Quiz 3
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Subject
Chemistry
Date
Jan 9, 2024
Type
docx
Pages
9
Uploaded by ColonelIce13156
Name:
Quiz 3
E=hν
λ =h/mv
1/λ = R(1/m
2
-1/n
2
)
h: 6.6x10
-34
Js
R= 1.097x10
-2
nm
-1
1.
Which of the following has the largest radius.
a.
O
2-
b. Mg
2+
c. Ne
d. F
-
e.
Al
3+
2.
Which of the following has the highest EA1.
a.
Na
b. C
c. N
d. F
e. Li
3.
What happens to an atom’s radius when it loses an electron?
a.
It gets larger
c.
It stays the same
b.
It gets smaller
d.
It depends
4.
What possible element has the following ionization energies (all in kJ/mol)?
IE
1
= 786
IE
2
= 1580
IE
3
= 3230
IE
4
= 4360
IE
5
= 16100
a.
Si
b.
P
c.
Al
d.
Mg
e.
Cl
5.
Which reaction below represents the
electron affinity
of K?
a. K(g) + e⁻ → K⁻(g) + EA1
b.
K(g) + EA1 → K⁺(g) + e⁻
c.
K(g) + e⁻ → K⁺(g)
+ EA1
d.
K⁺(g) + e⁻ → K(g) + EA1
e.
K⁺(g) + EA1→ K (g) + e⁻
6.
(2 points) Which of the following is not correct?
a.
n = 3
l
= 3
m
l
= 0
c.
n = 2
l
= 1
m
l
= 0
b.
n = 5
l
= 1
m
l
= -1
d.
n = 4
l
= 2
m
l
= -2
e. None of above
7.
(2 points) How many nodes in 5s orbital?
a.
0
b.
1
c.
2
d.
3
e.
4
8.
How many orbitals are contained in the third principal level (
n
= 3) of a given atom?
a. 8
b.
18
c.
10
d.
9
e.
5
9.
Theoretically, how many 15p orbitals exist?
a.
1
b.
3
c.
5
d.
7
e.
9
Name: __________________
10.
If ℓ = 0, which of the following may be true?
a
. n=6
b.
m
l
= -1
c.
m
l
= + 1
d.
m
s
= 0
e.
m
s
= +1
11.
Identify the correct values for a 2p sublevel
a. n = 2,
l
= 2, m
l
=0
c.
n = 2,
l
= 1, m
l
= 2
b. n = 2,
l
= 1, m
l
=-1
d.
n= 3,
l
= 1, m
l
= -1
12.
What are the possible values of quantum numbers
for an electron in a 4 f orbital?
a.
n = 4 and
l
= 3
c.
n = 3 and
m
l
= -2, -1, 0, +1, or +2
b.
n = 3 and
m
l
= -2, -1, 0, +1, +2
d.
n = 4 and
l
= 4
13.
Give the expected ground-state configuration of Cd (Z=48).
a.
[Kr] 5s
2
4d
10
b.
[Kr] 5s
2
4d
10
5p
2
c.
1s
2
2s
2
2p
6
3s
2
3p
6
3d
10
d.
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
14.
A Bohr model of an atom of hydrogen is shown in the figure. Which transition(s)
depicted by arrows result in energy emission, found as a line in the atomic emission
spectrum?
n
= 1
n
= 2
n
= 3
(1)
(2)
(3)
(4)
a.
Only 1
b.
Only 1 and 4
c.
Only 2
d. Only 2 and 3
15.
What are the possible values of quantum numbers
for an electron in a 4 f orbital?
a.
n = 4 and
l
= 3
c.
n = 3 and
m
l
= -2, -1, 0, +1, or +2
b.
n = 3 and
m
l
= -2, -1, 0, +1, +2
d.
n = 4 and
l
= 4
16.
What is the maximum number of electrons that can have the following set of quantum numbers? n = 4,
ℓ = 2, m
ℓ
= 1, m
s
= -½
a.
1
b. 3
c. 7
d. 6
e. 14
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17.
(4 points)What is the noble gas configuration of Zn
2+
?
Is this cation paramagnetic or
diamagnetic?
