Chemistry I Mid-Term
Review and Study Guide
The following guide is intended to be a study aid for the upcoming mid-term
exam in Chemistry. If you work to know the topic areas listed below you
will be well prepared for this test. The majority of the exam will cover the
topics listed below, although all information we went over in class may
potentially be on the test. I advise that you structure your study time to
focus on the points in this outline, but reserve some time to review all the
material we covered. Good luck with your studies!
Know the definitions of:
Chapters 1 & 2 -Intro/FOS/Co review
Scientific Method
Hypothesis
Experiment
Theory
Law
Independent Variable
Dependent Variable
Scientific Notation
Significant Figures
Accuracy
Precision
Certainty
Unit Analysis
Conversion Factor
Law of Definite Proportions
Chapter 12.1 - KMT
Kinetic Theory of Matter
Phase Diagram
Melting/Freezing
Vaporization/Condensation
Sublimation/Deposition
Pressure
Barometer
Vapor Pressure
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Chapter 3 - Matter
Substance
Matter
Element
Compound
Physical Property
Extensive Property
Intensive Property
Chemical Property
States of Matter
Solid
Liquid
Gas
Vapor
Physical Change
Chemical Change
Law of Conservation of Mass
Density
Chapter 13.1 - Gas Laws
Boyle’s Law
Charles’s Law
Gay-Lussac’s Law
Combined Gas Law
Chemistry I Mid-Term
Review and Study Guide
Know:
 Components of the scientific method: observation, hypothesis,
experiment, conclusion.
 Determine precision and certainty (Percent error); I’ll give you the
formula of
Experimental Value - Accepted value
Accepted value
x 100 = % Error







Apply the law of Conservation of Mass
Apply the law of Definite Proportions
Density is mass/volume
Use the Gas Laws (Boyle, Charles, Gay-Lussac, Combined).
Convert units of pressure and temperature.
Apply the law of conservation of mass
How to add, subtract, multiply, divide numbers and get proper number
of significant figures.
 Dimensional analysis to solve problems.
Know the Definitions of:
Dalton’s Atomic Theory
Nucleus
Proton
Neutron
Electron
Chapters 4 - The Atom
Atomic Number
Isotope
Mass Number
Atomic Mass Unit (amu)
Atomic Mass
Chapter 5 - Electrons of Atom
Electromagnetic Radiation
Quantum Mechanical Model of atom
Atomic Orbital
Wavelength (λ)
Principal Quantum Number
Frequency (ν)
Amplitude
Principal Energy Level
Electromagnetic Spectrum
Energy Sublevel
Quantum
Electron Configuration
Photoelectric Effect
Aufbau Principle
Photon
Pauli Exclusion Principle
Atomic Emission Spectrum
Hund’s Rule
Ground State
Valence Electron
Electron (Lewis) Dot Structure
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Chemistry I Mid-Term
Review and Study Guide
Know also:
 Dalton’s Atomic Theory
 Charge on a Proton, Neutron, and Electron
 What makes up the nucleus
 Rutherford’s Experiment and what that showed about the nucleus
 Atomic Number = Number of Protons = Number of Electrons
 Mass number = Number of Protons + Number of Neutrons; know how
to find any one given the other two.
 What shorthand notation means. i.e. C-14 means Carbon has 14
protons + neutrons, Carbon (C) is element #6 so it has 6 protons.
C-14 than has 8 neutrons.
 Know how to calculate the atomic mass of an element given the mass
and the abundance of the isotopes.
