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orgo > exam 1 (txtbook) > Flashcards

exam 1 (txtbook) Flashcards

1
Q

nucleus contains..

A

protons and neutrons

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2
Q

electron cloud contains

A

electrons

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3
Q

cation is

A

positively charged and has fewer electrons than protons

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4
Q

anion is

A

negatively charged and has more electrons than protons

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5
Q

mass number is

A

the total number of protons and neutrons in the nucleus

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6
Q

isotopes have different…

A

mass numbers

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7
Q

atomic weight is

A

the weighted avg of the mass of all its isotopes in AMU

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8
Q

shells are numbered…

A

1, 2, 3

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9
Q

types of orbitals?

A

s, p, d, f

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10
Q

each shell contains a certain number of

A

orbitals

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11
Q

an orbital is a region of space that is

A

high in electron density

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12
Q

each orbital can have a max of

A

2 electrons

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13
Q

what is higher in E: s or p orbital?

A

p orbitals

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14
Q

first row of PT has only

A

one orbital in the first shell (1s orbital)

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15
Q

second row of PT has a

A

filled first shell of electrons (all 2nd row elements have a 1s2 configuration)

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16
Q

second row can accept

A

2s orbital
3 2p orbitals (8 e- max)

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17
Q

outer most electrons are

A

valence electrons

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18
Q

because each of the four orbitals in the second shell can hold two electrons, there is a

A

max of 8 electrons for elements in the second row

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19
Q

group number of second row elements reveals

A

its number of valence electrons

i.e. carbon in group 4A = 4 valence electrons

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20
Q

joining two or more compounds =

A

COMPOUNDS

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21
Q

through bonding, atoms attain a

A

complete outer shell of valence electrons

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22
Q

through bonding: atoms gain/lose/share electrons to

A

attain the electronic configuration of the noble gas closest to them in the PT

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23
Q

a first row element like hydrogen can accomodate…

A

two electrons around it

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24
Q

a second row element is generally

A

most stable with eight valence electrons around it like neon

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25
Q

octet rule

A

elements with 8 valence electrons around it

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26
Q

ionic bonding is

A

the result of transferring electrons from one element to another

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27
Q

covalent bonding is

A

the result of sharing electrons b/w two nuclei

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28
Q

type of bonding is determined by location of…

A

an element in the PT

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29
Q

ionic bond generally occurs when elements on

A

far left side of the PT combine w far right side elements

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30
Q

resulting ions from ionic bonding are held…

A

together by extremely strong electrostatic interactions

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31
Q

a positively charged cation formed from the

A

element on the left side attracts an anion formed from the right side elements

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32
Q

examples of ionic inorganic compounds?

A

NaCl, KI

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33
Q

covalent bonding occurs with elements in the

A

middle of the PT and between elements on same side of the tablea

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34
Q

a covalent bond is a

A

two electron bond

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35
Q

compound with covalent bonds is called

A

a compound

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36
Q

how to calculate the predicted number of bonds

A

8 - number of valence electrons

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37
Q

atoms with 1, 2, 3, or 4 valence electrons form

A

1, 2, 3, 4 bonds respectively in neutral molecules

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38
Q

when second row elements form fewer than four bonds…

A

their octets consist of both bonding electrons and nonbonding electrons

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39
Q

unshared electrons are also called

A

lone pairs

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40
Q

lewis structures are

A

electron dot representations for molecules

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41
Q

three rules for lewis structures

A

1) draw only valence electrons
2) give every 2nd row element no more than 8 electrons
3) give each hydrogen two electrons

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42
Q

formal charge =

A

of valence electrons - number of electrons an atom ‘owns’

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43
Q

an atom owns all of its..

A

unshared electrons and half of its shared electrons

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44
Q

number of electrons owned =

A

number of unshared electrons + 1/2 (number of shared electrons)

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45
Q

the sum of the formal charges on the individual atoms =

A

the net charge on the molecule or ion

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46
Q

exceptions to the octet rule?

A

hydrogen because it accommodates only 2 electrons in bonding

  • additionally boron and beryllium, phosophorus, sulfur
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47
Q

resonance structures are formed when

A

there are multiple lewis structures for a molecule

  • same placement of atoms but a different arrangement of electrons
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48
Q

resonance hybrid

A

shows characteristics of both resonance structures

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49
Q

resonance allows

A

certain electron pairs to be DELOCALIZED over two or more atoms, adding stability

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50
Q

resonance stabilized means

A

a molecule has two or more resonance structures

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51
Q

are resonance structures real?

A

no (don’t accurately represent the structure of a molecule or ion)

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52
Q

are resonance structures in equilibrium?

