General Chemistry 1.1: Kinetic Molecular Theory and Atomic Structure

Vocabulary-style flashcards covering Kinetic Molecular Theory, states and properties of matter, chemical and physical changes, separation techniques, atomic theory, laws of stoichiometry, and the mole concept.

Particulate Theory of Matter

A theory stating that all matter is made of atoms which are in constant motion, attract each other, have spaces between them, and move faster as temperature increases.

Plasma

An ionized gas consisting of positively charged ions and free electrons where charges are separated due to ionization.

Extensive Properties

Physical properties that depend on the amount of matter present, such as mass, volume, length, and weight.

Intensive Properties

Physical properties that do not depend on the amount of matter present, such as density, melting point, boiling point, color, odor, hardness, solubility, malleability, ductility, conductivity, and luster.

Chemical Properties

A substance’s ability to undergo a specific chemical change and form a new substance, such as flammability, reactivity, toxicity, and heat of combustion.

Physical Change

A change in the form or appearance of a substance without changing its chemical identity, such as melting ice, boiling water, or dissolving sugar.

Chemical Change

A process involving the rearrangement of the molecular or ionic structure of a substance, such as burning wood, rusting iron, or digestion of food.

Homogenous Mixture

A mixture that has a uniform composition throughout.

Heterogenous Mixture

A mixture that is not uniform in composition.

Solvent

The substance referred to as 'pangtunaw' that dissolves another substance.

Solute

The substance referred to as 'tinutunaw' that is being dissolved.

Decantation

A method of separating mixtures by means of pouring.

Distillation

A separation technique that utilizes different boiling points of substances.

Weight

The force exerted by gravity on an object with a specific mass, typically involving $9.8\,m/s^2$.

Dalton’s Theory (1804)

A theory stating that all matter is composed of atoms; atoms of a given element are identical; and atoms are combined, separated, or rearranged in chemical reactions.

Law of Conservation of Mass

A law credited to Antoine Lavoisier stating that matter is neither created nor destroyed, and the mass of reactants equals the mass of products.

Law of Definite Proportion (Proust’s Law)

The principle that samples of a given compound always contain the same proportion of elements by mass.

Law of Multiple Proportions (Dalton’s Law)

The law stating that when two elements form more than one compound, the different masses of one element that combine with a fixed mass of the other are in a ratio of small whole numbers.

Atomic Number (Z)

The number of protons in the nucleus of an atom; it is equal to the number of electrons in a neutral atom.

Mass Number (A)

The total number of protons and neutrons in the nucleus of an atom, represented by the formula $A = \text{Protons (Z)} + \text{Neutrons (N)}$.

Isotopes

Atoms of the same element that have different numbers of neutrons and therefore different mass numbers.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Synthesis Reaction

A chemical reaction where two or more substances combine to form a single product, represented as $A + B \rightarrow AB$.

Decomposition Reaction

A chemical reaction where a single compound breaks down into two or more elements or new compounds, represented as $AB \rightarrow A + B$.

Combustion

A reaction involving burning, represented by the general formula $C_xH_x + O_2 \rightarrow CO_2 + H_2O$.

Mole (mol)

The amount of particles in matter, represented by Avogadro’s number, which is $6.02 \times 10^{23}$.

Molar Mass

The mass of one mole of a substance, expressed in $g\,mol^{-1}$, which is equal to the atomic mass or formula mass.

J.J. Thomson

A scientist who used the cathode ray tube to develop the Plum pudding model of the atom.

Robert Millikan

The scientist responsible for the Oil-drop experiment.

Ernest Rutherford

The scientist who conducted the Gold foil experiment.