chapter5_ardw

=The Periodic Table: an arrangement of elements in order of their atomic numbers so that elements with similar properties fall in the same column or group. =  || = Chapter 5 //The Periodic Table // =

**By: Alec Root & Dennis Wagner **
====**//Edited by: Grace Pratt, Mana Aliabadi, and Megan Matthews //** ====

History of the Periodic Table
//Important People//
 * **Dalton **- proposed an atomic theory that said all atoms of the same element are the same and described the atom as a simple sphere.
 * was later proved wrong on both accounts
 * **Dobereiner **- discovered triads (groups of three elements that have similar behaviors)
 * Triads work because each element has the same number of valence electrons
 * **Newlands **<span style="font-family: 'Comic Sans MS', cursive;">- arranged elements by increasing atomic mass, saw that properties reoccurred every eight elements
 * <span style="font-family: 'Comic Sans MS', cursive;">Named the reoccurrence of properties every eight elements "Law of Octaves" ←
 * <span style="font-family: 'Comic Sans MS', cursive;">Came up with octet rule (an element will be stable with eight valence electrons)
 * **<span style="font-family: 'Comic Sans MS', cursive;">Mendeleev **<span style="font-family: 'Comic Sans MS', cursive;">- "Father of the Periodic Table"- created the first version of the periodic table, organized it by increasing atomic mass
 * <span style="font-family: 'Comic Sans MS', cursive;">Left spaces for elements that had yet to be discovered
 * **<span style="font-family: 'Comic Sans MS', cursive;">Mosley **<span style="font-family: 'Comic Sans MS', cursive;">- created modern periodic table, organized it by increasing atomic number
 * <span style="font-family: 'Comic Sans MS', cursive;">Wrote Periodic Law "physical and chemical properties of the elements are periodic functions of their atomic numbers"
 * **<span style="font-family: 'Comic Sans MS', cursive;">Canizzaro **<span style="font-family: 'Comic Sans MS', cursive;">- developed method for accurately measuring the realative masses of atoms
 * <span style="font-family: 'Comic Sans MS', cursive;">Allowed chemists to agree on standard values for atomic mass, initiated a search for relationships between an element's properties & atomic mass

==<span style="display: block; color: #077fa6; font-family: 'Comic Sans MS', cursive; background-color: #c0c0c0; text-align: center;">The Periodic Table <span style="display: block; color: #000000; font-family: 'Comic Sans MS', cursive; background-color: #c0c0c0; text-align: center;"> //{// <span style="font-weight: normal; font-size: 17px; line-height: normal; webkit-border-horizontal-spacing: 3px; webkit-border-vertical-spacing: 3px;">//an organized chart of the elements in order of increasing number of protons, aligned so each column contains elements w/ similar properties}// ==

