par ROJAN REZAEETAZANGI Il y a 1 année
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Law of conservation of mass (Lavoisier)
In chemical reactions, no mass is lost or gained.
The pure substance that will dissolve the solute.
The pure substance being dissolved
Solubility
The measurement of how well a solute will dissolve in a solvent at a given pressure and temperature
ability of a solute to dissolve
Insoluble
Percipitate
a solid formed in a chemical reaction
Soluble
Single
When a free element replaces with a less active element that is in a chemical compound. (based on reactivity charts of metals and non-metals)
Double
Double displacement will not happen unless either water or a precipitate is being formed.
To predict if the double displacement reaction can occur or not we should use solubility rules chart.
Solubility rules
This type of reaction happens when an acid and a base combine to form water and salt.
When two or more reactants combine and form a new product
When a fuel (especially hydrocarbons) burns with oxygen to form carbon dioxide and water.
When one reactant breaks to form multiple products
Percent Yield=Actual Yield/Theoretical Yield x 100%
Stock solution
V
C
1 Mole=6.02 x 10*23 things
We use this formula to switch back and forth between different units and muasurments
L
Kg
Most acid and bases are colourless and clear it's hard to distinguish them so it's better to use indicators
HCL + H2O = H3O + CL
Chlorine gas ( The conjugate base)
Hydronium (The conjugate Acid)
Water (The Bronsted Lowry base)
hydrochloric acid (The Bronsted Lowry acid)
It contains hydrogen and a polyatomic that has hydrogen.
''ic'' acids
Nitric acid(HN3)
''Ous''acids
Nitrous acid(HNO2)
contains a hydrogen and another nonmetal
hydrochloric acid (HCl)
Solubility of CH4 in water
Solubility curves shows the maximum amount of solute that can be dissolved in a given amount of water over a range of temperatures.
Reading solubility curves
Super Saturated
Above the line
Saturated
Directly at the line
Unsaturated
Below the line
Tendency of an atom to attract shared pair of electrons within a molecular bond.
Electronegativity of elements
How easy it is for an atom to gain electron. Easier to gain= higher electron affinity
How easily a non-metal would become an anion.
How easily a metal would become a cation.
The distance from nucleus to the outermost shell.
compound lewis structure
Cation
Anion
Average weight
Atomic theory
Jemes Chadwick model
Bohr model
Rutherford and Nuclear model
Thomson model
Dalton model
Greek model
Electron
Neutron
Proton
bond polarity(Intramolecular forces)
This type of force is within the molecules(strong)
The type of bond will be determined by the difference in electronegativity of two atoms.
Ionic
Transfer of electrons
Molecular
sharing electrons
Intermolecular forces(molecule polarity)
This type of forces is between the molecules(weak)
Hydrogen bonding
A special type of dipole-dipole which occurs between hydrogen and either oxygen, nitrogen and fluorine. This intermolecular has a strong attraction because of big difference in electronegativities.
Dipole-Dipole
This intermolecular force forms between a slightly negative end of one Polar molecule and a slightly positive end of a neighbouring molecule causing them to pull towards each other
London dispersion
Electrons are always moving, sometimes they bunch up on one side of an atom, causing them to be slightly negative.
If this happens to a neighbouring molecule at the same time there would be a temporary attraction called London dispersion.
Polarity
Non-polar
Polar
Vsper shape
Vsepr shape allows us to predict the individual molecule structure and it's polarity based on the number of electron pairs that surround the center atom.
Valence shell electron pair repulsion theory
