C5 Electrons And Bonding Flashcards
What are shells regarded as
Energy levels
What is the principle quantum number n
Shell number or energy level number
What is the formula for the maximum number of electrons in a shell n
2n^2
What are shells made up of
Atomic orbitals
What is an atomic orbital
A regional around the nucleus that can hold up to 2 electrons, with opposite spins
How many electrons can an orbital hold
1 or 2 electrons but no more
What are the different types of orbitals
S-
P-
D-
F-
Do the orbitals have the same shapes
No
They each have different shapes
What is a shell
A group of orbitals with the same principle quantum number
How many electrons can the 1st shell hold
2
How many electrons can the 2nd shell hold
8
How many electrons can the 3rd shell hold
18
How many electrons can the 4th shell hold
32
What’s the shape of an s-orbital
Spherical
What’s the shape of a p-orbital
Dumb-bell shape
How many orbitals are found in a s-sub shell
1
How many electrons can be held in a s-subshell
2
How many orbitals does p-sub shell have
3
How many electrons can be held in a p-subshell
6
How many orbitals are present in a D sub shell
5
How many electrons can be held in a d sub shell
10
How many orbitals are found in a F sub shell
7
How many electrons can fill F sub shell
14
What are the rules by which electrons are arranged in the shell
Electrons are added 1 at a time
Lowest available energy level is filled first
Each energy level must be filled before the next one can fill
Each orbital is filled singly before pairing
4s is filled before 3d
Why does 4s orbital fill before 3d orbital
4s orbital has a lower energy than 3d before its filled
Whats an ionic bond
Electrostatic attraction between positive and negative ions.
Why does giant ionic lattices conduct electricity when (l) but not when (s)
When (s) ions fixed in place - cannot move
When (l) ions are mobile - freely carry charge
What’s a metallic bond
Electrostatic attraction between the positive metal ions and the sea of delocalised electrons
Why do giant metallic lattices have high MPs & BPs
Large amount of energy required to overcome strong metallic bonds
In what type of solvents do ionic lattices dissolve
Polar solvents
E.g.water
Why are ionic compounds soluble in water
Water has polar bond
Delta pos of H attracted and delta neg of O can attract ions
How many covalent bonds does a carbon form
4
How many covalent bonds does oxygen form
2
What’s a dative covalent bond
Bond where both of shared electrons are supplied by one atom
What does expansion of the octet mean
When a bonded atom has more than 8 electrons in the outer shell
What are the 2 types of covalent structure
Simple molecular lattice
Giant covalent lattice
Why do simple molecular structures have low MPs & BPs
Small amount of energy is enough to overcome the intermolecular forces
Can simple molecular structures conduct electricity and why
No
They’re non-conductors
They have no free charged particles to move around
In that type of solvents do simple molecular structures dissolve in
Non-polar solvents
Examples of giant covalent structures
Diamond
Graphite
Silicon dioxide, SiO2
Properties of giant covalent structures
High MPs & BPs
Non-conductors of electricity, except graphite
Insoluble in polar & non-polar solvents
How does graphite conduct electricity
Delocalised electrons present between layers are able to move freely carrying charge
Why do giant covalent structures have high MPs & BPs
Strong CBs within molecules need to be broken which requires a lot of energy
Describe the structure of a diamond
3D tetrahedral structure of C atoms
With each C atoms bonded to 4 others
By how many degrees does each lone pair reduce bond angle
2.5*
What does it mean when the bond is non-polar
Electrons in bond are evenly distributed
What’s the most electronegative element
Fluorine
What’s the strongest type of IMF
Hydrogen bonding
