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chem unit 1 > ch 3- reactions of metals > Flashcards

ch 3- reactions of metals Flashcards

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1
Q

-Ore(n.)

A

Deposit in Earth’s outermost layer containing metals and other minerals

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2
Q

-Cation(n.)

A

Positive ions formed when an atom loses its valence electrons

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3
Q

Where are metals extracted from

A

Metals are extracted from ores in the earth’s crust

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4
Q

Characteristics of metals in relation to ionisation energy

A

-Metals have low ionisation energies.
-Therefore, relatively small amounts of energy is required to remove valence electrons from atoms.
-When metal atoms lose one ore more valence electrons, they form cations.

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5
Q

-Metallic bonding(n.)

A

The electrostatic force of attraction between delocalised electrons and cations in a metallic lattice structure.

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6
Q

-Sea of delocalised(n.)

A

Electrons that move freely between metal cations in the metallic bonding model.

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7
Q

-Crystal lattice(n.)

A

Atoms of one type of metal element that are metallically bonded and organised in a pattern.

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8
Q

What is used to explain how metal atoms bond to each other in solids

A

The metallic bonding crystal lattice model

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9
Q

How is a metals lattice of cations held together.

A

A lattice of cations is held together electrostatically by a sea of delocalised electrons.

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10
Q

Fun fact

A

Metallic bonding is non-directional as the electrostatic forces of attraction between the cations and delocalised electrons are in all directions (unlike ionic and covalent bonding)

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11
Q

-Electrostatic force of attraction(n.)

A

Attractive force between charged particles

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12
Q

-Metallic bonding(n.) again cause why not

A

The electrostatic force of attraction between delocalised electrons and cations in a metallic lattice structure.

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13
Q

Why is metallic bonding strong

A

-Metallic bonding is strong because of the electrostatic force of attraction between the delocalised electrons and the cation lattice.

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14
Q

What are the limitations of the metallic bonding model

A

The metallic bonding model does not explain=
-Different melting and boiling points of metals
-Difference in electrical conductivity of metals
-Magnetic properties of iron, nickel and cobalt

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15
Q

What are the 6 characteristics of metals

A

-Malleable(n.)
-Ductile(n.)
-good Electrical conductivity(n.)
-good Heat conductor(n.)
-High melting and boiling points
-Lustrous

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16
Q

Malleable(n.) definition

A

Ability to deform under pressure without breaking.

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17
Q

Ductile(n.) definition

A

Ability to be hammered or stretched into a thin shape without breaking.

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18
Q

Electrical conductivity(n.) definition

A

Ability to allow an electric current to flow through

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19
Q

Heat conductivity(n.) definition

A

Ability to allow heat to pass through.

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20
Q

Lustre(n.) definition

A

Shiny and glossy appearance

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21
Q

Why do metals have high melting points

A

Metals have high melting and boiling points due to the strong intermolecular forces between atoms.

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22
Q

Melting points and boiling points

A

Felix definitions=

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23
Q

Oxidation(n.)

A

A chemical reaction where a chemical species loses electrons

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24
Q

Corrosion(n.)

A

When some metals react with gases in the atmosphere(mainly oxygen)

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25
Q

Why do metals tend to lose their valence electrons more easily than non-metals

A

-Metals tend to lose their valence electrons more easily than non-metals due to their lower ionisation energies.

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26
Q

Facts to know

A

-Most metals can react with acids, to different degrees
-Metals tend to lose their valence electrons more easily than non-metals due to their lower ionisation energies.
-The loss of electrons is called oxidation.
-Bubbles forming is a qualitative sign that a gas is being produced.

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27
Q

Hydrogen pop test(n.)

A

Edrolo def=Test used to indicated the presence of hydrogen gas

Felix def=qualitative test to check the identity of the gas(hydrogen) that’s produced from a reaction.

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28
Q

General reaction for reactive metal with acid(formula)

A

Acid + reactive metal -> ionic salt + hydrogen gas

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29
Q

What are the 6 qualitative signs of a chemical reaction.

A

Remember cobalt=
Colour
Odour
Bubbles
Appearance or disappearance of a solid
Light or sound
Temperature change

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30
Q

Ionic compound(n.)

A

A compound (salt) containing one or more cations with one or more anions.

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31
Q

Salt in chemistry(def.)

A

Ionic compound.

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32
Q

Cation(n.)

A

A positively charged ion.

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33
Q

Anion(n.)

A

A negative charged ion.

34
Q

What is reactivity series(n.)