 Energy of a EM radiation is proportional to its frequency
 The atomic orbitals (s, p, d, f)
 How to fill the atomic orbitals of a given element
 Number of orbitals in an energy level, n. (# orbitals = n2)
 Number of electrons in an energy level, n (#electrons = 2n2)
 Electron orbital notation. Ex. B = 1s22s22p1
 Orbital Box Diagram. Example: Carbon
o
1s
2s
2p
↑↓
↑↓
↑
↑
 How to spot violations of Aufbau, Hund’s rule, and the Pauli
Exclusion Principle
Know Definitions of:
Chapter 6 - Periodic Trends
Periodic Law
Transition element/metal
Group, Family, Column
Metal
Period
Alkali Metal
Representative Element
Alkaline Earth Metal
Inner Transition Metal
Nonmetal
Halogen
Noble Gas
Metalloid
Ion
Ionization Energy
Octet Rule
Electronegativity
Metallic Character
Z* (Zeff) = Z - S
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Chemistry I Mid-Term
Review and Study Guide
Know also:
 The classification of an element (metal, nonmetal, metalloid)
 How to locate an element by period, group, and block
 Whether the element is a representative element or a transition
element
 Trends of Zeff, atomic radius, ionic radius, ionization energy, metallic
character and electronegativity as you move across and down the
periodic table.
 Size relationship between a neutral atom its corresponding ion
Know the definitions of:
Chapter 7 – Ionic Compounds and Metals
Binary compound
Oxidation number
Chemical Bond
Polyatomic ion
Cation
Electron sea model
Anion
Delocalized electrons
Ionic bond
Metallic bond
Lattice Energy
Alloy
Formula unit
Interstitial alloy
Monoatomic Ion
Substitutional alloy
Multivalent Metal
Hydrate
Know how to:
 Make a compound neutral when you have positive and negative ions.
 Show that column (group) of the element effects its oxidation number.
 Explain that lattice energy is affected by ion size and charge
 Read the ion chart to identify elemental ions like oxide (O2-) and
polyatomic ions like carbonate (CO32-)
 Write out a formula from the name of the compound (Ex. potassium
nitrate is KNO3), and what to do when you have a transition element
(Ex. Cobalt(II) chloride is CoCl2) and a hydrated compound (Ex.
Barium iodide dihydrate is BaI2•2H2O).
 Write out a name when you have a formula. Ex. PbSO4 is lead(II)
sulfate. Same ideas as previous bullet point, just in reverse.
 Metallic bonding is the metal ions in a “sea of electrons”
 Note: You do NOT have to know the nomenclature rules for the
oxyanions
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Chemistry I Mid-Term
Review and Study Guide
Chapter 8 – Covalent Bonding
Covalent Bond
Bond dissociation energy
Molecule
Lone pair electrons
Lewis structure
Allotrope
Sigma (σ) bond
VSEPR Theory
Pi (π) bond
Tetrahedral shape
Endothermic
Linear
Exothermic
Trigonal planar
Structural formula
Trigonal bipyramidal
Polar covalent bond
Octahedral
Electronegativity
Pyramidal
2
3
Hybridization (sp, sp , sp )
Bent
Know how to:
 Name a molecular compound. (Ex. N2O5 is dinitrogen pentoxide)
 Write out a formula for a covalent compound if given the name.
 Identify simple common acids or bases (H3PO4 is phosphoric acid,
HCl is hydrochloric acid, etc.)
 Distinguish between an ionic compound and a covalent molecule.
 Draw Lewis structures of simple compounds and ions, be able to label
bonding electrons and lone pair electrons
 Determine type of bond between the two elements based on their
electronegativity difference
 Qualitatively determine how number of bonds and bond length affects
bond strength (i.e. double bonds are shorter and take more energy to
break them than single bonds)
 Shapes of simple molecules: Linear, trigonal, tetrahedral, etc.
 Relate shape of molecule to hybridization (Google Classroom
assignment)
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Chemistry I Mid-Term
Review and Study Guide
Remember for the mid-term, I will give you a booklet of:
 a periodic table
 a table of electronegativities
 a table of conversion factors
 an electromagnetic spectrum
 a list of equations and constants (Including the gas laws)
 maximum number of electrons an orbital holds (s=2; p=6; d=10;
f=14), block and dot structure periodic tables
 a list of ions with their respective charges
 a list of the hydrate/covalent compound prefixes
 a list of some common transition metals
It is your responsibility to know how to use them.
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