1In the current atomic model, how do electrons move around the nucleus?
Electrons move in fixed energy levels called shells or energy levels.
2What is the principal quantum number?
A number assigned to each shell; the further from the nucleus, the higher the principal quantum number.
3Why don't all electrons in a shell have the same energy?
Shells are divided into sub-shells with slightly different energies.
4How many electrons can each orbital hold?
Each orbital can hold up to 2 electrons.
5In which direction do electrons in the same orbital spin?
They spin in opposite directions.
6What is the rule for filling electron sub-shells?
Electrons fill the lowest energy sub-shells first.
7How do electrons fill orbitals within a sub-shell?
Electrons fill orbitals singly before pairing up.
8How do you configure ions in the s and p blocks?
Add or remove electrons from the highest energy occupied sub-shell.
9How is the electron configuration of Mg written?
1s²2s²2p⁶3s²
10What is the electron configuration of Mg²⁺?
1s²2s²2p⁶
11What unusual behavior do chromium and copper exhibit?
They donate one 4s electron to the 3d sub-shell for stability.
12What is the electron configuration of a chromium atom?
1s²2s²2p⁶3s²3p⁶3d⁵4s¹
13What is the electron configuration of a copper atom?
1s²2s²2p⁶3s²3p⁶3d¹⁰4s¹
14When transition metals become ions, which electrons are lost first?
The 4s electrons are lost before the 3d electrons.
15What is special about the s block elements (Group 1 and 2)?
They have 1 or 2 outer electrons and easily lose them to form positive ions.
16What type of ions do elements in groups 5, 6, and 7 typically form?
They gain electrons to form negative ions with an inert gas configuration.
17Why are Group 0 elements inert?
They have completely filled s and p sub-shells, so they don't need to gain, lose, or share electrons.
18How do d block elements (transition metals) form ions?
They tend to lose their s and d electrons to form positive ions.