Mr. Grosser's Science Resources



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Study Guide for Chemistry I Semester One Final Exam

|Chapt. |Topics |Book Examples |

|1 |Book Objectives: | |

| |What is chemistry | |

| |Know the steps in the scientific method | |

|2 |Book Objectives: |Pg.51 (18-19) |

| |Know the differences between solids, liquids and gases | |

| |Know the differences between elements, compounds and mixtures | |

| |Be able to tell the difference between chemical and physical changes (definition, examples) |Pg. 58 (45, 47, 49, |

| |Know what different separation techniques can separate (elements/compound/mix) |69) |

| |Know the law of conservation of matter | |

| | | |

| |EOC Targets: | |

| |C-Matter-101. I can define what matter is. | |

| |C-Matter-102. I can differentiate between a solid, liquid, and gas. | |

| |C-Matter-103. I can explain that matter cannot be created or destroyed in a chemical reaction or physical change. | |

| |C-Matter-104 I can classify matter as an element, compound, or mixture. | |

| |C-Matter-201. I can explain what physical and chemical properties are, and list examples. | |

| |C-Matter-202. I can describe how density relates to mass and volume for matter. | |

| |C-Matter-203. I can calculate density given the mass and volume, or calculate relationships between density, mass and volume | |

| |C-Matter-204. I can differentiate between mass and density. | |

| |C-Matter-301. I can explain what happens to matter during a physical or chemical change. | |

|3 |Book Objectives: |Pg. 70 (5, 6, 7, 8) |

| |Be able to determine the correct sigs figs / calculations (+-x÷) | |

| |Know the metric prefixes – sizes |Pg. 78 (16, 17) |

| |Be able to convert between °C and K | |

| |Be able to calculate density |Pg. 84 (33, 34) |

| |Be able to convert metric units | |

| |Be able to set up factor label problems |Pg. 91 (46, 47) |

| |Be able to convert between scientific notation and decimal notation | |

| |Know what different units measure | |

| |Know the difference between accuracy and precision | |

| |Know the difference between quality and quantity | |

| | | |

| |EOC Targets: | |

| |C-Measurement-1501. I can recognize the uncertainty of measurements. | |

| |C-Measurement-1502. I can choose and use appropriate lab equipment to measure properly. | |

| |C-Measurement-1503. I can choose appropriate SI units and convert between them. | |

| |C-Measurement-1504. I can use scientific notation and interpret the meaning of the power of ten. (For example, knowing that | |

| |10-6 is smaller than 10-2) | |

|4 |Book Objectives: |Pg. 112 (17-18) |

| |Know the subatomic particles (relative sizes and charges, location) | |

| |Be able to calculate the average atomic mass from isotope masses |Pg. 115 (23-24) |

| |Be able to write atomic symbols and determine number of p, n, e, mass number, or atomic number | |

| |Know the major scientists, their experiments and discoveries |Pg. 122 (43) |

| |Know early models of the atom | |

| |Know what isotopes are and how they are different | |

| |Know periods and families | |

| | | |

| |EOC Targets: | |

| |C-Atomic Structure -1801. I can identify the location, charge, and relative mass of each subatomic particle: (electron, | |

| |neutron, and proton). | |

| |C-Atomic Structure -1802. I can recognize that electrons exist in energy levels outside the nucleus. | |

| |C-Atomic Structure -1803. I can identify the element based on the number of protons. | |

| |C-Atomic Structure -1902. I can explain how the number of protons and electrons relates to the charge of the atom or ion. | |

| |C-Atomic Structure -2001. I can explain how the number of protons and neutrons relates to the mass number. | |

| |C-Atomic Structure -2002. I can define isotope by explaining that atoms of an element can contain different numbers of | |

| |neutrons. | |

|5 |Book Objectives: |Pg. 135 (8) |

| |Know Bohr’s model and how electrons behave, excite/ground state, atomic spectra | |

