CHEM 111 Final: CHEM111 FINAL REVIEW
18 Jun 2018
School
Department
Course
Professor
Final Exam:
American Chemical Society cumulative exam:
Number of questions: 70 questions
Length of time: 110 minutes
Date: Monday, December 12, 2016
Time: 10:25 am
Chapter 1
•Significant figures.
oUnderlined figures count
o0.00540, 05703.0,
•Density-based calculations
•Units
•Basic Math Skills
•Atomic Structure
Notes:
1) Chemistry is the study of the composition, structure and
properties of matter and energy and changes that matter
undergoes.
a. Matter – anything that occupies space and has mass. (mass
– the quantity of matter in a material)
b. Energy – the “ability to do work.”
2) Experiment and Explanation
a. An observation of natural phenomena carried out in a
controlled manner so that the results can be duplicated and
rational conclusions obtained.
b. After a series of experiments, a researcher may see some
relationship or regularity in the results.
c. Law is a concise statement or mathematical equation about
a fundamental relationship or regularity of nature.
c.i. Law of Conservation of Mass- The total mass remains
constant during a chemical change (chemical reaction).
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c.ii. Law of Definite Proportions: A pure compound,
regardless of its source, always contains constant
proportions of the elements by mass.
c.ii.1. For example, 1.0000 gram of sodium
chloride will always contain 0.3934 gram of
sodium and 0.6066 gram of chlorine.
d. Hypothesis: A tentative explanation of some regularity of
nature.
e. Theory: If a hypothesis is successful, it becomes a theory… A
tested explanation of basic natural phenomena
f. Scientific Method: Experiments-Results-Hypothesis
3) Matter: Physical State and Chemical Constitution
a. Matter: Whatever occupies space and can be perceived by
our senses
b. Classification: Its physical state: solid, liquid, or gas
Its chemical constitution: element, compound, or mixture.
b.i. Physical Property: A characteristic that can be
observed for a material without changing its chemical
identity. For example: Physical state, Boiling point,
Color
b.i.1. Physical change: Change in form of matter
but not its chemical identity.
b.i.1.a. Mostly reversible.
b.i.1.b. No new compounds are formed
b.ii. Chemical Property: A characteristic of a material
involving its chemical change. For example: Ability to
react with oxygen; Ability to react with fluorine
b.ii.1. Chemical change: New compounds are
formed
b.ii.1.a. In many cases the process is non-
reversible
b.ii.1.b. Chemical reaction
4) Matter: Substance
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a. Substance: A kind of matter that cannot be separated into
other kinds of matter by any physical process such as
distillation or sublimation.
a.i. Element
a.i.1. Cannot be decomposed into simpler
substances by any chemical reaction. For
example: Hydrogen, Carbon, Oxygen
a.ii. Compound
a.ii.1. Composed of two or more elements
chemically combined. For example: Water (H2O),
Carbon dioxide (CO2)
5) Matter: Mixture
a. A material that can be separated by physical means into two
or more substances
b. Heterogeneous Mixture: A mixture that consists of
physically distinct parts, each with different properties.
b.i. For example: Salt and iron filings, Oil and vinegar
c. Homogenous Mixture: A mixture that is uniform in its
properties; also called a solution.
c.i. For example: Saltwater, Air
d. Phase: One of several different homogeneous materials
present in the portion of matter under study
6) Temperature
a. The Celsius scale (formerly the Centigrade scale) is the
temperature scale in general scientific use.
a.i. – However, the SI base unit of temperature is the
Kelvin (K), a unit based on the absolute temperature
scale.
b. Temperature Units
b.i. Celsius, °C / Fahrenheit, °F / Kelvin, K
b.ii. K = oC + 273.15
b.iii. oF = 1.8(oC) + 32
7) Derived Units
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Document Summary
Chapter 1: significant figures, underlined figures count, 0. 00540, 05703. 0, density-based calculations, units, basic math skills, atomic structure. Notes: chemistry is the study of the composition, structure and properties of matter and energy and changes that matter undergoes, matter anything that occupies space and has mass. (mass. Law of conservation of mass- the total mass remains constant during a chemical change (chemical reaction). c. ii. Law of definite proportions: a pure compound, regardless of its source, always contains constant proportions of the elements by mass. c. ii. 1. Its chemical constitution: element, compound, or mixture. b. i. Physical property: a characteristic that can be observed for a material without changing its chemical identity. Physical change: change in form of matter but not its chemical identity. Chemical property: a characteristic of a material b. i. 1. b. b. i. 1. a. involving its chemical change. For example: ability to react with oxygen; ability to react with fluorine b. ii. 1. In many cases the process is non- reversible b. ii. 1. b.
