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Unit 3 Electron Configuration & Periodic Trends Formative 2025

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Question 1
1.

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Question 2
2.

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Question 3
3.

Question 4
4.

Question 5
5.

Question 6
6.

Question 7
7.

Question 8
8.

Question 9
9.

Question 10
10.

Question 11
11.

Question 12
12.

Question 13
13.

Question 14
14.

Question 15
15.

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Question 16
16.

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Question 17
17.

Which of the following has the larger atomic radius?

phosphorus or antimony

Question 18
18.

Which of the following has the larger atomic radius?

zinc or titanium

Question 19
19.

Which of the following has the larger atomic radius?

strontium or magnesium

Question 20
20.

Which of the following has the larger atomic radius?

manganese or germanium

Question 21
21.

Which of the following has the larger atomic radius?

boron or fluorine

Question 22
22.

Which of the following has the lower ionization energy?

platinum or nickel

Question 23
23.

Which of the following has the lower ionization energy?

potassium or selenium

Question 24
24.

Which of the following has the lower ionization energy?

calcium or cobalt

Question 25
25.

Which of the following has the lower ionization energy?

silicon or tin

Question 26
26.

Which of the following has the lower ionization energy?

fluorine or iodine

Question 27
27.

Which of the following has the lower electronegativity?

francium or potassium

Question 28
28.

Which of the following has the lower electronegativity?

cadmium or tellurium

Question 29
29.

Which of the following has the lower electronegativity?

arsenic or nitrogen

Question 30
30.

Which of the following has the lower electronegativity?

chlorine or aluminum

Question 31
31.

Which of the following has the lower electronegativity?

calcium or bromine

Question 32
32.

Which of the following has the smaller atomic radius?

fluorine atom or fluorine ion

Question 33
33.

Which of the following has the smaller atomic radius?

H or H+

Question 34
34.

Which of the following has the smaller atomic radius?

O or O-2

Question 35
35.

Which of the following has the smaller atomic radius?

magnesium ion or magnesium atom

Question 36
36.

Which of the following has the smaller atomic radius?

sulfur ion or sulfur atom

Question 37
37.

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Question 38
38.

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39.

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Question 40
40.

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Question 41
41.

Which element has the following electron configuration

[Kr]5s24d10

Question 42
42.

Which element has the following electron configuration

1s22s22p63s23p4

Question 43
43.

Write the electron configuration for the following: NO SPACES

Iodine

Question 44
44.

Write the electron configuration for the following: NO SPACES

Tungsten

Question 45
45.

Write the electron configuration for the following: NO SPACES

Silicon

Question 46
46.

Write the noble gas notation for Chlorine. NO SPACES

Question 47
47.

What is the principle quantum number of the last drawn electron of chlorine?

Question 48
48.

What is the aziumuthal quantum number of the last drawn electron of chlorine?

Question 49
49.

What is the spin quantum number of the last drawn electron of chlorine?

Question 50
50.

How many unpaired electrons does sulfur have?

Question 51
51.

What is the noble gas notation of sodium? NO SPACES

Question 52
52.

What is the principle quantum number of the last drawn electron of sodium?

Question 53
53.

What is the azimuthal quantum number of the last drawn electron of sodium?

Question 54
54.

What is the spin quantum number of the last drawn electron of sodium?

Question 55
55.

How many unpaired electrons does sodium have?

Question 56
56.

What is the noble gas notation for oxygen? NO SPACES

Question 57
57.

What is the principle quantum number of the last drawn electron of oxygen?

Question 58
58.

What is the azimuthal quantum number of the last drawn electron of oxygen?

Question 59
59.

What is the spin quantum number of the last drawn electron of oxygen?

Question 60
60.

How many unpaired electrons does oxygen have?

Match the following vocabulary to the correct definition.
Cation
Group you would find Rutherfordium
4
Number of electrons a full p orbital hold
Ionization Energy
Number of valence electrons the ground state of chlorine
Alkaline Earth Metals
The name of the quantum number that indicates the sublevel of electrons
Magnetic
The quantum number that represents the direction in which the electrons are traveling with either up and down arrows: +1/2, -1/2
Ionic
The name of the quantum number that indicates the orientation of an orbital around the nucleus
Noble Gas
The name of the quantum number that indicates the size of the atom
6
Group of elements that are considered to be electronically perfect
Azimuthal
Bond that forms between anions and cations as a result of the transfer of valence electrons
Atomic Radius
the name of the group that has 2 valence electrons and is found in compounds in nature
Principle
The name of the group of elements that has 1 valence electron, from very strong bases, and explode in water
d
Bond that forms by the sharing of electrons between two nonmetals
Alkali Metals
Electrons are found in the last main level of an atom
Electronegativity
Group where you would find radon
7
Ion that tungston will form
Covalent
Block you would find fluorine
18
Block you would find iridium
Valence
One-half the distance between nuclei of identical atoms that are bonded together
p
The energy required to remove the valence electrons from an atom
Spin
The measure of the ability of an atom in a chemical compound to attract electrons.
Match the scientist to their correct contribution to the quantum theory
Bohr
Published the first periodic table
Louis De Broglie
Said that it is not possible to know both the location and the speed of an electron at the same time.
Max Planck
He said that electrons act like waves with certain frequencies. He studied the photoelectric effect
Erwin Schrodinger
His works lead to the Periodic Law, which states that the physical and chemical properties of the elements are periodic functions of their atomic numbers
Hund
Said that electrons have both wave and particle nature
Dmitri Mendeleev
Suggested that hot objects emit energy in small, specific amounts called Quanta
Heisenberg
He stated that electromagnetic radiation had wavelike properties, that particles "stream," and each particle of light carries a quantum of energy
Albert Einstein
Said that electrons remain unpaired as long as possible
Henry Moseley
Said that electrons travel around the nucleus like planets orbiting the sun
Which of the following has 4 valence electrons?
carbon
oxygen
helium
hydrogen
nitrogen
Which of the following has 2 valence electrons?
helium
hydrogen
carbon
oxygen
nitrogen
Which of the following is an transition metal?
chlorine
astatine
lithium
helium
copper
Which of the following has 6 valence electrons?
fluorine
potassium
helium
oxygen
nitrogen
Which of the following is a halogen?
nitrogen
bromine
helium
carbon
sodium
Which of the following is a alkaline earth metal?
argon
magnesium
sodium
chlorine
zinc
Which of the following is an alkali metal?
sodium
chlorine
magnesium
argon
arsenic
Which of the following is an "d" block element?
chlorine
titanium
lithium
arsenic
gallium
Which of the following is a "s" block element
arsenic
chlorine
gallium
lithium
titanium
Which of the following is a halogen?
arsenic
barium
chlorine
argon
iron
Categorize the following elements into the type of ion each would form.
oxygen
carbon
nitrogen
lithium
sulfur
chromium
iodine
silver
tin
sodium
nickel
calcium
Cation
Anion
Categorize the following pairs into the type of bond they would have
phosphorus & iodine
zinc & selenium
lead & sulfur
carbon & oxygen
calcium & nitrogen
potassium & bromine
aluminum & oxygen
iodine & chlorine
Ionic
Covalent
Match the number of energy levels required to draw each of the following elements.
2
hydrogen
5
carbon
4
tin
3
barium
1
phosphorus
6
calcium
Match the following elements to their corresponding number of valence electons.
5
potassium
4
helium
8
aluminum
3
silicon
2
nitrogen
1
krypton
Match the following to their corresponding number of electrons found in that energy level.
3
2 electrons
4
8 electrons
2
18 electrons
1
32 electrons
Match the following sublevels to their corresponding number of orbitals.
f
1 orbital
d
3 orbitals
s
5 orbitals
p
7 orbitals
Match the following sublevels to their corresponding number of electrons when they are full.
p
2
f
6
s
10
d
14
Match the following elements to their corresponding number of unpaired electrons.
boron
3
chromium
1
lead
0
bismuth
2
mercury
4