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1. Science 20 Bilingual > A: Chemistry = Chemical Changes 2.3 The Reactivity of Metals > Flashcards

A: Chemistry = Chemical Changes 2.3 The Reactivity of Metals Flashcards

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1
Q

What do you think prospectors risked in order to get rich mining in the Yukon?

A

All that they owned and even their very lives

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2
Q

What can even relatively small amounts of gold make a person?

A

Very wealthy

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3
Q

What can cause the price of gold to fluctuate?

A

Market demand and other economic factors

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4
Q

How much was a small coffee cup filled with fine grains of gold worth in December 2005?

A

Over $80,000

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5
Q

What are the two main reasons that make gold a valuable metal?

A

Attractive appearance and its physical and chemical properties

Being rare also makes it more valuable and would be an acceptable answer.

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6
Q

Fill in the blank: Gold is considered a _______ metal.

A

Precious

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7
Q

True or False: Gold’s value is solely based on its appearance.

A

False

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8
Q

What activity related to gold is still a hobby for many people today?

A

Panning for gold

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9
Q

What is the most malleable and ductile metal known?

A

Gold

Gold’s malleability and ductility make it ideal for creating jewellery and intricate objects.

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10
Q

How thin can a gram of gold be stretched into wire?

A

Thinner than a human hair, 3.5 km long

A gram of gold can also be beaten into a sheet measuring 1 m by 1 m.

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11
Q

Does gold readily react with other elements?

A

No

Gold is a very stable metal and does not corrode or tarnish easily.

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12
Q

What happens to metal atoms during corrosion?

A

They are oxidized to form metal ions

Corrosion is a process that affects metals, leading to their degradation.

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13
Q

What makes gold almost indestructible from a chemical perspective?

A

It can resist the action of most strong acids

Gold’s stability allows it to be used and reused for centuries.

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14
Q

What is a significant factor that contributes to gold being considered a precious metal?

A

Its rarity

All refined gold in the world could form a cube with each side measuring 20 m.

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15
Q

Fill in the blank: Gold is so stable that it does not readily undergo _______.

A

corrosion

This property is due to gold’s strong tendency to keep its electrons.

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16
Q

True or False: Gold objects tarnish easily.

A

False

Gold does not tarnish or undergo corrosion due to its stability.

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17
Q

What property makes gold a precious metal?

A

Gold tends to not participate in chemical reactions

This property is due to its stability and reluctance to lose electrons.

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18
Q

Which other metal is indicated to have low chemical reactivity similar to gold?

A

Silver

Silver also tends to not be chemically reactive.

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19
Q

What occurs at the atomic level during chemical reactions?

A

Electrons are exchanged

This exchange is crucial for the formation of chemical compounds.

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20
Q

What do gold and silver atoms tend to do with their electrons?

A

They tend not to readily lose their electrons

This behavior contributes to their stability and low reactivity.

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21
Q

What is the relationship between metal stability and reactivity as an ion?

A

The more stable a metal atom is, the more reactive it is as an ion

This trend indicates that stability influences reactivity in metal ions.

For example, silver ions would much rather be silver solid metal more than other metal ions might want to be in their network metal form. Silver has a stronger tendency to do this even if the other metal slightly wants the same thing.

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22
Q

Which metal ION was found to be the most reactive in the previous investigation?

A

Silver ions, Ag (aq)

Their reactivity is due to their ability to gain electrons.

Silver ions have lost their electrons but would much rather have them back, so they will react to get their electrons back and no longer be an ion anymore.

They have a greater pull for electrons than the other metal ION would have.

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23
Q

Fill in the blank: The tendency of silver ions to react indicates they must be able to gain _______ in order to increase stability.

A

electrons

Gaining electrons helps increase the stability of silver ions.

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24
Q

True or False: Gold and silver are very unstable metals.

A

False

Gold and silver are characterized as very stable metals.

