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I forgot how to check for ionization energy, and that led for me getting questions wrong because I was ordering them in the wrong direction.

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Which of the following is in correct order by increasing ionization energy?

A.) Ir < Pd < Cu < S
B.) Zr < La < Ra < Fr
C.) Si < Ge < Sn < Pb
D.) Os < Re < W < Ta

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Which of the following has the greatest ionization energy?

Why does Oxygen have a higher amount of ionization energy when compared to Aluminum?

Oxygen has more ionization energy when compared to Aluminum because it's valence electrons are located much closer to it's nucleus than Aluminum's, which means that it's harder to remove them.

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I most likely missed these questions due to careless mistakes and/or forgetting/being unsure of the rules of the trend.

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Put the following elements in order of decreasing ionization energy.
Ni , Si , P, N

a) Ni > Si > P > N
b) N > P > Si > Ni
c) Ni > P > Si > N
d) N > Si > P > Ni

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Would the ionization energy be higher in a 1s sub-shell or in a 2s sub-shell?

The ionization energy would be higher in a 1s sub-shell because it has a stronger nuclear charge and is therefore harder to remove electrons.

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(Avery Lowrance)
When you move down a column of the periodic table does ionization energy increase or decrease and why?
Decreases, because the nuclear charge decreases and therefore, it's easier to lose an electron

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(Avery Lowrance)
Which element has the highest ionization energy?
A. C
B. Si
C. Ge
D. Sn

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I missed these because I flip flopped which way increases and decreases-spencer

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I missed these because I flip flopped which way increases and decreases-spencer

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Explain why Ar has a higher ionization energy than S. Ar has a higher ionization energy than S because it has more valence electrons.

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Multiple choice: Which element has the highest ionization energy?
A) Cl
B) S
C) P
D) Si
What does highest ionization really mean? The ionization energy is the amount of energy it takes to remove the valance electrons from the energy levels. Therefore it is the highest when it is closest to the nucleus because it is hardest to pull from there.

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Why does the Ionization energy down up the farther down on the periodic table?

As the energy levels increase the nuclear charge decreases.

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Why I missed these questions - Ethan Kraft

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Why I missed these questions - Ethan Kraft

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It all boils down to me using "everybody wants to be a noble gas" a little too much, as this topic doesn't have to do with that as much as it has to do with nuclear charge and valence electrons.

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Which element has the least ionization?

A Rb
B As
C Mn
D F

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Explain why noble gases have a higher ionization energy than other elements.
Noble gases have the most valence electrons in the PT, meaning they are bound tightest together, and therefore require the most amount of energy to separate.

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Which of the following elements has the lowest ionization energy?
A) F
B) Zr
C) O
D) Fe

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Why I Missed These Questions (Paityn York)

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Why I Missed These Questions (Paityn York)

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I feel somewhat confident about this topic, I just got confused when the questions began to talk about ionization energies beyond the first.

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Explain why P has a higher ionization energy than Al.

Phosphorous has a higher ionization energy because it has more valence electrons and more protons. These create a greater effective nuclear charge, pulling the atom in tighter, and making it harder to remove electrons from P than from Al.

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Which of the following has the highest ionization energy?

a) Cl
b) Sn
c) Rb
d) Ga

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I missed these questions because I was getting them confused with nuclear charge and I was getting confused on the order in which the trend goes. I also can get very confused on the topic in general.

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Out of the following elements, which has the lowest ionization energy?
A. K
B. Ne
C. Ga
D. Ba

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Why I missed these questions - James Voos

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Why I missed these questions - James Voos

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I miss read some of the questions and charts involving ionization energy.

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I missed these questions because I got confused when the second ionization energy was asked.

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Explain why the first ionization energy of Fluorine is greater than that of Arsenic.

Fluorine has a higher first ionization energy than Arsenic because Fluorine only has 2 energy levels, whereas Arsenic has 4 energy levels. This means that taking one electron away from Fluorine is more difficult than Arsenic because the electrons of Fluorine are closer to the nucleus and experience are stronger pull due to increased effective nuclear charge.

