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ChE LE Flashcards > Inorganic Chemistry Part 2 > Flashcards

Inorganic Chemistry Part 2 Flashcards

1
Q

Contributions:
Max Planck

A

discovered that atoms and molecules emit energy only in certain discrete quantities, or quanta

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2
Q

“Energy is quantized”

A

Max Plank
(energy comes in steps”

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3
Q

Describe quanta

A

E= hf = hc/L
Smallest amount of energy that can be emitted (or absorbed) in the form of electromagnetic radiation

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4
Q

Contributions:
James Clerk Maxwell

A

proposed that visible light consists of electromagnetic waves

“electromagnetic wave has an electric field component and a magnetic field component.”

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5
Q

Photoelectric effect equation

A

E = hf = KE + W

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6
Q

Continuous or line spectra of radiation emitted by substances.

A

Emission Spectra
Examples:
*glow of metal during smelting,
*shine of Tungsten bulb when lit

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7
Q

Light emission only at specific wavelengths.

A

line spectra

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8
Q

“Electron is allowed to occupy only certain orbits of specific energies”

A

Niels Bohr

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9
Q

Contributions:
Johannes Balmer

A

Made a mathematical model explaining the observed frequencies for Hydrogen Spectral Lines

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10
Q

Contributions:
Niels Bohr

A
  1. Hydrogen spectra
    “Electrons occupy only certain orbits”
  2. Planetary model
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11
Q

Why Niel’s Bohr was UNSUCCESSFUL in explaining Emission Spectra?

A

*Works for Hydrogen only (for atoms with only 1 electron)
*No reason why extra spectra lines are present when magnetic field is present

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12
Q

Why Niel’s Bohr was SUCCESSFUL in explaining Emission Spectra?

A

Can still make good approximations for multiple electron systems

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13
Q

Lowest energy state of a system

A

ground state

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14
Q

Higher in energy than the ground state

A

excited state

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15
Q

Explain behavior of Electron when absorbing or emitting energy

A

*Absorb photon: (+)E, electrons moves to higher energy level (excited state)
*Emit photon: (-) electrons move to lower energy level (ground state)

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16
Q

Meaning of LASER

A

Light Amplification by Stimulated Emission of Radiation

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17
Q

Contributions:
Louis de Broglie

A

de Broglie Wavelength:
L = h/mv

*Wave-Particle Duality
“If waves (light) behave as particles,
then particles (electrons) behave as waves)

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18
Q

Wave-Particle Duality of Light

A

Albert Einstein

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19
Q

Wave Particle Duality of Matter

A

Louis de Broglie

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20
Q

Contributions:
Clinton Davisson, Lester Germer and G. P. Thomson

A

Demonstrated that electrons INDEED do have wave-like properties

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21
Q

Explain Heisenberg
uncertainty principle

A

Paths of electrons are not well-defined
“It is impossible to know simultaneously both the momentum p (defined as mass times velocity) and the position of a particle with certainty.”

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22
Q

Contributions:
Erwin Schrödinger

A

*Tried to find way to solve Heisenberg Uncertainty Principle

*ELECTRON DENSITY: Came up with “wave function” that describes PROBABILITY where an electron is likely located

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23
Q

Gives the probability that an electron will be found in a particular region of an atom

A

Electron density

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24
Q

How the electrons are distributed among the various atomic orbitals

A

Electron configuration

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25
Q

Why Shielding Effect only exists in Multi-Electron Atoms?

