Electrons and Bonding Flashcards
All things ionic, covalent and electronic
What are atomic orbitals?
- These are regions around the nucleus that can hold up to 2 elecrtons with opposite spins!
spin = an electron qunatum property: DONT WORRY ABOUT IT!!
What happens when outer shell increases distance from the nucleus?
- The shell will increase in energy
- Each new period = each new shell
Describe the properties of the s-orbital…
- This is spherical in shape, with increasing orbital radius further from the nucleus
*
Describe the properties of a p-orbital…
- This is dumbell/figure of 8 shaped, only starts in the n=2
- Orbitals perpendicular to each other
What is the difference between Sub-shells and Energy Levels?
- Sub shells refer to specific orbital types, being similar (mostly) e.g s,p,d,f
- Energy levels refer to the main levels of shells with same value as “n” in an atom e.g. 1st, 2nd, 3rd ect…
“n” = PRINCIPLE QUANTUM NUMBER!
What happens when we move up a new shell in an atom?
- We will come across a NEW orbital
- This orbital has 2 elecrtons each
- Each corresponding shell will have a set number of orbitals (1,3,5,7 rule…)
- Hence, 2 * number of orbitals = number of electrons!
State the 3 conventions for electron filling
- Electron pair with opposite spins, ALWAYS!!!
- ALL orbitals on same energy level are occupied FIRST!
- Each electron occupies an orbital BEFORE pairing
What’s up with Chromium, Copper and all elements direcly below????
- These elements are EXEPTIONS to the electron configuration rule!
- Due to 3d sub-shell happens to be MORE STABLE when half-complete
- Hence, 1 electron jumps to the 4s sub-shell instead
How can we write shorthand electronic structure?
- Write the NOBLE GAS closest in atomic number in brackets like ”[]”
- Write the “suffix” of the rest of the electronic structure of the element!
What does “periodic table blocks” tell us?
- Shows the corresponding elemsnts with HIGHEST ENERGY LEVEL in these orbitals!!!
How can we represent ions electronic configuration?
- Add or subtract the electrons from the end of the written structure
- e.g. the 2s 1 from 1s2 2s1
Describe a GIANT ionic lattice!
- This is when metal transfers electrons to non metal, achieving outer shell
- ELECTROSTATIC FORCES OF ATTRACTION will occur in ALL DIRECTIONS of the molecule
How do we draw ionic bonding?
- Via DOT AND CROSS diagrams
- ALWAYS showing the FULL OUTER SHELLS
What link can be made with noble gasses and ions?
That they share same electronic structure!
think about it, you tested it out and it IS TRUE
Why does inoic compounds have high MP/BP?
- This is due to the STRONG ELECTROSTATIC FORCES that acts in all directions
- A lot of energy to overcome and break!!!
Why are ionic compounds soluble in polar solvents?
- This is due to water molecules able to surround individual ions, breaking the ionic lattice down!
IonIc ConDUctIng ElEcTrIcItY?!
- Only in a molten/dissolved form!!
- Due to DELOCALISED IONS able to carry electrical charge throughout the stucture!
How does ionic charges affect its properties??
- Greater charge=higher BP/MP
- = Reduced solubility
All due to HAVING GREATER ELECTROSTATIC FORCES OF ATTRACTION
What happens during covalent bonding?
check itttttttttt………
Here, atoms share electrons in pairs in between atome in order to complete outermost shell
in displayed formulae, a single line = a shared pair of electrons
What happens during the Expansion of the Octet?
- Normally, atoms look to fill to 8 electrons in outer shell..
- HOWEVER, Period 3 non-metal and non-inert elements can PROMOT/EXITE thier electrons to the NEXT ORBITAL (3d)
Including: Silicon, Chlorine ,Phosphouous and Sulfur has 3p orbitals
Hence, will make them VERY SIMILAR IN ENERGY to 3d orbitals, making little energy needed to exiteb the………….
What take place during Dative Covalent Bonding???
- Where BOTH ELECTRONS in shared pair are provided by ONE atom!
- Will have the same enthalpy as to a NORMALL covalent bond!
- Will casue ionic charges on such molecules, but not always (e.g. NH4+)
would otherwise remain as a lone pair……….
