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Bohr's theory of an Atom
when an atom absorbs energy in the form of heat, light or electricity it often re emits that energy as light.
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Bohr's theory (model)
Orbit- is a circular path around the shell of the nucleus at definite distance (fixed energy) in which electron moves (revolves)
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Drawbacks of Bohr's Model
Not fully successful in explaining line spectrum (emission, spectrum) exhibited by (colors) different elements with different atomic number (number of electrons)
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Quantum Mechanical Theory (Wave theory)
Orbital- is a three dimensional space around the nucleus where the probability of locating an electron is maximum at one particular time
orbitals are represented by a number (1,2,3,4..) and a letter (s,p,d,f..)
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Electron Configuration
Distribution of electrons of an element into various orbitals of increasing enery
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orbit:
orbital:
shell
sub-shell
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Pauli's Exclusion Principle
A maximum of only two electrons with opposite spin can be accommodated into any given orbital
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Quantized orbital
orbitals with fixed definite amount of energy
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Degenerate orbital
orbitals with equal (same) amount of energy
2px,2py,2pz
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Hund's Rule
Degenerate orbitals (equal amount of energy) are singly full with parallel spin before they are paired up with opposite spin
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Orbital Diagram
Each orbiral is represented as a square box
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Group number
stands for the number of electrons in the outermost shell orbit.
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valence electrons
Electrons of the outermost shell
corresponds to group number of an element
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Period number
stands for the number of shells into which electrons are distributed
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Periodic Trend in properties of Elements in Period table.
Atomic size-----increases-------- decreases
Metallic character--- increases----- decreases
Nonmetallic-------- decreases----- increases
Ionization energy--- decrease------ increases
Electron negitivity---decreases----increases
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Metals tend to lose electrons and for positive ion (Na+, Mg2+, Al3+)
Bigger atoms can easily lose electrons to form cation (positive ion)
Non metals tend to gain electrons to form negative ions (F1-, O2-, N3-)
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Ionization energy
- is the energy required to remove electrons from neutral gaseous atom.
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- further from the nucleus
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What is the most reactive metal of the period table?
Fr-Francium (lower left side)
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What is the most reactive of NON metal of the periodic table
Fluorine (upper right corner)
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Compare the size
Na°+ Na1+
Cl° Cl1-
Fe2+ Fe3+
N O
Li Na
- Na°>Na1+
- Cl°>Cl1-
- Fe2+>Fe3+
- N>O
- Li<Na
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Electron Negativity
Less attractive
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