SPS4. Students will investigate the arrangement of the Periodic Table.

Chapter 3: Atoms & The Periodic Table Why do coins shine? Their chemical properties determine their physical properties. Example: Gold vs. Silver

Atoms are the building blocks of ___________. Atomic Structure Atoms are the building blocks of ___________. In 1808, John Dalton proposed the Atomic Theory

The Atomic Theory Every element is made of tiny, unique particles called _________ that cannot be subdivided. Atoms of the same element are exactly alike Atoms of different elements can join to form __________.

Atoms have no overall charge ________ Atomic # =_________ 3 parts to an atom Protons Neutrons Electrons Atoms have no overall charge ________ Atomic # =_________ Atomic Mass =__________ Nucleus

Bohr’s Model Compares electrons to planets that orbit. Stated that electrons in an atom move in set paths around the nucleus. The path defines the electron’s ________ ________.

Energy Levels (Orbitals) Electrons can only be in certain energy levels Electrons must________ energy to move to higher energy level & _________ energy to move to a lower energy level. Ex. Elevator

Modern Model Electrons move more like _________ instead of orbits. It is impossible to determine the exact location of an electron or its speed & direction. Ex. Blades of a Fan

Electrons are found in orbitals within energy levels The region where electrons are found are called Orbitals. Electrons can occupy 4 kinds of orbitals The simplest orbital is the ____ orbital. The s orbital can have only ______ possible orientation in space. Shaped like a _________

Orbitals Continued The p orbital is dumbell-shaped and can be oriented 3 different ways in space. There are also d & f orbitals. There are 5 possible d orbitals There are 7 possible f orbitals Each orbital can only hold ____electrons.

Electrons usually occupy the ________energy levels available in an atom In any level, the _____ orbital has the lowest energy. The p orbital has slightly more energy The _____ orbital has slightly more than the p The ______ has the greatest energy.

Valence Electrons An electron in the outmost energy level is a __________ electron. Valence electrons determine the atom’s reactivity with other atoms.

Energy Levels First Energy Level Second Energy Level closest to nucleus contains one sublevel (s) contains only 2 electrons Second Energy Level Contains 2 sublevels (s & p) 1 s orbital & 3 p orbitals 8 total electrons

Third Energy Level Fourth Energy Level 3 sublevels (s, p, d) 1 s orbital, 3 p orbitals, & 5 d orbitals ______total electrons Fourth Energy Level 4 sublevels (s, p, d, f) 1 s orbital, 3 p orbitals, 5 d orbitals, & 7 f orbitals

Chapter 3 Section 2: The Periodic Table The periodic table groups __________ elements together. Makes it easier to predict the properties of an element based on its location on the table. The order is based on the # of protons in atom of that element has in it nucleus.

The Periodic Law States that when elements are arranged this way similarities in their properties will occur in a regular pattern

Atomic # Protons Neutrons Electrons Atomic Mass 8 16 18 26 17 31 23 10

Organization of the Periodic Table Horizontal Rows in the periodic table are called _________. The number of protons increases by 1 as you move from left to right. Vertical Columns are called ________. Elements in the same group have the same number of ___________ electrons Valence electrons determine the chemical properties of elements

Reactivity & Ionization Elements in Group 1 are reactive because their outermost levels are ________filled by electrons. Example: Hydrogen (only 1 electron) Atoms that don’t have their outermost energy levels filled may undergo Ionization They may gain or lose valence electrons Atoms are called __________.

When an atom loses an electron it becomes a __________. (positive ion) Ex. Li+ When an atom gains an electron it becomes an __________. (negative ion) Ex. Fl- Isotopes vary in the number of neutrons Example: Carbon 14

The Mass of an Atom An atomic mass unit (amu) is equal to 1/12th the mass of a carbon-12 atom An element’s average atomic mass is a weighted average of the masses of its naturally occurring isotopes.

Chapter 3 Section 3: Groups of Elements Members of the same “Group” have many similar chemical & physical properties because they have the same # of _______________ electrons Elements are classified in 2 main categories: _________________

Nonmetals & their compounds are plentiful on Earth. Elements with properties similar to metals & nonmetals are called _________________or Semiconductors. Nonmetals & their compounds are plentiful on Earth. Ex. Oxygen, Nitrogen, & Sulfur

Halogens & Noble Gases Halogens (Group 17) Noble Gases (Group 18) Example: Chlorine Noble Gases (Group 18) Examples: Neon & Helium Exist as single atoms instead of molecules Inert (Unreactive) Outer level is filled with electrons Do not gain or lose electrons Do not join to create compounds under normal conditions

Chp. 3 Sec 4: Moles The Mole is useful for counting _________ particles. Large counting unit Abbreviate mol 6022213670000000000000000 = 6.022 X 1023

6.022 X 1023 = 1 mol of a pure substance Avogadro’s Constant 6.022 X 1023 = 1 mol of a pure substance Molar Mass = The mass in grams of 1 mol of a substance

Conversion Factors A ratio equal to one that expresses the same quantity in 2 ways.