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chemistry > organic chem chapter 1 > Flashcards

organic chem chapter 1 Flashcards

1
Q

organic chemistry interaction allows us to

A

see, smell, fight,feel

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2
Q

what year that the term organic chemistry was used to mean chemistry of compound found in living organism

A

1700

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3
Q

low melting solid and more difficult to isolate, purify and work with high metals

A

organic compound

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4
Q

more than 99 percent of known chemical contains

A

carbon

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5
Q

what makes carbon special?

A
  • electronic structure of carbon
    -4A element that can share 4 valence electrons and form 4 covalent bond
  • carbon atoms can bond to one another by forming chain or ring
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6
Q

what makes carbon special?

A
  • electronic structure of carbon
    -4A element that can share 4 valence electrons and form 4 covalent bond
  • carbon atoms can bond to one another by forming chain or ring
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7
Q

what are the common elements found in periodic table

A

H,C, N, O,F,Si,Cl,Br,I

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8
Q

what is the m of an atom

A

2x 10-10 m

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9
Q

what is the m of nucleus

A

10-14 to 10-15 m

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10
Q

electrons

A

10-10 m

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11
Q

specific atoms can be describe

A

atomic number and its mass number gives total number of protons plus neutrons in its nucleus.

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12
Q

atoms of given element has same atomic number but differ in mass depending on how many ________ contain

A

neutrons

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13
Q

atoms with same atomic number but different in mass number called

A

isotopes

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14
Q

weighted average mass unit of an element naturally occuring isotopes

A

atomic mass

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15
Q

behavior f specific electron in an atom can be describe by a mathematical expression called

A

wave equation

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16
Q

the solution to a wave equation called

A

wave function or orbital

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17
Q

it can be define region of space around the nucleus where electrons are found

A

orbitals

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18
Q

it can be define region of space around the nucleus where electrons are found

A

orbitals

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19
Q

what are the orbitals

A

s,p,d,f

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20
Q

what are the most common orbital of organic biological chemistry

A

s and p

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21
Q

what is the spherical with nucleus at center

A

s orbital

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22
Q

it is a dumbell shaped can be oriented space along three perpendicular directions denoted as px,py,pz

A

p orbital

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23
Q

the two parts of p orbital have differ algebraic sign (+ and -) in wave function and separated by region of zero electron density called

A

node

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24
Q

the two parts of p orbital have differ algebraic sign (+ and -) in wave function and separated by region of zero electron density called

A

node

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25
Q

contains different number and kinds of orbital

A

electron shell

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26
Q

each orbital has a maximum of ___ electrons

A

2

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27
Q

each orbital has a maximum of

A

2 electrons

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28
Q

______ of atom is listing of orbitals that the atoms electrons occupy

A

ground state electron configuration

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29
Q

what principle that electrons will fill the lower energy levels moving to higher energy orbitals

A

Aufbau principle

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30
Q

what principle that can only occupy two electrons in orbital in opposite spin

A

Pauli-Exclusion principle

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31
Q

what rule that two or more empty orbital of equal energy are available, one electron must occupy each with the spins parallel until all orbitals are filled

A

Hund’s rule

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32
Q

who proposed all organic compound and state that carbon is tetravalent that laways form four bonds when joint to another element

A

August Kekule and Archibald Couper

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33
Q

who proposed all organic compound and state that carbon is tetravalent that laways form four bonds when joint to another element

A

August Kekule and Archibald Couper

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34
Q

who stated that carbon atoms can bond to another atom to form extended chain of link atoms

A

August Kekule

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35
Q

What did Jacob van’t Hoff and Joseph Le bel proposed

A

4 bonds to carbon are not oriented randomly but specific spatial direction

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36
Q

what does solid lines represent

A

bonds in plane page

37
Q

heavy wedge line represent

A

coming towards the viewer

38
Q

dashed lines represent

A

behind or back from the viewer

39
Q

draw a tetrahedral carbon atom

A
40
Q

why do atoms bond together

A

to result stability compound lower in energy that separate atoms .

