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Chem 104 > OChem (104) > Flashcards

OChem (104) Flashcards

1
Q

Methane

A

CH4

BP -164 degrees C

(gas at room temp)

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2
Q

Ethane

A

CH3CH<span>3</span>

BP -89 degrees C

gas at room temp

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3
Q

Propane

A

CH3CH2CH3

BP -44 degrees C

gas at room temp

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4
Q

Butane

A

CH3CH2CH2CH3

BP -0.5 degrees C

(gas at room temp)

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5
Q

Pentane

A

CH3CH2CH2CH2CH3

BP 36 degrees C

(96 degrees F)

liquid at room temp

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6
Q

HEXANE

A

CH3CH2CH2CH2CH2CH3

BP 68 degrees C

liquid at room temp

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7
Q

Heptane

A

CH3CH2CH2CH2CH2CH2CH3

BP 98 degrees C

liquid at room temp

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8
Q

OCTANE

A

CH3CH2CH2CH2CH2CH2CH2CH3

BP 125 degrees C

liquid at room temp

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9
Q

nonane

A

CH3CH2CH2CH2CH2CH2CH2CH2CH3

BP 151 degrees C

liquid at room temp

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10
Q

Decane

A

CH3CH2CH2CH2CH2CH2CH2CH2CH2CH3

BP 174 degrees C

liquid at room temp

(alkane chains longer than decane are solids at room temp)

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11
Q

METHYL

A

CH3–

Methyl is a common alkyl group

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12
Q

Ethyl

A

CH3CH2–

Ethyl is a common alkyl group

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13
Q

Propyl

A

CH3CH2CH2–

Propyl is a common type of Alkyl group

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14
Q

Butyl

A

CH3CH2CH2CH2–

Butyl is a common type of alkyl group

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15
Q

isopropyl

A

isopropyl is a common alkyl group

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16
Q

tert-butyl

A

tert-butyl is a common type of alkyl group

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17
Q

Constitutional (structural) isomers

A

Molecules that have the same molecular formula, but differ in how the atoms are connected.

Have different properties.

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18
Q

Strucure of an alkyne functional group

A
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19
Q

cycloalkane are formed with…

A

single C–C bonds in a ring formation

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20
Q

Characteristics of an alkene?

A
  • general formula CnH2n
  • one of 4 types of hydrocarbons
  • Contain at least one C–C DOUBLE bond, with sp2 hybridized carbons.
  • Unsaturated, i.e. contain less H than an alkane with the same number of C atoms
  • Rotation around the C–C double bond require breaking the π bond. Therefore, can form trans and cis geometric isomers.
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21
Q

Characteristics of an alkane?

A
  • one of 4 types of hydrocarbons
  • Saturated (every C has the max number of H)
  • Single C–C bonds
  • can be straight line or cyclo
  • generally very reactive, produce much energy so often burned for fuel
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22
Q

What are the 4 types of hydrocarbons?

A

Alkane

Alkene

Alkyne

Aromatic

23
Q

cycloalkane general formula

A

CnH2n

24
Q

straight-line alkane general formula

A

CnH2n+2

25
Q

Strucure of an aromatic functional group

A
26
Q

ALKENE FUNCTIONAL GROUP

A
27
Q

Strucure of an ether functional group

A

to name, add “ether” to end

28
Q

Strucure of an alcohol functional group

A

to name, add -ol to ending

29
Q

Strucure and notes about the amine class functional group

A

Amines are weak bases because the lone pair of electrons on the N is perfect for accepting protons.

They smell terrible! Ex. rotting meat

30
Q

Strucure of an aldehyde class functional group

A

to name, add -al to end

31
Q

Strucure of a ketone class functional group

A

to name, add -one to end.

32
Q

Strucure of a CARBOXYLIC ACID class functional group

A

To name, add -oic acid to end.

Weak acids. The anion O- is stablilized by resonance.

Ex. vinegar

33
Q

Strucure of an Ester class functional group

A
34
Q

Strucure of a carboxamide class functional group

(also called amide)

A
35
Q

Molecular geometry names and bond angles

A
36
Q

What is electronegativity?

A

Electronegativity is the ability of atoms in a molecule to attract electrons to themselves in a covelant bond.

The greater the difference in electronegativity between atoms in a molecule, the more polar the bond.

37
Q

Describe London Dispersion Forces

A

London Dispersion Forces are intermolecular forces where a diapole-diapole is induced.

As electrons move about, there is a moment when they create a partial charge. This induces a partial charge in neighboring moleules, and a domino of induced partial charges occurs.

Larger molecule = more electrons = more potential for polarizability = more london dispersion forces, so look at molar mass when assessing.

38
Q

Describe dipole-dipole forces.

A

Dipole-dipole forces are a type of intermolecular force where a molecule has a permenant dipole moment and is attracted to other molecules with a permenant dipole moment.

