you are here earlier, please write your question.

Why is Mg has smaller affinity than Na?  Mg has a full s sublevel, so energy is required to add an electron to begin a new sublevel.  Sodium has room in its 1s, so energy is released when an electron is added.  When energy is required for a process, it tends not to happen.  Therefore, Mg has a smaller affinity.higher Affinity means it takes higher affinity means that a greater amount of energy is released when an electron is added.  So higher negative affinity means more energy released and higher positive affinity means more energy required, right? yes. cool. I am confused, higher affinity means it takes more energy to add an e-?  In english, affinity means "like."  When adding electrons, if energy is required to add an electron,we assign the electron affinity a positive value.  This means that the atom will not "like" or have an affinity for electrons.  ok. MR. HOWE. Why I did this wrong. The question say list this in ordor of increasing affinity, I did " Iodine, Na,Mg,I-" The answer is the opposite why????  I- is large with a full sublevel, so it will have the lowest desire to add an electron and the highest positive electron affinity.  Mg has a full s sublevel, so it also will have a positive electron affinity, and a low desire to add electrons.   sodium has an empty spot in its outer shell, so it has a small negative value and a small desire to gain an electron.  Iodine has an almost full outer shell,and high effective nuclear charge since it is at the right end of the period.  So, it will have the highest desire to gain an electron. Mr. Howe!!So when you say a great amount of affinity, you mean the easiest to add e- one? yes--and a large negative value for the energy change.ok.

is there always less affinity when begining a new sublevel?  Elements for which the addition of an electron begins a new sublevel will have a positive affinity.  This means that they do not want to gain electrons, since energy will be required.  ok

When you are balancing an equation and there are parentheses around a polyatomic ions, do you need to carry over that subscript as well as the one within?  You only carry over the subscript that is part of the polyatomic ion.  The subscript outside of the parenthesis is not carried over.

  You need a parenthesis around a polyatomic ion if there is more than one ion.  For example, in Mg3(PO4)2, there are two phosphates, so you need to use parentheses.  

What is different about transition metals?  I am not sure what you mean?   In a question on a worksheet it asked what is so unique about transition elements and their electrons? There are answers to those on the site:
http://www.chs.clayton.k12.mo.us/ACADEMIC/SCICUR/howechemsite/H%20CHEM/Periodicitylinks/Sev.QuestwAns.pdf

Cr and Cu have different electron configurations that expected, why?  Because Cr and Cu are one elctron short of having a half full (Cr) or Full (Cu) sublevel. in the case of Cr, having one electron in the 4s and one in each 3d creates a lower energy state.  In the case of Cu, having a full d with a single electron in the 4s creates a lower energy state.  Are these irregularities common because there are so many irregularities I cannot keep them straight.
abbies above question has to do with the trend that things tend to revert to a lower energy state, right?.  Yes.  Remember we said that there are many irregularities in the d sublevel, but that the only ones you would have to remember would be associated with d4 and d9.  Cr and Cu are in these positions.  

What happens when Titanium forms a +2 (when forming a +2 ion, Ti loses the 4s electrons) or +4 (When forming a +4 ion, Ti loses 4s and 3d electrons ion? I don't understand what you are entering into the question. 
  Wait I think I understand. Doesn't Titanium lose a 3d and 4s2 electrons when forming a +2 electron?
Why does Ag have one valence elctron?  irregularity at d9.  the second 4s electron was promoted to the 3d. 

How do you deal with a subscript within parentheses with a subscript when balancing equations? for example Hg2(NO3)2 + CuCl2?   -- >  Cu(NO3)2 and Hg2Cl2 Could we spend time on balancing equations tomorrow, because that doesnt make a lot of sense to me.
I agree, I couldn't do much of the lab conclusion.  Yes we will spend some time on equations. Thanks.
It has to do with the charge of the elements. I dont have my stuff out, but you pair the elements with equal values of charge(I think?) like putting a +1 with a -1? and if the element is polyatiomic, you keep all of its subscript when balancing the equation. These are good questions.  You make the pairs by changing the cations.  (the cations change partners).  They keep their charge, and you use subscripts to make the total + charge equal the total - charge

Why is As more metallic than Se?.It is larger with a lower ionization energy, so it is more likely to lose an electron.  Losing electrons is a characteristic of metals. 

Why are Halogens an exception to the ionization energy rule? I believe ionization energy increases as you go down a family, but with halogens, it decreases. Why this is?   Check your values again.  I think you will find that ionization energy (ionization potential  on your table) decreases as you go down the family.oh yea, that's what i meant. but with halogens it increases. why is that? wait nevermind, that was a stupid question.  check this link.yea its same throughout table, i don't know what i was thinking. 

http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/ionize.html

What is the critria for an element to be metallic?   for this quiz, the ability to lose electrons.so less than 4 electrons? yes

how would the electrons change in Cu(NO3)2 and Hg2Cl2?  there was not change in electrons.  The PPT was Hg2Cl2.  These ions attract each other more than they attract water.what i mean is ??

What is an exothermic process, or negative energy, during an atomic process? Give off energy to environment. Thank you! u r welcome.

This is from the last quiz: Which of the following pairs would have the greatest difference in electronegativity? The answers were b. K and Cl or  c. Ti and F...  why? now i'm done Elements that are far apart left to right have a large difference in electronegativities.  I accepted K and Cl or Ti and ... because it would have been difficult to determine the difference with out knowing the actual electronegativity values .Just remember, that the more metallic an element is, the less electronegativity it has.   yes. why? ?  More metallic elements tend to lose electrons.  If an atom tends to lose electrons, it will not tend to gain them.

