Name: ________________________________________________ Date of Midterm: _____________________________
CP Chemistry Midterm Exam: Topic List and Review
Chapter One: Matter and Change
Definition of chemistry and matter
Characteristics of mixtures
Definition of physical and chemical change
Metals, non-metals and metalloids
Branches of chemistry
States of matter
Classification of matter
Elements & compounds
Chapter Two: Measurements and Calculations
Scientific method
Mass, volume and density
Accuracy and precision
Significant figures
Scientific notation
Metric prefixes
SI Units of measure
Conversion factors
Percent error
Calculations using significant figures
Qualitative vs. quantitative
Conversions between Kelvin and Celsius
Chapter 3: Atoms the Building Blocks of Matter
Dalton’s law of atomic theory
Law of definite proportions
Atomic structure
Properties of protons, neutrons and electrons
Atomic mass
Isotopes
Molar mass
Law of conservation of mass
Law of multiple proportions
Scientists/tools/experiments-atomic structure
Atomic number
Calculate average atomic mass*
Mole and Avogadro’s number
Gram↔ Mole↔ Atom Conversions
Chapter 4: Arrangement of Electrons in Atoms
Properties of Waves
Visible light spectra
Energy (E= hν)
Ground state and excited state electrons
Electromagnetic radiation
Speed of light (c = λν)
Line spectra
Electron configuration
Chapter 5: The periodic Law
Historical perspective of the periodic table
Groups / Periods
Organization of the periodic table
Electron configuration
Main group elements (s & p block)
Blocks of periodic table (s,p,d & f)
Family properties
Valence electrons
Periodic trends: atomic radius, ionization energy, electronegativity
Chapter 6: Chemical Bonding
Electronegativity & type of chemical bond
Polar covalent bonds
Lewis dot structures
Single, double, triple bonds and resonance
Common ions and ionic bonds
Ionic bonds
Non-polar covalent bonds
Chemical formulas
Lone pair electrons
Molecular geometry-VSEPR and polarity
Chapter 7: Chemical Formulas and Chemical compounds
Recognizes ions and charges
Write molecular formulas (covalent)
Gram/mole/mass conversions*
Calculate empirical formulas*
Write balanced formula units (ionic)
Molar mass (gram formula mass)*
Calculate percent composition*
* Be able to solve problems by performing calculations (similar to previous tests and worksheets)
CP Chemistry Midterm Review Page #1
Define the following.
1. Physical change 2. Chemical change (chemical reaction) 3. Quantitative observations 4. Qualitative observations –
5. Precision –
6. Accuracy Lab Safety.
7. Write down all lab safety procedures that apply to the following scenario:
Flame Test Lab
Procedure:
1. At each station there is a wooden splint soaking in a known compound.
2. Write down the name of the compound into your data table.
3. Pick up the wooden splint and hold it over the hottest part of the Bunsen burner flame. (This is the
center towards the base of the flame. Do NOT touch the wooden splint to the Bunsen burner.)
4. Record the color of the flame in your data table.
5. Replace the wooden splint into the solution.
6. Go to the next station and repeat steps 2-5.
7. Determine which element ion was responsible for the color.
8. Repeat steps 2-5 for the 4 unknown compounds. Record this information under the “Unknown
Compounds” in the Data section.
Applicable Safety Rules to Follow (be sure to number your procedures):
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CP Chemistry Midterm Review Page #2
Significant Digits. How many significant figures are in each measurement?
8. 1.20
__________
12. 0.20300
__________
9. 0.007
__________
13. 140000
__________
10. 123.400
__________
14. 5.698 x 1.23
__________
11. 7.8 X 1023
__________
15. 7.8/1.29
__________
Scientific Notation. Convert the following between scientific notation and standard notation.
16. 4,200
____________________
19. 3.50 x 105
____________________
17. 0.000652
____________________
20. 9.99 x 10-3
____________________
18. 1.23
____________________
21. 2.00 x 10-1
____________________
Density. Answer the following. Remember to round your answer to the appropriate number of significant figures.
22. An object has a mass of 5.25 g and a volume of 1.2 ml. What is the density?
23. An object has a density of 2.2 g/ml and a mass of 4.9 g. What is the volume?
24. An object has a volume of 3.25 ml and a density of 1.2 g/ml. What is the mass?
Percent Error
25. If a student determines the density of a copper object is 8.46 g/ml and the accepted value is 8.96 g/ml, what is
the percent error?
Unit Conversions
26. Convert 9,014 kg to g
27. Convert 7.2 L to mL
CP Chemistry Midterm Review Page #3
Define.
1. Atom -
2. Ion -
3. Isotope -
History.
