Unit 1 Notes PDF

Unit 1 notes Week 1 and 2 [Relate number & location of subatomic particles to atomic number, mass number, charge, and element symbol] 3 subatomic particles, location, mass, and charge Location Mass Charge abbreviation ---------- ---------- --------- -------- -------------...

Unit 1 notes Week 1 and 2 [Relate number & location of subatomic particles to atomic number, mass number, charge, and element symbol] 3 subatomic particles, location, mass, and charge Location Mass Charge abbreviation ---------- ---------- --------- -------- -------------- Proton Nucleus \~1 amu 1+ p^+^ Neutron Nucleus \~1 amu 0 n^0^ Electron Orbits \~0 amu 1- e^-^ Atomic number = number of protons - - Mass number = protons + neutrons - - Charge = protons - electrons - - - - Term: Isotopes - atoms of the same element with different numbers of neutrons (and therefore different mass numbers) Average atomic mass - - To calculate average atomic mass - - - - - - - Week 3 and 4 - - - - - The energy of light is inversely related to its wavelength - longer wavelengths (red end of spectrum) have lower energy. Shorter wavelength (violet end of spectrum) have higher energy Electrons are arranged into 7 energy levels. Each energy level is composed of one or more sublevels (s, p, d, or f). Each sublevel is composed of one or more orbitals. Each orbital can hold up to two electrons (spin up or spin down). Electrons always occupy the lowest energy position available. Energy level Sub-levels present Sublevel Orbitals Electrons -------------- -------------------- -- ---------- ---------- ----------- 1 s s 1 2 2 s p p 3 6 3 s p d d 5 10 4 s p d f f 7 14 5 s p d f 6 s p d f 7 s p d f To Write the electron configuration of an element, each sublevel is noted with a number for the energy level, an letter for the sublevel, and a superscript for the number of electrons in the sublevel. For example "1s^2^" would indicate the 1st energy level, s sublevel, containing 2 electrons. The electron configuration for F would be indicated as "1s^2^2s^2^2p^5^" An abbreviated notation can be used by indicating the noble gas of the previous row in brackets, and then the electrons that come afterwards. Fe would be "\[Ar\] 4s^2^3d^10^" The orbital notation includes boxes to represent each orbital, and arrows to represent the spin of each electron. Additional rules apply: Hund's rule indicates that when filling sublevels with multiple orbitals, electrons will not pair up within an orbital until each orbital has one electron with spins in the same direction. The Pauli Exclusion principle states that electrons within the same orbital must have opposite spins. Thus, the orbital notation for C would be