Chapter 5 Flashcards
Order the following: shells, subshells and orbital services
Shells made of subshells
Subshells made of orbitals
How many electrons per orbital
2 paired electrons
How many orbitals in s subshell
1
How many orbitals in p subshell
3
How many orbitals in d subshell
5
Subshells in shell 1
Only s
Subshells in shell 2
S and p
Subshells in shell 3
S,p and d
Subshells in shell 4
S,p,d and f
Number of electrons per shell number
2,8,18,32
What does this mean:
3P subscript 6
Shell number 3
Orbital p
6 electrons in those orbitals
Shape of s orbital?
S orbital shape of higher shells?
Sphere
Higher shells are larger in volume but same shape
Why do higher shell orbitals have higher volume
Higher shell electrons have more energy so on average they are further away from the nucleus
What do the orbitals actually represent?
What are the chances of finding an electron in the orbital?
The area around a nucleus where there is a high chance of finding an electron
but they move randomly and we have no idea of the electron’s direction or speed so theoretically they can be anywhere in the universe
95%
Shape of p orbital
Two lobes of same size which align with axes that they are named for. 3 orbitals in x y and z axis so perpendicular to each other. All three are equal energy
Dumbell shape
Shape of d orbital
4 lobes and one very strange shape all with equal energy
Why do two electrons in same orbital have opposite spin
Same charge so repel
What is an electron cloud
An orbital where an electron can potentially be found
How would you arrange 4 electrons in a p orbital
2 paired electron in first square
And 1 each in the other two squares
How do you remember order of energy
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
Diagonally down
Why does copper and chromium only have 1 electron in 4s orbital?
Stability because having full orbitals or half full sets of orbitals is more stable and favourable energetically
1s2 2s2 2p6 3s2 3p6 4s2 3d2
This atom becomes an ion and loses 2 electron
What is its config or from which orbital is the electron lost
4s2 orbital loses both electrons because of first in first out rule
When filling 4s is lower in energy so filled first but once filled it becomes higher energy so it is lost before 3d
3/4 rules of electron config in the orbitals
Fill electron with lowest energy level first
Only 2 electron in an orbital with opposite spins
Each orbital has 1 electron before 2nd is introduced or paired
What is shorthand rule
Any example?
Using previous noble gas and then add in outer electron subshells as normal
Na = Ne in square brackets then 3s1
What is ionic bonding
Electrostatic attraction between oppositely charged ions
Why is the ionic bonding structure a giant lattice
Each ion attracts oppositely charged ions in all directions
Finish sentence
The greater the … the stronger the electrostatic attraction between them
Charge
What is ionic bonding bp/mp like and why
Mp/bp is high cos ionic is strong bond so lots of energy needed to overcome this bond
What do ionic substances dissolve in or do they not
Do all ionic compounds dissolve
Polar solvents like water
Large charged compounds don’t dissolve as the bond is too strong
Which atom in h20 water has a positive dipole
H
Why does oxygen have a negative dipole in water
It has 2 lone pairs of electrons so that area has slight negative charge
How does water break down ionic lattice
H20 molecules pull ions apart by surrounding each ion which eventually breaks down the lattice
Why doesnt ionic compound conduct at solid
Ions are in foxed position and only vibrate on the spot
Why do ionic compounds conduct in aqueous or molten
Ionic lattice breaks down
Ions are free to move as mobile charge carriers
What is covalent bond
Strong electrostatic attraction between a shared pair of electrons and nuclei of the bonded atoms
Why do simple molecular covalent have weak intermolecular forces
The attraction of covalent bonding is only localised to the nuclei of the multiple atoms
What is intermolecular force
What is intramolecular force
Weak forces between different molecules
The actual covalent bond between the atoms
Which is stronger ionic or giant covalent
Giant covalent
What is a lone pair of electrons
Paired electrons that aren’t shared with another atom
What are simple molecular soluble in
And how/why
Non polar solvents like benzene
Van der waals forces form between solvent and molecule which weakens the lattice
What are the 3 giant covalent structures for a level
Graphite
Diamond
Silica or silicon dioxide
What are giant covalent soluble in
Why
Neither polar nor non polar as the bonds are too strong
Graphite properties and reason
Slippery as the layers have weak intermolecular forces between them
Conductive as there are extra electrons that form clouds of free electrons between the layers
What is a dative bond
Only the bonding atom supplies both electrons as the shared pair as the shared pair was originally a lone pair of electrons
What is average bond enthalpy
Measurement of covalent bond strength
Larger the value the stronger it is
Complete sentence
Covalent bonds have paired electrons that have same electron config as nearest noble gas which obeys the …… rule
Octet
Why is it not always possible to follow octet rule
2 points
May not have enough electrons to reach full octet
Have more electrons available as it can access the d orbitals so octet expands.
