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2: Classification of Matter
Chemistry: the study of matter and the changes that matter undergoes
Matter: anything that occupies space and has mass
Mass: a measure of the quantity of matter
Substance (or Pure Substance): types of matter that always has the same chemical
composition, no matter what their origin; cannot be separated into components by physical
means
Mixture: two or more pure substances that may vary in composition, can be separated by
physical means
Substances
Mixtures
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Homogenous Mixture (or
be broken down into simpler
Solution): has a uniform
substances even by chemical
composition throughout (i
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salt
reaction (i
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oxygen)
water)
a) Metals: characterized by
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e
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Compounds: substances
composed of two or more
elements combined in definite
proportions (i
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water), cannot
be separated by physical
means…separation of a
compound into its constituent
elements requires a chemical
reaction
Element Symbol: a shorthand version of an element’s longer name
Chemical Formula: describes the composition of a compound, using symbols for the elements
that make up the compound
Atom: the smallest unit of an element that has the chemical properties for that element
Molecule: two or more atoms bound together in a discrete arrangement
Physical State: a form that matter can take; solid, liquid, and gas
Aqueous Solution: a solution in which a substance is dissolved in water
*States of matter can be interconnected without changing chemical composition
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3: Scientific Measurement
Quantitative Properties: can be measured and expressed using numbers
International System of Unites (SI): a system of units based on metric units
Weight: the force exerted by an object or sample due to gravity
Mass: a measure of the amount of matter in an object or sample
• SI base unit of mass is the kilogram;
o 1kg = 1,000g = 1 x 103g
*There are two temperature scales used in chemistry: , K
*Celsius scale was originally defined using the freezing and boiling point of pure water at sea
level
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*Units of the Celsius and Kelvin scales are equal in magnitude, so a degree Celsius is equivalent
to a kelvin
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à K: K = + 273
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à : = ( - 32) x ()
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001g/mL
*1L = 1dm3 = 1,000mL
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e
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e
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e
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e
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5: Uncertainty in Measurement
Exact Numbers: numbers with defined values, also include those that are obtained by counting
Inexact Numbers: numbers measured by any method other than counting, including measured
numbers
Significant Numbers: meaningful digits in a measured or calculated value
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To avoid ambiguity, it is best to
express such numbers using scientific notation
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In addition and subtraction, the answer cannot have more digits to the right of
the decimal than the original number with the smallest number of digits to the
right of the decimal point
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In multiplication and division, the number of significant figures in the final
product or quotient is determined by the original number that has the smallest
number of significant figures
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Exact numbers can be considered to have an infinite number of significant
figures and do not limit number of significant figures in a calculated result
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6: Using Units and Solving Problems
conversion factor: a fraction in which the same quantity is expressed one way in the numerator
and another way in the denominator
dimensional analysis: the use of conversion factors in problem solving