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Chemistry - Coggle Diagram
Chemistry
Rates of reaction
Increase Temperature
Surface area
More area to react on
Increase rate of reaction
PH
Catalyst
Lower the activation of energy
Poison
Slow Down the reaction
Decreases temperature
PH
Decrease surface area
How to measure
Measure the mass
Measure the volume of gas released
Particle theory
Material properties
Structure of atoms
Protons
Positively charged
Neutrons
Neutral
Electrons
Negatively charged
mass number
Protons + Neutrons
Atomic number
No. of Protons
electronic configuration
2,8,8,18,32
Trends in the periodic table
Left side
Non - Metals
eg:- hydrogen, carbon, chlorine, and helium.
Right side
Metals
eg:- aluminum, copper, iron, gold, lead, silver, and zinc.
Other trends in the periodic table
Group 18
Do not react
Almost all are gases
MP increase ( -ve)
BP increase (-ve)
Group 1
They get softer as you go down the group
Reactivity increases
BP decreases
MP decreases
Group 17
They turn from gas to liquid to solid as we go down the group
reactivity decreases
BP decreases
MP increases
Periodic table
Groups
18
No. of electrons in the last shell
Periods
7
No.of shells
Covalent bond
Shares electrons
Ionic bond
Loose or gains electrons
Energy changes
Combustion reaction
Fire Triangle
Oxygen
Heat
Fuel
A substance when burned releases Large amount of energy
Exothermic in nature
Oxidation
Metal + Oxygen
Mg + O2 = Magnesium oxide
Removing of hydrogen
Loss of electrons
Addition of Oxygen
Releases energy
CH4+ 2 O2 → CO2+2 H2O
Exothermic reaction
Temperature increases
Releases Energy
Metals + Acid
Mg + HCL
Releases Hydrogen
Salt is formed
Metals + Water
K + H2O
Endothermic reaction
Temperature decreases
Energy absorbed
E.g. Melting of Ice
Substances
Combustible
Wood, Oil, Petrol
Non- Combustible
Metal, Glass, Cement
Salts
Making salt
Neutralization reaction
Acid + Base --> Salt + Water
Displacement reaction
Oxides + Acids
Acid + Metal -->Salt + Hydrogen
Zn + HCL ---> ZnCl2 + H2
Carbornates
We can use Carbonates to form other salts by reacting them with an acid
Sulfuric acid + Calcium carbonate ---> Calcium sulfate + H2O + CO2
Definition
Ionic compounds made of metal ion and a non metal ion
Reactivity
Reactivity series
K, Na, Ca, Mg, Al, C, Zn, Fe, Sn, Pb, H, Cu, Ag, Au
Least reactive
Most reactive
Displacement reaction
A more reactive metal kicks out the less reactive metal
eg:- Copper sulfate + Iron ---> Iron sulfate + Copper
Metal + Oxygen
Reactions
Displacement
chemical reaction in which a more reactive element displaces a less reactive element from its compound.
Fe+CuSO4→FeSO4+Cu
Thermite Reaction
Addition/ combination
an organic reaction where two or more molecules combine to form a larger one
MgO + CO2 → MgCO3
Decomposition
a chemical reaction in which one reactant breaks two from two or more products.
2FeSO4 → Fe2O3 (s) + SO2 + SO3
Neutralization
an acid and a base react to form water and a salt
NaOH→Na++OH−
Oxidation
Metal + Oxygen
Mg + O2 ---> Magnesium oxide
Basics of chemistry
Matter
States of matter
Liquid
Gas
Solid
Element
Metals
Metalloids
Non- Metals
Mixtures
Homogenous
Alloys
Heterogenous
Molecules
Compound
Bases
Metal oxides
Magnesium oxide
Zinc oxide
Lead oxide
Alkalis
Metal hydroxides
Sodium hydroxide
Potassium hydroxide
Iron Hydroxide
Metal carbonates
Calcium carbonate
Copper carbonate
Tin carbonate
Acids
Strong acids
HCL
H2SO4
HNO3
Weak acids
Carbonic acid
Always gives H+