Inorganic Chemistry 2 - Atomic Orbitals, Electronic Configurations and the Periodic Table Flashcards
Electrons (like photons) display the properties of both ___ and ___.
particles and waves
What is an atomic orbital?
An area within an atom with a high chance (>90%) of containing an electron/electrons
Orbitals can hold a maximum of ___ electrons.
two
What are the four types of orbitals?
s, p, d and f
Electrons within atoms have fixed amounts of energy called ___.
quanta
Each electron has ___ numbers that describe it.
What are they?
4 (n, l, ml, ms)
No two electrons in one atom can have the ___ four numbers.
same
n is called the…
What does n tell us?
n is somewhat related to the type of ___ containing the electron.
principle quantum number.
the energy level that the electron is on.
orbital
What is the lowest value of n which can have a d orbital?
3
L is called the…
L is always a value between _ and _.
What does L tell us?
angular momentum quantum number.
0 and n-1.
the type of orbital the electron is in
Name the orbital represented by the following values of L.
3
1
2
0
f,
p,
d,
s
ml is called the…
What does ml tell us?
ml is always a value between…
magnetic quantum number.
the orientation of the orbital.
-l and +l
If l=0, how many orbitals and which type is it?
If l=1, how many orbitals and which type is it?
If l=2, how many orbitals and which type is it?
If l=3, how many orbitals and which type is it?
one, s.
three, p.
five, d.
7, f
ms is called the…
What does ms tell us?
Name the possible values for ms.
How are these values represented?
spin magnetic quantum number.
the direction of spin of the electron.
+1/2, -1/2.
half arrows, pointing up or down
What is a subshell?
What is an electron shell?
a bunch of degenerate orbitals of one type. (eg the 2p subshell is three p orbitals, the 3d subshell is five degenerate d orbitals, each with a different orientation, given by ml)
an electron shell is all of the subshells on an energy level (eg the 3rd level, n=3, has a 3s subshell, a 3p subshell, and a 3d subshell).
State the Aufbau Principle.
electrons fill orbitals in order of increasing energy
What is Hund’s Rule?
when degenerate orbitals are available, electrons fill singly, keeping their spins parallel until the subshell is half full, when pairing starts
State the Pauli Exclusion Principle.
No two electrons in the same atom can have the same 4 quantum numbers (therefore orbitals can only hold 2 and they must have opposite spins)
Name the following methods of representing electrons within atoms.
1s2, 2s2, 2p6, 3s2, 3p6, 3d7, 4s2.
The one with arrows in boxes.
[Ar] 3d2, 4s2
spectroscopic notation,
orbital box notation,
shortened spectroscopic notation (rounded down to the nearest noble gas + the remaining electrons)
The periodic table is divided into _ blocks, corresponding to the ___ ___ ___ of the elements within these blocks.
4, outer electron configuration
The anomalous elements on graphs of first (and subsequent) ionisation energies can be explained by the relative ___ of different ___ configurations.
stabilities, electron
When are subshells most stable?
when they are half full or completely full
When explaining that half full/completely full subshells are more stable, state the specific ___ when possible.
subshell (eg in Nitrogen it’s 2p)
When an atom has a stable electron arrangement, its ionisation energy is ___.
higher
An example of an element with an ‘anomalous’ first ionisation energy is nitrogen, as it has a higher ionisation energy than oxygen, despite…
Nitrogen’s electron configuration is 2, 5.
This means it has a ___ full p subshell, which is ___ stable than oxygen’s p subshell.
Higher atomic number .
half, more
VSEPR theory can be used to predict what?
What does VSEPR stand for?
the shape of molecules and polyatomic ions.
Valence Shell Electron Pair Repulsion
Arrange the following electron pairs in order of increasing strength.
Bonding : Bonding
Non-Bonding : Non-Bonding
Bonding : Non-Bonding
Weakest
Bonding : Bonding
Non-Bonding : Bonding
Non-Bonding : Non-Bonding
Strongest
How do you find the number of electron pairs surrounding a central atom?
*There are four steps :)
- Take the atom’s valence number/group number/number of outer electrons
- Add one for every -ve charge and subtract one for every +ve charge
- Add one for every bond (or bonding atom assuming they’re single bonds)
- Divide by 2!
Electron pairs are _vely charged, and ___ each other.
-vely, repel
Electron pairs are arranged to maximise ___ and minimise ___.
separation, repulsion
Name the shape that the following number of electron pairs will take around a central atom, and state the angle(s) between them.
Two
Three
Four
Five
Six
Two: linear (180 degrees)
Three: Trigonal Planar (120 degrees)
Four: Tetrahedral (109.5 degrees)
Five: Trigonal Bipyramidal (90 and 120 degrees)
Six: Octahedral (90 degrees)
If all electron pairs are bonding, the bond angle will be (the same/different), compared to if all electron pairs are non-bonding.
the same.
If some electron pairs in an atom are bonding, and others are non-bonding, the bond angles may ___ slightly.
change (eg a tetrahedral electron pair arrangement with one non bonding pair will have a 107 degree bond angle, instead of its typical 109.5)
Non bonding electron pairs have a ___ repulsion force than bonding pairs.
stronger
An increase in the number of (bonding/non-bonding) electron pairs causes the bond angle to decrease.
Non-bonding (stronger repulsion force)
By how many degrees do bond angles decrease with each extra pair of non-bonding electrons?
2.5
