Electronic Configuration, Periodicity, and the Periodic Table

Flashcards about electronic configuration of elements, periodicity, and the periodic table based on lecture notes.

What is Chemistry?

The study of structure, synthesis, reactivity, and properties of matter.

What determines the physio-chemical properties of matter?

Nature and properties of the constituent atoms.

What historical experiments and theories have established our understanding of the atom?

Dalton's atom, discharge tube experiment, thermonic and photoelectronic emissions, isotopy, radioactivity, Rutherford's experiment, Millikan oil drop experiment, atomic spectra, Bohr's atom, particle-wave duality, Schrodinger wave equation, quantum numbers, electronic configurations.

What is the order of increasing energies of orbitals in a polyelectronic system?

1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d

What principles govern the filling of electrons in elements?

Aufbau Principle, Hund's Rule, and Pauli Exclusion Principle.

What does the electronic configurations of elements contribute significantly to?

The arrangement of elements in the periodic table.

How do s, p, d, and f orbitals differ?

They have different shapes and proximity to the nucleus.

Which orbitals have a greater probability of being nearer the nucleus?

s-orbitals

How does the penetrating effect alter the stability of orbitals with higher quantum numbers?

ns orbitals are more stable than (n-1)d orbitals, and ns, (n-1)s, and (n-1)p orbitals are more stable than (n-2)f orbitals.

What observation led to the periodic law?

Elements were observed to have varying degrees of reactivity leading to periodic sequences in their properties.

With the existence of atoms and their atomic weights/masses and valencies, what did scientists attempt to do?

Scientists attempted to classify elements based on these properties.