| |Know quantum model: orbitals, sublevels, energy levels, # electrons |Pg. 167 (8-9) |

| |Know the EMR spectrum, relative energy, wavelength and frequency | |

| |Know relationship between energy, wavelength and frequency | |

| |Be able to write electron configurations (ions and neutral atoms) | |

| |Know rules for writing orbital diagrams (AUFBAU, Hund, Pauli) | |

| |Be able to identify excited electron configurations/orbital diagrams | |

| |Know parts of a wave: amplitude, wavelength and frequency | |

|6 |Book Objectives: |Pg. 181 (39, 43) |

| |Know the trends on the periodic table (type ion, ion size, electronegativity, metal/NM( (highest vs lowest) | |

| |Know s, p, d, f blocks | |

| |Kow ion radius changes | |

| |Know family names and locations on Periodic Table | |

| |Know how Medeleev organized the periodic table and the periodic law | |

| |Know location of metals, nonmetals and metalloids | |

| | | |

| |EOC Target: | |

| |C- Periodic Table-2301. I can differentiate between groups and periods on the periodic table and what is common about elements| |

| |within a group. | |

| |C- Periodic Table-2302. I can locate metals, non-metals and metalloids on the periodic table. | |

| |C- Periodic Table-2303. I can list properties of metals, non metals and metalloids. | |

| |C- Periodic Table-2305. I can determine the charge of a main block (representative) ion. | |

| |C- Periodic Table-2306. I can determine the number of valence electrons for a main block (representative) element. | |

| |Book Objectives: |Pg. 207 (41, 63, 67, |

|7 |Be able to write electron configurations of ions |79) |

| |Be able to identify formulas as ionic or metallic | |

| |Be able to draw electron dot diagrams of ions | |

| |know what valence electrons are and how many an atom has | |

| |Know how ions form and why | |

| |Know structure and behavior of ionic and metallic bonds | |

| | | |

| |EOC Targets: | |

| |C-Atomic Structure -1901. I can explain how ions are formed and predict their charge. | |

| |C-Bonding- 2101. I can identify a compound as ionic from the types of elements in the compound. | |

| |C-Bonding- 2102. I can explain an ionic bond using electrostatic attraction. | |

| |C-Bonding- 2103. I can describe the general characteristics of an ionic compound (solubility, melting point, alternating ions | |

| |create a simple crystalline structure, electrical conductivity). | |

|9 | Book Objectives: |Pg. 264 (13) |

| |Be able to determine if elements will form ionic compounds | |

| |Be able to write names/formulas of ionic compounds (transition metal,8 polyatomic ions) |Pg. 281 (43, 57, 61, |

| |Know charges of ions by family location |65, 67, 69) |

| | | |

| | | |

| |EOC Targets: | |

| |C-Nomenclatrue-401. I can use naming rules to name or write the formula for ionic compounds. | |

|25 |Book Objectives: |Page 800 |

| |Recognize that an unstable nucleus loses energy by emitting radiation during the decay process. |Read table 25.1 |

| |Know how to write the symbols for an alpha particle, a beta particle, and a gamma ray. |Section review 25.2. |

| |Know the relative penetration ability of each form of radiation listed above. |Section review |

| |Know what can be used to shield yourself from each form of radiation. |25.3 |

| |Be able to identify the missing particle in a transmutation equation. | |

| |Know the difference between fission and fusion. | |

| |Know the nuclear process that fuels our sun. | |

| | | |

|Misc |Know lab safety rules and | |

| |Know lab equipment and how to read them | |

| |Be able to interpret graphs | |

Name _______ANSWER KEY_________________ Period _______________ Date__________________

1. Which of the following is/are qualitative observation(s)?

The metal is shiny. The Al has a mass of 7.0g. The density of Al is 2.70g/cm3. The metal is ductile.

Which of the following is/are quantitative observation(s)?

The metal is shiny. The Al has a mass of 7.0g. The density of Al is 2.70g/cm3. The metal is ductile.

