Things to Know for the Semester 1 Final Exam (Tuesday 7/17/12)
Chapters 1-10, parts of 11
• Know how to determine the number of significant figures in a measurement
• Know that when adding or subtracting measurements, the answer should have the least number of decimal places
whereas if you multiply or divide measurements, the answer should have the least number of significant figures.
• Know how to use the density equation
• Know the names and formulas of the acids from Elementary Knowledge
• Know the 7 diatomic gases from Elementary Knowledge (Hint: HOFBrINCl)
• Know your polyatomic ions (names, formulas, and charges) from Elementary Knowledge
• Know how to figure out the charge on an ion based on what group it is in on the periodic table
• Know how to figure out the name of a compound when given the name
1. Ionic compounds don’t have prefixes 2. Covalent compounds have prefixes
• Know how to get a chemical formula from the name
1. Covalent compounds have prefixes 2. Ionic compounds have charges to criss-cross
• Know the law of conservation of matter
• Know that elements in the same group have similar properties
• Know the trend for reactivity
• Know the trend for atomic size (i.e. across a period and down a group)
• Know the names and locations of these groups: alkali metals, alkaline earth metals, halogens, noble gases
• Know what determines the identity of an element
• Know what an isotope is
• Know how to write hyphen-notation for isotopes
• Know what the relative sizes and charges of the 3 subatomic particles: proton, electron, neutron
• Know how to use a periodic table to determine the # of protons an atom contains
• Know how to use a periodic table to determine the atomic mass of an atom
• Know the difference between these types of bonds: metallic, ionic, molecular covalent, & covalent network (metallic
bond)
• Know the difference between covalent bonding and ionic bonding (for example: nonmetals only versus metals bonded
to nonmetals)
• Know that electrons are shared in covalent bonds but transferred in ionic bonds
• Know which type of compound dissolves, conducts, and conducts when dissolved
• Know how to write electron configurations
• Know how to determine the # of valence electrons an atom has by looking at its electron configuration (hint: valence
electrons are the s electrons and the p electrons only.)
• Know how to determine the # of valence electrons an atom based on its group # in the periodic table
• Know how to determine how many valence electrons an atom will lose or gain to become a noble gas (ex: since calcium
is in group 2, it has 2 valence electrons. It’s easier to lose 2 than gain 6. Therefore, it will lose 2 electrons.)
• Know how to draw dot structures for single elements and for compounds
• Know the octet rule and HONC 1234 rule
• Know how to predict how many bonds an atom will form based on the HONC 1234 rule
• Know the trend for electronegativity (i.e. across a period and down a group)
• Know how to use electronegativities to determine if a bond will be polar (hint: the difference tells you if it will be
nonpolar, polar, or ionic)
• Know how to determine shape based on dot structures (VSEPR)
• Know how to determine polarity based on shape
• Know how to predict if a molecule will dissolve in water (solubility rules)
• If a molecule is polar, know how to determine which end is partially positive and which end is partially negative
• Know that nonpolar molecules have London Dispersion IMF’s, polar molecules have dipole-dipole IMFs, and
polar molecules containing H bonded to N, O, or F have hydrogen-bonding
IMFs.
• Know that intermolecular forces are just attractions to neighboring molecules and are much weaker than bonds.
Other topics that will be covered:
Physical vs. Chemical Properties and Changes
Counting Sig Figs
Scientific Notation
Using Dimensional Analysis to convert between units (especially metric units)
Determining # of protons, neutrons, electrons
Ions vs. Isotopes
Calculating Atomic Weight
Energy Levels (how many electrons in each)
Writing formulas and naming ionic, covalent, and metallic molecules
Lewis Dot Structures
Electron Geometry and Molecular Geometry (VSEPER)
Polarity
Hybridization
Intermolecular Forces: hydrogen bonds, london dispersion forces, dipole-dipole, ion-dipole, covalent network solids
Empirical and Molecular Formula
% Composition
We might get to the following (I will tell you if they will be on the test or not):
Writing and Balancing Chemical Equations
Types of Chemical Reactions and Predicting the Products
Solubility Rules
Study Questions (these will not be graded but you can use them to help study)
1. Define matter.
2. What is the density formula? What is the density of a coin with a mass of 5.5 grams and volume of 26.1 mL?
3. What lab equipment do you use to measure mass and take the volume of liquids? How do you read a meniscus and how
many sig figs do you take from instruments with different increments.
4. What would you observe at the molecular level in a sample of H2O(s), H2O(l), H2O(g)?
5. Using the periodic table, where are the metals and nonmetals? What is hydrogen?
6. Where are the alkali, alkaline earth, transition metals, halogens, and noble gases?
7. On the periodic table, what are the trends for atomic size, ionization energy, electronegativity, and ionic size?
8. a). What are valence electrons?
b). How many valence electrons do Mg, S, and Al have?
9. In ionic bonds, metals tend to lose electrons and nonmetals gain electrons. What happens to these elements to achieve
noble electron configuration?
a). oxygen b). chlorine c). sodium d). barium
10. What is the chemical formula of the compound formed when beryllium reacts with fluorine? When potassium reacts
with sulfur?
12. What is the HONC1234 rule? Draw the Lewis Dot structures for the following molecules. a). OCl2 b). SiI4
13. What is the difference between lone pairs and bonded pairs? How many lone pairs and bonded pairs are on the
molecules in question 12?
14. Write the molecular formula, structural formula, Lewis Dot structure, and ball-and-stick formula for water.
15. What is electronegativity? Where are the most and least electronegative elements?
16. How does the electronegativity differences determine nonpolar covalent, polar covalent, and ionic bonds? What are
happening to the electrons in these different bonds?
17. What are the chemical formula of the following polyatomic ions and their charges? a). sulfate b) sulfite c) hydroxide
d) nitrate e) nitrite
18. Answer the following questions about a mole.
a. How many atoms are in 1 mole of Cu, copper?
b. How many molecules are in 0.5 mole of H2O, water?
19. What is the molar mass of Al2(SO4)3?
20. Answer the following questions about the relationship between mole and mass.
a. How many moles are in 2.5 grams of H2O, water?
b. How many grams are 0.75 moles of H2O, water?
21. Use the following combustion reaction with propane, C3H8, to answer the following stoichiometry questions.
C3H8+ 5O2 → 3 CO2 + 4H2O
22. How many moles of O2, oxygen, will produce 2.5 moles of H2O, water?
23. How many grams of O2, oxygen, will be needed to react 1.50 moles of C3H8, propane?
24. How many moles of H2O, water, will be produced if there is 25.0 grams of CO2, carbon dioxide gas?
25. How many grams of C3H8, propane, are needed to produce 175 grams of CO2, carbon dioxide gas?