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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
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 __________.
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 –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– 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–______total electrons
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
8 16
18 26
17 31
23 10
Atomic # Protons Neutrons Electrons Atomic Mass
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:__________________________________
Elements with properties similar to metals & nonmetals are called _________________or Semiconductors.
Nonmetals & their compounds are plentiful on Earth.Ex. Oxygen, Nitrogen, & Sulfur
Halogens & Noble GasesHalogens (Group 17)
Example: Chlorine
Noble Gases (Group 18)Examples: Neon & HeliumExist as single atoms instead of molecules
Inert (Unreactive)Outer level is filled with electrons Do not gain or lose electronsDo not join to create compounds under normal
conditions
Chp. 3 Sec 4: MolesChp. 3 Sec 4: MolesThe Mole is useful for counting
_________ particles.
Large counting unit
Abbreviate mol
6022213670000000000000000 =
6.022 X 1023
Avogadro’s ConstantAvogadro’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 FactorsConversion Factors
A ratio equal to one that expresses the same quantity in 2 ways.