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Actual For Reals Honors Chemistry Fall Final Review Guide 2019

Name _____________________________________________________ Date ___________________

Unit 1: Numbers and MatterTerms to Know:• Metric conversions• Matter• Law of Conservation of Matter/Mass• Physical and chemical change• Physical and chemical property

• Intensive vs. extensive

Practice Problems:1. Convert the following to meters. Write your answer in scientific notation.

a. 0.035 mm = ____________________________

b. 120 km = ____________________________

c. 53000 dm = ____________________________

2. Which of the following indicate a chemical change: CIRCLE ALL THAT APPLY(a) fizzing (c) color change(b) burning (d) precipitate formation

3. Which of the following are physical changes: CIRCLE ALL THAT APPLY(a) state of changes (c) cracking open an egg(b) salt dissolving in water (d) boiling water

4. Answer the following calculations to the correct number of significant figures:

a. 3.0 m x 2.30 m = ____________________________

b. 2.3 cm + 3.44 cm = ____________________________

c. 3.44m x 2.0 m / 3.9 s = ____________________________

5. How many significant figures do the following numbers have?

a. 0.00321 ____________________________

b. 320001 ____________________________

c. 1.0000 ____________________________

d. 0.00210 ____________________________

6. A bottle contains 4.200 mL of a liquid. The total mass of the bottle and the liquid together is 6.635 g. The mass of the empty bottle is 3.450 g. What is the density of the liquid?

• Accuracy vs. Precision• Rules for sig fig counting and math manipulation• Scientific notation• Metal vs. nonmetal vs. metalloid• Density calculations

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7. An object has a density of 0.62 g/ml and a mass of 4.0 g what is its volume?

8. An object has a density of 1.2g/ml and a volume of 8.2 ml what is its mass?

9. There are 60 seconds per minute, 60 minutes per hour, 24 hours per day and 365 days per year. How many seconds are in a 3 years?

10. If 3.784 liters = 1 gallon, how many liters are in 4 gallons?

11. Convert 103.50 cm3 of Aluminum into grams of Aluminum (Density of Aluminum = 2.699g/cm3)

12. A field goal kicker who makes 20/21 field goals through the center of the uprights has:(a) poor accuracy but good precision (c) poor accuracy and poor precision(b) good accuracy and good precision (d) good accuracy and poor precision

Unit 2: ThermochemistryTerms to Know:• Temperature• Heat• Specific Heat• Calorimetry• Heat transfer flow• Heating curve of a substance

13. Using the graph above, what temperature does the substance melt? Evaporate?

14. What phase of matter is the substance at during point A → B? C →D?

15. Where is kinetic energy changing on the graph?

16. Where is the potential energy changing on the graph?

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17. What would happen to this substance after point D?

18. How much energy in J must be absorbed by 20.0 g of water to increase its temperature from 83°C to 96.0 °C?

19. What is the specific heat of a substance that absorbs 2.5 x 103 joules of heat when a sample of 1.0 x 104 g of the substance increases in temperature from 10.0oC to 70.0oC?

20. What is the final temperature of a 75.0 g sample of water that is cooled from 98.0oC and releases 950.0 J of heat?

21. Calculate the final temperature of the metal and water, based on the information below. Specific heat of metal is 0.75 J/goC

Mass of metal: 30g Temperature of water before: 27.0 ˚CMass of H2O: 46g Temperature of metal before: 365.0 ˚C

22. Calculate the specific heat of the unknown metal.Mass of metal: 30.0g Temperature of water before: 27.0 ˚CMass of H2O: 100.0g Temperature of metal before: 365.0 ˚C

Temperature of metal and water mixed 57.0 ˚C

Unit 3: Nuclear Chemistry & Atomic Structure

• Electron configuration• Periodic trends

• Ionization energy• Electronegativity

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Terms to Know:• Protons, Neutrons, and Electrons and how to determine• Ion• Isotope• Average atomic mass/percent abundance• Alpha, beta and gamma radiation• Half life• Fission/fusion• Element family/group names• Wavelength• Principle quantum number• Orbital notation

Practice Problems23. An atomic number is the same as the number of:

(a) Neutrons (c) Alpha particles(b) Electrons (d) Protons

24. An atom is defined as the smallest part of an element that:(a) Has protons, neutrons, and electrons (c) Can form an ion(b) Retains the chemical identity of that element (d) Has protons and neutrons

25. The atomic number (# of protons) and mass of chlorine are?(a) 17, 35 (c) 16, 32(b) 33, 75 (d) 29, 64

26. The neutrons of an atom are found:(a) In the nucleus (c) In the s block(b) Orbiting the nucleus (d) In the orbitals

27. Which subatomic particle has the smallest mass?(a) Protons (c) Electrons(b) Neutrons (d) Ions

28. What is the average atomic mass of an element that has the following 3 isotopes?65% 45.0 g 32% 49.5 g 3% 63.0 g

29. How do you write an isotopic chemical symbol for an atom? DRAW A DIAGRAM.

30. If an atom has 14 protons, 15 neutrons and, 14 electrons; its complete chemical symbol would be:

31. If an atom has 8 protons, 8 neutrons, and 10 electrons, its complete chemical symbol would be:

• Electron configuration• Periodic trends

• Ionization energy• Electronegativity

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32. If an atom has 13 protons, 14 neutrons, and 10 electrons, its complete chemical symbol would be:

33. If an atom has 11 protons, 12 neutrons, and 10 electrons, its complete chemical symbol would be:

34. After 3 half-lives, how much of a 400 gram sample of radioactive uranium remains?

35. 25% of a sample of carbon-14 remains, how old is the material containing the carbon-14? Carbon-14 half-life is 5 730 years.

