A1 Flashcards
(18 cards)
Development of Atomic Model (Order)
John Dalton, J.J Thompson, Ernest Rutherford, Neil’s Bohr
John Dalton
8 Ball Model (Atoms are solid spheres that are indivisible and indestructible; Same element= Same Size/Mass; Diff Element= Diff Size/Mass)
J.J Thompson
Plum Pudding Model (Used Cathode Ray Tube and discovered the existence of (e-); Atoms consist of (-) charged electrons embedded in spherical cloud of (+) charged
Ernest Rutherford
Rutherford Model (Used gold foil experiment to discover nucleus as alpha particles would deflect off something indicating that there was a small dense (+) charged nucleus; Discovered e- would orbit around nucleus)
Neil’s Bohr
Bohr Model- Conducted atomic line spectra experiments and discovered that electrons can jump between shells by absorbing or emitting electromagnetic radiation with a frequency determined by the difference in energy levels
Atomic Number
Quantity of protons (proton count determines identity of the element)
Relationship between e- and p+
P+=E- as ATOM is electrically neutral (Charged atom is an ION hence p+ DOES NOT = e-
Mass Number
Protons + neutrons
Isotopes
Atoms of the same element that have different numbers of neutrons
Atomic Mass
Average of the masses of different isotopes of the specific element based on abundance hence some atomic masses on the periodic table are not in whole numbers
Highest Energy Level
Furthest from nucleus
of Electrons in Each Shell
2,8,8
Period #
of Shells
Group #
of valence electrons
Most Reactive Groups
Alkali metals and halogens are very reactive as they are so close to a full octet so the will do anything to lose or gain a single electron to become stable
Cation
Gives away electrons hence losing negativity hence it is a + change (electrons less than protons)
Anion
Gains electrons hence gaining negativity hence it is a - charge (electrons greater than protons)
Distinguishing Anions from Cations
Anions change ending of name to end with “ide”