<span style="display: block; font-family: 'Comic Sans MS', cursive; text-align: center;"> ==<span style="display: block; font-family: 'Comic Sans MS', cursive; background-color: rgb(255,255,255); text-align: center;"> <span style="display: block; font-weight: normal; font-size: 17px; line-height: 25px; font-family: 'Comic Sans MS', cursive; background-color: rgb(192,192,192); text-align: center; webkit-border-horizontal-spacing: 0px; webkit-border-vertical-spacing: 0px;"> ==
 * **<span style="font-family: 'Comic Sans MS', cursive;">The Noble Gases **
 * <span style="font-family: 'Comic Sans MS', cursive;">The noble gases are the las column in the periodic table (Group 18)
 * <span style="font-family: 'Comic Sans MS', cursive;">They consisit of Helium, Neon, Argon, Krypton, Xenon, and Radon
 * <span style="font-family: 'Comic Sans MS', cursive;">Only elements that are completely stable, (they do not need to lose/gain any electrons to become stable
 * <span style="font-family: 'Comic Sans MS', cursive;">Sometimes regarded as the most significant addition to the periodic table
 * **<span style="font-family: 'Comic Sans MS', cursive;">The Lanthanides **
 * <span style="font-family: 'Comic Sans MS', cursive;">They are the 14 elements with atomic numbers from 58 (Ce-Cerium) to 71 (Lu- Lutetium)
 * <span style="font-family: 'Comic Sans MS', cursive;">Are located in period 6 between groups 3 and 4
 * <span style="font-family: 'Comic Sans MS', cursive;">Their chemical and physical properties are so similar that separating them was a very tedious task requiring many chemists
 * **<span style="font-family: 'Comic Sans MS', cursive;">The Actinides **
 * <span style="font-family: 'Comic Sans MS', cursive;">The actinides are the 14 elements with atomic numbers from 90 (Th- Thorium) to 103 (Lr- Lawrencium)
 * <span style="font-family: 'Comic Sans MS', cursive;">Are located in period 7 between groups 3 and 4
 * <span style="font-family: 'Comic Sans MS', cursive;">Usually set off below the main portion of the periodic table to save space
 * <span style="font-family: 'Comic Sans MS', cursive;">Radioactive
 * **<span style="font-family: 'Comic Sans MS', cursive;">Metals **[[image:http://media-2.web.britannica.com/eb-media/39/7339-004-23335A52.gif align="right"]]
 * <span style="font-family: 'Comic Sans MS', cursive;">Ductile- can be drawn into wires
 * <span style="font-family: 'Comic Sans MS', cursive;">Malleable- can be hammared into sheets
 * <span style="font-family: 'Comic Sans MS', cursive;">Conductors- transfer heat and electricity
 * <span style="font-family: 'Comic Sans MS', cursive;">Generally reflect light and have luster
 * <span style="font-family: 'Comic Sans MS', cursive;">Solids at room temperature with the exception of Hg
 * **<span style="font-family: 'Comic Sans MS', cursive;">Non-Metals **
 * <span style="font-family: 'Comic Sans MS', cursive;">Insulaters- do not transfer heat or electricity
 * <span style="font-family: 'Comic Sans MS', cursive;">Brittle and are not easily shaped or formed, break when hammered
 * **<span style="font-family: 'Comic Sans MS', cursive;">Semi-Metals/ Metalloids **
 * <span style="font-family: 'Comic Sans MS', cursive;">Elements along the division line between metals and non-metals
 * <span style="font-family: 'Comic Sans MS', cursive;">show properties of both metals and non-metals
 * **<span style="font-family: 'Comic Sans MS', cursive;">Periodicity **
 * <span style="font-family: 'Comic Sans MS', cursive;">The tendency of recurring patterns with respect to atomic numbers on the periodic table
 * <span style="font-family: 'Comic Sans MS', cursive;">The cause of periodicity is the arrangement of the electrons around the nucleus
 * <span style="font-family: 'Comic Sans MS', cursive;">Ex: the differances of the atomic numbers for noble gases is: 8, 8, 18, 18, 32.

<span style="font-size: 130%; color: #6203a5; font-family: 'Comic Sans MS', cursive;">Energy Sub Levels:
<span style="color: rgb(64,64,64); font-family: 'Comic Sans MS';"> <span style="color: rgb(64,64,64); font-family: 'Comic Sans MS';"> <span style="color: rgb(98,3,165); font-family: 'Comic Sans MS';"> <span style="display: block; color: rgb(64,64,64); font-family: 'Comic Sans MS', cursive; text-align: center;">
 * 1) <span style="color: rgb(64,64,64); font-family: 'Comic Sans MS', cursive;">**ENERGY LEVELS --** n=1, n=2, n=3....
 * 2) <span style="color: rgb(64,64,64); font-family: 'Comic Sans MS';">**ENERGY SUB-LEVELS[[image:orbitals.png width="280" height="164" align="right"]]**
 * <span style="color: rgb(128,0,128);">**n=1 : 1 sub-level : spherical "S"**
 * <span style="color: rgb(128,0,128);">**n=2 : 2 sub-levels : parabolic "S,P"**
 * <span style="color: rgb(128,0,128);">**n=3 : 3 sub-levels : diffuse : "S,P,D"**
 * <span style="color: rgb(128,0,128);">**n=4 : 4 sub-levels : fundamental : "S,P,D,F"**
 * <span style="color: rgb(128,0,128);">**n=5 : 5 sub-levels : "S,P,D,F,G"**
 * <span style="color: rgb(64,64,64); font-family: 'Comic Sans MS';">**Each sub-level has several variations or "Orbitals"**
 * <span style="color: rgb(64,64,64); font-family: 'Comic Sans MS';">**Each orbital can hold a maximum of 2 electrons** <span style="color: rgb(98,3,165); font-family: 'Comic Sans MS', cursive;"> **(s=1 orbital; p=3 orbitals; d=5 orbitals; f=7 orbitals)**

