3.1.3.4 Bonding and physical properties- Bonding structure Flashcards
how the ions are held together in solid sodium metal
Attraction /electrostatic forces/bonds/attractions between (positive)
ions/lattice and delocalised/free electrons/sea of electrons.
how the ions are held together in solid sodium chloride
Electrostatic attractions/forces between ions or attractions between
(oppositely charged) ions/ Na+ & Cl
why sodium metal is malleable (can be hammered into shape)
Layers can slide over each other – idea that ions/atoms/particles move
Description of the bonding that is present in metals
(electrostatic forces of) attraction / held together by interactions between
positive ions / cations / nuclei not just metal ions
and delocalised or free (outer shell) electrons / ‘sea’ of electrons / cloud of electrons
the bonding in a metal
positive ions (attract) delocalised electrons (1) (or sea of or free or mobile)
the type of crystal shown by OF2
(simple) molecular
the type of crystal structure shown by graphane
Giant covalent / giant molecular / macromolecular
how two carbon atoms form a carbon–carbon bond in graphane
Shared pair of electrons / one electron from each C atom
why the bonding in nitrogen oxide is covalent rather than ionic
Small electronegativity difference
the type of crystal shown by OF2
(simple) molecular
the type of crystal structure shown by graphene
Macromolecular / giant covalent / giant molecular / giant atomic
the type of crystal structure shown by titanium
(Giant) metallic / metal (lattice)
why these objects with different shapes have similar strengths
(Strong) (metallic) bonding re-formed / same (metallic) bonding / retains same (crystal) structure / same bond strength / same attraction between protons and delocalised electrons as before being hammered or words to that effect
the type of bonding in the element sodium
Metallic
the type of bonding in sodium chloride
Ionic
the type of crystal structure for each of iodine and graphite
Iodine – molecular
Graphite – macromolecular/giant covalent/giant atomic
the type of bonding involved in silver
(Silver) metallic (bonding)
the type of bonding involved in silver fluoride
Ionic (bonds)
Structure of sodium chloride
NaCl is ionic
cubic lattice
electrostatic attraction between ions
Structure of ice
Covalent bonds between atoms in water
Hydrogen bonding between water molecules
Tetrahedral representation showing two covalent and two hydrogen bonds
2 hydrogen bonds per molecule
Definition: macromolecular
macromolecule = a giant/massive/huge molecule/lattice/structure with covalent bonding
how the ions are held together in solid sodium metal
Attraction /electrostatic forces/bonds/attractions between (positive) ions/lattice and delocalised/free electrons/sea of electrons.
how the ions are held together in solid sodium chloride
Electrostatic attractions/forces between ions or attractions between (oppositely charged) ions/ Na+ & Cl–
Differences in properties of diamond and graphite
-Structure and hardness
both macromolecular/giant atomic/giant covalent/giant molecular
C atoms in diamond joined to 4 other C atoms / diagram with min 5 C atoms i.e. shows tetrahedral shape / coordination number = 4
C atoms in graphite joined to 3 other C atoms diagram with clear extended hexagonal plane/pattern i.e. shows trigonal planar shape / coordination number = 3
diamond hard / crystal strong
because of 3-D structure / rigid structure / not layered
graphite (soft) as layer can slide over each othe
as only (weak) van der Waals’ forces between layers
- Melting point (for either allotrope)
covalent bonds must be broken / overcome
which are strong / many / hard to break
- Other difference
diamond is non-conductor of electricity, graphite is conductor OR appropriate difference in appearance