A

no (no movement of electrons from one form to another)

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53
Q

are resonance structures isomers?

A

no - they differ ONLY in the arrangement of electrons

two isomers are different because of the arrangement of atoms AND electrons

54
Q

how to draw a resonance structure

A

1) two RS differ in position of multiple bonds and non-bonded electrons
2) placement of atoms and single bonds ALWAYS stays the same
3) two RS must have the same number of unpaired electrons
4) MUST BE VALID LEWIS STRUCTURES. hydrogen must have two electrons and a second-row element can have no more than 8 electrons

55
Q

curved arrow notation is…

A

a convention that shows how electron position differs between the two resonance forms

56
Q

curved arrow always

A

begins at an electron pair; ends at an atom or bond

57
Q

what are carbocations?

A

positively charged carbon atoms that are unstable intermediates because they contain a carbon atom lacking an octet of electrons

58
Q

“exceptions” to resonance structures?

A
  • RS can NEVER have more than 8 electrons (i.e. carbon can’t have 10 electrons)
  • RS CAN have an atom with fewer than 8 electrons
59
Q

what are heteroatoms?

A

an atom other than carbon or hydrogen

60
Q

what is a resonance hydrid?

A

composite of all possible resonance structures (electrons pairs are drawn in diff locations in individual resonance structures are delocalized)

61
Q

is the resonance structure more stable?

A

YES, because the resonance hybrid is more stable than any resonance structure because it delocalizes electron density over a larger volume

62
Q

when all resonance forms are identical…

A

each resonance form contributes equally to the hybrid

63
Q

when two resonance structures are different…

A

the hybrid looks more like the “better” resonance structure

64
Q

the major contributor is the…

A

“better” resonance structure

65
Q

minor contributors are…

A

all the other resonance structures

66
Q

the hybrid is the…

A

weighted average of the contributing resonance structures

67
Q

what makes a resonance structure ‘better’?

A
  • more bonds
  • fewer charges
68
Q

two common differences amongst resonance structures?

A

1) position of a multiple bond

2) site of charge

69
Q

notation for double bond position?

A

use a dashed line for a bond that is single in one resonance structure and double in another

70
Q

notation for location of charge?

A

partial neg charge and partial pos charge for an atom that is neutral in one RS and charged in the other

71
Q

what is bond length?

A

average distance between center of two bonded nuclei (reported in pm - picometers)

72
Q

trend for bond length?

A

decreases across a row of the PT as atom size DECREASES

73
Q

bond length increases…

A

down a column as atom size INCREASES

74
Q

what does bond angle determine?

A

the shape around any atom bonded to two other atoms

75
Q

to determine the bond angle and shape around a given atom…

A

first count how many groups surround the atom

76
Q

a group is either an

A

atom or a lone pair of electrons

77
Q

use (x) to determine the shape

A

VSEPR (based on the fact that electron pair repel each other)

78
Q

second row element has only three possible arrangements:

A

two groups (linear, 180)
three groups (trigonal planar, 120)
four groups (tetrahedral, 109.5)

defined by the number of the grounds surrounding it

79
Q

any atom surrounded by only two groups is…

A

LINEAR and has a bond angle of 180 degrees

  • no lone pair = 180 degree bond angle
80
Q

any atom surrounded by three groups is…

A

trigonal planar and has bond angles of 120 degrees

  • no lone pair = 120 degrees
81
Q

any atom surrounded by four groups is…

A

tetrahedral and has bond angles of ~109.5 degrees

81
Q

molecular shape of ammonia and water?

A

trigonal pyramidal (bond angle is 107 degrees)

  • one of the groups around N is a nonbonded electron pair
82
Q

types of shorthand representations used for organic compounds

A

condensed
skeletal

83
Q

condensed structures rules

A

1) all atoms are drawn in but two-electron bond lines are generally omitted
2) atoms are usually drawn next to the atoms to which they are bonded
3) parentheses are used around similar groups bonded to the same atom
4) lone pairs are omitted

84
Q

to interpret a condensed formula…

A

best to start at left side of molecules and MAKE SURE THAT carbon atoms are tetravalent

85
Q

skeletal structures rules

A

1) assume a carbon is located at the junction of any two lines or at the end of any line
2) assume each carbon has enough hydrogens to make it tetravalent
3) drawn in all heteroatoms and hydrogens directly bonded to them

86
Q

lowest energy arrangement of all electrons is…

A

the ground state

87
Q

a sigma bond is…

A

a single bond

  • concentrates electron density on the axis that joins 2 nuclei
88
Q

hybridization is…

A

the combo of two or more atomic orbitals to form the same number of hybrid orbitals

