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PORG > INTRO TO ORGCHEM : Structure And Bonding > Flashcards

INTRO TO ORGCHEM : Structure And Bonding Flashcards

1
Q

Study of carbon and carbon-related compounds.

A

Organic Chemistry

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2
Q

The name “organic chemistry” comes from the word?

A

Organism

(Because most of the organic compounds were isolated or obtained from organisms or their remains)

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3
Q

In year ____ , ______, a German Chemist, disproved the “Vitalism theory which states that all organic compounds come from living things. He was able to isolate ______ from an inorganic compound, __________.

A

• 1828
• Friedrich Wohler
• urea
• ammonium cyanate

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4
Q

What are the organic compounds found in living things?

A
  1. Sugars
  2. Lipids
  3. Proteins
  4. Nucleic Acids
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5
Q

A polymer made up of units called nucleotides.

A

DNA

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6
Q

What are the three different components that made up nucleotides?

A
  1. Sugar group
  2. Phosphate group
  3. Base
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7
Q

What are the 4 different bases?

A
  1. Adenine
  2. Thymine
  3. Guanine
  4. Cytosine
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8
Q

What holds DNA strands together?

A

Hydrogen bonds (between bases on adjacent strands)

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9
Q

______ compounds usually do not dissolve in water.

A

Organic

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10
Q

______ compounds usually dissolve in water.

A

Inorganic

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11
Q

_____ compounds generally dissolve in organic solvents like ether, alcohol, benzene, and choloroform.

A

Organic

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12
Q

_______ compounds generally do not dissolve in organic solvents.

A

Inorganic

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13
Q

_______ compounds have usually low melting points and boiling points; and they usually decompose on heating.

A

Organic

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14
Q

_______ compounds usually have high melting points and boiling points. They usually do not decompose on heating.

A

Inorganic

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15
Q

_______ compounds are inflammable; they catch fire easily.

A

Organic

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16
Q

_______ compounds are usually non inflammable; they do not burn easily.

A

Inorganic

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17
Q

_______ compounds exist as covalent molecules, so they are non-electrolytes.

A

Organic

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18
Q

Most of the _______ compounds are ionic, so they are electrolytes.

A

Inorganic

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19
Q

Carbon is able to form how many covalent bonds?

A

4 covalent bonds

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20
Q

What atoms have the ability to bond to each other to form long chains or rings?

A

Carbon atoms

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21
Q

What atoms link together to form chains of varying lengths, branched chains and rings of different sizes?

A

Carbon atoms

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22
Q

Smallest particle of an element

A

Atoms

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23
Q

Neutral subatomic particle

A

Neutron

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24
Q

Positively charged subatomic particle (+1 charge)

A

Proton

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25
Q

Negatively charged subatomic particle (-1 charge)

A

Electron

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26
Q

Center of an atom; contains protons and neutrons

A

Nucleus

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27
Q

Consists of a nucleus surrounded by electrons that are equal in number to the protons of the nucleus.

A

Atom

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28
Q

Atoms of the same element with different numbers of neutrons and thus different mass number.

A

Isotopes

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29
Q

Carbon-12 (stable isotope)

A

98.9%
6 protons & 6 neutrons

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30
Q

Carbon-13 (stable isotope)

A

1.1%
6 protons & 7 neutrons

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31
Q

Carbon-14 (unstable isotope; radioactive)

A

<0.1%
6 protons & 8 neutrons

32
Q

Fundamental building blocks of all substances.

33
Q
  • Region of space where there is a certain probability of finding an electron
  • Can hold 2 electrons
  • Also known as WAVE FUNCTION
34
Q

Shape of s orbital

35
Q

Shape of p orbital

36
Q

Shape of d orbital

A

4 leaf clover

37
Q

Shape of f orbital

A

Complex shape

38
Q

States that electron fill lower-energy atomic orbitals before filling higher-energy ones.

