Chapter 1. Chemistry: Matter and Measurement
1.1 Approaching Chemistry: Experimentation
1.2 Chemistry and the Elements
1.3 Elements and the Periodic Table
1.4 Some Chemical Properties of the Elements
1.5 Experimentation and Measurement
1.6 Measuring Mass
1.7 Measuring Length
1.8 Measuring Temperature
1.9 Derived Units: Measuring Volume
1.10 Derived Units: Measuring Density
1.11 Accuracy, Precision and Significant Figures in Measurement
1.12 Rounding Numbers
1.13 Calculations: Converting from One Unit to Another
Properties of Matter
Matter: anything that has both mass & volume.
Properties: describe or identify matter.
Intensive Properties do not depend on amount.
Extensive Properties do depend on amount.
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Properties of Matter
The boiling point of water is 100C at
normal temp and pressure. It is
independent of the quantity of water
and is an intensive property
The mass of a cube of sugar is, say, 5
grams. It tells us nothing about the
substance sugar other than the mass
and is an extensive property.
Properties of Matter
Physical Properties can be determined without
changing the chemical makeup of the sample.
Some typical physical properties are:
Melting Point, Boiling Point, Density, Mass, Touch, Taste,
Temperature, Size, Color, Hardness, Conductivity.
Some typical physical changes are:
Melting, Freezing, Boiling, Condensation, Evaporation,
Dissolving, Stretching, Bending, Breaking.
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Properties of Matter
Chemical Properties are those that do
change the chemical makeup of the sample.
Some typical chemical properties are:
Burning, Cooking, Rusting, Color change, Souring
of milk, Ripening of fruit, Browning of apples,
Taking a photograph, Digesting food.
Chemistry and the Elements
A. Element- a fundamental substance that can not be chemically
changes or broken down into anything smaller
Chemical symbol- used to represent the specific elements;
capitalize the 1st letter if 2nd letter present it is lowercase
B. Periodic table- a tabular organization of all 115 elements
YOU SHOULD LEARN THE NAMES AND SYMBOLS OF THE 1ST 36
ELEMENTS PLUS ALL ELMENTS YOU COME ACROSS IN THE LABORATORY
examples: C- carbon, N- nitrogen, Ca- calcium, He- helium, Pb- lead, Zn; zinc
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Elements and the Periodic Table
A. Periodic table- grid of the elements arranged in 7 rows and
18 columns
B. Periods- seven horizontal rows in the periodic table
C. Groups-
18 vertical columns ; groups numbered 1-->18
(or 1A->8A and 1B-->8B)
elements in a given group have similar chemical properties
D. The table is the most important organizing principle of chemistry
1. Regular progression in the size of the 7 periods;
similar regularity in atomic structure
2. Main Group elements: Groups 1A-8A
3. Transition metal elements- Groups 1B- 8B (middle of table)
4. Inner transition metals (Rare Earth)
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Special Groups of of the Elements
Group 1A Group 2A Group 7A-
Group 8A -
Alkali metals are silvery metals; i.e., Na
react rapidly with water
Alkaline earth metals
i.e., Ca
again silvery metals; less reactive to water
Halogens- corrosive, nonmetallic, react to from salts
i.e., Cl2
Noble Gases- gases which have very low
chemical reactivity i.e., Ne
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Alkali metals
Halogens
Noble
gases
Alkaline earth
metals
There are three major classes of Elements
Metals - largest group; on the left side (left of the heavy zigzag line)
all solids (except mercury), malleable, ductile (drawn into a wire)
conduct heat and electricity
Nonmetals- on right side ( right of heavy zigzag line)
gases, liquids or solids; brightly coloured; brittle solids
poor conductors of heat and electricity
Semimetals (metalliods) - boundary between metal and nonmetals
chemical properties fall between metals and nonmetals
brittle and poor conductors
6
semimetals
nonmetals
metals
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