General Chemistry Reviewer

Chapter 1

Ma  !   er  -anything that occupies space and has mass

Solid

Liquid

Gas

IMF

Strong

Moderate

Weak

Rate of Dissolution

very slow

moderate

fast

Diffusion

very slow

moderate

fast

Shape

definite

not definite

not definite

Volume

definite

definite

not definite, negligible

Density

high

h i gh

low

Motion of Particles

high

h i gh

low

moderately difficult

easy

Compressibility difficult

Chapter 2

Atoms and Elements  smallest particle of an element that retains the chemical identity of the element I.

Parts of an atom • Electron-negatively charged • Nucleus- contains the ff • Proton- positively charged • Neutron- neutral

II. History of the Atom • Democritus • tiny indestructible particles • atomos • Dalton • proposed the atomic theory of matter • like billiard balls • J.J. Thompson • electrical nature of atoms through cathode ray tubes • raisin bread • discovered the electron • Ernest Rutherford • established the properties of the nucleus • mostly empty space • + charged nucleus where mass is concentrated and where - revolve around the nucleus • Neils Bohr • proposed the planetary model of the atom III. Dalton’s Atomic Theory of Matter All mater is composed of tiny particles called atoms  All atoms of a given element are identical, but atoms of different elements are not alike. Atoms are neither created nor destroyed in any chemical reaction  Atoms unite in simple ratios to form compounds 

IV. Modern Atomic Theory • also known as the electron cloud model

• Electrons do not revolve around the nucleus in an orbit of definite radius, rather, there are regions within the atom where the electrons are most likely to be found • Quantum numbers are used to approximate the probable location of an electron • Orbit- regular path taken • Orbitals- region where electron is most probably found

V. Basic Laws in Chemistry • Law of Mass Conservation • Antoine Lavoisier • Total mass of reactants is equal to the mass of the products • Law of Definite Composition • Joseph Proust • a compound always contains the same elements in the same mass proportions • Law of Energy Conservation • energy cannot be created or destroyed – it only changes forms • Law of Multiple Proportions • atoms combine in multiple proportions of small whole numbers VI. Species and Subatomic Particles • the Periodic table of elements gives us the symbol, the atomic number, and the mass number of each element • Symbols • used in place of the name of the elements • Atomic Number • number of protons • Atomic Mass/Mass Number • sum of protons and neutrons VII. Ions • charged particles of atoms -> anions and cations VIII.Isotopes • atoms with the same number of protons but different number of neutrons

IX. The Periodic Table of Elements • 1789 • Lavosier published Traite Elementaire de Chimie • 1817 • Wolfgang Dobereiner • elemental triad • [Cl,Br,I] &[Li, Na, K] • 1862 • Chancourtois • notices the periodicity of elements • telluric helix • 1865 • Newlands • Classified elements according to physical properties which differed by some multiple of 8 in atomic weight • Law of Octaves • 1869 • Mendeleev • published the first periodic table by increasing atomic weight • 1914 • Mosely • resequenced the elements according to their increasing atomic number • 1943 • Seaborg • Actinide series

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