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25
Is it possible for a metal to be more stable in its ionic form than in its uncharged form?
Yes, a metal can be more stable in its ionic form ## Footnote This leads to the metal readily oxidizing and undergoing corrosion.
26
Which metal exemplifies the trend of stability in ionic form?
Iron ## Footnote Iron readily corrodes unless protected.
27
What happens to iron if it is not protected?
It readily corrodes ## Footnote Corrosion occurs unless measures are taken to protect the iron.
28
What is a consequence of iron being used in production?
It has undergone corrosion ## Footnote A significant amount of iron produced each year is affected by corrosion.
29
Fill in the blank: The metallic atom would readily ______ and easily undergo corrosion.
oxidize ## Footnote Oxidation is a key process leading to corrosion.
30
True or False: Iron is less likely to corrode if it is left unprotected.
False ## Footnote Iron is likely to corrode when unprotected.
31
What is the relationship between a metal's stability in ionic form and its susceptibility to corrosion?
A metal that is more stable in its ionic form is more susceptible to corrosion ## Footnote This is because it readily oxidizes.
32
What is the Activity Series?
A list that ranks metal atoms from most reactive to least reactive. This card doesn't state which is placed where in the actual activity series. More on placement to come later.
33
What governs the reactivity of metal atoms?
General rules that dictate the behavior of metallic ions.
34
Fill in the blank: The Activity Series organizes metal IONS from ______ to least reactive.
[most reactive] The ones at the top are most likely to be ions because the ones at the bottom are more likely to want to be neutrals more. The ones at the top are most likely to oxidize and thus are called reducing agents because they force the ones at the bottom to no longer be ions.
35
What type of metals are included in the Activity Series?
Metal atoms.
36
True or False: The Activity Series can be used to predict the reactivity of metals in solutions.
True.
37
What can be inferred from a metal's position in the Activity Series?
Its relative reactivity compared to other metals.
38
What is the significance of the Activity Series in chemistry?
It helps in understanding and predicting chemical reactions involving metals.
39
Fill in the blank: The Activity Series is organized based on the ______ of metal atoms.
[reactivity]
40
What is the activity series used for?
A tool to compare the reactivity of metals and metal ions
41
In the activity series, which ion is more likely to undergo reduction: Copper ion or Zinc ion? (Which is most likely to not stay in ionic formation?)
Copper ion Zinc is more reactive than copper metal and so it can displace copper from copper sulphate solution. Zinc displaces the metals present below it in the series. Zinc has a higher tendency to oxidize, losing electrons, and forming ions. When looking at the ions, you must reverse everything. So the copper ion is more likely to want to return back to solid copper, since zinc would like to remain an ion and be reactive in that way.
42
What does the position of metal ions in the activity series indicate?
The relative reactivity of metals.
43
In the activity series, do metals lower in the series have higher or lower reactivity?
Lower reactivity They are less likely to oxidize and form ionic compounds.
44
Which is more reactive according to the activity series: Cu(s) or Ag(s)? (Which is the most likely to oxidize and lose electrons?)
Cu(s) Copper is more likely to oxidize and become an ion in comparison to silver.
45
What characterizes a spontaneous reaction?
Occurs without the addition of external energy
46
What is an example of a spontaneous reaction observed in the investigation?
Placing a strip of zinc metal in a solution containing silver ions The zinc wants to oxidize more than if the situation were reversed giving a chance for silver to oxidize. Zinc wants to be ionic more than silver.
47
What type of reaction occurs when a strip of silver metal is placed in a solution of zinc ions?
Non-spontaneous reaction It would take energy to take make zinc so being an ion. Silver would rather not react if zinc is around instead to do the reacting.
48
What determines whether a reaction will occur between a metal and a metal ion in solution?
