Matter+and+PeriodicTable


 * **//__ Matter and Periodic Table Wiki __//** ||

Editor: Andrew Whalen

In this wiki, our class will be discussing the topics matter and the periodic table. Just a reminder to everyone that this wiki is due on 11/18. I will be printing it out at 10:00 pm on 11/17. I hope everyone is working on this completes their section in the given time table. As Mr. Desjardin's says, "Don't wait until the last minute." If anyone has any questions about group assignments or anything along those lines, feel free to contact me either on Facebook, Twitter: a_whalen15 or by cell: 401-487-4812. Thanks and good luck everyone!

= **__PROPERTIES OF MATTER__** =

Co-editor: Emily Mills Team 1: Joe Geraghty Section 2.1
 * __DESCRIBING MATTER__** (Emily Mills)
 * Observing its properties
 * Properties used to describe matter can be classified as extensive or intensive.


 * 1) **Extensive Properties** - a property that depends on the amount of matter in a sample
 * Matter is anything that has mass and takes up space.
 * **Mass**of an object is a measure of the amount of matter the object contains.
 * **Volume** of an object is a measure of the space occupied by the object.


 * 1) **Intensive Properties** - a property that depends on the type of matter in a sample, not the amount of matter
 * Examples: hardness; softness; material made from


 * __IDENTIFYING SUBSTANCES__**


 * Every object has its own chemical makeup or composition.
 * **Substance**is matter that has a uniform and definite composition.
 * Examples: gold and copper
 * Every sample of a given substance has identical intensive properties because every sample has the same composition.
 * **Physical Properties** are a quality or condition of a substance that can be observed or measured without changing the substance's composition.
 * 1) Examples: hardness; color; conductivity; and malleability.
 * 2) Help chemists identify substances.

Physical Properties of Some Substances

__**Substance State Color Melting Point (°C) Boiling Point (°C)**__ Neon Gas Colorless -249 -246 Oxygen Gas Colorless -218 -183 Chlorine Gas Greenish-Yellow. -101 -34 Ethanol Liquid Colorless -117 78 Mercury Liquid Silvery-white -39 357 Bromine Liquid Reddish-brown -7 59 Water Liquid Colorless 0 100 Sulfur Solid Yellow 115 445 Sodium chloride Solid White 801 1413 Gold Solid Yellow 1064 2856 Copper Solid Yellow 1084 2562


 * __STATES OF MATTER__** ( Joe Geraghty)


 * Solids-definite shape and volume
 * Liquids-indefinite shape, flows, yet has a fixed volume
 * Gases-form of matter that takes both the shape and volume of its container
 * Vapor-the gaseous state of a substance that is generally a liquid or solid at room temperature

__**PHYSICAL CHANGE**__


 * 1) Some properties of a material change, but the composition of the material does not change
 * 2) Reversible
 * Boil, freeze, melt, and condense
 * 1) Irreversible
 * Break, split, grind, cut, and crush



Mixtures - explained by group 2 Co-editor: Matt Moschella Members: Emily Healy Section 2.2

__**Classifying mixtures**__ a mixture is a physical blend of two or more components. based on the distribution of their components, mixtures can either be classified as heterogenous mixtures or homogenous mixtures.

__**Heterogenous mixtures**__ a mixture in which the composition is NOT uniform throughout. __**Homogenous mixtures**__ a mixture in which the composition is unifrom throughout. a **solution** is another name for a homogenous mixture. a **phase** is used to describe any part of a sample with uniform composition and properties. = = __**Separating Mixtures**__ Separating mixtures can sometimes be challenging Differences in physical properties can be used to separate mixtures Examples

__Filtration__ - the process that separates a solid from the liquid in a heterogeneous mixture
 * Filtration**

Distillation __Distillation__ - the process in which liquid is boiled to produce a vapor that is then condensed into a liquid during distillation any particles that dissolved in the liquid will be left behind = = and "cold water out" sections, cold water is previously put in that section to cool down the steam.
 * dont get confused by the "cold water in"

. It is very likely to attract electrons (when it bonds with any other element, it either attracts shared electrons or forms a negative ion).

