Transcript Select as many as apply.

Chapter 11
Modern Atomic Theory
Practice Problems
All atoms of the same element
have the same number of
1.
2.
3.
4.
5.
Protons
Neutrons
Electrons
Protons and Neutrons
Protons and Electrons
2
All atoms of the same element
have the same number of
1. Protons
• this is a good choice, but not the best
choice.
2. Neutrons
3. Electrons
4. Protons and Neutrons
5. Protons and Electrons
3
In the symbol below, the number
33 is the
X
33
1.
2.
3.
4.
5.
Atomic mass
Mass number
Atomic number
Charge
Number of X atoms attached to each
other.
4
In the symbol below, the number
33 is the
X
33
1.
2.
3.
4.
5.
Atomic mass
Mass number
Atomic number
Charge
Number of X atoms attached to each
other.
5
In the symbol below, the number 60
is the __ which tells us this is 60
1.
2.
3.
4.
X
Atomic mass, Ni
Mass number, Ni
Mass number, Ni or Co
Mass number, possibly any element in
the Ni & Cu “neighborhood.”
5. Atomic number, Ni or Co
6
In the symbol below, the number 60
is the __ which tells us this is 60
1.
2.
3.
4.
X
Atomic mass, Ni
Mass number, Ni
Mass number, Ni or Co
Mass number, possibly any element in
the Ni & Cu “neighborhood.”
5. Atomic number, Ni or Co
•
Mass number can not be used to identify
which element, only atomic number can.
7
The number of neutrons can be
known by
1. Dividing the mass number in half.
2. Subtracting the atomic number from
the mass number.
3. Subtracting the number of protons
from the atomic mass.
4. Looking at the atomic number.
5. It can not be known exactly because of
isotopes.
8
The number of neutrons can be
known by
1. Dividing the mass number in half.
2. Subtracting the atomic number from
the mass number.
3. Subtracting the number of protons
from the atomic mass.
4. Looking at the atomic number.
5. It can not be known exactly because of
isotopes.
9
The element represented by
2
10
2
[Ar] 4s 3d 4p is
1.
2.
3.
4.
5.
20Ca
22Ti
32Ge
50Sn
35Br
10
The element represented by
2
10
2
[Ar] 4s 3d 4p is
1.
2.
3.
20Ca
22Ti
32Ge
• All that you really need to look at is the
4p2 to be able to identify.
4. 50Sn
5. 35Br
11
The element represented by
2
9
[Kr] 5s 4d is
1.
2.
3.
4.
5.
29Cu
27Co
79Au
47Ag
45Rh
12
The element represented by
[Kr] 5s24d9 is
1.
2.
3.
4.
5.
29Cu
27Co
79Au
47Ag
45Rh
13
The element represented by 5p3 is
(assuming all lower energy orbitals
are filled)
1.
2.
3.
4.
5.
39Y
51Sb
33As
21Sc
83Bi
14
The element represented by 5p3 is
1.
2.
3.
4.
5.
39Y
51Sb
33As
21Sc
83Bi
15
Give highest energy orbital to
describe 74W
1.
2.
3.
4.
5.
6d6
7d6
6p4
6d4
5d4
16
Give highest energy orbital to
describe 74W
1.
2.
3.
4.
5.
6d6
7d6
6p4
6d4
5d4
17
How many valence electrons
in 15P
1.
2.
3.
4.
5.
6.
15
8
3
4
5
I don’t know what the word valence
means.
18
How many valence electrons
in 15P
1.
2.
3.
4.
5.
6.
•
15
8
3
4
5
I don’t know what the word valence means.
Valence means outermost electrons - the
“s” and “p” electrons in the last energy level.
19
When atoms turn into a positive ion
1.
2.
3.
4.
5.
Protons are gained.
Protons are lost.
Electrons are gained
Electrons are lost.
Either protons are gained or electrons
are lost.
20
When atoms turn into a positive ion
1.
2.
3.
4.
5.
Protons are gained.
Protons are lost.
Electrons are gained
Electrons are lost.
Either protons are gained or electrons
are lost.
