catalyst – september 1s 2 2s 2 2p 6 3s 2 3p 4 , 2010
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Catalyst – September 1s 2 2s 2 2p 6 3s 2 3p 4 , 2010. Review the electron configurations that you saw yesterday: Mg-1s 2 2s 2 2p 6 3s 2 Ne- 1s 2 2s 2 2p 6 Si- 1s 2 2s 2 2p 6 3s 2 3p 2 K- 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1. Now, write the electron configurations for… Iron (Fe) Oxygen (O). - PowerPoint PPT PresentationTRANSCRIPT
Catalyst – September 1s22s22p63s23p4, 2010
Review the electron configurations that you saw yesterday: Mg-1s22s22p63s2 Ne- 1s22s22p6
Si- 1s22s22p63s23p2
K- 1s22s22p63s23p64s1
Now, write the electron configurations for…
1. Iron (Fe)2. Oxygen (O)
Today’s Agenda
CatalystNoble Gas ConfigurationPeriodic TrendsWork TimeExit Question
Today’s Objectives
SWBAT write noble gas configurations for elements.
SWBAT describe the periodic trends for atomic radius and electronegativity.
Practice Problems: Electron Configuration
Be: 1s22s2
Ne: 1s22s22p6
Br: 1s22s22p63s23p64s23d104p5
Practice Problems: Electron Configuration
C: 1s22s22p2
Ca: 1s22s22p63s23p64s2
As: 1s22s22p63s23p64s23d104p3
Practice Problems: Electron Configuration
1s22s22p23s23p64s23d104p64s24d105p5: I (Iodine)
1s22s22p63s23p64s23d8: Ni
1s22s22p63s23p64s23d104p6
5s2 4d105p66s1: Cs
Noble Gas Configuration
Scientists are WAY too lazy to write all
that mess!
Electron ConfigurationFIGURE IT OUT YOURSELF!!!
Ba – [Xe]6s2
P – [Ne]3s23p3 Y – [Kr]5s24d1
Si-Rb-
Key Point #4: Noble Gas configuration starts with noble gas BEFORE the atom you are going to.
Noble Gas Configuration
Electron Configuration
Ag (instead of Hg)
Electron Configuration
Ag – [Kr]
Electron Configuration
Ag – [Kr]5s2
Electron Configuration
Ag – [Kr]5s24d9
Electron Configuration
S
Electron Configuration
S – [Ne]
Electron Configuration
S – [Ne]3s2
Electron Configuration
S – [Ne]3s23p4
Electron Configuration
Sm
Electron Configuration
Sm – [Xe]
Electron Configuration
Sm – [Xe]6s2
Electron Configuration
Sm – [Xe]6s25d14f5
PERIODIC TRENDS!!!VALENCE ELECTRONS
(CHECK!)ATOMIC RADIUS
ELECTRONEGATIVITY
Valence Electrons
Don’t forget!Valence electrons are the electrons in the outermost energy level.
Example
Electron configuration for silicon (Si): What is the highest energy level? So how many valence electrons?
1s22s22p63s23p2
2 + 2 = 4!
Valence Electrons
Valence Electron Trendson the Periodic Table
You have this in your notes – back of the
Periodic Table Basics
Notes!
What is Atomic Radius?
Key Point #1: Atomic radius is how big an atom is and is also known as atomic size
What is Electronegativity?
Key Point #2: Electronegativity is the ability of an atom to attract electrons to itself in a chemical bond
How much an atom wants electrons
So as you go LEFT to RIGHT… Key Point #3: As you move left to right across the periodic table, positive charge increases so… ELECTRONEGATIVITY INCREASES
Therefore, ATOMIC RADIUS DECREASES
Electronegativity Trends
On the Diag….onal
So as you go from TOP to BOTTOM…
Key Point #4: As you go from top to bottom on the periodic table, energy levels (shells) increase so… ATOMIC RADIUS INCREASES Therefore, ELECTRONEGATIVITY DECREASES
Electronegativity Trends
How are atomic radius and electronegativity related?
Key Point #5: Atomic radius and electronegativity are indirectly/inversely related.
ELECTRONEGATIVITY
ATOMIC RADIUS
Why is this relationship true? Atoms with HIGH
ELECTRONEGATIVITIES hold their electrons very close!
Sooooo, the atomic radius decreases High or low
electronegativity?
Large or small atomic size?
Why is this relationship true? Atoms with LARGE RADII can’t pull on
their electrons as much Soooo, ELECTRONEGATIVITY decreases!
Practice Problems
Rank the following elements in order of increasing atomic radius based on location on the periodic table (smallest to biggest)
Fr, Sc, P, Pd
F, As, Tl, S
P, Sc, Pd, Fr
Fluorine, Sulfur, Arsenic, Thallium
Practice Problems
Rank the following elements in order of increasing electronegativity based on location on the periodic table (smallest to biggest)
Mg, Sr, Be, Ra
Cl, Si, Al, S, P
Radon, Strontium, Magnesium, BerylliumAluminum, Silicon, Phosphorus, Sulfur, Chlorine
More Practice!
1. T or F? Atomic size decreases as you move right across the periodic table.
2. T or F? As you move down the Periodic Table, atoms get smaller.
3. Rank the following sets of elements in order of increasing atomic size (small big).
Set A: Bh, Mn, Re, Tc Set B: Sb, I, Ag, Ru Set C: Y, Ti, Sg, Ta
4. Rank the following sets of elements in order of decreasing atomic size (big small).Set A: Cl, At, I, F, Br Set B: Te, Xe, Sn, In
Set C: Rb, K, Sr, Ca
More Practice!
1. T or F? Electronegativity decreases as you move left across the periodic table.
2. T or F? As you move down the Periodic Table, atoms get more electronegative.
3. Rank the following sets of elements in order of increasing electronegativity (small big).
Set A: Bh, Mn, Re, Tc Set B: Sb, I, Ag, Ru Set C: Y, Ti, Sg, Ta
4. Rank the following sets of elements in order of decreasing electronegativity (big small).Set A: Cl, At, I, F, Br Set B: Te, Xe, Sn, In
Set C: Rb, K, Sr, Ca
GROUP WORK TIME!
Exit Question
1. Which element has atoms with the smallest radius: Cl, Se, P, or F?
2. Which element has the largest electronegativity: Ag, Cu, Hg, or Zn?
3. How are atomic radius and electronegativity related?