Bonding & structure questions Flashcards
Describe the motion of the atoms in a crystal of silicon dioxide
the atoms vibrate around in a fixed position
in terms of structure and bonding, describe what happens to the atoms in a crystal of silicon dioxide when it melts
the covalent bonds are broken and the atoms are free to move
state the type of intermolecular force(s) in BF3
London
state the type of intermolecular force(s) in NF3
London, dipole-dipole
what type of bond is formed between a molecule of BF3 and NF3
dative covalent bond
by referring to the types of intermolecular force involved, explain why energy must be supplied in order to boil liquid hydrogen chloride
energy is needed to overcome the London and Dipole-Dipole forced
Explain why the boiling point of hydrogen bromide lies between those of hydrogen chloride and hydrogen iodide
HBr has an intermediate size, as the London forces depend on molecular size
Explain why the boiling point of hydrogen fluoride is higher than that of hydrogen chloride
There are hydrogen bonds in HF, so the intermolecular forces are stronger than HCl
What is the electronic configuration of aluminium
1s2 2s2 2p6 3s2 3p1
what is the electronic configuration of vanadium
1s2 2s2 2p6 3s2 3p6 4s2 3d3
describe the bonding present in metals
the attraction between positively charged nuclei and the delocalised electrons in a cloud of electrons
explain how the bonding and structure of metals allow it to be electrical conductors
the freely moving electrons can carry a charge
explain how the bonding and structure of metals allow it to be malleable
the layers can slide over each other, whilst the attractive forces remain the same throughout the lattice
suggest a reason why aluminium is a better conductor of electricity than magnesium
Aluminium has more outer shell electrons,
AL+3 and MG+2
state and explain the trend in electronegativity of the elements across Period 3 from sodium to chlorine
there is an increase in electronegativity across a period, as the nuclear charge increases whilst shielding stays the same
why does a molecule of CH3Cl have a permanent dipole but CCL4 is not polar
CH3Cl has asymmetry of polar C-Cl bonds
use the kinetic theory to describe the changes that take place as calcium oxide is heated from 25°C to a temperature above its melting point
as temperature increases until the vibrations are so violent that the ions break free at the melting point
state 2 properties of calcium oxide that depends on its bonding
- has a high melting and boiling point
- is an electrical conductor as a liquid or gas
