Chem Subject Test 1 And 2 "bonding"

Front 1

Ionic bonding

Back 1

between metal and nonmetal

involve transfer of e-

electron in the bond leave one atom (cation) and are held by anion

Front 2

Covalent Bonding

Back 2

btw nonmetals

sharing of e-
-equally
-nonequally (polar)

Front 3

metallic bonds

Back 3

occur in transition metal atoms.

electron are spread out through entire material
"sea of electron"

Front 4

van der waals bonds

Back 4

weak intermolecular forces

aka london dispersion force

Front 5

hydrogen bond

Back 5

occurs when hydrogen atom bonded to a strongly electronegative atom (FON) interacts with the electronegative atom on another molecule

Front 6

intermolecular and intramolecular bond

Back 6

intramolecular bond
-ionic, covalent, metallic

interamolecular bond
-van der waals
-hydrogen bonding

Front 7

exception to octet rule

Back 7

P, Se, Br more than 8 valence e-

Front 8

incomeplete octet

Back 8

H, Be, B

Front 9

resonance structure

Back 9

more than one lewis representation due to delocalized e-

lewis structure with smallor no formal charge is prefered ovwer a lweis structure w/ large formal charge

negative formal charge placed on more electronegative atom is more stable than one in which the charge are placed on less electronegative atoms

Front 10

formal charge

Back 10

Valence E -[1/2 #bonding e + # nonbonding e]

Front 11

VSEPR

Back 11

valence shell electron-pair repulsion theory

arrangement of atos or groups around the central atom is determined by the repulsions btw the e- pairs in the valence shell of central atom

lone pairs do participate in the repulson but they do not in overall naming process

lone pair act as bonds in repulsion but the fact that they are nonbonding makes their repulsion stronger than bonding pair

Front 12

SP

Back 12

2 e-
liner
180

Front 13

SP2

Back 13

3 e-
trigonal planer
120

Front 14

SP3

Back 14

4e- (1 lone pair)
trigonal pyramid
107

4 e- (0 lone pair)
tetrahedral
109

Front 15

SP3d

Back 15

5 e- (0 lone pair)
trigonal bipyramid
90,120, 180

5e- (1lone pair)
see saw
90 120 180

5e[ (2lone pair)
T shape
90 18-

5e- (3lonepair)
linear
180

Front 16

SP3d2

Back 16

6 e- (0 lone pair)
octahedral
90 180

6e- (1lonepair)
planar pyramid
90 180

6e- (2 lone pair)
square pyramid
90 180

Front 17

compare bond distance btw single, double, triple

Back 17

triple<double<single

Front 18

compare bond enerey btw single, double, triple

Back 18

single<double<triple

Front 19

paramagnetic does what to magnetic field?

Back 19

drawn weakly to magnatic field

paramagnetic compound has odd number of valence electron
NO (5+6=11)

Front 20

draw lewis structure of the most likely ions of elementsfrom Na to Ca

Back 20

Na+ Ma2+, Al3+, Si4+,
P3-, S2-, Cl-, Ar
K+, Ca 2+

nonmetal starting P gain e-

Front 21

steps in drawing lewis structure

Back 21

1. find how many e- you have
2. find how many u need (must satisfy octet)
3. subtract (need-has) e-
4. divide by 2 and get how many bonds

5. finally check for the formal charge. no formal chage is the best structure and then - F.C on more electronegative atoms.

Front 22

arrange the following compounds in order of increasing boiling point

C2H6, CH3OH, LiF, HCL

Back 22

C2H6<HCL<CH3OH<LiF

C2H6-vander waals

HCl-dipole

CH3OH-Hbondig

LiF-Ionic

Front 23

electronic geometry

Back 23

position of all electron both bonding and nonbonding

angle of e- consider electron geometry

Front 24

molecular geometry

Back 24

position of nuclie

name of shape like bent

only consider molecular geometry

Front 25

bond dipole vs molecular dipole

Back 25

molecular dipole depends on bond dipole and molecular geometry of all bonding pairs