the periodic table

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THE PERIODIC TABLE Mr. Nelson Chemistry

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Mr. Nelson Chemistry. The Periodic Table. Periodic Table. Group – Vertical columns on PT Period – Horizontal rows on PT. Main-Group Elements. Groups 1 , 2 , and 13-18. Main-Group Elements. - PowerPoint PPT Presentation

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Page 1: The Periodic Table

THE PERIODIC TABLE

Mr. NelsonChemistry

Page 2: The Periodic Table
Page 3: The Periodic Table

Periodic Table

Group – Vertical columns on PT Period – Horizontal rows on PT

Page 4: The Periodic Table

Main-Group Elements

Groups 1, 2, and 13-18

Page 5: The Periodic Table

Main-Group Elements

The chemical properties of the main-group elements depends on their number of valence electrons

Valence electrons are the outermost electrons involved in chemical bonding

Page 6: The Periodic Table

Valence Electrons & Chemical Properties Each group of the main-group

elements has the same number of valence electrons

Each element wants to be as stable as possible

All main-group elements want a full shell of electrons, which is 8 valence electrons

Page 7: The Periodic Table

Valence Electrons & Chemical Properties Each group forms ions based on

the easiest way to obtain this full shell

Also known as the octet rule

Page 8: The Periodic Table

Family Groups

Noble Gases (Group 18) Examples: Ne, Xe Description:

stable, unreactive group of gases

Number of Valence Electrons: 8

Forms NO ions

Page 9: The Periodic Table

Family Groups

Halogens (Group 17) Examples: F, Cl Description: Highly reactive group of gases

Number of Valence Electrons: 7

Forms 1- ions

Page 10: The Periodic Table

Family Groups

Alkali Metals (Group 1) Examples: Na, K (not H) Description: Highly reactive group of metals

Number of Valence Electrons: 1

Forms 1+ ions

Page 11: The Periodic Table

Brainiac Movie

Page 12: The Periodic Table

Family Groups

Alkaline-Earth Metals (Group 2) Examples: Be, Mg Description: Slightly less reactive group

than alkali metals Number of Valence Electrons: 2 Forms 2+ ions

Page 13: The Periodic Table

Family Groups

Transition Metals (Group 3 – 12) Examples: Fe, Au, Ag Description: Fairly stable group of metals Forms multiple ions

Page 14: The Periodic Table

Family Groups

Lanthanides & Actinides Location: Bottom 2 periods of PT Description: Heavy metals, synthetics,

radioactive

Page 15: The Periodic Table

States of Matter

Metals and Nonmetals (Staircase)

Page 16: The Periodic Table

SECTION NEEDS TO BE REDONE

WITH THE GROUP/PERIOD

TRENDS OUTLINED FIRST!!!!!!!!!!!!!!!!

!!!!!

Page 17: The Periodic Table

Periodic Table Trends

Atomic Size Definition: The volume occupied by

the electrons around a nucleus Period Trend

Caused by: Increasing Effective Nuclear Charge

Page 18: The Periodic Table

Atomic Size

Effective nuclear charge is the amount of charge felt by outer electrons in an atom

Group trend Caused by: Increasing electron energy

levels

Page 19: The Periodic Table

Ionization Energy

Definition: The amount of energy required to remove one electron Period trend

Caused by: Inc. Effective Nuclear Charge

Page 20: The Periodic Table

Ionization Energy

Group trend Caused by: Electron shielding Electron shielding occurs when inner

electrons shield outer electrons from the pull of the nucleus

Page 21: The Periodic Table

Electron Affinity

Definition: The attraction of an atom for an electron

Period Trend Caused by: Inc. Eff. Nuclear

Charge

Page 22: The Periodic Table

Electron Affinity

Group trend Caused by: Inc. electron shielding

Page 23: The Periodic Table

Electronegativity

Definition: How much an atom in a chemical bond attracts electrons

Period trend Caused by: Inc. Eff. Nuclear

Charge

Page 24: The Periodic Table

Electronegativity

Group trend Caused by: Electron shielding/Inc. electron energy levels

Page 25: The Periodic Table

Electron shielding

Electron energy levels

Effective Nuclear Charge

Page 26: The Periodic Table
Page 27: The Periodic Table

Filling Electron Orbitals

Orbitals are the area in space where electrons are found Each individual orbital holds 2 electrons

There are four main shapes which hold a different number of electrons

Page 28: The Periodic Table

Shapes of Orbitals

The four shapes are s, p, d, and f

Page 29: The Periodic Table

Shapes of the Orbitals

Each shape holds a different number of orbitals s has 1 orbital, p has 3 orbitals, and d has 5 orbitals

www.ptable.com

Page 30: The Periodic Table
Page 31: The Periodic Table

Energy Levels Each period

is a new energy level Like an

elevator, electrons cannot exist between energy levels!

Page 32: The Periodic Table

General Rules

Aufbau Principle – Electrons fill lowest energy level first Analogy: Lazy Tenant Rule

Page 33: The Periodic Table

General Rules

Pauli Exclusion Principle – Electrons must have opposite spin (up/down) when in the same orbital

Analogy: Yin and Yang Rule

Page 34: The Periodic Table

General Rules

Hund’s Rule – Electrons in equal energy orbits fill orbitals with parallel spin Analogy: Empty Bus Seat Rule

Page 35: The Periodic Table
Page 36: The Periodic Table

Orbital Notation

Specific order for filling electrons – based on periodic table

Examples Beryllium

Oxygen

Page 37: The Periodic Table

Orbital Notation

Examples O2-

Titanium

Page 38: The Periodic Table

Electron Configuration

Examples Silicon

Selenium

Manganese

Page 39: The Periodic Table

Shorthand Electron Config

Shorter version of writing electron configurations Noble Gas Core

– inner core of electrons not involved in chemical bonding

Page 40: The Periodic Table

Shorthand Electron Config