Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Organic Chemistry I > Chapter 1: Bonding In Organic Compounds > Flashcards

Chapter 1: Bonding In Organic Compounds Flashcards

(74 cards)

Start Studying
1
Q

Organic Chemistry

A

of structure, properties and reactions of organic materials (matter that contains carbon atoms)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

how are carbon atoms linked in organic compounds

A

one or more atoms of carbon are covalently linked to atoms of other elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what are the most common atoms of other elements that carbon is linked to in organic compounds

A
  • hydrogen
  • oxygen
  • nitrogen
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what are not organic compounds

A

carbides, carbonates and cyanides

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

in 1828, who discovered another way that urea can be produced

A

Freidrich Wohler discovered that urea can be produced from inorganic compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

how is each orbital characterized

A

by a unique set of quantum numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

principal quantum number (n)

A

a whole number that specifies the electron shell and it related to the energy of the orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

angular momentum quantum number (s,p,d,f)

A

describes the shape of the orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

spin quantum number

A

the spin of an electron, it will be +1/2 or -1/2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what is the angular momentum quantum number of carbon

A

1s^2,2s^2,2p^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what is the probability of finding an electron in the s orbital

A

this is where the probability is high, 90-95%

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

shape of s orbitals?

A

spherically symmetric

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

shape of p orbitals?

A

like dumbells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

for what n numbers are p orbitals possible and not possible

A

not possible for n=1, but are possible for n=2 and higher

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

when n is greater than one, how many p orbitals are there per n value

A

there are 3 p orbitals for every value of n

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

octet rule

A

maximum stability results when an atom is isoelectronic with a noble gas, aka has 8 electrons in its valence shell (same as noble gases)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what is it called when an electron pair is shared between 2 atoms

A

a covalent bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

when is the octet rule most useful

A

in cases involving covalent bonds to Carbon, nitrogen, oxygen and fluorine (CNOF)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is another name for a double bond

A

a pi bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what is electronegativity

A

a measure of the ability of an element to attract electrons towards itself when bonded to another element

an electronegative element attracts electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

who made the electronegativity scale and what is it

A

Pauline made the scale and it goes from 0-4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

