Moles
To find the number of moles in a reaction we need the formula n=m/M where m is the mas and M is the molar mass
To find the number of moles when we have gases we need the formula n=V/Vm where V is the volume and Vm is the volume molar
To calculate the concentration of a substance in a reaction we need the formula Cm=n/V where n is the number of moles and V is the volume
1 dm3=1000 cm3
Empirical formula shows the simplest ratio in which atoms combine to form a compound ✅
Molecular formula shows the actual numbers of atoms that combine to forma a compound ✅
Yield equals to actual mass of product obtained/theoretical mass of product
Purity equals mass of pure product/mass of impure product obtained x100%
Chemistry
Organic chemistry
Groups
Alkanes
C(n)H(2n+2)
Saturated comopunds
C-H functional group
Cracking reaction
Alkenes
C(n)H(2n)
Periodic table
Groups
Group 2-4
Group 5-8
Group 1
Unsaturated compounds
Long ⛓ of alkane 💥 into shorter chains + alkene
➕ reaction
2 reactants enter, 1 product released
C2H4 + Cl2 -> C2H4Cl2
Addition reaction with steam
Alcohols
Saturated compounds
Functional group OH
C(n)H(2n+1)OH
Detailed Reactions
Polymerisation
Addition polymerisation
Condensation poleymerisation
Group 1
Sodium
Potassium
Lithium
long ⛓ made up of alkene monomers
Rubidium
Caesium
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Linkage groups
Ester linkage
🔧 from COOH + OH
C=O O
Trends of Group 1
Reactivity increases
Density increases
Transition elements
Amide linkage
Iron
🔧 from NH2 + COOH
CONH
Nicklel
Copper
Silver
Zinc
Gold
Platinum
Mercury
Chromium
Titanium
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Repeating chains of 2 monomers each with a linkage group linking them together
Trends
good conductors of heat and electricity
High density
Substitution reaction
C2H6 + Cl2 -> C2H5Cl + HCl
C=C functinoal group
The behavior of metals
Acts as catalysts
MP decrease
Halogen
Halogens
Astatine
Iodine
Flourine ⚠
Bromine ⚠
Chlorine ⚠
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Trends
Density increases
Going down the group reactivity decreases
MP and BP increases
All of them are toxic
Working in a lab
Metals
Substance tests
Non-metals
Malleable
Ductile
Strong
Metals
Non-Metals
🔥 test
Ion tests
High density
Na+ -> Yellow
K+ -> Lilac
Li+ -> Red
Good conductors of ⚡ and 🔥
Ca(2+) -> Orange-red
Ba(2+) -> Green
Cu(2+) -> Blue-green
low melting and boiling point
dull
Brittle
dont conduct electricity
Ions
SO3(2-)
Zn(2+)
Al(3+)
Fe(3+)
Ca(2+)
Fe(2+)
Cu(2+)
NH4
Cr(3+)
Sonorous
shiny 🔦
acidic oxides
covalent compounds
Add dilute NAOH(aq) + 🔥
NH3 gas released
Add dilute NAOH(aq)
A pale-green precipitate forms
Add dilute NAOH(aq)
Reactivity series
Red-brown precipitate forms
C
Zn
Al
Fe
Mg
H
Ca
Cu
Na
Ag
K
Add dilute NAOH(aq)
White precipitate + DISSOLVES in excess NH4OH
Au
Add dilute NAOH(aq)
White precipitate + NOT DISSOLVES in excess NH4OH
Rusting of iron
Add dilute NAOH(aq)
White precipitate + NO EFFECT when excess NAOH added
Metals above this line carbon cant reduce their oxides
Add dilute NAOH(aq)
Pale blue precipitate forms
Metals above this line they displace H from acis
Add dilute NAOH(aq)
Green precipitate forms
Rusting requires O and H2O
Halogens
React with AgNO3
Yellow precipitate = I-
White precipitate = Cl-
4Fe (s) + 3O2 (g) + 4H2O (l) -> 2Fe2O3.2H2O
React with BaNO3
White precipitate
Sulfite ions
Ways to prevent rusting
Add to acidified KMNO4
Solution turns colourless
Grease
Plastic
Paint
NO3(-)
Coasting with zinc is galvanising
Add small dilute NAOH(aq)
Sacrificial protection
Add aluminium foil
When a metal sacrifices another is called sacrificial protection. The metal should be more reactive
NH3 gas released
CO3(2-)
Add HCl
Releases CO2
Cream precipitate = Br-
Gases
NH3
CO2
Hold damp red litmus
Litmus paper turns blue
Bubble the gas through Ca(OH)2(aq)
Limewater turns milky
Cl2
Hold damp litmus paper
Litmus paper turns white
O2
Collect gas in test tube + hold glowing splint
Splint lights in fire
SO2
Hold damp KMnO4 paper
Turns white