Elements and Compounds- explained by group 3 Co-Editor- Alexandra Ortiz Members: Pat Hodge and Andrew Marcotte

-an **element** is the simplest form of matter -a **compound** is a substance containing two or more elements __//Breaking Down Compounds//__ You cannot physically break down a compound like you can physically break down a mixture A **chemical change** is a change that produces matter with a different composition An example of a chemical change is a glow stick. electricity Water > Hydrogen + Oxygen __//Properties of Compunds//__ Compounds are very different from elements examples of compounds: Water and Salt
 * __Distinguishing Elements and Compounds__** Pat Hodge page 48-49

Andrew Marcotte pgs 50-51 //__**Distinguishing Substances and Mixtures**__// -using general characteristics to distinguish between substances and mixtures -This chart summarizes the characteristics of elements, substances, and mixtures



-Chemists use chemical symbols to represent elements -They also use chemical formulas to represent compounds -first letter of symbol is always capitalized -based on the Latin names of the of the elements -below are some alchemy symbols from the 15th century
 * //__Chemical Symbols__//**



__**Symbols and Formulas**__... pg 52 - The English name and Latin name of an element is similiar i.e: > = =
 * Ca- Calcium
 * N- Nitrogen
 * S- Sulfur

__**Table 2.2 Symbols and Latin Names for Some Elements**__



 * = **ENGLISH NAME** ||= **SYMBOL** ||= **LATIN NAME** ||
 * = Sodium ||= Na ||= Natrium ||
 * = Potassium ||= K ||= Kalium ||
 * = Antimony ||= Sb ||= Stibium ||
 * = Copper ||= Cu ||= Cuprum ||
 * = Gold ||= Au ||= Aurum ||
 * = Silver ||= Ag ||= Argentum ||
 * = Iron ||= Fe ||= Ferrum ||
 * = Lead ||= Pb ||= Plumbum ||
 * = Tin ||= Sn ||= Stannum ||

__**Chemical Symbols**__ = =
 * -** they provide a shorthand way to write the chemical formulas of compounds

- chemical formulas are used to indicate the relative proportions of the elements in a compound
 * __Subscripts__**

ex: The subscript 2 in H20 indicates that there are always 2 parts of hydrogen for each part of oxygen in water


 * 2.4- chemical reactions**
 * Pgs. 53-55**
 * Group 4**
 * co-editor:Drew Humphrey**

__//Recognizing chemical Changes//__ For example //__Conservation of Mass__//
 * Members: Kelsey Persechini,Drew Humphrey**
 * There are many ways to see if a chemical change occurred
 * a [|gas] is produced,(bubbles)
 * the temperature changes,
 * a substance disappears,
 * a solid is formed
 * a colour change occurs,
 * a new odour is produced.
 * But these can also be a sign of a physical change
 * the only way to know for sure it was a chemical change is to test the composition of the substance
 * Mass stays the same in both chemical Reaction and Physical Change
 * Law of conservation of mass states that mass is neither destroyed or created in a chemical or physical change
 * When a ice cube that weights 15grams melts you still have 15 grams of water
 * When wood burns the Ashes may seem lighter but really gas are leaving and making it seem like matter is destroyed


 * chemical reaction** is a process that leads to the transformation of one set of [|chemical substances] to another. [|[1]] Chemical reactions can be either [|spontaneous], requiring no input of energy, or non-spontaneous, typically following the input of some type of energy, such as heat, light or electricity.

CHEMICAL REACTION: http://www.youtube.com/watch?v=hVK9Om4wzBM&feature=related

6.1- Organizing the Elements Pgs. 155-157 Group 5 c0-editor: Freddy Dwyer Members: Kevin Petterson

__**Searching for an Or**____**ganizing Principle:**__ (Kevin Petterson) which is a set of three elements with similar properties
 * Only 13 elements had been discovered by the year 1700
 * As Chemists began to use the scientific method to search for new elements, the rate of discovery increased
 * Chemists used the properties of elements to sort them into groups
 * 1829 German chemist J.W. Dobereiner published a classification system in which elements were grouped into triads,
 * Chemists used the properties of elements to sort them into groups
 * One element in each triad tended to have properties with values that fell midway between those of the other two elements
 * __**Not**__ all known elements can be classified as triads


 * From 1829 to 1869, many different systems of the periodic table were proposed but none of them were accepted.
 * In 1869, Russian chemist Dmitri Mendeleev published his version of the periodic table
 * He developed his periodic table while working on a textbook for his students
 * He arranged the elements in his periodic table in order of increasing atomic

(Freddy Dwyer) Here is an early version of Mendeleev's periodic table. Notice the question marks between the entries for zinc (Zn) and arsenic (As). Mendeleev left these spaces in his table because he knew that bromine belonged with chlorine and iodine. He predicted what their properties would be based on their locations in the table. The elements between zinc and arsenic were gallium and germanium, which were discovered in 1875 and 1886. There was a close match between the predicted properties and the actual properties of these elements.

