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Medical Chemistry 1 > Matter > Flashcards

Matter Flashcards

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1
Q

What does the Particle Theory of Matter describe?

A

The Particle Theory of Matter explains the physical properties of solids, liquids and gases.

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2
Q

What are the states of matter

A

Solid- tightly compact atoms that vibrate; have fixed shape and volume

Liquid- loose atoms that slide; fixed volume and no fixed shape

Gas- loose particles that bounce; no fixed shape or volume; compressible

Plasma- superheated matter where the electrons are stripped away from atoms to produce an ionized gas.

Bose-Einstein Condensate- Atoms are cooled to within a hair of absolute zero, they lose energy and start to clump together. They start to act as one atom instead of individual atoms.

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3
Q

Particle Theory of Matter

A

4 PRINCIPLES by John Dalton

  1. All matter is made of particles.
  2. Particles have spaces between them.
  3. Particles are always in constant random motion.
  4. Particles attract each other.
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4
Q

What does the Kinetic Theory of Matter help to explain?

A

The Kinetic Theory helps to explain the physical properties of a gas.

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5
Q

What are the 5 postulates of the Kinetic Molecular Theory?

A

Postulate #1- Gases are made of molecules that are in continuous motion

Postulate #2- Molecules are negligibly small compared to spaces between them.

Postulate #3- Pressure exerted by gas is as a result of collision of molecules with each other and their container.

Postulate #4- Gas molecules have no forces of attraction or repulsion between the molecules or container. Collisions are elastic.

Postulate #5- The average kinetic energy of a gas is equal to its Kelvin Temperarture.

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6
Q

Democritus

A

said that atoms (atomos) are the smallest, indivisible bit of matter

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7
Q

Aristotle

A

He said that “matter has a continuous composition that can be broken down into smaller pieces forever.”

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8
Q

Amonton’s Law

A

Is the direct proportional relationship between Pressure and Temperature.

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9
Q

Boyle’s Law

A

Is the Inverse proportional relationship between Pressure and Volume.

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10
Q

Charle’s Law

A

Is the direct proportional relationship between Volume and Temperature.

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11
Q

Avogadro’s Hypothesis

A

As the Numbers of particles increase so does Volume.

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12
Q

Dalton’s Law of Partial Pressure

A

The total number of collisions with wall is equal to the sum of collisions when each size of atom is present alone.

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13
Q

Graham’s Law of Diffusion

A

Is the rate at which gas diffuses and it is inversely proportional to the square root of their densities.

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14
Q

Graham’s Law of Effusion

A

Is the rate at which gas escapes through a pinhole into a vacuum. It is inversely proportional to the square root of their densities.

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15
Q

Osmosis

A

Is the selective diffusion across a semi-permeable membrane from less concentrated to more concentrated driven by osmotic pressure (available energy per unit volume).

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16
Q

What is the link between the Kinetic Molecular Theory and the Graham’s Laws?

A

The last postulate of the KMT explains Graham’ s Law. Temperature of a system is proportional to average kinetic energy of its particles.

Average kinetic energy of a sys. increases only if Temperature increases

17
Q

What are pure substances?

A

Elements

  • Grouping are the same.
  • Only one type of atom present
  • Chemically bonded
  • Separated by nuclear means

Compounds

  • Groupings are the same
  • Two or more atoms presents
  • Chemically bonded
  • Separated by chemical means
18
Q

Impure substances

A 
Mixtures 
- More than one types of atoms
- Groupings are all different 
- Physically bonded
= Separated by physical means
19
Q

Types of Mixtures

A

Solution

  • Very small particles
  • Homogenous
  • Transparent
  • Light passes through

Colloid

  • Particles are larger than solution but not visible to naked eye.
  • Heterogenous
  • Opaque
  • Light is scattered (Tyndall Effect)

Suspension

  • Particles are large enough to see
  • Heterogenous
  • Opaque
  • Blocks light
20
Q

What is the Tyndall Effect?

A

Light scatters because particles are large enough to block some light but still small enough to allow some light through.

happens with colloids and suspensions.

21
Q

What is Brownian Motion?

A

Is the constant & random motion of small, solid particles in fluids (liquids & gases)

Medical Chemistry 1 (9 decks)

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