IB Chemistry HL Final

ionic bonding

an electrostatic attraction between oppositely charged ions

what must the difference in electronegativities be greater than for a compound to be ionic

(greater than) 1.8

covalent bonding

an electrostatic attraction between a bonding pair of electrons and two positively charged nuclei

metallic bonding

sea of delocalized electrons around a lattice of positively charged nuclei

what is the carbon allotrope of diamond's structure

giant 3D macromolecule (covalently bonded)

what arrangement is diamond

tetrahedral

what arrangement is graphite

trigonal planar

what is the structure of graphite

sheet-like

what is the arrangement of C60

truncated icosahedron (20 hexagons and 12 pentagons)

exothermic

heat loss to surroundings from system

endothermic

heat absorbed by the system from surrounding

heat

total energy of a given amount of a substance

temperature

measure of "hotness" (average kinetic energy)

activation energy

the minimum energy needed to start a reaction

what is the haber process

production of NH3 (ammonia)

what is the contact process

production of SO3 (sulfur trioxide...precursor to H2SO4)

what are the strong acids?

HCl, H2SO4, HNO3

what are the weak acids?

H2CO3, CH3COOH

what are the weak bases?

NH3/NH4OH, C2H5NH2/CH3CH2NH2

what are the strong bases?

NaOH, KOH, Ba(OH)2

bronsted-lowry acid

proton donor

bronsted- lowry base

proton acceptor

strong

completely dissociated into its ion (-->)

concentrated

high # of mol/dm^3

weak

partially dissociated into its ion (equilibrium arrow)

dilute

low # mol/dm^3

lewis acid

electron pair acceptor

lewis base

electron pair donor

isotopes

all atoms of same element with same # of protons/atomic # but differing #s of neutrons

when something is isoelectronic to an element, they have the same # of...?

electrons (ex: Cl- and Ar)

relative atomic mass (Ar)

(relative to 12C) weighted average of naturally occurring isotopes

atomic radius

distance from nucleus to outermost electron

1st ionization energy

energy required to remove an electron from a neutral atom in the gaseous state

electronegativity

attraction of an atom to a shared/bonding pair of electrons

electron affinity

the change in energy when an electron is added to an isolated atom in the gaseous state

alkali are all...

bases!

the nature of the acid/base of Na2O is...

strongly basic (NaOH)

the nature of the acid/base of MgO is...

basic (Mg(OH)2)

the nature of the acid/base of Al2O3 is...

amphoteric

the nature of the acid/base of SiO2 is...

weakly acidic

the nature of the acid/base of P4O10 is...

acid (weak) (H3PO4)

the nature of the acid/base of SO3 is...

strongly acidic (H2SO4)

the nature of the acid/base of Cl2O7 is...

strongly acidic (HCl)

amphiprotic

can either donate/accept an electron

amphoteric

can act as either an acid or base

monoprotic

acid with one H+

diprotic

acid with two H+'s

hybridization

molecular orbital theory of bonding

sigma bonds are...

single bonds

pi bonds are...

multiple bonds

sigma bonds

formed by axial overlap of atomic overlap (same orientation) (head-on/axial)

pi bonds

2 p orbitals that overlap side-ways/parallel

bond angle for sp3

109.5

bond angle for sp2

120

bond angle for sp

180

resonance

equal probability of double bond in two or more directions

delta H f theta

change in enthalpy when one mol of a compound is formed from its elements under standard conditions (298K) (1 atm)

delta H c theta

change in enthalpy when one mol of compound is combusted (completely) in O2 under standard conditions (298K) (1 atm)

delta H at theta

change in enthalpy of atomization when 1 mol gaseous atom is formed under standard conditions (298K) (1 atm)

delta H ea theta

change in enthalpy of electron affinity when one electron is addd to an isolated atom in the gaseous state under standard conditions (298K) (1 atm)

delta H latt theta (endothermic)

change in lattice enthalpy when a crystalline solid is turned into gaseous ions under standard conditions (298K) (1 atm)

delta H latt theta (exothermic)

change in lattice enthalpy when gaseous ions are turned into a crystalline solid under standard conditions (298K) (1 atm)

delta H solution theta

change in enthalpy when one mol of ionic compound dissolves in water to make an infinitely dilute solution under standard conditions (298K) (1 atm)

delta H hydration theta

change in enthalpy when one mol of gaseous ions dissolve in water to give an infinitely dilute solution under standard conditions (298K) (1 atm)

entropy

(S) disorder

delta S reaction theta

S products theta - S reactants theta

spontaneity

will the reaction want to happen?

gibbs free energy

spontaneous if negative

equation for gibbs free energy

delta g theta = delta h theta - T (delta s theta)

isomerism

same MF, different structural formulas