Atomic structure electronic configuration

Question 1

Energy level

Answer 1

The fixed quantity of energy an electron can have

Question 2

Sub level

Answer 2

A group of orbitals of the same energy

Question 3

Orbital

Answer 3

Region in space where there is a high probability of finding an electron

Question 4

Energy sub level

Answer 4

s, p, d, f

Question 5

Aufbau principles

Answer 5

Electrons fill orbitals of lowest energy first

Question 6

Hunds rule

Answer 6

Electrons fill orbitals of the same energy singly first and then in pairs. Singly filled orbitals of the same energy have all their electrons spin in the one directions

Question 7

Pauli (Exclusion) Principle

Answer 7

Each orbital holds at most two electrons. Electrons in the same orbital spin in opposite directions

Question 8

Most stable electronic configurations

Answer 8

Full energy level or full sub level

Question 9

Middle stable

Answer 9

Half full sub level

Question 10

Least stable

Answer 10

Having one electron away from most stable

Question 11

Niels Bohr statements about line emission spectrum in hydrogen
1st

Answer 11

Atoms begin with their electrons in ground state
Ground state means the electrons are in the lowest possible energy level

Question 12

Niels Bohr statements about line emission spectrum in hydrogen]
2nd

Answer 12

Energy in the form of heat is given to the electron, the electron is promoted to a higher (excited state) energy level

Question 13

Niels Bohr statements about line emission spectrum in hydrogen
3rd

Answer 13

The electron does not like being at a higher energy level so it falls back down to either the ground state or a lower excited state energy level. It loses its energy in the form of light

Question 14

Niels Bohr statements about line emission spectrum in hydrogen
4th

Answer 14

Bohr called the higher of the two energy levels E2 and the lower one E1. He said E2 - E1 = hf
Where h = Planck constant and f is the frequency of light. He found this formula matched the frequency given off

Question 15

Niels Bohr statements about line emission spectrum in hydrogen
5th

Answer 15

Due to the fact that he had lines of coloured light on a black background, he concluded that only certain energy levels were available and that these energy levels were fixed or quantised

Question 16

Schrodinger’s Theory

Answer 16

Described the position of the electron in a different manner so Bohr’s theory is not correct

Question 17

Heisenberg uncertanty principle

Answer 17

It is impossible to simultaneously know both the position and momentum of an electron, as in the process of measuring one we change the other

Question 18

The Lyman series

Answer 18

When electron drop to n=1, this is a very high energy difference, these high energy differences are in the UV region of the spectrum.

Question 19

Balmer series

Answer 19

Drops to n=2 are in the visible region

Question 20

Paschen series

Answer 20

Drops to n=3 (and higher) are in the Infrared region.

Question 21

Atomic emission spectroscopy

Answer 21

method of chemical analysis that uses the intensity of light emitted from a flame, plasma, arc, or spark at a particular wavelength to determine the quantity of an element in a sample

Question 22

Louis De Broglie

Answer 22

First proposed the concept of the dual wave, particulate nature of matter

Question 23

S orbitals

Answer 23

Spherical

Question 24

P orbitals

Answer 24

Dumbell