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CHEM 151: FINAL
phase transitions |
solid to liquid - melting
solid to gas - sublimation
gas to solid - deposition
gas to liquid - condensation
liquid to gas - vaporization
liquid to solid - freezing |
extensive property |
depends on the amount of product (mass of salt added to soup) (mass, volume, weight, length) |
intensive property |
does not depend on amount (temperature, color, melting point/boiling point) |
ideal gas law |
PV=nRT |
phase changes for water |
why does it stay the same?
the energy is being used as potential energy to separate the molecules
polar condenses first |
intermolecular forces |
solids - strongest
liquid - medium
gas - weak
dispersion is weakest
dipole middle
hydrogen bonding strongest |
chemical changes |
does not just change the phase (iron rising, gas combusting) |
pure substance |
can be molecules with different elements, but has to be all the same with the same amount |
elements vs. compounds |
only one element on the periodic table
compounds are a mix of different elements |
phosphate |
PO4 |
Nitrate |
NO3 |
Hydroxide |
OH |
Carbonate |
CO3 |
Celsius to Kelvin |
temp + 273.15 = K |
Kelvin to Celsius |
temp - 273.15 = Celsius |
F to Kelvin |
(temp - 32) / 1.8 = tempC + 273.15 = K |
Celsius to F |
temp x 1.8 + 32 = F |
empirical formula vs. molecular formula |
empirical formula = molecular formula simplified |
ionic |
two elements, one from each side of the periodic table |
covalent |
two elements, both from the same side of the periodic table |
diamagnetic |
only paired electors |
paramagnetic |
have unpaired electrons |
Hund's Rule |
"bus rule" when completing orbital box notation, add singly to each orbital before doubling up on them. |
wavelength spectrum |
radio
microwave
infrared
visible
ultraviolet
x-ray
gamma ray
(shorter the wavelength, higher the energy and velocity) |
isoelectronic atoms |
have the same number of electrons (K+, A, and Cl-) |
valence electrons |
whatever group the element is in (O has 6 valence electrons) |
melting point / boiling point |
the more electrons shared and the bigger the compound, the higher the melting point (MgO will have a higher melting point than NaF). bigger have the lower melting point (bc farther form the nucleus). bigger change then smaller the size |
emission spectroscopy |
ionization energy gets smaller as going down the periodic table |
properties of metals |
1. malleable/ductile. (bendable)
2. conduct electricity in molten state can conduct as a solid.
3. high melting and boiling points |
atomic radius |
gets bigger left and down. bigger the attic radius the easier it is to remove an electron. |
electronegativity |
gets bigger right and up |
bond order |
number of bonds / outer elements |
bond angle |
linier = 180
bent = <120
trigonal planer = 120
trigonal p
tetrahedral = 109 |
molecular geometry |
actual geometry, does not include lone pairs (water is bent) |
electron geometry |
includes lone pairs as a bond (water is tetrahedral) |
formal charge |
atomic valence electrons - number of lone pair e - 1/2(the number of bonding pair e) |
resonance structures |
different forms that the same molecules can have. hybrid of all the possibility of all the molecule) |
cis vs. trans |
cis is polar (uneven), tran is nonpolar (even), polar will have a higher boiling point |
dipole-dipole |
pull of electrons by the more electronegative atoms (pulls toward the more electronegative atom) |
dispersion |
even distribution of atoms, all have dispersion, electrons are being spread out, in all chemical groups, usually represent the central location of the atom |
hydrogen bonding |
hydrogen atoms bonding with other hydrogen atoms as long as they are not attached to a carbon |
isomer |
one group of compounds having the same chemical formula but different molecular structures (trans vs cis) |
VESPR |
3D instead of a lewis structure. (methane is 109.5 degrees) *structure determines function (step two after connecting the molecule (lewis structure) ) electrons repel electrons. |
intermolecular forces vs. intramolecular forces |
intermolecular forces are usually week, from molecule to molecule
intramolecular forces are ones within a molecular (single, double, or triple), help determine the electron and molecular geometries within a molecule |
homogenous vs. heterogenous |
homogenous (milk and water) heterogenous (orange juice and pulp) |
rule of 4 |
tests solubility in water
product of the charges is greater than or equal to 4 = insoluble
example: CaS has +2 x -2 =4 and insoluble
exceptions: AgCl, AgBr, AgL, PbCl2, PbBr2, PbL2 |
solubility of covalent compounds in aqueous solution |
depends on intermolecular forces
"like dissolves like" |
strong electrolyte examples |
HCl, NaOH, NaCl
strong acids, strong bases, soluble salts |
weak electrolyte examples |
acetic acid (CH3COOH), Ammonia (NH3), and Hydrofluoric acid (HF)
weak acids and weak bases |
non electrolyte examples |
sucrose (C12H22O11), Methanol (CH3OH), MgO, AgCl, Hexane (C6H14)
insoluble compounds or compounds that do not dissolve |
acid formed |
when a chemical donates or "loses" a proton (H+) in water H3O+ is formed |
STRONG ACIDS MEMORIZE |
Hydrochloric Acid (HCl), Hydrobromic Acid (HBr)Acid (HBr), Hydroiodic Acid (HI), Perchloric Acid (HClO4), Nitric Acid (HNO3) and Sulfuric Acid (H2SO4) |
global equations |
include all the reactants and products of a given reaction (As Is) (Step 1) |
total ionic equations |
reflect dissociation of ionic compounds within aqueous solution
(broken up all aq) (step 2) |
Net ionic equations |
lack spectator ions, only exhibit the reactants which participate in formation of precipitate or are precipitates themselves
(ending when canceled out) (step 3 / final step) |
spectator ions |
ions that are canceled out when becoming a net ionic equation |
stoichiometry |
idea that matter can neither be created nor destroyed (low of conservation of matter), and chemical reactions take place in definite ratios of their chemical components. relationship of amount. amount is mole. aka 12 is dozen.. |
limiting reactants |
reactant that is depleted first, thereby effectively limiting the amount of product which can be formed
must be identified unless says it is "in excess" |
theoretical yield |
ideal/max yield of a given reaction (if 100% effciency |
actual yield |
refers to the experimental yield of the reaction in the laboratory when it takes place (actual result) |
percent yield |
percentage obtained when one divides the actual yield by the theoretical yield x 100
(% yield = (actual/theoretical) x 100 |
n, l, ms, ml |
n=1-7 debating on shells (rows)
l= n-1 up to 0 (s block is s=0)(p = l=1) d=l=2) blocks
ms= spin (up or down) + or - 1/2
ml= actual orbital, anywhere from -2 to 2
ex: 3d orbital
n=3
l=2
ml=
ex: 4p
n=4
l=1 |