Chemistry CP Unit 2 – Atomic Structure and Electron Configuration

Chemistry CP Unit 2 – Atomic Structure and Electron Configuration
Learning Targets (Your exam at the end of Unit 2 will assess the following:)
2. Atomic Structure and Electron Configuration
2-1. Give the one main contribution to the development of the atomic model from each of the following scientists: Dalton,
Thomson, Rutherford, Chadwick, and Bohr.
2-2. Identify elements by both name and chemical symbol using a periodic table.
2-3. Compare protons, electrons, and neutrons in terms of charge, mass, and location in an atom.
2-4. Use the periodic table to determine the number of protons, electrons, neutrons, and atomic mass for a given element.
2-5. Define isotope and state how the atomic structure for isotopes of the same element are similar and different.
2-6. Calculate the average atomic mass from the relative abundances and masses of each isotope.
2-7. Define valence electrons and determine the number of valence electrons for an atom.
2-8. Locate rows/periods and groups/families on the periodic table.
2-9. Draw the Bohr diagram for an atom showing protons and neutrons and the number of electrons in each shell. Draw the
Bohr diagram for the ion of an element, showing how the atom establishes a full valence shell. Determine the noble gas
that the atom resembles once it forms an ion.
2-10. Define ion and determine the charge for the ion of an element from the periodic table. Determine the number of
electrons for an ion. Give the symbol for the ion.
2-11. Define cation and anion.
2-12. List the four different kinds of atomic orbitals by their letter designation and state the number of electrons that each can
hold.
2-13. Give orbital notation for a given atom/ion.
2-14. Write electronic configuration for a given atom/ion.
2-15. Write noble gas configuration for a given atom/ion.
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2-1. Give the one main contribution to the development of the atomic model from each of the following scientists: Dalton,
Thomson, Rutherford, Chadwick, and Bohr.
Scientist
Experiment
Findings
Dalton
Thomson
Rutherford
Chadwick
Bohr
2
2-2. Identify elements by both name and chemical symbol using a periodic table.
2-3. Compare protons, electrons, and neutrons in terms of charge, mass, and location in an atom.
2-4. Use the periodic table to determine the number of protons, electrons, neutrons, and atomic mass for a given element.
Subatomic Particles
Name
Symbol
Symbol
Name
24
11
𝑁𝑎
80
35
𝐵𝑟
40
20
𝐶𝑎
197
79
𝐴𝑢
16
8
𝑂2−
39
19
𝐾+
Charge
Relative Mass
Atomic Number
Mass Number
34
78
22
47
91
231
Number of
Protons
Actual Mass (g)
Number of
Neutrons
Location
Number of
Electrons
3
WS #1 (Learning Target 2-4. Use the periodic table to determine the number of protons, electrons, neutrons, and atomic mass for
a given element.
4
WS #1 (con’t) (Learning Target 2-4. Use the periodic table to determine the number of protons, electrons, neutrons, and atomic
mass for a given element.
(11) Complete the following table for neutral atoms and/or ions.
Substance
symbol
Magnesium
atomic
number
mass
number
12
24
Iron
S
Beryllium
16
Pt+3
Atom or ion?
atom
13
16
9
atom
24
194
U+2
Oxygen
number of
electrons
24
13
24
Platinum
number of
neutrons
12
26
26
Sulfur
number of
protons
24
75
92
O2-
143
8
Gold
45
18
18
118
78
24
74
-1 ion
22
70
+2 ion
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Substance
symbol
atomic
number
mass
number
number of
protons
number of
neutrons
number of
electrons
Atom or ion?
Magnesium
Mg
12
24
12
12
12
atom
Iron
Fe
26
50
26
24
26
atom
Aluminum
Al
13
26
13
13
13
atom
Sulfur
S
16
32
16
16
16
Atom
Beryllium
Be
4
9
4
5
4
Atom
Chromium
Cr
24
48
24
24
24
Atom
Platinum
Pt+3
78
194
78
116
75
+3 ion
Uranium
U+2
92
235
92
143
90
+2 ion
Oxygen
O2-
8
16
8
8
10
-2 ion
Chlorine
Cl-
17
35
17
18
18
-1 ion
Gold
Au+
79
197
79
118
78
+1 ion
Chromium
Cr+2
24
45
24
21
22
+2 ion
Tungsten
W+2
74
144
74
70
72
+2 ion
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2-5. Define isotope and state how the atomic structure for isotopes of the same element are similar and different.