2. Read the graduated cylinder below: 6.60 mL

[pic]

3. If a graduated cylinder has markings for the 10’s, and 1’s, how many decimal places will be in your measurement?

10’s – measure to the ones place.

1’s – measure to the tenths place

4. What pieces of laboratory equipment can be used to accurately measure the volume of a liquid?

Graduated cylinder

5. Which of the following are units for volume? mm, mL, m, cm, cm3, g/cm3, g, kg, L

6. Which of the following are units for mass? mm, mL, m, cm, cm3, g/cm3, g, kg, L

7. What is the relationship between 1mL and 1cm3? 1mL = 1cm3

8. What is the difference between precision and accuracy?

Accuracy – how close a measurement is to the true value

Precision – how consistent a set of measurements are

9. Which set of data points show the greatest precision? Each student massed an object three times.

Student one: 2.1 g 2.2 g 1.9g – Most precise because the measurements are in a very narrow range. In other words, they are consistent.

Student two: 1.6 g 2.9 g 2.0g

Student three: 2.5g 3.0g 3.1g

10. Define matter.

Matter is anything that has mass and takes up space.

11. A student calculates the density of an object to be 3.00g/cm3. The true value is 2.50g/cm3. Calculate this student’s percent error.

|2.50 – 3.00|/2.50 x 100% = 20%

12. The density of pure water is 1g/cm3. Which of the following items will float in water? A cork with a density of 0.87g/cm3, a rock with a density of 8.9g/cm3, oil with a density of 0.87g/cm3

13. Which state of matter is compressible? Compressible means you can squish it into a smaller space.Gas

14. Draw the particles in a solid, liquid, and gas.

15. Classify the following as an element, compound or mixture.

a. NaBr __Compound_______________

b. Br2 __Element_______________

c. Na + Br2__Mixture_______________

16. What is the difference between a mixture and a compound?

A compound is two or more elements that are bonded together. A mixture is two or more substances that are in a container together but are not chemically connected.

17. What type of process is used to separate a mixture?(Is it chemical or physical?) Physical

18. What type of process is used to separate a compound?(Is it chemical or physical?) Chemical

19. What do the following symbols mean?

a. (s) __Solid_______________

b. (l) __Liquid_______________

c. (g) __Gases_______________

d. (aq) __Aqueous_______________

e. ( __Yields_______________

20. How can you separate a mixture of salt water?

Boil the salt water so that the water turns to gas. Salt will be left behind in the beaker.

21. How do you identify a substance as a compound?

Each substance has a unique set of properties by which it can be identified. For example, the color, melting point temperature, density, odor, and reactivity can serve as clues for identifying the substance.

22. List four examples chemical change. What happens to matter during this change?

Color change, formation of a gas, formation of a precipitate, and energy change (light or heat) are all signs that a chemical change has occurred. Bonds are broken, atoms are rearranged, and new bonds form during chemical changes.

23. List four examples a physical change. What happens to matter during this change?

Tearing a piece of paper, melting a stick of butter, dissolving salt in water, and crushing a peanut are all examples of physical changes. The material is altered but the chemical composition is unchanged during a physical change.

24. Would cooking be considered a chemical or physical change? Explain.

Cooking is a chemical change because the properties of the food are changed. For example, meat changes color from red to brown. The taste and odor of foods change when the food is cooked. These indicate that the chemistry of the food is altered.

25. What evidence suggests a chemical change has occurred?

Color change, formation of a gas, formation of a precipitate, and energy change (light or heat) are all signs that a chemical change has occurred.

26. Define the law of conservation of mass. Make drawing to represent this concept.

Matter cannot be created or destroyed.

OO + ∆Ω∆ ( OΩO + ∆∆

27. 2H2 + O2 ( 2H2O Label the reactants. Label the products.

If you have 4 grams of hydrogen and 32 grams of oxygen, how many grams

of water would you make?

Reactants - H2 and O2

Products - H2O

You would make 36 grams of water.

