Matter and Its Classification

Definition and States of Matter

Matter is defined as anything that has mass and occupies space. It exists in three primary physical states, each with distinct properties:

• Solid: Definite shape and volume; particles are closely packed in a fixed arrangement.

• Liquid: Definite volume but takes the shape of its container; particles are close but can move past one another.

• Gas: No definite shape or volume; particles are far apart and move freely.

Pure Substances and Mixtures

Pure substances have a fixed composition and distinct properties. They are classified as:

• Elements: Substances that cannot be broken down into simpler substances by chemical means (e.g., oxygen, gold).

• Compounds: Substances composed of two or more elements chemically combined in fixed proportions (e.g., water (H2O), carbon dioxide (CO2)).

Mixtures (not explicitly mentioned but important for context) are combinations of two or more substances that retain their individual properties and can be separated by physical means.

Additional info: Mixtures can be homogeneous (uniform composition) or heterogeneous (non-uniform composition).

Atomic Structure and the Periodic Table

Atoms and Subatomic Particles

Atoms are the basic units of matter, consisting of three main subatomic particles:

• Protons: Positively charged particles located in the nucleus.

• Neutrons: Neutral particles also found in the nucleus.

• Electrons: Negatively charged particles that orbit the nucleus in electron clouds.

The Periodic Table

The periodic table organizes elements by increasing atomic number (number of protons). It helps predict chemical properties and relationships among elements.

Chemical Bonds

Ionic and Covalent Bonds

Chemical bonds are forces that hold atoms together in compounds. The two main types are:

• Ionic Bonds: Formed when electrons are transferred from a metal to a nonmetal, resulting in the formation of oppositely charged ions that attract each other.

• Covalent Bonds: Formed when two atoms (usually nonmetals) share one or more pairs of electrons.

Example: Sodium chloride (NaCl) forms via ionic bonding, while water (H2O) forms via covalent bonding.

Measurements in Chemistry

SI Units

The International System of Units (SI) is the standard for scientific measurements. Key SI units include:

• Meter (m): Length

• Kilogram (kg): Mass

• Second (s): Time

• Kelvin (K): Temperature

• Mole (mol): Amount of substance

Significant Figures

Significant figures reflect the precision of a measured quantity. The number of significant figures in a value indicates the certainty of the measurement.

• All nonzero digits are significant.

• Zeros between nonzero digits are significant.

• Leading zeros are not significant; trailing zeros are significant only if there is a decimal point.

Example: 0.00450 has three significant figures.

Density

Density is a physical property defined as the mass of a substance per unit volume. It is calculated using the formula:

• d: Density (e.g., g/cm3)

• m: Mass (e.g., grams)

• V: Volume (e.g., cm3 or mL)

Example: If a sample has a mass of 10 g and a volume of 2 cm3, its density is .