[Ar] 3d
10
Diamagnetic
Name:
Quiz 3
E=hν
λ =h/mv
1/λ = R(1/m
2
-1/n
2
)
h: 6.6x10
-34
Js
R= 1.097x10
-2
nm
-1
1.
(2 points)What are the possible values of quantum numbers for an electron in a 4 d orbital?
a.
n = 4 and
l
= 3
c.
n = 3 and
m
l
= -2, -1, 0, +1, or +2
b.
n = 4 and
m
l
= -2, -1, 0, +1, +2
d.
n = 1, 2, 3, 4 and
m
l
= -2, -1, 0, +1, +2
2.
(2 points)Which of the following has the largest radius.
a.
Ca
b. Cl
-
c. P
3-
d. S
2-
e.
They are the same
3.
(2 points)Which of the following has the highest IE1.
a.
Cs
b. Cl
c. Na
d. Al
e. Not enough info
4.
(2 points)What happens to an atom’s radius when it gains an electron?
a.
It gets larger
c.
It stays the same
b.
It gets smaller
d.
It depends on situation
5.
What possible element has the following ionization energies (all in kJ/mol)?
IE
1
= 578
IE
2
= 1820
IE
3
=
2750
IE
4
= 11600
a.
Al
b.
P
c.
Si
d.
Mg
e.
Cl
6.
Which reaction below represents the
ionization
energy of F?
a.
F(g) + e⁻ → F⁻(g) +IE1
b.
F(g) +IE1 → F⁺(g) + e⁻
c.
F(g) + e⁻ → F⁺(g) +IE1
d.
F⁺(g) + e⁻ → F(g) +IE2
7.
Give the set of four quantum numbers that represent the
last electron added
(using the Aufbau
principle) to the Ni atom(atomic number 28).
a.
n
= 4,
l
= 3,
m
l
= 3,
m
s
= -
1
2
d.
n
= 3,
l
= 2,
m
l
= 0,
m
s
= -
1
2
b.
n
= 3,
l
= 1,
m
l
= 1,
m
s
= +
1
2
e.
n
= 3,
l
= 3,
m
l
= 2,
m
s
= -
1
2
c.
n
= 4,
l
= 2,
m
l
= 0,
m
s
= +
1
2
8.
(2 points) Give the expected ground-state configuration of Zn (Z=30).
a.
1s
2
2s
2
2p
6
3s
2
3p
6
3d
10
b.
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
c.
[Kr] 4s
2
3d
10
d.
[Kr] 4s
2
3d
10
4p
2
9.
(2 points) How many nodes in a 5p orbitals?
a.
0
b.
1
c.
2
d.
3
e.
4
Name: _______________
10. (2 points) Which of the following is not correct?
a.
n = 3
l
= 1
m
l
= -1
c.
n = 6
l
= 4
m
l
= 0
b.
n = 1
l
= 1
m
l
= 0
d.
n = 7
l
= 2
m
l
= -1
11. How many orbitals are present when
l
= 0?
a. 1
b.
3
c.
5
d.
7
e.
It does not exist
12. What are the possible values of quantum numbers for an electron in a 4 d orbital?
a.
n = 4 and
l
= 3
c.
n = 3 and
m
l
= -2, -1, 0, +1, or +2
b.
n = 4 and
m
l
= -2, -1, 0, +1, +2
d.
n = 1, 2, 3, 4 and
m
l
= -2, -1, 0, +1, +2
13. (2 points) Which species has this ground-state electron arrangement?
1
s
2
2
s
2
2
p
6
3
s
2
3
p
6
3
d
10
a.
Ni
b.
Ni
2+
c. Zn
d.
Zn
2+
14. Give the set of four quantum numbers that represent the
last electron added
(using the Aufbau
principle) to the Ni atom(atomic number 28).
a.
n
= 4,
l
= 3,
m
l
= 3,
m
s
= -
1
2
d.
n
= 3,
l
= 2,
m
l
= 0,
m
s
= -
1
2
b.
n
= 3,
l
= 1,
m
l
= 1,
m
s
= +
1
2
e.
n
= 3,
l
= 3,
m
l
= 2,
m
s
= -
1
2
c.
n
= 4,
l
= 2,
m
l
= 0,
m
s
= +
1
2
15. Which atomic orbital corresponds to this set of quantum numbers in a ground state atom of
boron?
