MRS. TAYSI

1
MRS. TAYSIS CHEMISTRY FINAL REVIEW

• REVIEW TO SUCCEED! STUDY, STUDY, STUDY.
• These are meant to help you studyexamples are
  given, but not necessarily all the answers!

2
1. What is chemistry?

• Two things
• Study of matter
• How matter changes

3
2. What is science?

• Is it
• Predictive?
• YES
• Reproducible?
• YES
• Definitive?
• NO
• Testable?
• YES
• Tentative?
• YES

4
3. Lab safety rules.

• What should you do if you spill a base or an acid
  on the lab bench? Your skin?
• How should you heat a test tube?
• How should you dispose of broken glass?
• How do you use a fire extinguisher?

5
4. Lab equipment

• Be familiar with the following pieces of
  equipment
• Beaker
• Graduated cylinder
• Test tube
• Eye dropper
• Erlenmeyer flask
• Which of the above is most precise in measuring
  liquid volume?

6
5. Chemical Equations

• BaCO3(s) 2HCl(aq) ? H2O(l) CO2(g) BaCl2(aq)
• Which represents/means 
• Solid, liquid, gas, dissolved in water
• Yields or produces
• Formula
• Coefficient, subscript
• Reactants
• Products

7
6. Experimental vocabulary

• Be able to identify the following for an
  experimental situation
• Independent variablewhat you are testing or
  experimenting with what YOU change
• Dependent variablewhat you are measuring about
  the IV what you expect to change
• Controlled variableswhat you keep the same
  between both the experimental and control groups

8
6. Experimental vocabulary

• Experimentationobserve, hypothesize, collect,
  analyze report data (the whole thing)
• Hypothesiseducated guess what you think will
  happen why (If...then)
• Interpretationan explanation of an observation
  (It turned blue because)
• Quantitative datanumbers (15 sec, 25 mL)
• Qualitative dataword descriptions (blue, red)

9
6. Experimental vocabulary

• Trialsrepetitions of the experiment to be sure
  of results
• Experimental groupgroup that has the
  experimental variable applied to it
• Control groupgroup that is left alone the
  normal situation done for comparison and not
  always possible to do for all experiments

10
6. Experimental vocabulary

• Take the hamburger lab and try to identify the
  different parts of the experiment.

11
7. Potential energy diagrams
12
8. Identify as elements, compounds or mixtures

• O2
• H2O
• air
• water
• sodium iodide
• tellurium

13
9. Element formulas

• BrINClHOFall are diatomic
• P4
• S8
• All the rest are monoatomic

14
10. Atom or molecule? Element or compound?

• Xe
• SF6
• PCl3
• Mn

15
11. Identify as physical or chemical changes
16
12. AIR?

• What is in air?
• Is it an element, compound or mixture?

17
13. Combustion

• Combustionburning of a hydrocarbon compound in
  the presence of oxygen.
• Complete combustionplenty of oxygen present, so
  CO2 and H2O are formed.
• Incomplete combustionnot enough oxygen is
  present, so CO instead of CO2 is produced, along
  with water.

18
14. Burner flamewheres the hottest part, and
how did we figure it out?
19
15. Alloys

• Alloy
• mixture of 2 or more metals
• Brass?
• zinc copper
• Steel?
• iron carbon(exceptionnonmetal!)

20
16. Types of steel crystal size

• Annealed
• heated and then slowly cooled
• Hardened
• heated and then quickly cooled
• Tempered
• heated and cooled slowly several times
• What happens to crystal size when cooled quickly?
  Slowly?

21
17. Separation techniques

• Electrolysis
• water was separated into its elements using
  electricity
• Chromatography
• a pen ink mixture was separated into its
  component pigments using water

22
18. Balancing equations

• Practice makes perfect!
• ___ H2 ___ O2 ? ___ H2O
• ___ S8 ___ O2 ? ___ SO2
• ___ NaCl ___ Fe(OH)3 ? ___ NaOH
• ___ FeCl3

23
19. Mass ?? mole conversions

• Remember to use the periodic table
• How many moles is 24.0 g of iron?
• How many grams is 2.25 moles of nitrogen gas?

24.0g Fe x 1 mole Fe 1 55.8g Fe
2.25 mol N2 x 28.0 g N2 1 1
mol N2
24
20. Stoichiometrymass to mass

• Balance this equation
• ___ H2 ___ O2 ? ___ H2O
• How many grams of water will be produced from
  reacting 32.0 g of oxygen gas with excess
  hydrogen?

25
21. Stoichiometrymole to mole

• Balance this equation
• ___ H2 ___ O2 ? ___ H2O
• How many mol of hydrogen gas is needed to react
  with 4.00 mol of oxygen gas?

26
22. Mass to particles

• 56.0 g nitrogen gas has how many particles?

27
23. Particles to mass

• 1.5 x 1024 particles of hydrogen gas equals how
  many grams of hydrogen gas?