21
Fluorine (F)
Does 9F want to lose or gain electrons? How many?
What will the new charge be?
1.
2.
3.
4.
5.
6.
7.
Lose 6 e-, 6+, cation
Gain 6 e-, 6-, anion
Lose 1 e-, 1+, cation
Gain 1 e-, 1-, anion
Lose 7 e-, 7+, cation
Gain 7 e-, 7-, anion
Will not lose or gain. It is happy(stable)!
22
Fluorine (F)
Does 9F want to lose or gain electrons? How many?
What will the new charge be?
1.
2.
3.
4.
5.
6.
7.
Lose 6 e-, 6+, cation
Gain 6 e-, 6-, anion
Lose 1 e-, 1+, cation
Gain 1 e-, 1-, anion
Lose 7 e-, 7+, cation
Gain 7 e-, 7-, anion
Will not lose or gain. It is happy(stable)!
23
Gallium (Ga)
Does 31Ga want to lose or gain electrons? How many?
What will the new charge be?
1.
2.
3.
4.
5.
6.
7.
Lose 4 e-, 4+, cation
Gain 3 e-, 3-, anion
Lose 1 e-, 1+, cation
Gain 1 e-, 1-, anion
Lose 3 e-, 3+, cation
Gain 4 e-, 4-, anion
Will not lose or gain. It is happy(stable)!
24
Gallium (Ga)
Does 31Ga want to lose or gain electrons? How many?
What will the new charge be?
1.
2.
3.
4.
5.
6.
7.
Lose 4 e-, 4+, cation
Gain 3 e-, 3-, anion
Lose 1 e-, 1+, cation
Gain 1 e-, 1-, anion
Lose 3 e-, 3+, cation
Gain 4 e-, 4-, anion
Will not lose or gain. It is happy(stable)!
25
Radon (Rn)
Does 86Rn want to lose or gain electrons? How many?
What will the new charge be?
1.
2.
3.
4.
5.
6.
7.
Lose 2 e-, 2+, cation
Gain 3 e-, 3-, anion
Lose 1 e-, 1+, cation
Gain 1 e-, 1-, anion
Lose 3 e-, 3+, cation
Gain 2 e-, 2-, anion
Will not lose or gain. It is happy(stable)!
26
Radon (Rn)
Does 86Rn want to lose or gain electrons? How many?
What will the new charge be?
1.
2.
3.
4.
5.
6.
7.
Lose 2 e-, 2+, cation
Gain 3 e-, 3-, anion
Lose 1 e-, 1+, cation
Gain 1 e-, 1-, anion
Lose 3 e-, 3+, cation
Gain 2 e-, 2-, anion
Will not lose or gain. It is happy(stable)!
27
Forming Bonds
1. Sodium Chloride
NaCl
2. Magnesium Oxide
MgO
3. Calcium Iodide
CaI2
4. Aluminum Oxide
Al2O3
28
Which light has the most
energy?
1. Red
2. Orange
3. Yellow
4. Green
5. Blue
29
Which light has the most energy?
1.
2.
3.
4.
5.
Red
Orange
Yellow
Green
Blue - most energy, highest
frequency, shortest wavelength.
30
Which light has the highest
frequency?
1. Red
2. Orange
3. Yellow
4. Green
5. Blue
31
Which light has the highest
frequency?
1. Red
2. Orange
3. Yellow
4. Green
5. Blue
32
Which light has the longest
wavelength?
1. Red
2. Orange
3. Yellow
4. Green
5. Blue
33
Which light has the longest
wavelength?
1. Red
2. Orange
3. Yellow
4. Green
5. Blue
34
Which light has the least
energy?
1. infrared
2. micro waves
3. green light
4. gamma
5. ultraviolet
35
Which light has the least
energy?
1. infrared
2. micro waves
3. green light
4. gamma
5. ultraviolet
36
In a hydrogen atom, an electron
undergoing the transition between
which energy levels would emit the
most energy?
1.
2.
3.
4.
5.
6.
