1 / 10

Vocabulary

Vocabulary. Write the terms and definitions for each vocabulary word from sections 2-1, 2-2 and 2-3. Keep these pages in your vocabulary divider. Extra credit if you use this format (1/2 pt. for each term). Chapter 2 The Chemistry of Life. 2-1: The Nature of matter. Atoms.

agnes
Download Presentation

Vocabulary

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. Vocabulary • Write the terms and definitions for each vocabulary word from sections 2-1, 2-2 and 2-3. Keep these pages in your vocabulary divider. • Extra credit if you use this format (1/2 pt. for each term)

  2. Chapter 2The Chemistry of Life 2-1: The Nature of matter

  3. Atoms • KeyC#1: What three subatomic particles make up atoms? • The subatomic particles that make up atoms are protons, neutrons and electrons. • Atom: basic unit of matter • Protons: (+) charge • Neutrons: no charge (neutral) • Electrons: (-) charge • How small is an atom?? • http://ed.ted.com/lessons/just-how-small-is-an-atom • Sketch figure 2-1 in your lecture notes.

  4. Elements and Isotopes • What are elements? • Let’s look at the periodic table of elements. (Appendix G) • KeyC#2: How are all the isotopes of an element similar? • Because they have the same number of electrons, all isotopes of an element have the same chemical properties. • Facts to know about elements: • Atomic number = # of protons • Atomic mass = sum of protons & neutrons • Isotopes differ in the number of neutrons • Some isotopes are radioactive • Let’s practice with some of the elements…

  5. Chemical Compounds • What is a chemical compound? • What are some examples of chemical compounds? • Physical and chemical properties of a compound are usually very different from those of the elements from which it is formed. (i.e. Na & Cl)

  6. Chemical Bonds • What holds atoms together? • What is the key player in these bonds? • KeyC#3: What are the two main types of chemical bonds? • Ionic and covalent bonds • Ionic bonds: transfer of electrons • Covalent bonds: sharing of electrons • Let’s look at figures 2-3 & 2-4 • What are molecules? • What does sharing electrons mean? • Electrons will travel in both orbits • 2 electrons = single bond • 4 electrons = double bond • Van der Waals forces: oppositely charged regions of molecules attract each other (intermolecular attraction)

  7. Chapter 2 The Chemistry of Life 2-2 Properties of water

  8. The Water Molecule • How is water neutral? • KeyC#1: Why are water molecules polar? • Uneven distribution of electrons between the hydrogen and oxygen atoms. • Oxygen (-) • Hydrogen (+) • Let’s draw! • Why are polar molecules attracted to each other? • What is the difference between COHESION and ADHESION? • What are some examples of each? • http://ed.ted.com/lessons/how-polarity-makes-water-behave-strangely-christina-kleinberg#watch

  9. Solutions and Suspensions • What is a mixture? Give me some examples of mixtures. • Physically mixed, but not chemically combined • Solution: solutes evenly distributed throughout the solvent (i.e. salt water) • Solute is diluted • Solvent is the disSOLVEr • Suspensions: materials that do not dissolve but are suspended (i.e. blood)

  10. Acids, Bases, and pH • What is the range of the pH scale? • What is an acid? • Substance with more H+ ions than pure water. pH < 7 • What is a base? • Substance with lower concentrations of H+ than pure water. pH > 7 • What do buffers do?

More Related