Ionization Energy by Shaun Bock

Multiple Choice

2017-09-25 15:15:47 UTC

Which direction on the periodic table does ionization energy increase?

A. Up to down
B. Left to right
C. Right to left
D. Diagno

Free Response

2017-09-25 15:19:34 UTC

Explain why ionization energy increases as you move right on the periodic table.

Multiple Choice

2017-09-25 15:52:23 UTC

(Abby Brewer)
Which of the following elements has the lowest ionization energy?

a. Fr
b. Na
c. K
d. Rb

Free Response

2017-09-25 15:54:11 UTC

(Abby Brewer)
Explain why ionization energy increases as you move up the periodic table.

Answer: Ionization energy increases as you move up on the periodic table because as you move up, you lose energy levels. This means that the valence electrons are closer to the nucleus, so it's harder to remove them.

Multiple Choice

2017-09-25 17:14:38 UTC

Which of the following groups has the highest ionization energy?
a) Alkali earth metals
b) Halogens
c) Noble Gases
d) Radioactive Elements

Free Response

2017-09-25 17:23:56 UTC

Explain the pattern of ionization energy on the periodic table.
Ionization energy increases from down to up and from

Explanation

2017-09-25 17:25:02 UTC

I mixed up ionization energy with ions in general.

Explanation

2017-09-25 17:55:41 UTC

I don't pay attention to the test during the whole test. Sometimes I just faze out.
(Rob)

Multiple Choice

2017-09-25 17:57:23 UTC

(Rob)
Which has a higher first ionization energy?
A. Y
B. N
C. C
D. Zr

Free Response

2017-09-25 18:01:40 UTC

(Rob)
What is ionization energy and why does ionization energy decrease as there are more energy levels?

A: Ionization energy is the energy required to take an electron from an atom. It increases with more energy levels because the electrons get farther away from the nucleus. This decreases the electrostatic attraction between the nucleus and the valence electrons.

Explanation(Caden Ryan)

2017-09-25 18:03:13 UTC

My situation for these kinds of problems is that I mix up the relations with other Periodic Trends(Nuclear Charge), and how it's represented on the Table(Going away from N.G. instead of towards). How to fix this is to just clarify and familiarize myself with the trend of Ionization Energy and its connections to others.

Free Response(Caden Ryan)

2017-09-25 18:07:31 UTC

Explain why Ionization Energy increases as you move towards noble gases on the Periodic Table?

Response:
Ionization Energy increases as elements move towards noble gases due to the the nuclear charge also increasing. As an atom loses/gains electrons the nuclear charge responds by increasing its electrostatic attraction, therefore restraining the electrons still present and making it harder to remove future electrons.

Kacie

2017-09-25 18:07:53 UTC

Ionization energy refers to which of the following?
A. The amount of energy it takes to remove an electron in a element as you move across a period
B. The energy that an ion of an element possesses
C. How much energy is required to remove a proton
D. The amount of attraction that an element has to gain or lose electrons.

Connor Gary

2017-09-25 18:08:12 UTC

I messed up my definition on the free response. and Im still shook about it.

Free Response

2017-09-25 18:08:49 UTC

Connor Gary
Describe the reason why the first ionization energy of fluorine greater than that of carbon?

Multiple Choice

2017-09-25 18:09:46 UTC

Which Of the following elements has the lowest Ionization Energy?

2017-09-25 18:10:07 UTC

a. Fr
b. Po.
C. Ar.
D. Zr
E. Ba

Connor Gary

Why Did I Get These Questions Wrong? (Chloe Russell)

2017-09-25 18:13:04 UTC

I got these questions wrong because of juvenile and careless mistakes.

Free Response (Chloe Russell)

2017-09-25 18:15:17 UTC

Explain why the first ionization energy of atomic Chlorine is greater than that of atomic Sulfur.
The first ionization energy of atomic Chlorine is greater than that of Sulfur because it's nuclear charge is greater because of high electrostatic attraction.

