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Chem > Intra Bonding > Flashcards

Intra Bonding Flashcards

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1
Q

define metallic bonding

A

electrostatic forces of attraction between cations and the sea of delocalised electrons that hold the cations in a metallic lattice structure

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2
Q

what does it mean for metallic bonds to be non-directional?

A

electrons in the metallic lattice are delocalised and do not belong to any particular cation

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3
Q

describe why a metallic lattice forms

A
  • metal elements have low ionisation energies compared to non-metal elements
  • metal atoms lose their valence electrons, such that they are free to move among the cations formed during ionisation
  • metallic bonding, hence held in a metallic lattice
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4
Q

what does the strength of metallic bonding depend on?

A
  • charge of positive ions
  • size of positive ions
  • way cations organised in the metallic lattice
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5
Q

state the physical properties of metallic substances

A

high melting and boiling points
strong
good thermal conductor
electrical conductor
malleable and ductile
lustrous

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6
Q

why do metallic substances have high MP/BP/Strong?

A
  • In a metallic substance, there are strong metallic bonds within a metallic lattice
  • large amount of energy/force needed to overcome/disrupt these metallic bonds
  • high melting point/strong
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7
Q

define malleable and ductile

A

malleable: able to be bent into sheets
ductile: able to be drawn into wires

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8
Q

why are metallic substances malleable and ductile?

A

when sufficient force is applied to the metallic substance,
- layers of positive ions move relative to one another
- there will still be metallic bonds (define) between sea of delocalised electrons and positive ions
- this is because metallic bonds are non-directional (define)
- metallic substance’s shape can be deformed while still maximising the metallic bond

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9
Q

Why are metallic substances electrical conductors?

A
  • to conduct electricity, there must be mobile, charged particles present
  • metallic substance, sea of delocalised electrons are mobile, charged particles, hence can conduct electricity
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10
Q

Why are metallic substances good thermal conductors?

A
  • thermal conduction is a result of KE being transferred when 1 particle collides with its neighbouring particle
  • sea of delocalised electrons are free to move through the lattice, can transfer kinetic energy rapidly though the lattice
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11
Q

define an alloy and state its metallic structure

A
  • mixture of a metal and another metal or a non-metal
  • same as metallic substance, but impurity atoms are incorporated into the lattice
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12
Q

how does an impurity atom increase hardness and strength of the alloy?

A
  • impurity atoms disrupt the orderly nature of the metallic lattice
  • make it more difficult for the layers of positive ions to slide over one another if the metal is bent
  • increase hardness and strength
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13
Q

define ionic bond

A

electrostatic forces of attraction between positively charged ions and negatively charged ions in an ionic crystal lattice structure

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14
Q

why is the ionic lattice held together so closely?

A

electrostatic forces of attraction between oppositely charged ions are greater than electrostatic forces of repulsion between like charged ions in the ionic crystal lattice, held together strongly

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15
Q

describe a NaCl lattice

A
  • made up of a continuous lattice of alternating Na+ and Cl-
  • each Na+ surrounded by 6 Cl-
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16
Q

why do ionic substances have high MP/BP/Strong?

A
  • In an ionic substance, there are strong ionic bonds within a ionic crystal lattice
  • large amount of energy/force needed to overcome/disrupt these ionic bonds
  • high melting point/strong
17
Q

why are ionic substances brittle?

A

if sufficient force is applied,
- forces ions with like charges to lie adjacent to each other
- electrostatic forces of repulsion between like-charged particles cause it to fracture
- brittle due to the directional force between positively charged and negatively charged ions in ionic crystal lattice

18
Q

why can’t ionic substances conduct electricity in solid?

A
  • to conduct electricity there must be mobile charged particles
  • positive and negatively charged ions are not free moving as they are held in the rigid 3D lattice
  • cannot conduct electricity
19
Q

why can ionic substances conduct electricity in molten/aqueous?

A
  • ionic substances dissociate into their ions and break away from rigid lattice
  • charged, mobile particles now present to conduct electricity
20
Q

why do metals form cations and non-metals form anions?

A
  • metals tend to lose electrons because of their high IE
  • non-metals tend to gain electrons because of their high EN
21
Q

define covalent bonds

A

forces of attraction formed when 1 or more of the pairs of electrons are shared between 2 atoms to achieve stable electron configuration

22
Q

why do covalent molecular have low BP MP/soft

A

weak intermolecular forces of attraction between discrete molecules, small amount of energy needed to to overcome/disrupt weak bonds

23
Q

covalent molecular electricity

A

pure form - non-conductors of electricity because no mobile charged particles
some ionise in solution - acids, bases, HF, CH3COOH, NH3

24
Q

covalent network high BP/strong

A
  • In an covalent network substance, there are strong covalent bonds within a covalent network lattice
  • large amount of energy/force needed to overcome/disrupt these covalent bonds
  • high melting point/strong
25
Q

describe diamond structure

A

each C covalently bonded to 4 other C in a tetrahedral arrangement, covalent network lattice

26
Q

diamond cannot conduct electricity

A

each C covalently bonded to 4 other C in a tetrahedral arrangement, covalent network lattice valence electrons all valence electrons are localised to the covalent bonds, no mobile charged particles

27
Q

diamond hard and brittle

A

high melting point, if diamond was subjected to extreme stress and one part of the lattice is disrupted, place stress on the rest of the lattice causing it to fracture - brittle

28
Q

describe graphite structure

A

covalent layer lattice, each C covalently bonded to 3 other C in hexagonal graphene sheets
weak intermolecular forces between graphene layers
1 delocalised electron per carbon atom

29
Q

graphite conductor of electricity

A

each C provides 1 delocalised valence electrons (charged mobile particle)

30
Q

graphite lubricant

A

slippery, layers slide easily, dry lubricant

31
Q

amorphous carbon

A

irregular structure of carbon atoms, many varieties exist with many different non-continuous packing arrangements

32
Q

silica structure

A

covalent network substance, each silicon atom bonded to 4 oxygen atoms in a tetrahedral arrangement

33
Q

fullerene structure

A

atoms are arranged in a series of pentagons and hexagons, each C covalently bonded to 3 C

Chem (6 decks)

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