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Inorganic Chemistry > Atomic > Flashcards

Atomic Flashcards

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1
Q

Coined the word atom

A

Democritus

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2
Q

Proposed the Atomic theory

A

John Dalton

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3
Q
  1. Elements are composed of tiny indivisible particles called atoms
  2. Atoms of different elements are chemically different; however atoms of a given element are of the same size, shape, mass and chemical properties
A

Atomic Theory

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4
Q

Proposed the “Law of Conservation of Mass”

A

Antoine Lavoiser

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5
Q

“A chemical reaction only involves separation, combination or rearragement of atoms”

A

Law of Conservation of Mass

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6
Q

Proposed the “Law of Multiple Proportions”

A

John Dalton

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7
Q

“When two elements combine with each other to form two or more compounds, the ratios of the masses of one element that combines with the fixed mass of the other are simple whole number ratios”

A

Law of Multiple Proportions

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8
Q

Proposed the “Law of Definite Proportions”

A

Joseph Proust

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9
Q

“A given chemical compound always contains the same elements in the exact same proportions by mass”

A

Law of Definite Proportions

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10
Q

Discovered the negatively-charged particles, electrons

A

Joseph John Thompson

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11
Q

Used to determine the electrons

A

Cathode Ray Tube

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12
Q

Suggested the Plum-Pudding Model

A

Joseph John Thompson

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13
Q

Determined the ratio of the electric charge to the mass of an electron to be -1.76x10¹¹ C/kg

A

Joseph John Thompson

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14
Q

Gave the name electron

A

George Johnstone Stoney

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15
Q

Determined the mass of an electron

A

Robert Millikan

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16
Q

Used to determine the mass of an electron

A

Oil drop experiment

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17
Q

Discovered the positively-charged particles, protons

A

Eugene Goldstein

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18
Q

Used to determine the protons

A

Anode Ray Tube

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19
Q

Discovered neutron by bombarding Be with alpha particles. These particles are not affected by electric field

A

James Chadwick

20
Q

Discovered nucleus by performing Goild foil experiment wherein a thin foil of gold is bombarded with alpha particles

A

Ernest Rutherford

21
Q

Is a phenomenon where electrons are emitted from the metal surface when the light of sufficient frequency is incident upon

A

Photoelectric effect

22
Q

Basis for solar panels

A

Photoelectric effect

23
Q

Is the minimum energy required to remove an electeon from the surface of the material

A

Work function

24
Q

1 eV = ___ J

A

1.6x10‐¹⁹ J

25
Q

1 kWh = ____ MJ

A

3.6

26
Q

Scattering of a photon by a charged particle, usually an electron

A

Compton Scattering

27
Q

Matter might also exhibit wave-like properties under suitable conditions

A

De Broglie Wavelength

28
Q

It states that “Any hot vibrating body does not emit nor absorb energy continuously, but discontinuously, in the form of small packets of quanta”

A

The Quantum Theory of Atoms

29
Q

It states that “ It is impossible to know exactly both the position and momentum of an electron or any other small particle simultaneously and accurately”

A

Heisenberg Uncertainty Principle

30
Q

It states that “Electrons behave as particles and waves”

A

Wave - particle duality

31
Q

It states that “Electrons revolved around the nucleus in elliptical orbits with different eccentricities of which Bohr’s circular is a special case”

A

Bohr -Sommerfield Theory

32
Q

Concluded that electrons behave more like waves than particles

A

Davisson - Germer Experiment

33
Q

The region in space around the nucleus where it is most probable to find an electron

A

Orbital

34
Q

Tells the

  1. Distance of an electron from the nucleus
  2. Energy of an electron in the orbit (energy levels)
A

Principal Quantum Number

35
Q

True or False

The larger the value ofthe principal quantum number, the farther is the electron from the nucleus

A

TRUE

36
Q

Tells the

  1. Shape of orbital
  2. Subshell position of electron
A

Azimuthal / Angular Quantum Numbers

37
Q

Tells about

  1. Orientation of orbitals in space
A

Magnetic Quantum Number

38
Q

Shows the spin of electrons

A

Spin Quantum Number

39
Q

Aufbau means

A

Filling up

40
Q

States that “the orbitals must be filled up in increasing energy levels”

A

Aufbau Principle

41
Q

States that “No two electrons in an atom can have the same set of quantum numbers and an atomic orbital must contain a maximum of two electrons with opposite spins”

A

Pauli’s Exclusion Principle

42
Q

States that

  1. The pairing up of electrons in an orbital of a subshell takes place only when all orbitals contain atleast on electron
  2. The most stable arrangement of electrons in subshells is the one with more parallel spins
A

Hund’s Rule of Maximum Multiplicity

43
Q

States that “The stablest structure is the one with carbon atom that has formal charge near to zero”

A

Kekule Rule of Resonance

44
Q

The hydrogen emission lines associated with the visible part of the spectrum is called the ____ series

A

Balmer

45
Q

The hydrogen emission lines associated with the ultraviolet part of the spectrum is called the

A

Lyman

46
Q

The hydrogen emission lines associated with the infrared part of the spectrum is called the _____ series

A

Paschen

Inorganic Chemistry (6 decks)

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