sps4. students will investigate the arrangement of the periodic table

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.