Strength of the force is…

proportionate to the difference in electronegativity

and dependent on the symetry of the molecule. Symetrical molecules can have dipole forces that cancel each other out.

39
Q

Describe Hydrogen Bonds as they relate to intermolecular forces.

A

When hydrogen bonds to a more electronegative molecule (F, O, Cl, N) in a way that makes a very polar molecule, it can form the strongest kind of intermolecular forces–hydrogen bonds.

The polar-covalent bonds of the atoms add to the dipole forces of the molecule.

Plus there are strong intermolecular foces from the dipole created from the asymetry of the molecule.

40
Q

Describe Ion-Dipole Forces.

A

Ion-dipole forces happen when you combine ions (atoms or molecules with a net charge) with a molecule that has a dipole moment.

There are Coulomb forces at play, so the strength of the charge matters (-1 vs. -2).

Ex: Put NaCl in water and it easily dissolves because the partial charges of the H2O are quickly attracted to the Na+ and Cl-.

41
Q

What are the steps to assess/compare intermolecular forces (and boiling point)?

A
  1. Look for hydrogen bonded directly to F, O, N, or Cl in a very polar molecule (ex. in a hydroxyl -OH group). These H bonds have a huge impact on neighboring molecules and are the strongest intermolecular forces.
  2. Look for dipole-dipole forces. Could be differences in electronegativity within molecules, or asymetry of molecules.
  3. Look at molar mass. Bigger molecules have London Dispersion Forces at play.
  4. Look for metals that indicate ion-dipole forces.
42
Q
  • at least one TRIPLE bond between two sp hybridized carbons.
  • Triple bond includes one σ (sigma) bond formed, and two π bonds. Two p orbitals from C are not used in the sp hybridization, so they form the π bonds.
A
43
Q

single bond = bond order of 1

double bond = bond order of 2

triple bond = bond order of 3

More bonds = stronger bonds. However, it is not 3x as strong, since the sigma bond is stronger than π bonds.

A
44
Q

Bond enthalpy

A

Bond enthalpy (kJ/mol) = the energy input needed to break 1 mole of bonds.

45
Q

Functional Group

A

functional group = Groups of atoms and bonds that are responsible for the characteristic chemical reactions of molecules.

46
Q

heteroatoms

A

something other than carbon or hydrogen

47
Q

Explain hydrogen bonding with H2O

A

Hydrogen bonding is usually found in situations represented by

D-H—A

where both the donor atom, D, and the acceptor atom, A, are one of the highly electronegative elements O, N, or F. The D-H bond is a normal covalent bond, and H—A is a hydrogen bond.

Hydrogen bonding is not expected to occur between molecules in which all of the H atoms are covalently bonded to C atoms, even when an acceptor atom is present.

However, since water is able to act as both a donor and an acceptor, molecules that have an acceptor atom can form H-bonds with water, even if they are not able to act as H-atom donors.

Of the molecules shown, both methyl alcohol and acetamide can act as either a donor or an acceptor in an H-bond with water, while diethyl ether is able to act as an acceptor.

Only cyclohexane is missing both a donor atom and an acceptor atom and cannot form an H-bond with water.

48
Q

What two compounds do you mix to form an ester?

A

Carboxilic acid and alcohol form an ester + H2O in a condensation reaction.

The O-H from the carboxilic acid + the H from the alcohol form H2O; the rest bonds to form the ester.

49
Q

What two functional groups react to form an amide?

A

A carboxylic acid, RCOOH, will react with an amine, R’NH2, in a condensation reaction to give an amide, RCONHR’.

Carboxilic acid and amine form an amide + H2​O.

The O-H from the carboxilic acid + the H from the amine form H2O; the rest bonds to form the amide.

50
Q

how to recognize a molecule that has cis/trans geometric isomers

A

Thus there are two requirements for cis-trans isomerism:

  1. Rotation must be restricted in the molecule.
  2. There must be two nonidentical groups on each doubly bonded carbon atom.

in other words…

Plan: Identify the fragments attached to each carbon of the double bond. If both carbons have two different fragments, then cis and trans isomers can exist. If either of the carbons has identical fragments, then there is no cis and trans isomerism.

51
Q

hydrolysis of an ester reacts to produce…

A

When an ester is hydrolyzed, it produces a carboxylic acid and an alcohol.

52
Q

what makes an acid?

what are some strong acids?

A

When a compond forms lots of H+ cations in an aqueous (water, aq) solution. AKA leading to H3O.

Common acids are HCl, HBr, HI, HClO4, H2SO4, HNO3

53
Q

what makes a base?

A

A base is able to accept a proton

(vs. acids donate protons)

when a compond forms lots of OH in an aqueous (water, aq) solution.

Chem 104 (4 decks)

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