Chapter 1
Physical properties Characteristics that can be observed without changing
the substance's composition (e.g., color, density,
melting point).
Chemical Characteristics that involve a chemical change, such
properties as flammability or reactivity with other substances.
Key States of Matter
Solid: Has a definite shape and volume; particles are closely packed and
vibrate in place.
Liquid: Has a definite volume but takes the shape of its container;
particles can move past one another.
Gas: Has no fixed shape or volume; particles are spaced widely apart and
move rapidly.
Property type extensive properties intensive
properties
definition Depend on the amount Do not depend on the
of substance amount of substance
examples Mass, volume, length Density, color, melting point
Measurement Changes with the size Remains constant regardless
impact of the sample of sample size
Classification of Matter
Pure Substances vs. Mixtures
Pure substances consist of only one type of element or compound, with
a fixed chemical composition and well-defined properties.
Mixtures contain two or more elements or compounds that have not
reacted chemically and can be separated by physical means.
Mixtures can be homogeneous (uniform composition) or
heterogeneous (distinct components).
, Chapter 2
Atomic Theory: The theory that all matter is composed of atoms, which
are indivisible and indestructible particles.
Periodic Law: The properties of elements are periodic functions of their
atomic numbers, leading to the organization of elements in the periodic
table.
To calculate the average atomic weight of an element:
Identify the isotopes of the element and their respective masses.
Determine the percent abundance of each isotope.
Multiply the mass of each isotope by its percent abundance (as a
decimal).
Sum the results from step 3 to get the average atomic weight.
Tip: Ensure that the percent abundances add up to 100%
Concept covalent compounds ionic
compounds
composition Formed by Formed by
sharing transfer of
electrons electrons
between atoms between atoms
bonding Strong covalent Strong ionic
bonds bonds
State at room Can be gases, Usually, solid at
temp liquids, or solids room temp
conductivity Poor conductors Good conductors
of electricity when dissolved
in water
examples Water (H2O), Sodium chloride
carbon dioxide (NaCl),
(CO2 magnesium
oxide (MgO)
Physical properties Characteristics that can be observed without changing
the substance's composition (e.g., color, density,
melting point).
Chemical Characteristics that involve a chemical change, such
properties as flammability or reactivity with other substances.
Key States of Matter
Solid: Has a definite shape and volume; particles are closely packed and
vibrate in place.
Liquid: Has a definite volume but takes the shape of its container;
particles can move past one another.
Gas: Has no fixed shape or volume; particles are spaced widely apart and
move rapidly.
Property type extensive properties intensive
properties
definition Depend on the amount Do not depend on the
of substance amount of substance
examples Mass, volume, length Density, color, melting point
Measurement Changes with the size Remains constant regardless
impact of the sample of sample size
Classification of Matter
Pure Substances vs. Mixtures
Pure substances consist of only one type of element or compound, with
a fixed chemical composition and well-defined properties.
Mixtures contain two or more elements or compounds that have not
reacted chemically and can be separated by physical means.
Mixtures can be homogeneous (uniform composition) or
heterogeneous (distinct components).
, Chapter 2
Atomic Theory: The theory that all matter is composed of atoms, which
are indivisible and indestructible particles.
Periodic Law: The properties of elements are periodic functions of their
atomic numbers, leading to the organization of elements in the periodic
table.
To calculate the average atomic weight of an element:
Identify the isotopes of the element and their respective masses.
Determine the percent abundance of each isotope.
Multiply the mass of each isotope by its percent abundance (as a
decimal).
Sum the results from step 3 to get the average atomic weight.
Tip: Ensure that the percent abundances add up to 100%
Concept covalent compounds ionic
compounds
composition Formed by Formed by
sharing transfer of
electrons electrons
between atoms between atoms
bonding Strong covalent Strong ionic
bonds bonds
State at room Can be gases, Usually, solid at
temp liquids, or solids room temp
conductivity Poor conductors Good conductors
of electricity when dissolved
in water
examples Water (H2O), Sodium chloride
carbon dioxide (NaCl),
(CO2 magnesium
oxide (MgO)
