Electronic Structure Flashcards
the energies of electrons is…
fixed
whats the principle quantum number
the shell number
what happens to energy and principle quantum number as the electron shells move further from the nucleus
energy increases and principle quantum number increases
name the sub shells
s, p, d and f shells
why do transition metals such as Chromium and Copper donate one of their 4s electrons to the 3d sub shell?
they are more stable
why do transition metals lose their 4s electrons before their 3d electrons when becoming ions
the 4s orbital has lower energy so it gets filled first
when the 3d orbital gets filled, the 4s is no longer lower in energy
so electrons are lost from 4s orbital first because it has the highest energy level (furthest from nucleus)
what decides the chemical properties of an element
the number of outer shell electrons
what groups does the s block include
groups 1 and 2
how do s block (group 1/2) elements outer shell electrons act
they lose 1/2 electrons easily to form positive ions with an inert gas configuration
what are the p block groups
groups 5, 6 and 7
how do p block (groups 5,6 and 7) elements outer shell electrons act
they gain 1, 2 or 3 electrons to form negative ions with an inert gas configuration
how do groups 4-7 act
share electrons to form covalent bonds
