Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
8 Cards in this Set
- Front
- Back
|
What are the 4 quantum numbers ? How do you get each
|
n = Principal shell #
l = azimuthal (Subshell) (0 =s; 1=p, 2=d, 3=d; orbitals) ml = magnetic # (Specific orbital) ms = spin (+/- 1/2) How to get them? ie. what are the quantum numbers for 3d n = shell # l = n-1 ml = -l to +l (include 0) ms = spin So n =3 l = 3-1 =2 ml = -2,-1,0,1,2 = 5 values ms = spin |
|
|
High nucleus binding energy =
low nucleus binding energy = |
stable nucleus
unstable nucleus (radioactive) |
|
|
Rank the following from strongest to weakest penetrating power
Alpha particles Gamma Ray Positron Beta |
Strongest
Gamma > Positron > Beta > Alpha Gamma is the strongest b/c it is no mass. |
|
|
Note: What happens to the penetrating power as the mass decreases?
|
Mass decreases then
Penetrating power increases |
|
|
How do we identify I stable nucleus?
|
Even # of Electrons = more stable
Odd # of Electrons = Almost for sure radioactive/unstable N (# of neutrons) / Z (# of protons) Further away from the 1:1 ratio the more likely they are not stable |
|
|
What are the octet exceptoins?
|
Under Octet:
H (one bond) Be (4 bonds) B, Al (3 bonds = lewis acid) Expanded/Over Octet: The third row of the periodic table and below (be careful b/c this is not always the case) Odd # of e- is not going to work |
|
|
What are the steps to draw lewis structures?
|
1) Count # Valence e-
2) Locate central atom by finding the atom that can make most bonds 3) make single bonds to outer atoms 4) place octet e- on outer atoms 5) Count # of e- to see if you need more or none. -> If need more? => place on central atom 6) Look at Central atom. Is it :) or :( - If :) = stop, your done - If :( = 1) find which one need more bonds to be happy 2) Both outer atoms need one bond to be :) then go -> F.C. Test = 1) Least amount of charge = more stable/ more :) 2) Neg (-) charge goes on most electronegative atom |
|
|
If you see halogens surrounding a central atom is there a quick way to find the lewis structure? ie SF4 or XeF2
|
Yes
Because Halogens usually always from 1 bond. 1) Draw single bonds from central atom to halogen 2) Is the central atom :) 3) Count of the number of e- and then place them on the central atom. Bam! you are done! |
