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Chem > Lect. 1-3 > Flashcards

Lect. 1-3 Flashcards

1
Q

Mixture

A

Contains particles or units of more than 1 specific atom or molecule i.e. solutions

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2
Q

Democritus

A

Atoms “atomos”

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3
Q

Antoine Lavoisier

A

Law of conservation of mass

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4
Q

Joseph Proust

A

Law of Definite Proportions: i.e. water is always 88.8% oxygen and 11.2% hydrogen

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5
Q

John Dalton

A

First guy with an atomic theory

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6
Q

Dalton’s 4 postulates:

A
  • Each element is composed of tiny particles called atoms
  • All atoms of a given element are identical, and all atoms of different elements are different
  • Atoms are not created or destroyed in a chemical reaction, they are dissociated, combined, or recombined
  • Compounds are formed when atoms of different elements combine with one another. A given compound always contains the same relative numbers and types of atoms
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7
Q

J.J. Thompson

A

Electrons: stream of particles through electric field

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8
Q

Earnest Rutherford

A

Nucleus, gold foil experiment

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9
Q

Mass number

A

Protons+neutrons: upper left hand corner

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10
Q

Atomic number

A

Number of protons: bottom left hand corner

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11
Q

Isotopes

A

Same element, but with different number of neutrons

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12
Q

The 2 types of pure samples are…

A

Elements and compounds

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13
Q

Mass Spectrometry

A
  • used to compare masses of isotopes
  • atoms from a pure sample of an element are ionized (electrons stripped) and sent through a magnetic field
  • isotopes with smaller masses are deflected more
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14
Q

Average atomic mass

A

(Mass#%)+(mass#%)+…

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15
Q

Mass %

A

}[(# of atoms of specific element)(elements atomic mass)]/(formula weight of compound)}*100

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16
Q

Law of Multiple Proportions

A

2 compounds made of the same 2 elements, the masses of the elements in each compound are small whole number ratios

17
Q

Mass ratio of elements in a pure sample of a compound (constant composition)

A

The ratio of isotopes of a certain element in any pure sample of a given compound is constant

18
Q

Wavelength, frequency, speed of light formula

A

c=λν

19
Q

Purple light

A

High frequency, high energy, small wavelength

20
Q

Red light

A

Low frequency, low energy, long wavelength

21
Q

Max Planck

A

Quantum theory

22
Q

Quantum theory

A

Energy increases and decreases in discreet units: by a full quantum or not at all

23
Q

Quantum theory/Planks constant Equation

A

E=hv
E-energy per quantum
H-plancks constant
V-frequency

24
Q

Photoelectric effect

A
  • high intensity, low frequency light won’t eject electrons no matter what
  • when threshold frequency is met, electrons are ejected immediately
  • increasing intensity of light will increase ejection rate, but not velocity
  • increasing frequency of light increases velocity of electrons
25
Q

Einsteins theory

A
  • a beam of light is a stream of particles called photons
  • energy of a photon is related to its frequency by e=hv
  • the quantum of Planck is a particle(photon)
  • if the frequency of an electron is below a certain threshold, no electrons are ejected
  • if the frequency of the photon is at or above a certain threshold, it’s energy is transferred to the electron
26
Q

Bohr Model

A

Forces of attraction between electrons and nucleus result from opposite charges
Shells
Electrons in shells have quantized energy levels

27
Q

Shielding effect

A

Electrons further away from nucleus are shielded by closer electrons

28
Q

Coulomb’s law

A 
Closer to nucleus=stronger attraction
F=k(q1q2/d2)
F-force of attraction
K-constant
Q-magnitude of charge associated with a particle - protons or electrons 
D-distance between charged particles
29
Q

First ionization energy

A

-minimum amount of energy required to remove the outermost, least tightly held electron

30
Q

Shell organization

A

SPDF

31
Q

Orbital

A

Graphic representation of the space an electron will occupy 90% of the time

32
Q

Quantum Mechanical Model

A

Solves the problem of subshells

33
Q

Periodicity

A

Predictable trends on the table

Chem (7 decks)

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