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4TH QUARTER SCIENCE
Electronic Structure
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According to
Democritus
, the world is made up of tiny indivisible particles called
atomos.
In 1803,
John Dalton
proposed the
solid sphere
of an atom.
In 1897,
Joseph John Thomson
(
JJ Thomson
) discovered the
electron
and made the
plum pudding
model.
In 1911,
Ernest Rutherford
discovered the
nucles
and proposed the
nuclear
model.
In 1913,
Niels Bohr
discovered
orbits.
Orbits
are also known as
energy levels
(
n
).
Ground state
is the original orbit of the
electron
Excited
state is the
highest
atomic orbit.
In 1924,
Louis de Broglie
made the quantum mechanical model and developed the
wave-particle
duality.
S <
2
P <
6
D <
10
F <
14
Principal
Quantum Number (
n
)
Refers to the
distance
of the electrons from the nucleus
Known as the
shell
Computed by
2n^2.
Azimuthal
Quantum Number (
l)
Refers to the
shape
of the atomic orbit.
Computed by
n - 1.
Magnetic
Quantum Number (
ml
)
The number of orbitals in a subshell.
The values are from
-l
to
+l.
Electron Spin
Quantum Number (
ms
)
Indicates the
spin
of the electron.
-1/2
(
counterclockwise
) or
+1/2
only (
clockwise
).
Electron Configuration
- shows how the
electrons
are
distributed
in an atom.
Aufbau
Principle
Must be filled from the
lowest
energy to the
highest
energy level.
Hund's
Rule
Must be filled
singly
before being
paired.
Pauli's Exclusion
Principle
No 2 electrons can
have the same set
of
quantum
numbers.
Chemical Bond
- is the
force of attraction
that
holds 2 atoms
together.
Chemistry
is the study of
matter.
Law of
Conservation of Mass
Proposed by
Antoine Lavoisier.
States that
matter
is neither
created
nor
destroyed
Law of
Definite Composition
/Proportions
Proposed by
Joseph Proust
A
compound
is made up of the same
proportions
of each
element.
Law of
Multiple Proportions
Proposed by
John Dalton
When
2 elements
combine to form
two or more
compounds.
Lewis Electron Dot Symbol
A method to represent
valence electrons
of
elements.
Noble Gases
The most
stable
atoms
Doesn't form
chemical bonds
with other atoms.
Octet Rule
States that an element must
lose
,
gain
, or
share 8 electrons
in its
valence shell
during
chemical bonding.