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I ran out of time and didn't think through my answer on one of the questions.

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Explain why S has a greater ionization energy then Si.
S has a greater ionization energy then Si because S has a greater nuclear charge which increases the nuclear pull on electrons which then requires more energy to remove the valence electrons

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Select the element that has the highest first ionization energy.

A. Fluorine
B. Arsenic
C. Thallium
D. Barium

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Which element listed has the lowest first ionization energy?
a)Y
b)Hs
c)Cd
d)Ar

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Which group on the periodic table has the highest first ionization energy required and why.
The Noble gasses because they have a full outer level of electrons, and a high effective nuclear charge.

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Put in order from least ionization energy to most K, P,  Ne,  Cl, and Fr.
The order would be Fr, k, P, Cl, and Ne.

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Which of these are in order of increasing ionization energy?
A) O, P, Ge, In
B) F, Cl, Br, I
C) Cs, Ca, Si, O
D) Cs, Ca, Na, Si

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What is Ionization Energy?

Ionization energy is the amount of energy it takes to take away an electron from an atom's outer shell of valence electrons.

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Which of the following has the smallest ionization energy?

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Which of the following has the smallest ionization energy?

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a. Carbon
b. Gallium
c. Titanium
d. Yttrium

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I missed these questions when comparing elements in different periods. I also missed these questions because I didn't know how to explain my answer without using the location on the periodic table.

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This gets a little confusing for me, but I think I’ve got it.

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Why is it easier to remove electrons from Mg, than it is from Fe?

Answer: It is easier to remove valence electrons from Mg because it has a lower ionization energy level.
(Hope McNish)

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Which element has the highest first ionization energy?
A. Argon
B. Selenium
C. Potassium
D. Bismuth

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Which of the following has the greatest ionization level?

a. Cs

b. Be

c. B

d. Ba
(Hope McNish)

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Why I missed these questions. (Jay Patel)

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Why I missed these questions. (Jay Patel)

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I was overthinking the questions and could not properly word my answers to fully answer the questions.

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Why does Argon possess greater ionization energy than Iodine?

Argon possess greater ionization energy because it becomes more difficult to remove valence electrons due to a greater electrostatic attraction between the electrons and the nucleus, as opposed to Iodine, which possesses more energy levels making the valence electrons further away from the nucleus. This increased distance results in less electrostatic attraction and lower ionization energy.

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Which of the following groups on the Periodic Table would contain the highest first ionization energies?
A. Alkali Metals
B. Halogens
C. Transition Metals
D. Noble Gases
Correct Answer: Noble Gases

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Put the following elements in order of increasing ionization energy: Ti, N, Cu, P, Sc

Sc, Ti, Cu, P, N

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Which of the following elements has the lowest ionization energy?

A. K
B. O
C. Na
D. Al

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Explain why O has a higher ionization energy than N.

Answer: Oxygen has a higher ionization energy than Nitrogen , because they are on the same energy level, but Oxygen has one more proton making it have a greater effective nuclear charge  and making it more difficult to lose an electron.

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Why I got these questions wrong- Ashley Armendariz

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Why I got these questions wrong- Ashley Armendariz

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I got the direction in which the ionization energy increases wrong, which caused me to eliminate the correct answer and choose the opposite of what the question was asking.

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Which set of elements are in order of increasing ionization energy?
A. K<Ca<Sc<Ti
B. N<C<B<Li
C. H<Li<Na<K
D. H<Na<K<Li

Answer: A

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I made careless errors by miscounting the amount of valence electrons needed to make the ionization energy jump.

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What trend is followed when it comes to increasing ionization energy?

