Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem > Organic chemistry (lesson 1-2) > Flashcards

Organic chemistry (lesson 1-2) Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What are the inorganic exceptions?

A
  • oxides of carbon(CO, CO₂), carbonates (CO₃), cyanides (CN) and carbides(C₂)
  • those which don’t include C-C or C-H bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Why might a compound be inorganic?

A

It is lacking both carbon-carbon (C-C) and carbon-hydrogen (C-H) covalent bonds.

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

What are organic compounds?

A

organic compounds are those in which carbon atoms are almost always bonded to each other, to hydrogen atoms and to a few other atoms (O, N, S, P).

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

What is the formula for Alkanes?

A

CₙH₂ₙ₊₂
eg) C₅H₁₂, C₂₀H₄₂, etc.

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

What are the characteristics of Alkanes?

A
  • They are hydrocarbons containing only single bonds
  • They are saturated

*can be long continuous chains, branched chains or ring structures (cycloalkanes)

  • They are nonpolar and therefore not soluble in water.
  • relatively unreactive because the single bonds are very stable
  • LDF increases when there are more e⁻

*As you move down the homologous series, boiling and melting points increase, and it goes from gas -> liquid -> solid

  • Liquid alkanes are very good solvents for other hydrocarbons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

How do different structures influence boiling point?

A

Higher Boiling point factors:

  • Symmetry of structure; symmetrical branched alkanes will typically have BP’s higher than unsymmetrical branched alkanes
  • straight-chain alkane, as opposed to branched-chain alkane will have a higher BP due to greater surface area in contact between adjacent molecules.
  • “stronger” bonds (double bond, triple bond etc.)
  • Dipole-Dipole interactions contribute to higher boiling points of polar substances
  • Hydrogen bonding significantly influences boiling points and solubilities
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are the characteristics of Alkenes?

A
  • Hydrocarbons containing one or more double bond
  • They are unsaturated
  • Can be long continuous chains, branched chains or ring structures (cycloalkenes),

*They are nonpolar therefore not soluble in water.

  • lower boiling point than alkanes because they have fewer e- which makes the LD forces of attraction weaker.
  • more reactive and less stable than alkanes due to greater repulsion between electrons and lengthening (they want to repel)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the formula for alkenes?

A

CₙH₂ₙ

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

What is the formula for Alkynes?

A

CₙH₂ₙ₋₂

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

What are the characteristics of Alkynes?

A
  • They are hydrocarbons containing one or more triple bonds
  • they are unsaturated
  • can be long continuous chains, branched chains
  • nonpolar
  • very reactive (more reactive than alkanes and alkenes) due to very high repulsion due to 6 electrons in the same area.
  • boiling points are higher because of the linear structure and nature of triple bonds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the characteristics of Aromatics

A
  • They are hydrocarbons containing one or more
    benzene rings, C₆H₆.
  • They are nonpolar
  • characterized by strong aromas
  • all bonds are the same length and strength
  • unknown reactivity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

when does LDF increase?

A

when there are more e-

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

What is the diagnostic test to determine if a substance is an alkane vs alkene?

A

use KMnO₄ (aq) or Br₂

  • alkenes (double bond) will react with these substances causing a noticeable colour change, alkanes will not.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

For geometric isomers in alkenes, what is the prefix for the two different types of geometric isomers?

A

trans –> different sides
cis –> same side

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

uses for alkanes

A

natural gas (primarly methane), BBQ’s (propane), lighter fluid (butane), gasoline, etc.
good for making plastics, lubricants

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

uses for alkenes

A
  • plastics (PVC), steroids, welding torches
  • ethylene made from ethane cracking
17
Q

uses for alkynes

A
  • welding torches
18
Q

uses for aromatics

A

ASA, amphetamines, adrenaline, anesthetics
moth balls, TNT
Wintergreen, menthol, vanilla, cinnamon
SPF in sunscreen

19
Q

What are some characteristics of determining organic compounds?

A
  • Organic compounds are those in which carbon atoms are almost always bonded to each other, to hydrogen and a few other atoms (Oxygen, Nitrogen, Sulfur, Phosphorous)
  • All contain covalent bonds
20
Q

why is carbon unique?

