Transcript ExtraReviewDay10.16

Unit 2 Extra Practice
October 15 (ODD)
October 16 (EVEN)
Do Now (5 min)
1. How much energy is given off by an electron
emitting a wave with a frequency of 7 x 1014 Hz?
2. As the wavelength of light increases,
A. The frequency increases
B. The speed of light increases
C. The energy decreases
D. The intensity increases
Justify your answer with a diagram. Use p. 139 as needed.
Announcements
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OWN Your Education
Office hours Wednesday and Friday
All makeup work due Monday 10/22
Unit 2 exam and quiz schedule:
Exam 2
Monday 10/22 (ODD)
Tuesday 10/23 (EVEN)
Review Questions
If you work efficiently, we may have
time to play a jeopardy game at the
end of class 
Bohr Model vs. Quantum Model
Questions (10 min)
Answer the questions from the sheet on a separate sheet
of paper that you will turn in at the end of class.
 (5 min)
 How many electrons are needed to fill the
first, second, and third principal energy
levels in the Bohr Model of the atom?
 Draw the Bohr Models for Aluminum and
Neon.
 What is an “orbital” (in the Quantum
Mechanical Model)? How is it different than
an “orbit” (in the Bohr Model)?
 How does the Bohr Model of the atom
differ from the Quantum Mechanical Model?
List at least three ways.
 (5 min)
 How many electrons can fit into the s, p,
and d sublevels? How is this information
shown on the periodic table?
 How many orbitals do the s, p, d, and f
sublevels have? What is the relationship
between the number of orbitals a sublevel
has and the number of electrons that
sublevel can hold?
 How is the amount of an energy an electron
has related to the orbit(al) that electron is in
(in both the Bohr Model and Quantum
Mechanical Model of the atom)
Electron Configuration
Questions (10 min)
Answer the questions from the sheet on a separate sheet
of paper that you will turn in at the end of class.
 (5 min)
 Make a rough sketch of the periodic
table and label the different sections:
s, p, d, and f.
 What do the 1, s, and 2 mean,
respectively, in this electron
configuration: 1s2?
 Write electron configurations for the
following elements: Lithium, Carbon,
Neon, Silicon, Iron.
 (5 min)
 Write the Noble Gas Configuration
(shortcut) configurations for Silicon and
Iron.
 Write electron configurations for elements
with the following numbers of electrons: 4,
7, 16.
 Where on the periodic table would you
expect to find an element whose groundstate electron configuration ended in 4p5?
3s1?
Orbital Diagram Questions
(10 min)
Answer the questions from the sheet on a separate sheet
of paper that you will turn in at the end of class.
1. How many boxes do the s, p, and d
sublevels get? How do these numbers
compare to the number of orbitals in
those sublevels?
2. Identify the problem in each of the
following orbital diagrams. Which rule(s)
is(are) being violated?
a.
b.
d.
1.
Write the symbol for the elements with the
following orbital diagrams:
How many unpaired electrons
(single electrons in an orbital) do
each of the following elements
have: Na, Ca, O?
Groups, Families and Valence
Electron Questions
(10 min)
Answer the questions from the sheet on a separate sheet
of paper that you will turn in at the end of class.
 How is the Periodic Table organized?
 Describe in 5 words or less where to find each of
the following on the periodic table: Metals,
Nonmetals, Metalloids (semi-metals).
 List three common physical properties of metals.
Do the same for nonmetals.
 Match the following families (groups) to their
columns on the periodic table:





