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Launch Grab your binder and immediately take a seat
Answer the following questions:
1. Using arrows, draw the trend for atomic radius.
2. Which atoms below have a larger atomic radius than aluminum (Al)?
i) Cl iii) Si v) Na
ii) B iv) He vi) Ca
Weekly Schedule Monday: Atomic Radius
Tuesday: Electronegativity & Ionization Energy
Wednesday: Metals, nonmetals, special groups
Thursday: Atomic structure & nuclear processes
Friday: Mid-Term Exam
We don’t have much time!
If you don’t understand something, ask!
What is the trend in ionization energy/electronegativity?
Mr. Heffner 10/13/09
Ionization Energy Ionization energy is…
how much energy it takes to steal an electron
Electronegativity Electronegativity is…
how good an atom is at stealing electrons
Ionization Energy/Electronegativity
The trend: 1. IE/E increases across a period (LR)
2. IE/E decreases down a group (Top Bottom)
Dec
reas
es
Increases
Example #1 Which has higher amount of ionization energy,
oxygen (O) or carbon (C)?
Step #1: Find the elements
Example Which has higher amount of ionization energy,
oxygen (O) or carbon (C)?
Step #2: Look at the keywords
Which has a higher amount of ionization energy,
oxygen (O) or carbon (C)?
Example Which has higher amount of ionization energy,
oxygen (O) or carbon (C)?
Step #3: Identify which is closest to He
Example Which is less electronegative,
Beryllium (Be) or potassium (K)?
Step #1: Find the elements
Example Which is less electronegative,
Beryllium (Be) or potassium (K)?
Step #2: Look at the keyword
Which is less electronegative,
Beryllium (Be) or potassium (K)?
Example Which is less electronegative,
Beryllium (Be) or potassium (K)?
Step #3: Identify which is closest to Fr
Practice Questions Review Worksheet #2
Use the 3-step method!
Ionization Energy/Electronegativity
The trend: 1. IE/E increases across a period (LR)
2. IE/E decreases down a group (Top Bottom)
Dec
reas
es
Increases
Atomic Radius The trend:
1. Atomic radius decreases across a period (LR)
2. Atomic radius increases down a group (Top Bottom)
Incr
ease
s
Decreases
Exit Slip 1. Which of the following atoms has the largest
atomic radius? a. oxygen (O) b. phosphorus (P) c. sulfur (S)
d. chlorine (Cl)
Exit Slip 2. In general, how does ionization energy vary
throughout the periodic table? a. it decreases across a period from left to right, and
decreases down a group from top to bottom b. it increases across a period from left to right, and
increases down a group from top to bottom c. it increases across a period from left to right, and
decreases down a group from top to bottom d. It decreases across a period from left to right, and
increases down a group from top to bottom
Exit Slip 3. Which of the following atoms has the smallest first
ionization energy? a. lithium (Li) b. beryllium (Be) c. sodium (Na)
d. potassium (K)
Exit Slip 4. Electronegativity is the
a. energy it takes to remove an electron from an atom. b. number of protons and neutrons in an atom.
c. measure of how good an atom is at stealing electrons.
d. distance from the nucleus to the valence ring.
Exit Slip 5. Which of the following correctly lists the elements
in order of increasing electronegativity (least to most)?
a. O < P < Al < Na
b. Na < Al < P < O c. P < O < Na < Al
d. Al < P < O < Na
Homework Finish Review Worksheet #2
Make a mind map – double points! In center oval: “periodic trends” In 3 ovals around:
“atomic radius”
“electronegativity”
“ionization energy”
In 3 boxes for each: definition of term
trend
picture