chemistry matter Scientific Method Technology Observation Theory Experiment Applied Chemistry

1. Inorganic Chemistry Inorganic is the study of matter that does NOT contain ________ Inorganic chemists study the structure, function, synthesis, and identity of non-carbon compounds Polymers, Metallurgy Carbon

2. Organic Chemistry Organic is the study of matter that contains ______ Organic chemists study the structure, function, synthesis, and identity of carbon compounds Useful in petroleum industry, pharmaceuticals, polymers carbon

3. Physical Chemistry Physical chemistry is the physics of chemistry… the forces of matter Rates and energy transfers Much of p-chem is computational

4. Analytical Chemistry Analytical chemistry is the study of high precision measurement Find composition and identity of chemicals Lead in drinking H2O Forensics, quality control, medical tests

5. Biochemistry Biochemistry is the study of chemistry in ______ things Cross between biology and chemistry Pharmaceuticals and genetics living

Properties of Matter Extensive properties depend on the amount of matter that is present. Extensive properties Volume Mass Energy Content (think Calories!) do not depend on the amount of matter present, but type of matter. Intensive properties Melting point, Boiling point Color Density Hardness

Law of conservation of mass In all physical and chemical changes, the mass of the reactants MUST equal the mass of the products.

Scientific Method State the problem clearly./Make Observ. Formulate a hypothesis Test the hypothesis. Evaluate the data to form a conclusion. If the conclusion is valid, then it becomes a theory. If the theory is found to be true over along period of time (usually 20+ years) with no counter examples, it may be considered a law. 5. Share the results.

Chapter 2

water, ammonia, sucrose, gold, oxygen Chemistry is the study of matter and the changes it undergoes Matter is anything that occupies space and has mass. “stuff” A substance is a form of matter that has a definite composition and distinct properties. water, ammonia, sucrose, gold, oxygen

Phase Differences Solid – definite volume and shape; particles packed in fixed positions. Liquid – definite volume but indefinite shape; particles close together but not in fixed positions Gas – neither definite volume nor definite shape; particles are at great distances from one another Plasma – high temperature, ionized phase of matter as found on the sun.

Physical Properties What are some physical properties? color melting and boiling point odor Create a definition for “physical properties”

Physical Changes boiling of a liquid melting of a solid can be observed without changing the identity of the substance Physical change Ex. boiling of a liquid melting of a solid dissolving a solid in a liquid to give a homogeneous mixture — a SOLUTION.

soft drink, milk, salt water A mixture is a combination of two or more substances in which the substances retain their distinct identities. Homogenous mixture – composition of the mixture is the same throughout. soft drink, milk, salt water Heterogeneous mixture – composition is not uniform throughout. Rocky Road Ice Cream, soil, pizza chicken noodle soup

Types of Mixtures Heterogeneous – visibly separate phases Homogeneous – Same throughout

Physical means can be used to separate a mixture into its pure components. distillation magnet Filtration

Separation of a Mixture Distillation

Separation of a Mixture The components of dyes such as ink may be separated by paper chromatography.

An element is a substance that cannot be separated into simpler substances by chemical means. “116” elements have been identified 82 elements occur naturally on Earth gold, aluminum, lead, oxygen, carbon 34 elements have been created by scientists technetium, americium, seaborgium

A compound is a substance composed of atoms of two or more elements chemically united in fixed proportions. Compounds can only be separated into their pure components (elements) by chemical means. Water (H2O) Glucose (C6H12O6) Ammonia (NH3)

Separation of a Compound The Electrolysis of water Compounds must be separated by chemical means. With the application of electricity, water can be separated into its elements Reactant  Products Water  Hydrogen + Oxygen H2O  H2 + O2

Can it be physically separated? Matter Flowchart Fill in the flow chart AND provide and example for each box. Matter yes no Can it be physically separated? Mixture Pure substance Is the composition uniform? no yes Can it be chemically decomposed? no yes Homogenous Heterogenous Compound Element

Organization of Matter a) Homogeneous (Solutions) Mixtures: a) Homogeneous (Solutions) b) Heterogeneous Pure Substances Elements Compounds Atoms Nucleus Electrons Protons Neutrons Quarks Quarks

Physical vs. Chemical Properties Examples: melting point flammable density magnetic tarnishes in air

Physical vs. Chemical Changes Examples: rusting iron dissolving in water burning a log melting ice grinding spices Chemical Physical

Sure Signs of a Chemical Change Change in Temp Light Gas Produced (not from boiling!) Precipitate – a solid formed by mixing two liquids together Color Change???

Chemical Properties and Chemical Change Chemical Property - Ability of a substance to undergo a chemical change Examples: Chemical Change – Change that produces matter with a different composition than the original matter.

Pure Chemistry – pursuit of chemical knowledge for its own sake. Use it or not? Pure Chemistry – pursuit of chemical knowledge for its own sake. Applied Chemistry – research that is directed toward a practical goal or application.