Science Lab Safety Rules - Georgetown High School



PAP Chemistry Fall Semester Final Exam Review

The final exam will be 50-80 multiple choice questions. Study your tests and foldables over each of the following units as well as answering the questions below.

Safety and Equipment Unit

Review safety rules and look over Safety and Equipment Test.

Measurements and Calculations Unit

1. How many significant figures are in each of the following? a. 1.03338000 b. 0.000033 X 108 c. 133,555,800

2. The density of an object is 2.88 g/cm3 with a volume of 4.55cm3. What is the mass of the object?

3. An irregularly-shaped solid is placed into a graduated cylinder filled with 25.8 mL of water and the level of the water rises to 33.9 mL. The mass is 5.9 g. What is the density of this solid?

4. Convert 35 in/sec to meters/day

5. Convert 4.9 x 106 μg to mg

6. Convert 1000 pL to cm3 (Don’t forget 1cm3 = 1mL)

The Atom Unit

7. Calculate the number of neutrons in an atom if the atomic number=42 and mass number=96.

8. How many electrons are present in an atom of mercury-201?

9. Calculate the number of protons in an atom if the mass number=19 and #neutrons=10.

10. Explain why atoms are neutral.

11. Which has less mass: an electron or a proton?

12. Write the nuclear symbol for an isotope of uranium with 142 neutrons.

13. Write using hyphen notation an isotope of carbon with 7 neutrons.

14. What is an ion?

15. Understand the law of conservation of mass.

16. How many moles are present in a 57.6g sample of magnesium chloride?

17. How many atoms are in a 76.9g sample of silver?

18. What is the mass (in grams) of 89.4 moles of potassium sulfide?

Electrons Unit

E=h ν h = Planck’s constant 6.63X10-34 J · s c= ν λ c= speed of light 3.00X108 m/s

19. If a wave has a frequency of 3.44X1014 Hz What is the wavelength?

20. What is the energy of one photon of light with a frequency of 5.50X1014 Hz?

21. Write the electron configuration for selenium.

22. Write the noble gas (or abbreviated electron configuration) for nickel.

23. Give the four q. n. that describes the location of the last electron for magnesium.

24. Give the four q. n. that describes the location of the last electron for arsenic.

25. Identify the element if the last electron has the following four q. n. 3, 2, -1, -1/2.

26. Identify the element if the last electron has the following four q. n. 2, 1, +1, +1/2.

Periodic Table Unit

27. As you move across the periodic table, from left to right, do the atoms get smaller or larger? Are the ionization energies increasing or decreasing? Are the metals becoming more or less reactive? Are the metals getting harder or softer?

28. Which main group elements have 1 valence electron?

29. Arrange the following elements based on their size (atomic radii) from largest to smallest Ca, Ge, Br, K, Kr.

30. Arrange the following elements from highest to lowest ionization energy Sr, Mg, Be, Ba, Ra.

31. Which of the following has a higher electron affinity Fe or K?

32. Which of the following has a lower electronegativity Fe or K?

33. When strontium becomes an ion are electrons lost or gained? How many? What will the charge of the ion be?

Chemical Bonding Unit

34. Explain the following terms: valence electrons and the Octet Rule

35. Draw electron dot structures for the following atoms or ions Rb atom, Rb ion, Se atom, Se ion.

36. Do ionic bonds form with electrons are shared or transferred?

37. Draw electron dot structures showing the formation of the following ionic compound: calcium phosphide

38. Draw electron dot structures for the following covalent compounds and determine the shape, bond angle, and molecular polarity for each: CO2, NH3, H2O, CH2Cl2, COCl2

Nomenclature Unit

39. Name or write the formula for the following ionic compounds or acids: CuBr2, SrO, HClO4, KNO2, Na2CO3, HF, PbSO4, copper (II) permanganate, nitric acid, iron (III) oxalate, strontium phosphide, calcium bromide, barium chlorite, hydrobromic acid

40. Name or write the formula for the following covalent or molecular binary compounds: CCl4, NH3, SF2, C2H2, sulfur hexafluoride, dinitrogen trifluoride, dihydrogen monoxide, carbon monoxide

PAP Chemistry Fall Semester Final Exam Review Answer Key

1a. 9 1b. 2 1c. 7 2. 13.1g 3. 0.73g/mL 4. 77000m/day 5. 4900mg 6. 1X10-6cm3 7. 54 8. 80

9. 9 10. In an atom the #protons = #electrons. 11. electron 12. 23492U 13. C-13

14. When an atom loses or gains electrons it becomes an ion. 15. In a chemical reaction the mass of the reactants will be the same as the mass of the products. Matter is not created or destroyed. 16. 0.605mol MgCl2

17. 4.29X1023atoms 18. 9860g K2S 19. 8.72X10-7m 20. 3.65X10-19J

21. 1s22s22p63s23p64s23d104p4 22. [Ar]4s23d8 23. 3 0 0 -1/2 24. 4 1 1 +1/2 25. Co

26. N 27. smaller, increasing, less reactive metals, harder metals 28. alkali metals

29. K, Ca, Ge, Br, Kr 30. Be, Mg, Sr, Ba, Ra 31. Fe 32. K 33. lost, 2, +2

34. valence electrons - electrons that are lost, gained, or shared during bonding. Octet rule – atoms will lose, gain, share electrons in order to obtain 0 or 8 valence electrons.

35. Rb atom 1 electron, Rb ion 0 electrons with a +1 charge, Se atom 6 electrons, Se ion 8 electrons with a -2 charge

36. transfer of electrons 37. Ca3P2 each Ca will have a +2 charge and each P will have a -3 charge

38. linear, 180º, nonpolar molecule trigonal pyramidal, ................
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