So metal lose e- in order to be active, and non-metal gain  yes or is it....ok who is you?

Can you define Halogens?They are elements with 7 valence electrons. They have relatively higher electronegativities than other elements because they have 5 electrons in the p sublevel - one away from being full.   Also, there is a greater effective nuclear charge at the right end of a period since we are increasing protons without adding energy levels. THIS IS CORRECT INFO, written in my color, but not by Mr. Howe.  I would prefer that whoever is using my color, please choose another.  

aren't those the ones in the second to last family? (17) Yes.

Is the size of an element depend on how many protons it has? yes IF the elements being compared are in the same series/period.  When moving down a family the addition of energy levels is more significant than the addition of protons, so size increases.  

So let me get htis straight, when going down a family, shielding is more important when determining the size of an element, but when going across a period, atomic number is more important?
yes.alright thanks

Where do you find exception of configuration of d sublevel?  d4 and d9.  (several others too, but we will ignore these).  oops--there is also La and Ac.  they should be f1 but are d1 instead.

Sheilding effect increases when going down a family, and to the right of a series correct?
Shielding effect increases when going down a family BUT REMAINS RELATIVELY CONSTANT ACROSS A SERIES.  

why does the atomic number not have as much of an effect when going down a family as the shielding does?  because the inside electrons repel the outer shell.  Thus reducing the effective nuclear charge.

when you refer to "higher electron affinity" does that mean more negative or less negative? Higher affinity is a higher negative value.  Also--see line 7.

So, the electron affinity is the gaining of electrons, or the amount of energy it takes to gain them?  Electron affinity is the energy change when an electron is added to an atom.  If the energy change is negative (energy released) this is considered desirable and the atom will be said to have an affinity for electrons.  The more energy released, the higher the affinity.

and electronegativity is... ?  Electronegativity is a "made up" scale that illustrates an atoms attraction for a pair of electrons in a chemical bond.  It has the same trend as electron affinity except for the s2 and p6 families. why? wait, is the answer at the first question asked here (line 7) right?  I am not sure I understand the last comment.  Electronegativity is a derived value that comes from combining the concepts of ionization energy and electron affinity, and bond energy.  It creates a generally "smoother" trend than that of electon affinity.
The line 7 question was about electron affinity.

How many questions are there on the quiz? I have to replace my last two quizes scores. The same number.  21 chances for 20 points.  :  ) great.

Mr. Howe, I know energy is always required to add an electron to a noble gas, but what about removing an electron from a noble gas? Would that require energy or yes.  Energy is always required to remove an electron from all atoms.  oh, but noble gasses are different in the sense that they require energy to add on electron right? yes.  they are most stable as atoms.  you have to put energy in to either remove or add an electron for these elements.  does this apply to alkali earth metals? ok thank you!
yes

how does electronegativity differ from electron affinity in the p6 and s2 families?  The electronegativity is greater for s2 than that of s1.  While the electron affinity of s2 is less than that of s1.  This means that electron affinity goes up and down across a series, while electonegativity continues to increase within a series.

A practice ratio problem:  What element would form an ion that is isoelectonic with Ar and combine with nitrogen in a 3:2 ratio (2 nitrogens)?
Ga?  Would Ga lose two electrons and be isoelectronic with Ar?
nevermind. Ca  yes

is it general notation to put given element at the end of a ratio in one of these problems (like you did with nitrogen)
yes.  I will try to clarify too.

if the noble gases have some of the highest electron affinities (according to the trends), why is it that they require energy to add an electron? is it because they already have a full p sublevel? yes. A "high" electron affinity means a large negative value for the energy change.  Nobe gases have positive values for the energy change, so they have a very low affinity for electrons.

does an element with a full energy level (p6) have less affinity than one with a full sublevel (s2).  no.  The least electron affinity (highest positive value) is the s2 family.  This is because the s2 family has less effective nuclear charge since it is on the left side of the table.   ok, i asked that as a verification question to the question about ordering in increasing electron affinity on line 7; does this mean the reasoning/answer there is incorrect, or did I just misinterpret it?  I don't think the answers contradict.  (but I was a little distracted by John Jay's catch.  : )
so do I ask you to check again or take your word for it?  Ask me in class tomorrow before the quiz.  We can pull up the pad.

how does the inequality of protons and electrons change the affinity of an ion/atom? aka which has more affinity and why: Iodine or Iodine -   Iodine ions have a full outer shell, so they will have a positive electron affinity. (no desire to add another electron).

is there a diff between thermodynamically and just plain stable?  not in this unit.  I have been trying to use the term thermodynamically stable to remind us that we are talking about energy being stored or released.  "Stable" is also used to talk about chemical reactivity, so the word can be confusing.

the greatest increase in ionization energy for an element is between the two electrons that...? 
However many electrons that are in the outer shell come off easily.  (relatively).  After the outer shell electrons are gone, there will be a huge increase in ionization energy.  for example.....Mg has two valence electrons.  There will be a huge increase in ionization energy after these two electrons are removed.

I forget why we began the Beer's Law lab by looking at a complete spectrum. Is it because we wanted to find the maximum absorbance for the CuSO4 solution?