Matter Flashcards
What does the Particle Theory of Matter describe?
The Particle Theory of Matter explains the physical properties of solids, liquids and gases.
What are the states of matter
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.
Particle Theory of Matter
4 PRINCIPLES by John Dalton
- All matter is made of particles.
- Particles have spaces between them.
- Particles are always in constant random motion.
- Particles attract each other.
What does the Kinetic Theory of Matter help to explain?
The Kinetic Theory helps to explain the physical properties of a gas.
What are the 5 postulates of the Kinetic Molecular Theory?
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.
Democritus
said that atoms (atomos) are the smallest, indivisible bit of matter
Aristotle
He said that “matter has a continuous composition that can be broken down into smaller pieces forever.”
Amonton’s Law
Is the direct proportional relationship between Pressure and Temperature.
Boyle’s Law
Is the Inverse proportional relationship between Pressure and Volume.
Charle’s Law
Is the direct proportional relationship between Volume and Temperature.
Avogadro’s Hypothesis
As the Numbers of particles increase so does Volume.
Dalton’s Law of Partial Pressure
The total number of collisions with wall is equal to the sum of collisions when each size of atom is present alone.
Graham’s Law of Diffusion
Is the rate at which gas diffuses and it is inversely proportional to the square root of their densities.
Graham’s Law of Effusion
Is the rate at which gas escapes through a pinhole into a vacuum. It is inversely proportional to the square root of their densities.
Osmosis
Is the selective diffusion across a semi-permeable membrane from less concentrated to more concentrated driven by osmotic pressure (available energy per unit volume).
What is the link between the Kinetic Molecular Theory and the Graham’s Laws?
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
What are pure substances?
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
Impure substances
Mixtures - More than one types of atoms - Groupings are all different - Physically bonded = Separated by physical means
Types of Mixtures
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
What is the Tyndall Effect?
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.
What is Brownian Motion?
Is the constant & random motion of small, solid particles in fluids (liquids & gases)
