Daily Lesson #1

Student's Name:

Williams

Student's ID:

Williams67

No Help:

First Question:

The Periodic Table is arranged in increasing atomic number, thus the number of protons in the element increases as you go right and down.Ý Since the number of protons and electrons are equal the number of electrons therefore also rises.Ý As electrons are added, they fill discrete energy levels or quanta.Ý Horizontal rows on the table are equivalent to these shells, K for n=1 in the first row to P or n=6 in row six.

Columns refer to the number of valence electrons, or electrons in the outer shell.Ý For an element to be stable, such as the inert gases, their outer shell must be filled with electrons.Ý The outer shell is the highest energy and electrons occupy the lowest energy levels possible.

Second Question:

Oxidation is the loss of electrons.Ý An oxidation state moniters the lost and gained electrons in an oxidation-reduction reaction.Ý Ions are charged particles formed when an atom (or small group of atoms) gains or loses and electron.Ý A cation is a positively charged ion, formed when a metal atom loses an electron or electrons.Ý An anion is the opposite, a negatively charged ion formed from the gain of electrons.Ý Ionization becomes harder as you proceed right due to the reluctanc of atoms to lose electrons from orbitals nearly filled.Ý Thus, the inert gases do not react with anything.Ý Their outer shells are filled.Ý The halogens have their outer shells filled with the exception of one electron, they are therefore likely to gain an electron, thus becoming a anion.Ý On the left, the outer shells easily lose the one and only electron in their outer shell, they thus become cations.

Third Question:

Comments about Assignment

I found the second question very unclear.Ý I actually think it is worded incorrectly.Ý I am a little unclear on the nature of the oxidation state.Ý It is the number of charges a bonded atom would have if electrons were held completely by the atom that attracts them strongly.Ý Thus, if Helium gave up an electron, because it was not held strongly since it was the only electron in its shell, it would have a +l charge.Ý So, the oxidation number is the cation which would be formed if the electron was lost with the charge denoted.Ý Does that sound correct?Ý

I think these internet questions and comments are great and I am so far enjoying the class.

Thanks

Emily

Student's Name:

Patel

Student's ID:

Patel5

No Help:

First Question:

Elements in the same column will gain or lose the same number of electrons to obtain stability.Ý They have the same oxidation state.Ý Elements in the same row will have the same orbital that is not filled completely. So, row 1 can fill the s orbital, row 2 has room in the p orbital, etc.

Second Question:

You want to gain or lose the least amount of electrons for stability.Ý It takes less energy, for example, to gain 1 electron than lose 7 electrons in a p orbital.Ý Therefore, the elements on the left side require more electrons to fill th orbitals, so they will lose the electrons to obtain stability, while the elements on the right side of the table will gain electrons for stability.

Third Question:

Comments about Assignment

Student's Name:

Gooden

Student's ID:

Gooden

No Help:

First Question:

Elements contained in the same row (1-7)

are all equal to the lettered shells (K-Q).Ý And going from left to right, the outer shell is filled beginning with the s orbital and ending with the p orbitals.

Elements in the same column all have the same number of electrons in their outermost shell.

Second Question:

The elements on the left, the metals, tend to donate electrons, which are negatively charged.Ý Therefore, they have a more positive oxidation state because they lose the negativly charged electron.Ý They are then called cations.

Elements on the right side of the periodic table, the nonmetals, are more likely to accept electrons.Ý They are then more negatively charged and become anions.

Third Question:

Comments about Assignment

I was a little confused with the ionization states.Ý I am sure it is very simple to figure out, it just took awhile!

