Name_____________________________
Date______________________
Period______
Chemistry – 1st Semester Final Exam
***ALL ANSWERS MUST INCLUDE THE PROPER UNITS AND NUMBER OF SIG FIGS***
1. 177 mL =
__0.177____ L
2. 0.093 kg =
__93000__ mg
3. How many seconds are there in 3.50 years? (1 year = 365 days) 1.10 x 108 seconds
4. If the beams are in balance, with the riders in the position shown, what is the total mass in grams of the object being
massed? 466.20 g
5.
When looking at a MSDS safety label, which color shows you the flammability? red
6. Which are these pieces of equipment called?
Erlenmeyer flask
Graduated Cylinder
Beaker
Volumetric Flask
7. The following weighings were made during a laboratory exercise:
Mass of evaporating dish....
59.260 g
Mass of evaporating dish + sugar sample..........
61.61 g
What is the mass of the sample, expressed to the proper number of significant figures? 2.35 g
8. The diagram below shows the upper part of a laboratory burner.
What letter represents the hottest part of the burner flame? C
9. A student has to measure the diameter of a test tube in order to calculate the tube's volume. Based on the diagram below,
the tube's diameter is closest to 1.25 cm
10. Which of the following is the correct reading of the meniscus as shown in the portion of the buret below? 41.35
11. Matter is defined as anything that occupies space and has ____mass___________________.
12. What are the two types pure substances? elements and compounds
13. Mixtures are defined as two or more substances physically combined____.
14. Compounds are usually broken down into their component elements by _chemical means________________________.
15. What is the frequency of light with a wavelength of 1.87 x 10-14 m?1.50 x 1022 hz
16. What is the wavelength of light with a frequency of 5.60 x 1014 Hz?5.36 x 10-7 m
17. What condition is an atom in, when all electrons are in their normal energy levels? Ground state
18. What is the distance between the crests of a wave? wavelength
19. List the types of EM energy from highest frequency to lowest. AM, shortwave, TV, FM, Microwave, infrared, visible, UV,Xray, gamma
20. List the colors of the visible spectrum. roygbiv
21. Complete the following:
If the Frequency increases the wavelength ___decreases__________________.
22. When energy is applied to an atom and electrons move to higher energy levels, it is in the ____excited__________ state.
23. How much energy is a photon whose frequency is 3.55 x 10 17 Hz?2.35 x 10-16 J
24. What is the correct electron configuration for
24
12𝑀𝑔
? 1s2 2s2 2p6 3s2
25. How many valence electrons are in the following element?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4
6
26. Draw the p-sublevel? Infinity symbol
27. Which element has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d5 ? Mangenese
28. What is the noble gas (shorthand) electron configuration of Silver? [Kr]5s24d9
29. Generally, how many valence electrons are needed for atoms to be most stable?
8
30. Chemistry is… study of matter and energy.
31. List three Intensive properties. Color, density,
32. What are the four phases of matter? Solid, liquid, gas, and plasma
33. What are the two main types of mixtures? Homogeneous and heterogeneous
34. What are the main types of pure substances? elements and compounds
Symbol
91
340𝑍𝑟
Hyphen notation
Zirconium-91
Zinc - _65__
Potassium-41
Zinc-67
Atomic #
40
30
19
30
Mass #
91
65
41
67
# of
Protons
40
30
19
30
# of
Neutrons
51
35
22
37
35. Write the orbital (spin) configuration of the 4 elements in the chart above.
36. What is the molecular mass of (NH4)3PO4
? 149 g/mol
37. How many grams of (NH4)3PO4 are there in 3.457 mols of (NH4)3PO4 ? 515 g
38. How many molecules of (NH4)3PO4 are in 0.0234 moles of (NH4)3PO4 ?1.41 x 1022 molecules
# of
Electrons
43
30
20
28
39. How mols of K2Cr2O7 are there in 12.5 grams of K2Cr2O7 ?0.0425 mols
40. How many grams of Ag2CO3 are there in 3.46 x 1034 molecules of Ag2CO3 ?1.59 x 1013 grams
41. What two parts does the nucleus contain? Protons and neutrons
42. What type of atom vary in the number of neutrons? isotope
43. Who discovered the electron? thomson
44. Who discovered the proton? rutherford
45. Who discovered the neutron? chadwick
46. Who discovered the nucleus? rutherford
47. Whose model do we use to study the atom? bohr
48.
The burning of gasoline
Chemical Change
Physical Change
49. A glass of pure water
Homogeneous
Heterogeneous
50. 325.5 liters
Mass
Volume
51. Mass of a substance
Intensive
Extensive
52. Round
Qualitative
Quantitative
53. Boiling
Chemical Change
Physical Change
54. Iced Sweet Tea
Homogeneous
Heterogeneous
o
55. 105 C
Qualitative
Quantitative
Label the following as Homogeneous, Heterogeneous, element or compound.
56. Air
____ Homogeneous _____
71. Colored Glass
___ Heterogeneous ______
57. Sodium Chloride ______ compound ______
72. Table sugar
_______ compound _____
58. Platinum
____ element _______
73. Sulfur
______ element ____
59. Granite
___ Heterogeneous ____
74. Grape juice
____ Homogeneous __
60. Orange juice (shake well)____ Homogeneous _
75. Nitrogen
_______ element ___
61. Salt water
_____ Heterogeneous ___
76. Baking soda (sodium bicarbonate) compound
62. Pepsi
____ Heterogeneous _____
77. Pure candle wax (paraffin) compound __
63. Milk
____ Heterogeneous ______
78. Ice
____ Heterogeneous ___
64. Water
_____ Heterogeneous ____
79. Blood
_____ Homogeneous _
65. Perfume
____ Heterogeneous ______
80. Ocean water
______ Heterogeneous _____
66. Hydrogen gas
______ element ___
81. Calcium
______ element ____
67. Smog-filled air
Heterogeneous ____
82. Vitamin C (ascorbic acid)_ compound ____
68. Soil
______ Heterogeneous ___
83. Dry ice
____ compound ___
69. Iron
____ element ___
84. Aluminum foil
_______ element ___
70. Milk (fresh from cow)__ Heterogeneous ____
85. Ethanol
_____ compound __
86.
Location
in atom
Charge
Relative
Mass
Discovered
by
Year
Discovered
Electron
Cloud
Negative
0
Thomson
1897
Proton
Nucleus
Positive
1
Rutherford
1919
Neutron
Nucleus
Neutral
1
Chadwick
1932