2-6. Calculate the average atomic mass from the relative abundances and masses of each isotope.
Isotopes are atoms of the _____________ _________________ that have _______________ numbers of ______________.
Isotope
Carbon-12
Carbon-13
Carbon-14
Atomic Number
Mass Number
Number of Protons
Number of Neutrons
Mass Number is the number of ________________ and _________________ in an atom.
Atomic Mass is the ______________________ _______________________ ___________________ of all the different isotopes of an
element ____________________ by the abundance of each isotope in nature.
Atomic mass is measured in Atomic Mass Units (_______)
(1 amu = 1/12 the mass of a carbon-12 atom)
Example: Silver (atomic number 47) has two naturally occurring isotopes, Ag-107 and Ag-109. Given their atomic masses and
percent abundances below, what is silver’s average atomic mass?
Isotope
Mass (amu)
Abundance (%)
Ag-107
106.90509
51.84
Ag-109
108.90476
48.16
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Example: Silicon (atomic number 14) has three naturally occurring isotopes, Si-28, Si-29 and Si-30. Given their atomic masses and
percent abundances below, what is silicon’s average atomic mass?
Isotope
Mass (amu)
Abundance (%)
Si-28
27.976927
92.23
Si-29
28.976495
4.67
Si-30
29.973770
3.10
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WS #2 (Learning Target 2-6. Calculate the average atomic mass from the relative abundances and masses of each isotope.)
(1) Isotopes are different “versions” of the same atom that have the same number of _____________ but different
numbers of _____________ and therefore different _____________ _____________.
(2) How many neutrons does each isotope have?
(a) Carbon-13
(b) Oxygen-18
(c) Potassium-40
(d) Scandium-45
(e) Manganese-55
(f) Tungsten-186
(3) There are two isotopes of copper: Copper-63 (69.17%) and Copper-65 (30.83%).
(a) Determine the number of neutrons in each of the isotopes.
(b) Calculate the average atomic mass of copper (round your answer to one decimal place).
(4) There are two isotopes of silver: Silver-107 (51.84%) and Silver-109 (48.16%).
(a) Determine the number of neutrons in each of the isotopes.
(b) Calculate the average atomic mass of silver (round your answer to one decimal place).
(5) There are three isotopes of magnesium: Magnesium-24 (78.7%), Magnesium-25 (10.1%), and Magnesium-26 (11.2%)
(a) Determine the number of neutrons in each of the isotopes.
(b) Calculate the average atomic mass of magnesium (round your answer to one decimal place).
(6) There are four isotopes of iron: Iron-54 (5.85%), Iron-56 (91.75%), Iron-57 (2.12%), and Iron-58 (0.28%)
(a) Determine the number of neutrons in each of the isotopes.
(b) Calculate the average atomic mass of iron (round your answer to one decimal place).
(7) There are two isotopes of gallium: Gallium-69 and Gallium-71.
(a) Determine the number of neutrons in each of the isotopes.
(b) Gallium-69 has an abundance of 60.11%, what is the abundance of Gallium-71?
(c) Calculate the average atomic mass of gallium (round your answer to one decimal place).
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WS #2 (con’t) (Learning Target 2-6. Calculate the average atomic mass from the relative abundances and masses of each isotope.)
(8) There are two isotopes of bromine: Bromine-79 and Bromine-81.
(a) Determine the number of neutrons in each of the isotopes.
(b) Bromine-79 has an abundance of 50.69%, what is the abundance of Bromine-81?
(c) Calculate the average atomic mass of bromine (round your answer to one decimal place).
(9) There are five isotopes of germanium: Germanium-70, Germanium-72, Germanium-73, Germanium-74, and
Germanium-76
(a) Determine the number of neutrons in each of the isotopes.
(b) Germanium-70 has an abundance of 21.23%, Germanium-72 has an abundance of 27.66%, Germanium-73
has an abundance of 7.73%, and Germanium-74 has an abundance of 35.94%. What is the abundance of
Germanium-76?
(c) Calculate the average atomic mass of germanium (round your answer to one decimal place).
(10) There are four isotopes of strontium: Strontium-84, Stronium-86, Strontium-87, and Strontium-88.
(a) Determine the number of neutrons in each of the isotopes.
(b) Strontium-84 has an abundance of 0.56%, Strontium-86 has an abundance of 9.86%, and Strontium-87 has
an abundance of 7.00%. What is the abundance of Strontium-88?
(c) Calculate the average atomic mass of strontium (round your answer to one decimal place).
