Topic 5: Metals Flashcards
Metallic Bonding
Is the electrostatic force between metal ions in a lattice structure and delocalised electrons
How/why can metals conduct electricity?
Because they contain delocalised electrons
The stronger the metallic bonds…
the higher the energy to break the bonds + higher melting and boiling points
What is formed when metals react with oxygen?
Metal oxides
Word equation for metals and oxygen
Metal + Oxygen —> Metal Oxide
What is formed when metals react with water?
Metal hydroxide
Word equation for metals and water
Metal + Water —> Metal Hydroxide + Hydrogen gas
What is formed when metals react with acids?
Metal salt
When a metal reacts, what will the metal atoms form? (oxidation)
Metal ions
Oxidation
is a loss of electrons by a reactant in any reaction
Reduction
is a gain of electrons by a reactant in any reaction
How can a metal ion turn back into an atom?
When a metal ion in a compound gains electrons (reduction)
Redox reactions
When both oxidation and reduction is happening
How to figure out an ion-electron equation is oxidation or reduction?
ROLR (right=oxidation, left = reduction)
Most reactive metals (K, Na, Ca…) need to be extracted by…
electrolysis
Most reactive metals (6)
Potassium, sodium, calcium, lithium, magnesium, aluminium
Quite reactive metals (5)
Zinc, tin, iron, nickel, lead
Not so reactive metals
Gold, copper, silver, mercury,
Why do most reactive metals need to be extracted by electrolysis?
Because the metals hold on to the oxygen really tightly, making it difficult to split
Electrolysis
A process used to break down ionic substances by passing a direct current through the substance.
Positive ions gain their electrons at the….
negative electrode
Negative ions lose their electrons at the…
positive electrode
Those in the middle of the reactivity series need to be extracted by…
A reducing agent (carbon or carbon monoxide…)
Metals that aren’t very reactive can be extracted by…
heat alone