what is the most electronegative element

A

fluorine (F) (4)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

how does a polar covalent bond happen

A

it is when atoms share electrons in their bond still, but not equally

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

relationship between electronegativity and polarity of a bond

A

the greater the difference in electronegativity, the more polar the bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
what is a dipole moment a measure of
it is a measure of the polarity of a bond, so more polar bonds mean a higher dipole moment
26
give an example of dipole moment and polarity using fluorine
since fluorine is the most electronegative, it will have the most polarity in a bond, and will therefore have the highest dipole moment
27
what is formal charge
the charge calculated for an atom in a lewis structure
28
what is the net charge
the sum of the formal charges
29
what does the formal charge correspond to the difference of
the difference between the number of valence electrons an atom has in the neutral free atom and the valence electron count for a covalently bonded atom
30
formal charge is shown as...
a + or - on a diagram
31
what is connectivity/constitution
the order in which the atoms of a molecule are connected
32
why is the constitution important in terms of lewis structure
they are necesary to write a lewis structure
33
what are isomers
different compounds that have the same molecular formula
34
what are constitutional isomers
isomers that differ in the order in which atoms are connected
35
what is another name for constitutional isomers
structural isomers
36
what is a condensed formula
it is abbreviated from the lewis structure and lists the groups of atoms in order ex) CH3CH2NH2
37
can 2 or more lewis structures be written for certain compounds or ions?
yes
38
when are lewis structures called resonance structures?
when they have the same connectivity of atoms and the same number of electrons and the same net charge
39
what is a resonance hybrid
when molecules exist as an average of the resonance structures is just the average of the resonance structures
40
what is the relationship between resonance and stability
the more resonance, the more stable, because it can't move as much and there is more structure
41
8 Rules for Resonance Structures
1. the atom connectivity must be the same (atoms can't just totally move) 2. Each must have the same number of electrons and the same net charge 3. Must have the same number of unpaired electrons (dots in lewis structure) 4. Second row elements (ex. N) must not have more than 8 valence electrons (can't have 10, for example) 5. The structure with the most bonding electron pairs is the most important ( for its chemical properties) (so double bond over single bond) 6. The structure with the lower amount of charged atoms is more important 7. The negative charge should be on the most electronegative atom and the positive charge should be on the least electronegative atom 8. Resonance structures show electron delocalization and this electron delocalization stabilizes molecules. Resonance stabilization is highest if the resonance structures are equally stable
42
3 main reasons why resonance structures are so important
1. resonance structures and resonance hybrids better represent delocalization of electrons between atoms 2. resonance structures help understand reactivity 3. molecules or ions in which the electrons are delocalized are unusually stable
43
relationship between NG and stability
the higher the NG content, the less stable
44
when rxns form unstable products...
the reaction takes longer
45
what is the most stable arrangement of groups attached to a central atom
when there is maximum separation (so the degree angle) between electron pairs
46
in molecules such as water, what determines the overall shape (for example, bent)
the nonbonding electron pairs
47
is valence shell electron repulsions more or less for bonded electron pairs
bonded electron pairs have less repulsion than nonbonded electron pairs, because they are kinda stuck together
48
linear arrangement special rule
4 electron double bonds and 6 electron triple bonds are considered one group of electrons in terms of spatial requirements and therefore are linear. an example of this is carbon dioxide
49
what is a dipole moment of a molecule
the sum of the individual dipoles, which happen when there are polar bonds
50
what happens if the dipoles cancel (arrows go in opposite directions)
the net dipole moment is zero (this is the only time that the dipole is zero)
51
how are reactivity and properties of molecules determined
by their strength and polarity STRUCTURE = FUNCTION
52
what are curved arrows used for
to track the flow of electrons in chemical reactions
53
how to the curved arrows work
the arrow begins where the electrons were originally and points to where they end up
54
what do X's mean
halogens
55
multiple curves arrows
can show how a reaction progresses, for example they can show a proton transfer reaction. can also show the movement of bonding electron pairs
56
IN THE PRESENCE OF ACID
H2O CAN BE PROTONATED
57
a bronsted acid is a
proton donor
58
a bronsted base is a
proton acceptor
59
in an acid base reaction, a proton is transferred from the...
acid to the base proton donor => proton acceptor
60
what are the acids and bases converted to in an acid-base reaction
a conjugate acid and conjugate base
61
strong acids have _______ Ka's and _______ pKa's
high, low
62
the stronger the acid, the ____________ its conjugate base
weaker
63
what are the major factors that affect the acidity (3)
- strength of the bond to hydrogen - electronegativity of the atoms from which the proton is lost - electron delocalization in the conjugate base
64
what happens to the bond to the hydrogen as the halogen size increases
the bond to the hydrogen becomes weaker | charge on the conjugate base is more spread out with the larger halide anions
65
why does electronegativity increase across the periodic table
the increased polarity of the bond to hydrogen increases the partial charge on the hydrogen which increases the electronegativity
66
what is the relationship between electronegativity and acidity
electronegative elements can influence acidity by the inductive effect. The electron withdrawing effect increases the partial positive charge and stabilizes the conjugate base
67
what happens to the acid when the conjugate base is stabilized by electron delocalization
the acid is stronger
68
what type of acid and base does equilibrium favor in an acid-base reaction
equilibrium favors the weaker acid and weaker base
69
how do you calculate the equilibrium constant
Ka of reactant acid/Ka of product acid
70
how can you predict the direction of proton transfer
use the pKa's for example, the wekaer acid has a higher pKa, and so the higher pKa is favored at equilibrium
71
Lewis acid
electron pair acceptor
72
lewis base
electron pair donor
73
lewis acid-base reaction
a non bonding electron pair on the base bonds to the acid. the acid and base may or may not have a formal charge
74
what is the lewis acid base idea also relevant to
substitution reactions and bronsted lowry proton transfer reactions

Organic Chemistry I (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions