Download Honors Chemistry Ms. K Pages 96

Name______________________ #_____
Period___
Honors Chemistry
Ms. K
Pages 96-131
Task Checklist:
Look at Online Textbook Materials
Look at Section 1 Visual Concepts
Look at Section 2 Visual Concepts
Look at Section 3 Visual Concepts
Take Section 1 Self-Check Quiz
Take Section 2 Self-Check Quiz
Take Section 3 Self-Check Quiz
Do the Protons and Neutrons Concept Map
Other Tasks
Read Section 1
Read Section 2
Read Section 3
Review Chapter Packet
Examine Class Website
Review PowerPoint
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
c = λν
Worksheet
E = hν
c: speed of light
λ: wavelength
ν: frequency
E: energy
h: Planck’s constant
1. If you suspected something as being ?Wavelike?, how could you prove it?
2. What are two characteristics that differentiate types of electromagnetic radiation?
3. Name one characteristic that all electromagnetic radiation have in common?
4. What is the speed of yellow light?
5. What is the frequency of a radio wave with a wavelength of 10.0 m?
6. What is the energy of an X-ray with a frequency of 1.0 x 1017 Hz?
7. If the wavelength of yellow light is 570. nm, what is the frequency of yellow light in Hertz?
8. What is the energy of blue light with a wavelength of 500.nm?
9. I sometimes listen to classical music on 89.3FM. What is the wavelength of the radio
ermine the frequency. See your notes.)
waves for this station? (The ?Call? numbers and the ?Band? help det
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d107p6
Write the ground state electron configuration for each of the following:
1. calcium
1. ______________________________________________________________
2. lithium
2. ______________________________________________________________
3. iron
3. ______________________________________________________________
4. sodium
4. ______________________________________________________________
5. oxygen
5. ______________________________________________________________
6. iodine
6. ______________________________________________________________
7. osmium
7. ______________________________________________________________
8. radium
8. ______________________________________________________________
9. fermium
9. ______________________________________________________________
10. argon
10. _____________________________________________________________
11. sulfide ion
11. _____________________________________________________________
12. calcium ion
12. _____________________________________________________________
13. chloride ion
13. _____________________________________________________________
14. hydrogen ion
14. _____________________________________________________________
Do you notice something strange about 10-13? We call these ?isoelectronic??remember this
term? If you don’t, can you figure out what it means by looking at 10-13?
Name the neutral atom that corresponds to the following electron configurations:
15. 1s22s22p63s23p64s23d104p2 __________
16. 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2 __________
17. 1s22s22p63s23p5 __________
18. 1s22s22p5 __________
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
1. Write the electron configurations for three things that are isoelectronic and provide their
symbols:
2. Write the most stable electron configurations for the following:
a. Nb
a. ______________________________________________________________
b. Mo
b. ______________________________________________________________
c. Cd
c. ______________________________________________________________
d. Ag
d. ______________________________________________________________
e. Sc+3
e. ______________________________________________________________
+2
f. Mn
f. ______________________________________________________________
3. Write the noble-gas notation (short-hand) for the following:
a. Ca
a. ______________________________________________________________
b. Cu
b. ______________________________________________________________
c. Cs
c. ______________________________________________________________
d. Cl
d. ______________________________________________________________
4. valence electrons ? the electrons available to be lost, gained, or shared in the formation of
chemical compounds
These are also the electrons in the highest energy level.
Example: Na: 1s22s22p63s1 Notice, the 3rd energy level is the highest occupied level, and it
contains one electron, thus, sodium has 1 valence electron.
Example: Se: 1s22s22p63s23p64s23d104p4 The 4th energy level is the highest occupied level, and it
contains 2 electrons in the 4s and 4 electrons in the 4p, thus Se has 6 valence electrons.
How many valence electrons are in the following atoms or ions?
a.
b.
c.
d.
Li _____
C _____
Kr _____
I _____
e.
f.
g.
h.