3-2
5-2
1-2
4-5
4-1
2-1
37
In a hydrogen atom, an electron undergoing
the transition between which energy levels
would emit the most energy?
1.
2.
3.
4.
5.
3-2
5-2
1-2
4-5
4-1
•
energy is emitted only for transitions from higher to lower
energy levels.
transitions to the first energy level are always more energy
than to other energy levels
•
6.
2-1
38
Which graph best represents the
relationship between wavelength
and frequency for “light” aka EMR
(ElectroMagnetic Radiation)?
lamba, λ, wavelength


ν


ν
ν
ν
nu, v, frequency
1
2
3
4
39
Which graph best represents the relationship
between wavelength and frequency?


ν
A


ν
ν
ν
B
C
D
Wavelength () and frequency (ν) are inversely
related.
40
Select the largest atom from the group:
3Li, 11Na, 38Sr, 53I
Be ready to explain your choice.
1. 3Li
2. 11Na
3. 38Sr
4. 53I
5. Cannot be determined since they are in
different families and different periods
41
Select the largest atom from the group:
3Li, 11Na, 38Sr, 53I
1. 3Li
2. 11Na
3. 38Sr
• Since Sr and I both have a 5th energy
level, yet Sr has a lower effective
nuclear charge, so it has larger size.
4. 53I
5. Cannot be determined since they are in
different families and different periods
42
Select the largest particle from the group:
-1,
+2,
-2
Xe,
I
Ba
Te
54
53
56
52
Be ready to explain your choice.
1. 54Xe
2. 53I-1
3. 56Ba+2
4. 52Te-2
5. They are all the same size because they
are isoelectronic.
6. I can’t choose because I don’t know what
isoelectronic means and I don’t know
about the size of charged particles.
43
Select the largest particle from the group:
-1,
+2,
-2
Xe,
I
Ba
Te
54
53
56
52
1. 54Xe
2. 53I-1
3. 56Ba+2
4. 52Te-2 This ion has less protons, only 52
to hold the 54 electrons, thus the e- repel
each other and cause larger size
5. They are all the same size because they
are isoelectronic.
6. I can’t choose because I don’t know what
isoelectronic means and I don’t know
about the size of charged particles.
44
16S
1.
2.
3.
is smaller than 11Na because
16S
has more protons and more electrons.
16S has more electrons.
16S has more protons pulling on electrons
in the same energy level.
4. 16S has fewer energy levels.
5. 16S has more neutrons to allow the atom
to squeeze in more.
45
16S
1.
2.
3.
is smaller than 11Na because
16S
has more protons and more electrons.
16S has more electrons.
16S has more protons (blocked by the
same core of 10 e- electrons that the Na
nucleus is shielded by) pulling on
electrons in the same energy level.
4. 16S has fewer energy levels.
5. 16S has more neutrons to allow the atom
to squeeze in more.
46
Select the atom below with the lowest
first ionization energy.
Be ready to explain your choice.
1. 11Na
2. 12Mg
3. 13Al
4. 14Si
5. 15P
47
Select the atom below with the lowest
first ionization energy.
1. 11Na because it is largest in size
2. 12Mg
3. 13Al
4. 14Si
5. 15P
48
The atom that has a really large increase
for its 3rd ionization energy would be
1. 11Na
2. 12Mg
3. 13Al
4. 14Si
5. 15P
49
The atom with the largest increase for its 3rd
ionization energy would be
1.
2.
11Na
(for Na it would be the 2nd IE)
12Mg
because it has 2 valence electrons and
stealing the third electron comes from a full
energy level.
3. 13Al (for Al it would be the 4th IE)
4. 14Si (for Si it would be the 5th IE)
5. 15P (for P it would be the 6th IE)
•
All successive IE are larger than the previous,
however,the really large increase occurs for the
electron that is one more than the number of valence
electrons.
50
In which set of elements would all the atoms
have very similar chemical properties?
(Choose all that apply.)
