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metals Flashcards

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1
Q

metallic structure

A

a lattice of positive metal ions
a sea of delocalised electrons

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2
Q

metallic bonding

A

-the electrostatic attraction between the positive metal ions and the negative delocalised electrons
very strong attraction

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3
Q

metallic properties

A

-high boiling points- because metallic bonding is very strong so requires lots of energy to break

-conduct electricity- delocalised electrons are free to move through the lattice

-metals are malleable- layers of metal ions can slide over eachother

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4
Q

metal carbonate reaction

A

the thermally decompose to form metal oxide + carbon dioxide

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5
Q

thermal decompostition of copper carbonate

A

-coper carbonate (green solid)> copper oxide (black solid) + carbon dioxide (colourless gas)

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6
Q

downward delivary

A

carbon dioxide is denser than air so it sinks to the bottom of a tube until collected

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7
Q

metal + water reaction

A

metal + water> metal hydroxide + hydrogen

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8
Q

observation of metal + water reaction

A

effervescence- hydrogen gas produced

solid disapears- used up in reaction

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9
Q

describe metal reactions with reactivity trends

A

metals that are less reactive that magnesium are so slow you cannot tell anything is happening

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10
Q

group one metal + water reactions

A

.they react violently to form metal hydroxide + hydrogen

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11
Q

observations of group one metal

A

.solid floats at start as it is less dense than water

-effervescence- hydrogen gas is produced

solid moves- effervescence propels solid around surface of water during reaction

solid disappears, used up in reaction

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12
Q

what happens when universal indicator is used afger reaction

A

turns dark blue,
alkali is present (metal hydroxide)

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13
Q

lithium reaction with water

A

fast reaction
vigirous

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14
Q

sodium reaction with water

A

.faster than lithium
.sodium melts

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15
Q

potassium reaction with water

A

fastest reaction
K melts
liliac flame produced

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16
Q

metal + steam reaction

A

forms metal oxide + hydrogen

17
Q

how to carry out a metal + steam reaction

A

1.)metal magnesium is placed into a metal tube with wet wool
2.) wet wool is heated producing steam
3.) steam reacts with magnesium to form magnesium oxide in tube

4.) hydrogen is burnt to safely destroy it

18
Q

metal + acid

A

salt + hydrogen
eg magnesium+ sulphuric acid > magnesium sulphate + hydrogen

19
Q

observations in acid + metal reaction

A

metal disappears- used up in reaction
fizzing- hydrogen in produced

20
Q

why can we not use metals that are less reactive than hydrogen e.g. gold or copper

A

less reactive, so cannot displace Hydrogen from the acid

21
Q

why can we not us Li Na and K

A

reaction with acids is too violent

22
Q

explain the trend in reactivity series and acid reaction

A

more reactive a metal is, faster it will react with an acid

23
Q

chemical test for hydrogen

A

lit splint > squeaky pop
combustion of hydrogen cause test tube to resonate

24
Q

which salts are always dissolvable in water

A

sodium- Na+
potassium- K+
Ammonium- NH4+
Nitrate- NO3-

25
Q

ores

A

metals are found in the earths crust as compounds with oxygen and sulfur as over time these metals have reacted

26
Q

natives

A

gold and silver are too unreactive to have combined with oxygen and sulphur

they are found chemically unchanged

27
Q

metal extractions to chemically extract metals from compounds

A

using electricity- metals more reactive than carbon cannot be displaced by carbon.
electricity is used instead eg aluminium

28
Q

carbon extraction

A

metals less reactive that carbon can be displaced by carbon
eg copper can be displaced from its ore using carbon

29
Q

rusting

A

chemical process in which iron is oxidised to form rust

30
Q

chemical name for rust

A

hydrated iron(III) oxide

31
Q

how does rusting work

A

1.) iron is oxidised (gains oxygen) to form iron(III) oxide. iron has also lost electrons

2.) iron(III) oxide is hydrated by water
amount of water varies

32
Q

rusting can be prevented by

A

using barriers
sacrificial protection

33
Q

how does barriers work

A

.coating iron in paint, oil grease or plastic prevents iron coming into contact with oxygen and water

oil - for moving parts (bike chain)
paint- more stationary objects

34
Q

sacrificial protection

A

attach a block of a more reactive metal to the iron
this sisplaces iron from rust
eg magnesium+ Iron(III) oxide > magnesium oxide + Iron

35
Q

galvanising

A

coating iron in zinc
.coating prevents O2 and H20 from coming into contact with iron
and zinc is more reactive so acts as a sacrificial protection too

36
Q
A

chemistry- (7 decks)

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