Download Study Guide – Honors Chemistry: Exam One

Study Guide – Honors Chemistry: Final
Matter:
 Different states of matter and key characteristics
 Mixtures – composition may vary
o Heterogeneous
o Homogeneous
 Pure substances
o Elements
o Compounds – fixed or constant composition
 Density calculations
 Chemical vs. physical properties
 Chemical vs. physical changes
Temperature:
 Celsius to Kelvin and back
 Roughly boiling and freezing points of water
 Definition of absolute zero
 SI unit is Kelvin
Experimental definitions:
 Hypothesis
 Theory
 Control
 Variables
Accuracy and precision
SI units and simple conversions with standard units, units2, and units 3
Given conversion factors, be able to convert from English to metric units.
Sig figs – know how to calculate/determine
 Rules for significant zeros
 Rules for calculations
o Addition and subtraction
o Multiple and division
Atoms –
 Atomic structure
o Neutrons
o Protons
o Electrons
 Relation to atomic number and weight
 Dalton’s atomic theory
Chapter 2 (2.7 & 2.8), Chapter 7 (7.1, 7.3, 7.5, & 7.6), Chapter 8 (8.1, 8.2, 8.3 & 8.5)
Section 2.7:
Be able to predict whether an element will form an anion or a cation and what the
oxidation state of the ion will be.
Predict the ionic charge (oxidation state) of each of the following elements and write the
element symbol with the correct format to indicate its charge:
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Sodium
Aluminum
Phosphorus
Calcium
Bromine
Selenium
Based on ionic charge, be able to predict the ratio with which anions and cations will
combine to form a compound.
Predict the formula for the following ionic compounds (use your book to remind yourself
of some of the polyatomic ions – you will be given a list of names and formulas for
polyatomic ions on the exam):
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Calcium oxide
Potassium oxide
Aluminum oxide
Magnesium chloride
Potassium iodide
Strontium nitrate
Lithium sulfate
Nitrogen trihydride
Name the following ions:
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Fe(NO3)2
NH4Cl
Ca(Br)2
Al2S3
Chapter 7:
How was the original periodic table devised?
How is the modern periodic table organized?
What is true about elements in the same group?
In general, what happens to the size of atoms as measured by atomic radii as you go
down a group? Across a period?
What happens to the size of ions as you go down a group? Or across a period? How does
the size of cations in a period compare to the anions in a period?
What is electron affinity and how does it change in general across a period and up or
down a group?
How does electron affinity compare to electronegativity? What is the most
electronegative element in the periodic table?
What are some general characteristics of metals? Which are the most metallic element(s)
in the periodic table? How does the electron affinity of a metal account for many or all of
its properties?
What are some general characteristics of nonmetals?
How do you explain the metalloids? List the main metalloids.
Chapter 8:
Be able to distinguish among the three main types of bonds – what is different about each
of them??
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Ionic –
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Covalent –
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Metallic –
Be able to draw Lewis dots structures of individual atoms, individual ions, and
compounds (both ionic and molecular).
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Ca and Ca2+
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CaCl2
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CH4
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C2I2
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MgO
General concepts to review Atomic Structure - history of the development of the modern atomic theory
 protons
 neutrons
 electrons
Basic principles of chemical bonding  atomic stability in terms of electron configuration
 nobel gas structures
 ionic vs. covalent bonding
 predicting ionic formulas based on ionic charges
Periodic trends  metals vs. nonmetals
 atomic size
 ionic radii
 electronegativity
 reactivity
 similar properties by group
Balancing equations - law of conservation of mass
Stoichiometry - using balanced equations to determine proportions and yield Limiting reactions -
Math concepts to review Metric conversions - including conversions with units squared or cubed - be able
to convert given English units to metric
Significant figures - rules for determining with addition/subtraction and
multiplication/division - purpose of significant figures
Balancing chemical equations
Moles to grams to moles to number of particles (Avogadro’s number) Stoichiometry with balanced equations
Theoretical yield vs. percent yield
Limiting reactants