28
24. Reaction typesname these

• 6. A BC ? AC B ________________
• 7. CH4 O2 ? CO2 H2O _______________
• 8. AB CD ? AD CB _______________
• 9. A B ? AB ________________
• 10. AB ? A B _________________
• 11. Na Cl2 ? NaCl _________________
• 12. C2H6 O2 ? CO2 H2O _____________
• 13. CaF2 Na3PO4 ? Ca3(PO4)2 NaF _____
• 14. CaCO3 ? Ca CO2 ______________
• 15. Al CuSO4 ? Al2(SO4)3 Cu
  __________

29
25. Identify the metric unit for each

• Temperature
• Volume
• Distance
• Mass
• Density

30
26. Density calculation

• A graduated cylinder with water in it has a
  volume of 24.5 mL. When a rock with a mass of
  25.0g is placed in the cylinder, the water volume
  increases to 28.3 mL. What is the density of the
  rock?

31
27. Mass calculation given density

• A block with dimensions of 1.0cm by 2.5cm by
  4.2cm. If the density of the block is 0.57
  g/cm3, what is the mass of the block?

32
28. Light phenomena

• What type of light phenomena is each
  example/description?
• Glow in the dark silly putty
• Fireworks
• Brightly colored packaging
• Light energy is absorbed and then is given off
  gradually over time
• Electrical or heat energy is taken in by
  electrons and light energy is given off

33
29. EM spectrum

• Which is higher in energy?
• gamma rays or UV
• radio waves or green light
• Which is lower in energy?
• microwaves or radiowaves
• infrared light or yellow light

34
30. Protons, electrons, neutrons isotopes

• What particle determines the isotope of an
  element?
• What particle determines the charge of an ion?
• What particle determines the identity of an
  element?
• How is lithium-6 different from lithium-7?

35
31. PEN, etc

• What type of atom has 5 protons in its atom?
• What is the atomic number of tungsten?
• Oxygen-18 has how many neutrons?
• A fluoride-19 ion (F-) has how many
• protons? neutrons? electrons?
• What is the charge on a sulfur atom that has 18
  electrons?

36
32. Alpha, beta gamma radiation

• Rank alpha, beta gamma in order of ability to
  penetrate substances, lowest to highest.
• Rank alpha, beta gamma in order of size,
  smallest to largest.

37
33. Groupings on the periodic table

• Make sure you have all 15 groups labeled
  correctly on your periodic table
• Metals, nonmetals metalloids
• Alkali metals, alkaline earth metals, transition
  metals, inner transition metals, lanthanides,
  actinides, B, C, N O groups, halogens and noble
  gases

38
34. Ion formation using octet rule

• What type of ion would sulfur form?
• What type of ion would sodium form?
• What type of ion would magnesium form?
• What type of ion would chlorine form?

39
35. The duet rule

• Which two elements obey the duet rule and why?

40
36. Electron configurations

• Be sure to bring your orbital diagram worksheets
  to the test!! Know how to use them!
• What is the full electron configuration for
  copper?
• Shorthand for copper?
• What is the full electron configuration for
  strontium?
• Shorthand for strontium?

41
37. Chemical Families

• Why do chemical families on the periodic table
  exhibit similar properties?

42
38. Lewis/Electron dot structures

• What is the electron dot structure for each of
  the following elements? (remember the general
  ruledoesnt work for transition elements)
• lithium
• antimony
• xenon
• zirconium

43
39. Bond types (metals or nonmetals?)

• Covalent bonds involve what types of elements?
• Ionic bonds involve what types of elements?

44
40. Bonding electronegativities

• Using the electronegativities chart determine the
  type of bonding for the following formulas
• MgS
• N2
• SiO2
• NO2

45
41. Bond type using metal/nonmetal rules

• Using the metal/nonmetal rules determine the type
  of bonding for the following formulas
• MgS
• N2
• SiO2
• NO2

46
42. Molecular Shapes

• For each formula, determine the shape of the
  molecule produced
• SiH4
• H2S
• BeCl2
• BF3
• NCl3

47
43. Solubility and polarity

• Determine whether or not the following pairs are
  soluble or insoluble
• H2O and NaI
• H2O and CF4
• SiH4 and NCl3

48
44. Determining partial charges

• Draw the bar diagram and label each formula with
  the proper d and d- charges.
• CH2F2
• CH4
• H2S

49
45. Polarity and chromatography

• Why did the Sharpie pen move in ethanol and
  acetone, but not water?
• Be able to use lab results to tell whether an ink
  is polar or not.

50
46. Water and Mickey Mouse

• If water is Mickey Mouse, what element represents
  the face and what represents the ears?

51
47. Covalent naming and formulas

• What is the name for each of the following
• NCl3
• SiO2
• What are the correct formulas for each of these
• sulfur dioxide
• carbon tetrachloride

52
48. Tie Dye

• What does the sodium carbonate solution do to the
  shirts?

53
49. Hamburger analysis lab

• Why is hexane used to extract fat instead of
  water?

54
50. Sand Lab

• A sand sample contains the following with the
  coded abundance from the lab
• Granite(1), quartz(1), coral(3), shells(2), sea
  urchin spines(2)
• What type of climate water is this from?

55
Balloons!

• Place the following balloons in order of their
  explosiveness(least to most)
• hydrogen, oxygen and hydrogen/oxygen mixed