2. •Syllabus presentation
•Introduction to assessment system
•General overview of the subject
Lecture 1 hr
The electronic structure of Atoms; The dual nature of the electron;
Quantum mechanical description of the hydrogen atom; quantum
numbers; Atomic orbitals; Electron configuration; The shielding
effect in many-electron atoms.
Seminar1hr: The principal quantum number; The angular
momentum quantum number; The magnetic quantum number; The
electron spin quantum number;
s-,p-,d-,f- orbitals; The energies of orbitals; The Pauli exclusive
principle; Hund’s rule
3. Medical chemistry
1. General Chemistry the essential concepts Raymond chang, Jason Overby. USA-New
York.2011
2.Klein D. - Organic chemistry Student study guide and solutions manual. John Wiley &
Sons, Inc 2012.
4.
5. What is Medical Chemistry?
The electronic structure of Atoms;
The dual nature of the electron;
Quantum mechanical description of the hydrogen atom;
Quantum numbers;
Atomic orbitals;
Electron configuration;
The shielding effect in many-electron atoms.
6. The Study of Chemistry
• chemistry is the study of matter and the
changes it undergoes;
• Matter is anything that occupies space and
has mass
• All matter is composed of discrete, tiny
particles called atoms.
7. Atoms, Elements, Compounds, and Ions
• Atom
• basic building block of all matter
• Element
•Substance that consists of only one type of atom.
•Molecule has two different atoms.
• Compound
• substance that consists of more than one type of element.
• Ion
• substance that has a positive or negative charge
8. Atoms have:
• A nucleus
• small, heavy part of the atom
•An electron cloud
• large, lightweight part of the atom
Nucleus Electron Cloud
9. Nucleus of an Atom
• Nucleus contains:
N
• Protons
• Have a positive charge
• All atoms are distinguished by
the number of protons it
has (atomic number)
• Neutrons
• Have no charge
• Have same mass as
protons
N
N
10. e-
e-
Electron Cloud of an Atom
An electron cloud contains:
• Electrons
• determine bonding properties of
substance
• have a very small mass compared to
protons and neutrons
• orbit the nucleus of the atom
• are contained within shells of the
electron cloud
• have a negative charge
11.
12. The symbols, relative mass and
the charge of subatomic particles
Subatomic
particle
Symbol Relative
mass
Charge
Proton p 1 +1
Electron e -1
Neutron n 1 0
1840
1
13.
14.
15.
16. Isotopes
Atoms of the same element always have the same number of
protons. However they may have different numbers of
neutrons. There are known as isotopes. Carbon has two
isotopes:
C C
6
14
6
12
Write down the number of protons, neutrons and electrons
in the two isotopes of carbon
Carbon-12 Carbon-14
65. Bohr’s Model of the Atom
• Einstein’s theory of light’s dual nature
accounted for several unexplainable
phenomena, but it did not explain why
atomic emission spectra of elements were
discontinuous.
66. Bohr’s Model of the Atom
• In 1913, Niels Bohr, a Danish physicist working
in Rutherford’s laboratory, proposed a
quantum model for the hydrogen atom that
seemed to answer this question.
– This model correctly predicted the frequency lines
in hydrogen’s atomic emission spectrum.
67.
68. Bohr’s Model of the Atom
• The lowest allowable energy state of an atom
is called its ground state.
• When an atom gains energy, it is in an excited
state.
69. Bohr’s Model of the Atom
• Bohr suggested that an electron moves
around the nucleus only in certain allowed
circular orbits.
70. Bohr’s Model of the Atom
• Each orbit was given a number,
called the quantum number.
– Bohr orbits are like steps of a ladder,
each at a specific distance from the
nucleus and each at a specific energy.
71. Bohr’s Model of the Atom
• The electron releases energy as it falls back
towards the ground state.
72. Quantum Mechanical Model
• Louis de Broglie (1892–1987) hypothesized
that particles, including electrons, could also
have wavelike behaviors.
– Electrons do not behave like particles flying
through space.
• We cannot, in general, describe their exact paths.
73. Quantum Mechanical Model
• Heisenberg showed it is impossible to take any
measurement of an object without disturbing
it.
• The Heisenberg uncertainty principle states
that it is fundamentally impossible to know
precisely both the velocity and position of a
particle at the same time.
74.
75. Quantum Mechanical Model
• The only quantity that can be known is the
probability for an electron to occupy a certain
region around the nucleus.
76. Quantum Mechanical Model
• Schrödinger treated electrons as waves in a
model called the quantum mechanical model
of the atom.
– Schrödinger’s equation applied equally well to
elements other than hydrogen (unlike Bohr’s
model).
77. Quantum Mechanical Model
• The quantum mechanical model makes no
attempt to predict the path of an electron
around the nucleus.
– Bohr orbits were replaced with quantum-
mechanical orbitals.
78. Quantum Mechanical Model
• Orbitals are different from orbits in that
they represent probability maps that
show a statistical distribution of where
the electron is likely to be found.
