Download Integrated Science 3

Chemistry
Semester One Final Exam Study Guide
1. Identify the following as quantitative or qualitative data:
(a) A flame is hot.
(b) A candle has a mass of 90g.
(c) Wax is soft.
(d) A candle’s height decreases 4.2 cm per hr.
2. Three students made multiply weighings of a copper cylinder, each using a different balance. The correct
mass of the cylinder had been previously determined to be 47.432g. Describe the accuracy and precision of
each student’s measurements.
Data Table 1: Cylinder Mass Measurements
Student 1
Student 2
Weighing 1
47.13 g
47.45 g
Weighing 2
47.94 g
47.39 g
Weighing 3
47.83 g
47.42 g
Weighing 4
47.47 g
47.41 g
Student 3
47.95 g
47.91 g
47.89 g
47.93 g
Student 1 __________________________________________________
Student 2 __________________________________________________
Student 3 __________________________________________________
3. A chemist needs 2.00 g of a liquid compound.
(a) What volume of the compound is necessary if the density of the liquid is
0.718 g.
(Use unit conversion/dimensional analysis method)
3
cm
4. What are the standard base SI units of measurement for each type of measurement?
Mass
Quantity of substance
Length Time
Temperature Volume
5. Explain what is meant by a derived value. Give an example.
6. Show as scientific notation (standard form):
(a) 0.000 000 000 0105 km
(b) 91 730 000 000 000 000 dimes
Show in long form:
(c) 6.05 x 10-6 cm
(d) 9.90 x 104 dimes
7. Sketch and draw the Lewis dot structures for CO2, H2O, CH4 and NH3. What shape is each molecule? Why
do they have different shapes?
8. Count the the total number of each type of element present in one formula unit.
a. Al2(CO3)3
b. (NH4)3PO4
9. When writing formulas and names for ionic and molecular compounds, what clues do you use to determine if
the compound is ionic or molecular?
10. Write the correct name for each compound. Identify whether it is ionic or molecular.
a. Mg(OH)2
b. BaSO4
c. Fe(NO3)3
d. CuCl2
e. SO2
11. Write the correct formula for the following compounds
a. carbon disulfide
e. Tin(IV) fluoride
b. Calcium oxide
c. Aluminum bromide d. Iron (II) phosphide
f. Ammonium sulfate
g. Calcium phosphate
h. dinitrogen tetroxide
12. Use Lewis dot to show the formation of covalent bonds in the following compounds, atoms or ions:
a) Mg
b) OHc) HF
d) PO43e) CO2
13. Sodium chloride, NaCl is bonded ionically. Chlorine gas, Cl2 is bonded covalently. Explain why there is a
difference in the bonding in these two molecules.
14. TEMPERATURE CONVERSION: Convert -8.0 oF to
a. oC
b. Kelvin
15. A sample of a mineral has a volume of 14.5 mL and a mass of 135.5 g. What is its density? (watch sig figs)
16. Use the density of the mineral sample in question #19 above to calculate the volume of 3.2 grams of that
mineral. (watch sig figs)
17.
(a)
(b)
(c)
(d)
If an element has an atomic number of 17 and a mass number of 37
Identify the element _____________
Identify the number of electrons ____________
What state is this element in at room temperature?_________
Draw the electron distribution of an atom of this element.
18. As your eyes move across the periodic table from left to right in the second period the atomic radii gets
____________.
Explain this pattern. What happens to ionization energy across a period?
19. What is true about the element immediately below the element that has an atomic number 17 in the periodic
table.
a) 17 electrons in its outer most level
c) 17 protons in nucleus
b) 7 electrons in its outermost level
d) 7 protons in its nucleus
20. Two atoms that are isotopes have the same number of which subatomic particles? ________________ and
_________________.
21. What is the number of valence electron in an atom of element number 19?
22. An ion is formed by the transfer of _______________(what subatomic particles) ?
23. Compare & contrast ionic bonding and covalent bonding.
24. How is a polar molecule different from a nonpolar molecule? Explain whether H2O and CO2 would be
polar or nonpolar molecules.
25. Which of the following are chemical changes and which are physical changes?
a. Mixing sugar in water.
b. Rusting of a water pipe.
c. The melting of ice to form water.
d. Digestion of carbohydrates.
e. Heating a compound.
f. Dilution of a concentrated acid to form a less concentrated acid.
