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Chapter 1 – Introduction: Matter & Measurements. Learning Targets • Distinguish between chemical and physical changes and properties. • Know the states of matter and characteristics of each. • Understand the difference between elements, molecules, compounds, and mixtures.
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Chapter 1 – Introduction: Matter & Measurements Learning Targets• Distinguish between chemical and physical changes and properties. • Know the states of matter and characteristics of each. • Understand the difference between elements, molecules, compounds, and mixtures. • Know the various techniques for separating the components of a mixture, and the principle upon which each of these operates. • Be familiar with the units of the metric system and the temperature scales. • Understand the concept of density and be able to answer all questions, both conceptual and mathematical, related to density. • Be able to convert measurements, especially within the metric system, by using dimensional analysis. • Determine the number of significant figures in a measurement and be able to express the results of a calculation with the proper number of significant figures.
Chapter 2 – Atoms, Molecules, and Ions Learning Targets• Understand the atomic theory, and how it relates to theories of chemistry. • Distinguish between protons, neutrons, and electrons, and be able to describe the composition of an atom of any particular element in terms of these subatomic particles. • Understand the difference between isotopes, as well as the two types of notations used with them. • Be aware of who discovered each subatomic particle and have an idea of how they did it. • Know the difference between an atom, and ion, and a molecule. • Have a basic knowledge of the periodic table, which includes being able to predict whether an element is a metal or a nonmetal, and what will be the probable charge of its ion • Know that the given atomic mass of an element is the weighted average of the atomic masses of all isotopes of that element. Be able to perform all related calculation. • Be able to give the name and/or formula for any given compound.
Key Words – Chapter 1 • Matter • Molecule • Distillation • Pure substance • Compound • Solution • Physical properties • Intensive properties • Physical change • Density • Atom • Filtration • Chromatography • Element • Mixture • Chemical properties • Extensive properties • Chemical change • Significant Figures
Key Words – Chapter 2 • Atom • Ion • Proton • Neutron • Electron • Atomic number • Nuclide • Group • Period • Anion • Molecule • Isotope • Mass Number • Atomic Weight • Metal • Nonmetal • Metalloid • Molecular Formula • Empirical Formula • Cation
Section 1: Separation TechniquesPages 11-12 RBQs # 15,16,78,79 • A mixture is a combination of two or more substances in which each substance retains its own chemical identity • Because they retain their chemical identities, a mixture can be separated by physical means, as opposed to a compound • Three common means of separating mixtures are filtration, distillation, and chromatography
Section 1: Separation TechniquesPages 11-12 RBQs # 15,16,78,79 • Filtration:
Section 1: Separation TechniquesPages 11-12 RBQs # 15,16,78,79 • Distillation:
Section 1: Separation TechniquesPages 11-12 RBQs # 15,16,78,79 • Paper Chromatography
Section 1: Separation TechniquesPages 11-12 RBQs # 15,16,78,79 • Gas Chromatography
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • Lab data can be either quantitative or qualitative • Qualitative: • Quantitative:
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • Quantitative data (measurements) MUST include a number and unit • The units in chemistry are called the SI Units; these are the internationally agreed upon set of units
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • The SI base units are modified using metric prefixes to make the number more manageable
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • The instruments used to make measurements have limitations which leads to estimations being made with measurements
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • When a measurement is made, all certain digits are recorded, and the final estimated digit is uncertain digit • Every measurement will contain all certain digits and one estimated uncertain digit; combined, these digits are known as the significant figures • To make sure the proper number of digits is always given, the rules of significant figures are applied to numbers and calculations
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • An important technique for problem solving is called dimensional analysis which uses conversion factors • This technique is used to convert a quantity to an equivalent quantity, but with a different unit • For example, dimensional analysis could show 3 dollars are equal to 12 quarters; same amount of money, different units
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • The first thing to know is the numerical relationship between the starting quantity and the desired quantity • For example, if the number of meters in a given number of inches is needed, one must know the number of inches in a meter (or vice versa) • There are 39.37 inches in 1 meter, and as a conversion factor, this information could be written as seen below:
Section 2: Units & Measurement Pages 13-17 RBQs # 19-25,29,30 • The conversion factor will always be a fraction, and once it is determined, the conversion factor is arranged so that the given unit is eliminated and replaced with the desired unit • For example, if the questions wants to know the number of meters in 69.5 inches:
Do This! A pencil is 7.000 in long. What is this length in cm? (1 in = 2.54 cm)
Do This! An N2 molecule moves at 515 m/s. What is this speed in mi/hr?