A: Up and to the right (noble gasses are included)

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Put these elements in order of decreasing ionization energy. (Li, F, Ba, K)
A) Ba, K, Li, F
B) F, Li, K, Ba
C) Li, K, Ba, F
D) F, K, Li, Ba

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I made errors with analyzing ionization energy by incorrectly looking at elements from moving to the right and then going up, which caused me to arrive at wrong numbers.

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How is ionization energy affected by an atom’s number of energy levels and protons.

Answer: As an atom increases in energy levels, its ionization energy decreases, because the valence electrons of an atom are getting farther away from the nucleus. This results in a lessening effective nuclear charge, making it easier to pull away electrons. So, as the number of energy levels decrease, the ionization energy increases. An increasing number of protons results in a greater electrostatic attraction and nuclear charge. This makes for more ionization energy required. So, a lesser number of protons, compared between elements in the same energy level, result in a lesser ionization energy needed.

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Which element has the highest first ionization energy?

A) O
B) N
C) I
D) K

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Which element has the greatest ionization energy?
A. I
B. Ar
C. Zr
D. Os

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Put these elements in order of decreasing ionization energy:

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Put these elements in order of decreasing ionization energy:

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Co, F, Rn, Sr

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I was confused on the FIRST ionization and SECOND ionization and what it all meant.

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Would an atom with more energy levels have a greater first ionization or a atom with less energy levels?

An atom with less energy levels would have a greater nuclear charge compared to an atom with more energy levels as it has a weaker nuclear charge.

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Which element listed his the highest first ionization energy?

A) Boron
B) Radium
C) Potassium
D) Iron

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Why I missed these questions. (Patrick Chan)

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Why I missed these questions. (Patrick Chan)

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I missed these questions due to making mistakes but I understand these questions.

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Why I got these questions wrong - Richard Whitfield

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Why I got these questions wrong - Richard Whitfield

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I did not think to write out the up/down configuration of arrows as well as electron configuration so I was unable to determine the correct answer.

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What may cause a discrepancy in the trend of ionization energy for an atom of Oxygen? Explain your answer.
Electron-Electron repulsion, caused by the presence of two electrons pushing away from each other, creates discrepancies in ionization energy trends. For an atom of Oxygen, the electron configuration ends in "2s4" which creates electron-electron repulsion that forces an atom to become larger in its radius. An atom with a larger radius has less ionization energy.

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I understand these however I made some careless mistakes.

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Which of the following lists a group of elements with decreasing first ionization energy?
A. Ba<O<Kr
B. P>Mn>Cs
C. O>Ge>Ne
D. Hf<Ba<Te
E. Fr>Mg>O

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Put the elements in order of increasing ionization energy.
Co, Rb, N, Al

a. Rb, Co, N, Al
b. N, Al, Co, Rb
c. N, Rb, Al, Co
d. Rb, Co, Al, N

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Why does Fluorine have a higher first ionization energy than Mercury?
Fluorine's first ionization energy is higher than Mercury because the electrons are closer to the nucleus in Fluorine. When the electrons are closer to the nucleus they are being pulled in more.

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What element the highest first ionization energy?
A. Neon
B. Flourine
C. Rubidium
D. Francium

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When you move from right to left and down towards Fr on the periodic table, what does you ionization energy do?

Your ionization energy decreases because you are getting further away from Helium which is the point of highest ionization energy.

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I mix this trend up with the radius trend and second guess myself.

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Which direction on the periodic table do you go to get a higher ionization energy?

Up and to the right.

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Which has the lowest ionization energy?

A.) Ne
B.) He
C.) Be
D.) H

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Which of these elements have the highest first ionization energy?
A. Ne
B. Al
C. Mn
D. Ac

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When you compare the ionization energies of Ne and Li, which one would have the greater ionization energy and why?

Because, Ne is a noble gas and it is already stable, so it has no more valence electrons to be removed.

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Why does the ionization energy of Ar, when compared to Al, rely on Nuclear charge?

The only difference between Al and Ar related to ionization energy is the amount of protons. Because there are more protons in Ar, its greater effective nuclear charge causes a higher ionization energy.