41
Q

when bonds forms

A

release energy and flows out chemical system

42
Q

electrons in outermost shell bond are formed, the valence shell would contain 8 electrons

A

valence electrons

43
Q

when metals bond to nonmetals

A

ionic bonds

44
Q

have low ionixation energy and easy to release electrons

A

metals

45
Q

have high electrons affinites and accept electrons

A

non metals

46
Q

what are the two types of bonds

A

ionic and covalent bond

47
Q

shared electrons hold atoms together by attracting nuclei both atoms

A

covalent bond

48
Q

proposed shared electrons bonds

A

Lewis

49
Q

neutral group of atoms held together by covalent is called

A

molecule

50
Q

what is the simpliest way in indicating covalent bonds in molecules

A

lewis structure

51
Q

non-bonding electrons that are not used for bonding is called

A

lone pairs electrons

52
Q

why cant and organic molecule have formula c2h7

A

since it has too much hyfrogen for 2 carbons

53
Q

how does electrons sharing lead to bonding between two atoms

A

(Valence bond theory,)
1.the covalent bonds form when two atoms approach to one another and one atom overlap to on other atom
2. the electrons are now paired with overlapping orbitals
3. electrons attract to both nuclei of atoms

54
Q

how close are the two nuclei in H2 molecule?

A

not to close yet not to far, if they are too close they will repel each other and if they are too far apart they wont able to share bonding electrons

55
Q

there is an optimum distance between nuclei ug H2 that leads to maximum stability called

A

bond length

56
Q

how many Bond length are there in H2

A

74 pm

57
Q

what did Linus Pauling proposed

A

that and s orbital and three p can combine or hybridize to form 4 equivalent atomic orbital with tetrahedral orientation

58
Q

tetrahedrally oriented orbitals are callled

A

sp3

59
Q

why does carbon atoms form four tetrahedral bonds?

A

because sp3 orbitals form stronger bonds than the unhybrid s or p orbitals

60
Q

bond angle of sp3

A

109.5 celcius

61
Q

bond angle of sp2

A

120

62
Q

bond angle of sp

A

180

63
Q

bond angle of linear

A
64
Q

H3C-CH3

A

SP3

65
Q

H2C-CH3

A

SP2

66
Q

CH—

A

SP

67
Q

H2C–CH3

A

SP2

68
Q

HC—CH

A

SP

69
Q

what bond is the stronger bond?

A

sp3

70
Q

geometry of sp3

A

tetrahedral

71
Q

geometry of sp2

A

planar

72
Q

geometry of sp

A

linear

73
Q

carbon to carbon bond length of sp3, sp2 and sp

A

sp3- 154 pm
sp2- 133 pm
sp-120 pm

74
Q

what is non-polar covalent bond

A

equal sharing of valence electrons and two nonmetallic atoms of the same electronegativitity

75
Q

polar covalent bond

A

-two nonmetallic atoms with different electronegativity
-unequal sharing of electrons
-bonding electrons are attracted towards more electronegative atom

76
Q

a bond between atoms whith similar electronegativity is

A

nonpolar covalent

77
Q

a bond between atom that electronegativity is less than 2 units is

A

polar covalent

78
Q

a bond between atom that electronegativity by two units or large is

A

ionic

79
Q

what color is electron rich

A

red

80
Q

what color is electron rich

A

red

81
Q

what color is electron poor

A

blue

82
Q

what does cross arrow indicate

A

the direction bond polarity
the tail is electron poor and head is electron rich

83
Q

what does cross arrow indicate

A

the direction bond polarity
the tail is electron poor and head is electron rich

84
Q

what does inductive effect means

A

shift electrons in polar bond response to electronegativity

85
Q

what does inductive effect means

A

shift electrons in polar bond response to electronegativity

86
Q

when atom is more electronegative than carbon then

A

electrons are attracted to X

87
Q

when atom is less than electronegative than carbon then it is

A

attracted to C

88
Q

when atom is less than electronegative than carbon then it is

A

attracted to C

89
Q

1 cal how many J

A

4186 J

chemistry (8 decks)

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