Definition Flashcards
Molecular orbital
result form interaction of atomic orbital of bonding atom
isotope
atoms who have the same atomic number but different mass number
covalent bond
a chemical bond which involved the sharing of electron pairs between atoms
delocalized bond
electron density is spread unevenly over the whole of the atom, rather then be fixed on one position
double bond
a chemical bond between the chemical elecments involving 4 bonding electrons insteed of 2
boiling point
temp when vapour pressure equals external pressure
CRITIAL temp
the temp about which the gas cannot be made to liquify, no matter the pressure applied
critical pressure
the min require to be applied to bring about liqefraction at critical temp
emulsion
a mix in which the liquid contains are immiscible in nature hence causing emulsion
suspension
a mix in which a solute particle do not dissolve but get suspended throughout the bulk of the solvent
coagulation
physical reaction, the action of a liquid to change to a solid or a semi-solid state.
micelle
it is aggregate of surfacent molecules dispured in liquid colloid
solubility
the ability for a given substance to solute ( to dissolve in solvent)
oxidation
loss of e
reduction
gain of e
galvanic cell
a electrochemical cell that uses transfer of electrons in redox reactions to supply electric current
electromotive force
a difference in potential that tends to give an electical current
colligative properties
depends upon conc of solute molecules
electrolysis
unit of electic current being converted into chemical energy
Ionization energy
energy required to remove the most loosely held electron from one mole of gaseous atoms to produce one mole of gaseous ions each with a charge of 1+
Electron affinity
The amount to energy released when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion
First law of thermodynamics
In any change that occurs in nature, the total energy of the universe remains constant (a version of the law of conservation of energy). The energy may be converted from one form to another.
Second law of thermodynamics
The entropy of an isolated system never decreases, because isolated systems always decay toward thermodynamic equilibrium, a state with maximum entropy.
Third law of thermodynamics
The entropy of a perfect crystal, at absolute zero Kelvin, is exactly equal to zero.
Hess’s law
(of constant heat summation)
The enthalpy change of a reaction is the same, regardless if the pathway (whether it is completed in one step, or in several steps)
hunds rule
two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs
Aufbau principle
It states that as the electrons are added, they assume their most stable conditions (they fill the orbitals starting at the lowest possible energy levels (e.g. 1s before 2s).
Pauli Exclusion Principle
It is impossible for two electrons of a poly-electron atom to have the same values for the four quantum numbers
Henry’s law
The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid
Avogadro’s law
Equal volumes of all gases, at the same temperature and pressure, have the same number of molecules
The Lewis acids
Lewis acid: free electron pair acceptor
Lewis base
: free electron pair donor
proprotion
A pure compound always contains different elements, combines in the same proportions by mass
multiple proportions
If two or more compounds are composed of the same two elements, the ratio of the masses of one element that combine with a fixed mass of the other element is a simple whole number
Multidentate ligand
Ligands with more than one donor atom are capable of occupying more than one position of a metal ion to form cyclic complexes called chelates
coordination number
Number of ligands around the central ion in the coordination sphere
Boyle’s Law
At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure.
Charles’ Law
At constant pressure, temperature is directly proportional to volume ( gases expand when heated)
Gay-Lussac’s Law
At a constant volume, the pressure of an ideal gas is directly proportional to its temperature.
Arrhenius concept
Acid: produces H+ ions in water
Base: produces OH- ions in water
Brønsted-Lowry base
accept a proton from another molecule
Brønsted-Lowry acid
donated a proton to another molecules