Student's Name:

traub

Student's ID:

traub71

No Help:

First Question:

Second Question:

Third Question:

Comments about Assignment

Student's Name:

TRAUB

Student's ID:

Traub71

No Help:

First Question:

Within the same row, the elements are increasingly filling up electron orbitals.Ý For example silicon, with atomic number 14, has an electron configuration of 1s2 2s2 2p6 3s2 3p2, while phophorous which is next in the row has an atomic number of 15, and has an electron configuration of 1s2 2s2 2p6 3s2 3p3.Ý The characteristic common to elements in the same column is that they all have the same number of electrons in their outer shell.Ý For example, all of the noble gases (column 8) have 8 electrons in their outermost shell.Ý

Second Question:

The elements of the far left side of the periodic table are more likely to take on a posiive oxidation state because they have few electrons in their outer shells so they are more likely to give them away to create a comple valence shell, giving them a positive charge.Ý

Those elements on the right side have much fuller outer orbitals so they are more likely to accept electrons from other elements to complete their valence shells, giving them a negative charge.

Third Question:

Comments about Assignment

Student's Name:

Angstmann

Student's ID:

Angstmann09

No Help:

First Question:

Elements that are contained in the same column in the periodic tableÝ all have the same number of electrons in their valence shells(this is indicated by the roman numerals at the top of the column).Ý The atomic structure characteristic that is common to elements in the same row is that the number of electrons in the orbitals increase the further to the right one goes.

Second Question:

Elements on the far left are cations because they have few electrons in their outer shell.Ý Because of this, they tend to give away electrons in order to become more stable.Ý To the far right, are anions because they do not have enough electrons to fully complete an octet so they tend to take electrons (usually from a cation in an ionic bond) to make themselves more stable.

Third Question:

Comments about Assignment

Student's Name:

Ratliff

Student's ID:

Ratliff56

No Help:

First Question:

Elements within the same row have electrons in the same outer shell.Ý Elements within the same column are in the same group, such as the lanthanide, rare earth, halogens, etc.

Second Question:

Elements on the right side become anions because they are more electronegative, therefore they take electrons from other atoms, making them carry a negative charge.

Third Question:

Comments about Assignment

It would be helpful to get an explanation from you, in addition to the text over shells.Ý Just a quick review would suffice.Ý Thanks!!

Student's Name:

Rebekah

Student's ID:

Williams04

No Help:

First Question:

Within the same row, the atomic number and atomic mass increase from left to right.Ý Within the same column, the amount of electrons that are found in the outer shell of an atom are equal.

Second Question:

The elements on the right side of the periodic table are close to being neutral with a total of eight electrons in thier outer shell, therefore they have more of a tendency to gain electrons therefore causing positive oxidation.Ý On the other hand, the elements on the left side of the periodic table are far from being satisfied with their electrons, and therefore are more likely to give up the few electrons that they do possess in order to become neutral, which is negative oxidation.

Third Question:

Comments about Assignment

Maybe I missed these directions, but where exactly do we know where to read in our book?...I didn't see a reading assignment on the syllabus...then again maybe I missed it.

Student's Name:

peek

Student's ID:

Peek62

No Help:

First Question:

The vertical columns list atoms whose outer shells contain the number of electrons equal to the Roman numeral at the top of teh column. All elements in column 1 have only 1 electron in the s orbital, column 2 has 2, column 3 has 3 and so on. In a left-right sequence in any given row, the outer shell of an atom is progressively filled, beginning with the s orbital and end with the p orbital.

Second Question:

Those elements on the far left side of the table are all metals, and those on the right side of the table are non-metals. The metals have a tendency to give up electrons giving them a positive oxidation state. The non-metals on the right side are all capable of aquiring more electrons giving them a negative oxidation state.

Third Question:

Comments about Assignment

I feel you should spend some more time on the ionization states of elements.

Student's Name:

Harlacker

Student's ID:

Harlacker97

No Help:

First Question:

Elements within a single row (or period) gradually fill the same outer shell with electrons as you read across the period; thus the first period fills the K-shell, the second fills the L-shell, and so on. In other words, they share their highest energy level (same value for the largest principal quantum number).Ý Elements in the same column (families or groups) have the same number of valence electrons (the number of electrons in that outer shell); therefore they behave similarly in chemical reactions.

