shit i need to memorize

for chem 202 final

light speed (C) equals what??

energy (E) equals what??

paramagnetic

unpaired electrons

diamagnetic

paired electrons

atomic radius periodic trend

• atomic radius increases as you go down a column

• atomic radius decreases as you go across a period

ionization energy periodic trend

• ionization energy decreases as you go down a column

• ionization energy increases as you go across a period

electronegativity periodic trend

• electronegativity decreases as you go down a column

• electronegativity increases as you go across a period

metallic character periodic trend

• metallic character increases as you go diagonally down left on the periodic table

  • away from flourine

• metallic character decreases as you go diagonally up right on the periodic table

  • towards flourine

quantum numbers (n)

• principal quantum number

• s and p block??? literally just your row number

• d block?? row number - 1

• f block?? row number - 2

quantum numbers (l)

• azimuthal quantum number

• n-1

  • or more if your n is higher

quantum numbers (m_l)

• orientation quantum number

• ± l

quantum numbers (m_s)

• spin quantum number

• ± ½

• no right or wrong answer

soluble ionic compounds and exceptions

• NO₃^- : always soluble, no exceptions

• C₂H₃O₂^- : always soluble, no exceptions

• Cl^-, Br^-, I^- (group 17’s) : not soluble with Ag⁺, Hg₂²⁺, and Pb²⁺

• SO₄^2- (sulfate) : not soluble with Sr²⁺, Ba²⁺, Hg₂²⁺, and Pb²⁺

• NH₄⁺

• alkali metals (group 1)

• alkali earth metals (group 2)

insoluble ionic compounds and exceptions

• S^2- : soluble with NH₄⁺, alkali metals, Ca²⁺, Sr²⁺, and Ba²⁺

• CO₃^2- and PO₄^3- : soluble with NH₄⁺ and alkali metals

• OH^- : alkali metals, Ca²⁺, Sr²⁺, Ba²⁺

breaking bonds

• REQUIRES ENERGY

• endothermic

• (+) delta H

• on the “reactants” side of the reaction

building bonds

• RELEASES ENERGY

• exothermic

• (-) delta H

• on the “products” side of the reaction

nonpolar

0-0.5

polar covalent

0.5-1.6

ionic

1.6-2

linear

• electron geometry: linear

• molecular geometry: linear

• 2 electron binding sites

• 2 bonds

• 0 lone pairs

• 180 degrees bond angles

• ex: CO₂

trigonal planar

• electron geometry: trigonal planar

• molecular geometry: trigonal planar

• electron binding sites: 3

• 3 bonds

• 0 lone pairs

• 120 degree bond angles

• ex: BCl₃

bent (trigonal planar)

• electron geometry: trigonal planar

• molecular geometry: bent

• electron binding sites: 3

• 2 bonds

• 1 lone pair

• less than 120 degree bond angles

• ex: SO₂

tetrahedral

• electron geometry: tetrahedral

• molecular geometry: tetrahedral

• electron binding sites: 4

• 4 bonds

• 0 lone pairs

• 109.5 degree bond angles

• ex: CH₄

trigonal pyramidal

• electron geometry: tetrahedral

• molecular geometry: trigonal pyramidal

• electron binding sites: 4

• 3 bonds

• 1 lone pair

• 107.5 degree bond angles

• ex: PH₃

bent (tetrahedral)

• electron geometry: tetrahedral

• molecular geometry: bent

• electron binding sites: 4

• 2 bonds

• 2 lone pairs

• 104.5 degree bond angles

• ex: H₂O

trigonal bipyramidal

• electron geometry: trigonal bipyramidal

• molecular geometry: trigonal bipyramidal

• electron binding sites: 5

• 5 bonds

• 0 lone pairs

• 120 degree equatorial bond angles

• 90 degree axial bond angles

• ex: PCl₅

seesaw

• electron geometry: trigonal bipyramidal

• molecular geometry: seesaw

• electron binding sites: 5

• 4 bonds

• 1 lone pair

• less than 120 degree equatorial bond angles

• less than 90 degree axial bond angles

• ex: SF₄

t-shaped

• electron geometry: trigonal bipyramidal

• molecular geometry: t-shaped

• electron binding sites: 5

• 3 bonds

• 2 lone pairs

• less than 90 degree bond angles

• ex: ClF₃

linear (trigonal bipyramidal)

• electron geometry: trigonal bipyramidal

• molecular geometry: linear

• electron binding sites: 5

• 2 bonds

• 3 lone pairs

• 180 degree bond angles

• ex: XeF₂

octahedral

• electron geometry: octahedral

• molecular geometry: octahedral

• electron binding sites: 6

• 6 bonds

• 0 lone pairs

• 90 degree bond angles

• ex: SF₆

square pyramidal

• electron geometry: octahedral

• molecular geometry: square pyramidal

• electron binding sites: 6

• 5 bonds

• 1 lone pair

• less than 90 degree bond angles

• ex: BrF₅

square planar

• electron geometry: octahedral

• molecular geometry: square planar

• electron binding sites: 6

• 4 bonds

• 2 lone pairs

• 90 degree bond angles

• ex: XeF₄

solution is what

solute and solvent mixed together

molarity (M)

molality (m)

mole fraction (X)

mol percent (mol %)

parts by mass (%)

raoult’s law (non-volatile, non-electrolyte)

raoult’s law (volatile, non-electrolyte)

raoult’s law (volatile?, electrolyte)

calculating change in freezing/boiling point

b/c of electrolytes (raoult’s law sorta)

henry’s law

converts atm to molarity basically

osmotic pressure equation

all those extra E_cell and delta G equations for electrochem and delta G

alpha decay particle

• highest ionization power

• lowest penetrating power

• always released

beta decay particle

• literally an electron

• mid ionization power and penetrating power

• BETA DECAY IS RELEASED OF ELECTRON

• a neutron converts into a proton and an electron basically

gamma emission

• literally just light

  • no mass or charge

• lowest ionization power

• highest penetrating power

• releases light (gamma radiation) b/c an element(?) is “meta stable” and needs to chill out

meta stable

element is too excited and needs to release gamma radiation in order to stabilize/chill out

positron particle and emission

• literally an “anti-electron”

• they get released

electron capture

• literally beta decay just in reverse

• an electron is CAPTURED

subatomic particles notation