<span style="font-size: 130%; color: #404040; font-family: 'Comic Sans MS', cursive;">ORBITAL DIAGRAMS: [[image:Image32.gif width="280" height="194" align="left"]]
<span style="display: block; color: rgb(0,0,128); font-family: 'Comic Sans MS', cursive; text-align: center;"> 1. Find which orbitals are filled 2. Construct Diagram 3. Add Electrons from bottom up<span style="display: block; color: rgb(64,64,64); font-family: 'Comic Sans MS', cursive; text-align: center;">
 * Every orbital is represented by a dot*Electrons are represented by arrows.*Orbital D is always offset by 1.*Orbital F is always offset by 2.

<span style="font-size: 130%; color: #404040; font-family: 'Comic Sans MS', cursive;">

//Noble Gas Configurations://

> > > > > > > > **Elements on the periodic are arranged so that they are with elements that share similar chemical properties. > Therefore they are organized vertically in groups, and horizontally in rows or periods.** <span style="color: rgb(128,128,128); font-family: 'Comic Sans MS', cursive;">
 * 1) <span style="display: block; color: rgb(0,128,0); font-style: normal; font-family: 'Comic Sans MS', cursive; text-align: left;">Starting @ the element, move BACKWARDS to the nearest noble gas (column 18)[[image:cabr_planet.gif width="215" height="158" align="right"]]
 * 2) <span style="display: block; color: rgb(0,128,0); font-style: normal; font-family: 'Comic Sans MS', cursive;">Write that gas in brackets { }
 * 3) <span style="display: block; color: rgb(0,128,0); font-style: normal; font-family: 'Comic Sans MS', cursive;">Write the rest of configuration normally.
 * The length of a row or period is determined by the number of electrons that occupy the sublevels being filled in the period.
 * The first period consists of the 1s sublevel being filled which can hold a total of two electrons. This means that only the elements Hydrogen and Helium are in the 1s sublevel.
 * In the second period, the 2s and 2p sublevels are being filled. The 1s sublevel can hold 2 electrons, and the 2p sublevel can hold 6 electrons, thus satisfying an octet.
 * Both the second and third period hold eight elements because they cover the 2s 2p and the 3s 3p sublevels.
 * The fourth and fifth periods hold 18 elements because they cover the 4s, 3d, 4p, and the 5s, 4d, 5p sublevels.
 * The seventh period has the same configuration as the sixth period, but only holds 29 elements because three of the elements have not yet been discovered.
 * When calculating what period an elements lands on, all you must do is see what the highest energy level is that the element occupies.



<span style="color: rgb(0,128,128); font-family: 'Comic Sans MS';"> ** THE S-BLOCK ELEMENTS ** <span style="display: block; color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive; text-align: center;"> <span style="font-weight: normal; color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive;">//Group 1: "Alkali Metals"// <span style="color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive;"> <span style="color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive;">Highly Reactive
 * <span style="color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive;">Found freely in nature

//Group 2: "Alkaline-earth metals"//
 * <span style="color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive;">Group two metals are found to be harder, denser, and stronger than the alkali metals in Group 1.
 * <span style="color: rgb(0,128,128); font-family: 'Comic Sans MS', cursive;">Too reactive to be found freely in nature.

