A brief History Of Chemistry-Chapter 00 Flashcards

1
Q

What are the 2 important ideas of Atomic Theory?

A
  1. Law of Definite Proportions
  2. Law of conservation of Mass
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2
Q

What does the Law of Definite Proportions Do?

A

-In a given compound, the elements are always combines in the same proportion by mass.

-You will always find 1g H to 8g O in water.

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3
Q

What does the Law of Conservation of Mass Do?

A

-No detectable gain or loss of mass occurs in Chemical reactions. Mass is conserved.
EXAMPLE—-> (If we have a closed vessel that contains 16g of O and @g of H and let them react, that vessel will contain 18f of water after the reaction completes.)

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4
Q

What is the atomic theory base on? What are atoms?

A

-Tiny submicroscopic particles
-Make up all chemical substances (which is everything)
-Smallest particle that has all properties of given element.

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5
Q

What are Dalton’s Atomic Theories?

A
  1. Matter(anything tangible) consists of atoms
  2. Atoms are indestructible
    -In chemical reactions, atoms rearrange but do not break apart.
  3. In any sample of a pure element, all atoms are identical.
  4. Atoms of different elements differ in mass and other properties.
  5. In a given compound, constituent atoms are always present in same fixed numerical ratio.
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6
Q

what does Cathode mean?

A

negative electrode.

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7
Q

What does Anode?

A
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8
Q

Who discovered the electron?

A

JJ Thompson (1987)

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9
Q

Who discovered the Atomic Nucleus?

A

Rutheford’s Alpha Scattering Experiment.

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10
Q

Where was the proton discovered?

A

Discovered in 1918 in Ernest Rutherford’s lab

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11
Q

Who discovered the Neutron

A

First postulated by Rutherford and coworkers also by James Chadwick

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12
Q

Define Attraction?

A

Attraction between protons and electrons
holds electrons around nucleus

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13
Q

Define Repulsion?

A

between electrons helps them spread out over volume
of atom

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14
Q

Isotopes?

A

Atoms of same element with different masses

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15
Q

Isoelectronic definition:

A

same number of electrons.

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