Download Chemistry 250 1st Semester Exam

Chemistry 250 1st Semester Exam
Materials: #2 pencils and a calculator
Expect multiple-choice and a small sampling of problems.
Start early and prepare a little every night. Budget certain
chapters for certain nights.
This study guide includes the major concepts we have covered
in quarters 1 and 2.
Chapter 1: Introduction to Chemistry
Vocabulary: Ozone layer, CFCs, chemistry, matter, mass, weight,
scientific method, qualitative data, quantitative data, hypothesis,
experiment, independent variable, dependent variable, control,
conclusion, model, theory, scientific law
Experiment 1: Making Factual Observations
1.
2.
3.
4.
5.
6.
7.
8.
9.
Explain the formation and importance of ozone
Describe the development of chlorofluorocarbons.
Compare and contrast mass and weight.
Explain why chemists are interested in a submicroscopic
description of matter.
Identify the common steps of scientific method.
Compare and contrast types of data.
Construct a well-controlled experiment.
Describe the difference between a theory and a scientific
law.
Apply knowledge of laboratory safety.
Chapter 2: Data Analysis
Vocabulary: base unit, second, meter, kilogram, derived unit, liter,
density, Kelvin, scientific notation, conversion factor, dimensional
analysis, accuracy, precision, percent error, significant figure, graph,
Experiment 3: Experimental Uncertainties
Experiment 4: Relationships Between Variables: Mass and
Volume of a Liquid
Problems: 1-3, 12-21, 31-39, 72-85, 87
1. Define SI base units for time, length, mass, and temperature.
2. Explain how adding a prefix changes a unit.
3. Compare the derived units for volume and density.
4. Express numbers in scientific notation.
5. Use dimensional analysis to convert between units.
6. Define and compare accuracy and precision.
7. Use significant figures and rounding to reflect the certainty of
data.
8. Use percent error to describe the accuracy of experimental data.
9. Create graphs to reveal patterns in data.
Chapter 3: Matter-Properties and Changes
Vocabulary: substance, physical property, extensive property,
intensive property, chemical property, states of matter, solid, liquid,
gas, vapor, physical change, chemical change, law of conservation of
mass, mixture, heterogeneous mixture, homogeneous mixture,
solution, filtration, distillation, crystallization, chromatography,
element, periodic table, compound.
Experiment 2: Conservation of Mass
1. Identify the characteristics of a substance
2. Distinguish between physical and chemical properties
3. Differentiate among the physical states of matter
4. Define physical change and list several common physical
changes
5. Define chemical change and list indications that a chemical
change has happened.
6. Apply the law of conservation of mass to chemical reactions.
7. Contrast mixtures and substances
8. Classify mixture as homogeneous or heterogeneous
9. List and describe several techniques used to separate mixtures
10. Distinguish between element and compounds
11. Describe the organization of elements on the periodic table
12. Assigned element symbols
Chapter 4: The Structure of the Atom
Vocabulary: atomic theory, atom, cathode ray, electron, nucleus,
proton, neutron, atomic number, isotope, mass number, atomic mass
unit (amu), atomic mass, nuclear reaction, radioactivity, radiation,
radioactive decay, alpha radiation, alpha particle, nuclear equation,
beta radiation, beta particle, gamma ray, half life
Legumium Lab
Problems: 11-17, 59-68
1. Discuss and explain the contributions of Aristotle, Democritus,
Dalton, Crooke, Thomson, Millikan, Chadwick, and Rutherford.
2. Summarize the different models of the atom: Dalton’s atomic
theory, Thomson’s Plum Pudding Model, Rutherford’s Nuclear
Model.
2. Define and describe the atom.
3. Distinguish between subatomic particles in terms of relative
charge and mass.
4. Describe the structure of the atom, including locations of
subatomic particles.
5. Explain the role of atomic number in determining the identity of
an atom.
6. Define an isotope and explain why atomic masses are not whole
numbers.
7. Calculate the number of electrons, protons, and neutrons in an
atom given its mass number and atomic number.
8. Explain the relationship between unstable nuclei and radioactive
decay.
9. Characterize alpha, beta, and gamma radiation in terms of mass
and charge.
Chapter 5: Electrons in Atoms
Vocabulary: amplitude, atomic emission spectrum, atomic orbital,
aufbau principle, electromagnetic radiation, electromagnetic
spectrum, electron configuration, electron-dot structure, energy
sublevel, frequency, ground state, Heisenberg uncertainty principle,
Hund’s rule, Pauli exclusion principle, photoelectric effect, photon,
principle energy level, principal quantum number, quantum,
quantum mechanical model, valence electron, wavelength
Problems: 1-4, 18-23, 25, 65-82
1. Compare the wave and particle model of light
2. Define quantum of energy and how it’s related to energy change
of matter
3. Contrast continuous electromagnetic spectra and atomic emission
spectra
4. Compare and contrast the Bohr model and quantum mechanical
model of the atom
5. Identify the relationships among energy levels, sublevels, and
atomic orbitals.
