Chapter 1
Chemistry - The study of matter, its properties, and the changes that matter undergoes.
Matter - The physical material of the world. It is anything that has mass and occupies space. Matter can either be a pure substance or a mixture.
Matter can exist in three states: solid, liquid, gas
Any substance can exist in the solid, liquid, or gas state depending on temperature and pressure.
Property - Any characteristic that allows us to recognize a particular type of matter and to distinguish it from other types.
Atoms - The small building blocks of matter.
Examples: H, O, C, Na (Hydrogen, Oxygen, Carbon, Sodium)
Elements - Pure Substance that are composed of only one kind of atom. They can be composed of single atom particles, or as molecules of the same atom.
Examples: O2, S8 (Oxygen, Sulfur), Iron, Hydrogen Gas
Molecule - A particle composed of two or more atoms joined together.
NOT ALL MOLECULES ARE COMPOUNDS!
Examples: O2, CO2, NaCl (Oxygen, Carbon Dioxide, Sodium Chloride)
Compounds - Pure substances that are composed of particles that contain more than one kind of atom joined together by a bond.
ALL COMPOUNDS ARE COMPOSED OF MOLECULES!
Examples: H2O, NaCl, NH3 (Water, Sodium Chloride, Ammonia)
Pure Substance - Matter that has distinct properties and a composition that does not vary from sample to sample.
Mixtures - Combinations of two or more substances in which each substance retains its chemical identity. They are not chemically combined and can be separated by physical or mechanical means. Components
of a mixture can be separated by physical processes (Magnetic properties, such as a mixture of iron and sulfur, and phase, which separates a solid phase from a liquid).
Homogeneous Mixtures - Also known as solutions, have a constant, uniform composition throughout. The percent composition of components can vary and are single phase.
Examples: Air, salt water, metal alloys, gasoline
Heterogeneous Mixtures - Have a non-uniform composition. The percent composition of components can vary and may contain multiple phase.
Examples: Oil & vinegar, granite, soil, ice water
Law of Constant Composition - First stated by French chemist Joseph Louis Proust, it is the observation that the elemental composition of a compound is always the same.
Example: Pure water from any source is composed of: two hydrogen (H) atoms, one oxygen (O) atom
Physical Properties - Characteristics of a substance that can be observed without changing the identity and composition of the substance.
Examples: Boiling/melting point, density, mass, color
Chemical Properties - Characteristics of a substance that can only be observed by changing it into a difference substance.
Examples: Flammability, reactivity, corrosiveness
Intensive Properties - Do not depend on the amount of sample being examined.
Examples: Boiling/melting point, density, temperature, color, hardness
Extensive Properties - Depend on the amount of the sample.
Examples: Mass, volume, internal energy, heat change
Physical Changes - A substance changes its physical appearance but not its composition.
Examples: Change of phase, temperature, volume
Chemical Changes - Also known as a chemical reaction, a substance is transformed into a chemically different substance.
Examples: Combustion, oxidation, decomposition
Distillation - A process that depends on the different abilities of substances to form gases.
Examples: Desalination of ocean water, alcohol production, separation of crude oil
Chromatography - Differences in solubility and/or adherence to a surface.
Examples: Water softener, blood testing, forensic testing
Density - The amount of mass in a unit divided by the volume of a substance. (d = m/v)
Example: Calculate the volume of 525g of lead. Density is 11.34g/cm3.
d = m/v (rearrange to solve) v = m/d
v = 525g/ 11.34g/cm3
v = 46.3 cm3
Significant Figures - All digits of a measured quantity.
• All non-zero digits are significant.
• Zeros between non-zero digits are always significant.
• Zeros at the beginning of a number are never significant.
• Zeros are the end of a number are significant if the number contains a decimal point.
Multiplication and Division
The answer will have the same number of sig figs as the number in the equation with the fewest sig figs.
Addition and Subtraction
The answer will have the same number of decimal places as the number with the fewest decimal places.
Rounding
If the leftmost digit removed is more than 5, the preceding number increases by 1.
If the leftmost digit removed is less than 5, the preceding number remains unchanged.
Dimensional Analysis (Unit Conversion) - Given unit x desired unit/given unit = desired unit
1 cm3 = 1 mL
12 in = 1 ft
1000 mm = 1 m
60 sec = 1 min
1 lb = 453.592 grams
1 in = 2.54 cm
Derived Unit - Obtained by multiplication or division of one or more base units.
Physical Quantity Name of Unit Abbreviation
Length Meter m
Mass Kilogram kg
Temperature Kelvin K
Time Second s or sec
Amount of substance Mole mol
Prefix Prefix Symbol Word Conventional Notation Exponential Notation
tera T trillion 1,000,000,000,000 1x1012
giga G billion 1,000,000,000 1x109
mega M million 1,000,000 1x106
kilo k thousand 1,000 1x103
deci d tenth 0.1 1x10-1
centi c hundredth 0.01 1x10-2
milli m thousandth 0.001 1x10-3
micro millionth 0.000001 1x10-6
nano n billionth 0.000000001 1x10-9
pico p trillionth 0.000000000001 1x10-12
Example 1: 5g to mg
5g/1 x 1mg/10-3g = 5000mg (g will cross each other out)
Example 2: 650 to L
Chemistry - The study of matter, its properties, and the changes that matter undergoes.
