final Flashcards
IMF in order from weakest to strongest
- induced dipole - induced dipole
- dipole - dipole
- hydrogen bonding
- ion - dipole interactions
- ion - ion interactions
when do induced dipole - induced dipole interactions increase?
when surface area increases
when does hydrogen bonding occur?
when hydrogen is attached to fluorine, oxygen or nitrogen
ion dipole interactions occur when
ionic solute is mixed with a polar solvent
atomic theory
by john dalton
- each element is composed of tiny indestructible particles called atoms, which are all conserved (neither created nor destroyed) during a chemical change, just rearranged into different combinations
- if two atoms are of the same element, they will be completely identical. if its 2 of different elements, they’ll be different
- atoms combine in simple, whole-number ratios to form compounds. no element is found as a fraction of an atom
plum pudding model
by thomson, disproved and improved by rutherford
- atom’s mass is spread throughout the atom
- positive charges are spread throughout the atom
- neg charges are balanced out by positive charges
nuclear model
proposed by rutherford to correct his mentor thompson’s plum pudding model
- atom’s mass is concentrated at the nucleus
- positive charge is concentrated at the nucleus
- neg charges balanced out by pos charges (that didnt change from plum pudding model)
mass number
- total number of protons and neutrons in an isotope
- given by variable “A” or as [element]-[mass number] (ex neon-22)
- sometimes given as a superscript to the left of the element symbol
carbonic acid immediately decomposes to produce…
H2CO3 (aq) -> H20 (L) + CO2 (g)
sulfurous acid immediately decomposes to produce…
H2SO3 (aq) -> H20 (L) + SO2 (g)
ammonium hydroxide immediately decomposes to produce…
NH4OH (aq) -> H2O (L) + NH3 (g)
ammonium sulfide immediately decomposes to produce…
(NH4)2S (aq) -> H2S (g) + 2NH3 (g)
when is activity taken into account for a chemical reaction
- when determining whether a metal will displace another metal (single displacement). in order to do so, the metal must be more active than the metal it is displacing.
- also in redox: the more active a metal is, the easier it is to oxidize
what makes a solution a good conductor of electricity
dissolved ions must be present to make it a conductor of electricity, so ionic compounds or strong acids. a good conductor of electricity is called and electrolyte
when the sign of ∆H is negative
- the reaction is exothermic
- kJ is on the products side
- reaction feels hot
- reactants themselves contain energy than the products (through the law of conservation of energy, both sides must be equal, therefor the energy produced in the reaction was previously contained in the reactants)
acid-base reaction
- contains an acid (H___) and base (typically ___OH, though it can be a carbonate, sulfide, or sulfite as well) and forms H20 (or S20)
- always exothermic
- always double displacement
signs of a chemical change
- color change
- production of an odor (g)
- change of temperature
- evolution of a gas (formation of bubbles)
- precipitate
trend of atomic radius on periodic table
increases as you go down and to the left (lower left corner is largest)
trend of ionization energy and electronegativity
increases as you go up and to the right (upper right corner is largest)
p orbital shape
dumbell
s orbital shape
a ball
d orbital shape
four leaf clover
boyle’s law
- studies v (volume) and p (pressure), where n (mols) and T (temp) are constant
- p*v=constant since they are inversely proportional
charles’ law
- studies V (volume) and T (temp)
- V/T=constant since they are directly proportional
avogadro’s law
-studies V (volume) and n (mols)
V/n= constant since they are directly proportional
STP
standard temp and pressure, 0 C and 1 atm
list of strong acids
- HCl
- HBr
- HI
- HClO4
- HNO3
- H2SO4
list of weak acids
-HF
-HC2H3O2
-H2CO2
-H2CO3
-H2SO3
H3PO4
list of strong bases
anything that contains OH and is soluble
list of weak bases
- NH3
- C5H5N
- CH3NH2
- CH3CH2NH2
- HCO3-
∆E in reaction with activation barrier
∆E from reactant to product (excludes activation energy)
activation energy
height of barrier that reactant must “climb”
