🤯Electron Configuration Flashcards
What is a molecule? What is matter?
A molecules is two or more atoms bonded together
Matter is all substances made up of atoms. It is anything that has a mass and takes up space.
Define an element
A bunch of the same molecules bonded together
Define and state the differences between compounds and mixtures
Compounds are two or more of different elements chemically bonded together, whilst mixtures are two or more of different elements not chemically bonded.
What is a synonym for main energy level?
Shell
True or false; do all electrons have the same energy? Why?
No, as shells are divided into sub levels, aka sub shells, that have different energies.
True or false; different shells have different energies.
True, as lower energies are closer to the nucleus and are harder to remove, vice versa for high energy.
What is an orbital?
It is the region around the nucleus that can hold up to two electrons with opposite spins.
What is the maximum each sub level can hold in terms of orbitals and total electrons?
Sub level s: can hold 1 orbital, 2 electrons
Sub level p: can hold 3 orbitals, 6 electrons
Sub level d: can hold 5 orbitals, 10 electrons
Sub level f: can hold 7 orbitals, 14 electrons
What is the maximum each main energy level can hold in terms of total electrons and sub levels?
Main energy level 1: can hold s sub level and max of 2 electrons
Main energy level 2: can hold s and p sub levels, and hold up to 8 electrons
Main energy level 3: can hold s, p and d sub levels and hold up to 18 electrons
Main energy level 4: can hold s, p, d and f sub levels, and hold up to 32 electrons
1s2; what is it and what does 1, s and 2 represent?
1= main energy level
s= sub level
2= electrons
Represents Helium
What is the shape of each sub level of you were to view it under a microscope? What about the electrons themselves?
S= spherical
P= dumb bell
D= can vary
F= can vary
Electrons= a cloud of negative charge
True or false;
Do orbitals with the lowest energy fill first?
True, as they require the least amount of energy
Why do electrons in the p, d and f sub level behave differently?
Electrons want to minimise the chance of collisions due to the opposite spins, so by each electrons going into different orbitals they lessen the chance of collisions. Hence why between the 4s2 comes first rather than 3d10, as it fills up first.
E.g/ 3d10 (Zinc)
(Where a= up arrow and b= down arrow)
ab ab ababab ab ababab ab
(1s2 2s2 2p6 3s2 3p6 4s2 3d10)
Which groups/ elements are in each sub level block?
Hydrogen, helium and all of group 1 and 2 are apart of the s sub level block.
Groups 3 to 0/8 are all apart of the p sub level block.
The transition metals are all apart of the d sub level block.
And the f sub level block are apart of all the elements left/ separated from the main periodic table.
How do you do the shorthand method for writing electron configuration?
Look at the row above the element you’re writing and look at the group 0/8 element on that row, put the element in square brackets and continue the electron configuration from there.
