Chapter 11: Oxidation-Reduction Reactions Flashcards

1
Q

Oxidation is ________

A

loss of e-

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2
Q

Reduction is ________

A

gain of e-

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3
Q

An oxidizing agent causes what?

A

Causes an atom to be oxidized, and is itself reduced

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4
Q

A reducing agent causes what?

A

Causes an atom to be reduced, and is itself oxidized

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5
Q

Almost all oxidizing agents contain what?

A

oxygen or another strongly electronegative element

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6
Q

What are some common oxidizing/reducing agents?

A
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7
Q

________________ ____________ are assigned to atoms to keep track of redistribution of electrons during chemical reactions

A

Oxidation numbers

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8
Q

What is the oxidation number of a free element?

A

Zero

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9
Q

The oxidation number of a monatomic ion is equal to what?

A

The charge of the ion

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10
Q

The oxidation number of Group VIIA is -1, except for when?

A

When combined with an element of higher electronegative.

Example: Cl- is -1 in HCl, but it is +1 in HOCl

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11
Q

Hydrogen is usually ____. However, it is ____ in compounds with less electronegative elements from Groups ____ and ____.

Hydrogen is ____ in HCl, but ____ in NaH.

A

+1; -1; Groups IA and IIA
+1, -1

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12
Q

In most compounds, the oxidation number of oxygen is ____. Except in peroxides (O22-), where oxygen is ____, and compounds with more electronegative elements like OF2, where oxygen is ____.

A

-2; -1, +2

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13
Q

The sum of oxdiation numbers in a neutral compound should be ____

A

zero

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14
Q

The sum of oxidation numbers of the atoms present in a polyatomic ion is equal to ____

A

the charge of the ion

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15
Q

Oxidation number assumes ________ ________ of electrons in bonds, “awarding” the electrons to the more electronegative element.

A

unequal division

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16
Q

Formal charge assumes ________ ________ of electrons in bonds, awarding one electron to each atom in the bond.

A

equal division

17
Q

When assigning oxidation numbers, start with what?

A

The known atoms

18
Q

What does assigning oxidation numbers accomplish?

A

Allows us to determine how many moles of each species are required for conservation of charge and mass, which is necessary to balance the equation

19
Q

How does the half-reaction method work?

A

Separate the redox reaction into two half-reactions, the oxidation part and the reduction part, then they are balanced separately

20
Q

________________ is a specific type of redox reaction in which an element undergoes both oxidation and reduction in producing its products.

A

disproportionation

21
Q

What is an example of disproportionation?

A

catalysis of peroxides by catalase