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CHM 101
Atomic structure
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Electron shells
are regions where
electrons
can be found, with different
energies
associated with them.
Subshells
have
specific shapes
that
determine
how
many orbitals
they
contain.
When an atom gains or
loses
electrons, it becomes
charged.
Orbitals
are the
actual
paths followed by
electrons
around the
nucleus.
The fourth electron shell has
four
subshells (s, p, d, f) and can hold up to
thirty-two
electrons per subshell.
The third electron shell has
three
subshells (s, p, d) and can hold
up
to
eighteen
electrons per subshell.
The
first
electron shell has
one
s subshell and can hold up to
two
electrons.
The second electron shell
has two subshells
(s,
p
) and can hold up to
eight electrons per subshell.
Ionic compounds consist of
positively charged metal cations
and
negatively charged nonmetal anions
held together by
electrostatic attraction.
Covalent bonds
form when atoms
share pairs
of
electrons
to complete their
outermost energy levels.
Electron configurations
show where all the electrons go in an atom's
energy levels.
Ionization energy
is the amount of
energy
required to remove an
electron
from an
atom.
Metallic bonding
occurs due to the sharing of
valence
electrons among all the
positive
ions in a
metallic lattice.
Atoms with full
valence
shells are
stable
and do not readily react
chemically.
Valence electrons
are those that participate in chemical reactions.
Hydrogen
is
unique
because it forms both
ionic
and
covalent
bonds depending on its
chemical environment.
Metals are
good
conductors of
heat
and
electricity
due to the
delocalized
nature of their
valence
electrons.
Atoms with
low
ionization energies are more likely to
lose
electrons than
gain
them.
Nonmetals have
high ionization energies
because it takes a lot of
energy
to pull off their
valence electrons.
Metals have
low ionization energies
because they easily give away electrons to become
positive
ions.
Elements
are
abbreviated
in
scientific shorthand.
All symbols on the
periodic table
are
short
or
abbreviated
ways to write the
name
of an
element.
Some symbols on the
periodic table
are from the
element’s name
(H, He, B, Be, I, F, Br, etc.).
Some symbols on the periodic table are from the old
Greek
or
Latin
name (
silver
is Ag for
Argentum
).
Some elements on the
periodic table
are named after some
scientists
(Es for Einsteinium, Lr for
Lawrencium
).
An
atom
is the
smallest piece
of
matter
that still has the
properties
of the
element.
Atoms
are made up of
subatomic
particles:
protons
,
neutrons
and
electrons.
Protons
are located in the
nucleus
of
atoms
and have an
electric charge
of
+1.
Neutrons
are located in the
nucleus
of
atoms
and do not have an
electric charge
, making them
electrically neutral.
Electrons
are located in
electron clouds
, called
orbitals
, and have an electric charge of
-1.
The number of
protons
in the
nucleus
of an atom is its
atomic number
, which identifies which
element
you have.
The number of
neutrons
plus
protons
in an atom is its
mass number.
In an atom, the number of
protons equals
the number of
electrons.
Atoms that have
lost
or
gained
electrons are called
ions.
The
atomic weight
or
atomic mass
is the
average
of the
mass numbers
of all of the
isotopes
of an
element.
Isotopes are
atoms
of the same
elements
that have
different
numbers of
neutrons.
Electrons
occupy a certain
energy level
(of a certain size) and once the
energy level
is
full
, a new
level
begins.
Examples of isotopes include
Oxygen-18
and
Oxygen-16.
In writing electronic configuration, three rules/principles are followed namely;
Aufbau
principle,
Hund’s
rule and
Pauli exclusion
principle.
Average atomic mass
is closest to its most
abundant isotope.
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