Atomic Structure and Periodic Table 1.3.1 (+ 1.3.2)

Describe how an emission line spectrum is produced

Describe how an emission line spectrum is produced

e- in ground state, right amount of energy as heat or electricity, jumps to higher level, excited state is unstable, drops to lower energy level, energy absorbed to make jump released as photon, frequency depends on difference in energy levels. E2-E1 = hf, E2 = excited state, E1 = ground state, h is Planks constant, f is frequency of light

Who unlocked the secret line of spectra?

Bohr

What is an energy level?

Shell which electrons of equal energy can occupy

Which energy level do electrons fall into to produce visible light?

N=2

What is the series of lines called when in n=2?

Balmer series

Give two ways to excite electrons.

High temperature, high voltage electricity

What is a sub-level?

Sub-divisions of a main energy level, consisting of one or more orbitals of the same energy

What is an orbital?

Region around nucleus in which there is high probability of finding an electron

State Heisenberg’s Uncertainty Principle

The more accurately we determine the position of an electron at any instant the less accurately we can determine its velocity

What is wave-particulate duality?

When you observe an electron it behaves like a particle, when you don’t observe an electron, it behaves like a wave

S orbital

Spherical, holds up to 2 electrons

P orbital

Dumb-bell shaped, sublevel made up of 3 orbitals; Px, Py, Pz, holds up to 6 electrons

D orbital

Made up of five orbitals, holds up to 10 electrons

F orbital

7 orbitals, holds up to 14 electrons

Aufau principle

Electrons occupy the lowest available energy level, fill sub levels from the nucleus outwards

Positive And Negative ions

Atoms that take in electrons form negative ions, for each electron taken in they gain a positive charge, atoms that give away electrons form positive ions, for each electron lost they gain a positive charge

Has 13 electrons so Al+3 has 10 electrons, how is it written?

[1s2, 2s2, 2p6]3+

Hund’s Rule ( of maximum multiplicity )

When two or more orbitals of equal energy are available the electrons occupy them singly and then in pairs

Pauli Exclusion Principle

Arrows in boxes show how electrons are distributed in orbitals, box represents orbitals and arrows represent electrons, no mare than two electrons may occupy an orbital and to do so they must have opposite spin