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