28. What is the rule for multiplying/dividing numbers using significant figures?

Among the numbers that are multiplied or divided, the number with the fewest significant figures determines the number of significant figures that the answer may have.

29. What is the adding rule for significant figures?

Among the numbers that are added or divided, the number that is the least detailed (stops at the earliest placeholder) limits how detailed the answer may be. For example, when adding 10.1 and 5.000005, 10.1 is the least detailed. It stops at the tenths spot. Therefore, the answer may only go to the tenths spot. 15.1

30. The following length measurements were taken by students using several different measuring devices. Find the average of the measurements. Make sure that your answer has the correct number of significant figures.

10.05 cm, 10.1 cm, 9.741 cm, 10.6 cm, 10.5 cm

(10.05 + 10.1 + 9.741 + 10.6 + 10.5) / 5 = 51.0 / 5 = 10.2

31. Convert 30.0mg to g 30.0 mg x (1 g / 1000 mg) = 0.030 g

Convert 50.0kL to mL. 50.0 kL x (1000 L / 1 kL ) x ( 1000 mL / 1 L ) = 5.00 x 107 mL

Convert 3.5kg to mg 3.5 kg x (1000 g / 1 kg ) x ( 1000 mg / 1 g ) = 3.5 x 106 mg

32. Convert – 35 ˚C to K.

TK = T ˚C + 273 TK = -35 + 273 TK = 238 K

33. How many sig figs are in these numbers?

a. 34.0 ___3_________

b. 0.0023 ___2_________

c. 4500 ___2_________

d. 100.00 ___5_________

e. 6.023 x 1023 ___4_________

34. Place the number 0.0000000067 into scientific notation. 6.7 x 10-9

35. Place the following numbers on the number line below: 1x1010, -1, 1x101, 100, 1x10-10, 10

0

36. Use factor label or dimensional analysis to convert 45.0 feet into cm. (12 inches = 1 ft ; 2.54cm = 1 inch)

45.0 feet x (12 inches / 1 ft) x (2.54 cm / 1 inch) = 1370 cm

37. In the measurement, 23.0 g, what is the estimated digit? The zero is the estimated digit.

38. Calculate the mass of an object with a density of 2.70g/cm3 and a volume of 45.2cm3.

Density = mass / volume 2.70 = mass / 45.2 (45.2)(2.70) = mass 122 g = mass

39. The density of osmium, which is the densest metal, is 22.57 g/cm3. Is a 230g block of metal that measures 1.00 cm [pic] 4.00 cm [pic] 2.50 cm osmium? Explain.

Volume = length x width x height = 1.00 cm [pic] 4.00 cm [pic] 2.50 cm = 10.0 cm3 230g / 10.0 cm3 =23 g/cm3

The sample is likely to be Osmium. Significant figures limit the precision of the answer so we cannot be sure.

40. Calculate the percent error for all the data recorded by the student of a glass rod labeled 23.490 cm. A student measures the length of a glass rod five times and records the data as:

23.487 cm Average = 23.495 cm % error = 100% x (accepted – experimental) / accepted

23.493 cm

23.516 cm % error = 100% x (23.490cm – 23.495cm)/(23.490cm)

23.501 cm

23.477 cm % error = 0.02 %

41. Does any change violate the Law of Conservation of Mass?

Matter cannot be created or destroyed. Matter can be converted into energy according to Einstein’s famous equation (E=mc2).

42. A 13-g sample of calcium reacts with bromine to form 24 g of calcium bromide. How many grams of bromine are used in the reaction? 11 grams

43. What is the “Gold Foil Experiment”? What did this suggest about the structure of the atom?

Rutherford shot alpha particles at a sheet of gold foil. Most of the particles when straight through the foil while a few were deflected. This suggests that the atom is mostly empty space in addition to having a small central core that is positively charged.