<span style="color: #ad6feb; font-family: 'Comic Sans MS', cursive;"> <span style="color: rgb(248,236,185); font-family: 'Comic Sans MS', cursive;">
 * <span style="color: #ad6feb; font-family: 'Comic Sans MS', cursive;">Hydrogen and Helium **
 * <span style="color: #ad6feb; font-family: 'Comic Sans MS', cursive;">Hydrogen and Helium are two rare cases on the periodic table where their properties do not match their position on the table.
 * <span style="color: #ad6feb; font-family: 'Comic Sans MS', cursive;">Even though Hydrogen has an electron configuration of 1s­­­1 in the first energy level of the first group, it does not share the same properties of the other elements in the first group. In fact, Hydrogen’s properties do not resemble those any group on the periodic table.
 * <span style="color: #ad6feb; font-family: 'Comic Sans MS', cursive;">Helium has a group configuration of ns2. The odd thing is, it is located in Group 18.
 * <span style="color: #ad6feb; font-family: 'Comic Sans MS', cursive;">This is because its highest occupied energy level is filled by two electrons, meaning Helium experiences special chemical stability. Thus it is paired with the other unreactive elements of Group 18.

<span style="font-size: 110%; color: #ff8780; font-family: 'Comic Sans MS', cursive;">
 * <span style="font-size: 110%; color: #ff8780; font-family: 'Comic Sans MS', cursive;">The d-Block Elements: Groups 3-12 **

<span style="color: rgb(170,170,170);">
 * <span style="color: rgb(255,135,128); font-family: 'Comic Sans MS', cursive;">The d-Block is capable of making 5 different orbitals. If two electrons are capable of fitting in each orbital, the d-block can hold 10 electrons.
 * <span style="color: rgb(255,135,128); font-family: 'Comic Sans MS', cursive;">The d-Block is odd because unlike the s, and p blocks, 1 energy level must be subtracted because it has a higher energy that the 4s sublevel. This means that the first level of the d-Block is 3d even though the d-Block begins in the fourth row.
 * <span style="color: rgb(255,135,128); font-family: 'Comic Sans MS', cursive;">The properties of d-Block metals are that they are metals with typical metallic properties and are often referred to as **//<span style="color: rgb(255,135,128); font-family: 'Comic Sans MS', cursive;">transition [[image:Untitled5.png align="right"]]<span style="color: rgb(255,135,128); font-family: 'Comic Sans MS', cursive;">metals. //**
 * <span style="color: rgb(255,135,128); font-family: 'Comic Sans MS', cursive;">Some are not even capable of forming compounds freely in nature because they are so unreactive.

<span style="display: block; color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive; text-align: center;"> The p-Block Elements: Groups 13-18 <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">

<span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">The p-block elements are also called the **//<span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">main-group elements. //**
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">To find the number of total electrons in the highest occupied energy level for the p-block elements, you must take the group number minus 10.
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">At the far right end, it contains //<span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">nometals //<span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;"> with the exception of Helium and Hydrogen.
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">HALOGENS (Group 17)
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">They are the most reactive of the non-metals.
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">The high reactivity is caused by being one valence electron short of becoming stable.
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">They are sufficiently reactive in nature, but only in compound form.
 * <span style="color: rgb(119,196,90); font-family: 'Comic Sans MS', cursive;">However, as free metals they are stable in the presence of air.

<span style="display: block; font-family: 'Comic Sans MS', cursive; text-align: right;"> Lanthanides Actinides
 * <span style="font-size: 110%; color: #ff00a7; font-family: 'Comic Sans MS', cursive;">The f-Block Elements: Lanthanides and Actinides **<span style="color: rgb(255,0,167); font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(255,0,167); font-family: 'Comic Sans MS', cursive;">They are position in such a way because they must fill the 4f sublevel.
 * <span style="color: rgb(255,0,167); font-family: 'Comic Sans MS', cursive;">The Lanthanides are shiny metals with similar reactivity to the alkaline earth metals. They are the 14 elements from Lanthanum, La, to Hafnium, Hf in the sixth energy level.
 * <span style="color: rgb(255,0,167); font-family: 'Comic Sans MS', cursive;">Actinides are all radioactive.