Mg _____
Al _____
As _____
S _____
i. F- _____
j. Na+_____
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
1. Write the electron configurations for three things that are isoelectronic and provide their
symbols:
2. Write the most stable electron configurations for the following:
a. Nb
a. ______________________________________________________________
b. Mo
b. ______________________________________________________________
c. Cd
c. ______________________________________________________________
d. Ag
d. ______________________________________________________________
e. Sc+3
e. ______________________________________________________________
+2
f. Mn
f. ______________________________________________________________
3. Write the noble-gas notation (short-hand) for the following:
a. Ca
a. ______________________________________________________________
b. Cu
b. ______________________________________________________________
c. Cs
c. ______________________________________________________________
d. Cl
d. ______________________________________________________________
4. valence electrons ? the electrons available to be lost, gained, or shared in the formation of
chemical compounds
These are also the electrons in the highest energy level.
Example: Na: 1s22s22p63s1 Notice, the 3rd energy level is the highest occupied level, and it
contains one electron, thus, sodium has 1 valence electron.
Example: Se: 1s22s22p63s23p64s23d104p4 The 4th energy level is the highest occupied level, and it
contains 2 electrons in the 4s and 4 electrons in the 4p, thus Se has 6 valence electrons.
How many valence electrons are in the following atoms or ions?
a.
b.
c.
d.
Li _____
C _____
Kr _____
I _____
e.
f.
g.
h.
Mg _____
Al _____
As _____
S _____
i. F- _____
j. Na+_____
Ms. K
Chemistry
Name_____________________________ #_____
Date______________________ Period_________
Niels Bohr Worksheet
Light and Energy Levels of the Atom
The quantum level occupied by an electron in an atom depends on the energy of the electron.
Changes in quantum level are related to absorption or emission of energy. The figure below represents
the four lowest energy levels of an atom. (n = 1 to 4). The six lettered arrows represent changes in the
energy level of an electron.
4
3
2
C
D
E
F
1
A
B
"And anyone who thinks they
can talk about quantum theory
without feeling dizzy hasn't yet
understood the first thing
about it."
– Niels Bohr
1. Why do these energy levels mean that the atom will show an emission spectrum of discrete lines
rather than a continuous spectrum of emitted light? ________________________________________
__________________________________________________________________________________
__________________________________________________________________________________
__________________________________________________________________________________
2. Which three of the lettered energy changes involve absorption of energy by the atom? __________
3. Which three of the lettered energy changes involve emission of light energy by the atom? _______
4. Of the three energy changes that involve emission , one results in the emission of blue light, one
results in yellow light, and one results in ultraviolet light.
a. Which lettered change involves the emission of blue light?
_____
b. Which lettered change involves the emission of yellow light?
_____
c. Which lettered change involves the emission of ultraviolet light?
_____
Name
Date
Class
CHAPTER 4 REVIEW
Arrangement of Electrons in Atoms
SECTION 1
SHORT ANSWER
Answer the following questions in the space provided.
1. In what way does the photoelectric effect support the particle theory of light?
2. What is the difference between the ground state and the excited state of an atom?
3. Under what circumstances can an atom emit a photon?
4. How can the energy levels of the atom be determined by measuring the light emitted from an
atom?
5. Why does electromagnetic radiation in the ultraviolet region represent a larger energy transition
than does radiation in the infrared region?
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ARRANGEMENT OF ELECTRONS IN ATOMS
25
Name
Date
Class
SECTION 1 continued
6. Which of the waves shown below has the higher frequency? (The scale is the same for each
drawing.) Explain your answer.
Wavelength
Wavelength
Wave A
Wave B
7. How many different photons of radiation were emitted from excited helium atoms to form the
spectrum shown below? Explain your answer.
Spectrum for helium
PROBLEMS
provided.
Write the answer on the line to the left. Show all your work in the space
8.
What is the frequency of light that has a wavelength of 310 nm?
9.
What is the wavelength of electromagnetic radiation if its frequency
is 3.2 102 Hz?
26
ARRANGEMENT OF ELECTRONS IN ATOMS
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Name
Date
Class
CHAPTER 4 REVIEW
Arrangement of Electrons in Atoms
SECTION 1
SHORT ANSWER
Answer the following questions in the space provided.
1. In what way does the photoelectric effect support the particle theory of light?
In order for an electron to be ejected from a metal surface, the electron must be
struck by a single photon with at least the minimum energy needed to knock the
electron loose.
