LT 1: Quantum numbers and electron configurations
This is the full electron configuration for boron
What is: 1s22s22p1
These are the two types of radiuses that allow us to measure atomic size, because we cannot simply take an atom's radius as if it were a circle
What is: van der Waals radius and Covalent radius
This is the difference between first ionization energy and the other ionization energies (second, third, etc.)
What is: how much energy is needed to remove the most loosely held electron from a mole of gaseous atoms, where 2nd = energy needed to remove the 2nd most loosely held electron, 3rd = 3rd most, etc.
This is what happens when a neutral atom becomes an anion.
What is: the atom gains an electron, making it's overall charge -1 (more negative than before)
This is an explanation for why Bohr's atomic model is inaccurate about atoms and where electrons are
OR
This is the full electron configuration for Galium
What is: electrons are not in fixed paths nor can they be exactly located, they are found in orbitals, which are cloud-like regions where they are likely to be found
OR
What is: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1
This is WHY we cannot simply take the radius of an atom as if it were a circle
What is: electrons are 1.) in orbitals, which are clouds of probability of where an electron can be, 2.) electrons can jump to different energy levels. mainly, they cannot be fully tracked.
This is one factor that affects ionization energy.
What is: (the answer depends!)
This is what happens when a neutral atom becomes a cation.
What is: the atom loses an electron, making its overall charge +1 (more positive than before)
These are the four quantum numbers
What is: principal quantum number, angular momentum quantum number, magnetic quantum number, and spin quantum number
As you go from top to bottom in the periodic table, this is how the size of the elements change
What is: they get bigger
These are the other 3 factors that determine ionization energy.
What is: (the answer depends!)
This is the difference between a monatomic ion and a polyatomic ion.
What is: monatomic = 1 atom, polyatomic = more than one atom (they can be the same element)
The quantum numbers of a random electron in a neutral atom of carbon are: n = 2, l = 1, m1 = -1, 0, 1, ms = + ½
This is the direction the electron is facing in the orbital.
What is: up
As you go from left to right in the periodic table, this is how the size of the elements change
What is: they get smaller
These are the members with the highest ionization energy in the entire periodic table.
Draw the bohr models for sodium and magnesium. This is the element out of the two whose ionization energy would dramatically increase if we were to take away 1 single electron.
Who is sodium?
The quantum numbers of a random electron in a neutral atom of iron are: n = 3, l = 2, m1 = -2, -1, 0, 1, 2 ms = - ½
This is the shape of iron's orbital.
What is: a double dumbbell
These are the two exceptions to the atomic size trends.
What is: noble gases are bigger than group 7 (halogens), and nitrogen is smaller than oxygen
This is the reason why helium has a higher ionization energy compared to hydrogen, even though helium has electrons which are paired as opposed to alone in the orbital
What is: since helium has 2 protons and hydrogen has 1 proton, even though the electrons are paired the bond between the electrons and protons are much stronger (because of that additional proton. remember: protons are MUCH heavier than electrons, so they are very powerful)
meow meow meow meow meow. did you ever think of that