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You Are In The HOT SEAT!

You Are In The HOT SEAT!. Bonus Round. Name the following compounds: a.) NaBr b.) Ca (OH) 2 c.) SF 6. What is the percent composition of the elements in C 2 H 5 Cl?. Write the formula equation for the following: Tin(IV) oxide and hydrogen gas produce tin and water.

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You Are In The HOT SEAT!

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  1. You Are In The HOT SEAT! Bonus Round

  2. Name the following compounds: a.) NaBr b.) Ca(OH)2 c.) SF6

  3. What is the percent composition of the elements in C2H5Cl?

  4. Write the formula equation for the following: Tin(IV) oxide and hydrogen gas produce tin and water

  5. 2H2 + O2 2H2O If 5.3 moles of oxygen are used up, how many grams of H2O is made?

  6. Draw the Lewis structures for the following: a.) C2H5Br b.) H2O c.) CO2

  7. Determine the chemical formulas for the following: a.) phosphoric acid b.) Iron(III) sulfate c.) magnesium nitrite

  8. Which are more electronegative? a.) silicon or chlorine b.) magnesium or calcium c.) fluorine or neon

  9. Write the electron configuration for scandium and give its electron (Lewis) dot notation

  10. 2C8H18 + 25O2--> 16CO2 + 18 H2O If 27.3g of C8H18are used, what mass of water will be produced?

  11. True or False a.) Most solid solutes increase in solubility in water with an increase in temperature. b.) Most gaseous solutes increase in solubility in water with an increase in temperature.

  12. What is the value of “n” for an electron in an s-orbital in the fourth energy level.

  13. Which will be come bigger than its atom when it becomes an ion? calcium or chlorine

  14. This states that no two electrons in the same atom can have the same four quantum numbers.

  15. What element is in group 14 and period 4?

  16. Which has a larger atomic radius? a.) potassium or rubidium b.) aluminum or silicon

  17. Consider the following: 1s2 2s2 2p6 3s2 3p6 4s2 3d5 a.) How many electrons are in the third principle energy level? b.) How many electrons are in the second principle energy levels p-sublevel? c.) How many electrons are in a 2p orbital?

  18. What two people both produced similar periodic tables at the same time that are considered the first modern periodic tables?

  19. Identify the Type of Reaction a.) 2HgO 2Hg + O2 b.) AgNO3 + NaCl → AgCl + NaNO3

  20. What type of bonding is expected between hydrogen and fluorine – non-polar covalent, polar covalent or ionic?

  21. What is the molecular shape of NH3?

  22. a.) Which is/are an alkali metal? P, Ge, Fe, Li, Ra, Ar b.) Which is/are a transitional metal? Mn, F, K, Ca, Au c.) Which is/are a lanthanide element? Rn,Pr, Pa, Bi, Cr

  23. Draw the orbital diagram for phosphorous

  24. Which of the following are not soluble in water? a.) BaSO4 b.) KOH c.) NaOH d.)silver chloride e.) potassium sulfate

  25. 100 grams of water are saturated with potassium nitrate at 70 ˚C. If the solution is cooled to 40˚C, how much potassium nitrate will precipitate out of solution?

  26. Bonus Round200 points to the first group with the correct answer; 100 points to the second group, 50 points to the third, 40 points to the fourth, 30 points to the fifth and 20 points to the sixth. The reaction between silver nitrate and sodium bromide produces silver bromide and sodium nitrate. 1.) Write the balanced chemical equation for this reaction 2.) Determine the type of reaction this is. 3.) If 5.3 grams of silver nitrate are used, how many grams of sodium nitrate are made?

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