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Chemistry: THE STUDY OF MATTER

This article provides an overview of the study of matter in chemistry, including its different states, the conservation of matter, basic types of matter, elements and compounds, and atomic structure.

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Chemistry: THE STUDY OF MATTER

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  1. Chemistry:THE STUDY OF MATTER

  2. So what is matter?

  3. Matter • Must have mass • It is different from weight…..Why? • Must occupy space (have volume)

  4. Therefore: all matter has a measurable density • Density of a Substance = Mass Volume

  5. States of Matter • Matter can exist in three basic states: • Solid (s), Liquid (l), Gas (g) • How are these states different from each other?

  6. Can Matter be Destroyed? • Example: • When 400 grams of wood are burned only about 30 grams of ash remain. • Why does the matter weigh less? • What happened to the missing matter?

  7. Law of Conservation of Matter • Matter cannot be created or destroyed Matter isn’t being lost but changing in form!

  8. During reactions atoms are all still there, they just get rearranged

  9. Chemical equations are “balanced” with coefficients to obey this law.

  10. Basic Types of Matter

  11. Elements • Made of atoms of one specific type • Have specific properties. • Cannot be broken down further by a chemical reaction

  12. Examples of Elements

  13. Elements and Their Symbols • Element symbols are composed of either one or two letters • If two letters, the second letter is written lower case. • Ex: • Write Cu for copper not CU • Why is this so important?

  14. Just Read: • Usually it is pretty easy to match an element to its symbol (Ex: Neon = Ne) • Sometimes the symbol is derived from a Latin name for the element. • Ex: Au = gold (comes from Latin word aurum)

  15. Na = sodium K = potassium Fe = iron Cu = copper Sb = antimony Sn = tin Pb = lead Hg = mercury W = tungstun Au = gold Ag = silver Some Tricky Elements

  16. Phases of Elements at STP • Gases: • H, He, Ne, Ar, Kr, Xe, Rn, N, O, F, Cl • Liquids: • Hg, Br • Solids: • All other elements are solids • Let’s make a note of these on our Periodic Tables!

  17. Diatomic Elements • Composed of two identical bonded atoms • Note: Most elements are monoatomic in pure form. Who are they? • Remember BrINClHOF • Let’s make a note of these on our Periodic Tables!

  18. Compounds • Two or more different elements bonded together Ex: C6H12O6, NO2, CO2, NaCl • Note: Most elements in nature do not exist in their pure state, but in compounds. • Why? They are more “stable” that way.

  19. Compounds have formulas that show the proportion of elements to each other. • Ex: Water is always H2O • This is called the “Law of Definite Proportions”

  20. Compoundshave different properties than the elements they are composed of. Ex: Sodium (Na) Toxic metal Chlorine (Cl) Toxic gas Sodium Chloride (NaCl) White edible crystal

  21. Focus Question • What makes atoms of one element different from another? • http://www.pbslearningmedia.org/asset/lsps07_int_theatom/

  22. Atomic Basics • Atoms consist of three basic parts. • Protons • Neutrons • Electrons

  23. Fill in Chart:

  24. Atomic Number: • Tells us the number of protons in nucleus • It is unique for each element

  25. Atomic Charge • Atoms are neutral particles • Number of electrons (-) = number of protons(+) • How many electrons does an atom of carbon have?

  26. Nuclear Charge • Nuclear Charge: • the charge on the nucleus of the atom. • (+) positive charge = to number of protons What is the Nuclear Charge? What is the Atomic Number? What is this Element?

  27. Ionic Charge • Ions: atoms with a charge • Protons don’t equal electrons!! • Atom has gained or lost electrons • Gain electrons: become (-) ion • Lose electrons: become (+) ion P = 9 E = 10 What is the element? What is it’s ionic charge?

  28. Ionic Charge Practice Try a few for practice…

  29. Finding the Atom’s Mass • Mass Number: • Sum of the number of protons + neutrons • Each has a mass of 1 amu. (atomic mass unit) Ex: P = 23 N = 21 What is the Atomic Mass Number? What is this element?

  30. Isotopes • Isotopes: atoms of the same element with different atomic mass. • Same # protons • Different # neutrons • Ex: Carbon-12, Carbon-13, Carbon-14 • How many protons? • How many neutrons?

  31. Average Atomic Mass: • Atomic mass you see on periodic table • Represents the average mass of all the isotopes of an element in a typical sample. • Based upon abundance of each isotope and their mass

  32. Calculating Average Atomic Mass • Mass of each isotope x abundance (change % abundance to decimal) • Add together answers • Ex: Chlorine

  33. Crash Course Kids: What is Matter? • https://www.youtube.com/watch?v=ELchwUIlWa8&safe=active • Crash Course: Atomic Basics • https://www.youtube.com/watch?v=FSyAehMdpyI

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