Multiple Choice (Chloe Russell)

2017-09-25 18:15:43 UTC

Which of the following has the highest third ionization energy?
A) Nitrogen
B) Carbon
C) Calcium
D) Vanadium

Multiple Choice (Adira Abdullah)

2017-09-25 19:08:01 UTC

Which of the following would have the highest ionization energy?
A. Zn
B. B
C. K
D. Ga

Free Response (Adira Abdullah)

2017-09-25 19:09:02 UTC

Why would Neon have a stronger ionization energy than Fluorine? Neon would have a stronger ionization energy because it has a stronger nuclear charge, causing it to become smaller than fluorine and making it harder to remove those valence electrons (requiring more ionization energy).

Multiple Choice (Landon Webb)

2017-09-25 19:10:33 UTC

Which of the following would have the highest second ionization energy?
a. K
b. Na
c. Cu
d. Cl

Free response (Landon Webb)

2017-09-25 19:12:48 UTC

Explain why Ionization Energy decreases as you go closer to the far left corner on the periodic table.
As you get closer to the far left corner the farther away you are from the nucleuses electrostatic attraction making is easier

Why I missed these questions (Adira Abdullah)

2017-09-25 19:16:04 UTC

I think I forgot that the stronger the nuclear charge, meaning the element will have a bigger atomic radius, causes the element to become smaller requiring more ionization energy vs. a smaller element because it'll have a weaker nuclear charge that causes less ionization energy due to the now bigger atomic radius. However, I did fairly well on these too.

Multiple Choice: Allison Roland

2017-09-25 19:19:14 UTC

Which of the following elements has the highest first ionization energy?
A.) Br
B.) As
C.) Pd
D.) W

Why I got these wrong... (Landon Webb)

2017-09-25 19:19:28 UTC

Careless thinking and mistakes. I would overthink the easy ones.

Free Response: Allison Roland

2017-09-25 19:22:20 UTC

Explain why S has a higher first ionization energy than Al. S has a higher first ionization energy because it has more electrons and a greater electrostatic attraction that makes it more difficult to remove electrons.

Explanation: Allison Roland

2017-09-25 19:39:33 UTC

I have a hard time understanding the periodic trend for ionization energy. I know what the trend is I just don't understand why it's like that.

Multiple Choice (Nick Oberlin)

2017-09-25 19:40:29 UTC

Which of the following would have a greater first ionization energy than Kr?
a. P
b. Ne
c. O
d. S

Free Response (Nick Oberlin)

2017-09-25 19:41:49 UTC

Why do the noble gases have the highest ionization energies?
They have a full valence shell so it would be the hardest to remove electrons from it.

Why I missed these questions (Nick Oberlin)

2017-09-25 19:43:07 UTC

I completely forgot about the periodic trends.

Multiple Choice

2017-09-25 19:47:25 UTC

What group has the highest ionization energy?
A) Halogens
B) Alkali Metals
C) Noble Gases
D) Alkali Earth Metals

Free Response

2017-09-25 19:50:48 UTC

Which has a higher first ionization energy level and why? Ne or Kr?
Ne because it has a lesser amount of energy levels, which causes a higher electrostatic attraction and makes it much harder to remove the valence electrons.

Free Response (Maggie Schall)

2017-09-25 19:54:11 UTC

Question: Which element would have a higher first ionization energy, O or S, and why?

Answer: O would have a greater first ionization energy because it has less energy levels present in atom making the loss of an electron much harder than that of S

I missed these because...

2017-09-25 19:55:31 UTC

I forgot what a 1st Ionization energy level was.

Multiple Choice(Caden Ryan)

2017-09-25 19:57:18 UTC

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

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

Multiple Choice (Maggie Schall)

2017-09-25 19:58:08 UTC

Which element would have the lowest ionization energy?

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

Why I missed these questions (Maggie Schall)

2017-09-25 19:59:56 UTC

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

Multiple Choice Colby Dennis

2017-09-25 20:28:44 UTC

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

Free Response Colby Dennis

2017-09-25 20:30:28 UTC

Why does Fluorine have higher ionization energy over Oxygen?

Why I missed these questions Colby Dennis

2017-09-25 20:31:55 UTC

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

Multiple Choice (Victoria Contreras)

2017-09-25 20:31:59 UTC

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

Free Response (Victoria Contreras)

2017-09-25 20:33:32 UTC

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.

Multiple Choice Ell Henderson

2017-09-25 20:34:23 UTC

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

Free Response Ell Henderson

2017-09-25 20:35:54 UTC

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.

