electronic structure

What are electrons shells made of

Subshells and orbitals

How are electrons arranged in the current accepted atomic model

They have fixed energies and move around the nucleus in certain regions of the atom called shells

What do you call the numbers given to label the shells

Principal quantum numbers

How does the larger the principal quantum number relate to the shell

The larger of the number the higher the energy level and the further it is from the nucleus

Experiments show that not all electrons in a shell have exactly the same energy how does the atomic model explain this

Shells are divided into subshells which have slightly different energies and different numbers of orbital which can hold up to two electrons which spin in opposite directions

What are the 4 subshells

S p d f

What are the two major roles to electron configuration

-Electrons fill the lowest energy subshell first

-electrons fill orbitals singly before they start sharing

Which sub shell is the exception to the 1st rule

4S subshells because even though it has a higher principal quantum number it has a lower energy level and so fills up before 3d

Which two transitional metals do not follow the first rule properly either

Chromium and copper

How do chromium and copper not follow the rule

They behave badly and donate one of their 4S electrons to the 3d subshell because they would rather have a more stable full or half full d subshell

How do transitional metals vary when we form ions

They lose their 4s electrons before their 3d electrons

What are the chemical properties of S block elements

1 or 2 outer shell electrons which are easily lost to form positive ions with an inert gas configuration

Chemical properties of p block elements

The gain 1, 2 or 3 electrons to form negative ions within an inert gas configuration

Chemical properties of group 0

Full sub shells making them inert

Chemical properties of d block

Lose electrons to form positive ions