| Question |
Answer |
| Plank's Constant (h) |
6.63x10^-34 J*s |
| Speed of light (c) |
3x10^8 m/s |
| Equation for the Energy of a photon |
hf or h*(c/wavelength) |
| Hund's rule |
electrons in the same subshel occupy available orbitals singly, before pairing up |
| Aufbau principle |
Electrons opccupy the lowest energy orbitals available |
| Pauli exclusion principle |
no two electrons in the same atom can have the same set of four quantum numbers |
| n,l,m(l),m(s) |
n = shell numberl = subshell number (n-1)m(l) = orbital numberm(s) = +1/2; -1/2 |
| diamagnetic |
has all electrons paired, repelled by magnetic field |
| paramagnetic |
not fully paired electrons; attracted to magnetic field |
| H |
Hydrogen, 1.0, 1 |
| He |
Helium, 4.0, 2 |
| Li |
Lithium, 6.9, 3 |
| Be |
Berillium, 9.0, 4 |
| B |
Boron, 10.8, 5 |
| C |
Carbon, 12.0, 6 |
| N |
Nitrogen, 14.0, 7 |
| O |
Oxygen, 16.0, 8 |
| F |
Fluorine, 19.0, 9 |
| Ne |
Neon, 20.2, 10 |
| Na |
Sodium, 23.0, 11 |
| Mg |
Magnesium, 24.3, 12 |
| Al |
Aluminum, 27.0, 13 |
| Si |
Silicon, 28.1, 14 |
| P |
Phosphorus, 31.0, 15 |
| S |
Sulfer, 32.1, 16 |
| Cl |
Chlorine, 35.5, 17 |
| A |
Argon, 39.9, 18 |
| K |
Potassium, 39.1, 19 |
| Ca |
Calcium, 40.1, 20 |
| Cu |
Copper, 63.5, 29 |
| Zn |
Zinc 65.4, 30 |
| Fe |
Iron, 55.8, 26 |
| Ag |
Silver, 107.9, 47 |
| Au |
Gold, 197.0, 79 |
| Pb |
Lead, 207.2, 82 |
| Beta Decay (B-) |
unstable nucleus contains too many neutrons; 1n-> 1p and 1e-; atomic number (z)increases by 1 but mass number stays the same [ex: 6C-> 7N + 1e-]; MOST COMMON FORM OF BETA DECAY |
| Beta Decay (B+) |
unstable nucleus contains too few neutrons; 1p-> 1positron + n; atomic number (z) decreases by 1 but mass number stays the same [ex: 9F-> 8O + 1e+] |
| Alpha Decay (a) |
nucleus becomes more stable by ejecting alpha particle (2p and 2n) {same as a helium molecule}; reduces atomic number (z) by 2 and the mass number by 4; Ex: (210, 84, Po) -> (206, 82 Pb) + (4, 2 alpha) |
| Electron Capture |
nucleus combines an e- with a p to make a neutron; atomic number (z)decreases by 1, atomic number remains the same |
| Gamma Decay |
an excited nucleus that has undergone beta or alpha decay relaxes by emitting energy in the form of 1 or more photons which have very high frequency and energy. Gamma decay penetrates matter most effectively, no mass, charge, or effect on z or n |
| mass defect |
the mass of the combined nucleus is less than the sum of the masses of all its nucleons individually, stable nucleus will always have a positive mass defect |
| eV |
electronvolts, 1eV= 1.6 x 10^-19 J, |
| 1kg = ?? Joules |
19 x 10^16 J |
| 1 amu = ??? kg |
1.66 x 10^-27 kg |
| Equation for mass-energy equivalence |
E=mc^2 (in joules); or E= m(in amu) x 931.5 eV |
| Alkali metals |
Group I ns^1 |
| Alkaline earth metals |
Group II ns^2 |
| Halogens |
Group VII ns^2np^5 |
| Transition metals |
d block |
| Representative metals |
p block (except for Group VIII) |
| Rare earth metals |
f block |
| Noble gases |
Group VIII ns^2 np^6 |
| the horizontal row on the periodic table |
period |
| vertical column on the periodic table |
group |
| Metalloids |
elements that contain properties of both metals and non metals: B, Si, Ge, As, Sb, Te, Po |
| Atomic and Ionic Radius Trend |
moving from left to right across a period, atomic radius decreases (b/c increasing numbers of protons pulls the electrons in stronger) going down a group atomic radii increases via increased shielding |
| Ionization energy (energy needed to remove an electron) trend |
left to right ionization energy increasesb/c valence e- are bound tighter |
| Electron Affinity |
halogens have large negative electron affinities, they readily accept electrons which causes E to be released |
| Electronegativity |
F>O>N>CL>Br>I>S>C>H {Foncl Brisch} is a measure of an atoms ability to pull electrons to itself when it forms a covalent bond increases from left to right |
| Acidity |
how well a compound donates protons, accepts electrons, or lowers pH. acidity increases from left to right, and increases as you go down a group |
| Formal Charge |
FC= Valence - 1/2(Bonded) - number of lone pair electrons |
| coordinate covalent bond |
one atom will donate both of the shared electrons in a bond |
| Lewis Acid |
Accepts a pair of electrons |
| Lewis Base/Ligand |
Donates a pair of electrons; must have a pair of nonbonding electrons to be a lewis base |
| Linear, Trigonal planar, tetrahedral, trigonal bipyramid, octahedral |
has no lone pairs of electrons on the central atom |
| Bent, trigonal pyramid, see-saw, square pyramid |
has 1 pair of electrons on the central atom |
| Bent, T-shaped, Square planar |
has 2 pairs of electrons on the central atom |
| Hybridization of Linear |
sp |
| Hybridization of Trigonal Planar |
sp^2 |
| Hybridization of Tetrahedral |
sp^3 |
| Hybridization of Trigonal bipyramidal |
sp^3 d |
| Hybridization of Octahedral |
sp^3 d^2 |
| Heat of Transition ΔH |
amount of energy required to complete a transition |
| q (heat) = n x ΔH{of a phase change} |
If q and ΔH are positive heat is absorbed if negative heat is released |
| 1 Calorie = ??? Joules |
4.2 J ; is the amount of heat required to raise 1 g of water 1 degree |
| q (heat) = mCΔT |
... |
| specific heat |
the higher the specific heat of a substance the better it holds on to absorbed heat |
| Temperature change is proportional to the heat absorbed, but inversely proportional to heat capcity |
... |
| During a phase transition tempature doesn't change the greater the value for the heat of transition the longer the flat line on a phase change diagram , Heat of Vap always > Heat of Fusion |
... |
| Triple point |
is the temperature and pressure at which all three phases exist simultaneouly in equilibrium |
| critical point |
marks the end of the liquid-gas boundary beyond this point a substance displays properties of both a liquid and a gas (supercritcal fluid) |
| supercritcal fluid |
no amount of pressure can force the gas back into a liquid state |
Poultry