Why I missed these questions (Victoria Contreras

2017-09-25 20:36:09 UTC

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

Multiple Choice (Evan B)

2017-09-25 20:36:35 UTC

Which element below has the highest ionization energy?

a. Cl

b. Na

c. Fr

d. W

Free Response (Evan B)

2017-09-25 20:36:59 UTC

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.

Multiple Choice (Jared Henry)

2017-09-25 20:41:21 UTC

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

Free response- Carter Gamble

2017-09-25 20:47:23 UTC

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.

Multiple Choice- Jenna Trantham

2017-09-25 20:48:30 UTC

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.

Multiple Choice-Carter Gamble

2017-09-25 20:48:48 UTC

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

Why I miss them Carter Gamble

2017-09-25 20:49:50 UTC

Sometimes I mix up questions and do them backwards.

Multiple Choice - Grace Kisting

2017-09-25 20:50:01 UTC

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.

Multiple Choice Natalia Wilson

2017-09-25 20:51:52 UTC

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

Free Response Natalia Wilson

2017-09-25 20:53:16 UTC

Explain why noble gasses have the highest ionization energy

Why I missed these questions Natalia Wilson

2017-09-25 20:55:02 UTC

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

Why I miss them Ell Henderson

2017-09-25 20:58:16 UTC

I simply was rushing through the test

Free Response - Grace Kisting

2017-09-25 21:00:51 UTC

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.

Explanation - Grace Kisting

2017-09-25 21:10:05 UTC

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

Free Response- Jenna Trantham

2017-09-25 21:17:52 UTC

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.

Reasons for missing this question- Jenna Trantham

2017-09-25 21:18:14 UTC

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

Multiple Choice (Oliver Meade

2017-09-25 21:24:33 UTC

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

Free Response (Oliver Meade)

2017-09-25 21:34:22 UTC

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.

Free Response - Caitlin Mann

2017-09-25 21:45:59 UTC

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.

Multiple Choice - Garrett Balog

2017-09-25 21:51:29 UTC

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

Multiple Choice - Caitlin Mann

2017-09-25 21:52:18 UTC

Which has the lowest ionization energy?

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

Free Response - Garrett Balog

2017-09-25 21:55:21 UTC

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

Up and to the right.

Why I Miss These - Garrett Balog

2017-09-25 21:57:43 UTC

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

Free Response - Savannah Amick

2017-09-25 21:58:04 UTC

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.

Devin Cooke Multiple choice

2017-09-25 21:58:23 UTC

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

Devin Cooke Free Response

2017-09-25 22:00:45 UTC

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.

Multiple Choice - Savannah Amick

2017-09-25 22:03:49 UTC

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

Multiple Choice - Richard Whitfield

2017-09-25 22:07:50 UTC

Which of the following lists a group of elements with decreasing first ionization energy?
A. BaB. P>Mn>Cs
C. O>Ge>Ne
D. HfE. Fr>Mg>O

Why I missed these. - Savannah Amick

2017-09-25 22:10:28 UTC

I understand these however I made some careless mistakes.

Free Response - Richard Whitfield

2017-09-25 22:10:36 UTC

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.

Why I got these questions wrong - Richard Whitfield

2017-09-25 22:13:56 UTC

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.

Why I missed these questions. (Patrick Chan)

2017-09-25 22:15:57 UTC

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

Multiple Choice (Patrick Chan)

2017-09-25 22:18:34 UTC

Which element listed his the highest first ionization energy?

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

Free Response (Patrick Chan)

2017-09-25 22:20:16 UTC

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.

Why I missed these:

2017-09-25 23:47:46 UTC

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

Put these elements in order of decreasing ionization energy:

2017-09-25 23:48:12 UTC

Co, F, Rn, Sr

Multiple Choice:

2017-09-25 23:49:11 UTC

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

Multiple Choice by Vandanaa

2017-09-25 23:53:23 UTC

Which element has the highest first ionization energy?

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

Free Response by Vandanaa

2017-09-25 23:54:19 UTC

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.

Explanation of Mistakes by Vandanaa

2017-09-25 23:54:53 UTC

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.

