FINALAMENTE – Flashcards
Unlock all answers in this set
Unlock answers| nitric acid |
| HNO3 |
| phosphoric acid |
| H3PO4 |
| Hydrogen Sulfate Ion |
| HSO4- |
| lactic acid |
| C3H6O3 |
| Acetic acid |
| CH3COOH |
| Carbonic acid |
| H2CO3 |
| Boric acid |
| H3BO3 |
| hydrocyanic acid |
| HCN |
| Sodium Hydroxide |
NaOH
(base) |
| Ammonia |
NH3
(base) |
| 1KWh = how many kJ; how many MJ? |
| 3600 kJ; 3.6 MJ |
| what is a calorie? |
| the energy needed to raise the temperature of 1 g of water by 1° C/K |
| 1 cal = |
| 4.184 J |
| BOYLE'S LAW def |
| Pressure and volume are inversely proportional, when the temperature and # moles are constant |
| BOYLE'S LAW |
| P1V1=P2V2= nRT at constant temp. |
| CHARLE'S LAW def |
| Volume and temp. are directly proportional when the pressure and number of moles are constant |
| CHARLE'S LAW |
| V1/T1 = V2/T2 = nR/P at constant pressure |
| AVAGADRO's LAW def |
| equal volumes of gas at the same temp. and pressure contain the same # of molecules |
AVAGADRO's LAW |
| V1/n1 = V2/n2 = RT/P |
| STP |
| T=273° K; P=1atm |
| standard molar volume |
| 22.4 L |
| ideal gas law |
| PV= nRT |
| ethanol |
| C2H5OH |
| Ionic bond |
| metal + nonmetal; transfer of e's takes place |
| Covalent bond |
| sharing of electrons;;uses prefixes |
| Phosphate |
| PO43- |
| Nitrate |
| NO3- |
| Kinetic Molecular Theory |
;
; |
| Intermolecular bonds in order of strength |
Hydrogen Dipole-dipole Dispersion |
| Intensive |
| the amount does not matter, ex: temp |
| Extensive |
| the amount matters, ex: mass |
| hydrogen bonds |
| btwn H and strongly electroneg. atoms (O,N,F) |
| dipole-dipole bonds |
| btwn any 2 polarm molecules |
| physical property |
| properties that can be observed without changing the nature of the substance (ie: tasting an apple) |
| dispersion/london forces |
nonpolar but temporary delocalization of electrons;; although weak, many of them, keep liquid/solid together |
| Anode |
| positively charged electrode where oxidation occurs; |
| Cathode |
| negatively charged electrode where reductions occurs |
| Ions: def/types |
atom(s) that carry a charge ; ANIONS: negative CATIONS:positive |
| Dalton's postulates |
all elements are made of small indivisable particles:atoms
all atoms have almost identical (chemical) properties
atoms combine in whole number ratios to form compounds
atoms can't be created or destroyed in a chemical reaction |
| prefixes |
| 1:mono, 2:di, 3:tri, 4:;tetra, 5:penta, 6:hexa, 7:hepta, 8:;octa, 9:nona, 10:deca |
| When oxidation occurs, energy is usually________. |
| released |
| OIL-RIG |
Oxidation: electons/energy is lost ; Reduction: electrons/energy is gained |
| For reactions with oxygen, oxygen is always... |
| reduced |
| OXIDATION |
;electrons LOST; hydrogen atoms lost; gain of oxygen atoms |
| A reducing agent is... |
| a compound that gets oxidized |
| atomic # is the _______ |
| # of protons OR #electrons |
| How were electrons discovered? |
| Crookes tubes- produced streams called cathode rays. |
| Group 1 |
| Alkali metals |
| Group 2 |
| Alkali earth metals (soapy) |
| Group 6A |
| Chalogens (most stable on earth) |
| Group 7A |
| Halogens (salt generators) |
| SI units for mass |
grams; kg=1000g;; ; mg=1/1000 g ; ;g=1/106 g ; ng= 1/109 g ; pg= 1/1012 g |
| Reduction |
the addition of hydrogen to a substance; ; the gain of electrons |
| Some catalysts used when hydrogen is added to a compound |
Pd (palladium) Ni (nickel) Pt (platinum) |
| Acids are... |
| proton donors. |
| Bases are... |
| proton acceptors. |
| Weak acids produce... |
a relatively small fraction of the maximum number of possible hydronium ions. |
