Atomic Structure and Atomic Bonding Flashcards
It is the imitation of the models,
systems, and elements of nature for the purpose of solving
complex human problems.[1] The terms “biomimetics” and
“biomimicry” derive from Ancient Greek: βίος (bios), life, and
μίμησις (mīmēsis), imitation, from μιμεῖσθαι (mīmeisthai), to
imitate, from μῖμος (mimos), actor. A closely related field
is bionics.
Biomimetics or biomimicry
WHY STUDY Atomic Structure and Interatomic Bonding?
the type of bond allows us to explain
a material’s properties
is a poor conductor of electricity
diamond
is a good conductor of electricity
graphite
consists of a very small
nucleus composed of protons and
neutrons and is encircled by
moving electrons
atom
number of protons in the nucleus
atomic number (Z)
sum of the masses of protons and neutrons (N)
within the nucleus
atomic mass (A)
Both electrons and protons
are electrically charged, the
charge magnitude being
1.602 × 10^-19 𝐶
how protons and electrons balance out
Net charge
elements have two or more different atomic masses
Isotopes
may be used to compute atomic weight.
atomic mass unit (amu)
defined as 1/12 of the atomic mass of the most common
isotope of carbon
1 amu
1 amu/atom (or molecule) =
1 g/mol
Dictate the number of state within each subshell of Bohrs energy
level which is separated into electron subshells
Quantum Numbers
may take
on integral values beginning with unity
Principal quantum number n
designates
the subshell or sublevel
The second (or azimuthal)
quantum number,
l
The number of electron
orbitals for each subshell is
determined by the
third (or
magnetic) quantum number, mL
are those that occupy the outermost shell. These electrons are extremely
important; as will be seen, they participate in the bonding between atoms to form atomic and
molecular aggregates. Furthermore, many of the physical and chemical properties of solids are
based on these
valence electrons
How two isolated atoms interact as they are brought close together from an infinite
separation
Bonding Forces and Energies
the sum of both attractive and
repulsive components;
net force FN
net force FN formula
FN = FA + FR
where;
FA = attractive force
FR = repulsive force
rO is approximately
0.3 nm = 0.000,000,003
meters
he established that matter is consist of indivisible atoms. toms are arrange in different combination
to make different compounds
Dalton’s model
Atom are not indivisible, he
discovered that atom have electrons
which is much smaller than atom
He proposed that if you
split atom in half, you will
find tiny electrons stuck
inside on it.
The positive and negative
charge are distributed
Sir Joseph John Thomson
Atoms have nucleus
All positive charge of atom
are all concentrated at the
center.
nuclear model 911
He was a New Zealand physicist who
came to be known as the father of
nuclear physics
Ernest Rutherford, 1st Baron Rutherford
of Nelson
Bohr model 1913
Electrons are not
distributed as Rutherford
theory. Instead it is on an
orbit like a planet
revolving around the sun.
The electrons are revolving
around the nucleus
He was a Danish physicist who made
foundational contributions to understanding atomic structure and quantum theory, for which he rece
Niels Henrik David Bohr
Electron is no longer
treated as
a particle moving in a
discrete orbital; rather,
position is considered to be
the probability
of an electron’s being at
various locations around
the nucleus. In other
words, position is
described by a probability
distribution or electron
cloud.
Quantum Mechanical model or cloud model
(1920’s)
He established Quantum Mechanical model or cloud model
(1920’s)
Erwin Schrodinger or Erwin Schroedinger
Discover that nucleus have
neutrons. (Quantum Mechanical model
or cloud model with
neutrons (1932’s))
He was an
English physicist who was awarded the 1935 Nobel Prize in
Physics for his discovery of the neutron in 1932.
Sir James Chadwick
electrically neutral
neutrons
how protons and electrons balance out
net change
When ___ and ___ are equal in magnitude but opposite in sign, there is no net force
Fa and Fr
Three different types of primary or chemical bond are
found in solids
ionic bond, covalent bond, metallic bond
always found in compounds composed of both metallic
and non-metallic elements, elements situated at the horizontal
extremities of the periodic table.
ionic bonding
Hard, brittle, electrically
and thermally insulative
ceramic materials
states that the electrical force between two charged objects is directly
proportional to the product of the quantity of charge on the objects and inversely
Coulomb’s Law
Is found in materials whose atoms have small differences in electronegativity—that is, that
lie near one another in the periodic table
Covalent Bonding
Gave away electrons of steal electrons from other atom
ionic bond
No stealing of electrons, only sharing
covalent bond
No stealing of electrons, only sharing
covalent bond
Why atoms bond?
Octet Rule – Atoms are trying to fill their “valence” shell.
Want to attained noble gas configuration
soft, flexible, low electric
conductivity, low boiling and melting point
polymer materials
is a molecule consisting of two atoms held by
covalent bond
diatomic molecule
is a molecule consisting of two atoms held by
covalent bond
diatomic molecule
The final primary bonding type, is found in metals and their alloys
The attraction between metal ions and delocalized electrons
A bond found in metals; holds metal atoms together very strongly
metallic bonding
is a material’s
ability to deform under compressive stress; this is often
characterized by the material’s ability to form a thin sheet by
hammering or rolling.
malleability
