CHM 115 Principal Energy Levels

Exam 2 Prep

0, 1, 2, 3

What is the Angular Momentum of each orbital type in this order: s-orbital, p-orbital, d-orbital, f-orbital

0

What is the magnetic quantum number of s-orbitals?

-1, 0, +1

What is the magnetic quantum number of p-orbitals?

-2, -1, 0, +1, +2

What is the magnetic quantum number of d-orbitals?

-3, -2, -1, 0, +1, +2, +3

What is the magnetic quantum number of the f-orbitals?

1, 3, 5, 7

What are the umber of orbitals in each sublevel in this order: s-orbitals, p-orbitals, d-orbitals, f-orbitals

1, 4, 9, 16

What is the number of orbitals in energy level in this order: 1, 2, 3, 4

Nodes

A specific point in an atom's orbital where there is a zero probability of finding electrons

Same Energy And Agree With Bohr Theory

Bohr theory: Energies of atom orbitals are degenerate (For a 1-electron atom or ion) =

No And Splitting of energy levels is observed

For a multi-electron atom or ion: anything with more electrons than one, can Bohr theory predict these energies and what is observed?

n And increases And Overlap

In general, for atoms containing more than one electron, energies of sublevels increase as _ increases and as l _______. In addition, as n increases, some sublevels _____.

Stable And Nucleus

2s is lower in energy than 2p because: The 2s sublevel is more _______ than the 2p because it penetrates closer to the ______.

1, 3, 5, 7

How many orbitals are in each sublevel in this order: s-orbital, p-orbital, d-orbital, f-orbital

2, 6, 10, 14

How many electrons are in each sublevel in this order: s-orbital, p-orbital, d-orbital, f-orbital

Partial Orbital Diagram

Shows only the highest energy sublevels being filled

[Ne]3s²3p^1

What is the partial orbital diagram of Al?

[Ar](4s^1)3d^5

What is the partial orbital diagram or condensed electron configuration of Cr?

[Ar](4s^1)3d^10

What is the partial orbital diagram or condensed electron configuration of Cu?

Inner Core Electrons

Those the atom has in common with the previous noble gas

Outer Electrons

Those in the highest energy level( highest n and furthest from nucleus)

Valence Electrons

Those involved in forming bonds

outer electrons

Main group - valence =

outer + x # of d electrons

Transition Metals - valence =