B1 Moles, Formulae + Equations Flashcards
Charge of group 1 ions
1+
Charge of group 2 ions
2+
Charge of group 3 ions
3+
Charge of group 5 ions
3-
Charge of group 6 ions
2-
Charge of group 7 ions
1-
Formula and charge of nitrate
Formula and charge of carbonate
Formula and charge of sulfate
Formula and charge of hydroxide
Formula and charge of ammonium
Formula and charge of zinc
Formula and charge of silver
How to write ionic equations
- Write balanced symbol equation
- Aqueous compounds split, solid remain unchanged
- Remove spectator ions
- Cancel down
Define Mole
A unit containing 6.02 x10 (23) particles
Define Avagadro’s constant
The number of particles per mole
Equation for the mass of one atom, using avagadro’s constant
Define Empirical Formula
The simplist whole number ratio of atoms of each element present in a compound
Define Molecular Formula
The number and type of atoms of each element in a molecule
Define Anyhdrous
A compound containing no waters of crystallisation
Define Hydrated
A compound containing waters of crystallisation
How to calculate the empirical formula of a compound/waters of crystallisation
- Calculate moles of each substance in the compound
- Find the simplest whole number ratio
Moles equation, with mass
Moles equation, with volume
Moles equation, with concentration
Moles equation, with concentration in grams/dm3
Ideal Gas Equation
PV = nRT
What must you always remember when solving a problem using the ideal gas equation
Re-arrange the equation as symbols before solving
Unit of pressure for ideal gas equation, and how to convert from atmospheres
- Pascals
- 1atm = x10(5) pa
Unit for volume in ideal gas equation, and how to convert from other units
- meteres^3
- cm = x10(-6)
- dm = x10(-3)
n in ideal gas equation
Moles
Unit for temperature in ideal gas equation, and how to convert
- Kelvin
- Celcius to kelvin
- +273
Equation for pecentage yield
Equation for atom economy
Equation for percentage uncertainty
When to multiply uncertainty by 2 when calculating percentage uncertainty
- Titres
- Mass
- Temperature
What is the only gaseous alkali
Ammonia (NH3)
Define an acid
Releases H+ ions in aqueous solutions
Describe the difference between weak and strong acids
- Weak acids partially dissociate H+ ions in aqueous solutions
- Strong acids partially dissociate H+ ions in aqueous solutions
Define an alkali
Releases OH- in aqueous solutions
Define a salt
The metal ion (X+) has replaced the H+ ion
How many decimal places should be used in titre volumes
2dp
Describe how to obtain a crystal sample
- Heat in evaporating basin until crystals start to form around outside
- Leave to cool and crystallise
- Filter to obtain solid crystals
- Dry by dabbing with filter paper
What are concordant results
Results within 0.1cm(^3) of each other
Define Standard Solution
A solution of a known concentration
Describe and explain how to prepare a standard solution
- Weigh mass of crystals in beaker on mass balance to 2dp
- Dissolve in distilled water
- Transfer to 250cm volumetric flask
- Rinse beaker and transfer washings to volumetric flask
- Make up to mark wtih more water, so bottom of meniscus is on mark
- Use dropping pipette when filling to the mark
- Put a stopper on top, and invert several times to mix