A

-Reactivity series(n.)=A ranking of substances based on chemical reactivity

35
Q

What is the reactive series of metals with dilute acids

A

A ranking of substances based on chemical reactivity

Lowest reactivity on bottom to highest reactivity on top. REACTION WITH DILUTE ACIDS=
Potassium(violent reaction)
Sodium(violent reaction
Calcium(rapid bubbling)
Magnesium(rapid bubbling)
Aluminium(rapid bubbling but slow at first)
Zinc(slow bubbling)
Iron(slow bubbling)
Tin(very slow bubbling)
Lead(very slow bubbling)
Copper(no reaction)
Silver(no reaction)
Gold (no reaction)
Platinum(no reaction)

36
Q

Metal hydroxide(n.)

A

An ionic compound containing one or more metal cations and hydroxide ions.

37
Q

Chemical formula of hydroxide ions

A

OH-

38
Q

Sodium hydroxide chemical formula

A

NaOH

39
Q

Potassium hydroxide chemical formula

A

KOH

40
Q

Magnesium hydroxide chemical formula

A

Mg(OH)2

41
Q

Calcium hydroxide chemical formula

A

Ca(OH)2

42
Q

How do group 1 and 2 metals react with water

A

-Group 1 metals=can react explosively with water.
-Group 2 metals=react less than group 1 but still react.

43
Q

How do metals going down a group react with water

A

-going down a group=lower ionisation energy= easier to remove a valence electron, hence more reactive with water.

44
Q

General reaction for reactive metal with water(formula)

A

Water + reactive metal -> metal hydroxide + hydrogen gas

45
Q

What is phenolphthalein used for and how does it work

A

-Using phenolphthalein to see if solution changes colour is another qualitative test to see if chemical reaction has taken place.

-Phenophalien is an indicator, and changes colour in different ph levels, and a change in ph levels within a mixture or substance is an indication that a chemical reaction has taken place. Phenolphthalein is colourless below pH 8.5 and attains a pink to deep red hue above pH 9.0.

46
Q

What is the reactive series of metals with water

A

A ranking of substances based on chemical reactivity

Lowest reactivity on bottom to highest reactivity on top. REACTION WITH WATER=
Potassium(violent with cold water)
Sodium(violent with cold water)
Calcium (slow with cold water, Rapid with steam)
Magnesium(slow with cold water, Rapid with steam)
Aluminium(usually no reaction)
Zinc(usually no reaction)
Iron(rust slowly)
(hydrogen)(I don’t know personally why this is here)
Copper(no reaction)
Silver(no reaction)
Gold(no reaction)

47
Q

Metal oxide

A

An ionic compound containing one ore more cations and oxide ions.

48
Q

Facts

A

-Many metals can react with oxygen
-Many more metals can react with oxygen than with water and acid

49
Q

Why is iron the only metal that rusts

A

-Only iron rusts, no other metal rusts.(its just a name only for iron corroding)

50
Q

General reaction for metal with oxygen(formula)

A

Metal and oxygen -> metal oxide

51
Q

Sodium oxide chemical formula

A

Na2O

52
Q

Magnesium oxide chemical formula

A

MgO

53
Q

Calcium oxide chemical formula

A

CaO

54
Q

Aluminium oxide chemical formula

A

Al2O3

55
Q

What is the reactive series of metals with oxygen

A

A ranking of substances based on chemical reactivity

Lowest reactivity on bottom to highest reactivity on top. REACTION WITH OXYGEN=

Potassium(react with oxygen to form oxides)
Sodium(react with oxygen to form oxides)
Calcium (react with oxygen to form oxides)
Magnesium(react with oxygen to form oxides)
Aluminium(react with oxygen to form oxides)
Zinc(react with oxygen to form oxides)
Iron(react with oxygen to form oxides)
Tin(react with oxygen to form oxides)
Lead(react with oxygen to form oxides)
Copper(react with oxygen to form oxides)
Mercury(do not react with oxygen under normal conditions)
Silver(do not react with oxygen under normal conditions)
Gold(do not react with oxygen under normal conditions)

56
Q

What is the reactive series of metals with oxygen, dilute acids and cold water

A

REACTIVE TO MOST REACTIVE, And weather they react with oxygen, dilute acids, and cold water.