Answers: Isotopes (1) Isotopes are different “versions” of the same atom that have the same number of protons but
different numbers of neutrons and therefore different atomic masses (2) (a) 7 (b) 10 (c) 21 (d) 24 (e) 30 (f) 112 .
(3) (a) 34, 36 (b) 63.6 amu (4) (a) 60, 62 (b) 108.0 amu (5) (a) 12, 13, 14 (b) 24.3 amu (6) (a) 28, 30, 31, 32 (b) 55.9 amu
(7) (a) 38, 40 (b) 39.89% (c) 69.8 amu (8) (a) 44, 46 (b) 49.31% (c) 80.0 amu
(9) (a) 38, 40, 41, 42, 44 (b) 7.44% (c) 72.67 amu (10) (a) 46, 48, 49, 50 (b) 82.58% (c) 87.7 amu
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2-7. Define valence electrons and determine the number of valence electrons for an atom.
2-8. Locate rows/periods and groups/families on the periodic table.
2-9. Draw the Bohr diagram for an atom showing protons and neutrons and the number of electrons in each shell. Draw the Bohr
diagram for the ion of an element, showing how the atom establishes a full valence shell. Determine the noble gas that the
atom resembles once it forms an ion.
Periods on the periodic table go ______________ and __________________.
Groups on the periodic table go ______________ and __________________.
Valence Electrons =
How to determine the number of valence electrons an atom has:
Sample Problem. How many valence electrons?
Carbon
Magnesium
Chlorine
Helium
11
WS #3 (Learning Target 2-9: Draw the Bohr diagram for an atom showing protons and neutrons and the number of electrons in
each shell. Draw the Bohr diagram for the ion of an element, showing how the atom establishes a full valence shell. Determine
the noble gas that the atom resembles once it forms an ion. )
12
13
WS #4 (Learning Targets 2-10 and 2-11: Define ion and determine the charge for the ion of an element from the periodic table.
Determine the number of electrons for an ion. Give the symbol for the ion. Define cation and anion.)
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WS #4 (Learning Targets 2-10 and 2-11: Define ion and determine the charge for the ion of an element from the periodic table.
Determine the number of electrons for an ion. Give the symbol for the ion. Define cation and anion.)
15
2-12. List the four different kinds of atomic orbitals by their letter designation and state the number of electrons that each can hold.
Orbital Letter
Orbital Shape
16
2-13. Give orbital notation for a given atom/ion.
2-14. Write electronic configuration for a given atom/ion.
2-15. Write noble gas configuration for a given atom/ion.
Order of Filling Orbitals:
Atom
Atomic Number
Number of Electrons
Orbital Notation
_____
1s
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
_____
1s
Electron
Configuration
Noble Gas
Configuration
17
Atom
Atomic Number
Number of Electrons
Orbital Notation
_____ _____
1s
2s
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
18
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
Atom
Atomic Number
Number of Electrons
Orbital Notation
Electron
Configuration
Noble Gas
Configuration
19
WS #5 (Learning Targets 2.13, 2.14, 2.15)
Complete the following table:
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(2) Give the orbital notation and electron configuration notation for the following elements:
(a) Sc
(b) Fe
(c) Pd
(d) Kr
(e) Ga
(f) Co
(g) In
(h) Cs
(i) Sn
(j) Ce
(3) Give the electron configuration notation and noble gas notation for the following elements:
(a) Be
(b) F
(c) Na
(d) P
(e) Ti
(f) Te
(g) Cd
(h) Al
(i) La
(j) Ac
(4) Give the orbital notation, electron configuration notation, and noble gas notation for the following elements/ions:
(a) V
(b) Ge
(c) Y
(d) Zn
(e) Sr
(f) Rb+
(g) Ca2+
(h) Li+
(i) I –
(j) N3–
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WS #6 (Unit 2 Review – part 1)
1.
(Learning Target 2-1) Identify the main contribution each of the following made to the development of the atomic theory.
a. Dalton
b. Thomson
c. Rutherford
d. Chadwick
e. Bohr
2.
(Learning Target 2-3) Compare protons, electrons, and neutrons in terms of charge, mass, and location in an atom.
Charge
Proton
Neutron
Electron
3.
Relative Mass
1
Mass (amu)
Location
(2-2, 2-4) Complete the following table for NEUTRAL atoms.
Atomic Number
Element
Symbol
Atomic Mass
Protons
Electrons
Neutrons
(Show Your Work)
Fluorine
36
Os
112
4.
