1 / 23

Chapter 2

Chapter 2. Dr. C.’s AP Chemistry Lake Dallas High School Fall 2014. Law of Conservation of Mass. Mass is neither created nor destroyed in a chemical reaction (it just changes form) Burning of a candle. Law of Definite Proportion.

uriel
Download Presentation

Chapter 2

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 2 Dr. C.’s AP Chemistry Lake Dallas High School Fall 2014

  2. Law of Conservation of Mass • Mass is neither created nor destroyed in a chemical reaction (it just changes form) • Burning of a candle

  3. Law of Definite Proportion • A given compound always contains exactly the same proportion of elements by mass • H2O

  4. Dalton’s Atomic Theory • Each element is made up of tiny particles called atoms • The atoms of a given element are identical; the atoms of different elements are different in some fundamental way • Chemical compounds are formed when atoms of different elements combine with each other. • Chemical reactions involve reorganization of the atoms (different bonding) but the atoms are not changed.

  5. History of Atomic Theory

  6. Modern Atomic Structure • Nucleus (10-13 cm diameter) • Electrons (avg. distance 10-8 cm from nucleus) • Nucleus contains: • Protons & Neutrons • Nucleus accounts for almost all of the atoms mass.

  7. Number of electrons determines the chemical properties of an atom. • The number of protons determines the identity of the atom

  8. Practice • Ca • Fe • Fe2+ • Br-

  9. Groups/Families have similar chemical properties Atomic Radius increases down the groups

  10. Isotopes • Same number of protons, different number of neutrons. • Dalton’s assumption that all atoms of the same element were identical in all their properties.

  11. Which Carbon isotope is the most common/abundant? 12C 13C 14C Why?

  12. Charges on Transition Metals • PbCl2 • MnO2 • CuCl ** Charges must balance each other **

  13. Polyatomic Ions (p. 65 in your book)

  14. Naming Ionic CompoundsFrom Formula to Name • Metal + Non-metal OR Metal + Polyatomic • 1st Name the cation. • If the cation is a transition metal its charge must be written in ( )’s. • 2nd Name the anion and change its ending to -ide OR Write full name of the polyatomic anion

  15. Practice • CoBr2 • Al2O3 • CaCl2

  16. Naming Ionic CompoundsFrom Name to Formula • Metal + Non-metal OR Metal + Polyatomic • 1st Write the symbol for the cation and its charge. • 2nd Write the symbol for the anion and its charge • 3rd Circle the charges and “cross” them to balance charges.

  17. Practice • Gallium Bromide • Manganese (IV) Oxide • Lead (II) Chloride • Calcium hydroxide

  18. Homework Wednesday We Will Discuss Naming Covalent Compounds and Naming Acids • Work on your journal article • Read pages 54 – 70 • Start on Homework #2 (page 72- 80) 5, 12, 23, 24, 36, 42, 50, 56, 58, 64, 68, 72, 74, 76, 78, 80, 84, 86, 90, 94, 96, 98, 112, 120

More Related