Metallic behaviour
Metallic elements are found on the left-hand side of the periodic table
Metallic atoms tend to be larger than non-metals in the same period
Metallic atoms have a lower effective nuclear charge (core charge)
This means that atoms tend to lose their outer shell electrons
Atoms which lose electrons are no longer neutral
They form positive ions, called cations
Predicting charges of cations
The cation charge of metals can be determined by losing electrons until the shells have a stable noble gas electronic configuration
(i.e 8 valence electrons/full p orbital)
Group 1 metals form +1 cations, lose one electron
Group 2 metals form +2 cations, lose two electrons
Group 13 metals form +3 cations, lose three electrons
Examples:
Write the electronic configuration of the atoms below and hence determine the charge of the ion. (you may choose to use the shell or subshell model)
a) Calcium b) Aluminium
1s2, 2s2, 2p6, 3s2, 3p6, 4s2 1s2, 2s2. 2p6, 3s2, 3p1
charge of ion: +2 charge of ion: +3
Reactivity of metals
Although metals all tend to lose electrons, they way in which metals can lose electrons can vary significantly between metals.
Reactivity refers to how easily an atom or element undergoes a chemical reaction, often by losing, gaining, or sharing electrons to form a stable configuration.
Atoms which are unreactive are described as inert
Reactions with water, oxygen and acids
Reactivity depends on not just the metal but also what it is reacting with
We often react with water, oxygen and acids as these are commonly found in environments or in laboratory conditions
Metals which react with water typically form H2 and metal hydroxides
Oxygen is very good at taking electrons and often reacts with metals to form their metal oxides (this process is known as oxidation)
Acids which react with metals will corrode the metal and produce hydrogen gas and metal salts
Reactivity series
Chemists have used experimental data to produce a reactivity series of metals
In general, the more loosely-bound valence electrons
are to the nucleus, the more reactive the metal
Going down group:
reactivity increases
Because... atomic radius increases, valence electrons are further from nucleus, therefore more reactive
Going across period:
reactivity decreases
Because...atomic radius decreases, valence electrons are closer to the nucleus, therfore less reactive
Explain why metals such as iron, copper, titanitum and aluminium must be mined in their oxide forms (ores) but metals such as gold and platinum can be found naturally on earth in their elemental forms?
Metals like iron, copper, titanium, and aluminium must be mined as oxides (ores) because they are highly reactive and readily combine with oxygen and other elements in the Earth's crust. In contrast, gold and platinum are found in their elemental forms because they are very unreactive.
Reactivity of metals
Metallic behaviour
Metallic elements are found on the left-hand side of the periodic table
Metallic atoms tend to be larger than non-metals in the same period
Metallic atoms have a lower effective nuclear charge (core charge)
This means that atoms tend to lose their outer shell electrons
Atoms which lose electrons are no longer neutral
They form positive ions, called cations
Predicting charges of cations
The cation charge of metals can be determined by losing electrons until the shells have a stable noble gas electronic configuration
(i.e 8 valence electrons/full p orbital)
Group 1 metals form +1 cations, lose one electron
Group 2 metals form +2 cations, lose two electrons
Group 13 metals form +3 cations, lose three electrons
Examples:
Write the electronic configuration of the atoms below and hence determine the charge of the ion. (you may choose to use the shell or subshell model)
a) Calcium b) Aluminium
1s2, 2s2, 2p6, 3s2, 3p6, 4s2 1s2, 2s2. 2p6, 3s2, 3p1
charge of ion: +2 charge of ion: +3
Reactivity of metals
Although metals all tend to lose electrons, they way in which metals can lose electrons can vary significantly between metals.
Reactivity refers to how easily an atom or element undergoes a chemical reaction, often by losing, gaining, or sharing electrons to form a stable configuration.
Atoms which are unreactive are described as inert
Reactions with water, oxygen and acids
Reactivity depends on not just the metal but also what it is reacting with
We often react with water, oxygen and acids as these are commonly found in environments or in laboratory conditions
Metals which react with water typically form H2 and metal hydroxides
Oxygen is very good at taking electrons and often reacts with metals to form their metal oxides (this process is known as oxidation)
Acids which react with metals will corrode the metal and produce hydrogen gas and metal salts
Reactivity series
Chemists have used experimental data to produce a reactivity series of metals
In general, the more loosely-bound valence electrons
are to the nucleus, the more reactive the metal
Going down group:
reactivity increases
Because... atomic radius increases, valence electrons are further from nucleus, therefore more reactive
Going across period:
reactivity decreases
Because...atomic radius decreases, valence electrons are closer to the nucleus, therfore less reactive
Explain why metals such as iron, copper, titanitum and aluminium must be mined in their oxide forms (ores) but metals such as gold and platinum can be found naturally on earth in their elemental forms?
Metals like iron, copper, titanium, and aluminium must be mined as oxides (ores) because they are highly reactive and readily combine with oxygen and other elements in the Earth's crust. In contrast, gold and platinum are found in their elemental forms because they are very unreactive.