2. What is the difference between the ground state and the excited state of an atom?
The ground state is the lowest energy state of the atom. When the atom absorbs
energy, it can move to a higher energy state, or excited state.
3. Under what circumstances can an atom emit a photon?
A photon is emitted when an atom moves from an excited state to its ground
state or to a lower-energy excited state.
4. How can the energy levels of the atom be determined by measuring the light emitted from an
atom?
When an atom loses energy, it falls from a higher energy state to a lower energy
state. The frequency of the emitted light, observed in an element’s line-emission
spectrum, may be measured. The energy of each transition is calculated using the
equation E hv, where v is the frequency of each of the lines in the element’s lineemission spectrum. From the analysis of these results, the energy levels of an atom
atom of each element may be determined.
5. Why does electromagnetic radiation in the ultraviolet region represent a larger energy transition
than does radiation in the infrared region?
Energy is proportional to frequency, and ultraviolet radiation has a higher frequency
than infrared radiation. To produce ultraviolet radiation, electrons must drop to
lower energy levels than they do to produce infrared radiation.
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ARRANGEMENT OF ELECTRONS IN ATOMS
25
Name
Date
Class
SECTION 1 continued
6. Which of the waves shown below has the higher frequency? (The scale is the same for each
drawing.) Explain your answer.
Wavelength
Wavelength
Wave A
Wave B
Wave B has the higher frequency. Wavelength is inversely proportional to
frequency, so as the wavelength decreases, its frequency increases.
7. How many different photons of radiation were emitted from excited helium atoms to form the
spectrum shown below? Explain your answer.
Spectrum for helium
Six different photons were emitted. Each time an excited helium atom falls back
from an excited state to its ground state or to a lower energy state, it emits a
photon of radiation that shows up as this specific line-emission spectrum. There are
six lines in this helium spectrum.
PROBLEMS
provided.
8.
9.
26
Write the answer on the line to the left. Show all your work in the space
9.7 1014 Hz
9.4 109 m
What is the frequency of light that has a wavelength of 310 nm?
What is the wavelength of electromagnetic radiation if its frequency
is 3.2 102 Hz?
ARRANGEMENT OF ELECTRONS IN ATOMS
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Name
Date
Class
CHAPTER 4 REVIEW
Arrangement of Electrons in Atoms
SECTION 2
SHORT ANSWER
1.
Answer the following questions in the space provided.
How many quantum numbers are used to describe the properties of electrons in atomic
orbitals?
(a) 1
(b) 2
2.
(c) 3
(d) 4
A spherical electron cloud surrounding an atomic nucleus would best represent
(a) an s orbital.
(b) a p orbital.
3.
(c) a combination of two different p orbitals.
(d) a combination of an s and a p orbital.
How many electrons can an energy level of n 4 hold?
(a) 32
(b) 24
4.
(c) 8
(d) 6
How many electrons can an energy level of n 2 hold?
(a) 32
(b) 24
5.
(c) 8
(d) 6
Compared with an electron for which n 2, an electron for which n 4 has more
(a) spin.
(b) particle nature.
6.
(c) energy.
(d) wave nature.
According to Bohr, which is the point in the figure below where electrons cannot reside?
(a) point A
(b) point B
(c) point C
(d) point D
Orbitals
D
Nucleus
7.
A
B
C
According to the quantum theory, point D in the above figure represents
(a)
(b)
(c)
(d)
the fixed position of an electron.
the farthest position from the nucleus that an electron can achieve.
a position where an electron probably exists.
a position where an electron cannot exist.
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ARRANGEMENT OF ELECTRONS IN ATOMS
27
Name
Date
Class
SECTION 2 continued
8. How did de Broglie conclude that electrons have a wave nature?
9. Identify each of the four quantum numbers and the properties to which they refer.
10. How did the Heisenberg uncertainty principle contribute to the idea that electrons occupy “clouds,”
or “orbitals”?
11. Complete the following table:
Principal quantum
number, n
Number of sublevels
Types of orbitals
1
2
3
4
28
ARRANGEMENT OF ELECTRONS IN ATOMS
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Name
Date
Class
CHAPTER 4 REVIEW
Arrangement of Electrons in Atoms
SECTION 2
SHORT ANSWER
1.
d
Answer the following questions in the space provided.
