Atomic theory ect. Part 2

Question 0

Absorption

Answer 0

When energy is absorbed by an atom, electrons jump up to higher and larger orbits

Question 1

Niels Bohr

Answer 1

• Rutherford’s student
• made modifications to his atom model
• his model explained line spectra (connected Balmer’s math. relationship with Rutherford’s planetary model)
• proposed electrons orbit around the nucleus in circular paths of specific sizes
• each orbit has an energy level associated with it
  2,8,8,18
• by combining Balmer’s equation with Planck’s equation - he calculated the energy dif. between orbits and the wavelength/frequency of light given off during fluorescence
• his diagram explains emission line spectrum of HYDROGEN

Question 2

Emission/ fluorescence

Answer 2

These electrons can drop back down to lower orbits and in doing so they release energy in the form of light

Question 3

Further experiments by Thomson and others using CRT’s discovered..

Answer 3

Proton

Question 4

Sir James Chadwick discovered

Answer 4

neutron

Question 5

Natural abundance

Answer 5

The amount of an isotope in a pure sample of the element expressed as a %

Question 6

How do we get the natural abundances?

Answer 6

Mass spectrometer

Question 7

Orbits

Answer 7

Two dimensional path around the nucleus in a Bohr’s diagram

Question 8

Orbitals

Answer 8

Volumes of space
Can hold max 2 electrons
Almost all are overlapping and can share the Same space

Question 9

S orbitals

Answer 9

Round and spherical

Question 10

P orbitals

Answer 10

Two lobes down the Same axis

ALWAYS IN SET OF 3

Question 11

D orbitals

Answer 11

ALWAYS COME IN SET OF 5

Question 12

F orbitals

Answer 12

ALWAYS COME IN SETS OF 7

Question 13

Exceptions

Answer 13

Cr. …4s1 3d5

Cu. …4s1 3d10

Question 14

Electronic configuration

Answer 14

Description of the orbitals that are occupied by electrons in an atom or ion

Question 15

Aufbau principle

Answer 15

Orbitals are filled one at a time starting with the lowest energy levels first. The lowest available energy orbital must be full before advancing to the next one

Question 16

Pauli exclusion principle

Answer 16

No two electrons can be exactly the same in each orbital. Therefore if one orbital has 2 electrons, one must be spin up and the other must be spin down

Question 17

Hund’s rule

Answer 17

When dealing with degenerate (the same energy level) orbitals, full each orbital with one electron first before pairing up

Question 18

Isoelectric

Answer 18

Two chemical species that have the same electronic configuration

Question 19

Means: The same energy level

Answer 19

Degenerate

Question 20

What is used to observe a line spectrum?

Answer 20

Spectrometer

Question 21

Emission line spectrum

Answer 21

The collection of the different colours of light that an element/substance emits

Question 22

Isotopes

Answer 22

Atoms of the Same element with different masses due to a different number of neutrons

Question 23

Ground state

Answer 23

State in which the electrons are in the lowest energy orbitals

Question 24

Exited state

Answer 24

State in which the electrons are not in the lowest energy orbital