13288378
Description
Flashcards by I Shouldn't be awake, updated more than 1 year ago
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Created by I Shouldn't be awake
over 6 years ago
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| Question | Answer |
| What does an increase in shell number an increase in shell number n | The greater the radius of its orbital |
| What is the formula for number of electrons within that shell? | 2n^2 e.g. in 5 energy level orbital you have 2*5^2 = 50 electrons |
| how many orbitals can fit into the s/p/d/f-subshell? | 1,3,5,7 |
| how many electrons can fit in orbitals of the s/p/d/f sub-shell? | 2,6,10,14 |
| Why must electrons have opposite spin in an orbital? | Helps counteract repulsion between the - charges, or else they'd just be blasted away and no longer orbit the nucleus |
| So, in one energy level there are multiple subshells. | So n=2 has 2s and 2px/y/z orbitals |
| Blocks and the periodic table | S-block, highest energy electron is in s-subshell. SO highest e- could be in 1s or 5s etc. |
| What occurs to D-block elements 3d sub-shell energy level when the 3d shell is filled? | It falls below the 4s sub-shell |
| So order of emptying filling in d-block? | 4s empty and fills before the 3d |
| Ionic melting and boiling points | Near all are solid at RTP Insufficient energy to overcome strong electrostatic forces of attraction between oppositely charged ions in the giant ionic lattice. Therefore, high mpt and bpt. |
| Solubility | Soluble in polar solvents dependent on relative strength of attraction within the giant ionic lattice and the attraction of the ions to the water molecules. Therefore decreases as charge increases. |
| Electrical conductivity | Solid- No mobile charge carriers non-conductor liquid/dissolved: Solid ionic lattice breaks down ions free to move as mobile charge carriers |
| Covalent bonding | Strong electrostatic attraction between shared pair of electrons and the nuclei of the bonded atoms by an overlap of orbitals, each containing 1 orbital |
| Why can boron only for 3 bonds? | 1s2 2s2 2p1 Only 3 valence (outershell) electrons can participate in covalent bonding. |
| Sulphur bonding | Can tease out all 6 valence electrons to become unpaired to bond with other atoms Expansion of the octet, only available from n=3 onwards |
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