//**<span style="display: block; font-family: 'Comic Sans MS', cursive; background-color: rgb(192,192,192);">Electron Configuration & Periodic Properties **//
<span style="display: block; font-family: 'Comic Sans MS', cursive; background-color: rgb(192,192,192); text-align: center;">

<span style="font-size: 110%; color: #38045d; font-family: 'Comic Sans MS', cursive;">**<span style="color: rgb(170,170,170); font-family: 'Comic Sans MS', cursive;">Atomic Radii **<span style="color: rgb(170,170,170); font-family: 'Comic Sans MS', cursive;">

<span style="font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(170,170,170); font-family: 'Comic Sans MS', cursive;">An **//<span style="color: rgb(170,170,170); font-family: 'Comic Sans MS', cursive;">atomic radius //**<span style="color: rgb(170,170,170); font-family: 'Comic Sans MS', cursive;"> is defined as one-half the distance between the nuclei of identical atoms that are bonded together. [[image:http://www.grandinetti.org/Teaching/Chem121/Lectures/AtomicRadii/assets/radiitable.gif width="515" height="263" align="right"]]
 * **<span style="color: rgb(170,170,170); font-family: 'Comic Sans MS', cursive;">Period Trends **
 * As you move down the periodic table, more energy levels are added and thus the atomic radii increases
 * <span style="color: #810a9e; font-family: 'Comic Sans MS', cursive;"> As you move across the periodic table, there are more protons in the nucleus that attract the electrons, making the atom smaller
 * <span style="color: rgb(170,170,170); font-family: 'Comic Sans MS', cursive;"> <span style="color: #810a9e; font-family: 'Comic Sans MS', cursive;">Group Trends
 * <span style="color: #810a9e; font-family: 'Comic Sans MS', cursive;">In general, the atomic radii of the main-group elements increase down a group.

<span style="font-family: 'Comic Sans MS', cursive;"> **<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">Ionization Energy **<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">

<span style="font-family: 'Comic Sans MS', cursive;"> <span style="color: rgb(170,170,170);">
 * <span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">With enough energy, an electron can be removed from an atom.
 * <span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">An **//<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">ion //**<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;"> is an atom or group of bonded atoms that has a positive or negative charge. [[image:Picture_2.png width="506" height="257" align="right"]]
 * **//<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">Ionization //**<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;"> is any process that results in the formation of an ion.
 * **//<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">Ionization Energy //**<span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;"> is defined as the energy required to remove one electron from a neutral atom of an element.
 * <span style="color: rgb(15,64,149); font-family: 'Comic Sans MS', cursive;">As an element gets closer to becoming isoelectric with a noble gas, the harder it becomes to lose an electron.

<span style="color: #d11a1a; font-family: 'Comic Sans MS', cursive;">Removing Electrons from Positive Ions<span style="font-family: 'Comic Sans MS', cursive;"> <span style="font-family: 'Comic Sans MS', cursive;">
 * <span style="color: #d11a1a; font-family: 'Comic Sans MS', cursive;">The energies for removal of additional electrons from an atom are referred to as the second ionization energy (IE2), third ionization energy (IE3), and so on.
 * <span style="color: #d11a1a; font-family: 'Comic Sans MS', cursive;">Each successive electron removed from an ion feels an increasingly stronger effective nuclear charge because fewer electrons remain within the atom to shield the attractive force of the nucleus.

