Periodic Table Flashcards
What are Group B elements?
The transitions elements including the inner transition
Metals
Found on left side and in middle of periodic table
Active transition and LA series
Lustrous except mercury (a liquid in standard conditions)
USUALLY high mp and densities
Malleable
Ductile
Low effective nuclear charge
Low electroneg
Large atomic radius
Low ionic radius
Low ionization energy
Low electron affinity
Good conductors
Transition have two or more oxidation states
Nonmetals
Upper right side of periodic table
Brittle
Lusterless
High ionization energies
High EA
High electroneg
Small atomic radii
Large ionic radii
Poor conductors
Metalloid
Stairstep elements (ignore Al)
In between ass traits
Zeff
Effective nuclear charge
A measure of the net positive charge experienced by the outermost electrons
Same period, Zeff inc left to right
Atomic radius
increase toward bottom left
Ionic radii
Assumptions: metals lose electron pos, nonmetal gain electron neg, metalloid depend on side
Nonmetals close to metalloid line possess a larger ionic radius
Metals close to metalloid line possess a smaller ionic radius
Removing an electron is a ____ process
endothermic
Ionization energy
Inc left to right, inc bottom to top
Which has greater ionization energy? Univalent cation formation or divalent cation formation?
Divalent
Active metals
Groups IA and IIA
low ionization energies
found as ionic compounds
Because IA ionization results in noble gas configurations, second ionization energies are crazy high
Electron affinity
Energy dissipated by a gaseous species when it gains an electron
Exothermic process
The stronger the electrostatic pull Zeff the greater the energy release when atom gains electron
Inc left to right, dec top to bottom
Noble gases have EA is 0 bc stable octet
Most metals have low EA
Electroneg
Closer to F, higher (top right)
First three noble gases have negligible electroneg
Inc top right
Electroneg, IE, EA
Dec top right
Atomic radius
Alkali metals
Group IA
density lower than other metals
Loosely bound electron
Zeff very low
Largest atomic radii in respective period
Low IE, EA, and electroneg
React readily with nonmetals esp halogens (NaCl)
Form strong base in water
Alkaline Earth Metals
Group IIA
Share most IA characteristics
Slightly high Zeff and slightly smaller atomic radii
Two electrons in valence shell and form divalent cations
Chalcogen
Group VIA or Group 16
Nonmetals and metalloids
Small atomic radii
Large ionic radii
Halogen
Group VIIA or Group 17
Highly reactive nonmetals
Desperate for an electron to complete octet
Highly reactive
Found in their ionic halide state as diatomic molecules
Noble gases
Group VIIIA or 18
Minimal reactivity
No measurable electroneg
Low bp exist as gas at room temp
Transition metals (B)
Group IB to VIIIB 3-12
Low EA, IE, electroneg
Hard
High mp and bp
Malleable, good conductors due to loosely held electrons that progressively fill the d-orbitals in their valence shells
Many have different oxidation states and thus make up a lot of ionic compounds
Can lose diff numbers of e from s- and d-orbitals
Complex ions often associate w water or nonmetals
variable solubility
Explain why transitions metal ion complexes have distinct colors
Because the ability to elevate electrons from a lower to higher energy d orbitals allow certain frequencies to be absorbed and others to be reflected
