1.4.10 Effects of Structure & Bonding Flashcards
Different types of structure and bonding have different effects on the
physical properties of substances such as their melting and boiling points, electrical conductivity and solubility
Ionic compounds are strong as
the strong electrostatic forces in ionic compounds keep the ions strongly together
Ionic compounds are brittle, meaning
ionic crystals can split apart easily
onic compounds have high
melting and boiling points
Ionic compounds have high melting and boiling points, the
strong electrostatic forces between the ions in the lattice act in all directions and keep them strongly together
Melting and boiling points increase with
charge density of the ions
Melting and boiling points increase with charge density of the ions due to
the greater electrostatic attraction of charges
Ionic compounds are what in water
soluble
Ionic compounds are soluble in water as
they can form ion - dipole bonds
Ionic compounds only conduct electricity when
molten or in solution
Ionic compounds only conduct electricity when molten or in solution, when molten or in solution
the ions can freely move around and conduct electricity
Ionic compounds only conduct electricity when molten or in solution, in the solid state
they’re in a fixed position and unable to move around
Metallic structures are malleable, when a force is applied
the metal layers can slide
Metallic structures are malleable, the attractive forces between
the metal ions and electrons act in all directions
Metallic structures are malleable, so when the layers slide
the metallic bonds are re-formed
Metallic structures are malleable, the lattice is
not broken and has changed shape
Metallic lattices are strong and hard, due to
the strong attractive forces between the metal ions and delocalised electrons
Metals have high
melting and boiling points
Pure metals are what in water
insoluble
Metals can conduct electricity when in
the solid or liquid state
Metals can conduct electricity when in the solid or liquid state, as both in the solid and liquid state
there are mobile electrons which can freely move around and conduct electricity
Metals are malleable as the layers can slide over each without breaking the attraction diagram
Simple covalent lattices have low
melting and boiling points
Simple covalent lattices have low melting and boiling points, these compounds have
weak intermolecular forces between the molecules
Simple covalent lattices have low melting and boiling points, only little energy
is required to break the lattice
Most compounds are insoluble with water, unless
they are polar and can form hydrogen bonds (such as sucrose)
Simple covalent lattices do not conduct electricity in the solid or liquid state as
there are no charged particles
Some simple covalent compounds do conduct electricity in solution, but
this is a reaction with the water than produces ions such as HCl which forms H+ and Cl- ions
Giant covalent lattices have very high
melting and boiling points
Giant covalent lattices have very high melting and boiling points, these compounds have a large number of
covalent bonds linking the whole structure
Giant covalent lattices have very high melting and boiling points, a lot of energy is required to
break the lattice
Giant covalent lattices compounds can be
hard or soft
Graphite is soft as
the forces between the carbon layers are weak
Diamond and silicon(IV) oxide are hard as
it is difficult to break their 3D network of strong covalent bonds
Most compounds do not conduct electricity however some do, graphite has
delocalised electrons between the carbon layers which can move along the layers when a voltage is applied
Most compounds do not conduct electricity however some do, diamond and silicon(IV) oxide
do not conduct electricity
Most compounds do not conduct electricity however some do, diamond and silicon(IV) oxide do not conduct electricity as
all four outer electrons on every carbon atom are involved in a covalent bond so there are no freely moving electrons available
Characteristics of Different Compound Structure Types Table
