Download unit 4b hw packet File

Chemistry
Unit #4-B Plan (Electrons in Atoms)
Name ____________________
I. Assignments / Handouts
A)
Terms, equations and formulas (info --- pg 2)
B)
Electromagnetic spectrum / Aufbau diagram (info --- pg 3-4)
C)
Chapter 5 textbook assignement (required --- pg 5-6)
D)
Homework problems (required --- pg 7-8)
E)
Spectral Analysis Lab
II.
Text Support
III.
Learning Targets (I can …)
A)
Compare and contrast different regions of the electromagnetic spectrum.
B)
Describe how spectral lines can be used to identify elements and reveal
information about the electron structure of elements.
C)
Visualize the relationship between the movement of electrons within an
atom and light.
D)
Draw orbital diagrams and write electron configurations for atoms.
E)
Distinguish between ground state and excited state electrons.
F)
Identify the usefulness and limitations of various models of the atom
(shells, rings, energy levels, electron cloud, …)
IV.
Tentative schedule
Fri
10/26 Flames of different colors
Electromagnetic spectrum
Line spectra of elements - connection to energy levels in atoms
Prep spectral analysis lab
10/29 Spectral analysis lab
10/30 Electron hotel
Electron configurations
10/31 Electron configurations
11/1 Quiz; unit 4b hw packet due
Quarter #1 final exam review guide
Mon
Tue
Wed
Thu
 Read chapter 5 pg 132-139 (atomic structure review)
 Study chapter 5 pg 140-161 (electrons in atoms)
On-Line Text: www.lab-aids.com
Username:
evhs1
Password:
smeyer
(Log in as student in upper right corner. This is a common username and
password for all my chemistry students.)
Week of 11/5 – 11/9 Quarter #1 final exam / prep
V.
Terms (to assist with writing electron configurations)
1.
Orbital – place where electrons are likely to be found.
2.
Node – place where electrons are not found.
3.
Aufbau principle – electrons fill lowest energy levels first.
4.
Pauli exclusion principle – maximum of 2 electrons in one orbital. Two
electrons in one orbital will have opposite electron spin.
5.
Hund’s rule – electrons filling an orbital set will have same spin and fill
different orbitals until the orbital set is half full.
6.
Heisenberg uncertainty principle – can not know exact momentum (speed)
and location of an object at the same time. This applies to very small
objects such as electrons.
7.
Wave nature – explains diffraction of an electron.
8.
Particle nature – massless particles called photons carry energy.
9.
Ground state – lowest energy state of an atom
10.
Excited state – state in which an atom has higher potential energy than its
ground state.
VI.
Terms (to assist with using the electromagnetic spectrum)
1. Electromagnetic radiation – a form of energy that exhibits wavelength
characteristics as it travels through space
2. Electromagnetic spectrum – all the forms of electromagnetic radiation
Visible range of electromagnetic spectrum
 4.3 x 1014 hertz (red) – 7.5 x 1014 hertz (blue)
 700 nanometers (red) – 400 nanometers (blue)
3. Energy (E) – the ability to do work or produce change
(measured in kilocalories/mol, kilojoules/mol, electron volts, etc)
4. Frequency (ν) – the number of waves that pass a given point in a specific time
(measured in hertz or cycles/second)
5. Wavelength (λ) - the distance between corresponding points on adjacent
waves (measured in meters, centimeters, nanometers, etc.
Hint: If energy increases; then frequency increases and wavelength decreases
If energy decreases; then frequency decreases and wavelength increases
On-line support
 ChemTeam
www.chemteam.info (see section on “electrons in atoms”)
This website may help you in your quest to understand chemistry. Explanations can get
quite involved – depending on the topic. It may be helpful at the introductory level. It will
be especially helpful if you are looking for extra detail.
Posted Answers on Moodle
Answers to some problems in the homework packet are posted on my “chemistry”
moodle site. Please check in the back of your classroom for “the work” behind these
answers.
