Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

chemistry all note flashcards - 3rd And 4th > 3.5 - Metals > Flashcards

3.5 - Metals Flashcards

(108 cards)

Start Studying
1
Q

what are the two components in the structure of a metal

A
  • lattice of positive metal ions
  • sea of delocalized electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what charges do metal ions in the metal structure have

A

their usual charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what were the delocalized electrons lost by and how do they move

A

lost by the metal ions and they move freely through the lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is metallic bonding

A

the electrostatic attraction between the positive metal ions and the negative delocalized electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what type of attraction is metallic bonding

A

usually very strong

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what are the properties of metals

A

have high melting points
conduct electricity
malleable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

why do metals tend to have high melting points

A

because the metallic bonding is very strong so lots of energy is needed to break it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

why do metals conduct electricity

A

the delocalized electrons are free to move through the lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

why are metals malleable

A

the layers of metal ions can slide over each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what is thermal decomposition

A

a thermal decomposition reaction is when heat energy is used to break down a substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what is the equation for a thermal decomposition

A

metal carbonate –> metal oxide + carbon doxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what would the thermal decomposition of copper carbonate look like

A

copper carbonate –> copper oxide + carbon dioxide
CuCO3(s) CuO(s) CO2(g)
green solid black solid colourless gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what is carbon dioxide often collected by in thermal decomposition

A

downward delivery

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

why is carbon dioxide collected by downward delivery

A

because carbon dioxide is denser than air

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what is downward delivery

A

the carbon dioxide sinks to the bottom of a tube and stays there until you want to use it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

list the metal reactivity series from lowest to highest

A

Au Ag Cu (H) Pb Fe Zn (C) Al Mg Ca Li Na K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

why are hydrogen and carbon included in the reactivity series despite being non-metals

A

their positions are important when considering displacement reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what do metals react with cold water to form

A

metal hydroxides and hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is the metal and water reaction equation

A

metal + water –> metal hydroxide + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what are the two significant observations of metal and water reactions

A

effervescence - due to the hydrogen gas produced
solid disappears - due to being used up in the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what are the metals in group 1 of the periodic table called

A

alkali metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

how do the metals in group 1 of the periodic table react with water

A

violently to form metal hydroxides and hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

group 1 metal and water reaction equation

A

metal + water –> metal hydroxide + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