Second Question:

Both parts of this question draw on the same principle: that during ionization, atoms "want" to have a full outer electron shell.Ý Thus, elements on the far left side tend to become cations because they have few electrons in their outer shell, which they tend to lose when ionized; this results in an overall positive charge.Ý Those on the far right tend to become anions because their outer orbitals are almost complete, so it is "more efficient" for them to gain electrons (and an overall negative charge) to complete the shell.Ý (And the elements on the extreme right are the noble gases, which already possess a full outer shell and are generally not reactive.)

Third Question:

Comments about Assignment

High school chemistry is slowly coming back to me, though I have to admit, the electron configuration notation (1s1,etc.) was a rather dim memory.Ý The information I got from that chemistry links website was very helpful in that regard.

Student's Name:

johnson

Student's ID:

johnson63

No Help:

First Question:

Elemnets within the same column have a particular binding number, or have a way that are particular to have they bind with other elements.Ý Exmple:H is a #1 and O a 2-.Ý Therefore, the chemical equation of these binding energies would be H20.Ý

Second Question:

This occurs because the elements on the left hand side are searching for electorns to complete their ionic state.Ý Elements on the right sdie are looking to give away an electon to be at a natural state.Ý

Third Question:

Comments about Assignment

I do not know all of these answers considering there was not enough copies of the book ordered.Ý Hopefully, you will take this into consideration for those who do not have the text!Ý For the thrid answer I have no idea what the answer is.

Student's Name:

Barnes

Student's ID:

Barnes22

No Help:

First Question:

The roman numerals above the vertical columns correspond to the number of electrons in their outermost shell.Ý Knowing the number of electrons in the outer shell, we can also find the valence number which is essential in bonding.Ý The horizontal rows refer to the number of shells that the elements electrons occupy.Ý These rows are also numbered and,Ý each number is a new shell.

Second Question:

The right hand side of the periodic table has elements which have just begun to fill their outter most shell.Ý Thus, these elements are more likley to dominate this electron because there is not enough energy to withstand an

element from the left hand side of the periodic table whenever their outter shell is nearly full they accept the low number of electrons.Ý This is why columns 1-3 are cations and columns 5-7 are anions.Ý Column 4 can either be an anion or a cation and, column 8 is inert.

Third Question:

Comments about Assignment

Student's Name:

Cordero

Student's ID:

Cordero25

No Help:

First Question:

Columns, aka groups,correspond with the number of electrons found in the element's outermost shell. Columns are signified by Roman numerals.Ý Rows, aka periods, represent principle Quantum Number.Ý These are assigned Arabic numerals.Ý Increasing the value of PQN results in increasing the energy of the shell.

Second Question:

Those elements found on the right side of the periodic table typically become anions because there is less difficulty for an element to gain e- as the number of e- increases in the outermost shell. The purpose of this process attempts to fill or stabilize the outer shell will e-.Ý

Third Question:

Comments about Assignment

I am looking forward to using the web for assignments.Ý For this assignment I was especially happy using the chem tutorials; I think suchÝ cross-referencing is valuable.

Found this excerise difficult, nonetheless, simply b/c chemistry has never been my forte and frankly, as a general rule, I need quite a bit of time to read and digest material. Otherwise, I think this exercise was fair.Ý

Student's Name:

Cutter

Student's ID:

Cutter83

No Help:

First Question:

The periodic table is organized in a manner which conviently details the chemical and physical properties of each respective, element.Ý The elements are arranged horizontally in order of increasing atomic number(# of protons).Ý This pattern is reflective of the charge of the element and of the number of electrons.Ý The vertical grouping of the periodic table represents the number of electrons in the outermost shell of comparable elements.Ý For example, the noble gases (He,Ne,Ar,Kr,Xe and Rn) represent the most stable of elements because their outermost electron shell is filled. The electron configuration for these elements are 1S^2, 1S^2 2S^2 2P^3,etc...

Second Question:

In addition to being organized horizontally and vertically, the periodic table also diferentiates between metals and nonmetals. The metals are situated on the left hand side of the table. These elements are similiar in that they have the properties which allow them to be electon donors. On the otherhand nonmetals are labeled as electron acceptors.