Matter - The physical material of the world. It is anything that has mass and occupies space. Matter can either be a pure substance or a mixture.
Matter can exist in three states: solid, liquid, gas
Any substance can exist in the solid, liquid, or gas state depending on temperature and pressure.
Property - Any characteristic that allows us to recognize a particular type of matter and to distinguish it from other types.
Atoms - The small building blocks of matter.
Examples: H, O, C, Na (Hydrogen, Oxygen, Carbon, Sodium)
Elements - Pure Substance that are composed of only one kind of atom. They can be composed of single atom particles, or as molecules of the same atom.
Examples: O2, S8 (Oxygen, Sulfur), Iron, Hydrogen Gas
Molecule - A particle composed of two or more atoms joined together.
NOT ALL MOLECULES ARE COMPOUNDS!
Examples: O2, CO2, NaCl (Oxygen, Carbon Dioxide, Sodium Chloride)
Compounds - Pure substances that are composed of particles that contain more than one kind of atom joined together by a bond.
ALL COMPOUNDS ARE COMPOSED OF MOLECULES!
Examples: H2O, NaCl, NH3 (Water, Sodium Chloride, Ammonia)
Pure Substance - Matter that has distinct properties and a composition that does not vary from sample to sample.
Mixtures - Combinations of two or more substances in which each substance retains its chemical identity. They are not chemically combined and can be separated by physical or mechanical means. Components
of a mixture can be separated by physical processes (Magnetic properties, such as a mixture of iron and sulfur, and phase, which separates a solid phase from a liquid).
Homogeneous Mixtures - Also known as solutions, have a constant, uniform composition throughout. The percent composition of components can vary and are single phase.
Examples: Air, salt water, metal alloys, gasoline
Heterogeneous Mixtures - Have a non-uniform composition. The percent composition of components can vary and may contain multiple phase.
Examples: Oil & vinegar, granite, soil, ice water
Law of Constant Composition - First stated by French chemist Joseph Louis Proust, it is the observation that the elemental composition of a compound is always the same.
Example: Pure water from any source is composed of: two hydrogen (H) atoms, one oxygen (O) atom
Physical Properties - Characteristics of a substance that can be observed without changing the identity and composition of the substance.
Examples: Boiling/melting point, density, mass, color
Chemical Properties - Characteristics of a substance that can only be observed by changing it into a difference substance.
Examples: Flammability, reactivity, corrosiveness
Intensive Properties - Do not depend on the amount of sample being examined.
Examples: Boiling/melting point, density, temperature, color, hardness
Extensive Properties - Depend on the amount of the sample.
Examples: Mass, volume, internal energy, heat change
Physical Changes - A substance changes its physical appearance but not its composition.
Examples: Change of phase, temperature, volume
Chemical Changes - Also known as a chemical reaction, a substance is transformed into a chemically different substance.
Examples: Combustion, oxidation, decomposition
Distillation - A process that depends on the different abilities of substances to form gases.
Examples: Desalination of ocean water, alcohol production, separation of crude oil
Chromatography - Differences in solubility and/or adherence to a surface.
Examples: Water softener, blood testing, forensic testing
Density - The amount of mass in a unit divided by the volume of a substance. (d = m/v)
Example: Calculate the volume of 525g of lead. Density is 11.34g/cm3.
d = m/v (rearrange to solve) v = m/d
v = 525g/ 11.34g/cm3
v = 46.3 cm3
Significant Figures - All digits of a measured quantity.
• All non-zero digits are significant.
• Zeros between non-zero digits are always significant.
• Zeros at the beginning of a number are never significant.
• Zeros are the end of a number are significant if the number contains a decimal point.
Multiplication and Division
The answer will have the same number of sig figs as the number in the equation with the fewest sig figs.
Addition and Subtraction
The answer will have the same number of decimal places as the number with the fewest decimal places.
Rounding
If the leftmost digit removed is more than 5, the preceding number increases by 1.
If the leftmost digit removed is less than 5, the preceding number remains unchanged.
Dimensional Analysis (Unit Conversion) - Given unit x desired unit/given unit = desired unit
1 cm3 = 1 mL
12 in = 1 ft
1000 mm = 1 m
60 sec = 1 min
1 lb = 453.592 grams
1 in = 2.54 cm
Derived Unit - Obtained by multiplication or division of one or more base units.
Physical Quantity Name of Unit Abbreviation
Length Meter m
Mass Kilogram kg
Temperature Kelvin K
Time Second s or sec
Amount of substance Mole mol
Prefix Prefix Symbol Word Conventional Notation Exponential Notation
tera T trillion 1,000,000,000,000 1x1012
giga G billion 1,000,000,000 1x109
mega M million 1,000,000 1x106
kilo k thousand 1,000 1x103
deci d tenth 0.1 1x10-1
centi c hundredth 0.01 1x10-2
milli m thousandth 0.001 1x10-3
micro millionth 0.000001 1x10-6
nano n billionth 0.000000001 1x10-9
pico p trillionth 0.000000000001 1x10-12
Example 1: 5g to mg
5g/1 x 1mg/10-3g = 5000mg (g will cross each other out)
Example 2: 650 to L