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • The atom is the basic building block of matter; it is defined as the smallest unit of an element that retains the properties of that element→ An atom of gold is the smallest piece of gold that is yellow and shiny→ An atom of oxygen is the smallest unit of oxygen that we can breathe • The concept of the atom has been around for thousands of years, but this idea has only been backed by scientific experimentation since the 1700’s • The atom’s existence and structure was confirmed and determined through a number of experiments by several scientists
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • All matter is composed of extremely small particles called atoms • Atoms of a given element are identical • Atoms cannot be created, destroyed, or divided • Atoms combine in whole number ratios to form compounds • In chemical reactions, atoms are separated, rearranged and combined John Dalton. Smart, but not always right.
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • J.J. Thompson did most of the heavy lifting in the discovery of electrons with the cathode ray tube
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • Ernest Rutherford was all up in the nucleus with the gold foil/alpha particle experiment
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • Another thing learned through all this research was that all atoms of a given element do not have the same mass • Isotopes are atoms of a given element that have different masses; the difference in these masses results from different numbers of neutrons • An atom of a specific isotope is called a nuclide
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • These different nuclides are detected and counted using a technique called mass spectrometry which can be used to identify unknowns and determine atomic masses
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • The result is a mass spectrum such as this:
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • The y-axis will have a scale that can be read, but let’s just let the computer give us the numbers • Based on the height of each peak, the amount of each isotope/nuclide in the sample is determined • The spectrum above shows 100 nuclides with a mass of 12 and 23 nuclides with a mass of 10
Section 3: Atomic Structure & MassPages 35-45 RBQs # 13-21,23,24 • The mass spectrum data can also be given in the form of percent abundance
Section 4: Periodic Table, Molecules, IonsPages 46-56 RBQs # 29-32,36-38,41-50 • The elements are arranged by increasing atomic number • Elements are in groups (columns) and periods (rows) • Elements are also categorized as metals, metalloid, nonmetals, and noble gases
Section 4: Periodic Table, Molecules, IonsPages 46-56 RBQs # 29-32,36-38,41-50 • The real fun starts when elements combine to form compounds • Sometimes these compounds are called molecules
Section 4: Periodic Table, Molecules, IonsPages 46-56 RBQs # 29-32,36-38,41-50 • Once metals get involved, we have ionic compounds
Section 4: Periodic Table, Molecules, IonsPages 46-56 RBQs # 29-32,36-38,41-50 • Ion charges can be predicted using the periodic table
Section 5: Chemical NomenclaturePages 56-65 RBQs # 51-66 • Determining the names and formulas of a chemical compound is kind of a big deal in chemistry • There are four types of compounds that each have their own rules when it comes to nomenclature • Ionic compounds, covalent/molecular compounds, acids, and organic compounds
Section 5: Chemical NomenclaturePages 56-65 RBQs # 51-66 • For ionic compounds, just give the name of each ion, with the cation always first • The name of monatomic cation is the same as the element • The only exception is when the monatomic cation can have multiple charges, like most transition metals
Section 5: Chemical NomenclaturePages 56-65 RBQs # 51-66 • The name of monatomic anion keeps the same base as the element , but the ending changes to –ide • The name of a polyatomic ion never changes
Section 5: Chemical NomenclaturePages 56-65 RBQs # 51-66 • Binary covalent compounds are named using prefixes to indicate the number of each element present in each molecule • The name of the compound always ends in –ide • The prefix mono- is never used with the first element