what similar observations do the reactions of Li, Na and K with water share

A
  • solid floats - it is less dense than water
  • effervescence - hydrogen gas is produced
  • solid moves - the effervescence propels it around the surface of the water
  • solid disappears - it is used up in the reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
what happens when universal indicator is added to the water after its reaction with Li, Na or K
it turns dark blue - the metal hydroxides are alkalis because they donate OH-
26
what happens to the reaction of group 1 metals and water` as the reactivity increases
it gets more vigorous
27
what is the increasing reactivity order of Lithium, Sodium and Potassium
lithium (Li) , sodium (Na), potassium (K)
28
what are the extra observations of lithium reacting with water
fast
29
what are extra observations of sodium reacting with water
faster (than lithium) Na melts
30
what are the extra observations of potassium reacting with water
fastest (out of it, sodium and lithium) K melts lilac flame
31
what happens to the group 1 metals as you go down the group
they get more reactive
32
what happens when a group 1 metal atom reacts
it loses its outer-shell electrons to get a full outer shell
33
why does losing outer shell electrons and getting a full shell happen more easily down the group of group 1 metals
- atoms get bigger and have more shells - the outer-shell electron is further from the nucleus - the attraction between the nucleus and the outer-electron is weaker - so less energy is needed to break the attraction
34
what do metals react with steam to produce
metal oxide and hydrogen
35
metal reaction with steam equation
metal + steam --> metal oxide + hydrogen
36
what is a metal and steam reaction usually conducted in
a horizontal tube
37
in a metal and steam reaction what set up inside the horizontal tube
wet wool is heated to generate steam for the Mg to react with the H2 gas product is ignited to safely destroy it
38
why do metals react with cold water and hot steam to produce different products
steam has more energy, so both bonds in the water molecule can break
39
what do acids react with metals to form
a salt and hydrogen gas
40
acid and metal reaction equation
acid + metal --> salt + hydrogen
41
what happens in an acid and metal reaction
a salt compound is formed when H is displaced from the acid
42
what salt does hydrochloric acid form
metal chloride (contains Cl-)
43
what salt does sulphuric acid form
metal sulphate (contains SO4 2-)
44
what salt does nitric acid form
metal nitrate (contains NO 3-)
45
what salt does phosphoric acid form
metal phosphate (contains PO4 3-)
46
is sodium (Na +) soluble
yes
47
is potassium (K +) soluble
yes
48
is ammonium (NH4 +) soluble
yes
49
is nitrate (NO3 -) soluble
yes
50
is chloride (Cl -)
yes - except with Ag + and Pb 2+
51
is sulphate (So4 2-) soluble
yes - except with Ca 2+, Ba 2+ and Pb 2+
52
is carbonate (CO3 2-) soluble
no - except with Na +, K+ and NH4 +
53
is hydroxide (OH -) soluble
no - except with Na +, K+ and Ca 2+
54
is oxide (O 2-) soluble
no - except with Na +, K+ and NH4 +)
55
what are the two important observations in an acid and metal reaction
the metal disappears there is fizzing
56
why does the metal disappear in a metal and acid reaction
because it is used up in the reaction
57
why is there fizzing in a metal and acid reaction
because a gas (hydrogen) is produced
58
what happens to the reaction of a metal and an acid as the reactivity of a metal increases
the faster it reacts
59
which metals cannot react with acids and why
Au, Ag and Cu it is not possible because they are less reactive than H so cannot displace it
60
which metals are not allowed to react with acids and why
Li, Na and K reaction with acids is too violent
61
what is the chemical test for hydrogen
hydrogen in a test tube lit splint -> squeaky pop because the combustion of the hydrogen causes the test tube to resonate
62
what happens in displacement reactions
more reactive metals can displace less reactive metals from their compounds
63
what would the equation for the displacement of magnesium from copper from copper suphate
magnesium + copper sulphate --> copper + magnesium sulphate Mg(s) + CuSO4(aq) --> Cu(s) + MgSO4(aq) grey solid blue solution pink-orange colourless solid solution
64
what are the two observations to always think about in metal displacement reactions
solid colour change solution colour change
65
what happens to the non-metal part of the compound in a displacement reaction
remains unchanged
66
when can a displacement reaction occur
if the metal used is more reactive than the metal already in the compound
67
where are most metals found and what as
in the Earth's crust as compounds with oxygen and sulphur this is because over a long time those metals have reacted with oxygen and sulphur
68
what are ores
rocks containing specific metal compounds
69
what does native mean
chemically uncombined
70
which elements are too unreactive to combine with oxygen or sulphur
gold - Au silver Ag
71
why don't native metals need to be chemically extracted
they already exist on their own
72
what do metal ores need to be chemically extracted from
their compounds
73
what ways can metal ores be chemically extracted
1- using electricity 2- carbon extraction
74
what is using electricity for extraction of ores
metals more reactive than carbon cannot be displaced by carbon instead we have to use electricity to break down their ore compounds
75
what is using carbon extraction for ores
metals less reactive than carbon can be displaced by carbon
76
what type of reaction is using carbon to displace a metal from its compound
a redox reaction
77
what is reduction
loss of oxygen
78
what is a reducing agent
takes oxygen away from something else
79
what is oxidation
gain of oxygen
80
what is oxidising agent
gives oxygen to something else
81
what is redox
reduction and oxidation in the same reaction
82
what is rusting
a chemical process by which iron is oxidised to form rust
83
what is the chemical name for rust
hydrated iron(III) oxide
84
what is the word equation for rust
iron --> iron(III) oxide --> hydrated iron(III) oxide
85
what is the chemical equation for rust
Fe(s) ---> Fe2O3(s) ---> Fe2O3.xH2O(s)
86
what are the properties of iron
grey shiny malleable
87
what are the properties of rust - hydrated iron(III) oxide
brown dull brittle
88
what two substances does rusting require
oxygen and water
89
how does rusting happen
1- iron is oxidized by oxygen to form iron(III) oxide Fe has gained oxygen and it has also lost electrons to form Fe 3+ ions - it has been oxidized 2- iron(III) oxide is hydrated by water
90
what methods can prevent rusting
using barriers sacrificial protection galvanising
91
what is using barriers
coating the iron in paint, oil, grease or plastic prevents iron from coming into contact with oxygen or water this only works as long as the coating is intact - as soon as it breaks rusting happens
92
what barrier would you use for a bike chain or for buckets
oil or grease for moving parts such as bike chains paint or plastic for larger stationary objects such as buckets
93
what is sacrificial protection
attach a block of a more reactive metal to the iron this works by displacing the iron from rust as soon as the rust forms
94
what is the downside to the sacrificial protection
the block such as block of magnesium has to be replaced often
95
what is galvanising
specifically involves coating the iron in zinc
96
why does galvanising work both ways
coating it prevents O2 and H2O from coming into contact with the iron but even if a crack appears zinc is more reactive than iron so acts as sacrificial protection as well
97
what are alloys
mixtures of a metal with one or more other elements, usually other metals or carbon
98
list common alloys
steel brass bronze
99
elements in steel
iron + carbon
100
elements in brass
copper + zinc
101
elements in bronze
copper + tin
102
why are alloys harder than pure metals
because the different-sized atoms/ions prevent the layers of metal ions from sliding over each other which means the alloy is less malleable
103
what is the use of iron and why
making steel because it is more useful than iron
104
what is the use of low-carbon steel and why
ships, cars, bridges etc because it is strong but carbon can also be hammered into many shapes
105
what is the use of high-carbon steel and why
tools - knives and screwdrivers because high-carbon so less malleable and stiffer than low-carbon steel
106
what is the use of stainless steel and why
cutlery, cooking utensils, kitchen sinks because Cr forms oxide layer that resists corrosion so stays shiny and clean
107
what is the use of copper and why
wires, cooking pans, water pipes because excellent conductor of electricity, excellent conductor of heat, unreactive and malleable
108
what is the use of aluminiun and why
aircraft bodies, power cables low-density and high strength, low-density and conducts

chemistry all note flashcards - 3rd And 4th (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions