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Chemistry

Chemistry. Matter. All living things are made of matter Cannot be created or destroyed. Atoms. Smallest unit of an element that still has the same chemical properties Three subatomic particles Protons + (inside nucleus) Neutrons 0 (inside nucleus) Electrons – (outside nucleus).

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Chemistry

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  1. Chemistry

  2. Matter • All living things are made of matter • Cannot be created or destroyed

  3. Atoms • Smallest unit of an element that still has the same chemical properties • Three subatomic particles • Protons + (inside nucleus) • Neutrons 0 (inside nucleus) • Electrons – (outside nucleus)

  4. Periodic Table • Letter is the atomic symbol • Atomic number is how many protons the atom has • Atomic mass is the number of protons and neutrons • In a neutral atom protons And electrons will be the same

  5. Element • substances that can’t be broken down chemically into simpler substances • Examples- • Hydrogen • Oxygen

  6. Molecule • 2 or more atoms come together to make a molecule • Examples • H2 • H2O • C4

  7. Compound • 2 or more elements together in a fixed ratio. • Examples: • H2O, NH3, NaCO3 • For every 1 oxygen, there are 2 hydrogens • All compounds are molecules, but not all molecules are compounds

  8. Electron shells • Areas of electrons around the nucleus • Atoms have 2 electrons in the first shell • 8 in the following shell • Sulfur can bond with 2 other molecules

  9. Valence Electrons • The amount of electrons in the outer shell • Determine chemical properties • Determine how many bonds they can make

  10. Valence Electrons • When outer most energy shell is not full, atoms find ways to fill energy shells by taking, giving away or sharing electrons

  11. Lewis Dot Diagrams • An easy method to show outer energy shell and predict how the elements will bond together. • Shows valence electrons only

  12. Types of bonds • Ionic Bonds- One or more electrons get passed to another element • Very weak bond • Na will pass one e- • Chlorine will accept one e-

  13. Types of bonds • Covalent bonds- Share electrons between two elements • Very strong bond • Polar covalent- shares electrons unequally (will be a charge) • Non-polar covalent- shares electrons equally

  14. Types of bonds • Hydrogen bonds- attractive interaction of a hydrogen atom with an electronegative atom • Weak by itself • Strong when there are many Water depends on H-bonds

  15. Chemical reactions (rxn) • Making or breaking of chemical bonds • Reactants- left side of the equation, what goes into reaction • Products- right side of the equation, what comes out of the reaction • Comment: All atoms in the reactants must be accounted for in the products

  16. Chemical rxn examples • 2H2O  2H2 + O2 • H + Cl  HCl • Number at front means 2 water molecules • Subscript numbers represent the amount of H in the molecule

  17. Biochemistry • Study of compounds found in living things • Organic compounds- always contain Carbon • Important Elements in Biology: HONC P S • HONC for Biology!!

  18. Metabolism • All chemical activities and changes that happen in a cell or organism • synthesis: building up • decomposition: breaking down

  19. Types of reactions • Synthesis rxn- Simple molecule + simple molecule  Complex molecule Decomposition rxn- Complex molecule  simple molecule + simple molecule

  20. Bonds • Making complex molecules takes energy! • Breaking down a complex molecule releases energy!

  21. Homework/Classwork • Draw one square from the periodic table on a half sheet of computer paper. Include: • Atomic number • Atomic mass • Name of element • Lewis Dot diagram • 5 pictures of molecules that include your element • 3 reasons why your element is important in Biology (being part of living things is not enough)

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