<span style="font-family: 'Comic Sans MS', cursive;"> <span style="color: rgb(128,128,128); font-family: 'Comic Sans MS';"> <span style="color: rgb(128,128,128); font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(128,128,128); font-family: 'Comic Sans MS', cursive;">Electron Affinity **<span style="color: rgb(128,128,128); font-family: 'Comic Sans MS', cursive;"><span style="font-family: 'Comic Sans MS', cursive;"> [[image:Electron-affinity-1-Cl-3D-ionic.png width="219" height="75" align="left"]]
 * **//<span style="color: rgb(128,128,128); font-family: 'Comic Sans MS', cursive;">Electron affinity //**<span style="color: rgb(128,128,128); font-family: 'Comic Sans MS', cursive;"> is the energy released when an atom gains an electron.

<span style="font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(128,0,0); font-family: 'Comic Sans MS', cursive;">Period Trends **<span style="color: rgb(128,0,0); font-family: 'Comic Sans MS', cursive;">

<span style="color: rgb(128,0,0); font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(128,0,0); font-family: 'Comic Sans MS', cursive;">Halogens are the group that most readily accepts electrons.
 * <span style="color: rgb(128,0,0); font-family: 'Comic Sans MS', cursive;">This is why they are referred to as Love Electrons, because they want to become isoelectric with the nearest noble gas.

<span style="font-family: 'Comic Sans MS', cursive;">

<span style="font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(0,128,0); font-family: 'Comic Sans MS', cursive;">

Ionic Radii **<span style="color: rgb(0,128,0); font-family: 'Comic Sans MS', cursive;">

<span style="font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(0,128,0); font-family: 'Comic Sans MS', cursive;">A positive ion is known as a cation **<span style="color: rgb(0,128,0); font-family: 'Comic Sans MS', cursive;">. ** (remember the drawing of the cat streched out in a "+")
 * <span style="color: rgb(0,128,0); font-family: 'Comic Sans MS', cursive;">A negative ion is known as an anion. (remeber the drawing of an ant shaped like "---")
 * <span style="color: rgb(0,128,0); font-family: 'Comic Sans MS', cursive;">As there is a gradual increase of atomic radii down a group, there is also a gradual increase of ionic radii.

<span style="font-family: 'Comic Sans MS', cursive;"> **<span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;">Valence Electrons **<span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;">

<span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;">
 * **//<span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;">Valence electrons //**<span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;"> are the electrons available to be lost, gained, or shared in the formation of chemical compounds.
 * <span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;">They are often located in incompletely filled main-energy levels.
 * <span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;">The easiest way to determine how many valence electrons an atom has is to see what group it is in. Group 1 has 1 valence electron, group 2 has 2, Group 3 has 3, and so on excluding the d-block.

<span style="color: rgb(235,212,111); font-family: 'Comic Sans MS', cursive;"> <span style="color: rgb(85,145,165); font-family: 'Comic Sans MS', cursive;">
 * <span style="color: rgb(85,145,165); font-family: 'Comic Sans MS', cursive;">Electronegativity **<span style="color: rgb(85,145,165); font-family: 'Comic Sans MS', cursive;"> [[image:http://www.chem.ubc.ca/courseware/121/tutorials/exp7A/images/fig4.jpg width="378" height="236" align="right"]]
 * **//<span style="color: rgb(85,145,165); font-family: 'Comic Sans MS', cursive;">Electronegativity //**<span style="color: rgb(85,145,165); font-family: 'Comic Sans MS', cursive;"> is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.
 * <span style="color: rgb(85,145,165); font-family: 'Comic Sans MS', cursive;">Electronegativity follows the same trend as Electron Affinity. It tends to (with some exceptions) increases going up and to the right of the periodic table.
 * <span style="color: rgb(85,145,165); font-family: 'Comic Sans MS', cursive;">Noble gases do not form compounds, and thus they do not have electronegativities.



Sources


 * Davis, Raymond E., et al. Modern Chemistry. Austin: Holt, Rinehart and Winston, 2006.


 * Steele, Bill. “Art of communicating science is displayed in an exhibition of larger-than-life charts.” Chronicle Online. 7 January 2008 []