AQA Chemistry C3 Part 1
Stuff you need to know from the first section of the separate science chemistry bit (elements, acids and water)
- Created by: Abbie
- Created on: 22-05-12 19:47
Periodic Table
Early 1800s - categorise elements by physical/chemical properties & atomic mass
Newlands' Octaves - every 8th element similar properties BUT left no gaps for unknown elements, so not all had similar properties, mixed up metals & non-metals
Mendeleev - left gaps so similar properties were in the same group, gaps predicted unknown elements - convincing evidence that periodic table useful
NOW - based on electronic structure (in order of atomic number)
Max number of electrons in each shell is:
- 1st = 2
- 2nd = 8
- 3rd = 18,
Alkali Metals (Group 1)
As you go down group 1:
- Bigger atoms
- More reactive
- More dense
- Lower melting point & boiling point
All:
- Reactive
- Have 1 outer-shell electron
- Form ionic compounds
- Reaction with water produces hydrogen gas (& the solution becomes alkaline)
Halogens (Group 7)
As you go down group 7:
- Less reactive
- Higher melting & boiling points
All:
- Travel in pairs
- Do both ionic and covalent bonding
- React with metals to form salts (2Al + 3Cl2 ---------> 2AlCl3)
- More reactive ones displace less reactive ones
- Flourine - poisonous, yellow gas
- Chlorine - poisonous, green gas
- Bromine - poisonous, red/brown liquid
- Iodine - dark grey solid, or purple vapour
Transition Elements
- Good conductors
- Dense, strong & shiny
- Not very reactive
- High melting points
- Often have more that one ion (Fe2+, Fe3+)
- The compounds are colourful
- Make good catalysts (iron for Haber process)
Properties because of the way the electron shells fill - further away from nucleus shells start to overlap effecting the way shells fill:
Sc: 2,8,9,2 Ti: 2,8,10,2 V: 2,8,11,2 Cr: 2,8,13,1 Mn: 2,8,13,2 Fe: 2,8,14,2 Co: 2,8,15,2 Ni: 2,8,16,2 Cu: 2,8,18,1 Zn: 2,8,18,2
Acids and Alkalis
Arrhenius - acids release hydrogen ions (H+) in water & all alkalis for hydroxide ions (OH-) in water. BUT only worked for acids & alkalis that dissolved in water, exceptions (ammonia gas) so scientists didn't believe him
Bronsted and Lowry - acids release H+ ions (proton donors), alkalis accept H+ ions (proton acceptors)
Acidic solutions - the acid molecules dissociate and release lots of H+ ions, which become hydrated (surrounded by water molecules)
Basic solutions - water molecules dissociate into H+ and OH- ions, some base molecules take hydrogen ions from water causing more molecules to dissociate, other bases release OH- ions straight into the solution
Acids, Alkalis and Titration
Strong Acids (sulfuric, hydrochloric, nitric) ionise/dissociate almost completely in water - lots of H+(aq)
Weak Acids (ethanoic, citric, carbonic) ionise slightly - small numbers of H+(aq)
Strong Alkalis (sodium & potassium hydroxide)
Weak Alkalis (ammonia)
Titrations:
- How much acid needed to neutralise an alkali - concentration
- Alkali in a flask add acid
Indicators:
- Strong acid & strong alkali - any
- Strong acid & weak acid - methyl orange
- Weak acid & strong alkali - phenolphthalein
Titration Calculations in MOLES per dm3
Step 1 - Calculate number of moles of known substance
Step 2 - Write out equation and ratio moles
Step 3 - Work out the concentration of 'unknown stuff'
Titration Calculations in GRAMS per dm3
Step 1 - Work out relative formula mass for the unknown substance
Step 2 - Work out concentration in grams using the concentration in moles that you just worked out
Water
Water cycle - sun causes evaporation > water carried upwards as warm air rises > cools > water condenses to form clouds > droplets get too big > fall as rain > back to sea
Water dissolves most ionic compounds - water molecules surround the ions and disrupt the bonding, slightly positive hydrogen attracts the negative side & slightly negative oxygen attracts the positive side
These ionic compounds dissolve in water:
- Salts of sodium, potassium & ammonium
- Nitrates
- Chlorides except from silver & lead
- Sulphates apart from barium & lead
Solubility
Saturated solution can't hold any more solid at that temp
Solubility increases with temp
Cooling causes crystallisation
Higher pressure, more gas dissolves
Lower temp, less gas dissolves
Hard Water
Problems: Won't form lather - more soap, scale on inside of pipes & kettles, thermal insulator - longer for kettle to boil, scum
Caused by: Ca2+ & Mg2+ ions - rainwater runs over rocks
Good points: Ca2+ good for teeth & bones, scale forms protective coating inside pipes - stops lead poisoning
Removing hardness:
- Add sodium carbonate - carbonate joins on to calcium/magnesium to form an insoluble precipitate
- Ion exchange column - swaps calcium & magnesium ions for sodium ones
- Scale can be dissolved by acid
Water Quality
Water must be free of poisonous salts and harmful microorganisms - treated
Treatment:
- Through mesh screen - remove big bits (twigs)
- Treated with ozone/chlorine - kill microorganisms
- Chemicals added - makes solids & microorganisms stick together and fall to the bottom
- Filtered through gravel beds - remove all solids
- pH corrected
- Chlorinated to kill any microorganisms left
Water filters:
- Contain carbon or silver to remove substances from tap water
- Carbon - removes chlorine taste
- Silver - kills bugs
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