Chapter 2 Flashcards
periodic law
chemical and physical properties of elements are dependent on atomic numbers
group
column, same valence and chemical properties in groups
valence electrons
have highest PE and held less tightly
metals
left, middle
shiny, high MP, density, malleable, ductle
Low effective nuclear charge, low EN, IW, low electron affinity
large atomic radius, small ionic radius, good conductor
non metals
upper right, brittle
high IE, high electron affinity, high EN
small atomic radii, large ionic radii
metalloids
semi- metals
B, Si, Ge, As, Sb, Te, Po, At
Periodic table trends horizontal
Zeff, IE, EN, affinity increase left to right
atomic radius increases right to left
periodic table trends vertical
shielding and atomic radius increase top to bottom (more shells)
IE, EN, and affinity increase bottom to top
effective nuclear charge
Zeff
net positive charge experienced by outermost electrons
principal quantum number
increased by 1 down a groups (has more shells)
more separate leads to decrease in electrostatic attraction between electrons and nucleus
shield cancels the positive charge from nucleus so that Zeff is constant within a group
atomic radius
1/2 distance between center of 2 atoms
add electrons to outer, while inner electrons remain same
add protons for stronger pull
ionic radii
depends on ionization
gain electrons makes it larger
ionization energy
energy to remove electrons, is endothermic
large Zeff is small radius, tight, hard to remove
active metals
have low IE
includes 1A and 2A
in ionic compounds
electron affinity
energy released when gaining electrons
higher Zeff pull means higher delta H
