Chapter 3-4 Flashcards
Scientific Perspective
Leads to research and explains natural phenomena
Technological Perspective
Concerned with development and use of machines instruments and processes that have a social purpose
Ecological Perspective
Considers relationships between organisms and the environment
Economic Perspective
Focuses on the production, distribution, and consumption of wealth
Political Perspective
Involved governments, vote, getting actions, or arguments based on ideology
Physical Change
Any changes where the fundamental entities remain unchanged at a molecular level, there is no change in the chemical formula
Chemical Change
Involves some kind of change in the chemical bonds within the fundamental entities of a substance, there is a change in chemical formula. New substance
Is formed with different physical and chemical properties
Nuclear Change
Changes within the nucleus, creates entirely new atomic entities, formulas show new atomic symbols different from original matter
Kinetic Molecular Theory
Smallest entities of a substance are in continuous motion
Why do chemical reactions occur
Collisions between entities, if the collision has a certain orientation and sufficient energy they will rearrange to form new entities
Evidence for Chemical Reactions
Colour change, odour change, state change (formation of a precipitate), energy change (release or absorption)
Law of conservation of mass
The total mass of matter present after a chemical change is always the same as total mass present before
Balanced Chemical Equation
Total number of each kind of atom or ion in the reactants is equal to the total number of the same kind of atom or ion in the products
Chemical amount
SI quantity for the number of entities in a substance measured in units of moles
Avogadro’s number
6.02 x 10^23 (mole)
Mole
Unit of chemical amount of substance with number of entities corresponding to Avogadro’s number
Molar mass
Molar mass of a substance is the mass of one mole of the substance (unit grams per mole)
Formation reaction
Reaction of 2 or more elements to form an ionic compound
Simple Decomposition
Breakdown of a compound into its elements
Complete Combustion Reaction
Burning of a substance with sufficient oxygen available to produce most common oxides of the elements making up the substance that is burned (ectothermic)
Solute
Substance being dissolved
Solvent
Substance that does the dissolving
Solubility
Maximum quantity of the substance that will dissolve in a solvent at a given temp
Precipitate
Solid substances formed from reactions in solution
Single replacement
Reaction of an element with a compound to produce a new element and an ionic compound
Double Replacement
Between 2 ionic compounds, they change partners
Neutralization
Double replacement reaction where an acid reacts with a base, producing water and an ionic compound
