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Honors Chemistry 2015 Midterm Review
Chapter 1
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Define chemistry.
List the six examples chemistry branches.
Define basic research, applied research, and technological development.
Define mass and matter.
Explain the difference between an atom, element, and compound.
Explain the difference between extensive and intensive properties.
List the four states of matter and compare their atomic arrangements and amounts of energy.
List two examples of homogenous and heterogeneous mixtures and solutions.
Explain the difference between groups and periods.
List three properties of metals, metalloids, and nonmetals.
Chapter 2
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List the steps of the scientific method.
What are SI units used for and name the units for length, mass, temperature, and amount of substance.
List the equivalents for the following prefixes: centi, milli, micro, nano, Angstron, and pico.
What are derived units and name the units for area, volume, density, and molar mass.
Define conversion factor.
Convert 40 nanograms into grams.
Draw four targets and show the differences between accuracy and precision.
Write the equation for percentage error.
Write Avogadro’s number in scientific notation and long form.
Draw an example of direct and indirect proportions.
Chapter 3
1. List and define the three laws of chemistry.
2. List the parts of Dalton’s atomic theory and explain why two are no longer accurate (what have we discovered).
3. Make a chart comparing the people, experiment, particle discovered, and name of the example for: Aristotle,
Democritus, Dalton, Thomson, Millikan, Rutherford, Bohr, and Chadwick.
4. Draw a chart comparing the three parts of the atom, their charge, their abbreviation, their charge, and their
mass number.
5. What is the difference between atomic number and mass number?
6. What is an isotope and how do you find it?
7. Write the hyphen notation and the nuclear symbol of isotopes for the three types of hydrogen.
8. What is average atomic mass?
9. What is the difference between Avogadro’s number and molar mass?
10. Convert 34 grams of glucose into moles and molecules.
Chapter 4
1. Draw the electromagnetic spectrum, label the types of waves, label the colors, and label the ends based on
wavelength, frequency, and energy.
2. List the two equations for light.
3. Explain the difference between ground and excited state for an electron.
4. Draw an electron going through absorption and emission.
5. What is the difference between an emission-line spectrum and a continuous spectrum?
6. Make a chart comparing the following people and their experiments: Planck, Bohr, Einstein, de Broglie,
Heisenberg, and Schrodinger.
7. Define the four quantum numbers.
8. Draw the chart comparing the principal energy levels, the shapes, orbitals, number of possible electrons, and
number of total electrons.
9. Explain Aufbau’s principle, Hund’s rule, and Pauli exclusion principle.
10. Draw an electron orbital notation, configuration, and noble gas notation for carbon, silicon, and iron.
Chapter 5
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Explain what Mendeleev and Moseley did for the periodic table.
Define periodic law.
Name all the group names and list two properties for each.
Draw a periodic table outline and show where each block is located.
Explain the difference between ionization energy, electron affinity, electronegativity, and atomic radii.
List the units for the four trends.
List the elements that are highest for each trend.
Explain what valence electrons are used for and what they determine.
In water what is the most electronegative element?
Explain the difference between ion, cation, and anion.
Chapter 6
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List and define the four types of bonds and the two types of forces.
Define polarity.
Explain how to name ionic and covalent bonds regarding the types of elements in the bond.
Compare and contrast ionic and covalent bonds regarding types of elements and strength and
Define the octet rule and when can it be loop-holed (what type of elements and which block)?
Lewis structure versus Bohr diagram: which electrons do they show?
Explain the use of resonance structures.
Define VSPER theory and hybridization.
Draw and label the three main geometry shapes for hybrid orbitals with angular degrees and names.
What is a polyatomic ion and draw the Lewis structures for hydroxide and hydronium.
Chapter 7
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What is a hydrocarbon?
List the steps for writing binary ionic compounds in formula and nomenclature.
Define oxyanions and explain the difference between –ite and –ate.
List the steps for writing molecular (covalent) compounds in formula and nomenclature.
Explain the difference between an acid and a salt.
List the oxidation numbers for each of the groups.
How do you find the formula mass?
How do you find the percent composition?
What is the difference between empirical and molecular formulas?
What three types of information are used to find an empirical formula from percentage composition data?