| Period v.s. Group |
period = Row, across, in the periodic table. ; group = verticle grouping, columns |
| Sig.figs |
Leading zeroes are NOT sig. ; Trailing zeroes after the decimal point ARE. ; Internal zeroes ARE. ; Whole numbers ending in zeroes are ambiguous; solved by placing a . or converting to scientific notation |
| Exact numbers |
| no uncertainty; infinate # of significant figures |
| xRAYs |
Alpha = 2+ positive; 4g ; Beta= 1- negative; 1/2000 g ; Gamma= neutral; no mass |
| isotopes def. |
atoms with the same number of protons, but different number of neutrons ; ; (same place on periodic table) |
| Ground state; Realxation |
ground state: when the electrons stay close to nucleus ; ; relaxation: after excitation, the electrons come close again; energy is given back during this state |
| How do you find the # possible electrons per orbit level? |
2n2 ; n being the orbit level |
| When electrons jump from a higher to lower orbit, |
| there is an emission of light. |
| Ag is... |
| Silver; always 1+ |
| Zinc always has a charge of |
| 2+ |
| Naming covalent compounds |
Most Metallic element is first (CO2) ; Oxygen is always last. ; Use prefixes! ; ends in -ide. |
| Guessing polarity based on electronegativity scale |
NONpolar: difference is ; 0.5 ; polar: 0.5 ; difference ;2 ; ionic: if difference is ; 2 ; ; the higher the EN#, the more love for electrons; the higher EN is the neg. end and the lower is the + end. |
| carbonate |
| CO32- |
| Lewis formulas (HONC) |
hydrogen has 1 bond oxygen has 2 bonds nitrogen has 3 carbon has 4 ; if there are several atoms the least electronegative will be in the cener (except H) ; distribute to peripheral e's first, then central |
| free radical |
| have odd # of electrons; very reactive |
| electron geometry v.s. molecular shape |
each pair of e's = an electron set *a double bond counts as 1 set ; ; E.G refers to central atom, bonding; nonbinding ; M.S. refers to bonded atoms ; 3Dshape |
| electron domain |
| 1 pair of electrons, bonding or nonbinding; could be a;double bond; a triple bond |
| Avagadro's # |
| 6.022 x 1023 atoms |
| Molar mass v.s. formula mass |
molar mass is in g/mol
formula (molecular) mass is in amu |
| Stoichiometry |
In balenced chemical equations: A,B, and C are equivalent
A+B =C
A/B is an ex: the stoichiometric factor |
| temperature |
measure of kinetic energy of atoms and molecules INSIDE an object
kelvin is the SI unit. K° = C° + 273° |
| Exothermic |
| heat is produced; hot to the touch |
| Endothermic |
| Heat is required for the process; feels cold to the touch |
| photovoltaic energy is derived from |
| the sun; solar converted to electrical energy |
| intRAmolecular forces v.s. intERmolecular |
A. what keeps atoms together in molecules; covalent and ionic bonds
B. what keeps molecules together |
| electrolytes |
solutions of ionic substances that conduc electricity
if dissociation is complete: they're strong electrolytes if dissociation is partial: they're weak electrolytes if no dissociation, they're NONelectrolytes ; not all ionic substances are soluble ; not all soluble substances are electrolytes |
| ion-dipole interaction |
| in solutions of polar solvent + ionic solute, the STRONG force between the dipoles of solvent and the ions |
| ANHYDRIDES |
react with water to form acids/bases ; metal oxides are basic anhydrides nonmetal oxides are acidic anhydrides |
| How are antioxidants recuding agents? |
| They prevent the oxidation of other* molecules in the body by being oxidized themselves. |
| convert grams --> mol |
| divide by molar mass |
| mol --> grams |
| multiply by molar mass |
