Metallic and ionic bonding Flashcards

1
Q

a metal atom loses electrons to become a positively charged

A

cation

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2
Q

a non metal gains electrons to become a negatively charged

A

anion

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3
Q

what happens when lots of cation and anions form in this way

A

when large amounts of cations and anions are formed in this way, they arrange themselves into a three dimensional lattice

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4
Q

cross over method

A

| /\

|

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5
Q

the _____ ion is placed before the ______ eg MgO

what is the one exception

A

cation before the anion

sodium ethanoate CH3COONa

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6
Q

the total charged of the cation and anion should be

A

0 balanced

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7
Q

subscripts

A

subscripts are used when there are more one ions in a compound

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8
Q

what are polyatomic ions

A

polyatomic ions are ions that contain more than atom and have an overall charge.
some examples are
Nitrate NO3 -
carbonate CO3 2-

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9
Q

what does the anion end in

A

ide

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10
Q

for polyatomic anions containing oxygen

A

they end in -ite or -ate

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11
Q

properties of metals

A
conductors of electricity and heat
malleable
ductile
high boiling temperatures
high densities
lustrous 
low ionisations energies and electroneagtivities
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12
Q

important exceptions of metal properties

A

mercury is liquid at room temperature

chromium is brittle
group 1 metals are soft

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13
Q

Transition metals

A

found in the D block
are in the human body in low concentrations
compared to main group metals:
they are harder, have higher densities, higher melting points, some have magnetic properties

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14
Q

the metallic bonding model

A

the metallic bonding model is a 3D lattic of cations that are surrounded by a sea of delocalised electrons. the lattice is held together by a sea of electrostatic attractions

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15
Q

limitations of the metallic bonding model

A

cannot explain range of melting temperatures
density variations
different electrical conductivity

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16
Q

metal reactivity with water

A

metals react violently with water. group 1 metals are more reactive than main group metals. exothermic reaction

metal + water = metal hydroxide + Hydrogen gas

17
Q

metal reactivity with acids

A

metal + acid = salt + hydrogen gas

Cu (s) + 2HCl (aq) = CuCl2 (aq) + H2(g)

18
Q

metal reactivity with oxygen

A

metal + oxygen = metal oxide

19
Q

reactivity series of metals

A

chemists have experimentally made a list of metals that indicate the reactivity of metals

20
Q

ore

A

an ore is a natural compound that contains a metal

iron ore is a mineral

21
Q

extraction of iron from its ore

A

coke reacts iron = carbon monoxide reacts with iron ore = Iron and slag molten are at the bottom
Fe2O3 = 3CO = 2Fe + 3CO2

22
Q

environmental, economic issues and social issues with metallic extraction

A

environmental: pollution, disposal of slag
economic: benefits countries
social issues: land use issues with mining, tourism tourism and farms

23
Q

metal modification

A

some metals are used in their pure form - aluminium and copper. other are modified

24
Q

how metals are be modified

A

alloying
heat treatment and work hardening
coating

25
alloying
involes melting and mixing metals together and then cooling them into a solid. alloys are harder, less malleable and poorer electrical conductors
26
substitutional alloys
made from elements similar in size and chemical properties
27
interstitial alloys
made from different sized atoms
28
crystals
regions in a solid in which particles are arranged in a regular way. the malleability and brittleness is dependent on the size of the crystals and their arrangement
29
smaller crystals vs larger crystals
smaller crystals are harder, less movement of layers of ions more malleable. larger crystals more breaks, brittle more gaps