The atomic mass of iodine (I) is 126,90. the atomic mass of tellurium (Te) is 127.60. Based on its chemical properties, iodine belongs in a group with bromine and chlorine. So Mendeleev broke his rule and placed tellurium before iodine in his periodic table.He assumed that the atomic masses for these elements were incorrect, but they were not. Iodine has smaller atomic mass than tellurium does. A similar problem occurred with the other pairs of elements. Mendeleev developed his table before scientists knew about the structure of atoms. He was not aware of the unique number of protons atoms have. **THE NUMBER OF PROTONS IS THE ATOMIC NUMBER IN AN ELEMENT**. So in the modern periodic table, elements are arranged in order of increasing atomic mass.The periodic table has 7 periods. Period 1 has 2 elements, period 2 has 8 elements, period 4 has 18 elements, period 6 has 32 elements. Each period corresponds to a principal energy level. Elements within the same period share similar properties. **PERIODIC LAW: WHEN ELEMENTS ARE ARRANGED IN ORDER OF INCREASING ATOMIC NUMBER, THERE IS A PERIODIC REPETITION OF THEIR PHYSICAL AND CHEMICAL PROPERTIES.**
 * THE PERIODIC LAW**

6.1 Organizing the Elements Group 6 co editor: Sean Doherty Members: Matt McKeon

__**Metals, Nonmetals, and Metalloids.**__ -The periodic table consists of three main groups which are metals, nonmetals, and metalloids. -Ratio of each group: Metals:80% Nonmetals:15% Metalloids: 5%

-Clean cut of metal will usually have high luster, or sheen. -__Sheen-__ A metals ability to reflect light. -All metals are solids at room temperature.(Exception of mercury) -Must metals are ductile, or able to be formed into wires. -Most metals are malleable, or able to be formed into sheets.
 * Metals**
 * -**Good conductors of heat and electrical current.

Copper(Cu)

- Gases at room temperature. -Include the main components of air- nitrogen and oxygen. -Few nonmetals are solids, such as sulfur and phosphorus. -Also one nonmetal, bromine, is a dark red liquid. -Variation among nonmetals makes it difficult to describe one set of general properties that apply to all nonmetals. -Nonmetals are not metals, as their name implies. -They tend to have properties that are opposite of those of metals. -In general, nonmetals are poor conductors of heat and electric current. -Carbon is an exception to this rule. -Solid nonmetals tend to be brittle, meaning that they will shatter if hit with a hammer. Fluorine(F)
 * Nonmetals**

- A metalloid generally has properties that are similar to metals and nonmetals. -Under some conditions a metalloid may behave like a metal. -Under other conditions, a metalloid may behave like a nonmetal. -The behavior often can be controlled by changing the conditions. -For example, Pure Silicon is a poor conductor of electric current, like most nonmetals. But if a small amount of boron is added to the silicon, the mixture is a good conductor of electric current, like most metals. Silicon(Si) In this picture of the periodic table the nonmetals are to the right of the yellow line represtented in the green color. The metalloids are represented in the light grey color on the left and right of the yellow line.
 * Metalloids**

6.2 Classifying Elements Group 7 co editor: Chris Delude Members: Katie Manis

__ **Chapter 6.2 pages 161-167** __ The Periodic table displays the symbols and names of the elements, along with information about the structure of their atoms. Periodic Tables vary in all fonts and colors which represent numerous things. Some change color of the element name to distinguish which form of matter (solid, liquid, or gas) the element is at room temperature. Some have different background colors to distinguish groups of elements, such as alkali elements or alkaline earth metals. The Periodic Table categorizes elements by their electrons because electrons play a key role in determining an element’s properties.

