General Chemistry Midterm Review

100 Multiple choice problems

1 problem sheet (e configuration, lewis dot structures, molar mass etc.)

You may use a 3”x5” notecard on your exam provided that notecard is turned in prior to the end of class on the Monday before exams start.

Major topics covered

Unit 1 Introduction

Theory

Law

Scientific Method

Lab safety

Sig figs

Dimensional analysis (field goals)

Metric system

Density

Unit 2 Atomic theory

Subatomic particles

Proton

Neutrons

Electrons

Nucleus

Rutherford

Thomson

Bohr

Heisenberg

Orbitals

Energy levels

Electron configuration

Quantum numbers

Unit 3 Periodic Table

Elements

Compounds

Mixture

Homogeneous/heterogeneous

Periodic Table

Periodic trends

Metals

Nonmetals

Metalloids

Alkali metals

Alkaline Earth Metals

Transition metals

Halogens

Noble gases

Mole

Molar Mass

Mole gram conversion

Mole atom conversion

Unit 4 Nomenclature

Ions

Cations

Anions

Ionic bonding

Polyatomic ions

Naming ionic compounds

Determining ionic formulas

Ionic dissociation

Molar mass

Covalent Naming

Covalent Prefixes

Naming Acids

Unit 5 Chemical Reactions

Products

Reactants

Energy

Exothermic

Endothermic

Balancing Equations

Preciptiate

Redox reaction

Combustion Reaction

Single Replacement Reaction

Double Replacement reaction

Synthesis Reaction

Double Replacement Reaction

Spectator Ions

Acid Base Reactions

Unit 5 Chemical Bonding

Covalent bonding

Electronegativity

Polar Covalent Bond

Nonpolar covalent bond

Determining the type of bond

Lewis dot structures

Practice problems

Draw the orbital diagram, electron configuration for the following elements, draw the electron configuration and condensed electron configuration (circle electron w/ given quantum numbers, and circle your own)

W- 3, 2,1,+½ S- 2, 1, 0, –½

Rb- 3, 2, 2, +½ Cu 2,1,-1 –½

Element / Symbol / Atomic number / Mass Number / protons / neutrons / electrons
Zirconium / 40 / 51
Bromine / 80 / 35
Magnesium / 12 / 24
Silicon / 14 / 14
Ion / Symbol / Atomic number / Mass Number / protons / neutrons / electrons
Iron (II) / Fe2+ / 26 / 56
Chloride / Cl- / 17 / 36
Calcium / Ca2+ / 20 / 41


Determine the formula of the following compounds.

Potassium sulfide

Magnesium chlorate

Ammonium iodide

Equations

Balance the following equations

CaCl2 + NaOH ® Ca(OH)2 + NaCl

Na3PO4 + Sr(NO3)2 ® NaNO3 + Sr3(PO4)2

Li3PO4 + NH4F ® LiF + (NH4)3PO4

Mole Problems

How many moles are in 320 g of ammonium carbonate?

How many grams are in 5.23 mol of C3H8?

How many grams are in 5.1 mol of sulfur hexachloride?

How many moles are in 12.5 g of Nitrogen trichloride?

Empirical formulas and percent composition

Determine the percent composition of Li3BO3

Determine the percent composition of C2H5OH

What is the empirical formula of something that is 11.6% N and 88.4% Cl

What is the empirical formula of something that is 35.9 % Al and 64.1 % S

Name the compound, draw the Lewis dot structures for the following compounds and determine the shape.

Mg(NO2)2

NH4OH

NI3

C2H3F

SiO2

CaF2