(2, 1, –1, ½)
a.
b.
c.
d.
16. What is the maximum number of electrons that can have the following set of quantum numbers?
n = 4, ℓ = 3, mℓ = 3, ms = -½
a.
1
b. 3
c. 7
d. 6
e. 14
17. (4 points) What is the noble gas configuration of Cu
+
?
Is this cation paramagnetic or
diamagnetic?
[Ar] 3d
10
Diamagnetic
Name:
Quiz 3 Makeup
E=hν
λ =h/mv
1/λ = R(1/m
2
-1/n
2
)
h: 6.6x10
-34
Js
R= 1.097x10
-2
nm
-1
1.
Which of the following has the smallest radius.
a.
O
2-
b. Mg
2+
c. Ne
d. F
-
e.
Al
3+
2.
Which of the following has the lowest EA1.
a.Na
b. C
c. N
d. F
e. Li
3.
What happens to an atom’s radius when it loses an electron?
a.
It gets larger
c.
It stays the same
b.
It gets smaller
d.
It depends
4.
What possible element has the following ionization energies (all in kJ/mol)?
IE
1
= 577
IE
2
= 1820
IE
3
= 2750
IE
4
= 11600
IE
5
= 14800
a.
Si
b.
P
c.
Al
d.
Mg
e.
Cl
5.
Which reaction below represents the
electron affinity
of K?
a. K(g) + e⁻ → K⁻(g) + EA1
b. K(g) + EA1 → K⁺(g) + e⁻
c.
K(g) + e⁻ → K⁺(g)
+ EA1
d.
K⁺(g) + e⁻ → K(g) + EA1
e.
K⁺(g) + EA1→ K (g) + e⁻
6.
Give the set of four quantum numbers that represent the
first electron removed
(using the
Aufbau principle) to the Ni atom(atomic number 28).
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a.
n
= 4,
l
= 1,
m
l
= 3,
m
s
= -
1
2
d.
n
= 3,
l
= 2,
m
l
= 0,
m
s
= -
1
2
b.
n
= 3,
l
= 1,
m
l
= 1,
m
s
= +
1
2
e.
n
= 3,
l
= 3,
m
l
= 2,
m
s
= -
1
2
c
.
n
= 4,
l
= 0,
m
l
= 0,
m
s
= +
1
2
7. Write the complete ground-state electron configuration of Fe²⁺.
a.
1s²2s²2p⁶3s²3p⁶3d⁶
b.
1s²2s²2p⁶3s²3p⁶4s
2
3d
8
c.
1s²2s²2p⁶3s²3p⁶4s
2
3d
4
d. .
1s²2s²2p⁶3s²3p⁶3d
5
e.
1s²2s²2p⁶3s²3p⁶4s
2
3d
3
8.
Theoretically, how many 15d electrons exist?
a.
1
b.
3
c.
5
d.
7
e.
10
9. If ℓ = 0, which of the following may be true?
a
. n=6
b.
m
l
= -1
c.
m
l
= + 1
d.
m
s
= 0
e.
m
s
= +1
10.
Which atomic orbital corresponds to this set of quantum numbers in a ground state
atom of boron?
(2, 1, –1, -½)
a.
b.
c.
d.
11.
How many orbitals are contained in the third principal level (
n
= 3) of a given atom?
a. 8
b.
18
c.
10
d.
9
e.
5
12.
If ℓ = 0, which of the following may be true?
a
. n=6
b.
m
l
= -1
c.
m
l
= + 1
d.
m
s
= 0
e.
m
s
= +1
13. Identify the correct values for a 2p sublevel
a. n = 2,
l
= 2, m
l
=0
c.
n = 2,
l
= 1, m
l
= 2
b. n = 2,
l
= 1, m
l
=-1
d.
n= 3,
l
= 1, m
l
= -1
14. What possible values of quantum numbers is wrong
for an electron in a 4 d orbital?
a.
n = 4 and
l
= 2
c.
n = 4 and
m
l
= -2, -1, 0, +1, or +2
b.
n = 4 and
m
s
= -1/2, +1/2
d.
n = 4 and
l
= 3
15. Give the expected ground-state configuration of Cu (Z=29).
a.
[Ar] 4s
2
3d
10
b.