Elements can be sorted into these categories based on their electron configuration: · Noble gases · Representative elements · Transition metals · Inner transition metals


 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">__Electron Configurations in Groups__: **
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">there is a connection between an element's electron configuration and its location on the periodic table.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">Elements can be sorted into noble gasses, representative elements, transition metals, or inner transition metals based on their electric configurations.

__<span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">The Noble Gasses __
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">the noble gasses are the elements in group 8A of the periodic table.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">these nonmetals are sometimes called the inert gasses because they rarely take place in a reaction.

__<span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">The Representative Elements __
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">elements that display a wide range of physical and chemical properties.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">some are metals, some are non-metals and some are metalloids.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">most of them are solids but some of them are gasses at room temperature and one of them is a liquid. (bromine)
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">in atoms of representative elements the //s// and //p// sublevels of the highest occupied energy level is not filled.

__**<span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">Transition Elements: **__
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">transition elements are elements in the B group of the periodic table which provide a connection between the two sets of representative elements.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">there are two types of transition elements. they are transition elements and inner transition metals.

__<span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">Transition metals __
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">group B elements that are usually displayed in the main body of a periodic table.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">copper, silver, gold and iron are examples.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">in atoms of a transition metal the highest occupied sublevel and nearby sublevel contain electrons.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">these elements are characterized by the presence of electrons in orbitals.

__<span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">Inner transition metals __
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">appear in the main body of the periodic table.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">in atoms of an inner transition metal, the highest occupied sublevel and nearby sublevel generally contain electrons.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">the inner transition metals are characterized by orbitals that contain electrons.

__**<span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">Blocks of Elements **__ <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">[|**Click here for an interactive periodic table experience**]
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">the periodic table is divided into sections or blocks that correspond to the highest occupied sublevels.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">Each period on the periodic table corresponds to a principal energy level.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">for transition elements electrons are added to a sublevel with a principal energy level that is one less than the period number.
 * <span style="color: #000000; font-family: Georgia,serif; vertical-align: super;">for the inner transition metals the principal energy level of the sublevel is two less than the period number.


 * Chapter 6: Lesson 3 Periodic Trends**
 * Pgs. 170 - 178**

6.3 Periodic Trends pgs. 170-172 Group 8 Co-editior: Monika Maczuga (second half of 171-172) Group Members: Michael Clarke (170- first half of 171)

__Periodic Trends in Atomic Size__ v Each element has one more proton and one more electron than the preceding element. v Across a period, the electrons are added to the same principal energy level. v The __shielding effect__ is constant for all elements in a period. v The increasing nuclear charge pulls the electrons in the highest occupied energy level closer to the nucleus and the atomic size decreases. ü Generally, atomic size **decreases** across a period from left to right.

v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">An **ion** is an atom or group of atoms that has a negative or positive charge. v __<span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Both __<span style="font-family: 'Times New Roman','serif'; font-size: 16px;"> positive and negative ions form when electrons are transferred between atoms. v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Atoms of **metallic** elements tend to form ions by __losing__ one or more electrons from their highest occupied energy levels. v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">In a sodium ion, the number of electrons (10) is no longer equal to the number of protons (11). Thus the sodium ion has a __net positive charge.__ Protons dominate! v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">A **cation** is an ion with a positive charge. v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">The charge for a cation is written as a __number__ followed by a __plus sign.__ __<span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Good to Know: __<span style="font-family: 'Times New Roman','serif'; font-size: 16px;"> If the charge is 1+, the number 1 is __usually__ omitted from the complete symbol of the ion. v **<span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Nonmetallic **<span style="font-family: 'Times New Roman','serif'; font-size: 16px;">elements tend to form ions by __gaining__ one or more electrons. v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">In a chloride ion, the number of electrons (18) is no longer equal to the number of protons (17). Thus the chloride ion has a __net negative charge.__ Electrons dominate! v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">An ion with a negative charge is called an **anion.** v <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">The charge for an anion is written as a __number__ followed by a __minus sign.__
 * Ions**
 * <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Example: Sodium **
 * <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Example: **<span style="color: black; font-family: 'Arial','sans-serif';">Na +.
 * <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Example: **<span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Chlorine
 * <span style="font-family: 'Times New Roman','serif'; font-size: 16px;">Example **<span style="font-family: 'Times New Roman','serif'; font-size: 16px;">: <span style="color: black; font-family: 'Arial','sans-serif';">Cl-

