Statue of Liberty Arrives in New York (1885)

1. Statue of Liberty Arrives in New York (1885) • Reading: Chapter 4 sections 1-6 (quiz) • HW #3: DUE Wednesday • 1, 3-7 (all), 11, 13, 17, 18, 21-31 (odd), 39, 45, 49, 50, 51, 56 (only assignment from this chapter) • HW#4.1: DUE Thursday • 9-13 (all), 17, 19, 20, 23, 25, 29, 31, 35, 37, 42, 46, 51, 53 • HW #4.2: DUE Monday • 59, 60, 65-79 (all), 83, 84, 85, 89, 94, 95, 99, 101, 103, 106 • For lab tomorrow (wet lab) • You must have your goggles!!!! • You must have a lab book and lab manual

2. Substances have both physical and chemical properties. Physical Properties:Density, color, and melting point are physical properties of matter. Observing a physical property can be done without altering the makeup of a substance.

3. Physical Change: Does not alter the chemical makeup of a substance. • Chemical reactivity is unchanged. • Changes in state, changes in particle size, and the formation / separation of mixtures are all examples of physical change. • Melting of ice to form liquid water is a physical change. In this case only a change in form takes place. The chemical makeup of the substance remains H2O.

4. Phase Transitions!! ADD ENERGY sublimation melting boiling solid liquid gas freezing condensation deposition REMOVE ENERGY

5. Substances have both physical and chemical properties. Chemical Properties:Chemical composition, what matter is made of, and chemical reactivity, how matter behaves, are chemical properties. Observing a chemical property alters the substance.

6. Chemical Change: • Alters the makeup of a substance. • Reactivity changes with the formation of new substances. • Heat, light, or electrical energy is often emitted or absorbed. • Potassium reacting with water is an example of a chemical change.

7. Classification of Matter • Pure Substance: Matter that is constant in its chemical composition and properties. • Mixture: A blend of two or more pure substances in any ratio each retaining their identity. • Physical changes can separate mixtures into one or more pure substances.

10. Element • A pure substance that cannot be broken down into a simpler substance by chemical means. pure substances compound compound element mixture ice cream  sugar  CO2  carbon physical changes chemical changes

11. Each element has its own unique symbol. One or two letter symbols are used to represent elements. The first letter is always capitalized and the second letter is always a lower case. Examples: C, Cr, P, Pb Most are “easy” to remember. ‘H’ for hydrogen, ‘O’ for oxygen, ‘N’ for nitrogen Some are more difficult to learn. ‘Na’ for sodium (from its Latin name Natrium) ‘Pb’ for lead (from its Latin name Plumbum)

13. Pure Substances Chemical Compounds: Two or more elements combined chemically in specific ratios to form a pure substance. Water = H2O Methanol = CH3OH Nitroglycerine = C3H5(NO3)3

14. Chemical Formula: A notation for a chemical compound using symbols and subscripts to show how many atoms of each element are present. When no subscript is given for an element a subscript of ‘1’ is “understood”.

16. Mixtures Hetero Heterogeneous Mixture: A mixture of matter in which the properties change from sample to sample. change Sand and sugar Quartz and gold

18. Mixtures Homo Homogeneous Mixture: A mixture of matter in which the properties remain constant from sample to sample. constant Salt water Brass Kool-Aid

19. Periodic Table of the Elements Periodic: Having or marked by repeating patterns Table: An arrangement of words, numbers, or symbols, or combinations of them, as in parallel columns, to exhibit a set of facts or relations in a definite, compact, and comprehensive form Elements: A substance that cannot be broke down into simpler substances by chemical means

20. Metals: 90 of the 114 elements are metals. They appear on the left side of the Periodic Table. • Some common properties of metals are: • Solid at room temperature • (except mercury which is a liquid) • Good conductor of heat and electricity • Lustrous on fresh surfaces • Malleable and ductile

21. Metals

22. Metals: • (a) Gold is very unreactive and is used primarily in jewelry and in electronic components. • (b) Zinc, an essential nutrient, is used in the manufacture of brass, roofing materials, and batteries. • (c) Copper is widely used in electrical wiring, in water pipes, and in coins.

23. Nonmetals: Appear on the right side of the Periodic Table. 17elements are nonmetals. • Elevenare gases at room temperature (H, N, O, F, Ne, etc.) • Five are solids (C, P, S, Se, I) • One is a liquid (Br). • Nonmetals are poor conductors of heat and electricity.

24. Non-Metals

25. Nonmetals: • (a) Nitrogen constitutes almost 80% of air and is a colorless gas at room temperature. • (b) Sulfur, a yellow solid, is found in large underground deposits in Texas and Louisiana. • (c) Iodine crystals.

26. Metalloids: Seven elements are metalloids. • Their properties are between those of metals and nonmetals. • Metalloids are semiconductors and are important to the electronics industry.

27. Metalloids

28. Metalloids: • (a) Boron • (b) Silicon

30. Foiled again

32. The Atom • REALLY early atomic theory… • Democritus ~350 BC • Atomos - Greek meaning indivisible • Modern Definition: • Smallest piece that matter can be broken up into and still maintain the properties of an element

33. My Atom Broke • Subatomic Particles • Nucleus • Protons – p+ • Carry a single positive charge • Number of p+ = ATOMIC NUMBER

35. My Atom Broke • Subatomic Particles • Nucleus • Neutrons – no • No charge • # can vary from atom to atom • Roughly the same size

36. My Atom Broke • Subatomic Particles • Outside the nucleus • Electrons – e- • Carry a single negative charge • 1/1900th the size of p+ and no • Responsible for most of the chemistry that ever happens