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FOUNDATIONS OF MATTER NOTES

This resource provides comprehensive notes on the properties of matter, including its composition, physical and chemical properties, and separation techniques. It also covers the concept of atoms, ions, and isotopes, as well as the early history of atomic theory.

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FOUNDATIONS OF MATTER NOTES

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  1. FOUNDATIONS OF MATTER NOTES

  2. Matter mass • MATTER- has _____________ and occupies ____________________. • All matter consists of tiny particles called ________________. space atoms

  3. Solid Gas Liquid fixed • SOLID- has a _______ shape and volume • LIQUID- has a _______ volume but takes the shape of the container • GAS- has ___________fixed volume or shape definite no

  4. characteristic • PHYSICAL PROPERTIES- a __________________ of a substance that can change without the substance becoming a different substance • CHEMICAL PROPERTIES- the _____________ of a substance to change into a different substance • PHYSICAL CHANGE- a change in the _________ of a substance, but not in its _________________ nature; chemical bonds are not broken in a physical change • CHEMICAL CHANGE- the change of substances into _____________ substances through a ______________ of the atoms; a ________________________ ability form chemical reorganization other chemical reaction

  5. Matter Prezi: http://prezi.com/kbcpimj8z80o/?utm_campaign=share&utm_medium=copy

  6. Learning Check Compound Element, diatomic Compound Heterogeneous mix. Element Heterogeneous mix. Heterogeneous mix. Heterogeneous mix. Heterogeneous mix., emulsion/suspension Homogeneous mix., solution Homogeneous mix., solution, alloy Heterogeneous mix. Element, diatomic Homogeneous mix., solution Homogeneous mix., solution Element Homogeneous mix., solution Heterogeneous mix., suspension Element Compound • Element, Compound or Mixture?

  7. Separation Techniques • DISTILLATION- a method of separating the components of a ___________ that depends on the differences in the ease of vaporization of the components liquid

  8. FILTRATION- a method of separating the components of a mixture containing a ____________ and a ____________. solid liquid

  9. CHROMOTOGRAPHY – a method of separating components of a heterogeneous mixture by their polarities. • Ex. Separating components of ink on paper

  10. Separating a Mixture Lab

  11. Formulas of Compounds 1. Symbols - • used to represent the element • first letter is capital, second letter (if necessary) is lower case 2. Subscripts – • small number to the lower right of the element symbol • represents the relative composition of each element in a compound or molecule 3. Superscripts – • small number to the upper right of the symbol/formula • used to represent the charge of an ion 4. Coefficients – • big number in front of the formula • indicates the number of compounds present C = carbon Ca = calcium Cr = chromium CO2 = 1 carbon, 2 oxygen Ba(NO3)2 = 1 barium, 2 nitrogen, 6 oxygen Ca+2 Br-1 NO3-1 3 CO2 = 3 carbon dioxide or 3 carbon, 6 oxygen

  12. Protons 1. ____________ charge 2. mass is almost equal to the mass of the ___________ 3. Found in the _____________ 4. Number of protons is __________ to the atomic number Neutrons 1. ____________ charge 2. mass is __________________________ than the proton 3. Found in the _____________ 4. Neutrons act as the glue that holds together the nucleus. - too few or too many neutrons can result in nuclear instability and then radioactivity Electrons 1. ____________ charge 2. mass is ___________________ than the proton 3. Found moving around the nucleus at near the speed of light. - sometimes called _______________________ or ______________________ 4. The Quantum Mechanical Model - currently accepted model of the atom (Chapter 11) - for now we will use the Bohr model, rings of electrons Modern Concept of the AtomThe atom is made of three elementary particles. positive negative 2000 x less neutrons nucleus equal charge cloud electron cloud no or neutral slightly greater nucleus

  13. neutral same • Atoms are always _____________ • Isotopes • Atoms with the __________ number of protons but a ______________ number of neutrons • A different number of neutrons results in a different mass. • Mass of individual atoms is determined by only the protons and neutrons, the electrons are too light to be significant. • Mass Number = __________ + ___________ • Isotope notations • 40K means that potassium has a mass number of 40 • Potassium-40 also means a mass number of 40 different protons neutrons

  14. 23Na 35Cl 17 11 X A Z X = Element symbol Z = Atomic number = # of protons in nucleus = # on periodic table A = Mass number = # of protons + # of neutrons in nucleus 14 6 8 6 6 18 17 17 11 11 23

  15. Ions Electron When an atom gains or loses an __________________ it takes on a charge and becomes an ion the charge is determined by the #e- (negative charge) when compared to #p+ (positive charge) Calcium ions (Ca+2) has 20 p+ and 18 e- because the calcium atom lost 2 electrons Fluoride ions (F-1) has 9 p+ and 10 e- because the fluorine atom gained one electron Positive Ions are called _______________ Negative Ions are called _______________ Cations Anions 14 6 8 10 6 35 17 18 18 17 23 11 23 10 11

  16. Early History of the ATOM • Democritus (Greek Philosopher 460 B.C.) 2. Dalton’s Atomic Theory Elements are made of tiny particles called ____________. All atoms of the same element are ________________ . (Not really but close, isotopes) Atoms of a given element are ________________ from those of any other element. Atoms of one element will combine with other atoms to form _________________ . Atoms are __________________ during chemical reactions; they are never created or destroyed. (He was not talking about nuclear reactions) Atoms are indivisible and everywhere Atoms identical different compounds indivisible

  17. Atomic Theory Timeline

  18. Average Atomic Mass • Average Atomic Mass – the weighted average of the masses of the isotopes of an element • Every element is composed of several naturally occurring isotopes of that element-each with its own atomic mass • A weighted average of the percentage of each isotope that exists versus the atomic mass of each isotope is used to calculate the atomic mass that appears on the periodic table. Step 1) Change each percent abundance into a decimal weight. Step 2) Multiply each atom’s mass by its decimal weight to get the contribution for each isotope. Step 3) Add all the contributions together to get the average atomic mass. • Has units of amu, atomic mass unit.

