Download 1st Semester Review

1st Semester Review
Chemistry I
Chapter 1: The Science of Chemistry
Suggested Review Problems - #35, 46, 47, 52, 53, 54, 57, 73
1.1 What Chemistry is About

Measurements & Units: Mass & weight; 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

1.2 Scientific Inquiry (cont.)

repeatable

procedure

scientific method
1.3 Matter and Energy

matter def
o phases of matter

energy def
o Law of Conservation of Energy
Chapter 2: Matter and Atoms
Suggested Review Problems - #32, 39, 44, 58, 64, 66, 67, 70-73, 75
2.1 Matter and the Elements

substance vs. mixture
o element

physical properties & physical change

chemical properties & chemical change
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Periodic Table

mole
o Avogadro's number
o calculations
2.2 Molecules and Compounds

defs

chemical formula

molecular compound
2.2 Molecules and Compounds (cont.)

ionic compound

formula mass
2.3 Mixtures and Solutions

homogeneous vs. heterogeneous

solution
o solute
o solvent
o 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
Suggested Review Problems - #23, 28, 32, 38
5.1 The Atom Has a Structure

Historical development of atomic theory
o Democritus, Dalton, Thomson, Rutherford
5.1 The Atom Has a Structure (cont.)

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
Chapter 8: Compounds & Molecules
Suggested Review Problems - #s 22, 24, 26, 27, 28, 30, 37, 38, 48, 51
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

NAMING:
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
8.2 Covalent Compounds (cont.)

Network covalent

Formulas
- empirical formula
- molecular formula

NAMING:
o binary covalent compounds, prefixes
8.4 Formula Masses

calculation of molar mass

Percent Composition: formula

Calculating Empirical Formulas

Calculating Molecular Formulas
Chapter 4: Physical and Chemical Change
Suggested Review Problems - #39, 42, 45-47, 50, 56, 57, 59, 61, 70
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
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precipitate

salt

precipitation reaction

redox reaction

acid-base reaction
Chapter 13 = Acids & Bases
Review Problems - #s 21, 23, 24, 27, 29, 30, 31, 32, 35, 40, 44, 52, 58, 60
13.1 The Chemical Nature of Acids & Bases
- neutral
- acid
- base

The importance of the H+ ion
- Arrhenius theory
- hydronium ion
13.1 The Chemical Nature of Acids & Bases (cont.)

Brønsted-Lowry definition
- acid
- base
-amphoteric

Brønsted-Lowry: acid-base pairs

Identifying acids/bases: acids have leading "H", strong bases have "OH"
- strong
- weak
13.2 The pH Scale: acids-pH<7, neutral-pH = 7, bases-pH>7
-logarithm

Definition of pH

Calculating pH for acids

Calculating pH for bases

pH indicators
- indicator =