How many quantum numbers are used to describe the properties of electrons in atomic
orbitals?
(a) 1
(b) 2
2.
a
(c) 3
(d) 4
A spherical electron cloud surrounding an atomic nucleus would best represent
(a) an s orbital.
(b) a p orbital.
3.
a
(c) a combination of two different p orbitals.
(d) a combination of an s and a p orbital.
How many electrons can an energy level of n 4 hold?
(a) 32
(b) 24
4.
c
(c) 8
(d) 6
How many electrons can an energy level of n 2 hold?
(a) 32
(b) 24
5.
c
(c) 8
(d) 6
Compared with an electron for which n 2, an electron for which n 4 has more
(a) spin.
(b) particle nature.
6.
c
(c) energy.
(d) wave nature.
According to Bohr, which is the point in the figure below where electrons cannot reside?
(a) point A
(b) point B
(c) point C
(d) point D
Orbitals
D
Nucleus
7.
c
A
B
C
According to the quantum theory, point D in the above figure represents
(a)
(b)
(c)
(d)
the fixed position of an electron.
the farthest position from the nucleus that an electron can achieve.
a position where an electron probably exists.
a position where an electron cannot exist.
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ARRANGEMENT OF ELECTRONS IN ATOMS
27
Name
Date
Class
SECTION 2 continued
8. How did de Broglie conclude that electrons have a wave nature?
Scientists knew that any wave confined to a space could have only certain
frequencies. De Broglie suggested that electrons should be considered as waves
confined to the space around an atomic nucleus; in this way, electron waves could
exist only at specific frequencies. According to the relationship E h , these
frequencies correspond to the specific quantized energies of the Bohr orbitals.
9. Identify each of the four quantum numbers and the properties to which they refer.
The principal quantum number refers to the main energy level. The angular
momentum quantum number refers to the shape of the orbital. The magnetic
quantum number refers to the orientation of an orbital around the nucleus. The spin
quantum number indicates the spin state of an electron in an orbital.
10. How did the Heisenberg uncertainty principle contribute to the idea that electrons occupy “clouds,”
or “orbitals”?
The Heisenberg uncertainty principle states that it is impossible to determine
simultaneously both the position and velocity of an electron (or any other particle).
Because measuring the position of an electron actually changes its position, there is
always a basic uncertainty in trying to locate an electron. Thus, the exact position of
the electron cannot be found. An electron cloud or orbital represents the region
that is the probable location of an electron.
11. Complete the following table:
28
Principal quantum
number, n
Number of sublevels
Types of orbitals
1
1
s
2
2
s,p
3
3
s,p,d
4
4
s,p,d,f
ARRANGEMENT OF ELECTRONS IN ATOMS
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Name
Date
Class
CHAPTER 4 REVIEW
Arrangement of Electrons in Atoms
SECTION 3
SHORT ANSWER
Answer the following questions in the space provided.
1. State the Pauli exclusion principle, and use it to explain why electrons in the same orbital must
have opposite spin states.
2. Explain the conditions under which the following orbital notation for helium is possible:
↑
↑
1s
2s
Write the ground-state electron configuration and orbital notation for each of the
following atoms:
3. Phosphorus
4. Nitrogen
5. Potassium
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ARRANGEMENT OF ELECTRONS IN ATOMS
29
Name
Date
Class
SECTION 3 continued
6. Aluminum
7. Argon
8. Boron
9. Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital
diagrams?
3s2
a.
2p6
2s2
1s2
b.
2p4
2s2
1s2
30
ARRANGEMENT OF ELECTRONS IN ATOMS
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Name
Date
Class
CHAPTER 4 REVIEW
Arrangement of Electrons in Atoms
SECTION 3
SHORT ANSWER
Answer the following questions in the space provided.
1. State the Pauli exclusion principle, and use it to explain why electrons in the same orbital must
have opposite spin states.
The Pauli exclusion principle states that no two electrons in an atom may have the
same set of four quantum numbers. If both electrons in the same orbital had the
same spin state, each electron would have the same four quantum numbers. If one
electron has the opposite spin state, the fourth quantum number is different and
the exclusion principle is obeyed.
