The document discusses the laws and principles that support the atomic theory of matter. It outlines three laws: the law of definite proportions, the law of conservation of mass, and the law of multiple proportions. It also lists the five principles of John Dalton's atomic theory, which include that all matter is made of atoms, atoms are identical within an element but different between elements, atoms cannot be created or destroyed, atoms combine in whole number ratios, and atoms are rearranged in chemical reactions.

1. Chapter 3.1 Substances are Made of Atoms Atoms and Moles

2. Objective 1: State the three laws that support the existence of atoms. Law of Definite Proportions States that a chemical compound contains the same proportions by mass regardless of the size of the sample or source of the compound Sodium Chloride – Always 39.34 % Na by mass 60.66% Cl by mass

3. Law of conservation of mass States that mass is neither destroyed nor created during ordinary chemical reactions or physical changes. If you start with 12 g of reactant, you will be left with 12 grams of product Law of multiple Proportions If 2 or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the element is always a ratio of small whole numbers Ex: NO2 , N2O4 CO , CO2

4. Objective 2List the five principles of John Dalton’s atomic theory Dalton’s Atomic Theory In 1808, and English School teacher, John Dalton came up with these assumptions of the atom. All matter is composed of extremely small particles called atoms Atoms of a given element are identical in size, mass, and other properties Atoms cannot be subdivided, created, or destroyed. Atoms of different elements combine in simple whole-number ratios to form chemical compounds In chemical reactions, atoms are combined, separated, or rearranged.

5. Atomic Theory