6. Apply the Pauli exclusion principle, the aufbau principle, and
Hund’s rule to write electron configurations using orbital diagrams
and electron configuration.
7. Define valence electrons and draw electron-dot structures
representing an atom’s valence electrons.
Chapter 6: The Periodic Table and Periodic Law
Vocabulary: periodic law, group, period, representative element,
transition element, metal, alkali metal, alkaline earth metal, transition
metal, inner transition metal, nonmetal, halogen, noble gas,
metalloid, ion, ionization energy, octet rule, electronegativity
1. Trace the development and identify key features of the periodic
table
2. Explain why elements in the same group have similar properties.
3. Identify the four blocks of the periodic table based on electron
configuration.
4. Compare period and group trends of several properties.
5. Relate period and group trends in atomic radii to electron
configuration.
Chapter 8: Ionic Compounds
Vocabulary: alloy, anion, cation, chemical bond, delocalized
electrons, electrolyte, electron sea model, formula unit, ionic bond,
lattice energy, metallic bond, monatomic ion, oxidation number,
oxyanion, polyatomic ion
Problems: 19-23, 74-78
1. Define chemical bond.
2. Relate chemical bond formation to electron configuration.
3. Describe the formation of positive and negative ions
4. Describe the formation of ionic bonds.
5. Account for many of the physical properties of an ionic
compound.
6. Write formulas for ionic compounds and oxyanions.
7. Name ionic compounds and oxyanions.
8. Describe a metallic bond and explain the physical properties of
metals in terms of metallic bonds.
9. Define and describe alloys.
Chapter 9: Covalent Bonding
Vocabulary: coordinate covalent bond, covalent bond, Lewis
structure, molecule, oxyacid, polar covalent bond, resonance,
structural formula, VESPR model, Table 9-3 (Geometries)
Experiment 14: Model Building
Problems: 94-114
1. Apply the octet rule to atoms that bond covalently
2. Describe the formation of single, double, and triple covalent bonds
3. Identify the names of binary molecular compounds from their
formulas
4. Name acidic solutions
5. List steps used in drawing Lewis structures
6. Explain why resonance occurs and identify resonance structures
7. Explain and identify exceptions to the octet rule
8. Discuss the VESPR bonding theory
9. Predict the shape of and the bonding angles in a molecule
10. Describe how electronegativity is used to describe bond type
11. Compare and contrast polar and nonpolar covalent bonds and
molecules
12. Describe the characteristics of compounds that are covalently
bonded
Chapter 10: Chemical Reactions
Vocabulary: aqueous solution, chemical equations, chemical
reaction, coefficient, combustion reaction, decomposition reaction,
double-replacement reaction, precipitate, product, reactant, singlereplacement reaction, solute, solvent, synthesis reaction
Experiment 8: Precipitation Reactions
Problems: 71-94
1. Recognize evidence of chemical change.
2. Represent chemical reactions with balanced equations.
3. Classify chemical reactions.
4. Identify the characteristics of different classes of chemical
reactions.
5. Describe an aqueous solution.
6. Predict what reactions in aqueous solutions will produce.
Chapter 11: The Mole
Vocabulary: mole, Avogadro’s number, molar mass, molecular
formula, percent composition, empirical formula, dimensional
analysis
Experiment 7: Determination of the Empirical Formula for
Manganese Chloride
Problems: 89-150
1. Describe how a mole is used in chemistry.
2. Relate a mole to common counting units.
3. Convert moles to number of representative particles and number
of representative particles to moles.
4. Relate the mass of an atom to the mass of a mole of atoms.
5. Calculate the number of moles in a given mass of an element and
the mass of a given number of moles of an element.
6. Calculate the number of moles of an element when given the
number of atoms of the element.
7. Recognize the mole relationships shown by a chemical formula.
8. Calculate the molar mass of a compound.
9. Calculate the number of moles of a compound from a given mass
of the compound, and the mass of a compound from a given number
of moles of the compound.
10. Determine the number of atoms or ions in a mass of a
compound.
11. Explain what is meant by the percent composition of a
compound.
12. Determine the empirical and molecular formulas for a compound
from mass percent and actual mass data.
Chapter 12: Stoichiometry
Vocabulary: actual yield, excess reactant, limiting reactant, mole
ratio, molar volume, percent yield, stoichiometry, theoretical yield,
percent yield
Problems: See Worksheets and 61-90
1. Identify the quantitative relationships in a balanced chemical
equation.
2. Determine the mole ratios from a balanced chemical equation.
3. Explain the sequence of steps used in solving stoichiometric
problems.
4. Use the steps to solve stoichiometric problems.
5. Identify the limiting reactant in a chemical equation.
6. Identify the excess reactant and calculate the amount remaining
after.
7. Calculate mass of product when amounts of more than one
reactant are given.
8. Calculate the theoretical yield of a chemical reaction from data.
9. Determine the percent yield for a chemical reaction.