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chemistry > organic chem chapter 1 > Flashcards

organic chem chapter 1 Flashcards

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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
contains different number and kinds of orbital
electron shell
26
each orbital has a maximum of ___ electrons
2
27
each orbital has a maximum of
2 electrons
28
______ of atom is listing of orbitals that the atoms electrons occupy
ground state electron configuration
29
what principle that electrons will fill the lower energy levels moving to higher energy orbitals
Aufbau principle
30
what principle that can only occupy two electrons in orbital in opposite spin
Pauli-Exclusion principle
31
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
Hund's rule
32
who proposed all organic compound and state that carbon is tetravalent that laways form four bonds when joint to another element
August Kekule and Archibald Couper
33
who proposed all organic compound and state that carbon is tetravalent that laways form four bonds when joint to another element
August Kekule and Archibald Couper
34
who stated that carbon atoms can bond to another atom to form extended chain of link atoms
August Kekule
35
What did Jacob van't Hoff and Joseph Le bel proposed
4 bonds to carbon are not oriented randomly but specific spatial direction
36
what does solid lines represent
bonds in plane page
37
heavy wedge line represent
coming towards the viewer
38
dashed lines represent
behind or back from the viewer
39
draw a tetrahedral carbon atom
40
why do atoms bond together
to result stability compound lower in energy that separate atoms .
41
when bonds forms
release energy and flows out chemical system
42
electrons in outermost shell bond are formed, the valence shell would contain 8 electrons
valence electrons
43
when metals bond to nonmetals
ionic bonds
44
have low ionixation energy and easy to release electrons
metals
45
have high electrons affinites and accept electrons
non metals
46
what are the two types of bonds
ionic and covalent bond
47
shared electrons hold atoms together by attracting nuclei both atoms
covalent bond
48
proposed shared electrons bonds
Lewis
49
neutral group of atoms held together by covalent is called
molecule
50
what is the simpliest way in indicating covalent bonds in molecules
lewis structure
51
non-bonding electrons that are not used for bonding is called
lone pairs electrons
52
why cant and organic molecule have formula c2h7
since it has too much hyfrogen for 2 carbons
53
how does electrons sharing lead to bonding between two atoms
(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
how close are the two nuclei in H2 molecule?
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
there is an optimum distance between nuclei ug H2 that leads to maximum stability called
bond length
56
how many Bond length are there in H2
74 pm
57
what did Linus Pauling proposed
that and s orbital and three p can combine or hybridize to form 4 equivalent atomic orbital with tetrahedral orientation
58
tetrahedrally oriented orbitals are callled
sp3
59
why does carbon atoms form four tetrahedral bonds?
because sp3 orbitals form stronger bonds than the unhybrid s or p orbitals
60
bond angle of sp3
109.5 celcius
61
bond angle of sp2
120
62
bond angle of sp
180
63
bond angle of linear
64
H3C-CH3
SP3
65
H2C-CH3
SP2
66
CH---
SP
67
H2C--CH3
SP2
68
HC---CH
SP
69
what bond is the stronger bond?
sp3
70
geometry of sp3
tetrahedral
71
geometry of sp2
planar
72
geometry of sp
linear
73
carbon to carbon bond length of sp3, sp2 and sp
sp3- 154 pm sp2- 133 pm sp-120 pm
74
what is non-polar covalent bond
equal sharing of valence electrons and two nonmetallic atoms of the same electronegativitity
75
polar covalent bond
-two nonmetallic atoms with different electronegativity -unequal sharing of electrons -bonding electrons are attracted towards more electronegative atom
76
a bond between atoms whith similar electronegativity is
nonpolar covalent
77
a bond between atom that electronegativity is less than 2 units is
polar covalent
78
a bond between atom that electronegativity by two units or large is
ionic
79
what color is electron rich
red
80
what color is electron rich
red
81
what color is electron poor
blue
82
what does cross arrow indicate
the direction bond polarity the tail is electron poor and head is electron rich
83
what does cross arrow indicate
the direction bond polarity the tail is electron poor and head is electron rich
84
what does inductive effect means
shift electrons in polar bond response to electronegativity
85
what does inductive effect means
shift electrons in polar bond response to electronegativity
86
when atom is more electronegative than carbon then
electrons are attracted to X
87
when atom is less than electronegative than carbon then it is
attracted to C
88
when atom is less than electronegative than carbon then it is
attracted to C
89
1 cal how many J
4186 J

chemistry (8 decks)

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