4 for test 2 Flashcards
acid + metal
salt and hydrogen gas
acid + base
salt and water
acid + metal carbonate
salt and water and CO2
Base + ammonium salt
salt and water and ammonia gas (pungent colourless gas)
precipitation reaction
2 aqueous solutions produce dissolved salt and insoluble salt
ionic equations
only break soluble ionic substances (aqueous) and strong acids. When cancel out the equation will show what is reacting.
Strong acids
HCl, HNO3, H2SO4. Will dissociate into their ions in ionic question.
Weak acids
Dont dissociate
At room temp metallic, ionic and cov are
M and I - solid
C - gas, liquid or solid. existing in pairs like Cl2
distinguishing between pairs
- state and colour appearance
- solubility of substances
- reaction to both substances and observe how they react
Precipitation reaction to distinguish 2 aqueous solutions
Add xNO3. x should form are solution with one of the reactants and a solid with the other. Group 1 will not form precipitate
Flow chart tests
- Appearance (colour, shiny, state)
- solubility
- if it reacts with acid
- base
- precipitation reaction. Can identify with colour precipitate
- conductivity from what type of bond is present
Solution formed from a weak acid
also wont dissociate
name Br2, name FeBr2
Br2 - Bromine as it is in molecular form
FeBr2 - Iron(II) Bromide. Ide prefix as it s made of bromide ions bonded to Iron ions.
Group 1 metals - alkali metals
Never form a precipitate so don’t use them for precipitate reactions