A

All orbitals within a shell no longer have the same energy levels

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26
Q

Explain Shielding Effect

A

Inner e- shields valence e- from attractive force of the nucleus

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27
Q

Relation of Shielding Effect to Ionization Energy

A
  • More shielding e- = Lower Ionization Energy
  • Grp 13 elements have LOWER Ionization Energy than Grp 2
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28
Q

Rule that limits the total number of electrons in an orbital to 2

A

Pauli Exclusion Principle
(up and down lang possible, doble na if may additional)

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29
Q

Aufbau principle

A

Orbitals are filled in order of increasing energy, with no more than 2 e- per orbital

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30
Q

Pauli Exclusion Principle

A

No two e- could have the same set of quantum numbers

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31
Q

Hund’s Rule

A

For degenerate orbitals, the lowest energy is attained when the number of e- having the same spin is maximized

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32
Q

Contributions:
Otto Stern and Walther Gerlach

A

Conclusive proof of electron spins
*beam of atoms through magnetic field, 2 spots pertaining to 2 spins

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33
Q

Alloy of mercury + another metal or metals

A

Amalgam

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34
Q

Metals strongly attracted to magnets

A

Ferromagnetic metals

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35
Q

Describe Band Theory

A

Delocalized electrons move freely through “bands” formed by overlapping molecular orbitals

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36
Q

Closely spaced filled energy levels in metals

A

Valance Band

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37
Q

Closely spaced empty levels in metals

A

Conduction bands

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38
Q

Energy gap between the valence and conduction bands

A

Band Gap

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39
Q

Differentiate Intrinsic and Extrinsic Semiconductors

A

*Intrinsic Semiconductors: small, fixed band gap

*Extrinsic Semiconductors: size of band gap controlled by adding impurities (“doping”)

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40
Q

Solids containing donor impurities

A

n-type semiconductors
(negative)

41
Q

Solids containing acceptor impurities

A

p-type semiconductors
(positive)

42
Q

Differentiate Acceptor and Donor Impurities

A

Acceptor: electron deficient, accepts electron
Donor: electron rich, donates electrons

43
Q

Process of converting nitrogen and hydrogen into Ammonia

A

Haber process

44
Q

Hydrazine is commonly used as a ___

A

rocket fuel

45
Q

Aqua regia is a mixture of ___

A

HCl and Nitric acid

46
Q

____ is the most important fertilizer in the world

A

Ammonium nitrate

47
Q

By far the most abundant element in Earth’s crust

A

Oxygen

48
Q

Gas commonly used to purify drinking water, to deodorize air and sewage gases, and to bleach waxes, oils, and textiles.

A

Ozone O3

49
Q

Process of extracting sulfur from underground deposits

A

Frasch process

50
Q

Process of creating sulfuric acid using V2O5 as catalyst

A

Contact process

51
Q

Process of electrolysis of a concentrated aqueous NaCl solution (called brine) to produce chlorine gas

A

Chlor-Alkali Process

52
Q

Process of electrolysis of molten NaCl

A

Downs process

53
Q

Common source of magnesium

A

Seawater

54
Q

Toxic and reactive elements that are found only in compounds with other elements

A

Halogens

55
Q

Most toxic phosphorus allotrope

A

White Phosphorus P4

56
Q

Exceptions to Octet Rule

A
  1. Radicals
  2. Incomplete Octets: compounds with Be, B, Al have less than 6 valence e-
  3. Hypervalent: 3rd period Nonmetals
57
Q

Molecular compound distinguished by a high molar mass, ranging into thousands and millions of grams, and made up of many repeating units

A

Polymer

58
Q

Chemical Name of Rubber

A

Polyisoprene

59
Q

Showed that polymers are enormously large molecules

A

Hermann Staudinger

60
Q

Meaning of Monomers

A

Simple repeating units

61
Q

Meaning of Homopolymers

A

Polymer made up of only one type of monomer

62
Q

Meaning of Copolymer

A

Polymer containing two or more different monomers.

63
Q

Plant where natural rubber came from

A

Hevea brasiliensis

64
Q

Meaning of SBR

A

styrene-butadiene rubber

65
Q

Invented Vulcanization

A

Charles Goodyear

66
Q

Catalyst of Vulcanization

A

ZnO Zinc Oxide

67
Q

Also known as Elastomers

A

Synthetic rubber

68
Q

Primary Raw Materials for Vulcanization

A

Sulfur

69
Q

SBR is what type of polymer?