1. 11Na, 12Mg, 13Al
2. 14Si, 32Ge, 50Sn
3. 90Th, 91Pa, 92U
4. 26Fe, 27Co, 28Ni
5. 7N, 8O, 9F
6. 16S, 34Se, 52Te
7. I have no idea how to even begin to
answer this question.
51
In which set of elements would all the atoms
have very similar chemical properties?
1.
2.
11Na, 12Mg, 13Al
3.
4.
5.
6.
90Th, 91Pa, 92U
14Si, 32Ge, 50Sn
this family crosses the metal nonmetal
barrier and thus would have different chemical
properties
26Fe, 27Co, 28Ni
7N, 8O, 9F
16S, 34Se, 52Te These elements are all in the same chemical
family which all have the same number of valence electrons.
7. I have no idea how to even begin to answer this
question.
52
When rubidium (37Rb) turns into its preferred
ion by losing an electron, (Select all that apply.)
It is isoelectronic with 35Br-1
It becomes positively charged
It turns into Kr
The resulting ion will be smaller than the
atom it came from
5. Its electrons will be the same as the
strontium ion’s electrons (38Sr+2)
1.
2.
3.
4.
53
When rubidium (37Rb) turns into its preferred
ion by losing an electron,
1. It is isoelectronic with 35Br-1
»
The bromide ion has gained one e- making 36 electrons
2. It becomes positively charged
»
because it lost one electron: 37+ and 36-
3. It turns into Kr
»
(Of course the Rb+1 ion does not become Kr because it still only
has 37 protons, not 36 like Kr)
4. The resulting ion will be smaller than the atom it came
from
»
Cations (+ ions) are always smaller than their parent atom.
5. Its electrons will be the same as the strontium ion’s
electrons (38Sr+2)
»
The electrons for both of these ions will be the same as Kr’s
electrons: 1s22s22p63s23p64s23d104p6
54
Which is more reactive?
1. 3Li
2. 11Na
3. 19K
4. 37Rb
5. They are equally reactive because they
are in the same chemical family.
6. I have no knowledge of how I might
even decide this.
55
Which is more reactive?
1. 3Li
2. 11Na
3. 19Na
4. 37Rb rubidium would be most reactive
because the alkali metals are losing an
electron, and it will be lost most vigorously
when the electron being lost is furthest from
the + pull of the nucleus.
5. They are equally reactive because they are
in the same chemical family.
6. I have no knowledge of how I might even
decide this.
56
Which is more reactive?
1. 9F
2. 17Cl
3. 35Br
4. 53I
5. They are equally reactive because they
are in the same chemical family.
6. I have no knowledge of how I might
even decide this.
57
Which is more reactive?
1.
2.
3.
4.
5.
6.
9F
Halogens like to gain electrons and a smaller
atom does that more vigorously because it is the
nucleus (protons) pulling in the electron to be
gained, and the closer it comes to the nucleus,
the more vigorously it comes.
17Cl
35Br
53I
They are equally reactive because they are in the
same chemical family.
I have no knowledge of how I might even decide
this.
58
Which is more reactive?
1. 8O
2. 16S
3. 34Se
4. 52Te
5. They are equally reactive because
they are in the same chemical family.
59
Which is more reactive?
1. 8O Like the halogens, these atoms like to
gain electrons and a smaller atom does that
more vigorously because it is the nucleus
(protons) pulling in the electron to be gained,
and the closer it comes to the nucleus, the
more vigorously it comes.
2. 16S
3. 34Se
4. 52Te
5. They are equally reactive because they are
in the same chemical family.
60
Which will normally form a negative
ion? (Select as many as apply.)
1.
2.
3.
4.
5.
6.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3
1s22s22p63s23p1
61
Which will normally form a negative
ion? (Select as many as apply.)
1.
2.
3.
4.
5.
6.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3
1s22s22p63s23p1
62
Which will normally form a negative
ion? Select as many as apply.
1.
2.
3.
4.
5.
6.
[Ar] 4s1
[Ar] 4s2
[Ar] 4s23d104p6
[Ar] 4s23d104p5
[Ar] 4s23d104p2
[Ar] 4s23d6
63
Which will normally form a negative
ion? Select as many as apply.