  19. Average Atomic Mass = Σ [(isotope mass) * (percent abundance of isotope)] 100 Example 1: The element copper occurs naturally as 69.17% of copper-63 with a mass of 62.9296 amu and 30.83% of copper-65 with a mass of 64.9278 amu. What is the average atomic mass of copper?

  20. Example 2: The atomic weight of gallium is 69.72 amu. The masses of the naturally occurring isotopes are 68.9257 amu and 70.908 amu for 69Ga and 71Ga respectively. Calculate the % abundance of each isotope.

  21. Learning Check Naturally occurring element consists of 75.78% atoms with a mass of 34.969 amu and 24.22% atoms with a mass of 36.966 amu.  Calculate the average atomic mass. b) Based on the average atomic mass, what is the element?

  22. Nuclear Reactions

  23. Nuclear Reactions vs. Normal Chemical Changes NUCLEAR REACTIONS involve the ___________. PROTONS and NEUTRONS are ______________in the nucleus, releasing a tremendous amount of energy. “Normal” CHEMICAL REACTIONS involve _____________, not protons and neutrons. NUCLEUS REARRANGED ELECTRONS

  24. Why do Nuclear Reactions happen? Nuclear Instability The stability of a nucleus is dependent on the neutron to proton ratio (N:Z) For light nuclei (elements 1-20), the N:Z ratio should be 1:1 For heavy nuclei (elements above 20), the N:Z ratio should be 1.5:1

  25. Atoms that lie either above or below the band of stability will undergo nuclear decay to achieve stability. Atoms that lie ABOVE the band of stability have TOO MANY NEUTRONS. Atoms that lie BELOW the band of stability have TOO MANY PROTONS.

  26. Two Types of Nuclear Reactions Fission ___________– nucleus splits into smaller nuclei to become more stable. • atomic bombs (like those dropped on Hiroshima and Nagasaki). • Nuclear reactors ___________– nuclei fuse into one larger nucleus to become more stable. • the sun (or any star) • Creating elements larger than Element 92 (U) • Elements 1-92 occur naturally in the universe Fusion

  27. Half-Life • Using the known half-life of elements to determine the age of artifacts • Radioisotope: an unstable, radioactive atom that decays over time to become more stable. • Half-Life: the amount of time that it takes half of a radioisotope sample to decay.

  28. Ex 1) Assuming a half-life of 1599 years, how many years will be needed for the decay of 15/16 of a given amount of radium-226? Ex 2) The half-life of radon-222 is 3.824 days. How much time must past for 25% of a given amount of radon to remain? Ex 3) The half-life of radium-224 is 3.66 days. What was the original mass of radium-224 if 0.0800g remains after 7.32 days?

  29. Nuclear Decay RADIATION: particles & electromagnetic waves released during nuclear decay. Most radiation comes from the SUN & COSMIC RADIATION.

  30. 4 2 He 4 2 or Nuclear Decay Products ALPHA particle: α is a Helium-4 nucleus has POOR PENETRATING ability – can be stopped by PAPER.

  31. e e 0 +1 0 -1   0 +1 0 -1 or or Nuclear Decay Products BETA particle: β aka. ELECTRON or NEGATRON has a negative charge A NEUTRON emits a negatron and then BECOMES a PROTON POSITRON aka. ANTIELECTRON has a positive charge A PROTON emits a positron and then BECOMES a NEUTRON Penetrate BETTER than ALPHA particles, but can be stopped by an ALUMINUM sheet.

  32. g 0 0 Nuclear Decay Products GAMMA ray: γ is a gamma PHOTON. has GREAT PENETRATING ability – can ONLY be stopped by LEAD or CONCRETE. is very DANGEROUS. can be released with other forms of decay.

  33. n 1 0 Nuclear Decay Products NEUTRON: n can be ABSORBED or RELEASED during a nuclear reaction combine with other nuclei in secondary reactions, which could create harmful radiation. has GREAT PENETRATING ability – can be stopped by CONCRETE.

  34. Nuclear Decay Products

  35. Yield Reactants Products Nuclear Equations Nuclear equations must be BALANCED. The sum of the MASS NUMBERS and the sum of the ATOMIC NUMBERS must be the SAME on both sides of the equation.

  36. 238 U Th + He 234 4 92 90 2 Alpha Decay Reaction Mass # Change: decrease by ___ Atomic # Change: decrease by ___ 4 2

  37. 14 C N + e 14 0 6 7 -1 Beta Decay Reaction Mass # Change: ______________ Atomic # Change: increase by ___ no change 1

  38. 0 51 Cr + e V 51 24 -1 23 Electron Capture Reaction Mass # Change: ___________ Atomic # Change: decrease by ___ no change 1

  39. 49 Cr V + e 49 0 24 23 +1 Positron Emission Reaction Mass # Change: _____________ Atomic # Change: decrease by ___ no change 1

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