26. What is the difference between:
a. Compound and element
c. mixture and compound
b. atom and molecule
d. heterogeneous mixture and homogeneous mixture
27. Decide if the following are mixtures or pure substances. If it is a pure substance, decide if it is a compound
or element. If it is a mixture, decide if it is heterogeneous or homogeneous.
a) chicken soup
c) sugar water
e) concrete
g) air
b) pure gold
d) bronze
f) NaCl
28. Round the following numbers to the indicated number of digits or decimal place
Round to 3 digits:
245.4 _________
.3347 _________
12.0099________
2.509 _________
Round to 4 digits:
.143098 _______
23.5555_______
Round to the tenths place:
.449 __________ 3.054 __________
10034_________
99999_________
9.999 __________
0.099 __________
29. Complete the following mathematical operations and round your answer to the correct number of
significant figures and in scientific notation.
710 x 0.587 = _________
3.95 x 1012 mm3 / 7.8 x 107 mm = __________
0.3795 x 25 = _________
1.54 x 10-6 cm2 / 8 x 103 cm____________
2.84 x 10-5 x 6.06 x 100 ________
9.111 x 108 L3/ 3.71 x 1023 L2 = _________
50059400 x 41.3 _________
3.770 g + 910.55 g + 14.7 g = ___________
30. What's the difference between an alpha and a beta particle?
31. Show the alpha particle decay of radium - 222 to radon - 218.
32. Show the beta particle decay of iodine - 131 to xenon - 131.
33. What types of evidence indicate that a chemical reaction has taken place?
34. Study the molecular models of Rutherford, Dalton, Bohr and Schrodinger.
35. If a molecule is polar it is
A) positive
D) slightly negative
B) negative
E) slightly positive on one side and slightly negative on the other side
C) slightly positive
Electron emission and absorption: (See Questions 36 –39)
C
D
B
E
A
F
36. Which three of the lettered energy changes show absorption of energy by the atom? ___________
37. Which three of the lettered energy changes show emission of light energy by the atom?___________
Of the three lettered energy changes that involve emission, one results in the emission of violet light, one results
in the emission of green light and one results in the emission of red light.
38. Which of the changes results in red light? ______ How can you tell?
39. Which of the changes results in violet light? ______ How can you tell?
40. The element bromine has two isotopes. One isotope has a mass of 78.92 amu and a relative abundance of 50.69%.
The second isotope has a mass of 80.92 amu and a relative abundance of 49.31%. Calculate the atomic mass
(weighted average) of the element bromine. Show your work.
41. The substance calcium chloride is a chemical combination of which particles?
a. calcium atoms and chlorine molecules (Cl2)
b. calcium atoms and chlorine atoms
c. Calcium ions and chlorine molecules
d. calcium ions and chlorine ions
42. Answer the following for the element Magnesium:
a. Atomic number ________
b. Atomic mass _________
c. Mass number ________
43
a. Number of protons in Mg__________
b. Number of electrons in Mg _________
c. Number of neutrons in Mg _________
44. Fill in the following chart according to each element’s properties:
Element
Cesium
Bromine
Calcium
Solid at room temp
Liquid at room temp
Gas at room temp
Metal
Non-metal
Metalloid
Group Name
Use the electronegativity table to classify the bond in each of the following substances as ionic, non-polar
covalent, or polar covalent. Also give the difference in electronegativity.
45. CsCl ______________________
46. O2 __________________________
47. Indicate which of the following two compounds conduct an electric current in solution:
conducts
non-conductor
A) KBr
_______
________
Explain:________________________________
B)
P2O5
_______
________
Explain: ________________________________
Matching: Write the letter of the term on the blank line that best answers each question. Answers may be used once,
more than once or not at all, only one answer per blank.
A) Covalent bond
E) Oxygen family
I) Halogens
_____48.
_____49.
_____50.
_____51.
_____52.
B) Transition metal
F) Metals
J) Nitrogen family
C) Noble gases
G) Non-metals
K) Molecule
D) Ionic bond
H) Representative element
L) Formula unit
What family of elements has a full valence energy level?
Members of what family of elements have five valence electrons?
What type of chemical bond is formed in molecular compounds?
What type of element often requires a Roman numeral in the name?
Compounds formed by which type of bond can have a low melting point?
Classify the following as a heterogeneous mixture, homogeneous mixture, compound, or element.
53. oxygen (O2)___________________________
54. gasoline___________________________
55. A stream with gravel on the bottom___________________________
56. silicon (Si)___________________________
57. table salt (NaCl)___________________________