Atoms Flashcards
Explain electrostatic attraction
Electrons are at different distances from the nucleus. The closer an electron is to the nucleus, the stronger the bond will be as there is more energy.
What are the different sublevel and what energy level do they start at?
Sublevel s starts at level 1, sublevel p starts at level 2, sublevel d starts at level 3, sublevel f starts at level 4
What are the maximum number of electrons for each sublevel?
s = 2, p = 6, d = 10, and f = 14
How many orbitals are in each sublevel?
s = 1 orbital, p = 3 orbitals, d = 5 orbitals, f = 7 orbitals
What are the three rules that dictate the filling order of electrons?
The Aufbau priciple, the Pauli exclusion, and Hund’s rule
Explain each principle for the filling of electrons
Aufbau principle states that electrons enter the orbital of the lowest energy first, Pauli exclusion states that an atomic orbital can only obtain 2 electrons at most, Hund’s rule states that all upwards pointing arrows must be entered before the downwards pointing arrows
What are the two exceptions to the Aufbau principle and why?
Chromium and copper. Because all their boxes need to have at least one electron in an orbital in order to be stable
How do neutral atoms become a noble gas?
By gaining or losing electrons
For a nuclear symbol of an element, on the left side, what goes on top and what goes on the bottom?
Mass number (neutrons + protons/total number of particles in the middle) on top and atomic number (protons) on bottom
How is a charge determined?
By the ratio of protons to electrons
Explain atomic and ionic radius
Atomic is the orginal size of the atom (not when it is an ion). Ionic is smaller than the atomic radius when the ion is positive and larger than the atomic radius when the ion is negative.
