electrons, energy level and atomic orbitals Flashcards
what is the principle quantum number including what is used to represent it
the principal quantum number is the energy levels/shells represented by “n”
what are subshells?
sublevels which makeup the energy level
what are the subshells available?
s, p, d and f
what is the energy level number equal to?
eg; n=2
the number of subshells
eg; n=2
subshell = s and p
what are the subshells found for energy levels 1 to 4
n=1 (s)
n=2 (s, p)
n=3 (s, p, d)
n=4 (s, p, d, f)
what is each shell made up of?
subshells
what are orbitals
“compartments” with a maximum of 2 electrons found in subshells
how many orbitals do each subshell contain?
subshell s = 1 orbital
subshell p = 3 orbitals
subshell d = 5 orbitals
subshell f =7 orbitals
explain how orbitals are represented by
orbitals are represented by a box with maximum of 2 arrows which are the opposite to show that each electron in the orbital travel the opposite direction
what is ground state?
the most stable arrangement of an atom
in what order is the electronic configuration made in?
increasing energy
what is the pattern of the electronic configuration and how is it made?
1s 2s 2p 3s 3p 4s 3d 4p 5s….
made by arranging the subshells in each shell e.g.
4s 4p 4d 4f and then making a horizontal line passing through subshell s
explain the electronic configuration in terms of energy level of the electrons
the further away a shell is from the nucleus, the higher the energy( general statement) and so it is arranged in order of increasing energy level
explain the electronic configuration in terms of inter-electron repulsion
* include the important rules of electronic configuration
electrons close to an another will repel due to having the same negative charge. To prevent much repulsion, a)
in each subshell, each orbital is filled up with an electron in the same direction first.
b)Once there are no empty orbitals, the electrons are paired up but the second pair of electron is in the opposite direction. This is all to minimize the repulsion.
describe the notation used in full electronic configuration using 3p^5 as an example
3- stands for the shell number
p- the type of subshell
5- the number of total electrons in the subshell
describe the short hand electronic configuration
to make the electronic configuration shorter, other elements with the same electron number can be be used to represent a part of the electronic configuration
e.g. for chlorine
full electronic configuration
= 1s2 2s2 2p6 3s2 3p5
shorthand configuration
-neon has the electron number 10 which can be represented by a part of chlorines configuration
=1s2 2s2 2p6
neon can be used to represent the first 10 electrons instead such as:
[Ne] 3s2 3p5
how many orbitals can be found?
each type of subshell has its own specific orbital
describe the s orbital
the s orbital has a spherical shape where the nucleus is found in its center
how does the s orbital change as the principal quantum number increases?
as n increases, the size of the s orbital also increases
how many types of p orbitals are they including their names
3
px orbital along the x-axis
pz orbital along the z-axis
py orbital along the y-axis
determine position of the x, y and z axis
x- horizontal
y-vertical
z-bottom left to top right
describe the p orbital
the p orbital is made up of 2 lobes making up a dumbbell like shape and 3 different orientations of the p orbitals can be found
what is a free radicle?
an atom or molecule with one or more unpaired electron in their outer orbit
is oxygen a free radicle if yes/no, explain
no, oxygen has the configuration of 2,6 where each electron is paired into 2,2,2,2,2 which makes up a total of 8 electrons
