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Alkali Metals
Group 1 (G1)
Description of Alkali metals
Soft, less dense, high boiling and melting points; extremely reactive with water and air. Gray.
Alkaline Earth Metals
Group 2 (G2)
Halogen Groups
Group 17 (G17)
Description of Halogens
Most reactive, poisonous and have a strong smell
Nobel Gasses
Group 18 (G18)
Description of Nobel gasses
Very stable, no reaction
Most reactive groups?
G1 and G17
Newlands did what?
arranged by atomic mass, repeated every 8th element called Law of Octaves
Meyer did what?
arranged by atomic mass, repeated, but did not publish in time.
Mendeleev
Arranged by atomic mass, left blank spaces for elements but put them in the wrong spot, posted first
Mosely
increased order of atomic number
What is reactivity determined by?
Number of valance electrons
Representative elements?
S and P blocks
Transition metals?
D block
Description of transition metals?
high density, strong, high melting and boiling point, colorful, forms more than 1 charge
inter-transition metals?
F block
Metals description
group 1-12 (blue block) stretched and bent, solid at room temperature, makes heat and electricity
Metalloids description
shiny but brittle, gives electric currents in certain situations (the green block)
Nonmetals description
used for gasses, brittle, dull looking solids, gasses at room temperature, no electric current or heat
Atomic Radius?
Half way point from 2 adjacent atoms. MUST do diatomic atoms.
What is the trend of Atomic Radius?
As it goes down a group, it increases due to the addition of orbitals.
Down a period we decrease due to the attraction of the electrons to the protons, making the radius smaller.
Largest Element in the periodic table is
Fr
Trend of Ionic radius?
As it goes down a group it increases due to the number of orbitals also increasing. (Even though the last circle losses a orbital, the next one is still bigger) (Down a period, it gets smaller, then a jump, back to small.)
What is Cation?
When it has 1 more proton than electrons
What is Anion?
When it has 1 more electron than proton
Atomic Radius
Down a period it goes Big to small
How do you determine if an atom is bigger?
# of orbitals
# of protons
# of electrons
Ionization energy trends?
Down a group the bigger the atom gets causing less attraction and less energy
Down a period the smaller the atom gets the more attraction it has, more energy
Smallest Ionization atom?
He
Electronegativity trends?
Down a group the bigger the atom gets causing less attraction and less energy
Down a period the smaller the atom gets the more repulsion to each other, more energy
Highest electronegativity?
F
Octet rule?
Gains or loses electrons to have a filled orbital (8)
Ion?
Charged atom, gain or lose
What shape is S
Sphere
What shape is P
Dumbell
What shape is D
Clover
Electrons inside orbital diagram example
The arrows → ←
Orbital diagrams example
The Squares
Note 
Flashcard (63)