Atomic Structure Review

Outside nucleus in electron cloud 3 Parts of the Atom: Subatomic Particle Relative Mass Charge Where Found Proton 1 +1 In Nucleus Neutron 0(neutral) Electron -1 Outside nucleus in electron cloud

How many electrons can each energy level hold? 1st—2 2nd—8 3rd—18 4th –32

Match the Diagram with the Name Dalton Bohr Rutherford Thomson

Properties of the Atom

Atomic Number Chemical Symbol Element Average Atomic Mass

Atomic # # of protons in an atom In a neutral Atom, # of protons=# of electrons Atomic # of a given element will never change, therefore, the # of protons of an element will never change.

Mass Number EX) Oxygen Avg. Atomic Mass = 15.999 Sum of the protons and neutrons Closest whole # to the Avg. Atomic Mass(from periodic table) WHY? EX) Oxygen Avg. Atomic Mass = 15.999 Therefore, Mass # = 16

Average Atomic Mass Mass of atom in Atomic Mass Units Given on periodic table as average mass of all isotopes of that element.(we’ll discuss isotopes) The number of neutrons sometimes varies!!! Atomic Mass Unit—defined as 1/12 the mass of a Carbon-12 atom

What is the atomic # of Potassium? 39.10 39 19 20

What is the Average Atomic Mass of Magnesium? 12 24.31 24 12.31

What is the Mass # of Magnesium? 12 24.31 24 12.31

How many protons are found in Potassium? 19 20 39 21

Isotopes Atoms of the same element with the same # of protons, but different # of neutrons.

2 ways of writing Isotopes H-1 H-2 H-3 Each of these represents Hydrogen The number represents the mass # Each of these represents Carbon The top # represents the mass # The bottom # represents the Atomic #

Isotopes of Carbon

A neutron walked into a bar and asked how much for a drink A neutron walked into a bar and  asked how much for a drink.  The bartender replied,  "for you, no charge." 

Ions Ions Ions Ions Ions Ions

Ions + ions 2. - ions Atoms become (+) by losing electrons A “charged” atom. Atoms become charged by gaining or losing electrons. 2 Types of Ions: + ions Atoms become (+) by losing electrons 2. - ions Atoms become (-) by gaining electrons

Determine the Atomic # and Mass # Atomic # = # protons Using the Periodic Table to determine the # protons, # electrons, and # of neutrons: Determine the Atomic # and Mass # Atomic # = # protons # protons = # electrons Mass # = # neutrons + # protons

# p = 6 # e = 6 # n = 6 A # = 6 M # = 12 Atomic # Atomic Mass M # = # p + # n 12 = 6 + #n A # = 6 M # = 12

# p = 11 # e = 11 # n = 12 A # = 11 M # = 23 Atomic # Atomic Mass M # = # p + # n 23 = 11 + #n A # = 11 M # = 23

# p = 19 # e = 19 # n = 20 A # = 19 M # = 39 Atomic # Atomic Mass M # = # p + # n 39 = 19 + #n A # = 19 M # = 39

# p = 27 # e = 27 # n = 32 A # = 27 M # = 59 Atomic # Atomic Mass M # = # p + # n 59 = 27 + #n A # = 27 M # = 59

Element Atomic # Mass # # of Protons # of Neutrons # of Electrons Phosphorus 15 31 16 Carbon 6 13 7 Helium 2 4 Beryllium 10 Iodine 53 126 73 Argon 18 40 22 Fluorine 9 19