not malleable

high melting/boiling point

don't conduct electricity except when dissolved (free ions)

stronger than ionic

don't conduct electricity

low melting/boiling point

not solid at room temp

distinct molecules

Atomic Radius Trends

increases going down a group

decreases from L--> R

Ga < Al

Ga has higher Zeff

increases left to right

decreases going down a group

B<Be and Al<Mg

N>O, P>S, As>Se

count number of IEs before HUGE JUMP in value

that equals valence e-

that equals group number

amount of energy to add e-

positive or negative

Halogens: -(favorable)EA

Noble gases: +(unfavorable)EA

C has -EA

N has +EA

trend in gaining or losing e-

Anions: radius increase, IE decrease

Cations: radius decrease, IE increase

series of atoms and ions with exact same number total e-

can only have 1 neutral atom

transfer e-

metals and nonmetals

share e-

nonmetals

pooling of e-

metals

electrostatic energy equation

lattic energy trends

ion size increases, lattice energy decreases

ion charge increase, lattice energy increases

highest charge

smallest radius

strong bond = high BE

weak bond = low BE

how close we can get the nuclei

sum of the covalent radii

bond: leads to energy of reactions (PE)

translational: moving around in space (KE)

rotational: spin (KE)

vibrational: bond wiggling (KE)

each molecule has all at once, all the KEs

 move all KE at same temp, bond energy leads to energy changes in reaction

melting points and boiling points break...

lattice interactions

diamond is a very hard network of carbons

hard substance

high melting point

covalently bonded

electronegativity

EN trends

increases towards F

EN for H=P

B<H<C

F is the highest at 4.0

∆EN > 0

bonds between two different nonmetals

∆EN = 0

bond between two atoms of the same nonmetal

H-P bond nonpolar

   ---------------------------→

  -------------------------→

increases L-->R

decreases down a group

no set # of atoms in a metal sample

metals deform instead of shatter--malleable

conducts electricity and heat (solid and liquid state)

most are solids

moderate-high melting point

much higher boiling point

ammonium

CH₃COO^-

(C₂H₃O₂^-)

perchlorate

ClO₄^-

nitrate

hydrogen carbonate

(bicarbonate)

hydrogen sulfate

(bisulfate)

1

mono-

9

how do you find number of H atoms for alkanes?

heptane

want lowest magnitude of formal charge

most negative formal charge on most electronegative atom

sum of atomic masses of every atom in one molecule

g/mol

amu/molecule

Give name of metal (cation)

Name of nonmetal with -ide suffix

Ex: LiBr --Lithium Bromide

Ionic Nomenclature--Transition Metals

Give name of metal (cation)

Add charge in parentheses and in roman numerals

Add name of nonmetal with -ide suffix (anion)

Ex: FeCl₃--Iron (III) chloride

Use name

No suffixes

Ex: NaNO₃--Sodium nitrate

Name of 1st element--lower group number, or higher period number (H is never first)

Name 2nd element with -ide suffix (O with hallogen, name hallogen 1st)

Indicate number of atoms with prefix (never used mono- with 1st element)

Ex: P₂Cl₅-- diphosphorous pentachloride

H₂O: water

NH_3: ammonia

C_nH_2n+2: alkane

Place elements relative to each other (pick central atom--lowest group # or highest period #, noble gas)

Count valence e-

Add single bonds between central atoms and terminal atoms

Calculate bonding pairs

Fill out octets with lone pairs

Count valence e- used (if equals # valence e-, then we're done)

actual structure = average of all resonance structures

involves placement of double and triple bonds

(bonding pairs)/(bonds)

Ex:O₃=3/2

e- not stuck in between two atoms, free to roam across molecule

count bonding pairs as 1

lone pairs separately

decide charge if more or less than number valence e-

not enough e- (Be or B)

odd number e- (at the end, take away from least electronegative element--NO₂ is weird)

too many e- (expand octets--in row 3 or lower, extra e- on central atom)

bond or lone pair each count as one

dependent on atoms (terminal) around central atoms

where the atoms can be based on number of e- groups

valence shell e- pair repulsion

e- groups arrange themselves around atoms to maximize distance between them

linear: 180°

trigonal planar: 120°

trigonal bipyramid: 90°, 120°, 180°

(t-shaped: 90°, 180°

linear: 180°)

octahedral: 90°, 180°

A: central atom

X: terminal atom

E: lone pair

only count lone pairs on central atom

start with an s orbital

need as many hybrid orbitals as e- groups

end with as many hybrid orbitals as starting atoms

mix in p orbitals to get proper number

add d orbitals when necessary

form σ bonds or hold lone pairs

π bonds with unhybridized p orbitals

head-to-head overlap of hybrid orbitals

first bond between any 2 atoms

side-to-side overlap of unhybridized p orbitals

any multiple bonds

cannot be rotate

each p orbital can only form 1 π bond, not 2

how many σ bonds and π bonds in a single bond?

double bond?

triple bond?

1 σ, 0 π

1 σ, 1 π

1 σ, 2 π