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Chapter 1. The Science of Chemistry. Chemistry. What is Chemistry? -The study of the composition, structure and properties of matter and the reactions by which matter may be formed or converted into other forms. Classification of Matter
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Chapter 1 The Science of Chemistry
Chemistry • What is Chemistry? • -The study of the composition, structure and properties of matter and the reactions by which matter may be formed or converted into other forms. • Classification of Matter • Matter - an object that has mass and takes up space (volume)
Mixtures • 1. Mixture- Two or more kinds of matter that can be separated by physical means. • Techniques for physical separations- filtration, straining/sifting, magnetism, & distillation • a. heterogeneous mixture - non-uniform distribution of matter • b. homogeneous mixture - uniform distribution • solution- another name for a homogeneous mixture
Pure Substance- matter that cannot be separated by physical processes • a. Element- cannot be broken down into simpler forms of matter • b. Compound- pure substances that can be broken down into simpler forms only by chemical processes.
Chemical reactions • Chemical Changes- A change in matter that produces new substances with new properties (chemical reaction) • a. reactants- substances that undergo changes • b. products- new substances that are formed • precipitate- a solid produced from solution during a reaction
Ten signs of chemical change • 1. Bubbles of gas appear • 2. A precipitate forms • 3. A change in color • 4.Temperature changes • 5.Light is emitted • 6.A change in volume • 7.A change in electrical conductivity • 8.A change in melting or boiling point • 9.A change in smell or taste (not to be performed in lab) • 10.A change in chemical or physical properties
States of matter • Solid- uniform shape, volume and low internal heat • Liquid- variable shape, uniform volume and medium internal heat • Gas- variable shape, volume and high internal heat
Density • Density is amount of mass per unit of volume… units are based on what you are given • Standard is g/mL • D=M/V • M= DxV • V=M/D
Converting • Factor-Label !!! • 1. Read the problem carefully; determine what is being solved for. • 2. Tabulate the data given. Label measurements with units; use correct factors (powers of ten). • 3. Determine which unit relationships are necessary. • 4. Set up the problem in a logical fashion; make sure unwanted units cancel. Use the conversion equation for converting from one unit to another.