36. Show the alpha decay of an atom of .

37. Show the beta decay of an atom of .

38. What is the electron configuration (1s22s2, etc.) for the following atoms:

Long Hand Noble Gas Conf.

a. Co ____________________________________ _______________________

b. N ____________________________________ _______________________

c. Al ____________________________________ _______________________

d. Ca ____________________________________ _______________________

e. S ____________________________________ _______________________

f. Ar ____________________________________ _______________________

39. What is the orbital diagram (↑↓) for the following atoms:

a. Co ________________________________________________________________

b. N ________________________________________________________________

c. Al ________________________________________________________________

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d. Ca ________________________________________________________________

e. S ________________________________________________________________

f. Ar ________________________________________________________________

40. The number of protons always equals the number of __________ in a neutral atom.

41. The mass number of an element tells the # of __________ and __________

42. Isotopes have the same number of __________ but different numbers of __________ and different atomic __________.

43. Who is credited with the development of the first periodic table? ____________________

44. How did Mosely’s periodic table differ from Mendeleev?

45. What does Hund’s rule state?

46. What does the Aufbau principle state?

47. What does the Pauli Exclusion principle state?

48. Define these terms AND draw arrows to represent how these trends increase across the period and within each group:

a. Atomic Radius:

b. Ionization Energy:

c. Electronegativity:

Unit 4: Nomenclature and Structures of BondsTerms to Know:• Naming domain rules (ionic, covalent, acid, hydrocarbon)• Intermolecular forces

• London dispersion forces• Dipole-dipole forces• Hydrogen bonding

Practice Problems

• Bond polarity• Molecular polarity• Polar vs. nonpolar molecules• VSEPR theory

• Shapes• Bond angles

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49. Naming Ionic Compounds a. NH4Cl __________________________________________________

b. Fe(NO3)3 __________________________________________________

c. Cu3P __________________________________________________

d. Al(CN)3 __________________________________________________

e. Pb(SO4)2 __________________________________________________

50. Formula of Ionic Compounds a. lead (II) nitride __________________________________________________

b. silver bromide __________________________________________________

c. chromium (VI) phosphate __________________________________________________

d. vanadium (V) sulfide __________________________________________________

e. potassium bicarbonate __________________________________________________

51. Naming Covalent Compounds a. IO2 __________________________________________________

b. C2Br6 __________________________________________________

c. BBr3 __________________________________________________

d. N2O3 __________________________________________________

52. Naming and Formulas of Acidic Compounds a. HCl __________________________________________________

b. H2SO4 __________________________________________________

c. Hydronitric acid __________________________________________________

d. Phosphoric acid __________________________________________________

53. Formula of Covalent Compounds a. tetraphosphorus triselenide __________________________________________________

b. disilicon hexabromide __________________________________________________

c. diselenium diiodide __________________________________________________

d. tetrasulfur dinitride __________________________________________________

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54. Diatomic molecules : What are the seven diatomic molecules (names and formulas)? Draw their Lewis Structures.

55. VSEPR Theory : (a) draw the following molecules in their correct VSEPR shape and label bond angle. (b) determine if the molecule is polar or non polar. (c) determine the IMF between multiples of the molecules.

a. H2O

b. CClF3

c. NCl3

d. HCN

Unit 5: Chemical ReactionsTerms to Know:• Balancing chemical equations• Word equations from a balanced chemical equation• 5 types of reactions• Predicting reactions

Practice Problems1. Balance, and write a word equation: __AlBr3(aq) + __CaSO4(s) → __Al2(SO4)3(s) + __CaBr2(aq)

2. Write a chemical equation for the reaction: aqueous sodium phosphate reacts with lithium metal to form aqueous lithium phosphate and sodium metal.

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3. Provide a description and pattern (i.e. A +B → AB) for each type of chemical reaction.

a. Combustion Reaction

b. Synthesis Reaction

c. Decomposition Reaction

d. Single Replacement Reaction

e. Double Replacement Reaction

4. Identify the type of chemical reaction. BALANCE.

a. ____ Mg + ____ Fe2O3 → ____ Fe + ____ MgO Type of Reaction: ________________

b. ____ C2H4 + ____ O2 → ____ CO2 + ____ H2O Type of Reaction: ________________

c. ____ PbSO4 → ____ PbSO3 + ____ O2 Type of Reaction: ________________

d. ____ H2O + ____ SO3 → ____ H2SO4 Type of Reaction: ________________

e. ____ H2SO4 + ____ NH4OH → ____ H2O + ____ (NH4)2SO4 Type of Reaction: ________________

Identify the type of reaction, predict the products and write a balanced chemical equation. a. _____NaOH(aq) + _____ MgCl2(aq) →

b. Iron (IIII) phosphate + sodium carbonate →

c. _____ CaBr2(aq) + _____ (NH4)2CO3(aq) →

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d. _____ Zn(s) + _____FeCl3(aq) →

e. _____Na(s) + _____Br2(g) →

f. _____H2O(l) →

g. _____ C9H15O (s) +_____O2(g) →

h. Zinc nitrate + potassium phosphate →