3.1.3.4 Bonding and physical properties- Bonding structure

Question 1

how the ions are held together in solid sodium metal

Answer 1

Attraction /electrostatic forces/bonds/attractions between (positive)
ions/lattice and delocalised/free electrons/sea of electrons.

Question 2

how the ions are held together in solid sodium chloride

Answer 2

Electrostatic attractions/forces between ions or attractions between
(oppositely charged) ions/ Na+ & Cl

Question 3

why sodium metal is malleable (can be hammered into shape)

Answer 3

Layers can slide over each other – idea that ions/atoms/particles move

Question 4

Description of the bonding that is present in metals

Answer 4

(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

Question 5

the bonding in a metal

Answer 5

positive ions 
(attract) delocalised electrons (1) (or sea of or free or mobile)

Question 6

the type of crystal shown by OF2

Answer 6

(simple) molecular

Question 7

the type of crystal structure shown by graphane

Answer 7

Giant covalent / giant molecular / macromolecular

Question 8

how two carbon atoms form a carbon–carbon bond in graphane

Answer 8

Shared pair of electrons / one electron from each C atom

Question 9

why the bonding in nitrogen oxide is covalent rather than ionic

Answer 9

Small electronegativity difference

Question 10

the type of crystal shown by OF2

Answer 10

(simple) molecular

Question 11

the type of crystal structure shown by graphene

Answer 11

Macromolecular / giant covalent / giant molecular / giant atomic

Question 12

the type of crystal structure shown by titanium

Answer 12

(Giant) metallic / metal (lattice)

Question 13

why these objects with different shapes have similar strengths

Answer 13

(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

Question 14

the type of bonding in the element sodium

Answer 14

Metallic

Question 15

the type of bonding in sodium chloride

Answer 15

Ionic

Question 16

the type of crystal structure for each of iodine and graphite

Answer 16

Iodine – molecular

Graphite – macromolecular/giant covalent/giant atomic

Question 17

the type of bonding involved in silver

Answer 17

(Silver) metallic (bonding)

Question 18

the type of bonding involved in silver fluoride

Answer 18

Ionic (bonds)

Question 19

Structure of sodium chloride

Answer 19

NaCl is ionic
cubic lattice
electrostatic attraction between ions

Question 20

Structure of ice

Answer 20

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

Question 21

Definition: macromolecular

Answer 21

macromolecule = a giant/massive/huge molecule/lattice/structure with covalent bonding

Question 22

how the ions are held together in solid sodium metal

Answer 22

Attraction /electrostatic forces/bonds/attractions between (positive) ions/lattice and delocalised/free electrons/sea of electrons.

Question 23

how the ions are held together in solid sodium chloride

Answer 23

Electrostatic attractions/forces between ions or attractions between (oppositely charged) ions/ Na+ & Cl–

Question 24

Differences in properties of diamond and graphite

Answer 24

-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

Question 25

the bonding in a metal

Answer 25

positive ions
(attract) delocalised electrons
(or sea of or free or mobile)

Question 26

the bonding in a crystal of iodine

Answer 26

covalent between atoms

Van der Waals’ between molecules

Question 27

the crystal type which describes an iodine crystal

Answer 27

molecular

Question 28

Similarity in the bonding of diamond and iodine (solid)

Answer 28

Both covalent

Question 29

Difference in structures of diamond and iodine (solid)

Answer 29

Iodine = molecular /I2
Diamond = giant molecular/macromolecular/giant covalent / giant atomic

Question 30

reason why ice is less dense than water

Answer 30

Water or H2O or molecules (in ice) are held further apart (than in liquid water)/(more) space/gaps/holes in structure/Water or H2O or molecules (in ice) are more spread out