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1 st Six Weeks Review

1 st Six Weeks Review. Chemistry. 1. What are the 4 parts of Dalton’s Atomic Theory?. All matter is made up of atoms Atoms cannot be divided Atoms combine in whole # ratios (1:2, 2:3, etc) to form compounds Compounds react to form new substances during reactions.

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1 st Six Weeks Review

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  1. 1st Six Weeks Review Chemistry

  2. 1. What are the 4 parts of Dalton’s Atomic Theory? • All matter is made up of atoms • Atoms cannot be divided • Atoms combine in whole # ratios (1:2, 2:3, etc) to form compounds • Compounds react to form new substances during reactions

  3. 2. Describe J.J. Thompson’s contribution to atomic theory and find a picture to illustrate it. • Discovered the Electron • Used Cathode Ray tube experiment

  4. 3. Describe Ernest Rutherford’s contribution to atomic theory and find a picture to illustrate it. • Discovered the nucleus • Used the gold foil experiment – shooting alpha particles at gold foil- some particles went through, some bounced off in all directions.

  5. 4. Describe Niels Bohr’s contribution to atomic theory and find a picture to illustrate it. • Proposed the planetary model of the atom • Described Electron energy levels

  6. 5. Describe Eugene Goldstein’s contribution to atomic theory find a picture to illustrate it. • Discovered the proton • Particles going opposite electrons in cathode ray tube.

  7. 6. Describe James Chadwick’s contribution to atomic theory find a picture to illustrate it. • Discovered Neutrons

  8. 7. Describe Erwin Schrodinger contribution to atomic theory find a picture to illustrate it. • Proposed the Quantum Mechanical Model • Orbitals predict location of electrons • Electrons in energy levels • Currently accepted atom model

  9. 8. Find a picture & 3 statements that describe a proton. • Positive charge • Mass = 1 amu or 1.67 x 10-24g • Found in the nucleus

  10. 9. Find a picture & 3 statements that describe a neutron. • Neutral charge • Mass = 1 amu or 1.67 x 10-24g • Found in the nucleus

  11. 10. Find a picture & 3 statements that describe an electron. • Negative charge • Mass = .0005 amu or 1.4 x 10-28g • Moving rapidly around nucleus

  12. 11. True or False: The nucleus contains most of the atom’s volume. • False! • The nucleus contains most of the atoms mass. • The electron cloud contains most of the atoms volume.

  13. 12. Illustrate an element square from the periodic table & label the information it provides.

  14. 13. True or False: Most of the volume of an atom is occupied by the electron cloud. • True!

  15. 14. A neutral carbon atom has how many protons, neutrons & electrons? • Protons = 6 • Neutrons = 6 • Electrons = 6 • Total subatomic particles = ?

  16. 15. Magnesium is classified which of the following: solution, alloy, mixture or pure substance? • Pure substance!

  17. 16. What is an isotope? • Isotope is atom of the same element that has the same # of protons, but a different # of neutrons

  18. 17. What are the three isotopes of hydrogen? How many protons, neutrons & electrons does each one have? Protium Deuterium Tritium Protons 1 1 1 Neutrons 0 1 2 Electrons 1 1 1 Atomic Mass 1 amu 2 amu 3 amu

  19. 18. For the isotope Nitrogen-15, how many subatomic particles are present?(protons, neutrons, & electrons) • Total = 21particles • Atomic # = 7 (7 p, 7e-) • Atomic mass = 14 (14-7 = 7 neutrons)

  20. 19. Potassium has an atomic number 19 and an atomic mass of 39. How many protons, neutrons and electrons does it have? • Protons = 19 • Electrons = 19 • Neutrons = 39 – 19 = 20

  21. 20. What is average atomic mass? How do you calculate it? • Weighted average of the naturally occuring isotopes of that element. To calculate 1. Convert % to decimal 2. Multiply decimal by mass of isotope 3. Add numbers to complete average

  22. 21. What is the average atomic mass of silver? .5186 x 106.9amu = 55.438 .4814 x 108.9amu = 52.424  107.9 amu Extra Practice: • http://www.algebralab.org/practice/practice.aspx?file=algebra_averageatomicmass.xml

  23. 22. Classify each of the following as an element, compound or mixture: • Sulfur - Element • Salad oil - Mixture • Newspaper - Mixture • Orange - Mixture • MgCl2 - Compound • Cardboard - Mixture • Apple juice - Mixture

  24. 23. What is density and how do you calculate it? • Density is the amount of matter in a given volume of substance. mm • D = V m = D*V V = D

  25. 24. Visit the following site:http://www.explorelearning.com/ • Type “Density” in the Search Bar. • Click on “Density Laboratory.” • Click on “Gizmo” above the picture. • Move objects onto the scale & into the cylinder & calculate the density to predict if the object will sink or float.

  26. 25. Give 4 examples and a picture of physical changes. • Cutting • Mixing • Molding • Evaporating • Distillation • Freezing • Condensing

  27. 26. Give 4 examples and a picture of chemical changes. • Burning • Exploding • Neutralizing • Corroding • Rusting

  28. Draw lines to match the following: 1. Electron a. neutral particle w/mass of 1.67 x 10-24 g 2. Proton b. – particle w/ mass of 9.11 x 10-28 g 3. Neutron c. + particle w/ mass of 1.67 x 10-24 g 4. Heterogeneous d. sample with uniform & definite composition 5. Homogeneous e. physical blend of 2 or more substances 6. Mixture f. uniform mixture 7. Element g. substance that can be chemically separated 8. Compound h. simplest form of a substance 9. Pure substance i. mixture that is not uniform throughout

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