Metals Flashcards
Properties of metals
- good thermal conductor
- shiny
- good electrical conductor
- most are solids at room temperature
- lustrous (can be polished
- sonorous (make a ringing sound when it)
- hard/strong
- high melting and boiling points
Properties of non-metals
- dull
- bad thermal conductor
- bad electrical conductor
- most are liquids or gases at room temp
- brittle
- weak
- low melt and boil pnts
Properties of Metallic bonding
– solid at room temp and pressure
- high melt and boil points
- good conductors of heat and electricity
- malleable
- ductile
- strong
- dense
What structure does metallic bonding create
Giant Metallic Lattice Structure
what is Metallic Bonding
The electrostatic force of attraction between positive metal ions and a sea of delocalized electrons
Why are metallic structures Malleable, Ductile, and Strong
The layers of metal ions are able to slide over each other so the structure will not shatter.
The metallic bonds do not break because the delocalized electrons are free to move around the structure
Unique characteristics of Group 1 Alkaline Metals
- Soft (can be cut with a knife)
- Low density (float on water)
- Low melt and boil pts (Na melts into a ball in cold water)
Group 1 Alkaline Metal Trends: Density, Boiling Points, Reactivity
As you go down the group:
Density increases
Melt and Boil pts decrease
Reactivity increases
What happens to Potassium when added to water
Bursts into a lilac flame
What happens to Sodium when added to water
Melts into a ball
What is thermal decomposition
When heat energy is used to break down a substance
What is OIL RIG
Oxidisation is loss of electron (or gain of oxygen)
Reduction is gain of electrons (or loss of oxygen)
What is the Thermite Reaction
Iron(111) Oxide + Aluminium -> Aluminium Oxide + Iron
What is the Thermite Reaction used for
Welding tracks together
What is a REDOX reaction
The simultaneous reduction and oxidation of a species in a reaction
What is rust
The corrosion of iron (other metals don’t rust they corrode)
What is the chemical name for rust
Hydrated iron (lll) oxide
Methods of preventing Rust
- Sacrificial Protection (coating in Zinc)
- galvanising
- Barrier methods (Coat in oil or grease or paint or plastic)
What needs to be present for iron to rust
Both oxygen and water
what is an alloy
a compound consisting of a metal with at least one other element
what is steel a mix of
carbon and iron
iron + oxygen + water ->
hydrated iron (lll) oxide
why does reactivity increase as you go down group 1 (alkaline metals)
because the atoms get bigger with more shells meaning more shielding, less attraction to the nucleus and so they are more likely to lose their outer electron
what is the oxidising agent
gains electrons from other atoms (it itself reduced)
what is the reducing agent
donates electrons to the other atom (it itself being oxidised)
what is a REDOX reaction
when reduction and oxidation simultaneously occur
how are unreactive metals found in the earth’s crust
as the uncombined element
how are most metals extracted from the earth’s crust
as ores
what is the method of extraction of a metal related to? give 2 examples
its position in the reactivity series
- carbon extraction for iron -
- electrolysis for aluminium -
al = more reactive than: iron
why are alloys harder than pure metals
because the larger ‘other’ atoms cause an irregular pattern which doesn’t allow particles to slide over each other
what is thermal decomposition
when heat energy is used to break down a substance
equation for the thermal decomposition of a metal carbonate
metal carbonate -> metal oxide + carbon dioxide
how is carbon dioxide normally collected and why
through downward delivery
CO2 is denser than air so it sinks to the bottom of a tube and will stay there until you want to use it
state the reactivity series
equation for when metals react with cold water
metal + water -> metal hydroxide + hydrogen
what are the two observations of a reaction between metal and cold water
- effervescence (hydrogen gas)
- solid disappears
what are the four observations of Lithium Sodium and Potassium with water
solid floats - it is less dense than water
effervescence - hydrogen
solid moves - effervescence propels it around
solid disappears
what would you see when adding universal indicator in a reaction between a metal and cold water
turns dark blue because metal hydroxides are alkaline
what can be observed when sodium reacts with cold water
solid melts
solid floats - it is less dense than water
effervescence - hydrogen
solid moves - effervescence propels it around
what can be observed when potassium reacts with water
solid melts
lilac flame
solid floats - it is less dense than water
effervescence - hydrogen
solid moves - effervescence propels it around
why are the products of reacting metals with water and steam different
steam has more energy so both bonds in the water molecules can break
how are metal + steam reactions normally carried out
equation for the reaction between metal and steam
metal +steam -> metal oxide + hydrogen
3.5.4
What are the observations when an excess of magnesium powder is added to an aqueous solution of copper (II) sulfate
- pink/brown solid forms
- solution turns colourless
What is the meaning of exothermic
A reaction that gives out thermal energy