44. List the number of protons, neutrons, and electrons in [pic]C.

6 protons, 7 neutrons, and 6 electrons

45. Where in the atom do you find all of the subatomic particles? It might be helpful to draw an atom.

Protons and neutrons are found in the center of the atom, called the nucleus. The electrons move about in the electron cloud that surrounds the nucleus.

46. Which subatomic particle(s) defines the identity of the atom? Protons

47. Which subatomic particle(s) determines chemical properties? electrons

48. Which subatomic particle(s) have a relative mass of 1 amu? 0amu?

Protons and neutrons have a mass of 1 amu. Electrons have a mass of 0 amu.

49. Which subatomic particle(s) have a charge?

Protons are positively charged. Electrons are negatively charged.

50. What element has the atomic mass of 24 and an atomic number of 11? Sodium

51. What is the difference between an atom and an ion?

An atom is neutral. It has equal numbers of protons and electrons. An atom becomes an ion when it gains or loses electrons.

52. What is the charge of an element with 12 protons and 10 electrons? +2

53. What is the difference between an atomic number and a mass number?

Atomic number is the number of protons in an atom. The mass number of an atom is the number of protons and neutrons.

54. Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0% abundant. Calculate the average atomic mass for element Z?

[ (19.0)(55.0) + (21.0)(45.0) ] / 100 = 19.9

55. Draw a model of the atom as described by Dalton, Thomson, and Rutherford.

Dalton Thomson Rutherford

56. In what block would you find the following elements?

K ___s___ Ba ___s_____ Cl ____p____ Sn___p___ Cu___d____ U____f___

57. Consider the following: Ca -40 Ca-41

a. How many protons do these isotopes have? ______20_____ _____20______

b. How many neutrons do these isotopes have? ______20_____ _____21______

c. How many electrons do these isotopes have? ______20_____ _____20______

58. What is the definition of an isotope? How could you predict the most common isotope of an element?

Isotopes are atoms that have the same number of protons but different numbers of neutrons. The most common isotope of an element has a mass number nearest to the average atomic mass of the element.

59. Where are the most active nonmetals located on the periodic table? Most active metals?

The mose active nonmetals are located up and to the right on the periodic table. These nonmetals have high electronegativities, which means that they have a strong tendency to attract electrons. The most active metals are found down and to the left on the periodic table. These elements have low ionization energies, which means that little energy is required to remove an electron from these elements during a reaction.

60. In Bohr’s model, where are the electrons located?

Electrons are located on rings that surround the nucleus. The rings represent different energy levels.

61. What is the difference between the ground state and an excited state in reference to electron configuration?

When atoms are in the ground state, electrons fill orbitals of lowest energy first. In other words, they abide by Aufbau’s Principle. The electron configurations of atoms in the ground state follow the typical filling order that is laid out on the periodic table. When electrons are excited, they fill orbitals of higher energy regardless of vacancies on lower energy levels. The electron configurations deviate from the typical filling order that is laid out on the periodic table.

62. Which type of electromagnetic radiation has the highest frequency?

Gamma rays

63. Which color of visible light has the longest wavelength? The shortest?

Longest wavelength – Red Shortest Wavelength – Violet

64. Why do metals emit photons when heated?

The heat energy is absorbed by electrons in the metallic atoms. The electrons become excited to a higher energy level. They then fall back down to the ground state and emit the energy that they had absorbed.

65. The quantum mechanical model is based on mathematical _probabilities___.

66. How many orbitals are in an

a. s sublevel? __1_____

b. p sublevel? __3________

c. d sublevel? ___5________

d. f sublevel? ___7________

67. What is the maximum amount of electrons that can occupy an orbital? Two

68. Pauli’s exclusion Principle states that no more than two electrons can occupy an orbital, provided they have opposite spins. In what directions can these electrons spin?

