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Atomic and Nuclear
Chad Video and Kaplan Book Chemistry
| Question | Answer |
|---|---|
| What does Z symbolize | number of protons |
| What does N symbolize | N |
| change in mass number but same atomic number | ISOTOPE |
| [Ar] 4s1 3d5 NOT 4s2 3d4 d half full and s half full so preferred- (exception) | Cr |
| [AR} 4s1 3d 10 this fills up d shell and s shell is incomplete | Cu |
| configuration of Cu+ | [Ar] 4s1 3d10 --> [Ar]3d 10 |
| something that has unpaired electrons attracted to magnetic field | paramagnetic - |
| no unpaired electrons slight repulsion to magnetic field | diamagnetic |
| odd number of electrons --> paramagnetic or diamagnetic | paramagnetic |
| principal quantum number and their range | gives shell number n = 1, 2, 3, 4 range [ 1 to infinity] |
| azimuthal quantum number | gives subshell- tells if you are in s, p, d, or f orbital l= [0 to n-1] |
| azimuthal number when in s orbital | n=1 l=0 (n-1) |
| azimuthal number when in p orbital | n= 2 l= can be 0 or 1 (n-1) |
| azimuthal number when in d orbital | n=3 l= (3-1) 0, 1, or 2 |
| azimuthal number when in f orbital | n =4 4-1= 3 l= 0, 1, 2, or 3 |
| magnetic quantum number | Ml gives orientation in space |
| what is the range for magnetic quantum number | -l to +l |
| magnetic quantum number for s orbital | -0 to +0 |
| magnetic quantum number for p orbital | -1, 0, +1 represents x, y , z |
| magentic quantum number for d orbital | l=2 [-l to +l] -2, -1, 0, 1, 2 |
| what is incorrect in the quantum number: [3, 2, -1, -1] | fourth number, magnetic spin, should be 1/2 |
| magnetic spin | Ms can be -1/2 or +1/2 |
| what is incorrect in the quantum number: [3, 3, -1, 1/2] | second number- azimuthal number is n-1 so should be 2 not 3 |
| what is incorrect in the quantum number: [3, 2, -3, 1/2] | third number - magnetic number is -l to +l so cannot be -3, should be -2 |
| what is the configuration for the excited state: ground state: [Ar] 4s2, 3d10, 4p5 | [Ar] 4s2, 3d10, 4p4, 5s1 |
| 1st criteria to check for unstable nucleus | if odd number of protons and neutrons- it will be RADIOACTIVE |
| 2nd criteria to check for unstable nucleus | check ratio of N/Z (neutrons/protons) |
| for elements larger than Ca: N/Z ratio should be | 1.6 |
| for elements upto Ca (Z=20) N/Z ratio should be | 1 |
| alpha decay what does it cause | reduction in mass by 4 |
| what does alpha decay affect | heavy elements greater than atomic number 83 (want to lose mass so do alpha decay) |
| 232/90 Th alpha decay--> | 228/88 Rn + 4/2 alpha particle |
| B- decay (electron emission) 232/90 Th --> | 0/-1 B + 232/91 Pa N/Z ratio too high - above belt of stability |
| B + decay (positron emmision) 232/90 Th | 0/+1 B + 232/89 Ac N/Z ratio too low- too many neutrons so add protons |
| Electron capture 232/90 Th + 0/-1 e --> | 232/89 Ac when N/Z ratio too low so want to add protons |
| gamma decay 232/90 Th --> | 0/0 gamma + 232/90 Th |
| each element is excited to its distinct energy level so it has its own line spectrum that serves as a fingerprint for the element | atomic emission spectrum |
| hydrogen emission lines from n>2 to n=2 | Balmer series |
| hydrogen emission lines from n >1 to n= 1 | Lyman series |
| energy absorbed as an electron jumps from an orbital of low energy to high energy which characterizes each element | absorption spectrum |
| atomic radius as you go down the period? | it will decrease because more electrons are added |
| atomic radius as you go down the group | it will increase because electrons are farther from the nucleus |
| energy required to remove an electron from a gaseous atom or ion | ionization energy |
| as you go across the period to the right: ionization energy | Increases as you go across because require more energy to remove electrons because they all want to gain electrons to fill octet |
| as you go down the column: ionization energy | decrease as you go down- electrons are farther and loosely held |
| energy change that occurs when an electron is added to a gaseous atom | electron affinity |
| as you go across the period to the right: electron affinity | increases: elements want to add electron to fill their octet so eagerly accept the electron |
| as you go down the column: electron affinity | decreases as you go down: |
| measure of the attraction an atom has for electrons in a chemical bond | electronegativity |
| as you go across the period to the right: electronegativity | increase |
| as you go down the column: electronegativity | decrease |
| why does Be have a higher ionization energy than Li | it has a filled s subshell so wants to hold on to its electron more |
| shiny solids, malleability, ductility, good conductors, high melting point and density | METALS |
| brittle, no metallic luster, high ionization energy, poor conductor, high electron negativity | NON-Metals |
| why is N have a higher ionization energy than oxygen? | trend reverses because N has half filled orbital so it is stable and satisfied so it is an exception |
| good semiconductors | metalloids |
| have largest atomic radii, high reactivity, low ionization energy, low electronegativity; similar to metals | alkali metals |
| metallic properties, 2 valence electrons, low electronegativities, and positive electron affinity | alkaline earths |
| highly reactive nonmetals with seven valence electrons, high electronegativity | HALOGENS |
| electron affintiy: exothermic or endothermic | exothermic; gets more negative as go to the left because there is a greater release of energy |
| inert gas; non reactive; complete valence shell; low boiling point; gas at room temperature | noble gas |
| metals; high melting and boiling point; malleable; oxidation states; highly colored solutions; | transition elements |
| which transition metal has higher ionization energy | 3d 10 with Zn, Cd, Hg because their d subshell is filled |
| metal with nonmetal; high melting/boiling point; brittle | ionic bond |
| nonmetal with nonmetal; lower melting/boiling point | covalent bond |
| metal with metal; high melting point | metallic bond |
Created by:
sfkhan7797
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