Access this site at http://learn.district196.org . Choose High School /Eastview / Chemistry.
(Currently it’s an open site – anyone may log in as a guest.)
Name _______________________________
Atomic Structure Book Assignment (Chapter 5 – pages 140-161)
1. What is the “electron cloud”?
2. The charge on an atom is neutral; meaning # of protons _________ # of
electrons.
3. What is gained, lost, or shared when atoms form chemical bonds?
4. When an atom loses electrons; it forms ions with a _____________ charge.
5. When an atom gains electrons; it forms ions with a _____________ charge.
6. According to quantum theory; which of the following statements are
true?
a. Electrons are arranged in an atom in a manner which maximizes
stability (or minimizes energy).
b. More than 1 electron can have the same quantum state at the same
time.
c. Electrons are found in distinct quantum states that correspond to
distinct amounts of energy.
7. True or False: According to quantum theory; the mass, size, and location
of an electron is spread out into a wave.
8. __________________ is the rate at which an oscillation repeats.
9. __________________ is the distance between any 2 successive points of a
wave.
10. What is a photon?
11. What letters represent the 4 main spatial shapes?
12. What is the Pauli exclusion principle?
13. What is the maximum number of electrons that can be held by each
shape in an energy level?
a. s =
b. p =
c. d =
d. f =
14. Write the electron configuration for silicon.
15. Which of the following statements about the electromagnetic spectrum
are true?
a. Visible light occupies the majority of the electromagnetic
spectrum.
b. Violet light has more energy than red light.
c. Violet light has a longer wavelength than red light.
d. UV (ultraviolet) light has a higher frequency than visible light.
16. Why does each element have its own unique set of spectral lines?
Homework Problems
Name __________________________
Part II – Electron Configurations and Orbital Diagrams
1. Fill in the electron orbital diagram for the following atoms. Assume all atoms are in
their ground state.
A. O (Oxygen)
B. Ar
C. Mg
D. Mn
E. F
2. What atom is represented by each orbital diagram?
A.
B.
C.
D.
E.
3. Write the electron configurations for the following atoms or ions.
A. K
B. Sr
C. Bi
D. Re
E. Br
4. What atom is represented by each electron configuration?
A.
1s22s22p63s23p5
B.
1s22s1
C.
1s22s24d1
D.
Xe6s24f145d106p3
E.
Kr5s1
Multiple Choice - Choose the best answer.
1.
1s22s22p63s23p4 is the ground state electron configuration for which atom?
a.
b.
c.
d.
e.
2.
1s22s22p63s23p6 is the ground state electron configuration for which atom?
a.
b.
c.
d.
e.
3.
8.
1s2 2s2p6 3s2
1s2 2s2p6 3s1
1s2 2s2p6
1s2 2s2p5
1s2 2s22p3
Which electron configuration corresponds to a mercury atom at ground state?
a.
b.
c.
d.
e.
7.
Si
P
Cs
Rb
Mg
Which electron configuration corresponds to a nitrogen atom at ground state?
a.
b.
c.
d.
e.
6.
Te
Se
S
Kr
Sr
1s22s22p63s23p25s1 is an excited state electron configuration for which atom?
a.
b.
c.
d.
e.
5.
N
Se
S
Ar
F
[Ar]4s23d104p4 is the ground state electron configuration for which atom?
a.
b.
c.
d.
e.
4.
N
Se
S
Ar
F
[Xe]6s25d10
[Xe]6s24f145d46p6
[Xe]6s26f146d10
[Xe]6s24f145d10
[Xe]6s25f145d10
Which of the electron configurations would represent an alkali metal?
a. 1s2 2s22p6 3s2
b. 1s2 2s22p6 3s1
c. 1s2 2s22p6
d. 1s2 2s22p5
e. 1s2 2s22p3
Which of the following atoms has no unpaired electrons?
a. Na
b. Mg
c. C
d. P