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Between Ne and F, which has a higher ionization energy and why?

A) The Atomic mass causes a greater electrostatic attraction
B) F, There is a smaller greater effective nuclear charge
C) Ne, It has a greater effective nuclear charge
D) Ne, There are more energy levels

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Reasons for missing this question- Jenna Trantham

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Reasons for missing this question- Jenna Trantham

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Noble gasses are included! This deals with the removal of valence electrons.

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Why is it easier to remove electrons from the outer ring?

Answer: The electrons on the outer ring are the valence electrons and are further away from the nucleus making the electrostatic attraction decrease.

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I missed these questions because I found it hard to distinguish between the first and second ionization energies.

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Explain what second ionization energy is.

Answer: Second ionization energy is the amount of energy it takes to remove the second electron from an element.

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I simply was rushing through the test

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Why I missed these questions Natalia Wilson

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Why I missed these questions Natalia Wilson

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Not judging the jumps in ionization energy correctly led to me identifying elements incorrectly.

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Explain why noble gasses have the highest ionization energy

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Ionization energy _____ as you move towards the noble gasses and increases as you go ______ the periodic table.
A Increases, Down
B Increases, Up
C Decreases, Down
D Decreases, Up

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What happens to the ionization energy as you travel from right to left?

A. Decreases because the nuclear charge decreases
B. Decreases because there are less neutrons.
C. Increases because the number of isotopes decreases.
D. Increases because the energy level is about to change.

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Sometimes I mix up questions and do them backwards.

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Which has the greatest first ionization energy?
a. Sr
b. Hf
c. Te
d. C

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Which element has greater first ionization energy Al or Si, explain.
Si, because it has more protons which increases the electrostatic attraction and nuclear charge therefore making it more difficult to remove an electron.

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Which element has a lower first ionization energy: Mg or Ca? Explain your answer.

answer: Ca because it has more energy levels therefore the valence electrons are further from the nucleus and are less affected by the nuclear charge.

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Which element below has the highest ionization energy?

a. Cl

b. Na

c. Fr

d. W

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Why I missed these questions (Victoria Contreras

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Why I missed these questions (Victoria Contreras

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I missed these questions because I got confused when comparing ionization energies in order to identify elements.

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On an ionization energy chart,  why is the energy lowest in the box labeled 1st?
A). The energy is never lowest in the first box.
B). Not as much energy is required in the first level do to it being a valence electron.
C). There are more protons and neutrons.
D). There is more electrostatic attraction in this level.

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Why is it hard to take electrons from a noble gas? Answer: The electrostatic attraction is strong because Noble gases ave a full shell of 8 valence electrons.

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Which element has the highest initial ionization energy?
a.Kr
b.Po
c.Mg
d.H
Answer: Po

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Explain why Na has a higher first ionization energy than K.

Na has a higher first ionization energy than K because it has 3 energy levels while K has 4. This means that it has a stronger electrostatic attraction making it harder to remove electrons therefore requiring more energy.

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Which element has the lowest first ionization energy?
A) P
B) Ar
C) Cl
D) S

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Why I missed these questions Colby Dennis

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Why I missed these questions Colby Dennis

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I missed these questions because I didn't know that binding energy meant ionization energy.

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Why does Fluorine have higher ionization energy over Oxygen?

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Which has the highest first ionization energy?
A. N
B. O
C. F
D. Ne

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Which of the following atoms have the highest second ionization energy?
A. Al
B. Rb
C. Ca
D. Na
E. Fr

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Why I missed these questions (Maggie Schall)

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Why I missed these questions (Maggie Schall)

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I missed these questions because I was mixing up the different trends in my head.

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Which element would have the lowest ionization energy?

A. F
B. Ru
C. O
D. Ba

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Out of the following ions, which doesn't have the least First Ionization Charge?

A. Br^-
B. Ga^3+
C. Rb^+
D. Ga^3-