chapter 6.1, 6.3 the periodic table

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Chapter 6.1, 6.3 The Periodic Table

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Chapter 6.1, 6.3 The Periodic Table. Day One Thursday October 27 th. Organization of the Elements. The Elements. As scientists learned more about the elements, they organized them in different ways…think about how a grocery store is organized. Organized by the properties of the elements - PowerPoint PPT Presentation

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Page 1: Chapter 6.1, 6.3  The Periodic Table

Chapter 6.1, 6.3 The Periodic Table

Page 2: Chapter 6.1, 6.3  The Periodic Table

ORGANIZATION OF THE ELEMENTS

Day OneThursday October 27th

Page 3: Chapter 6.1, 6.3  The Periodic Table

The Elements

• As scientists learned more about the elements, they organized them in different ways…think about how a grocery store is organized.– Organized by the properties of the elements

• So who came up with this wonderful Periodic Table of Elements?

Page 4: Chapter 6.1, 6.3  The Periodic Table

Antoine Lavoisier

• Made a list of all of the known elements at the time of the late 1700s.

• Industrial Revolution played a major role in the advancement of chemistry.

• Once we started using the same method for determining atomic mass, scientists could begin trying to understand the relationships among the elements.

Page 5: Chapter 6.1, 6.3  The Periodic Table

Organizing Elements Activity

• How did you arrange the elements?

– Trends in color (periods and groups)– Trends for mass (periods and groups)– Where would you put Fuchsia gas? Range for the

mass?– Properties for the element that would fill the last

remaining gap in the table?

Page 6: Chapter 6.1, 6.3  The Periodic Table

Xn Ad Tu Qa

Bp Pd Lq

Rx Cx Ax

The wavelength decreases across the period and color becomes lighter down the group.

The mass increases across the period and down the group. Cx does not fit the period trend for mass, but it fits in thethird column with other green brittle solids.

Ph would fit in the third period, first column based oncolor and stated trends. The mass would be between99-106g.

The remaining gap would be a yellow-colored liquid with a mass most likely between70g-82g.

Page 7: Chapter 6.1, 6.3  The Periodic Table

John Newlands 1865: English Chemist

• Arranged the known elements according to properties and in order of increasing atomic mass

• He noticed that all elements in a given row had similar properties and this pattern repeated every eight elements (Law of Octaves)– Patterns like this occur periodically (periodic table)

Page 8: Chapter 6.1, 6.3  The Periodic Table

Dmitri Mendeleev 1869: Russian Chemist

• Invented the first Periodic Table (my hero!)

• Organized the 63 known elements according to their properties and predicted elements not yet known to exist.

• Periodic Law: repeating physical and chemical properties change periodically with their atomic #

• Two interesting things came from this:1. Gaps2. Elements did not necessarily fit according to atomic mass

Page 9: Chapter 6.1, 6.3  The Periodic Table

Mayer

• Worked at the same time as Mendeleev, but didn’t get his work published quick enough to get credit for it.

• Demonstrated connection with element properties and atomic mass.

Page 10: Chapter 6.1, 6.3  The Periodic Table

Henry Mosley

• Discovered the problems with Mendeleev’s arrangement of the periodic table.

• Discovered that atoms contain a unique # of protons called the atomic #.

• Rearranged the elements in order of atomic # -which gave way to periodic patterns of the properties.

Page 11: Chapter 6.1, 6.3  The Periodic Table

The Periodic Table • Organized in rows and columns

– Rows = PERIODS – Columns = (GROUPS or FAMILIES)

• Each box is for all of the information for a single element.– Contains the name, symbol, atomic #, and atomic mass.

• Elements in groups 1,2, and 13-18 have a much larger range of chemical/physical properties. They often get called main group or representative elements.

• Groups 3-12 are referred to as transition elements.

Page 12: Chapter 6.1, 6.3  The Periodic Table

• www.learn360.com

– Power of the Periodic Table

Page 13: Chapter 6.1, 6.3  The Periodic Table

Page 49 Name of Group Location on the

Periodic Table Main Characteristics

Alkali

Alkaline Earth

Halogen

Noble

Transition

Page 14: Chapter 6.1, 6.3  The Periodic Table

FAMILIES DISCUSSION METAL/NONMETAL & ELECTRON CONFIGURATION

NOTES

Day Four Tuesday November 4th

Page 15: Chapter 6.1, 6.3  The Periodic Table

Discussion of Families Lab

• Let’s look at Mg, Ca, Ba. – What family are they in? – Do you notice any trends with reacting with

chemicals?

• Let’s look at Cl, Br, I. – What family are they in? – Do you notice any trends with reacting with

chemicals?

Page 16: Chapter 6.1, 6.3  The Periodic Table

Based on what we observed, which pairs of elements would you expect to behave similarly?

Scandium and Lawrencium

Rhodium and Silver

Potassium and Hydrogen

Neon and Carbon

Neon and Krypton Selenium and PoloniumActinium and Thorium

Germanium and Lead

Page 17: Chapter 6.1, 6.3  The Periodic Table

Characteristics of Metals/ Nonmetals

• Conducts electricity • Malleable (bends

without breaking) • Reacts with Acid

• Doesn’t conduct • Brittle • Doesn’t react with acid

Where are they located?

BAtMAN!!!!!

Page 18: Chapter 6.1, 6.3  The Periodic Table
Page 19: Chapter 6.1, 6.3  The Periodic Table

METAL/NONMETAL LAB M/NM & FAMILIES LAB W-UP

Day FiveWednesday November 5th

Page 20: Chapter 6.1, 6.3  The Periodic Table

Recording Data for Metal/Nonmetal Lab

1. (.) shiny

2. ( ) dull

3. (-) malleable

4. ( +) reacts with acid

Conductivity 4. ( ) bright light 5. ( ) dim light 6. (X) no light

Page 21: Chapter 6.1, 6.3  The Periodic Table

POSTER ON ELEMENTS

Day Nine and Ten Tuesday November 11th and Wednesday

November 12th