A

Aufbau Principle

39
Q

Maximum of 2 electrons can occupy thr same orbital only if they have opposite spins.

A

Pauli’s Exclusion Principle

40
Q

For degenerate orbitals, electrons fill the orbitald singly before they pair up.

A

Hund’s Rule

41
Q

Determine the size of the particle.

A

Principal Quantum Number

42
Q

Subshell or sublevel, determines the shape

A

Azimuthal or Angular Momentum

43
Q

Orbitals, determines orientation

44
Q

Direction of spin or orientation

45
Q
  • Symbolic notation of the manner in which the electrons of its atoms are distributed over different atomic orbitals.
  • Summary of where the electrons are around a nucleus
A

Electron Configuration

46
Q

Number of negatively charged subatomic particles in the highest energy level of atoms that enters into formation of chemical bonds.

A

Valence Electrons

47
Q
  • joining of two atoms in a stable arrangement
  • may occur between atoms of the same or different elements.
  • favorable process because it always leads to lowered energy and increased stability
  • octet rule - atoms react in a way that achieve valence shell of eight valence electrons.
A

Chemical Bonding

48
Q
  • bond between cation and anion
  • atom may lose or gain enough electrons to acquire a completely filled valence shell
  • anions gain electrons; cations lose electrons
A

Ionic Bond

49
Q

Sharing of electrons

A

Covalent Bond

50
Q
  • electron dot structure
  • valence shell electrons of an atom are represented as dot
A

Lewis Structure

51
Q
  • line bond structure
  • each shared electron is represented by line between the atom symbols
A

Kekule Structure

52
Q

Pair of valence electrons that are not used for bonding.

A

Lone-pair electrons / non-bonding electrons

53
Q

Associated with any atom that does not exhibit the appropriate number of valence electrons.

A

Formal Charge

54
Q

Measure of the ability of an atom to attract electrons.

A

Electronegativity

55
Q

Seperation of electric charge along a bond, leading to a molecule or its chemical groups having an electric dipole or dipole moment

A

Bond polarity

56
Q

Formula of formal charge

A

of valence electrons - sum between non bonded electrons + # of line bonds

57
Q

Most electronegative element

58
Q

Equally shared electrons between the atoms.
(Difference in electronegativity < 0.5

A

Non-polar covalent bond

59
Q

Not equally shared electrons between atoms. (0.5 - 1.7 electronegativity)

A

Polar covalent bond

60
Q

Withdrawal of electrons towards a highly electronegative atom which causes the formation of partial charges.

61
Q

Average out energy

A

sp³ hybridization

62
Q

Å is?

A

(Angstrom) - Unit for length

63
Q
  • total number of sigma bonds and lone pairs
  • indicated the number of electron pairs (bonding and non-bonding) that are repelling each other.
A

Steric number

64
Q

How to get steric number?

A

of bonds + # of lone pairs

65
Q

Bond angle: 107 degrees
- e.g. ammonia

A

Trigonal pyramidal

66
Q

Bond angle: 105

67
Q

Bond angle: 120 degrees
- e.g. Boron trifluoride

A

Trigonal planar

68
Q

subshell is known as?

A

atomic orbitals

69
Q

Equally shared electrons between 2 atoms

A

Non-polar covalent bond

70
Q

Not equally shared electrons between atoms

A

Polar covalent bond

71
Q

Is < 0.5 polar or non-polar?

A

Non-polar covalent bond

72
Q

Is 0.5 - 1.7 polar or non-polar?

A

Polar covalent bond

73
Q

If the central atom is connected to the same groups/atoms (symmetrical)

(Non-Polar or Polar)

74
Q

It has no lone pair (in the central atom)

(Non-Polar or Polar)

75
Q

If the central atom is connected to different groups/atoms (asymmetrical)

(Non-Polar or Polar)

76
Q

If it has a lone pair (in the central atom)

(Non-Polar or Polar)

PORG (16 decks)

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