chapter 4 exam Flashcards
how to write shorthand config
write as far into the periodic tbale as it goes. d= n-1
f=n-2
how to determine what subshells contain valence electrons
1st and last subshell of the sequence
how to find how many electrons in a shell
count how mnay electrons came before what was listed
atomic radius as you go across a period
decreases; because the effective nuclear charge increases across the period. This means valence electrons are drawn tighter to the nucleus, making the size of the atom smaller.
atomic radius as you go down a group
increases; the valence elctron of-in the -shell is farther from the nucleus, meaning their is more sheliding, making a larger atomic radius.
ionization energy going across a period
increases; effective nuclear charge increases, meaning electrons are pulled tighter towards the nucleus, meaning more energy is required to strip outside elctrons
ionization energy going down a group
decreases; valence electrons are in the- , meaning its farther from the nucleus and less energy is required to strip
electron affinity across a period
increases; it increases with effective nuclear charge, energy to atrract electrons increases
electron affinity down a group
decreases; electrons get farther from the nucleus because they are at higher energy levels.
how was mendelevs period table organizesd originally compared to today
he produced 63 elements, listed according to increasing atomic mass. He discovered groups
how did mosely reorganize the table
he changed it to increasing atomic number.
what is todays periodic table based on
periodic law
atomic radius
size of the atom
ionization energy
energy required to strip an electron from the outermost shell
electron affinty
the atoms ability to attract and maintain a new electron
