1 / 64

Chemistry Jeopardy Review!!!

Chemistry Jeopardy Review!!!. Final Jeopardy. Introduction to Chemistry 100. Introduction to Chemistry 200. Introduction to Chemistry 300. Introduction to Chemistry 400. Introduction to Chemistry 500 True or false? Melting point is an example of chemical property.

moses
Télécharger la présentation

Chemistry Jeopardy Review!!!

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. Chemistry Jeopardy Review!!!

  2. Final Jeopardy

  3. Introduction to Chemistry 100

  4. Introduction to Chemistry 200

  5. Introduction to Chemistry 300

  6. Introduction to Chemistry 400

  7. Introduction to Chemistry 500 True or false? Melting point is an example of chemical property

  8. Introduction to Chemistry 600

  9. Introduction to Chemistry 700 If you had 350g of gold and you added 315g of gold to it, you would have this mass of gold.

  10. Introduction to Chemistry 800 When converting grams to kilograms, you need to ________ by _______.

  11. Introduction to Chemistry 900

  12. Introduction to Chemistry 1000

  13. Atoms and Elements 100 What subatomic particle is equal to the atomic number?

  14. Atoms and Elements 200 Which noble gas has the smallest atom?

  15. Atoms and Elements 300 • Atomic theory is a set of rules of elements developed by John Dalton (same guy are partial pressures) • Which of the following was not one of his postulates? • All matter is made of atoms. • Atoms of an element are identical. • Each element has the same weight. • Atoms of different elements combine in constant ratios to form compounds. • Atoms are rearranged in reactions.

  16. Atoms and Elements 400 What is the main difference between isotopes and ions from elements on the periodic table? Ions are heavier Ions are always negative particles Isotopes have more protons than electrons Isotopes have a different number of neutrons

  17. Atoms and Elements 500 . Name the atom.

  18. Atoms and Elements 600 This formula is for finding which of the following? Average percent mass of isotopes Average atomic mass of ions Average percent mass of partial Mass of only neutrons in an isotope

  19. Atoms and Elements 700 True or false An element can be separated into simpler materials

  20. Atoms and Elements 800 Which of the following is an example of two separate elements?

  21. Atoms and Elements 900 • Which of the elements below is a positive ion with a charge of one? • 1 • 2 • 3 • 4

  22. Atoms and Elements 1000 Which is the isotope? Li – 7 or Li - 6

  23. Molecules, Mixtures and Compounds 100 Kool aid and water is what type of mixture? Heterogeneous or homogeneous?

  24. Molecules, Mixtures and Compounds 200 What is an example of a physical change?

  25. Molecules, Mixtures and Compounds 300 When two or more elements or compounds are combined without reacting chemically you’ve got a _______________.

  26. Molecules, Mixtures and Compounds 400 A compound is made when two or more _________ bond together in a ____________ reaction.

  27. Which of the following does not show a chemical change? 1. 2. 3. 4. Molecules, Mixtures and Compounds 500

  28. Molecules, Mixtures and Compounds 600 True or false Compounds cannot be broken down by a chemical change

  29. Molecules, Mixtures and Compounds 700 Salt-water is a ________________ (heterogenous or homogenous) mixture.

  30. Molecules, Mixtures and Compounds 800 • Which basic lab technique involves the separation of a mixture’s components through differences in particle size? • Filtration • Extraction • Distillation • Crystallization

  31. Molecules, Mixtures and Compounds 900

  32. Molecules, Mixtures and Compounds 1000 Sodium and chlorine and both poisonous in their elemental forms. Why are they safe when in a compound? (what changed?)

  33. Periodic Table 100 Which group are the alkali metals located?

  34. Periodic Table 200 The modern periodic table is arranged in order of increasing • atomic mass • atomic number • atomic size • atomic radius

  35. Periodic Table 300 Which two elements have the most similar chemical properties? a. Be and Mg b. Cl and Ar c. Ca and Br d. Na and P

  36. Periodic Table 400 What is the name for all element in group 18?

  37. Periodic Table 500 Which choice below is not a typical characteristics of metals? • good conductor • good insulator • malleable • generally loose electrons

  38. Periodic Table 600 Which family of elements typically has the highest ionization energies?

  39. Periodic Table 700 Which of the following have the fewest number of elements in their category? Metals Nonmetals Metalloids Period 4

  40. Periodic Table 800 Why does the atomic radius increase as you move down a group

  41. Periodic Table 900 Why is K more reactive than Na?

  42. Periodic Table 1000 Definition: Ionization energy is the amount of__________ required to remove an ___________________ from a neutral atom.

  43. Kinetic Theory & Gas Laws • 100 • Gas pressure is caused by: •   gas molecules colliding with container surfaces •   barometers •   gas molecules condensing to a liquid •   gas molecules hitting other gas molecules

  44. Kinetic Theory & Gas Laws • 200 • According to Charles’ law, the volume of a fixed amount of gas is directly proportional to • isoelectric mixture • vapor concentration • barometric pressure • kelvin temperature

  45. Kinetic Theory & Gas Laws 300 Using your knowledge of KMT, explain the following: If you place an opened soda in a refrigerator, why does it stay carbonated for longer than if it were left outside? (think about gas molecules)

  46. Kinetic Theory & Gas Laws 400 • If a deep-sea diver’s tank is filled with a helium-oxygen mixture to a pressure of 170 atmospheres and the partial pressure of helium is 110 atmospheres, the partial pressure of oxygen is- • 60 atm • 110 atm • 140 atm • 280 atm

  47. Kinetic Theory & Gas Laws 500 • Name the law needed to solve and give the new volume: • An unknown gas has a volume of 1000mL at 5 atm and -14C. What is its volume at STP?

  48. Kinetic Theory & Gas Laws 600 If you brought an air-tight sealed bag of potato chips to the top of a mountain (0.5 atm), would the bag be bigger or smaller then from sea level (1 atm)?

  49. Kinetic Theory & Gas Laws 700 According to Graham’s Law, if we spray 2 moles of Hydrogen gas (H2) and 2 moles of carbon dioxide (CO2), which would diffuse faster and why?

  50. Kinetic Theory & Gas Laws • 800 • If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 ml, and a temperature of 87 0C, how many moles of gas do I have? • In the problem above name the law you would use to solve and what would have to be converted before solving

More Related