Chapter 2: Strong Bonding Flashcards

1
Q

Metallic Bonding

A
  • Electrostatic attraction between positive ions and a sea of delocalised valence electrons that holds the positive ions together.
  • Strength of bonds depend on
  • > charge of +ive ions
  • > more valence e- = stronger bonds
  • > size of ions
  • > way in which ions arranged
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Physical properties of metals

A
  • high electrical conductivity -> delocalised, mobile charge carriers
  • heat conductivity -> delocalised, mobile e- transfer kinetic energy
  • malleable and ductile -> layers of +ive ions move when metal bent stretched, delocalised e- move into regions b/w and keep structure
  • lustre -> interaction b/w photons of light and mobie e- sea

high mp -> +ive ions w/ larger charge have stronger bonds

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

Alloys

A

Same basic structure w/ impurities incorporated into lattice

  • the impurity disrupts orderly nature, more difficult for layers to slide therefore harder and stronger
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Ionic Bonding

A

Electrostatic attraction b/w positive and negative ions

  • Transfer of electrons / lose electrons and gaining electrons
  • arranged in orderly lattice
  • > metal loses e’ due to low ionisation energy
  • > non-metal gain e’ due to high electronegativity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Physical properties of ionic bonds

A
  • Non conductors in solid state -> ions held in rigid lattice are not mobile
  • Conductors in molten/ soln -> ions break away from rigid lattice and become mobile. Act as charge carriers free to move.
  • Hard and brittle -> Bonding holding ions in lattive strong therefore hard. When put under pressure, layers of ions pushed causing like charges in close proximity therefore fall apart

High mp and bp -> Much energy required to overcome forces

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

Covalent Molecular Bonding

A

Electrostatic attraction b/w adjacent nuclei and shared valence electrons

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

physical properties of covalent molecular bonding

A

low MP and BP -> covalent bonds b/w atoms are strong BUT bonds b/w molecules are weak

  • Solids are soft -> bonds b/w molecules are weak therefore little force required

Do not conduct -> neutral molecules, e- and protons are localised

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

Covalent Network Substances

A
  • atoms bonded together by shared e- pairs

- Bond together in vast lattice arrays not just discrete molecules

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

Physical Properties

A

High mp/BP -> each atom held in lattice by very strong covalent bonds, much energy required

  • Extremely hard and brittle -> atom held in lattice by strong covalent bonds. One area disrupted strains rest of lattice and falls apart
  • Non conductors -> e- are localised in pairs around each atom
How well did you know this?
1
Not at all
2
3
4
5
Perfectly