<span style="color: black; font-family: 'Arial','sans-serif';">For an interactive display of how ionic bonds form, please visit:

[]

In this game, you are challenged to create several compounds using ions:

[]

In love with ions? In this activity, you are challenged to transform elements into their appropriate ions:

[]



6.3 Periodic Trends

pgs. 173-174

Co-editior: Sejal Batra

Group Members: Abby Williams, Kendall Parsons Abby Williams: pgs. 173-174 ionization energy: energy required to remove an electron from an atom
 * Trends in Ionization Energy**
 * First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period


 * 1) atomic size increases as atomic number increases
 * 2) nuclear charge has smaller effect as size of atom increase

Group Trends in Ionization Energy:

Each green dot represents the data for one element. In general, first ionization energy decreases from top to bottom within a group. As the size of the atom increases, nuclear charge has a smaller effect on the electrons in the highest occupied energy level. So less energy is required to remove an electron from this energy level and the first ionization energy is lower.

Electronegativity explained by Group 10 Members: Lindsey Trafford (Co-editor) p177Lauren Rossi p178Nathaniel Gallishaw p177 <span style="display: block; font-family: arial,helvetica,sans-serif; text-align: center;">__**Trends in Electronegativity**__ <span style="color: #000000; font-family: Arial,Helvetica,sans-serif; vertical-align: super;">- noble gases do not form many compounds <span style="color: #000000; font-family: Arial,Helvetica,sans-serif; vertical-align: super;">- Linus Pauling was the first to define **electronegativity** <span style="color: #000000; font-family: Arial,Helvetica,sans-serif; vertical-align: super;">*he won a Noble Prize in Chemistry for his work on =<span style="font-family: Arial,Helvetica,sans-serif; font-size: 14px; font-weight: normal; line-height: 16px;">chemical bonds =
 * <span style="color: #000000; font-family: Arial,Helvetica,sans-serif; vertical-align: super;">Electronegativity - the ability of an atom to attract electrons when the atom is in a compound [[image:mrdesjardinsgg12wiki/eneg6.jpg align="right"]]
 * <span style="color: #000000; font-family: Arial,Helvetica,sans-serif; vertical-align: super;">it is a property that can be used to predict the type of bond that will form during a reaction

Generally, values for electronegativity decrease when moving from the top to the bottom of a group. In representative elements, these values increase when moving from the left to the right of a period. Therefore, metals on the left side of the periodic table have low electronegative values. Nonmetals on the right side of the periodic table (except for the noble gases) have high electronegative values. There is not a trend in values for the transition metals. Cesium's 0.7 value makes it the least electronegative element. It is least likely to attract electrons (when it reacts, it usually loses electrons and forms positive ions). Fluorine's 4.0 value means that it is the most electronegative element. It is very likely to attract electrons (when it bonds with any other element, it either attracts shared electrons or forms a negative ion).
 * Electronegativity Trends in the Periodic Table** (Nathaniel Gallishaw)


 * Electronegativity Values for Selected Elements** (Nathaniel Gallishaw)
 * H 2.1 ||  ||   ||   ||   ||   ||   ||
 * Li 1.0 || Be 1.5 || B 2.0 || C 2.5 || N 3.0 || O 3.5 || F 4.0 ||
 * Na 0.9 || Mg 1.2 || Al 1.5 || Si 1.8 || P 2.1 || S 2.5 || Cl 3.0 ||
 * K 0.8 || Ca 1.0 || Ga 1.6 || Ge 1.8 || As 2.0 || Se 2.4 || Br 2.8 ||
 * Rb 0.8 || Sr 1.0 || In 1.7 || Sn 1.8 || Sb 1.9 || Te 2.1 || I 2.5 ||
 * Cs 0.7 || Ba 0.9 || Tl 1.8 || Pb 1.9 || Bi 1.9 ||  ||   ||

**Summary of Trends**
Properties such as atomic size, ionization energy, ionic size, and electronegativity vary within groups and across periods

The trends that exist among these properties can be explained by variations in atomic structure.

Chart Found on page 178