





Volume; Density; Pressure
Accuracy & precision
Significant figures
Scientific notation
Dimensional analysis
1.2 Scientific Inquiry

natural laws

inquiry

theory

hypothesis

experiment

variable

experimental variable

control variables

error

average

conclusion

significant difference

objective

repeatable

procedure

scientific method
1.3 Matter and Energy
matter def o
energy def o
phases
1 st Semester Review
Chemistry I
Chapter 1: The Science of Chemistry
1.1 What Chemistry is About

Measurements & Units: Mass & weight;
Law of Conservation of Energy
Chapter 2: Matter and Atoms
2.1 Matter and the Elements

substance vs. mixture o element

physical properties & physical change

chemical properties & chemical change

Periodic Table

mole o Avogadro's number o calculations
2.2 Molecules and Compounds





defs
chemical formula
molecular compound
ionic compound
formula mass
2.3 Mixtures and Solutions



homogeneous vs. heterogeneous
solution o o o
solute
solvent
dissolved
concentration o concentrated vs. dilute o solubility o molarity o calculations
 percent by mass
 molarity

mixtures of gases o molar volume o STP

Chapter 5: The Structure of the Atom
5.1 The Atom Has a Structure

Historical development of atomic theory o Democritus, Dalton, Thomson,
Rutherford

atom interior o nucleus o electron cloud o properties of subatomic particles

atomic number, atomic mass o isotope o average atomic mass

ions
5.2 The Quantum Atom

quantum theory o quantum state o 5 statements

waves & particles o frequency o wavelength o photon o Planck's constant o relationship btwn frequency & wavelength, energy & frequency; wavelength & energy

electrons as waves o allowed wavelengths

orbitals

energy levels o Pauli exclusion principle

Periodic Table & energy levels
5.3 Electron Configurations

def

writing electron configurations
5.4 Light and Spectroscopy

spectrum

spectrometer

electromagnetic spectrum

interactions between light and matter o emission spectrum o absorption spectrum
Ch 20: Radioactivity
20.1 Nuclear Equations

atomic number (Z)

mass number (A)

neutron number (N)

chemical reactions vs. nuclear reactions
20.2 Nuclear Reactions

nuclear reactions-def

radioactivity-def

radiation

alpha decay o alpha radiation = alpha particle o parent nuclide o daughter nuclide

beta decay o beta radiation = beta particle

gamma decay

positron emission o positron

Chapter 6: Elements and the Periodic Table
6.1 The Periodic Table

periodic properties

Mendeleev

atomic level periodic properties o atomic radius o electronegativity o ionization energy

historical development

orbitals & atomic radius
6.2 Properties of Groups of Elements

alkali metals

alkaline earth metals

transition metals

C, N & O

halogens

noble gases

why compounds form: filled vs. partially filled energy levels
6.3 Valence

valence electrons

determining valence electrons

main group elements

Lewis dot diagram
Chapter 4: Physical and Chemical Change
4.1 Understanding Chemical Changes
 def
 irreversible
 interatomic forces vs intermolecular forces
 chemical bonds o covalent bond – molecule o ionic bonds
 enthalpy of formation
 reactivity
4.2 Chemical Reactions
 chemical reaction
 reactants & products
 balance equation
 coefficient
 endothermic vs. exothermic o activation energy
4.3 Chemical Reactions in the Lab
 symbols for states of matter
 precipitate
 salt
 oxidation vs. reduction
 acid-base reaction o pH scale

Chapter 7: Bonding
7.1 What is a Chemical Bond?
- polarization

Forming Bonds: overlapping orbitals, attractive force, equilibrium distance, two bond types

Bond Models & Diagrams

Predicting Bond Type: electronegativity difference
- electronegativity
- ionization energy

Covalent Bonds:
- covalent bond
- nonpolar covalent
polar covalent

Ionic & Metallic Bonds: ionic crystals
-ionic bond
-metallic bond

Polar Molecules: polarity & physical properties
7.2 Valence Electrons & Bonding Patterns

Bonding: unpaired valence electrons form bonds

The Octet Rule
-octet rule

Valence electrons & Ion Formation: ion patterns

Electron Configuration of Ions – same as noble gases

Simple Ionic Formulas – formulas must be neutral

Covalent Bonds
– number of covalent bonds possible = number of unpaired electrons
7.3 Molecular Geometry & Lewis Structures

drawing Lewis dot diagrams
- isomer

Double & Triple bonds

Molecular Geometry
- VSEPR
- region of electron density
Review Problems - #s 21, 22, 26, 29, 30, 31,
33, 34

Chapter 8: Compounds & Molecules
8.1 Ionic Compounds

Properties

charges cancel

Polyatomic ions

Writing Formulas: total positive charge must balance total negative charge

Formulas with Polyatomic ions: use parentheses

Names: o binary ionic compounds o compounds with polyatomic ions o compounds with transition metals
8.2 Covalent Compounds

Properties
- molecule

Small molecules

Medium-sized molecules
- lipid
- steroid
- hydrocarbon

Polymers
- polymer
- monomer
- homopolymer
- copolymer

Network covalent

Formulas
- empirical formula
- molecular formula

Naming: o binary covalent compounds, prefixes
8.3 Intermolecular Forces
- intermolecular forces
- van der Waals attractions

Dipole-dipole attractions
- dipole-dipole attractions
- hydrogen bonding
-surface tension (p. 247 & 264)

Water - special properties

London dispersion attraction: o factors that affect London dispersion attraction
- London dispersion attraction
8.4 Formula Masses

calculation of molar mass

Percent Composition: formula

Calculating Empirical Formulas

Calculating Molecular Formulas
Review Problems - #s 22, 24, 26, 27, 28, 30,
37, 38, 39, 42, 45, 46, 47, 48, 51
Ch 17: Organic Chemistry
17.1 Carbon Molecules

saturated

unsaturated

alkane o parent compound o R group

structural isomer

alkene

alkyne
17.2 Functional Groups

alcohol

ether

aldehyde

ketone

carboxylic acid

amine

ester