Third Question:

Comments about Assignment

Student's Name:

lentz

Student's ID:

lentz32

No Help:

First Question:

The horrizontal rows are called periods. The first period consists of H and He. Each element has it's electron or electrons in the first and only energy level.Ý In the second period all of the element's electrons are located in the first and second energy levels. The third and forth period work in the same way as the third period had three energy levels and the forth four and so on. So a quick summery would be to say that the period is in correspondance with theÝ atoms number of atomic levels.

Vertical columns are called groups. There are 8 A groups and 10 B groups. Starting with the A group to the far left (IA) we know that all of the elements in that group have one electron in it's outer energy level. In group IIA all the elements in that group have two electrons in it's outer level.Ý The same pattern continues till and including VIII or also known as the nobal gasses which have the maximum number of electrons in it's outer level (8). All of the B groups are metals and have two electrons in their outer level.

Second Question:

The elements on the left side of the table tend to take on a positive charge when oxidized because they loose the electron(s) in their outer level.Ý And loosing their negitige charge makes the have a positige charge.Ý The elements to the right become positive when they oxidize because they are the elements that steal the electron from the left side elements.Ý The addition of a electron(s) to the outer level of those elements will make the anion negitive.

Third Question:

Comments about Assignment

None of the information i wrote about was found in our text book.Ý is that what the ideas is in the sence that you want us to lok in alternitive sources for information?Ý i just wanted to make sure.Ý also, sorry about all the mispellings. :)

Student's Name:

gilbert

Student's ID:

gilbert61

No Help:

First Question:

A row is called a period. They are arranged in increasing atomic number (Z). Aother way to state this is that the principal quantum number, n, determines the position of the horizontal rows.

A column can also be refered to as a group.Ý The elements in the same column have the same number of electrons in their outer shell.Ý

Second Question:

Cations (+) loss electrons, metals.

Anions (-) gain electrons, nonmetals.

Elements like to have 8 electrons in their outer shell to be stable.Ý It would be easier (require less energy) for a metal to lose 2 electrons than to gain 6 electrons.

Third Question:

Comments about Assignment

I am confused about #3.Ý The adding of an electron always confuses me.Ý I think I have the correct answer for # 3 but I compared it to the example of Si and I am confused about the configuration being +4.Ý I also have a question about when the weekly homework is due.Ý Is it due the Monday after this ( Sept. 13) or is it due this Monday (Sept. 6)?

Student's Name:

wingate

Student's ID:

wingate24

No Help:

First Question:

Elements in the same row have the same number of orbital shells. The number of electrons in the subshells are different for each element. For example, Be is in second row of the periodic table, it has a 1s and a 2s shell. Neon, which is also in the second row has a 1s, 2s, and 2p shell. An element in the third row would have a 1s2s2p configuration with all of the electron spots filled, and then the 3s shell would be added for the first element in the third row (Na). By the end of the third row the 3s,3p, and 3f subshells would be full and the first element in the fourth row would start the 4s subshell. This continues up through the end of the periodic table and 7 rows.

The characteristic common to elements in the same column is similar properties. For instance, Group 1A are known as alkali metals, they are soft metals that react easily with water (with the exception of Hydrogen).Ý

Second Question:

Elements on the left side of the periodic table give away electrons more easily than elements on the right side of the periodic table which gain an electron more readily. This is because the elements are trying to achieve a "noble gas" state where all of their electron shells are full. Elements in Group 1A have 1 electron in their first subshell (s). They have to gain a lot more electrons to achieve a noble gas configuraton for their row (i.e. 1,2,3,4,etc) it is easier for them to give away one electron and achieve the configuration of the noble gas at the end of the previous row. For example, Potassium would give away 1 electron, have a +1 charge, and have a configuration like Argon. Elements on the far right side have most of the electrons in their subshells so they will hold onto the electrons that they have and grab more from other places, this is what gives them their negative charge. For example, it is easier for Chlorine to gain 1 electron to have the noble gas configuration of Argon and a -1 charge than it would be for it to give away 7 electrons to have a configuration like neon's and a positive charge.

