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

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
Einsteins theory
- 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
Bohr Model
Forces of attraction between electrons and nucleus result from opposite charges Shells Electrons in shells have quantized energy levels
27
Shielding effect
Electrons further away from nucleus are shielded by closer electrons
28
Coulomb's law
``` 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
First ionization energy
-minimum amount of energy required to remove the outermost, least tightly held electron
30
Shell organization
SPDF
31
Orbital
Graphic representation of the space an electron will occupy 90% of the time
32
Quantum Mechanical Model
Solves the problem of subshells
33
Periodicity
Predictable trends on the table