Halogens
Noble Gases
Alkali Metals
Alkaline Earth Metals
Transition Metals (list the range of columns)
 Are the elements in a group (column) or period (row)
on the periodic table more similar to each other?
Explain.
 How does reactivity change as you go down the
periodic table? Which element is more reactive than
potassium, but less reactive than Cesium?
 What family would elements with the following
electron configuration belong to:
 1s2 2s2
 1s2 2s2 2p5
 1s2 2s2 2p6
 [Ne] 3s1
 [Ne] 3s2 3p6
 [Ar] 4s2 3d6
 What is a valence electron? Where can
you look on the periodic table to
figure out how many valence
electrons an element has?
 How many valence electrons do the
following elements have: Sodium,
Calcium, Neon, Fluorine, Chlorine,
Oxygen, Phosphorous?
Periodic Trends Questions
(10 min)
Answer the questions from the sheet on a separate sheet
of paper that you will turn in at the end of class.
Periodic Trends Questions
 Define electronegativity, atomic radius, and ionization
energy.
 How does electronegativity vary from left to right on
the periodic table?
 How does atomic radius vary across a period and
down a group in the table?
 Which two atomic properties have similar trends?
Offer a possible explanation for this similarity.
 Why do noble gases have the highest ionization
energy?
 Which is more reactive? Lithium or Potassium?
Oxygen or Fluorine?
Electromagnetic Spectrum
Questions
(10 min)
Answer the questions from the sheet on a separate sheet
of paper that you will turn in at the end of class.
Electromagnetic Spectrum
 Write the equation relating the speed of light with
frequency and wavelength. Write the equation
relating energy and frequency. Label the variables in
each.
 The speed of light always equals ____________.
 Answer questions #11-14 on p. 157.
 Which has more energy, a radio wave or a gamma
ray?
 If a radio wave has a frequency of 106 Hz, what is its
wavelength? How much energy does it carry?
 If purple light has a wavelength of 4.00 x 10-7 m, how
much energy does it have?
Atom Models
Electron
Configuration
Orbital
Diagram
Periodic
Table/Trends
Electromagnetic
Spectrum
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Name the 4 orbitals and
describe the shapes – 10
Points
Sodium (Na) has how
many electrons in the third
energy level? – 20 Points
Copper has how many
electrons in the 3d
sublevel? – 30 Points
Draw the Bohr model for
Argon (Ar)– 40 Points
Draw the quantum model
for Neon– 50 Points
What is the electron
configuration for Neon
(Ne) – 10 Points
Write the electron
configuration for an
element that would have
14 protons – 20 Points
Silicon has an electron
configuration of
1s22s22p63s23p2. How
many electrons does
silicon have in its highest
sublevel? – 30 Points
Write the electron
configuration for Bromine
(Br) – 40 Points
Which element would have
the following shortcut
electron configuration:
[Ar]4s23d104p4– 50 Points
Which rule is being
violated in the orbital
diagram below? – 10
Points
    _  _
1s
2s
2p
3s
Which element is
represented by the
following orbital diagram –
20 Points
        
1s
2s
2p
3s
3p
Which rule is being
violated in the orbital
diagram below? – 30
Points
        
1s
2s
2p
3s
3p
Which rule is being
violated in the orbital
diagram below?– 40 Points
        ___
1s
2s
2p
3s
3p
Draw the orbital diagram
for Silicon – 50 Points
What are the rows and
columns called in the
periodic table – 10 Points
Which has the greater
Ionization Energy?
Electronegativity? Atomic
radius? Fluorine or
Oxygen?– 20 Points
If I am an element that is
shiny, hard, and a good
conductor of heat and
electricity, what kind of
element am I? – 30 Points
If I react vigorously with
water, what family am I in
and where can you find me
on the periodic table and
how many valence
electrons do I have? – 40
Points
What family does the
following element belong
to and how many valence
electrons does it have:
1s22s22p63s23s5– 50 Points
What is the wavelength for
a wave with a frequency of
2 x 103 Hz– 10 Points
What is the frequency for a
wave with a wavelength of
100 m – 20 Points
What is the energy if the
frequency is 4 x 1010 Hz? –
30 Points
What is the frequency if
the energy is 2 x 10-19?– 40
Points
What is my energy if my
wavelength is 300 m– 50
Points