A

It can bond with other carbon atoms to form long chains, rings, spheres, tubes, sheets etc

It can form combinations of single, double and triple bonds (no other element does this!!)

21
Q

Polar bonds are formed when…

A

there is an uneven pull on e⁻ within a molecule

22
Q

Polar compounds are formed when the polar bonds within a molecule…

A

do not cancel each other out

23
Q

can polar compounds dissolve in water?

A

Yes, The presence of dipole-dipole forces and hydrogen bonding will allow polar compounds to dissolve in water, since water is also polar

24
Q

can non-polar compounds dissolve in water?

A

no, non-polar compounds only have LD forces between molecules and will not dissolve in water

25
Q

As the number of electrons in a compound increases, so does…

A

the London Dispersion Forces

26
Q

What is the difference between intermolecular forces and intramolecular forces

A

intermolecular forces are the forces that occur between molecules, they are generally weaker than intramolecular forces and dictate things like boiling point, melting point viscosity and source tension. Some examples are: dipole-dipole forces, London dispersion forces, hydrogen bonding, and ion-dipole forces

intramolecular forces are the forces that occur within a molecule. They involve the atoms within a molecule and are generally much stronger than intermolecular forces. These forces hold the atoms together in a molecule, determining the molecules shape. Examples of intramolecular forces include covalent bonds, ionic bonds and metallic bonds.

27
Q

What are dipole-dipole forces?

A

A Moderate intermolecular force that occurs between polar molecules, where the positive end of one molecule is attracted to the negative end of another molecule.

Example: Occurs in polar molecules like hydrogen chloride (HCl) and water (H2O).

28
Q

What are London Dispersion Forces (LD forces)?

A

A weak intermolecular force that occurs between all atoms and molecules, polar or nonpolar, due to temporary uneven distribution of electrons creating temporary dipoles.

Example: Occurs between all types of molecules, but especially significant in noble gases and nonpolar molecules like helium or methane.

29
Q

What is hydrogen bonding?

A

A special, stronger type of dipole-dipole interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom (like nitrogen, oxygen, or fluorine) and is attracted to another electronegative atom nearby.

Example: Significant in water (H2O), where it contributes to unique properties like high boiling point.

*note: hydrogen bonding is not a bond in the same sense that covalent or ionic bonds are, instead it is an intermolecular force

30
Q

What are Ion-Dipole Forces?

A

A strong intermolecular force that occurs between an ion and a polar molecule, where the charged ion is attracted to the oppositely charged end of the polar molecule.

Example: Occurs in mixtures of ionic compounds and polar molecules, like when sodium chloride (NaCl) is dissolved in water (H2O).

31
Q

What are the three different ways that organic molecules can be drawn?

A

Complete structural diagram - shows all bonds

Condensed structural diagram - shows carbon-to-carbon bonds, but includes the hydrogens etc. attached to each carbon

Line structural diagram - shows only carbon-to-carbon bonds

32
Q

What does a molecular formula of organic molecules show?

A

the number of each type of atom in the molecule
Ex: propane: C₃H₈ (g)

33
Q

What is the homologous series?

A

a sequence of molecules with similar structure and differing in number of repeating units

CH₄
CH₃CH₃
CH₃CH₂CH₃
CH₃CH₂CH₂CH₃

34
Q

What are isomers?

A
  • Isomers are compounds with the same molecular formula but a different structure.
  • More carbons = more isomers
    *Over 4 million for C30H62 !!!
35
Q

What is an alkyl branch?

A

Branch consisting of only carbon and hydrogen atoms

36
Q

What is the parent chain?

A

The longest continuous chain of carbon atoms

37
Q

What is the formula for cycloalkanes?

A

CₙH₂ₙ

38
Q

What are the characterisics of cycloalkanes

A
  • Saturated cyclic hydrocarbon
  • Similar physical and chemical properties to chained alkanes
39
Q

Alkanes, alkenes, and alkynes are all?

A

aliphatic

Chem (16 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions