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Organic Chem > Exam 2 Flashcards > Flashcards

Exam 2 Flashcards

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1
Q

bonding has what?

A

greater stability so lower energy

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2
Q

octet rule

A

want to get the same number of outer shell electrons as found in noble gases

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3
Q

exception hydrogen as far as octets rule

A

only needs two electrons

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4
Q

ionic bonds is what?

A

a transfer of electrons

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5
Q

covalent bonds are what?

A

sharing of valence electrons

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6
Q

normal valence

A

number of bonds an atom typically forms

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7
Q 
what is the normal valence of 
H, 
O, 
N, 
C
 the halogens F, Cl, Br, and I?
A 
1 or 2
2
3
4
and 1
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8
Q

what does it mean if an atom deviates from normal valencey

A
  1. atom has a formal charge
  2. has an unpaired electron “radical”
  3. there’s an error in the drawing
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9
Q

to draw lewis what do you do first?

A

add up all the electrons and to see how many lone pairs you will need to complete

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10
Q

in drawing lewis structures, what is the second step?

A

move lone pairs to fill up bonds until left full and with rest of pairs

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11
Q

if lewis structure has a formal charge of -1 what do you do?

A

add one electron to the electrons counted.

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12
Q

how do you find a formal charge?

A

compare the number of electrons in the atoms valence shell to that of the number it gets from the addition. if it gets more than one number it has a negative charge, less than gets positive.

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13
Q

formal charge ex.

A

oxygen has seven electrons on lewis but six on periodic table. that means it has an extra electron and has a charge of negative one.

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14
Q

isomers definition

A

compounds with same molecular formula but are different compounds. two types 1) constitutional 2)stereoisomers

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15
Q

constitutional isomer def

A

different atoms are connected to different atoms, i.e a different connectivity

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16
Q

stereoisomers def

A

same connectivity of atoms but different attachment (3D)

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17
Q

exceptions to octet rule

A

hydrogen only needs two electrons not eight

Be and B (boron is electron deficient

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18
Q

2nd row atoms can’t do what?

A

exceed 8 electrons

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19
Q

condensed structural drawing tip

A

let the valence electrons guide you

when drawing lone pair optional but formal charges and unpaired electrons shown

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20
Q

in skeletal bonds assume and do what?

A

assume there are hydrogens to each end carbon unless formal charge or unpaired electrons shown.
draw all atoms other than carbon and hydrogen attached
hydrogens are always connected to carbons

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21
Q

bond length is given in what and it’s measure in what?

what is it’s trend

A

angstroms; 10^-10 meters

decreases as u move up a column or from left to right across a row

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22
Q

bond angle def

A

the average angle between three nuclei

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23
Q

what is the bond lengths in order from shortest to longest?

A 
triple = shortest 
double = medium 
single = longest
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24
Q

vespr stands for what?

A

valence shell electron paid repulsion : states that electron pairs repel each other and result in shapes because they want to be mutually fat away from each other as possible

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25
Q

trigonal planar bond angle and shape

A

~120; looks like a three way baby toy

26
Q

tetrahedral bond angle and shape

A

109.5 except for water which is 104.5. looks like baby toy with extra leg

27
Q

linear bond angle and shape

A

180 and circles in a line

28
Q

tetrahedral with lone pairs bond angle and shape

A

109.5; trigonelle pyramidal with lone pairs on the tippy top

29
Q

tetrahedral bond angle and shape

A

109.5; bent

30
Q

steric number in correlation with shape

A 
#2=linear;180
#3=trigonal planar; 120
#4=tetrahedral; 109.5
#4=tetrahedral; 109.5; trigonal pyramidal 
#4=tetrahedral; 109.5; bent
31
Q

bonds formed by head on overlap of orbitals

A

sigma

32
Q

sideways overlap of parallel orbitals; they most like do what?

A

pi bonds; will likely react and form a bond with another atom; always 90 degrees

33
Q

hybridization is?

A

the mixing of atomic orbitals

34
Q

for any second row element (except F)

A

the atom uses sp3 hybridization

35
Q

what do these signs mean?
________ ?
///////// ?
wedge ?

A

line: in the plane
a dash: going away from you
a wedge: coming towards you

36
Q

any second row atom that has steric number of 3?

A

uses sp2 hybridization

37
Q

a double bond contains?

A

one sigma bond and one pi bond

38
Q

a triple bond in hybridization is what?

A

one sigma bond and two pi bonds

39
Q

which elements don’t hybridize?

A

hydrogen and holden’s (F, Cl, Br, I) not central atoms so form only one bond

40
Q 
steric #:  hybrid? molec.? angle? 
#4.               ?            ?            ?
#3.              ?            ?            ?
#2              ?              ?            ?
A

sp3. tetrahedral 109.5
sp2. trigonal planar. 120
sp. linear. 180

41
Q

to find a positive or negative charge what do you do?

A

complete lewis structure and add up all electrons and then find the valence electrons for periodic table and find the difference of those two numbers. if there is more than the valence it is positive, if there’s if there is less it’s negative, and zero is no charge

42
Q

ionic bond is between?

A

a metal (big EN) and nonmetal (small EN)

43
Q

nonpolar covalent def

A

equal sharing of electrons so basically no charge

44
Q

rule of thumb for polar and non polar:

  1. two atoms is blank than blank (EN)on the pauling scale implies blank
  2. if (EN) is less than blank it will be blankety blank
  3. if EN difference is blankety blank and blank than it’s blankety blank
A
  1. two atoms is greater than two (EN)on the pauling scale implies ionic
  2. if (EN) is less than 0.5 it will be nonpolar covalent
  3. if EN difference is between 0.5 and 2.0 than it’s polar covalent
45
Q

dipôle symbol

A

looks like a u with long front part going down

46
Q

vector:
velocity:

A

magnitude and direction

speed and direction

47
Q

if dipoles cancel out meaning all facing opposite directions equally what happens?

A

bet dipole is zero

48
Q

in a tetrahedral with lone pairs showing where are the dipoles going to point?

A

to the lone pairs

49
Q

trigonal planar with no lone pairs; where are the dipoles?

A

facing away and cancel out

50
Q

key point of V.D.W.

A

larger surface area, greater V.D.W. attraction

51
Q

V.D.W. is for what element?

A

everyone because it only needs two electrons to happen

52
Q

structural forms in V.D.W. comparison?

which atoms are more polarizable

A

branching decreases surface area so the more spread out the better
larger atoms in radius so F is smaller and I bigger

53
Q

dipole dipole interactions

A

stronger than V.D.W.

have to be somewhat polar

54
Q

hydrogen bonds explain with vdw

A

stronger than dipole dipole

requires a hydrogen bond donor and bond acceptor

55
Q

h-bond donor explain

h-bond acceptor explain

A

h is covalently bonded to an electrically negative atom ( usually O or N; sometime F)
a lone pair on a different electron negative atom (usually O or N)

56
Q

compounds that have what and what will be able to do what and tend do have what?

A

h-bond donor
h-bond acceptor
high boiling points

57
Q

boiling points increase as what because of what

A

surface area increase and VDW attractions increase

58
Q

to have a hydrogen bond must have what interaction

A

dipole dipole

59
Q

melting point: more what have higher mp?

A

symmetrical molecules

60
Q

solubility principle

A

like dissolves like

non-polar compounds to non polar solvents and polar compounds to polar solvents

61
Q

why do oil and water not mix?

A

because oil is non polar and water is highly polar

Organic Chem (4 decks)

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