2. Explain the conditions under which the following orbital notation for helium is possible:
↑
↑
1s
2s
This orbital notation is possible if the helium atom is in an excited state.
Write the ground-state electron configuration and orbital notation for each of the
following atoms:
3. Phosphorus
↑↓
↑↓
↑↓
↑↓ ↑↓
↑↓
1s
2s
2px 2py 2pz
3s
↑↓
↑↓
↑
1s
2s
1s22s22p63s23p3;
↑
↑
↑
3px 3py 3pz
4. Nitrogen
1s22s22p3;
↑
↑
2px 2py 2pz
5. Potassium
1s22s22p63s23p64s1;
↑↓
↑↓
↑↓ ↑↓
↑↓
↑↓
↑↓
↑↓ ↑↓
↑
1s
2s
2px 2py 2pz
3s
3px 3py 3pz
4s
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
ARRANGEMENT OF ELECTRONS IN ATOMS
29
Name
Date
Class
SECTION 3 continued
6. Aluminum
↑↓
↑↓
↑↓ ↑↓ ↑↓
↑↓
1s
2s
2px 2py 2pz
3s
↑↓
↑↓
↑↓ ↑↓ ↑↓
↑↓
↑↓ ↑↓ ↑↓
1s
2s
2px 2py 2pz
3s
3px 3py 3pz
↑↓
↑↓
↑
1s
2s
1s22s22p63s23p1;
↑
3px 3py 3pz
7. Argon
1s22s22p63s23p6;
8. Boron
1s22s22p1;
2px 2py 2pz
9. Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital
diagrams?
3s2
a.
Pauli exclusion principle
b.
Hund’s rule
2p6
2s2
1s2
2p4
2s2
1s2
30
ARRANGEMENT OF ELECTRONS IN ATOMS
MODERN CHEMISTRY
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Ms. K
Honors Chemistry
Name_______________________ #______
Date________________ Period_____
Chapter 4 Review Sheet
REVIEW TERMS AND CONCEPTS
energy
work
Joules, calories, and Calories
Law of conservation of energy
forms of energy
kinetic vs. potential energy
absolute zero
electromagnetic radiation
electromagnetic spectrum
waves
nodes
amplitude
wavelength
frequency
speed of light
energy
radio station’s frequency
Planck’s constant
photoelectric effect
quantum
photon
ground state
excited state
bright-line emission spectrum
continuous spectrum
Bohr model of the atom
Niels Bohr
orbit
emission
absorption
diffraction
interference
double-slit experiment
Thomas Young
Heisenberg uncertainty principle
Werner Heisenberg
quantum theory
orbital
s, p, d, f
degenerate orbitals
electron dot model
quantum mechanical model
quantum numbers
principal quantum number, n
energy level
angular momentum quantum number, l
magnetic quantum number, m
spin quantum number, s
orbital diagrams
electron configurations
Aufbau principle
Pauli Exclusion principle
Hund’s Rule
Exceptions ? Cr, Cu, Mo, Ag
ion electron configuration
noble-gas configuration
isoelectronic
valence electrons
REVIEW QUESTIONS
1. Which form of electromagnetic radiation has the higher ν, blue light or radio waves?
2. Which form of electromagnetic radiation has the higher λ, red light or orange light?
3. Which form of electromagnetic radiation has the higher E, ultraviolet light or microwaves?
4. Which form of electromagnetic radiation has the higher speed, green light or infrared waves?
5. Write the equation for the calculation for the energy of any photon of light.
6. Write the equation for the calculation for the wavelength of light.
7. What is it called when a light of high enough frequency is shined on a metal and electrons are emitted?
8. Why do you see discrete lines when a beam of emitted light from an element is shined through a prism
and not a continuous spectrum?
9. Why is Ag?s electron configuration not in the ground state?
10. Write the electron configuration for element 116, both long-hand and short-hand.
11. Be able to answer the following questions from you textbook, pages 124-127:
4, 6, 8, 10, 11, 12, 13, 14, 18, 19, 22, 23, 24, 25, 26, 27, 28, 30, 31, 32, 35, 36, 37, 38, 41