unit viii atoms and the periodic table lesson#2 electronic structure/configuration
TRANSCRIPT
VIII.1 THE STRUCTURE OF THE ATOM
F. The Electronic Structure of the Atom
Energy Level Diagrams:
ENERGY LEVEL: is a specific amount of energy which an electron in an atom can possess (n)
QUANTUM: the energy difference between two particular energy levels
VIII.1 THE STRUCTURE OF THE ATOM
ORBITAL: is the actual region of space occupied by an electron in a particular energy level
SHELL: is the set of ALL orbitals having the same n-value
SUBSHELL: is a set of orbitals of the same type
VIII.1 THE STRUCTURE OF THE ATOM
Four Different Types of Oribitals:1. s-type: 1 s-orbital2. p-type: 3 p-orbitals3. d-type: 5 d-orbitals4. f-type: 7 f-orbitals
* each orbital contains only 2 electrons
The Five 3d orbitals chime d-orbitals more
VIII.1 THE STRUCTURE OF THE ATOM
Electron Configurations:
Definition: a description of which orbitals in an atom contain electrons and how many electrons are in each orbital
VIII.1 THE STRUCTURE OF THE ATOM
TWO RULES when adding electrons to orbitals:1.As atomic number increases, electrons are added to orbitals with lower energy first
2.A maximum of 2 electrons can be placed in each orbital
ENERGY LEVELS (N)
n=1 contains only s
n=2 contains s, p
n=3 contains s,p,d
n=4 contains s,p,d,f
n> 4 also contain s,p,d,f
Remember…
Four Different Types of Oribitals:1. s-type: 1 s-orbital max of 2. p-type: 3 p-orbitals max of3. d-type: 5 d-orbitals max of4. f-type: 7 f-orbitals max of
* each orbital contains only 2 electrons
How to write electronic configuration
H: 1 electron, goes to lowest energy level, n=1
N: 7 electrons
VIII.1 THE STRUCTURE OF THE ATOM
Core Notation:
CORE of an ATOM – is the set of electrons with the configuration of the nearest noble gas (He, Ne, Ar, Kr etc...)
OUTER electrons – consist of all electrons outside of the core
*core electrons usually don’t take part in chemical reactions
VIII.1 THE STRUCTURE OF THE ATOM
Ex: Predict the electron configuration of the following ions, using CORE NOTATION
Rb:
Ge:
Ni:
Fe:
*Ar:
VIII.1 THE STRUCTURE OF THE ATOM
If the d-shell is one electron short of being filled or half-filled, one electron from the s-shell comes over to fill it…makes it more stable
Cr ([Ar] 4s2 3d4) d4 – not stable
Cr ([Ar] 4s13d5) d5 – much more stable
Cu([Ar] 4s2 3d9) d9 – not stableCu([Ar] 4s13d10) d10 – stable
VIII.1 THE STRUCTURE OF THE ATOM
Electron Configuration for IONS:
Negative Ions: ADD electrons to the last unfilled subshell
Positive Ions: REMOVE electrons from outermost shell (largest n-value) first, if electrons are in p and s, remove from p first!
Core Vs Valence Electrons
Core Electrons usually don’t take part in chemical reactions
Valence Electrons: electrons which can take part in chemical reactions *all electrons in an atom except those in CORE or filled d and f shells
Core Vs Valence Electrons
Ex: How many valence electrons do the following contain?
B
Li
Is there a trend??? You betcha!
Number of column/group = number of valence electrons!
Cs
Core Vs Valence Electrons
Try: How many valence electrons are in?
Number of column/group = number of valence electrons!
Po
Sb+3
O2-
Br-
HOMEWORK
Electronic structure of atom
Hebden p. 155 # 26 a,c,d,f,g,k p. 156 #27 ( for any 4 of your choice) p. 157 # 28 choose 2 positive ions and 2
negative ions. p. 158 #29 (a i )
The quarks are permanently confined by forces coming from the exchange of "gluons." He and others later constructed …quantum chromodynamics," which seems to account for all the nuclear particles and their strong interactions." ...
In 1969, Professor Murray Gell-Mann received the Nobel Prize in physics for his work on the theory of elementary particles …he found that all of those particles, including the neutron and proton, are composed of fundamental building blocks that he named "quarks."