U1: Topic 2 Atomic orbitals Electronic configurations & periodic table

Question 1

The lowest enegry level is giving what quantum number?

Answer 1

n=1

Question 2

What does each line on the emission spectra show?

Answer 2

Energy released when an electron moves between two energy levels.

Question 3

What suggests that energy levels are divided into subshells?

Answer 3

Lines on emission spectra often made up of multiple lines.

Question 4

What subshells make up each quantum number?

Answer 4

N=1 - s
N=2 - s,p
N=3 - s,p,d
N=4 - s,p,d,f

Question 5

What is the maximum electrons for each subshell?

Answer 5

S - 2
P - 6
D - 10
F - 14

Question 6

How are electrons considered to behave?

Answer 6

Both as particles and waves.

Question 7

If an electron is treated as a wave the movement of the electron around the nucleus can be described how?

Answer 7

Mathematically

Question 8

What are standing waves?

Answer 8

Waves that vibrate in time but do not move in space.

Question 9

What is it possible to do with standing waves?

Answer 9

Produce a picture to create a region around the nucleus where it is most likely that the electron will be found.

Question 10

Descirbe S orbitals.

Answer 10

Spherical. Size and energy increases as principal quantum number increases.

Question 11

Describe P orbitals.

Answer 11

Double-lobed. 3 possible orientations in space. These degenerate orbitals lie at right angles to each other one along the all axis’s. Size and energy increase as principal quantum number increases.

Question 12

Describe the D orbitals.

Answer 12

5 different orientations. 4 are similar 4lobed shape. all degenerate.

Question 13

Describe F orbitals.

Answer 13

7 orientations all degenerate and complex shape.

Question 14

What is the Aufbau Principle?

Answer 14

Orbitals filled in order of increasing energy.

Question 15

What is filled first 3d or 4s and why?

Answer 15

4S is filled first because it has a lower energy than 3D.

Question 16

What is Hund’s rule?

Answer 16

when degenerate orbitals are available, electrons will fill each singly with parallel spins before pairing occurs.

Question 17

What is Pauli exclusion principle?

Answer 17

no two electrons can have the same set of four quantum numbers.

Question 18

What 2 ways can you represent electronic configuration?

Answer 18

Orbital box notation
Spectroscopic notation

Question 19

What is the principal quantum number?

Answer 19

Indicates the main energy level for an electron. (N) Related to size of orbital. bigger the number further away from the nucleus and more energy.

Question 20

What is the Angular momentum number?

Answer 20

Indicates the shape the orbital resides in.
S - 0
P - 1
D - 2
F - £

Question 21

What is the magnetic quantum number?

Answer 21

indicates the orientation of the orbital.

Question 22

What is the spin magnetic quantum number?

Answer 22

Indicates direction of the spin can be either -1/2 or +1/2. Orbital containing 2 electrons must have one + and one -.

Question 23

What order are the quantum numbers set out?

Answer 23

N, L, Ml, Ms

Question 24

What is ionisation energy?

Answer 24

energy required to remove one mole of electrons from one mole of atoms in the gaseous state.

Question 25

There is a general trend of what across a period?

Answer 25

Increasing ionisation energy however it is not a smooth increase.

Question 26

Ionisation energy provides evidence for the existence of what?

Answer 26

subshells which can be explained by using relative stability of certain electronic configurations.

Question 27

The more stable the electronic configuration the what?

Answer 27

Higher the ionisation energy.