Electronic structure Flashcards
what did the bohr model say about electrons ?
that they are arranged in shells
how are these shells defined ?
by the principle qauntum number ,given the symbol ‘n’
what does the lowest energy shell have ?
n=1
the higher the n of an electron ……
the further from the nucleus it orbits
how do you find the max number of electrons in a shell?
2n^2
what is a sub level ?
all of the orbitals of the same type in the same shell
what happens with the sub levels for atoms with more than one electron ?
the shells are split into sub shells
what energy is a sub shell?
they are all slightly different energies
what does n mean in shells ?
the number of subshells
what are sub shells composed off ?
orbitals
how many electrons can orbitals hold ?
2
what do orbitals in the same subshell have ?
same energy
what is the requirement of 2 electrons existing in the same orbital?
one must have a up spin and one must have a down spin
are electrons particles ?
no they are negative charge clouds
what shape does the negative charge cloud take ?
whatever shape the orbital it occupies is
how certain can scientist be about where an electron exists ?
95%
what are the types of atomic orbitals?
s,p,d,f
describe the orbitals in electron shells ?
shell 1 : 1s orbital =2 electrons
shell 2 : 1 s ,3 p =8 electrons
shell 3 : 1 s , 3 p , 5 d = 18 electrons
shell 4+ : 1s,3p,5d ,7 f =32 electrons
orbitals of exactly the same energy are called …….
degenarate
explain subshell notation
Energy level , subshell and the number of electrons (electrons in the square place)
explain the arrows in boxes technique of showing electron configuration
Each box represents an orbital , each arrow represents one electron , the up and down arrows represent the electrons spinning in opposite directions , the energy level and subshell are written about the orbital diagram
Explain energy level diagrams in electron configuration
Shows the energy of the electron in diffrent orbitals and the number of electrons , their is an arrow for energy from lowest to highest up the paper
Name the three key rules of electron configuration?
Electrons fill up the lowest energy sub shells first (4s has allowed energy than 3d so 4s first )
electrons fill orbitals in a sub shells singly before they start sharing (because electrons with the same way of turning repell)
for the configuration of ions from the s and p blocks of the periodic table ,just add or remove the electrons to or from the highest energy occupied sub shell .
Elements with their outer electrons in an s sub shell are called s block elements,same goes for p block elements and the p orbital
How do u do noble gas config ?
Square brackets with element before then the following shells .
E.g.,calcium as [Ar]4s2
What is the annonmly in electron config if transition metals ?
Chromium and copper donate one of their 4s electron to their 3d sub shell due to them wanting a more stable full or half-full d sub shell .
when transition metals become ions they lose their 4s electrons before their 3d electrons .
what decides the chemical properties of an element ?
the number of outer shell electrons
explain the chemical properites of s block elements ?
1-2 electrons in the outer shell .(group 1/2) ,These are easily lost to form positive ions with an inert gas config .
explain the p block chemical properites ?
groups 5 ,6 ,7 .can gain 1,2 or three electrons to form negative ions with an inert gas config .
what groups 4-7 do when they form covalent bonds ?
they can share electrons
explain how electron configuration effects group 0 elements ?
they have completely filled s and p sub shells and don’t need to gain ,lose or share electrons .their full sub shells make them inert