A

Copolymer

70
Q

Final Product of between hexamethylenediamine and adipic acid

A

Nylon 6-6

71
Q

Dacron is a ___

A

Polyester

72
Q

Polymers of amino acids

A

Proteins

73
Q

Contains 100 or more amino acid residues

A

Polypeptide chain

74
Q

Predicted the geometry of proteins (alpha helix and beta structures)

A

Linus Pauling

75
Q

Corresponding # of Electron Groups for each Geometry

A

Linear = 2 electron grps
Trigonal Planar = 3
Tetrahedral = 4
Trigonal Bipyramidal = 5
Octahedral = 6

76
Q

Corresponding # of Electron Groups for each Hybridization

A

sp = 2
sp2 = 3
sp3 = 4
sp3d = 5
sp3d2 = 6

77
Q

Came up with the Bing Bang Theory

A

George Gamow

78
Q

Properties on the atomic or molecular scale, must be determined by an indirect method

A

Microscopic properties

79
Q

Properties that can be determined directly

A

Macroscopic properties

80
Q

Invented the Geiger counter

A

Johannes Hans Wilhelm Geiger

81
Q

Catalyzed the discovery of the Nucleus

A

AKA Geiger- Marsden Experiment
* Johannes Hans Wilhelm Geiger
* Ernest Marsden

82
Q

Developed the Mass Spectrometer

A

Francis William Aston

83
Q

Developed the ‘panspermia’ theory

A

Svante August Arrhenius

84
Q

Proposed the Bronsted-Lowry acids and bases

A
  • Johannes Nicolaus Brønsted
  • Thomas Martin Lowry
85
Q

Received the Nobel Prize in Physics in 1910 for his work on the properties of gases and liquids.

A

Johannes Diderck van der Waals

86
Q

Received the Nobel Prize in Physics in 1922 for his theory explaining the spectrum of the hydrogen atom

A

Niels Henrik David Bohr

87
Q

Demonstrated the wave properties of electrons.

A

DAVISSON-GERMER-THOMSON
* Clinton Joseph Davisson
* George Paget Thomson
* Lester Halbert Germer

88
Q

Formulated wave mechanics, which laid the foundation for modern quantum theory.

A

Erwin Schrödinger

89
Q

Made important contributions to the study of magnetic properties of atoms and the kinetic theory of gases.

A

Otto Stern

90
Q

Provided conclusive proof of electron spin

A

Otto Stern and Walther Gerlach

91
Q

Received the Nobel Prize in Physics in 1954 for his interpretation of the wave function for particles.

A

Max Born

92
Q

Came with a process to synthesize ammonia from atmospheric nitrogen

A

Fritz Haber

93
Q

Inventor of dynamite

A

Alfred Nobel

94
Q

Discovered of X-ray diffraction

A

Max Theodor Felix von Laue

95
Q

Rewarded the Nobel Prize due to their contributions in X-ray crystallography

A

*William Henry Bragg
*William Lawrence Bragg

96
Q

Offers the most accurate method for determining bond lengths and bond angles in molecules in the solid state.

A

X-ray diffraction techniques

97
Q

Tells us the relative electron densities at various locations in a molecule

A

Electron-density contour map

98
Q

Developed the industrial process for preparing nitric acid that now bears his name

A

Wilhelm Ostwald

99
Q

Petroleum Products: (# of C’s and Phase)

a) Petroleum Gas
b) Gasoline
c) Kerosene
d) Fuel Oil
e) Lubricating Oil
f) Residue

A

a) Petroleum Gas: C1 to C4
Gas
b) Gasoline (naphtha): C5 to C12
Liquid
c) Kerosene: C12 to C16
Liquid
d) Fuel Oil: C15 to C18
Liquid
e) Lubricating Oil: C16 to C20
Liquid
f) Residue (asphalt): > C20
Solid

ChE LE Flashcards (20 decks)

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