[Ar] 5s
2
4d
10
5p
2
c.
1s
2
2s
2
2p
6
3s
2
3p
6
3d
10
d.
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
9
e.
1s
2
2s
2
2p
6
3s
2
3p
6
4s
1
3d
10
16. (5 points) What is the noble gas configuration of Scandium?
How many charges carried by
Scandium is the most stable ion.
[Ar] 4s
2
3d
1
+3
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ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
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- Pls help ASAParrow_forwardFocus+Concept+Review+Quantum+and+Electron+Configuration [Modo de compatibilidad] - Microsoft Word DISEÑO DE PÁGINA REFERENCIAS CORRESPONDENCIA REVISAR VISTA 12 Aa - A:= ,- AaBbCcDc AaBbCcDc AaBbCc AaBbCcDc AaBbCcDc AaBbCo = x, x A - aly 1 Normal 1 Párrafo... 1 Puesto 1 Sin espa.. 1 Table Par.. 1 Texto i Fuente Párrafo 17 Estilos (3) Which set of quantum numbers cannot specify an orbital and state why not. a. n=2, l=1, m=-1 b. n=3, l=2, mı=0 C. n=3, l= 3, mj =2 d. n=4, l=3, mj=0 (4) Write the abbreviated electron configuration for each element and write the orbital diagram а. С b. P c. I d. Na OS UNIDOS) >> Escritorioarrow_forwardEcological Footprin... Gizmo: Electron Configuration Fill-in View Insert Format Tools Extensions Help P 100% Y Normal text T + to the document will New Tab +Revenge Gardening... 鬼 EE 7 Arial Symbol Cr Cu Au Last edit was Q Search 11 + G HEHE nutes ago *** "I, Too" by Langsto... B I U A BIUA GO 99+ Im IL I D. The following elements also do not follow the diagonal rule. Predict their electron configurations and write your prediction. Check it with the Gizmo and put the actual configuration in the table. = + I Predicted Electron Config. Actual Electron Config. D N E-1E = E Y Y *** * * : □ □ 4x D A X Share A 9:53 PM 3/22/2023 *** > + 20 31 .. O .. O 1arrow_forward
- Can you please help me answer thisarrow_forward6. An electron starts from rest 24.5 cm from a fixed point charge with Q = - 6.50 nC (-6.50 x 10 °C). How fast will the electron be moving when it is very far away. Mass of electron m =9.11 x 10-31 kg and charge of the electron is e = -1.6022 x 10-19 C.arrow_forwardPart A Place the following elements in order of decreasing atomic size: silicon, nitrogen, helium, potassium, magnesium, and carbon. Rank from largest to smallest. To rank items as equivalent, overlap them. Reset Help K Mg SiCN He Largest Smallest O The correct ranking cannot be determined. 37°F Mostly cloudy F7 F8 F9 F10 F11 F12 PrtSc Pause Ins Del A Scr Lk SysRq Break & + Backspacearrow_forward
- In each of the following pairs, which has the bigger radius? 0²- Mg2+ N F P p3- Rb+ W: X: Y: Z: A. B. C. D. E. B E C A W K+ X Mg2+ N Mg²+ F 0²- 0²- Y Z p3- P N P p3- N Mg2+ F p3- K+ K+ Rb+ Rb+ K+arrow_forwardCe CEstelae et O Empower 2021 O ir A educate.lindsay.k12.ca.us/iFrame.aspx?iCtrl-STUDENT BASE HOME CONTROL Bookmarks IXI O Impower 2020 E Google Docs č indsay High School R Physics Safety & Sk. E Gided practice 3L Why does the atomic radius get smaller as you go toward the right side of the penodic table? As you move to the right on the penodic table, the number of protons in the nucleus increases, which makes the nucleus O A more attracted to the electrons and pulls the rings inward making the radius of the atom smaller. As you move to the right on the periodic table the atoms become older and begin to shrink. This causes the overall radius of the atom to be smaller on the left side of the periodic table. Because the number valence electrons increases as you move to the right on the perioic table, the valence shell becomes more creowded and causes the atomic radius to be smaller on the left side of the table. Although the atomic mass increases as you move to the right side of the…arrow_forwardPls help ASAParrow_forward
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