Welcome!!! Again--remember that this is a completely public site...........
On my screen I am purple.... Mr. Howe
THIS IS WHAT YOU NEED TO STUDY TONIGHT: These three quizez in order.~Julian
http://www.sciencegeek.net/Chemistry/taters/Unit2PeriodicTrends.htm
http://ths.sps.lane.edu/chemweb/unit8/problems/ptrend/
http://www.quia.com/quiz/1041890.html?AP_rand=1121229392
AND spend time answering the questions on quiz one and two.
If you need some help refer to the tables on the FB page, but defiantly try a couple times without. Because we need to know this stuff.
hi~ i have a question about finding similar electron configurations...if there is more than one element that fits, how do you find the right one? I think I need context for this one. There will only be one element that fits. Do you have an example? Why did you ask this question?
Okay. Here are the trends we've been going over:
Atomic Radii: Size of atom i.e the amount of electrons associated
Ionization potential: The amount of energy required to remove electrons yes. Technically this is the energy change when an electron is removed, but the values are always positive, so we are talking about energy required.
Electronegativity: attractivness of atom to electron to a shared pair of electrons in a chemical bond.
Electron affinity: energy change when an electron is added. Usually negative -- except for the noble gases and the alkaline earth metals. Negative values are desirable, because of the the universal trend toward lower energy. so....the bigger the negative value, the more the atom desires to gain electrons.
Ashley, you need to spend time on the quizzes listed on the web site. There are two that include answers with explanations. ok how do i get to those??
howechem.net, advanced chemistry, periodicity, practice quizzes. LISTED UNDER HW FOR 10/18......I DON'T SEE PERIODICITY ETC...<Its under Periodic Properties Thank you!
look on the same page where you found the link to this page. The quizzes are at the bottom.
(I posted the lnk to the FB page...) But its called periodic propeties on the website
Did u get my email? no. I haven't checked since 5:00 or so though.ok
I'm gonna fail :(
There is also some interesting stuff on the FB page. because I posted some stuff on the trend. Pretty fun. Lol sounds fun. Thanks!
Tis fun. Tis fun.
Okay, Mr Howe, What are the big overall concepts that we should be going back over for this test? As a freference for new commers so we don't repeat
The quiz will be most like the homework assignment that I collected in class yesterday, and like quiz one and two on the web site
Okay. Awesome.
Big question. Oxidation. It really confuzed me on the assginment. COuld you explain exactly how that worked?
V What I needed I think...Okay. cool
Oxidation is defined as the loss of electrons. Oxidation numbers are the potential charges that result from the loss or gain of electrons. so, an atom that loses two electrons would have an oxidation number of + 2. an atom that gains electrons would have a negative oxidation number.Okay.
What is the difference between like bromine and Bromine ion?
Bromine is an atom that has not lost or gained an electron. A bromine ion is an atom of bromine that has gained one electron and thus has a negative one charge. Bromine gains one electron since it has 7 in its outer shell and it will tend to get to 8.
this stumped me on the most recent quiz we took in class. the relationship of ionization energy and shielding effect going down and going left to right on the periodic table. i know that more ionization energy means less shielding effect.... ionization energy is less for bigger atoms. more energy levels make bigger atoms, so it is easier to remove electrons. k right? so, going down the periodic table the ionization energy would decrease and the shielding effect would increase.
but going left to right the ionization energy increases and the shielding effect, should, decrease. but NO. it stays the SAME. WHy? yeah. ohhhh.
Shielding effect is caused by the addition of more layers of electrons, (more energy levels).
As you move across a period, you are not adding energy levels, just adding protons, while the outermost energy level stays the same. Consequently, shielding effect is relatively constant across a period. ok, that makes a whole heck of a lot more sense now : ) see above
OK.... so :) thank you
Hey so we talked ealier and I was confuzed about cations and how they work?
Cations are formed by the loss of electrons. The general rule is that if an atom has 4 or less VALENCE electrons the atom will tend to lose them in a chemical reaction. If there are five or more valence electrons, the atom will tend to gain electrons from another atom in order to get to 8 valence electrons. Losing electrons causes a positively charged ion that we call a cation. Gaining electrons creates a negatively charged ion that we call an anion.
Are you guys still there?.......yeah sorry thank you for clearing that up, I'm making some flashcards.
So when your asking about inner transition elements and their energy levels.... well can you just explain that for me real quick?
the inner transition metals are the f block. the filling order goes from 6s to 4f, so the inner transition metals are filling a sublevel two energy levels below the outer shell of the atom. The next series goes from 7s to 5f. alright cool
Yep. any more questions??
Are we allowed to come in early to talk to you in person? Sure
I am going to take a break. I will check back in 20 minutes or so. (9 ish). List any other questions that come up below this point, and I will answer when I get back.
ok
are you collecting lab books tomorrow? yes--- the halogen lab only. You only have to answer the questions and get the info. in your book. hand written is OK. We did most of the questions in class.
I am back. Are there any more questions?
kind of, it has to do with one of the questions for the halogen lab. #6
should i type the Q? i just need to know if
Is it the one about why Br is more active than Iodine? yep
i got "bromine is more chemically active then iodine b/c it has a higher capability to loose e- than iodine...." that's what i wrote in my lab book. bromine.yay. Which is the larger atom? Br or I? Wait......Br is not as big as I. I is lower on the chart. Do you understand? no What happens to atomic size as you move down a family?
it gets larger. oh! because of shielding effect you add energy levels and the valence electrons are pushed outward to i :> yes! So.....do nonmetals react by losing electrons or by gaining electrons?...losing?
The general rule is that if there are 4 or less electrons in the valence shell, the atom will lose electrons. 5 or more menas the atom will tend to gain electrons.......
Br has 5 7 7 valence e- so.... they gain yes. So would big atoms or small atoms gain electrons easier? bigger atoms bigger atoms have more shielding,(inside layers of electrons) so they will lose electrons easier. However, they will have a harder time gaining electrons. So---which gains electrons easier----Br or I? Br because it's smaller. yES..... so that means that Bromine will be more active than iodine, since it is able to more easily gain electrons.
k. i'm going to go write this down in my notes, thank you
The most active metal is Fr, because it is the biggest. The most active nonmetal is F, because it is the smallest (that has openings in the outer shell--He is smaller, but full)
Due to lack of intense questioning I am going to take another break.... I will check back at appx. 9:40 for the last time tonight...
I'm Back....
Last call for questions.........
Good night everyone.
Are people still here?