1.
2.
3.
4.
5.
6.
[Ar] 4s1
[Ar] 4s2
[Ar] 4s23d104p6
[Ar] 4s23d104p5
[Ar] 4s23d104p2
[Ar] 4s23d6
64
Which will have the lowest ionization
energy?
1.
2.
3.
4.
5.
6.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3
1s22s22p1
65
Which will have the lowest ionization
energy?
1.
2.
3.
4.
5.
6.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3
1s22s22p1
66
Which has(have) the greatest
number of unpaired electrons?
Select more than one in the case of a tie.
1.
2.
3.
4.
5.
6.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3
1s22s22p1
67
Which has(have) the greatest
number of unpaired electrons?
Select more than one in the case of a tie.
•
1.
2.
3.
4.
5.
6.
Draw orbital notation to help with this question.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3 ↑↓
1s22s22p1
↑↓ ↑ ↑ ↑
68
Which model below best represents
the valence electrons for oxygen?
1.
2.
3.
4.
5.
6.
↑↓ ↑↓ ↑↓ ↑↓ ↑
↑↓ ↑↓ ↑↓ ↑
↑↓ ↑↓ ↑
↑↓ ↑↓ ↑↓ ↑ ↑
↑↓ ↑↓ ↑ ↑ ↑
↑↓ ↑↓
69
Which model below best represents
the valence electrons for oxygen?
1.
2.
3.
4.
5.
6.
↑↓ ↑↓ ↑↓ ↑↓ ↑
↑↓ ↑↓ ↑↓ ↑
↑↓ ↑↓ ↑
↑↓ ↑↓ ↑↓ ↑ ↑
↑↓ ↑↓ ↑ ↑ ↑
↑↓ ↑↓
70
Which metal would combine with
oxygen in a one to one ratio.
Select as many as apply.
1.
2.
3.
4.
5.
6.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3
1s22s22p1
71
Which metal would combine with
oxygen in a one to one ratio.
Select as many as apply.
1.
2.
3.
4.
5.
6.
1s22s22p63s2
1s22s22p63s1
1s22s22p6
1s22s22p4
1s22s22p3
1s22s22p1
72
Which represents the valence
electron configuration of the
halogens?
1. ns1
n represents the
2. ns2
energy level
3. ns2np1
4. ns2np4
5. ns2np5
6. ns2np6
7. Without knowing which halogen,
an answer can not be given.
73
Which represents the valence
electron configuration of the
halogens?
1. ns1
n represents the
2. ns2
energy level
3. ns2p1
4. ns2p4
5. ns2p5
6. ns2p6
7. Without knowing which halogen,
an answer can not be given.
74
A certain nonmetallic element forms a
compound with gallium having the
general formula Ga2X3. Element X must
be a member of which group?
1.
2.
3.
4.
5.
6.
7.
1A
2A
3A
4A
5A
6A
7A
75
A certain nonmetallic element forms a
compound with gallium having the
general formula Ga2X3. Element X must
be a member of which group?
1.
2.
3.
4.
5.
6.
7.
1A
2A
3A
4A
5A
6A
7A
76
How many p orbitals are
occupied in 6C?
1.
2.
3.
4.
1
2
3
none
77
How many p orbitals are
occupied in 6C?
1.
2.
3.
4.
1
2 both are half full, 1 e- each
3
none
78
How many p orbitals are
occupied in 16S?
1.
2.
3.
4.
5.
6.
7.
2
3
4
5
6
10
none
79
How many p orbitals are
occupied in 16S?
1.
2.
3.
4.
5.
2
3
4
5
6
1s2 2s2 2p6
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
7.
8.
3s2 3p4
↑↓
↑↓ ↑ ↑
10
none
80
How many unpaired electrons
in 16S?
1.
2.
3.
4.
5.
6.
1
2
3
4
5
6
81
How many unpaired electrons
in 16S?
1.
2.
1
2
[Ne] 3s2 3p4
↑↓
3.
4.
5.
6.
3
4
5
6
↑↓ ↑ ↑
82