Starter S-44

A. What is Lithium’s electron configuration?

B. What column of the periodic table is it in?

C. What is Sodium’s electron configuration?

D. What column of the periodic table is it in?

The Periodic Table

Chapter 6

6.1 Organization of the Elements

Chapter 6

In ancient times the known elements wereGold, Silver, Copper, Iron, Lead, Tin,

Mercury, Sulfur, Carbon

Up until the 1700’s only 4 more had been discoveredArsenic, Antimony, Phosphorus, Zinc

6.1 Organization of the Elements

1829 JW Dobereiner – puts elements in triads

Sets of 3 elements with similar chemical properties

6.1 Organization of the Elements

1864 John Newland – Law of Octets

When elements are placed in order of atomic mass, properties seem to repeat every 8 elements

6.1 Organization of the Elements

1869 – Dimitri Mendeleev – arranged by increasing atomic mass and properties

The table is periodic – properties repeat

6.1 Organization of the Elements

1913 – Henry Mosley – used atomic number instead of atomic mass

6.1 Organization of the Elements

The Periodic Law – when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

6.1 Organization of the Elements

Period – row

7 rows

6.1 Organization of the Elements

Group – column

18 groups (some have names)

6.1 Organization of the Elements

Alkali MetalsAlkaline Earth MetalsHalogensNoble GasesTransition Metals

Draw the zig-zag line on your periodic table and label the metals and nonmetals

6.1 Organization of the Elements

Metals

Good conductors, lusterous, ductile, malleable

6.1 Organization of the Elements

Nonmetals

Poor conductors, dull, brittle

6.1 Organization of the Elements

Metalloids

Sometimes behaves like a metal, sometimes like a nonmetal

6.1 Organization of the Elements

6.2 Classifying the Elements

Chapter 6

Information on the periodic table

Electron configuration is determined by the elements position on the periodic table

6.2 Classifying the Elements

s1

s2 p1 p2 p3 p4 p5

p6

d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

Remember

1st s is level one, 1st p is second, 1st d third

1st f fourth

6.2 Classifying the Elements

s1

s2 p1 p2 p3 p4 p5

p6

d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

6.2 Classifying the Elements

s1

s2 p1 p2 p3 p4 p5

p6

d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

Noble Gas Configuration

1. Find the noble gas before the element

2. Put that element in brackets [ ]

3. Fill out the rest of the configuration using the pattern in the periodic table

For example Strontium (Sr)

[Kr]5s2

6.2 Classifying the Elements

s1

s2 p1 p2 p3 p4 p5

p6

d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

Sr

Germanium (Ge)

[Ar]4s23d104p2

6.2 Classifying the Elements

s1

s2 p1 p2 p3 p4 p5

p6

d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

Ge

Starter S-45

What are the names of the elements in

1. Group 1

2. Group 2

3. Group 3-12

4. Group 17

5. Group 18

6.3 Periodic Trends

Chapter 6

6.3 Periodic TrendsAtomic Size – The size of an atom of a

particular element

Increases down a group

Decreases across a period

Video

6.3 Periodic TrendsNot always an exact pattern

6.3 Periodic Trends2. Ions – charged atoms

Lost (+) or gained (-) electrons

Cation – lost electrons

Anion – gained electrons

Ion Formation

Table of ionic radii

6.3 Periodic Trends3. Ionization Energy

The energy required to remove an electron from an atom

1st ionization energy – energy to remove the first electron

Decrease down a group

Increase across a period

Ionization energy video

6.3 Periodic Trends4. Electronegativity

Ability of an atom to attract electrons when the atom is in a compound

Increases across periodic table

Decreases down periodic table

6.3 Periodic Trends

6.3 Periodic Trends5. Density

6.3 Periodic Trends

6.3 Periodic Trends5. Melting Point

6.3 Periodic Trends

6.3 Periodic TrendsMain reasons for patterns

1. Increasing nuclear charge down a group and across a period

more protons, larger positive charge

2. Increased shielding down a group

as energy levels increase, those electrons further out, are shielded by the inner ones

6.3 Periodic Trends