Potassium(Oxygen)(dilute acids)(react with cold water)
Lithium(Oxygen)(dilute acids)(react with cold water)
Sodium(Oxygen)(dilute acids)(react with cold water)
Lithium(Oxygen)(dilute acids)(react with cold water)
Calcium(Oxygen)(dilute acids)
Magnesium(Oxygen)(dilute acids)
Aluminium(Oxygen)(dilute acids)
carbon(Oxygen)(dilute acids)
Zinc(Oxygen)(dilute acids)
Iron(Oxygen)(dilute acids)
Tin(Oxygen)(dilute acids)
Lead(Oxygen)(dilute acids)
Copper(Oxygen)
Magnesium(Oxygen)
Silver(Oxygen)
Gold(reacts with nothing)
Platinum(reacts with nothing)

57
Q

Linear economy(n.)

A

Operates on a ‘take-make-dispose’ model, making use of resources to produces products that will be discarded after use.

58
Q

Circular economy(n.)

A

A continuous cycle that focusses on the optimal use and re-use of resources from the extraction of raw materials through to production of new materials, followed by consumption and re-purposing of unused and waste materials.

59
Q

Why do we need to transition towards a circular economy from a linear economy

A

The transition from a linear towards a circular economy=
-In order to use critical elements(including metals) in the future= we need to move from linear economy to circular economy.

-Linear=Natural resource->take->make->distribute->use->dispose
-Circular=Natural resource->(take->make/remake->distribute->use/re-use/repair->sort transfer->Recycle/compost/enrich->take) x ∞

60
Q

-Green chemistry principles(n.)

A

Principles aimed at reducing the chemical-related impact on both humans and the environment through dedicated sustainability management programs.

61
Q

-Sustainable development(n.)

A

Principles aimed at reducing the chemical-related impact on both humans and the environment through dedicated sustainability management programs.

62
Q

Pollution prevention(n.)

A

It is better to prevent waste than to treat or clean up waste after it has been created.

From

63
Q

Atom Economy(n.)

A

Synthetic methods should be designed to maximize incorporation of all materials used in the process into the final product.

From

64
Q

Less hazardous chemical syntheses(n.)

A

Wherever practicable, synthetic methods should be designed to use and generate substances that possess little or no toxicity to human health and the environment.

From

65
Q

Design safer chemicals(n.)

A

Chemical products should be designed to preserve efficacy of function while reducing toxicity.

From

66
Q

Safer solvents and Auxiliaries(n.)

A

The use of auxiliary substances (e.g., solvents, separation agents, etc.) should be made unnecessary wherever possible and, innocuous when used.

From

67
Q

Design for energy efficiency(n.)

A

Energy requirements should be recognized for their environmental and economic impacts and should be minimized. Synthetic methods should be conducted at ambient temperature and pressure.

From

68
Q

Use renewable feedstocks(n.)

A

A raw material or feedstock should be renewable rather than depleting whenever technically and economically practicable.

From

69
Q

Reduce derivates(n.)

A

Unnecessary derivatization (use of blocking groups, protection/deprotection, temporary modification of physical/chemical processes) should be minimized or avoided if possible, because such steps require additional reagents and can generate waste.

From

70
Q

Catalysis(n.)

A

Catalytic reagents (as selective as possible) are superior to stoichiometric reagents.

From

71
Q

Design for degradation(n.)

A

Chemical products should be designed so that at the end of their function they break down into innocuous degradation products and do not persist in the environment.

From

72
Q

Real-time analysis for pollution prevention(n.)

A

Analytical methodologies need to be further developed to allow for real-time, in-process monitoring and control prior to the formation of hazardous substances.

From

73
Q

Inherently safer chemistry for accident prevention(n.)

A

Substances and the form of a substance used in a chemical process should be chosen to minimize the potential for chemical accidents, including releases, explosions, and fires.

From

74
Q

Why do we need to transition from a linear to a circular economy

A

In order to use critical elements(including metals) in the future= we need to move from linear economy to circular economy

75
Q

Alloy(n.)

A

Mixture of elements with base metals.

76
Q

What is mining

A

Natural resource is taken from the environment. This is a highly energy intensive activity.

77
Q

Linear economy steps

A

Natural resource->take->make->distribute->use->dispose

78
Q

Circular economy steps

A

Natural resource->(take->make/remake->distribute->use/re-use/repair->sort transfer->Recycle/compost/enrich->take) x ∞

79
Q

Sustainable(n.)

A

can be produced at a rate that is greater than consumption without compromising future generations

80
Q

Sustainable chemistry(n.)

A

Can be produced at a greater rate than it is consumed.1Consequences of the use of this chemical product are minimal for society and the environment.2

chem unit 1 (9 decks)

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