Third Question:

Comments about Assignment

Student's Name:

Swan

Student's ID:

Swan41

No Help:

First Question:

The characteristic common to elements within the same row is the reactivity of them.Ý The characteristic common to elements within the same column is the oxidation number or charge of those elements.

Second Question:

The elements on the left side of the periodic table have a more positive oxidation state because they all share the same, "giving," valence electron configuration.Ý This configuration is one that yeilds a trend of shedding electrons, i.e. a positive charge.Ý The right side of the table, with the exception of the noble gasses, displays the opposite valence behavior of those elements on the right.Ý They are configured to attract and add electrons making them negativly charged.

Third Question:

Comments about Assignment

Other than the fact that i need a textbook to help me do the reading, I'm very excited about this course.

Student's Name:

PORFIDIO

Student's ID:

PORFIDIO73

No Help:

First Question:

a.)Ý The row numbers 1-7 are equivalent to the shells K-Q.Ý In a given row, from left to right the shell assigned to that row is filled.Ý For example if row one elements fill the K outer shell (1s2).

b.)Ý The Roman numeral at the top of each column corresponds to the number of valence electrons each element of that column has.

Second Question:

Ý As electron orbitals are filled, atoms are more reluctant to donate electrons (become cations), since their orbitals are nearly full.Ý This would explain the trend for elements on the right-side of the periodic table to be negatively charged (anions).Ý Elements on the left-side of the periodic table tend to give up electrons more easily (become cations) because it requires less energy to remove them due to their instability.

Third Question:

Comments about Assignment

Student's Name:

kerr

Student's ID:

kerr 14

No Help:

First Question:

Elements in the same row haveÝ the same energy level and the energy levels of the seperate rows increase as the move down the periodic table. Elements in the same columns have the same number of valence electrons which means elements in the same column bond similarly.

Second Question:

Elements in the far left are likely to give up an electron to bond ionicly while those on the right are likely to acept an electron during ionic bonding.

Third Question:

Comments about Assignment

Student's Name:

Wood

Student's ID:

Wood90

No Help:

First Question:

Elements in the same column of the periodic table share the same number of electrons in their outermost shell (this corresponds to the column number).ÝÝ Elements in the same row have progressively filled electron shells (from left to right along the row, beginning with the s orbital and ending with the p).

Second Question:

The elements on the left (metals) tend to donate electrons in a chemical bond, thus aquiring a positive charge and becoming cations.Ý The opposite is true of the elements on the right (nonmetals), which tend to gain electrons and become anions.

Third Question:

Comments about Assignment

you could spend some time on ionization states, if you didn't mind.Ý i'm not quite confident with them.Ý thanks!

Student's Name:

Bolton

Student's ID:

Bolton96

No Help:

First Question:

The atomic structure in common to all elements in the same row is that they all have the same shell being filled. The characteristic in common to elements in the same column is that the outer shell has the number of electrons as the column number.

Second Question:

This is due to the number of electrons in the outer shell and the fact that the more electrons that are in this shell the more energy it takes to remove an electron. So the pattern is formed because going from left to right the number of electrons in the outer shell increases.Ý Thus the ones to the left give electorns more readily becuse they have more empty outer shells with less energy necessary to take elctrons away, and the ones to the right with more full shells take electrons because the energy necessary to take the electrons is high.

Third Question:

Comments about Assignment

Student's Name:

vanover

Student's ID:

vanover 16

No Help:

First Question:

Elements in the same columns share the same valence, either negative or positive.Ý Elements in the same row share the same n number of their highest energy level.