Up spin and down spin…or….+1/2 spin and -1/2 spin

69. What is the maximum number of electrons in the first energy level? The second energy level?

First energy level – 2 electrons Second energy level – 8 electrons

70. Give the electron configuration for a neutral atom and an ion for each element below.

|Element |Electron Configuration of Atom |Electron Configuration of Ion |

|Argon |1s22s22p63s23p6 |1s22s22p63s23p6 |

|Chlorine |1s22s22p63s23p5 |1s22s22p63s23p6 |

|Beryllium |1s22s2 |1s2 |

|Potassium |1s22s22p63s23p64s1 |1s22s22p63s23p6 |

|Nitrogen |1s22s22p3 |1s22s22p6 |

71. What are valence electrons? How do you determine the valence electrons for a given atom?

The electrons in the outermost energy level, you can determine the valence electrons for groups IA-VIIIA by looking at the periodic table.

72. Complete the following table.

|Element |Atomic Number |Orbital Diagram |Electron Configuration |

|Magnesium |12 |[pic] [pic] [pic][pic][pic] [pic] |1s22s22p63s2 |

| | |1s 2s 2p | |

| | |3s | |

| Nitrogen |7 |[pic] [pic] |1s22s22p3 |

| | |1s 2s 2p | |

|Neon |10 |[pic] [pic] [pic][pic][pic] |1s22s22p6 |

| | |1s 2s 2p | |

73. Explain why the 4s sublevel fills before the 3d sublevel begins to fill as electrons are added.

Electrons fill the sublevel with the lowest energy first. The 4s is lower in energy than the 3d.

74. How many periods are on the periodic table? 7 How many groups? 18

75. Where are the nonmetals located on the periodic table? Upper Right

76. Where would you find the transition elements? D-block….Middle of the periodic table. Group B elements.

77. What is the name of the group on the periodic table that is considered to be inert? Noble Gases

78. What are the properties of metals? Good conductors, high luster, ductile, malleable

79. What are the properties of nonmetals? Poor conductors, brittle, dull

80. What is the first element in each family?

a. Alkali metals ________lithium____________

b. Alkaline Earth metals ________beryllium____________

c. Halogens ________fluorine____________

d. Noble Gases ________helium____________

81. How many valence electrons do elements in each family have?

a. Alkali metals ______1______________

b. Alkaline Earth metals _______2_____________

c. Halogens _______7_____________

d. Noble Gases _______8_____________

82. Draw the electron dot structure (Lewis Structure) for the Halogen in the third period. [pic]

83. Draw the electron dot structure (Lewis Structure) for the Alkali metal in the fifth period[pic]

84. Draw the electron dot structure (Lewis Structure) for the Nobel gas in the fourth period. [pic]

85. What do elements in the same group have in common?

Same number of valence electrons, they will also have similar properties.

86. When elements in the following families form ions, what is the ion charge?

a. Alkali metals ___ +1 _________________

b. Alkaline Earth metals ___+2 _________________

c. Halogens ___-1_________________

d. Noble Gases ____neutral (no charge)_______________

1. As you move across the periodic table from left to right, what happens to the following properties?

a. atomic number __increases__________________

b. atomic radius __decreases__________________

c. ionization energy __increases__________________

d. electronegativity __increases__________________

2. As you down a group, what happens to the following properties?

a. atomic number ___increases_________________

b. atomic radius ___increases_________________

c. ionization energy ___decreases_________________

d. electronegativity ___decreases_________________

87. Which is larger, an ion of potassium or an atom of potassium? K+ the atom is larger than the cation.

88. Which is larger, an ion of oxygen or an atom of oxygen? The oxygen ion is larger, anions are larger than their atom.

89. Arrange the elements given below in the increasing order of their atomic size. (smallest) A, D, B, C (largest)

Element A: 1s22s22p6

Element B: 1s22s2

Element C: 1s22s22p63s1

Element D: 1s22s22p3

90. What is the charge of an aluminum ion? A chloride ion? A nitride ion? A phosphide ion? A magnesium ion?

Al+3 Cl-1 N-3 P-3 Mg+2

91. What are the properties of ionic compounds? Use the following terms in your answer: electronegativity, melting point, conducting electricity, crystalline structure, and solubility.

| |Ionic Compounds |

|Electronegativity |0.4 – 2.0 |

|Melting points |high |

|Physical state |Solid (crystalline) |

|Electrical Conductivity |High when dissolved or melted |

| |No conductivity as a solid |

|Solubility |Usually high in water |

92. What are elements trying to achieve when forming compounds?

Noble gas configuration (octet rule) – eight valence electrons

93. What is a cation? How do atoms become cations?

Positively charged ion, they are formed by a neutral atom losing electrons.

