1.3 Bonding Flashcards
Explain, in terms of its structure and bonding, why metals have high melting point.
strong electrostatic force of attraction between positive metal ions and a sea of delocalised electrons
Draw a labelled diagram to show the arrangement of particles in a crystal of nickel. In your answer, include at least six particles of each type.
just six cirlces with a plus
- you made mistake of putting electrons around, just put the positives
Explain why nickel is ductile can be stretched into wires
Layers of ions can slide over each other
Identify one substance that could react with both SO2 & HCl
NaOH / NH3 / CaCO3 / CaCO
Explain why calcium has a higher melting point than strontium.
M1 positive ions are smaller, smaller radius
M2 Ca^2+ has stronger attraction between the positive ions and the delocalised electrons
In terms of structure and bonding explain why Calcium has a higher melting point than methane
Calcium has a metallic lattice and strong metallic bonding
Methane has a simple molecular structure and weak van de waals forces between molecules.
Metallic bonding in Ca is stronger than the van de waals between CH4
More energy is required to overcome the metallic bonds in Ca
In terms of structure and bonding explain why Sodium Oxide has a higher melting point than phosphorus pentoxide
Na2O has an ionic lattice with ionic bonding
P4O10 is simple molecular with van de waals forces between molecules
Ionic bonding in Na2O is stronger than the van de waals forces in P4O10
More energy is required to overcome the ionic bonds in Na2O
for a bonding question, for a macromolecular and simple molecule, which should you say has strong covalent bond and the other has weak van de waals between molecules
macromolecular has strong covalent bonds
Explain why aluminium has a higher melting point than sodium.
Aluminium has more protons and a higher charge
Attracts delocalised electrons more strongly
Forming stronger metallic bonds
Deduce the type of crystal structure that graphane has
b) State how two carbon atoms form a carbon–carbon bond in graphane
c) Deduce the empirical formula of graphane.
macromolecular
b) Shared pair of electrons as it is a covalent bond
c) Deduce the empirical formula of graphane.
two physical properties of silicon dioxide
hard, brittle (not malleable), non-conductor, insoluble
Describe structure and bonding of phosphorus oxide
P4O10
- simple molecule / molecular
- weak covalent bonds & weak van de waals between molecules
Why is graphite soft
it has planes that have weak van de waals forces between them
Compare the electrical conductivity of solid sodium metal with that of solid sodium chloride. Explain your answer.
Sodium conducts, sodium chloride doesnt
delocalised electrons can flow around metal
electrons can carry current
ions cant move in sodium chloride
Explain why the melting point of sodium chloride is high.
Strong electrostatic attraction between oppositely charged ions
Shape name and bond angle of 3 bond pairs and 0 lone pairs
Shape name and bond angle of 4 bond pairs and 0 lone pairs
Shape name and bond angle of 5 bond pairs and 0 lone pairs
Shape name and bond angle of 6 bond pairs and 0 lone pairs
Shape name of 2 bonds pairs, 1 lone pair
Shape of 3 bond pairs and 1 lone pair
Shape of 4 bond pairs and 1 lone pair
Shape of 5 bond pairs and 1 lone pair
Shape of 2 bond pairs and 2 lone pairs
Shape of 3 bond pairs and 2 lone pairs
Shape of 4 bond pairs and 2 lone pairs
Explain how the electron pair repulsion theory can be used to deduce the shape of, and the bond angle in, NHF2.
