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Organic Chem > Chapter 1 > Flashcards

Chapter 1 Flashcards

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1
Q
  • in 1807, he proposed that
    compounds derived from living things
    were organic and that all others were
    inorganic
  • coined the term “organic chemistry”
A

Jöns Jācob Berzelius

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2
Q
  • sometimes called “vitalism”
  • vital means life force
  • organic compounds could be produced only
    within living systems.
  • Living things
    possessed a vital force as a result of their
    origin in living sources.
A

Vital force theory

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3
Q
  • In 1828, the Vital Force Theory was
    disproved synthesized urea, an organic substance.
  • found in urine of mammals, from
    inorganic starting materials (ammonium
    cyanate) without using living organisms.
A

Friedrich Wöhler

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4
Q
  • the study of the compounds of carbon
  • refers to the study of hydrocarbons (compounds of carbon
    and hydrogen) and their derivatives
A

ORGANIC CHEMISTRY

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5
Q
  • is a field which provides a host of
    organic chemicals for use in every area of modern living.
A

Modern Organic Chemistry

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6
Q

The reason why carbon is so special

A
  • non-metallic element
  • sixth most abundant element in the universe, second most common element in the human
    body after oxygen.
  • present in all living organisms like
    carbohydrates, proteins, fats
    major chemical constituent of most organic
    matter
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7
Q
  • with the valency of four, carbon is
    capable of bonding with four other
    atoms
A

Tetravalent/Tetravalency

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8
Q
  • atoms are most stable when their
    valence shells are filled with eight
    electrons
A

Octet rule

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9
Q
  • self-linking property of an atom
  • carbon atoms has a unique ability
    to bond together to an extent not
    possible for atoms of any other
    element
  • carbon can unite with itself
    indefinitely due to its tetravalent
    nature
A

Catenation

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10
Q
  • characteristic structural units
  • cannot be overstated.
    A functional group determines all the following properties
    of a molecule:
    • bonding and shape
    • type and strength of intermolecular forces
    • physical properties
    • nomenclature
    • chemical reactivity
A

Functional groups

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11
Q
  • it was something Friedrich Wöhler synthesized using inorganic materials
  • organic component of the urine of animals
  • H2NCONH2
A

Urea

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12
Q

Meaning of IUPAC

A

International Union of Pure and Applied
Chemistry

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13
Q
  • general system of nomenclature
    systematic method of naming organic
    compounds
  • advantage: name and structural formula
  • three parts: PREFIX, PARENT and SUFFIX
A

The IUPAC System

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14
Q
  • CnH2n+2
  • single bonds
  • saturated hydrocarbon
  • straight chain
  • branched alkane
A

Alkanes

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15
Q
  • atom or group of atoms attached to a chain (or ring) of carbon atoms (side chains)
A

Substituent

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16
Q
  • The forces of interaction between molecules or intermolecular forces like London forces, Dipole-dipole forces and hydrogen bonding.
A

Van der Waals Forces

17
Q
  • exists between an ion and the partial charge on the end of a polar molecule. - Positive ions are attracted to the negative end of a dipole, and vise versa
A
  • Ion-Dipole Force
18
Q
  • exists between neutral polar molecules. Polar molecules attract each other when the positive end of one molecule is near the negative end of another.
A

Dipole-Dipole Force

19
Q
  • Intermolecular forces resulting from attractions between induced dipoles.
  • was introduced by Fritz London
A

London Dispersion Forces

20
Q
  • Intermolecular forces resulting from attractions between induced dipoles.
  • was introduced by Fritz London
A

London Dispersion Forces

21
Q
  • is a special type of intermolecular attraction that exists between the hydrogen atom in a polar bond
A

Hydrogen bonding

22
Q
  • shows the number of each type of atom that is present in the molecule of the compound.
A

Molecular formula

23
Q
  • shows the number of each type of atom that is present in the molecule of the compound.
A

Molecular formula

24
Q
  • shows the details of the bonding present in the molecule, (i.e., which atoms are connected to which other atom.)
A

Structural Formula

25
Q

Types of structural formula

A

• Full/Expanded structural formula
• Condensed structural formula
• Skeleton structural formula
• Line structural formula

26
Q
  • All the atoms and bonds are indicated.
A

Full or Expanded Structural Formula

27
Q
  • an abbreviated form of writing formulas.
  • Shows no bonds
  • Shows all carbon-carbon bonds but no carbon-hydrogen bonds.
  • ex. CH3CH3
A

Condensed Structural Formula

28
Q

shows only the carbon atoms in the molecule.

A

Skeleton Structural Formula

29
Q
  • uses lines to show the structure of the compound where;
A

Line structural formula

30
Q
  • compounds that have the same molecular
  • formula but different structures
  • same collection of atoms
  • differ in one or more physical or chemical
    properties (color, solubility, rate of
    reactions)
A

Isomers

31
Q
  • same molecular formula
  • different structures
  • differ in connectivity
A

CONSTITUTIONAL
ISOMERS

32
Q
  • same molecular formula
  • same order of attachment of atoms
  • different 3-D orientation in space
A

STEREOISOMERS

33
Q

Two types of stereoisomers

A

• ENANTIOMERS
• DIASTEREOMERS

34
Q

nonsuperimposable or mirror images

A

ENANTIOMERS

35
Q
  • not mirror images
A

DIASTEREOMERS

36
Q

• molecular formula CnH2n
• contain carbon atoms arranged in a ring

A

CYCLOALKANE

37
Q

• Cycloalkanes are named by using similar rules,
• but the prefix cyclo- immediately precedes the
name of the parent

A

NOMENCLATURE OF CYCLOALKANE

38
Q
  • from greek “cheir” meaning hand
A

Chiral

39
Q
  • from greek “cheir” meaning hand
A

Chiral

Organic Chem (1 decks)

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