The activity series If the metal is more likely to oxidize then it is most likely to be found in an ionic compound and displace the other metal that was there. In this chart the metals most likely to oxidize are on top. Notice that gold is on the bottom since it would prefer to not react.
49
How are stronger oxidation reactions represented in the activity series?
Closer to the top of the series
50
How are stronger REDUCTION reactions represented in the activity series pictured?
Closer to the bottom of the series
51
Fill in the blank: A spontaneous reaction occurs if a metal ion has a stronger tendency to _______ electrons than a metal atom.
gain This is because the metal atom (the one that might want to react and oxidize) would prefer to lose electrons. So the ION prefers to gain in a reduction reaction so that the ATOM can lose electrons, because the atom is found to be more likely to oxidize in the activity series.
52
Fill in the blank: A non-spontaneous reaction does not occur without the addition of _______ energy.
external
53
True or False: This activity series compares the ability of metal ions to donate electrons.
False Technically shows the ability to reduce, since the equation arrow points to the right, so compares the ability to metal ions to gain electrons and lead themselves back. Re + duct = lead back
54
In the activity series, which ion is more reactive: Cu (aq) or Zn (aq)?
Cu (aq) They are asking which is most likely to change, and since the only option here for both of these is to no longer be an aqueous ion they only have the option of undergoing reduction. Copper is already an ion and would less hate to no longer be one, gaining back is electrons and undergoing reduction, mostly because Zn wants to oxidize more than copper does. Zn is bossy and wants to oxidize so much that copper is forced to reduce. So zinc is the stronger reducing agent because it forces copper to reduce. Zinc would most like to oxidize.
55
What does the position of metal ions in the activity series indicate?
The relative reactivity of metal ions
56
In the activity series, do metals lower in the series have higher or lower reactivity?
Higher reactivity
57
Which is more reactive according to the activity series: Cu(s) or Ag(s)?
Cu(s)
58
What characterizes a spontaneous reaction?
Occurs without the addition of external energy
59
What is an example of a spontaneous reaction observed in the investigation?
Placing a strip of zinc metal in a solution containing silver ions
60
What type of reaction occurs when a strip of silver metal is placed in a solution of zinc ions?
Non-spontaneous reaction
61
What determines whether a reaction will occur between a metal and a metal ion in solution?
The activity series
62
How are stronger reduction reactions represented in the activity series?
Closer to the top of the series
63
How are stronger oxidation reactions represented in the activity series?
Closer to the bottom of the series
64
Fill in the blank: A spontaneous reaction occurs if a metal ion has a stronger tendency to _______ electrons than a metal atom.
gain
65
Fill in the blank: A non-spontaneous reaction does not occur without the addition of _______ energy.
external
66
True or False: The left side of the activity series compares the ability of metal ions to donate electrons.
False
67
What is the primary function of the activity series?
To predict whether a reaction will occur
68
What is the significance of the placement of half-reactions in the activity series?
Indicates the tendency to gain or donate electrons
69
What is the reduction half-reaction in the zinc and copper solution scenario? A piece of zinc metal is placed in a solution containing Cu 2+ (aq).
Cu (aq) + 2e⁻ → Cu (s) ## Footnote This reaction describes the gain of electrons by copper ions.
70
What is the oxidation half-reaction in the zinc and copper solution scenario?
Zn (s) → Zn (aq) + 2e⁻ ## Footnote This reaction describes the loss of electrons by zinc metal.
71
How can you determine if a reaction is spontaneous based on half-reactions?
If the reduction half-reaction is above the oxidation half-reaction in the activity series, the reaction will be spontaneous. ## Footnote The activity series ranks metals based on their reactivity.
72
What would you observe in the reaction between zinc metal and copper ions?
Copper ions would precipitate out as copper metal, and zinc would enter the solution as zinc ions. ## Footnote A visible precipitate of copper metal would form.
73
Fill in the blank: In the reaction between zinc and copper, copper ions _______ and zinc metal _______.
precipitate out as copper metal; enters the solution as zinc ions.