94. What is an anion? How do atoms become anions?

Negatively charged ion, they are formed by a neutral atom gaining electrons.

95. Which of the following can form ionic compounds? (Choose all that apply)

a. Two cations

b. Two anions

c. A cation and an anion

d. Two nonmetals

e. Two metals

f. A metal and a nonmetal

96. What happens to electrons in an ionic compound?

Electrons are gained or lost . Metals (cations) lose their electrons, while nonmetals (anions) gain those electrons.

97. What is the formula for each compound below?

a. magnesium hydroxide? Mg(OH)2

b. strontium nitrate? Sr(NO3)2

c. ammonium sulfide? (NH4)2S

d. potassium phosphate? K3PO4

e. magnesium chloride? MgCl2

98. Name the following compounds. Hint: Use the Stock system.

a. CuCl Copper (I) chloride

b. SnCl2 Tin (II) chloride

c. FeBr3 Iron (III) bromide

d. SnO Tin (II) oxide

99. What is a metallic bond?

Metallic bonds join metal cations together. The metal atoms become cations by donating electrons to the “sea of electrons” that surround the metal cations. The electrons in the “sea of electrons” are delocalized (spread out) around the metal cations.

100. Why are metals good conductors of electricity?

The electrons in the “sea of electrons” are free to flow through the metal forming an electric current.

101. What piece of equipment do you use to move a hot beaker?

Beaker tongs

102. What piece of equipment do you use to move a hot crucible?

Crucible tongs

103. What should be the last thing you do before leaving the lab table?(Think safety!)

Wash your hands!

104. Which of the following types of radiation has the most penetration power? Alpha, beta, or gamma

Gamma radiation

105. What are the symbols used to represent an alpha particle, a beta particle, and a gamma ray?

Alpha α Beta β Gamma [pic]

4 0

He e

2 -1

106. What two particles make up a neutron?

Proton and electron

107. What is the charge of an alpha particle, a beta particle, and a gamma ray?

Alpha particle +2 Beta particle -1 Gamma ray has no charge

108. What type of material would help to shield you from the effects of gamma rays?beta particles? Alpha?

You need thick lead or concrete to shield yourself from gamma rays.

You need materials like plastic, glass, or wood to shield yourself from beta radiation.

You need paper to shield yourself from alpha radiation.

109. What is fusion? Where does this process occur?

Fusion occurs in stars where there is sufficiently high temperatures and pressure. Small nuclei undergo fusion when they join together to form larger nuclei. This process releases enormous amounts of energy.

110. What is fission? How is this process started?

Fission occurs when a large nuclei breaks into two smaller daughter nuclei. This process is triggered by shooting a neutron at an atom of Uranium-235. The mass increases to 236 and the nucleus becomes unstable. The nucleus then breaks apart and releases an enormous amount of energy.

111. Which process is responsible for the creation of the elements?

Fusion

112. What particle is needed to complete the following nuclear equation?

209 4 205

Po ( He + Pb

84 2 82

113. What particle is needed to complete the following nuclear equation?

45 0 45

Ca ( e + Sc

20 -1 21

114. What particle is needed to complete the following nuclear equation?

22 0 22

Na ( e + Ne

10 -1 11

115. What particle is needed to complete the following nuclear equation?

238 4 234

U ( He + Th

92 2 90

-----------------------

1x10-10

1x1010

1x101

100

-1

10

[pic]

electrons

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