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Topic 2 - Atomic Structure - Coggle Diagram
Topic 2 - Atomic Structure
2.2A Electron configuration & Atomic Orbitals
Every atom has 2,8,8,8 and so on
Atoms has different energy levels, and within the energy levels are
electron orbitals
.
Orbitals named
s, p, d, f
, each orbital can hold 2 electrons
Each orbital has a specific number of "instances" || s=1, p=3, d=5, f=7
Therefore, s can hold 2, p can hold 6, d can hold 10, f can hold 14
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 4f
S orbital = Spherical in shape and can hold a maximum of 2
p orbital= Barbell in shape and 3 shapes
d orbital= 5 shapes
f orbital= 7 shapes
Electron configuration principles
Aufbau principle
: Electrons enter the lowest energy level first
Hund's Rule
: Electrons enter each orbital singly, one at a time, with the same spin, then double up with opposite spin.
Pauli Exclusion rule
: An orbital can only hold 2 electrons.
Exceptions
to the rules
Chromium: Electron configuration is 3d^5 4s^1 not 3d^4 4s^2
Copper: 3d^10 4s^1 not 3d^9 4s^2
ALL transition metals
lose electrons from the 4s orbital
before 3d orbital
Ions
Ions lose or gain electrons from the highest energy level to have a full outer energy level
2.2B The electromagnetic spectrum
The
shorter
the wavelength, the
higher
the energy and frequency.
The
longer
the wavelength, the
lower
the energy and frequency.
Visible light can be observed by the naked eye at wavelengths 400 - 700 nm.
Violet light has the
highest
energy and frequency, hence shorter wavelength.
Infrared light has the
lowest
energy and frequency, hence longer wavelength.
Continuous Spectrum
2.1 - Atomic Structure
Atomic number (Z) = Number of protons || Mass number (A) = Number of protons + neutrons
Electron
Location: Outside of nucleus
Mass: 1 / 1836
Charge: -1
Neutron
Charge: 0
Mass: -1
Location: Nucleus
Proton
Location: Nucleus
Mass: -1
Charge: +1
Isotopes
are (1) atoms of an element with the
same amount of protons
but
different amount of neutrons
, (2) have
same chemical properties
but
different physical properties
, (3) same Z (number of protons)
Radioactive isotopes have unstable nuclei which dissipates excess energy by spontaneously emitting radiation (ionising radiation).
Used for medicine: (1) Cobalt-60: Radiation therapy to prevent cancer, (2) Carbon-14: Carbon dating of organisms and substances (Archeology)