Periodic Table Flashcards
Differences between Mendeleev’s table and Modern Periodic Table
Elements arranged in order of atomic weight - elements arranged in order of atomic number
No noble gases present (not discovered) - noble gases present
Gaps are left for undiscovered elements
No block of transition metals presents - a block of transition metals is present
No actinides or lanthanides present - actinides and lanthanides are present (block of elements at the bottom of the table.)
Differences between metal and non-metal
Melting point - High - Low ( except graphite and diamond)
Malleability - malleable - not malleable
Ductility - ductile - not ductile
Sonority - sonorous - not sonorous
Conduction of heat/electricity - Good - Poor
What are common factors of ionic equations
2 species
No spectator ions present
What is a displacement reaction? And ionic version of a displacement reaction
A more reactive element can displace a less reactive element in a compound
Magnesium + Copper Sulfate —> Magnesium sulfate + Copper
Mg + CuSO4 —> MgSO4 + Cu
Ionic equation removes spectator ions
Mg(s) + Cu(aq) —> Mg(aq) + Cu(s). (Add in charges)
What is an neutralisation reaction? And the ionic version?
When an alkaline and acidic substance neutralise each other and create a salt + water
E.g Sodium Hydroxide + Hydrochloric acid —> sodium chloride + water
NaOH + HCl —> NaCl + H2O
Ionic equation removes spectator ions
OH(aq) + H(aq) —> H2O(l). (Add in charges)
What is a precipitation reaction? And the ionic version?
Precipitation reactions occur when cations and anions in aqueous solution combine to form an insoluble ionic solid called a precipitate.
Barium chloride + sodium sulfate —> Barium sulfate + sodium chloride
BaCl2 + Na2SO4 —> BaSO4 + 2NaCl
Ionic
Ba(aq). + SO4(aq) —> BaSO4(s) (Add in charges)
oxidation reaction
Alkali metal + oxygen —> alkali metal oxide
Alkaline hydroxide reaction
Alkali metal + water —> alkali metal hydroxide + hydrogen
Why and how are group 1 metals stored?
They are stored in oil to stop them reacting with the oxygen
Properties of group 1 metals
Are metals with low density
Lithium, Sodium and Potassium are less dense than water and float on its surface.
Have low melting and boiling points
They are stored in oil as they tarnish rapidly in air
Are soft enough to be cut by a knife
Shiny when freshly cut but rapidly tarnish in air
React rapidly with water and form an alkaline solution alkaline and Hydrogen gas.
What are the observations for lithium’s reaction with water
> Moves on the water surface
bubbles
heat released
Li disappears at the end of the reaction
colourless solution produced
What are the observations for Sodium’s reaction with water
> Moves on the water surface
Na melts into a tiny ball
bubbles
heat released
Na disappears at the end of the reaction
colourless solution produced
What are the observations for Potassium’s reaction with water
> Moves on the water surface
K melts into a tiny ball
produces a lilac flame
bubbles
heat released
Na disappears at the end of the reaction
colourless solution produced
crackles at the end of the reaction
Word and symbol equation for lithium + water
Lithium + Water —> Lithium Hydroxide + Hydrogen
2Li(s) + 2H2O(l) —> 2LiOH(aq) + H2(g)
Word and symbol equation for Sodium + water
Sodium + Water —> Sodium Hydroxide + Hydrogen
2Na(s) + 2H2O(l) —> 2NaOH(aq) + H2(g)
Word and symbol equation for Potassium + water
Potassium + Water —> Potassium Hydroxide + Hydrogen
2K(s) + 2H2O(l) —> 2KOH(aq) + H2(g)
Symbol equation for half equations for group 1 ions
X —> x+ + e-
Na —> Na+ + e-
Why does reactivity increase going down group 1
As you go down group 1 the outer shell’s electrons are further from the nuclear charge.
They are less strongly attracted to the positive nucleus and easier to lose.
What colour is the halogen fluorine and what state is it at room temperature
Pale yellow - gas
What colour is the halogen Chloride and what state is it at room temperature
Green-yellow. - gas
What colour is the halogen bromine and what state is it at room temperature
Red-brown - liquid
What colour is the halogen iodine and what state is it at room temperature
Grey-black - solid
What happens to iodine when heated
Sublimes and produces a purple vapour
Half equations for group 7 ions
X2 + 2e- —> 2X-
I2 + 2e- —> 2I-
Why does reactivity decrease going down group 7
As the number of shells increases the outer shells is further from the attraction of the positive nucleus so its more difficult to attract the incoming electron.
Displacement of halogens
A more reactive halogen will always displace a less reactive halide from its compounds in solution.
Colour of halogen chlorine in solution
Pale green solution
Colour of halogen Bromine in solution
Orange solution
Colour of halogen iodine in solution
Brown solution
How does toxicity effect halogens?
All halogens are toxic and it decreases going down the group
Properties of elements in group 0
Colourless gases at room temp
unreactive/inert
What happens to the boiling points of elements in group 0 as you go down the group?
They increase as the strength of the van deer Waals forces increases.
Why are elements in group 0 unreactive?
As they are already stable, have a full outer shell of electrons and don’t need to gain or lose electrons.
What are the physical properties of transition metals?
- High Melting Point
- High Density
- Low Reactivity with water
- Reacts to form ions with different charges
- Form coloured compounds
What colour is copper (ll) oxide
Black
What colour is copper (ll) carbonate
Green
What colour is hydrated copper (ll) sulphate
Blue
What colour are copper (ll) salts usually in solution
Blue
What are the physical properties or group 1 metals?
Low melting point
Low density
Very reactive with cold water
react to form 1+ ions e.g. K+
Forms white compounds
What can you do when risk assessing for the reaction of alkali metals and water?
Use tweezers to lift the metals to prevent handling the metal directly as it could react with water in the skin
Use a safety screen as this prevents corrosive hydroxide solution from splashing out and causing damage to the skin
How do you prepare alkali metals for reaction with water?
- Cut a small piece of metal
- Remove the oil layer with filter paper
- Use tweezers to drop the metal into a large trough of water behind a safety screen and wearing safety glasses
