Chapter 1 Flashcards
Stoichiometric relationships
Stoichiometry
Relationship between amount of reactants and amount of products in a chemical reaction
Law of conservation of mass
- The sum of masses of all reactants must be equal to sum of masses of all products
- Matter cannot be created or destroyed in a chemical reaction
- No matter is gained or lost during chemical change
States of matter
- Solid
- Liquid
- Gas
- Plasma- ionised gas (mainly found in outer space)
Determination of the state of matter
Matter can exist in different states depending on temperature and pressure
Different physical properties of matter
Are due to:
- Different arrangement and movement of particles
- Depends on amount of kinetic energy of that particle
Kinetic energy
Energy related to the motion of an object
Properties of solids
- particles are closely packed
- strong forces between particles, vibrate about fixed positions
- fixed shape
- fixed volume
Properties of liquids
- particles are more spread out than in solids
- weaker forces between particles, they can move past each other
- take the shape of the container
- fixed volume
Properties of gases
- particles are very spread out
- negligible forces between particles, they move randomly
- no fixed shape
- no fixed volume
Changes of state
Directly related to changes in temperature
- increase in temp. = increase in avg. KE of particles in a substance
- when heated, particles gain KE + able to intermolecular forces that exist between them
- results in a change of state
Intermolecular forces
Attractive forces that exist between particles
Changes of state:
- SOLID to LIQUID
- LIQUID to GAS
- SOLID to GAS (no liquid state)
- GAS to LIQUID
- LIQUID to SOLID
- GAS to SOLID (no liquid state)
- Melting (energy absorbed)
- Evaporation/Boiling (energy absorbed)
- Sublimation (energy absorbed)
- Condensation (energy released)
- Freezing (energy released)
- Deposition (energy released)
Evaporation vs. Boiling
Evaporation:
- change of a liquid to a gas
- BUT only takes place at surface of a liquid
- can occur at temperatures below BP of liquid
Boiling:
- change of a liquid to a gas
- takes place throughout liquid (bubbles of gas are formed within the liquid, not only at surface)
- occurs at a specific temperature
Steps of the heating curve of a solid
- Upward slopes, temp. increases as substance is heated
- KE of particles increases, and they vibrate faster
- BUT, during changes of state, temp. remains constant. At these points, energy is used to overcome intermolecular forces between particles
- During melting, energy input is used to overcome intermolecular forces that hold particles in solid in fixed positions
- During boiling, energy input is used to overcome intermolecular forces that hold particles in liquid together
- Hence, during changes of state, temp. remains constant
- Once change of state is complete, temp. starts to increase again
Elements
- made up of same kind of atom
- can’t be broken down by chemical means into a simpler substance
- can be divided into metals, non-metals and metalloids (properties of both)
Atom
- smallest particle that shows characteristic properties of that element
Compounds
A substance composed of two or more different elements that are chemically combined
- when atoms of different elements react, they lose their characteristic properties
- properties of the elements are replaced by those of new compound formed in chemical reaction
Molecule
Consists of two or more atoms that are chemically bonded together
Properties of molecules
- not all molecules can be classes as compounds, as they are composed of same kind of atom bonded together
- electrically neutral, although some have a dipole
Mixture
Composed of two or more substance that aren’t chemically combined- each substance retains its original properties