Solution Manual for Chemistry The Central Science 13th Edition by Theodore E. Brown

Solution Manual for Chemistry The Central Science 13th Edition by Theodore E. Brown , H. Eugene LeMay, Bruce E. Bursten

ISBN-10 ‏ : ‎ 0321910419, ISBN-13 ‏ : ‎ 978-0321910417

Chapter 1. Introduction: Matter and Measurement
Common Student Misconceptions
• Students often confuse mass and weight.
• Students have difficulty with algebraic manipulation. Conversion of temperatures between Celsius
and Fahrenheit scales is particularly problematic.
• Students tend to equate density with mass.
• Students often either are unfamiliar with the prefixes used in the metric system or cannot use them
properly (e.g., 1 pm = 1  10–12 m  1 m = 1  1012 pm).
• Students often use precision and accuracy interchangeably.
• Students often do not appreciate that in chemistry, measurement yields numbers determined with
certain precision and in certain units; both depend on the type of measuring device.
• Students often cannot find exact numbers in calculations.
• Students confuse significant figures and decimal places in arithmetic manipulations.
• Students often either round off too soon in calculations, or they report the result to as many figures as
their calculators produce.
• Some students do not understand the use of a conversion factor of exactly one.
• In dimensional analysis problems, students do not see that a physical quantity is a multiplication of
value and units. Therefore, they do not perform algebraic operations on both the number and units.
Teaching Tips
• Many students have problems using dimensional analysis (“from physics”) in chemistry. This text
bases the whole of stoichiometry on dimensional analysis: students should be encouraged to embrace
the concept as soon as possible.
• Emphasize the importance of quickly mastering the use of common metric prefixes and scientific
notation.
• Conversion involving commonly encountered metric prefixes needs frequent reinforcement; for
example, 106
µg = 103
mg = 1 g = 10–3 kg.
Lecture Outline
1.1 The Study of Chemistry
• Chemistry:
• is the study of properties of materials and changes that they undergo.
• can be applied to all aspects of life (e.g., development of pharmaceuticals, leaf color change
in fall, etc.).
The Atomic and Molecular Perspective of Chemistry1,2,3,4,5,6,7
Chemistry involves the study of the properties and the behavior of matter.
1
“The First Demonstration: Proof that Air is a Substance” from Live Demonstrations
2
“Oxygen” 3-D Model from Instructor’s Resource CD/DVD
3
“Water” 3-D Model from Instructor’s Resource CD/DVD
4
“Carbon Dioxide” 3-D Model from Instructor’s Resource CD/DVD
5
“Ethanol” 3-D Model from Instructor’s Resource CD/DVD
6
“Ethylene Glycol” 3-D Model from Instructor’s Resource CD/DVD
7
“Aspirin” 3-D Model from Instructor’s Resource CD/DVD
Introduction: Matter and Measurement
• Matter:
• is the physical material of the universe.
• has mass.
• occupies space.
• A property is any characteristic that allows us to recognize a particular type of matter and to
distinguish it from other types of matter.
• About 100 elements constitute all matter.
• Elements:
• are made up of unique atoms, the building blocks of matter.
• Names of the elements are derived from a wide variety of sources (e.g., Latin or Greek,
mythological characters, names of people or places).
• For some elements, the basic unit is not an atom, but a molecule (e.g., O2, S8.)
• Molecules:
• are combinations of atoms held together in specific shapes.
• Macroscopic (observable) properties of matter relate to submicroscopic realms of atoms.
• Properties relate to composition (types of atoms present) and structure (arrangement of
atoms) present.
Why Study Chemistry?8,9,10
We study chemistry because:
• it has a considerable impact on society (health care, food, clothing, conservation of natural resources,
environmental issues, etc.).
• it is part of your curriculum! Chemistry serves biology, engineering, agriculture, geology, physics,
etc., Chemistry is the central science.