined element has an OS of zero
-Some elements have the same OS in all their compounds
-For a compound, the OS of each atom in the compounds formula counts separatley and the numerical sum is zero
-For an element exsisting as an ion , the OS is the charge on that ion
-For compound ions the sum of the OS of the atoms is the charge on the ion

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7
Q

What is the exceptions of the OS of H

A

Normally +1
In metal hydrides it is -1

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8
Q

What is the exception of the OS of O

A

Normally -2
In peroxides and when combined with F it is -1

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9
Q

What is the exception for the OS of Cl

A

Normally -1
When combined with O it varies

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10
Q

What do roman numeral indicate

A

The OS
To differentiate between oxo-acids
Naming salts and oxo-anions

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11
Q

How do OS link with redox reactions

A

Oxidation is an increase in OS
Reduction is a decrease in OS

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12
Q

What is an oxidising agent

A

A specis that accepts electrons

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13
Q

What is a reducing agent

A

A species that donates electrons

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14
Q

How do you balance more complex half equations

A

-Balance atoms undergoing redox
-Balance any oxygen atoms by adding water
-Balance H atoms by adding H+ ions
Balance charges by adding electrons

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15
Q

How do you combine half -equations

A

One equation must show oxidation and the other reduction
The number of e- being transferred but be the same
2 half equations can be added and any species that appears on both sides of equation are canclled

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