3 Redox I Flashcards

1
Q

Define “oxidation”

A

Gain of oxygen or removal of hydrogen/electrons

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2
Q

Define “reduction”

A

Gain of hydrogen/electrons or removal of oxygen

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3
Q

Define “redox”

A

When reduction and oxidation take place

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4
Q

How does electronegativity changes within different elements?

A

Electronegativity increases across a period and decreases down a group

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5
Q

When would hydrogen not have an oxidation state of +1?

A

As atoms and molecules (0) or hydride ion in metal hydrides (-1)

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6
Q

When would oxygen not have an oxidation state of -2?

A

As atoms and molecules (0), in hydrogen peroxide (-1) or in F2O (+2)

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7
Q

When would fluorine not have an oxidation state of -1?

A

As atoms and molecules (0)

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8
Q

How do metals behave in redox?

A
  • have positive values in compounds
  • value is usually that of the Group No.
  • several possibilities the values go no higher than the Group No.
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9
Q

How do non-metals behave in redox?

A
  • mostly negative based on their usual ion
  • can have values up to their Group No.
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10
Q

Define “disproportionation reaction”

A

A reaction in which an element in a single species is being simultaneously oxidised and reduced

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