  • each having the same shape and energy
89
Q

one 2s orbital and three 2p orbitals =

A

four sp3 hybrid orbitals

90
Q

one 2s orbital and two 2p orbitals =

A

three sp2 hybrid orbitals

91
Q

one 2s orbital and one 2p orbitals =

A

two sp hybrid orbitals

92
Q

sp2 and sp hybridization leave…

A

one and two 2p orbitals unhybridized on each atom

93
Q

forming two sp hybrid orbitals uses

A

one p and two p orbitals, leaving two 2p orbitals unhybridized

94
Q

forming three sp2 hybrid orbitals uses

A

one 2s and two 2p orbitals, leaving one 2p orbital unhybridized

95
Q

types of hybrid orbitals

A

2 groups, 2 orbitals used, two sp hybrid orbitals

3 groups, 3 orbitals, three sp2 hybrid orbitals

4 groups, 4 orbitals, four sp3 hybrid orbitals

96
Q

what orbitals are used to form the two bonds of the C-C double bond?

A

b/c C has 4 valence electrons, each of these orbitals has one electron that can be used to form a bond

  • remember: sp2 hybrid orbitals are formed from one 2s and two 2p orbitals, leaving one 2p orbital unhybridized
97
Q

pi bond is..

A

weaker than sigma bonds

98
Q

sigma bond is formed by

A

end on overlap of two sp2 hybrid orbitals

99
Q

pi bond is formed by

A

side by side overlap of two 2p orbitals

100
Q

carbon-carbon triple bond has three components:

A

1) a sigma bond formed by end on overlap of two sp hybrid orbitals
2) two pi bonds formed by side by side overlap of two sets of 2p orbitals

101
Q

covalent bonding in carbon compounds

A

4 groups bonded to C, sp3 hybridization, 109.5 degrees, one sigma bond

3 groups, sp2, 120 deg, one sigma + one pi bonds

2 groups, sp, 180 deg, one sigma + two pi bonds

102
Q

as number of electrons between two nuclei increases…

A

bonds become shorter and stronger

103
Q

triple bonds are shorter ad stronger than double bonds which are

A

shorter and stronger than single bonds

104
Q

double bonds consisting of…

A

both a sigma and pi bonds are stronger

105
Q

the pi component of the double is

A

weaker than the sigma component

106
Q

higher hybridization means

A

decreasing bond strength

107
Q

increasing bond length means

A

weaker bonds

108
Q

percent s character indicates

A

the fraction of a hybrid orbital due to the 2s orbital used to form it

109
Q

sp hybrid has how much s character

A

one 2s orbital / two hybrid orbitals = 50% s character

110
Q

sp2 hybrid

A

one 2s / three hybrid = 33% s character

111
Q

sp3 hybrid

A

one 2s orbital / 4 hybrid orbitals = 25% s character

112
Q

as s-character increases…

A

a hybrid orbital holds its electron closer to the nucleus and the bond becomes shorter/stronger

113
Q

electronegativity is the measure of

A

an atom’s attraction for electrons in a bond (increases as a row of PT, decreases down a column)

114
Q

carbon carbon bond is

A

nonpolar

115
Q

c-h bonds are

A

nonpolar b/c electronegativity diff is small

116
Q

c-o bond is

A

polar/polar covalent

  • has a dipole (partial separation of charge)
117
Q

usually a polar bond will be one in which the

A

electronegativity difference between two atom is > 0.5 unit

118
Q

electrostatic potential map shows

A

the distribution of electron density in a molecule

119
Q

because alkanes have no functional group, they are…

A

much less reactive than other organic compounds

120
Q

alkanes are aliphatic hydrocarbon having only…

A

C–C and C–H sigma bonds

121
Q

because their carbon atoms can be joined together in chains or rings…

A

alkanes can be categorized as acyclic or cyclic

122
Q

acyclic alkanes have the molecular formula…

A

CnH2n+2 where n = an integer

123
Q

acyclic alkanes contain only

A

linear and branched chains of carbon atoms

124
Q

acyclic alkanes are also called

A

saturated hydrocarbons b/c they have the max number of hydrogen atoms per carbon

125
Q

cycloalkanes contains carbons…

A

joined in one or more rings

126
Q

general formula of cycloalkanes?

A

CnH2n

127
Q

cycloalkanes have fewer

A

H atoms than an acyclic alkane with the same number of carbons

128
Q

what are isomers?

A

two different compounds with the same molecular formula (constitutional or stereoisomers)

129
Q

drugs have three names:

A

systemic: follows nomenclature rules and indicates IUPAC name
generic: official name
trade: name assigned by manufacturing company

130
Q

skip

A

skip

orgo (6 decks)

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