Download Chemistry I – Semester I Final Review

Chemistry I PAP (2010) – Semester I Final Review
All students will complete a semester exam review regardless of exemption status. The student
should be able to do the following:
Chapter 1 (Matter) & 2 (Measurements)
- interpret a correctly made graph from laboratory data
- list and define common metric base units and prefixes
- construct conversion factors from equivalent measurements and apply techniques of
dimensional analysis (factor-label method) in problem solving
- report measurements to the correct number of significant digits
- express large and small numbers in scientific and standard notation
- demonstrate safe laboratory procedures and attire
- identify common laboratory equipment and know their uses
- classify a sample of matter as an element, compound, or mixture (homogeneous vs.
heterogeneous)
- classify properties as either physical or chemical (physical: color, odor, shape, mass
solubility, malleability, ductility, melting and boiling points, density, conductivity,
chemical reactivity, flammability)
- distinguish between physical and chemical changes (states) and know the three states of
matter
- Practice: Sketch the tree map on page 15
- p. 18 2
p. 24 3
p. 42 2,3,5
p. 57 2,3,4,6,7,8
VOCAB: chemical and physical change, homogeneous and heterogeneous mixtures, compound, element
Chapter 3 (Atoms)
Define and apply the Law of Conservation of Mass
- define atom, nucleus, electron, neutron, isotope, proton (including relative size and
charge of subatomic particles, average atomic mass, cation, anion, atomic number, atomic
mass
- discuss the evolution of atomic theory to the present electron cloud model emphasizing
that the atom is mostly empty space. (Rutherford, Thompson, Bohr, quantum mechanical
model)
- use the mass number and atomic number to determine the element and its number of
protons, electrons, and neutrons
- determine the atomic number and mass number of an element when the number of
protons, neutrons, and electrons is specified
- know how isotopes of an atom differ and understand how relative abundance of isotopes
determine atomic mass
VOCAB: isotope, average atomic mass, atom, electron, nucleus, neutron, proton, isotope, cation, anion,
atomic number, atomic mass
1.
Practice Problems: p. 74 2 (a, b), 3
Additional Questions:
p. 85 1-7
Write the chemical configuration, including atomic number & mass number, for the following
isotopes.
a. carbon-14
c. nickel-63
b. chromium-53
d. zirconium-92
2.
3.
4.
5.
Complete the table for the following isotopes.
Zn
Symbol
Atomic #
20
Mass #
65
74
40
# of protons
34
# of
21
neutrons
# of
18
electrons
Calculate the average atomic mass of copper if 69.17% of the copper atoms occurring in nature
are 63Cu and 30.83% are 65Cu.
What is the charge of an ion that has 26 protons, 30 neutrons, and 24 electrons?
What is the charge of an ion that has 15 protons, 16 neutrons, and 18 electrons?
Chapter 4 (Electrons in Atoms) & 5 (Periodic Law)
- write electron configurations and orbital filling diagrams (including energy level,
sublevels, and orbitals for any element)
- recognize the difference between excited state and ground state configuration and
everyday applications (fireworks, neon light)
- understand the periodic properties due to repeating outer electron configurations and the
properties of the representative elements (s and p block)
- understand the organizing principles of the periodic table to include: atomic number,
placement of metals, non-metals, and metalloids (semi-metals), and names of and
location of groups (families) and periods
- define and describe the following trends: atomic radius, electronegativity, ionization
energy, and ionic radius
- Be able to apply the Aufbau principle, the Pauli exclusion principle, and Hund’s rule
when writing electron configuration and orbital notation
- Calculate various wave problems
- Know the mathematical relationship between wavelength and frequency
VOCAB: ground state, electron configuration, quantum numbers, orbital filling diagrams, dot
diagram, valence electrons, energy level
- Practice Problems: p. 104 1,3 p. 116 3-5
p.118 8
p.154 1
- Additional Questions
-
Calculate the wavelength if the frequency is 2.5 x 10 5 Hz.
Find the energy of a photon if frequency is 7.31 x 10 14 Hz.
Fill in the table for the following elements.
Electron configuration
Symbol Atomic # Orbital Diagram
Quantum numbers
F
V
Chapter 7 (Formulas and Compounds)
-
convert between moles, mass, and number of particles given a chemical formula
calculate empirical and molecular formulas
solve hydrate problems
determine the percent composition of a substance
use cations and anions to write chemical formulas
given the formula for a compound, write its name
interpret the information conveyed in a chemical formula
determine the formula / molecular mass of a substance
VOCAB: moles, atoms, molecule, formula unit, empirical and molecular formulas, percent composition,
alkanes, alkenes, alkynes, hydrocarbons, alcohols, acids, hydrates
-
Practice Problems: p. 215 2-4
p.219 1,2
p. 228 3,5,6
p.233 1-5
Dot
diagram
-
P.237 35, 42
Additional Questions
1. Draw the structural formula of 2,2-dimethyl octane.
2. Write formulas for the following compounds (HINT: First determine ionic/acid/covalent).
a. calcium bromide
d. octane
b. iron(III) sulfate
e. dinitrogen tetroxide
c. hydrofluoric acid
f. sulfurous acid
Chapter 8 (Rxns)
- identify the reactants and products in a chemical equation and the following symbols
used in equation writing – s, l, g, aq, , 
- Understand and apply the activity series in predicting reactions
- write a balanced equation and predict the products when given names of formulas of all
products and reactants in a chemical reaction
- classify reactions as double replacement (ionic), single replacement, synthesis
(combination / composition), decomposition (analysis), and combustion.
- Define the terms precipitate, activity series, exothermic, and endothermic, and identify a
reaction as to the change in energy involved
- Practice Problems: 264 2-4