4. Describe the experiment that JJ Thomson used to discover the electron.
5. Ernest Rutherford conducted the gold foil experiment to disprove Thomson’s plum pudding model. Describe the
outcome of the experiment.
Atomic Structure.
6. The smallest unit of an element that still maintains the properties of that element is a(n) ___________________.
7. The subatomic particles, ___________________ and ___________________ have about the same mass.
8. Fill in the table (parts of an atom).
Charge
Proton
Neutron
Electron
Location
CP Chemistry Midterm Review Page #4
9. Fill in the Chart
Element
Ion
2
Atomic
Number
Mass
Number
Protons
H+1
24
Mg+2
39
K
15
N-3
16
O-2
7
Li+1
Electron Configuration and Dot Diagrams
10. Write the electron configuration for Fluorine.
11. Write the electron configuration for Cadmium.
12. Identify the following elements by symbol and name:
a. 4d10
__________________________________________
b. 6p2
__________________________________________
c. 5s1
__________________________________________
13. Draw the Lewis dot structure for Chlorine.
14. Draw the Lewis dot structure for Boron.
Neutrons
Electrons
CP Chemistry Midterm Review Page #5
Periodic Table Trends.
1. Label the table with the following:
Alkali Metals
Halogens
Alkaline Earth Metals
Metalloids
Chalcogens
Lanthanide Series
Transition Metals
Actinide Series
Noble Gases
Metals
Nonmetals
+1, +2, +3, +/-4, -1, -2, -3
s, p, d, f blocks
Group
Period
2. In terms of electron arrangement, which group is chemically un-reactive due to a full outside shell?
___________________________
3. Which element touching the staircase is not a metalloid? ____________________________
4. Follow the numbers in the boxes of the elements in one group as you trace down the group. What do you notice
about the changes in the atomic mass as you go down the group? _____________________________
a. What about the number of electron shells? ______________________________________________
5. Atomic radius ________________ across a period and _________________ down a column.
6. Electronegativity ________________ across a period and _________________ down a column.
7. Ionization energy ________________ across a period and _________________ down a column.
8. The major reason for each of these trends across a period is an increase in _______________ ______________.
The major reason for each of these trends down a group is an increase in ________________ ______________.
CP Chemistry Midterm Review Page #6
Formula Writing and Percent Composition. Calculate the formula weight for the following and determine the percent
composition for the underlined element:
9. Na2SO4
10. (NH4)3PO4
Formula writing
Write the formulas for the following
1. aluminum oxide
_______________
6. aluminum phosphate
_______________
2. copper (I) nitrate
_______________
7. manganese (II) bromate _______________
3. calcium sulfate
_______________
8. diboron tetrabromide _______________
4. chromium (IV) silicide _______________
9. carbon tetrachloride
_______________
5. aluminum sulfate
10. iodine pentafluoride
_______________
_______________
Write the names for the following
11. Na2O
__________________________________
12. KOH
__________________________________
13. (NH4)2SO3
__________________________________
14. Fe2O3
__________________________________
15. Cu2SO4
__________________________________
16. S5Cl9
__________________________________
17. CH4
__________________________________
18. N2S3
__________________________________
19. CO
__________________________________
20. HNO3
__________________________________
Bonding.
19. Ionic bonds usually occur between ____________________________ and ____________________________
and involves the sharing/transfer of electrons. (circle one)
20. Covalent bonds usually occur between ___________________________ and ____________________________
and involves the sharing/transfer of electrons. (circle one)
CP Chemistry Midterm Review Page #7
Match the characteristic/properties with the appropriate type of bonding (either a or b goes on each line):
a. Covalent Bonds
b. Ionic Bonds
21. ______ Low solubility
25. ______ Does not conduct electricity
22. ______ Soluble in water
26. ______ Conducts electricity
23. ______ High electronegativity difference
27. ______ Low melting point
24. ______ Low electronegativity difference
28. ______ High melting point
Based on electronegativity, predict if they will form ionic, covalent, or polar covalent bonds.
ie. Bromine monoxide
3.5- 2.8 = 0.7
(type of bond)
29. Phosphorus trichloride
__________________
_________________
30. Magnesium fluoride
__________________
_________________
31. Iodine (I2)
__________________
_________________
32. Rubidium chloride
__________________
_________________
33. Potassium oxide
__________________
_________________
34. Carbon monoxide
__________________
_________________
Wavelength, Frequency and Energy.
1. Calculate the wavelength of light if the frequency of the radiation is 9.8 x 1014 Hz.
2. Calculate the energy of a radiant energy with a frequency of 2.70 x 1015 Hz.
3. What frequency is radiation with a wavelength of 2.90 x 10-6 cm? What is the energy?