two properties of simple ionic bonds
- high melting and boiling points because their strong electrostatic forces of attraction between oppositely charged ions/ ionic bonds which require a lot of heat to break
- can conduct electricity when molten because there are some free electrons/ions which can carry charge
- brittle
two properties of simple covalent bonds
- low melting and boiling points because they have weak intermolecular forces which require little heat to break.
- can not conduct electricity because there are no free electrons to carry charge
- gases and volatile liquids at room temperature
what are ‘-ate’ ions?
negatively charged compound ions with oxygen
what are ‘-ide’ ions
negatively charged ions
two properties of metals
- high melting and boiling points because of their strong metallic bonds which require a lot of heat to break
- can conduct electricity and heat because of the sea of delocalized electrons around metal ions which can carry charge
- malleable (easy to shape) and ductile (easy to carry charge) because of their lattice structure (in layers)
- shiny
properties of giant covalent bonds
- high melting and boiling points because of their strong covalent bonds
- most cannot conduct electricity because there are no delocalized electrons to carry charge
name the allotropes of carbon
- diamond
- graphite
- buckminsterfullerene or buckybal
two properties of diamond
- high melting and boiling points because of strong covalent bonds which require a lot of head to break.
- hard
- cannot conduct electricity because there are no free electrons to carry charge
two properties of graphite
- high melting and boiling points because of strong covalent bonds which require a lot of head to break.
- slippery because of their structure (in layers)
- can conduct electricity because they have delocalized electrons which can carry charge
properties of alkali metals that are different from normal metals
- soft and can be cut with a knife
- low density
- low melting and boiling point
properties of alkali metals that are similar to normal metals
- shiny
2. good conductors of heat and electricity because of their delocalized electrons which can carry charge
the alkali metals
Lithium (Li) Sodium (Na) Potassium (K) Rubidium (Rb) Caesium (Cs) Francium (Fr)
two properties of sand (silicon dioxide)
- high melting and boiling point because of the strong covalent bonds which require a lot of heat to break.
- huge number of covalent bonds
- made up of two elements (silicon and oxygen)
chemical properties of alkali metals
- alkali metals react with oxygen to form an alkali metal oxide
alkali metal + oxygen -> alkali metal oxide
- the rate at which the alkali metal reacts with oxygen increases down the group
chemical properties of alkali metals
- alkali metals react with oxygen to form an alkali metal oxide
alkali metal + oxygen -> alkali metal oxide - the rate at which the alkali metal reacts with oxygen increases down the group
- reaction between an alkali metal and oxygen is known as an oxidation reaction. this happens when the delocalized electron is lost and forms an ionic bond with oxygen.
reaction with water
all alkali metals react vigorously with water and the reaction becomes more vigorous as you tren down the group.
alkali metal + water hydroxide -> alkali metal + hyprogen
2M(s) + 2H20(l) -> 2MOH (aq) + H2(g)
features of alkali metals
- density increases as you go down the group
- reactivity increases as you go down the group
- melting and boiling point decrease as you go down the group
- rarely found as pure elements
two differences between diamond and graphite
- graphite is soft and slippery while diamond is hard
2. graphite can conduct electricity while diamond can not
metallic bonding
strong electrostatic attraction between delocalized electrons and metal ions
alloys
when an element is added to a metal to strengthen it. when this happens, it reduces its malleability and ductility.
allotropes
different forms of the same element
what type of rings does graphite form?
hexagonal rings in layers