(Learning Target 2-5) Among isotopes, which of the following are the same? Which are different?
Atomic Number?
Mass Number?
Atomic Mass?
# protons? # neutrons? # electrons?
5.
(Learning Target 2-6) Calculate the average atomic mass from the relative abundances and masses of each isotope.
There are four isotopes of lead: Lead–204 (1.4%), Lead–205 (24.1%), Lead–207 (22.1%), and Lead–208 (52.4%).
(a) Determine the number of neutrons in each of the isotopes.
Lead–204 = ________
Lead–205 = ________
Lead–207 = ________
Lead–208 = ________
(b) Determine the average atomic mass of Lead. Give the answer to one decimal place.
Average atomic mass = _________
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WS #9 (con’t) (Unit 2 Review – part 1)
6.
(Learning Target 2-7, 2-9, 2-10) Draw the Bohr diagram for the atom and the ion. Indicate the number of protons,
electrons, and neutrons. Give the symbol and charge for the ion.
(a) boron ___ p ___ e ___ n symbol: ____
Atom:
7.
(b) chlorine ___ p ___ e ___ n symbol: ____
Ion:
Atom:
Ion:
(Learning Target 2-10) Complete the following table for IONS.
Atomic
Number
Element
Symbol
Atomic Mass
Protons
Electrons
(Show Your Work)
Neutrons
(Show Your Work)
Beryllium
51
Lu3+
210.1
8.
(Learning Target 2-8) Where are periods located on the Periodic Table? Groups? Families?
9.
(Learning Target 2-11) Distinguish between a cation and an anion.
10. (Learning Target 2-12) Draw a picture of one of each of the following orbitals.
Orbital
Letter
Orbital Shape
s
p
d
f
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11. (Learning Targets 2-13, 2-14, 2-15)
(i) Give the orbital notation for the following elements.
(a) sodium
(b) iron
(c) europium
(ii) Give the electron configuration notation for the following elements.
(a) neon
(b) bromine
(c) thallium
(iii) Give the electron configuration for two possible excited states for neon.
(iv) Give the noble gas notation for the following elements.
(a) fluorine
(b) titanium
(c) americium
(v) Give the electron configuration notation and noble gas notation for the following ions.
(a) O2-
(b) Y3+
Answers: (1) (a) developed the atomic theory (b) discovered the electron in his cathode ray experiment, developed plum pudding
model (c) discovered the nucleus in his gold-foil experiment (d) discovered the neutron (e) developed the orbital model of the atom
(2)
Proton
Neutron
Electron
Charge
+1
0
-1
Relative Mass
1
1
1/1836
Mass (amu)
1
1
0
Location
nucleus
nucleus
Outside of nucleus
(3)
Atomic Number
9
36
76
112
Element
Fluorine
Krypton
Osmium
Copernicium
Symbol
F
Kr
Os
Cn
Atomic Mass
19.00
83.80
190.23
285
Protons
9
36
76
112
Electrons
9
36
76
112
Neutrons
(Show Your Work)
10
48
190 – 76 = 114
4 – 112 = 173
24
(4) same atomic number, different mass number, different atomic mass, same # protons, different # neutrons, same # electrons
(5) (a) 122, 123, 125, 126 (b) 207.0 amu (6) (a) 5p, 5e, 6n (b) 17p, 17e, 18n
(7)
Atomic
Number
4
51
71
85
Element
Symbol
Atomic Mass
Protons
Beryllium
Antimony
Lutetium
Astatine
Be2+
Sb3Lu3+
At-
9.012
121.76
174.97
210.1
4
51
71
85
Electrons
(Show Your Work)
4–2=2
51 + 3 = 54
71 – 3 = 68
85 + 1 = 86
Neutrons
(Show Your Work)
5
71
104
125
(8) periods – horizontal rows, groups (aka families) – vertical columns (9) cation = positive ion, anion = negative ion
(10)
Orbital
Letter
Orbital Shape
s
p
d
f
(11) (i)
(ii) (a) 1s2 2s2 2p6 (b) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 (c) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p1
(iii) answers will vary; Sample examples: 1s2 2s2 2p5 3s1 or 1s2 2s2 2p5 3p1 (iv) (a) [He] 2s2 2p5 (b) [Ar] 4s2 3d2 (c)
[Rn] 7s2 5f7 (v) (a) 1s2 2s2 2p6 , [Ne] (b) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 , [Kr]
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