Page 6 - PRE-U STPM CHEMISTRY TERM 1

CHAPTER ELECTRONIC STRUCTURE
2 OF ATOMS

Concept Map

Electronic Structure of Atoms

Electromagnetic Line Spectrum Bohr’s Model of Modern Atomic Filling of
Radiation of Hydrogen Hydrogen Atom Model Electrons

Electronic Electronic Ionisation Energy Atomic
Configuration Configuration of Hydrogen Orbitals
of Ions • Ionisation energies
and electronic shells

L earning O utcomes
Learning Outcomes

Students should be able to: • define and apply Aufbau principle, Hund’s rule and
Electronic energy levels of atomic hydrogen Pauli exclusion principle.
• explain the formation of the emission line spectrum Classification of elements into s, p, d and f
of atomic hydrogen in the Lyman and Balmer series blocks in the Periodic Table
using Bohr’s Atomic Model. • identify the position of the elements in the Periodic
Atomic orbitals: s, p and d Table as 1
• deduce the number and relative energies of the s, p (a) block s, with valence shell configurations s and
s ,
2
and d orbitals for the principal quantum numbers 1,
2 and 3, including the 4s orbitals; (b) block p, with valence shell configurations from
s p to s p ,
2 1
2 6
• describe the shape of the s and p orbitals. (c) block d, with valence shell configurations from
1 2
10 2
Electronic configuration d s to d s ;
• predict the electronic configuration of atoms and ions • identify the position of elements in block f of the
given the proton number (and charge); Periodic Table.

02 Chapter 2.indd 36 3/26/18 3:14 PM