Periodicity
An atom with all its electrons as close to the nucleus as allowed.
What is in the ground state
An orbital can hold only two electrons and they must have opposite spin
Pauli Exclusion Principle
Emission of electrons when a light shines on metal
Photoelectric effect
Which has the higher electronegativity: S or As? Explain in terms of Coulomb's Law.
S. The "q" is larger for S because Zeff is larger, and the distance is shorter (because fewer shells)
Which in each pair has the biggest radius. Explain in terms of Zeff and shielding.
Ba vs. Ca
K vs. Ca
Ba - more shells so larger
K - same # shells [same shielding] but smaller # protons (so smaller Zeff --> smaller nuclear pull on electrons)
The noble gas configuration of tungsten.
What is [Xe] 6s2 4f14 5d4?
•Electrons occupy orbitals of lower energy first.
Aufbau Principle
Difference between electron cloud and Bohr models in their view of the electron
quantum = wave; Bohr = particle in fixed circular orbit
Group
The have the same outer (valence) shell electrons.
What is electronegativity? What element has the largest EN?
The ability of an atom to attract electrons to itself IN A BOND. Fluorine
The electron configuration of nitrogen.
What is 1s2 2s2 2p3?
Electrons fill a set of orbitals such that there are the maximum number of parallel spins
Hunds Rule
An orbital
region around the nucleus where electrons are likely to be found
A halogen in the 5th period
What is iodine?
The energy required to remove an electron from an atom AND its periodic trend.
What is ionization energy? Increases up and to the right.
The orbital notation for nitrogen
(draw this on board)
Color with the highest energy:
Orange, Green, Red, Violet, Yellow, Blue
What is violet
Produced a model of the atom with "energy levels" as electrons can only occupy certain energy levels.
Who is Bohr?
Block, period, group (number AND name), and common charge of Barium
s ; 6 ; 2 (alkaline earth) ; +2
the physical and chemical properties of elements are periodic functions of their atomic numbers
What is the periodic law
What each number and letter represent in the electron configuration 1s2
1 = energy level (period/principal quantum level)
s = sublevel (orbital shape)
2 = number of electrons in that orbital
Which is largest ? Explain why
O or O2-
O2- Same effective nuclear charge, so same force of attraction to nucleus, but greater e -e repulsion (more e's) so larger.
Heisenberg uncertainty principal
“One cannot simultaneously determine both the position and momentum of an electron.”
Group # and 3 properties of alkali metals
Group 1. EC = ns1. Form +1 cations. soft. React violently with water. Very reactive.