1 / 15

All-you-need-to-know Inorganic Chemistry for Honors Biology students (ch. 2)

All-you-need-to-know Inorganic Chemistry for Honors Biology students (ch. 2). Chemistry in Biology / Organic Chemistry Unit Atoms, Elements, and Compounds (2.1 part 1). Chemistry is the study of matter and how it combines to form new substances.

walt
Download Presentation

All-you-need-to-know Inorganic Chemistry for Honors Biology students (ch. 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. All-you-need-to-know Inorganic Chemistry for Honors Biology students (ch. 2)

  2. Chemistry in Biology / Organic Chemistry Unit Atoms, Elements, and Compounds (2.1 part 1) Chemistry is the study of matter and how it combines to form new substances. Organic and inorganic matter are both made of atoms. The atoms in organic matter are arranged in larger,more complex units or “biomolecules.”

  3. Hierarchy / Levels of Organization of Matter in the Biosphere Chapters 2 &3 Atoms biological molecules  Organelles  Cells  Tissue  Organ  Organ system  Organism  Population  Community  Ecosystem  Biosphere Atoms are the inorganic building blocks that make up organic matter.

  4. Levels of Organization of Matter in the Biosphere     ETC…

  5. Atoms - The Building Blocks of Matter • Protons are positively charged particles. • Neutrons are particles that have no charge. • Electrons are negatively charged particles that are located outside the nucleus. • The first shell/orbital of an atom fits 2 electrons; the next two shells fit 8 electrons.

  6. Comparing the Parts of an Atom Mass in AMUs (Atomic Mass Units)

  7. Atoms, Elements, and Compounds Elements • An element is a pure substance that cannot be broken down into other substances by physical or chemical means. • There are over 100 known elements, 92 of which occur naturally. • Each element has a unique name and symbol. • Elements are defined by their atomic number, or number of protons. Aluminum Gold Helium Silver

  8. Most Abundant Elements in the Human Body (~70% of body weight is water, H2O!) Calcium (Ca) (needed for bones, muscle contraction) Nitrogen (N) (normally a gas, here a liquid, makes up most of air, needed for proteins and DNA) Oxygen (O) (normally a gas, here a blue liquid; most abundant in body, needed to get energy from food, found in water and air) Carbon (C) (found in all organic molecules) Hydrogen (H) (ionized gas, In a galaxy, found in water and air) Chlorine (Cl) (gas) Phosphorus (P) (found in DNA) Magnesium (Mg) (silver color) Potassium (K) Sulfur (S) Sodium (Na)

  9. Element song

  10. Abbreviated Periodic Table / Chart 6 C 12.01 Atomic Number  Element Symbol  Atomic Mass  (a.m.u.)

  11. Introduction to the Periodic Table • The periodic table shows all of the known elements in order of increasing atomic number. • The periodic table is organized to group elements with similar properties in vertical columns. • Nonmetals  • (right of “stairs”) The elements we will use are in these areas  Metals (left of “stairs”)

  12. Atomic Number, Mass Number, Atomic Mass • Atomic number = no. of protons (p+), identifies the element • The atom is neutral (net charge = 0), thereforeno. protons = no. electrons • Mass Number = no. of atomic mass units in nucleus = no. protons + no. neutrons(1 a.m.u. = mass of one nuclear particle) • Atomic Mass = average mass of all isotopes (different atoms)of an element in a.m.u. round the atomic mass  mass number

  13. Isotopes • Isotopes are atoms of the same element (same number of protons) that have different numbers of neutrons (and different mass no.) • Symbol for isotope – element symbol-mass no.: C-12, C-14, Na-23, Na-24, etc.

  14. Heavy or radioactive isotopes can be used for many applications in industry, medicine, environmental science, etc. In medicine, less common stable and radioactive isotopes, are used as biological tracers.

More Related