starter s-44 a. what is lithium’s electron configuration? b.what column of the periodic table is...
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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?
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The Periodic Table
Chapter 6
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6.1 Organization of the Elements
Chapter 6
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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
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1829 JW Dobereiner – puts elements in triads
Sets of 3 elements with similar chemical properties
6.1 Organization of the Elements
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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
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1869 – Dimitri Mendeleev – arranged by increasing atomic mass and properties
The table is periodic – properties repeat
6.1 Organization of the Elements
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1913 – Henry Mosley – used atomic number instead of atomic mass
6.1 Organization of the Elements
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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
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Period – row
7 rows
6.1 Organization of the Elements
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Group – column
18 groups (some have names)
6.1 Organization of the Elements
Alkali MetalsAlkaline Earth MetalsHalogensNoble GasesTransition Metals
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Draw the zig-zag line on your periodic table and label the metals and nonmetals
6.1 Organization of the Elements
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Metals
Good conductors, lusterous, ductile, malleable
6.1 Organization of the Elements
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Nonmetals
Poor conductors, dull, brittle
6.1 Organization of the Elements
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Metalloids
Sometimes behaves like a metal, sometimes like a nonmetal
6.1 Organization of the Elements
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6.2 Classifying the Elements
Chapter 6
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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
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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
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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
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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
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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
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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
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6.3 Periodic Trends
Chapter 6
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6.3 Periodic TrendsAtomic Size – The size of an atom of a
particular element
Increases down a group
Decreases across a period
Video
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6.3 Periodic TrendsNot always an exact pattern
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6.3 Periodic Trends2. Ions – charged atoms
Lost (+) or gained (-) electrons
Cation – lost electrons
Anion – gained electrons
Ion Formation
Table of ionic radii
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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
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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
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6.3 Periodic Trends5. Density
6.3 Periodic Trends
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6.3 Periodic Trends5. Melting Point
6.3 Periodic Trends
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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