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Chem > Metals > Flashcards

Metals Flashcards

1
Q

define metallic bonds

A

strong electrostatic forces of attraction between metal cations and sea of delocalised valence electrons

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2
Q

list all 8 properties of metals

A
  1. shiny appearance
  2. solid state @ rtp
  3. high density
  4. strong + tough
  5. ductile (stretch) + malleable (bend)
  6. high mp & bp
  7. good conductor of electricity
  8. good conductor of heat
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3
Q

why do metals have high mp & bp

A

due to strong electrostatic forces of attraction (between metal cations and sea of delocalised electrons)

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4
Q

why are metals good heat & electricity conductors

A

due to presence of mobile electrons even when solid

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5
Q

what are some metal exceptions to 1. solid state at rtp & 2. high mp + bp

A
  1. mercury
  2. mercury + alkali metals
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6
Q

define alloy

A

a mixture of a metal w/ one or a few other elements

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7
Q

why are alloys used instead of pure metals (3)

A
  1. in pure metals, layers of atoms with same sizes can slide over each other easily
  2. in alloys, layers of atoms cannot slide over each other easily bc layers of atoms of alloying elements with different sizes disrupt the orderly arrangement of the metal atoms
  3. pure metals too malleable & hv less resistance to corrosion
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8
Q

list reactivity series

A

please - potassium
send - sodium
cats - calcium”
monkeys - magnesium
and - aluminium^
cute - carbon
zebras - zinc
into - iron
large - lead^
heavy - hydrogen”
cages - copper
securely - silver
guarded - gold

“ - non-metal
^ - special metal that reacts diff

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9
Q

what does potassium sodium and calcium have in common (reaction)

A
  1. explode in steam; not safe to carry out
  2. react explosively with acids
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10
Q

what does potassium sodium calcium magnesium and aluminium have in common (reaction)

A

reacts with cold water to form metal hydroxide + hydrogen
* aluminium + magnesium reacts slowly

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11
Q

what does magnesium aluminium zinc and iron have in common (reaction)

A
  1. reacts w/ steam to form metal oxide + hydrogen
  2. reacts w/ acids to form salt + hydrogen
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12
Q

how is lead diff from copper silver and gold (reaction)

A

reacts w/ acids
rest do not

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13
Q

what does lead copper silver and gold have in common (reaction)

A

no observable reaction 4 cold water/steam

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14
Q

how is potassium sodium calcium magnesium and aluminium extracted

A

extracted by electrolysis

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15
Q

how is zinc iron lead copper and silver extracted

A

extracted by reduction w/ carbon or hydrogen
* zinc cannot reduce from zinc oxide with hydrogen

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16
Q

how is gold extracted

A

found naturally; else only need simple heating

17
Q

list reaction speeds of potassium sodium calcium magnesium and aluminium w/ cold water

A
  1. potassium - very violently
  2. sodium - violently
  3. calcium - readily
  4. magnesium - very slowly
  5. aluminium - very slowly
18
Q

list reaction speeds of magnesium aluminium zinc iron (and lead) w/ steam

A
  1. magnesium - violently
  2. aluminium - readily
  3. zinc - readily
  4. iron - slowly
  5. (lead - nil)
19
Q

list reaction speeds of potassium sodium calcium magnesium aluminium zinc iron and lead w/ acid

A
  1. potassium - explosive rxn
  2. sodium - explosive rxn
  3. calcium - vigorously
  4. magnesium - rapidly
  5. aluminium - rapidly
  6. zinc - moderately fast
  7. iron - slowly
  8. lead - slowly
20
Q

why alkali metals (grp 1 metals) so explosive in cold water

A

heat produced during rxn causes h2 gas to catch fire and explode

21
Q

why does lead stop reacting with acid after a while

A

insol. layer of lead (ii) chloride formed arnd lead metal

22
Q

why does aluminium react slower/does not react at all at the start with water/acid

A

has a layer of non-porous aluminium oxide on surface, prevent water/acid from coming into direct contact with aluminium

23
Q

why is carbon used more frequently by manufactorers instead of hydrogen

A

cheaper, more effective as reducing agent

24
Q

why does h2 need to keep passing through the set-up for reduction of metal oxide by h2 until the tube is cool

A

to prevent re-oxidation of the metals when reacting w/ o2 in the air

25
Q

describe displacement reactions in 2 sentences

A
  1. more reactive metal can displace less reactive metal from oxide/solution
  2. more reactive metal oxidised to form ions, less reactive metal reduced to form atoms
26
Q

describe thermal stability of metal carbonates in 2 sentences

A
  1. more reactive metal forms more stable carbonate
  2. thus need absorb more heat energy to decompose by heating
27
Q

describe thermal stability of potassium and sodium [carbonate]

A
  1. stable to heat w/ bunsen burner
  2. no decomposition
  3. only decompose when temp very high
28
Q

describe thermal stability of calcium magnesium zinc iron lead and copper [carbonate]

A
  1. decomposes to metal oxide + carbon dioxide w/ increasing ease down reactivity series
  2. CuCO3 (s) -> CuO (s) + CO2 (g)
29
Q

describe thermal stability of silver [carbonate]

A
  1. decompose to silver, oxygen and carbon dioxide
  2. Ag2O thermally unstable; further decompose to form Ag
  3. Ag2CO3 (s) -> Ag2O (s) + CO2 (g)
  4. 2 Ag2O (s) -> 4 Ag (s) + O2 (g)

Chem (10 decks)

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