Multiple Choice (Mackenzie Reed)

2017-09-26 00:19:31 UTC

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

Free Response (Mackenzie Reed)

2017-09-26 00:22:21 UTC

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

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

Explanation (Mackenzie Reed)

2017-09-26 00:24:09 UTC

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

Multiple Choice: Payton Tucker

2017-09-26 00:30:43 UTC

Which set of elements are in order of increasing ionization energy?
A. KB. NC. HD. H
Answer: A

Why I got these questions wrong- Ashley Armendariz

2017-09-26 00:38:45 UTC

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.

Free Response: Payton Tucker

2017-09-26 00:39:06 UTC

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.

Multiple Choice- Ashley Armendariz

2017-09-26 00:40:51 UTC

Which of the following elements has the lowest ionization energy?

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

Free Response-

2017-09-26 00:45:24 UTC

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

Sc, Ti, Cu, P, N

Multiple Choice (Jay Patel)

2017-09-26 00:50:30 UTC

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

Free Response (Jay Patel)

2017-09-26 00:52:51 UTC

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.

Why I missed these questions. (Jay Patel)

2017-09-26 00:56:55 UTC

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

Multiple Choice

2017-09-26 01:09:15 UTC

Which of the following has the greatest ionization level?

a. Cs

b. Be

c. B

d. Ba
(Hope McNish)

Multiple Choice - James Voos

2017-09-26 01:09:27 UTC

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

Free Response

2017-09-26 01:09:35 UTC

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)

Reasoning

2017-09-26 01:10:12 UTC

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

Why I missed these questions.

2017-09-26 01:14:20 UTC

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.

Which of the following has the smallest ionization energy?

2017-09-26 01:16:24 UTC

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

Written Response

2017-09-26 01:17:41 UTC

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.

Multiple Choice (Kayla Stissel)

2017-09-26 01:24:50 UTC

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

Free Response - James Voos

2017-09-26 01:25:32 UTC

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.

Multiple Choice (Shawn Brown)

2017-09-26 01:26:34 UTC

Select the element that has the highest first ionization energy.

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

Free Response (Kayla Stissel)

2017-09-26 01:28:45 UTC

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

Free Response (Shawn Brown)

2017-09-26 01:29:25 UTC

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.

Explanation (Shawn Brown)

2017-09-26 01:33:44 UTC

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

Why I missed these questions - James Voos

2017-09-26 01:38:21 UTC

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

Multiple Choice - Lizzie Maguire

2017-09-26 01:41:06 UTC

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

Explanation - Lizzie Maguire

2017-09-26 01:42:42 UTC

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.

Multiple Choice (Paityn York)

2017-09-26 02:17:47 UTC

Which of the following has the highest ionization energy?

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

Free Response (Paityn York)

2017-09-26 02:19:21 UTC

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.

Reason - Claire Sholar

2017-09-26 02:20:04 UTC

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

Why I Missed These Questions (Paityn York)

2017-09-26 02:22:39 UTC

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

FRQ - Claire Sholar

2017-09-26 02:24:54 UTC

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.

Multiple Choice - Claire Sholar

2017-09-26 02:37:20 UTC

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

Multiple Choice - Ethan Kraft

2017-09-26 02:37:32 UTC

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

Free Response - Ethan Kraft

2017-09-26 02:38:32 UTC

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.

Multiple choice-Spencer

2017-09-26 02:43:22 UTC

Which element has the least ionization?

A Rb
B As
C Mn
D F

Why I missed these questions - Ethan Kraft

2017-09-26 02:46:39 UTC

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.

FRQ-Spencer

2017-09-26 02:50:35 UTC

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

As the energy levels increase the nuclear charge decreases.

Free Response - Lizzie Maguire

2017-09-26 02:55:18 UTC

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

Meghan Greenwell

2017-09-26 02:55:45 UTC

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.

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

2017-09-26 02:56:42 UTC

Multiple Choice

2017-09-26 04:11:38 UTC

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

Free Response

2017-09-26 04:15:15 UTC

(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

Free Response (Toula Lampropoulos)

2017-09-26 04:43:48 UTC

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.

Multiple Choice (Toula Lampropoulos)

2017-09-26 04:46:13 UTC

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

Reflection (Toula Lampropoulos)

2017-09-26 04:50:23 UTC

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

Free response. (Hannah Miller)

2017-09-26 15:56:28 UTC

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.

Multiple choice(Hannah Miller)

2017-09-26 16:03:09 UTC

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

Reflection(Hannah Miller)

2017-09-26 16:05:38 UTC

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.