Second Question:

Elements on the left side are typically positive because they are likely to give up electrons during an ionic bond.Ý Elements on the right side are typically negative because they are likely to take extra electrons during an ionic bond.Ý

Third Question:

Comments about Assignment

Student's Name:

Spalt

Student's ID:

Spalt35

No Help:

First Question:

All of the elements in the same column have the same number of unpaired electrons.Ý For instance, the elements in the first column each have one unpaired electron.Ý Elements in the same row have similar numbers of protons and somewhat similar atomic weights.Ý The number of protons in an element increases by one as you move along the periodic table.ÝÝ

Second Question:

Elements on the far left side (the first two columns for example) have one or two unpaired electrons, that is they want to give one or two electrons up, so they end up with a positive charge.Ý Elements on the right (excluding the ideal gases) have high numbers of electrons and want to complete their shell.Ý In order to do so, they have to gain electrons from other elements.Ý When they gain an electron, their charge becomes more negitive because electrons have a -1 charge.

Third Question:

Comments about Assignment

I have not been able to get a book yet (I checked today), and I didn't realize until now that the assignment was due at 9 tonight.Ý I thought it was due tomorrow morning and was planning on borrowing a book from a friend.Ý So, I haven't read the assignment yet, but I do remember most of the information from Chemistry, so I went ahead and answered the questions.Ý I looked at some of my old textbooks for reference.Ý I will go back and read the chapter once I get the book.Ý Hope that is okay.Ý

Student's Name:

McCall

Student's ID:

McCall49

No Help:

First Question:

Elements in the same columns have the same number of electrons in their outer shells.Ý Elements in the same columns are also grouped according to physical characteristics: an example is column 1=alkali metals, 2=alkali earth metals, 8=nable gases, and so on.Ý Elements in the same rows, from left to right, progressively fill the outershell of the atoms with electrons in a similar fashion.Ý

Second Question:

This has to do with first ionization energy which is the amount of energy it takes to remove a valence electron.Ý In comparing metals and nonmetals, it takes less energy for the metals to give up their few electrons than the nonmetals to give up all of theirs when their orbitals are almost full.

Third Question:

Comments about Assignment

Student's Name:

renton

Student's ID:

renton48

No Help:

First Question:

Elements are grouped in increasing atomic number. Elements in the same group have similare chemical and physical properties; the same number of electrons in their outermost energy level. Elements in the same period have different chemical properties.

Second Question:

Metals are mainly on the left and it takes less energy for a metal to remove an electron to become stable than to add electrons so they lose electrons and become positively charged ions. Nonmetals are on the right and it costs less energy for them to gain electrons than lose electrons, therefore they gain electrons to become stable and become negatively charged ions.

Third Question:

Comments about Assignment

i like atomic structure, chemistry rocks! (but, of course, is nowhere near as great as geology.)

i've had this before so it all made sense.

Student's Name:

voakes

Student's ID:

voakes07

No Help:

First Question:

Elements in the same row have their outer shells filled as one moves from the left side of the table to the right.Ý Elements in the same column all have the same number of electrons in their outer shells.Ý

Second Question:

The elements on the left side of the table have low first ionization potentials, so it is easy for the to give up the negatively charged electrons.Ý Thus they become positively charged much more easily.Ý

Third Question:

Comments about Assignment

Sorry this is late, I didn't have a chance to check the web until about 9:50 tonight.Ý The page looks good, comprehensible and easy to use.Ý Concerning question #3;Element Y is Aluminum.Ý Doesn't Al usually have a +3 charge?Ý

Thanks,

Nick Voakes

Student's Name:

Caudill

Student's ID:

Caudill22

No Help:

First Question:

The common characteristic in the same column is the number of electrons in the outer shell.Ý This number of electrons is equal to the roman numeral at the top of the column.Ý In the rows the common characteristic is moving in a sequence from left to right the outer shell of an atom is filled.Ý This starts with the s orbital and moves to the p orbital.

Second Question:

The elements of the far left side then to give off electrons and those on the right tend to recieve electrons.

Third Question:

Comments about Assignment

Jim,

ÝÝÝÝ Sorry that this is late by two hours.Ý I intended on completing this assignment last night but was overtaken by the stomach flu.Ý I hope you will accept this, this will not become a habit...

Shane

ÝÝ