Chem 134 chapters 1-3

Dalton's Atomic Theory

Proposed that all matter is composed of tiny, indivisible particles called atoms.

Law of Conservation of Mass

Atoms cannot be created or destroyed, aligning with this law.

Identical Atoms

Atoms of a given element are identical in mass and properties according to Dalton's theory.

Groundwork for Modern Chemistry

Dalton's work laid the foundation for modern chemistry and understanding chemical reactions.

Law of Definite Proportions

All samples of a given compound have the same proportions of their constituent elements.

Law of Multiple Proportions

Ratios of the masses of one element that combine with a fixed mass of another can be expressed as small whole numbers.

Predictable Chemical Combinations

The laws of chemical composition highlight the predictable nature of chemical reactions.

Cathode Ray Experiment

Conducted by J.J. Thomson, leading to the discovery of the electron.

Millikan's Oil Drop Experiment

Determined the charge of a single electron, providing a fundamental constant in physics.

Rutherford's Gold Foil Experiment

Showed that atoms consist mostly of empty space with a dense, positively charged nucleus.

Intensive Properties

Properties independent of the amount of substance present (e.g., density, boiling point).

Extensive Properties

Properties that depend on the amount of substance present (e.g., mass, volume).

Hydrates

Ionic compounds that contain water molecules within their structure.

Binary Acids

Acids containing only two elements, named with the prefix 'hydro-' and the suffix '-ic'.

Oxyacids

Acids containing oxygen and a polyatomic ion, named based on the polyatomic ion (e.g., 'ate' becomes '-ic').

Alkanes

Saturated hydrocarbons with single bonds (C-C).

Alkenes

Unsaturated hydrocarbons with at least one double bond (C=C).

Alkynes

Unsaturated hydrocarbons with at least one triple bond (C≡C).

Hydrocarbon Structure

The structure of hydrocarbons determines their reactivity and physical properties.