Atomic Structure and Atomic Bonding Flashcards
the imitation of the models,
systems, and elements of nature for the purpose of solving
complex human problems.
Biomimetics or biomimicry
according to him Matter consist of indivisible atoms, Atoms are arrange in different combination to make different compounds
Daltons Model
He proposed that if you
split atom in half, you will
find tiny electrons stuck
inside on it. (Plum pudding model)
Joseph John Thomson
according to him Atoms have nucleus,
All positive charge of atom
are all concentrated at the
center (nuclear
model)
Ernest Rutherford,
Electrons are not distributed as on his theory. Instead it is on an
orbit like a planet revolving around the sun. The electrons are revolving
around the nucleus (Bohr model)
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.(Quantum Mechanical model or cloud model)
Erwin Schrodinger
Discover that nucleus have
neutrons (Quantum Mechanical model or cloud model with
neutrons)
Quantum Mechanical model
or cloud model with neutrons
number of protons in the nucleus
atomic number (Z)
sum of the masses of protons and neutrons (N) within the nucleus
atomic mass (A)
how protons and electrons balance out
Net charge
elements have two or more different atomic masses
Isotopes
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. Connect metals and non- metals (Gave away electrons of steal electrons from other atom)
Ionic bonding
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 proportional to the square of the separation distance between the two objects.
Coulomb’s Law Equation
stable electron configurations are assumed by the sharing
of electrons between adjacent atoms. (No stealing of electrons, only sharing)
Covalent bond