74
What is a reducing agent?
A substance that makes the reduction process possible by losing electrons. ## Footnote In a reaction, the reducing agent is oxidized.
75
What is an oxidizing agent?
A substance that makes the oxidation process possible by gaining electrons. ## Footnote In a reaction, the oxidizing agent is reduced.
76
In the reaction Zn(s) + 2 AgNO₃(aq) → Zn(NO₃)₂(aq) + 2 Ag(s), which substance acts as the reducing agent?
Zinc (Zn) ## Footnote Zinc promotes the reduction of silver nitrate by losing electrons.
77
In the reaction Zn(s) + 2 AgNO₃(aq) → Zn(NO₃)₂(aq) + 2 Ag(s), which substance acts as the oxidizing agent?
Silver nitrate (AgNO₃) ## Footnote Silver nitrate promotes the oxidation of zinc by gaining electrons.
78
True or False: Oxidation and reduction can occur independently of each other.
False ## Footnote Oxidation and reduction always occur together.
79
Fill in the blank: A reducing agent is oxidized when it _______.
loses electrons.
80
Fill in the blank: An oxidizing agent is reduced when it _______.
gains electrons.
81
How can the term 'agent' help in understanding the roles of reducing and oxidizing agents?
It indicates what the substance does. ## Footnote For example, a reducing agent makes reduction possible, similar to how a travel agent facilitates travel.
82
What happens to silver in the reaction Zn(s) + 2 AgNO₃(aq) → Zn(NO₃)₂(aq) + 2 Ag(s)?
Silver gains electrons. ## Footnote This indicates that silver is being reduced.
83
What is a reducing agent?
A substance that makes the reduction process possible by losing electrons. ## Footnote In a reaction, the reducing agent is oxidized.
84
What is an oxidizing agent?
A substance that makes the oxidation process possible by gaining electrons. ## Footnote In a reaction, the oxidizing agent is reduced.
85
In the reaction Zn(s) + 2 AgNO₃(aq) → Zn(NO₃)₂(aq) + 2 Ag(s), which substance acts as the reducing agent?
Zinc (Zn) ## Footnote Zinc promotes the reduction of silver nitrate by losing electrons.
86
In the reaction Zn(s) + 2 AgNO₃(aq) → Zn(NO₃)₂(aq) + 2 Ag(s), which substance acts as the oxidizing agent?
Silver nitrate (AgNO₃) ## Footnote Silver nitrate promotes the oxidation of zinc by gaining electrons.
87
True or False: Oxidation and reduction can occur independently of each other.
False ## Footnote Oxidation and reduction always occur together.
88
Fill in the blank: A reducing agent is oxidized when it _______.
loses electrons.
89
Fill in the blank: An oxidizing agent is reduced when it _______.
gains electrons.
90
How can the term 'agent' help in understanding the roles of reducing and oxidizing agents?
It indicates what the substance does. ## Footnote For example, a reducing agent makes reduction possible, similar to how a travel agent facilitates travel.
91
What happens to silver in the reaction Zn(s) + 2 AgNO₃(aq) → Zn(NO₃)₂(aq) + 2 Ag(s)?
Silver gains electrons. ## Footnote This indicates that silver is being reduced.
92
What is the relationship between the stability of metal atoms and their reactivity as metal ions?
The more stable a metal atom is, the more reactive it is as a metal ion. ## Footnote This indicates a direct correlation between stability and reactivity in metal chemistry.
93
What can be inferred about the reactivity of metal ions based on their stability?
The more stable a metal ion is, the more reactive it is as a metal. ## Footnote This suggests that stability influences the ability of metal ions to participate in chemical reactions.
94
What does the activity series for metals and metal ions indicate?
It lists metal ions from most reactive to least reactive and metals from least reactive to most reactive. ## Footnote This series is crucial for predicting chemical reactivity and potential reactions.
95
How can the activity series be used in chemical reactions?
It can be used to predict whether a reaction between a metal and a metal ion will be spontaneous or non-spontaneous. ## Footnote Understanding the activity series helps chemists determine reaction feasibility.
96
Fill in the blank: The more stable a metal atom is, the more reactive it is as a _______.
metal ion
97
True or False: A less stable metal ion is more reactive as a metal.
False ## Footnote The statement contradicts the relationship established between stability and reactivity.
98
Fill in the blank: The activity series helps predict whether a reaction will be _______ or non-spontaneous.
spontaneous

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