Matter and Periodic Table

EDITOR: BRANDON BOISCLAIR

Group 1

 Co-Editor: Becky Hyatt
Mitchell Martin
Christian Cooke
Evan Sommerich
Alex Nunan
Shannon Lamy

Classifying Mixtures

By: Mitchell Martin

Mixture- a physical blend of two or more components







Mixtures can be classified as heterogeneous and homogeneous.

heterogeneous mixture: a mixture in which the composition is not uniform throughout.

homogeneous mixture: a mixture in which the composition is uniform throughout. this is also called a solution. An example of a solution is air. a liquid solution can be oil & vinegar.

EXTENSIVE PROPERTIES vs. INTENSIVE PROPERTIES
By: Christian Cooke
matter- has mass and takes up space
mass- amount of matter
volume-space occupied by and object
EXTENSIVE PROP depends on the amount of matter in a sample
INTENSIVE PROP depends on the type of matter in a sample, not the amount e.g. hardness/density
Identifying Substances
physical property- a quality or condition of a substance that can be observed/measured without changing the composition
- used to help identify substances
- some exapmples of physical properties include hardness, color, conductivity, and malleability.

States of Matter- Page 41

Physical Change- Page 42

By: Evan Sommerich

Three states of matter are solid, liquid, and gas. There are also two other forms that are not certain or used in the periodic table; these are boseinstien and plasma.
Solids are forms of matter that has a definite shape and volume.


Liquids are forms of matter that has a indefinite shape, flows and has a fixed volume.


Gases are forms of matter that takes up both shape and volume of its container its in.

Vapors describe the gaseous state of a substance that is generally a liquid or solid at room temperature, as in water vapor.


Physical Change
Physical Change- properties of material change, but the composition of the material does not change.
Words such as “freeze, melt, and boil,” all words to describe physical changes.
Physical changes can be classified as reversible or irreversible.

Symbols and Formulas- pg.51

Chemical Changes- pg.53

By: Alex Nunan

Symbols and Formulas

chemical symbol- a one or two letter representation of an element:

Chemical symbols- represent elements
Chemical formulas- represent compounds

• using symbols is not a new idea
  • system used today based on system created by Jons Jacob Berzelius' (1779-1848)
  • symbols based on Latin names of elements
  • first letter = capital, second letter = lowercase
• symbols make it easier to writeout formulas
• chemical formula for water is H2O
  • subscript- used to indicate the relative proportions of the elements in the compounds
  • the subscript 2 says that there are always two parts of hydrogen for each part of oxygen in water
    • compounds are fixed compositions- formulas for compounds always the same

all of the elements have symbols

Chemical Changes

chemical change- a change that produces matter with a different composition than the original matter:
chemical property- the ability of a substance to undergo a specific chemical change:

• examples: burn, rust, rot, decompose, ferment, explode, corrode
• can be used to identify substance
• only observed when substance undergoes chemical change
• 
  

composition of matter always changes in a chemical reaction
chemical change is also called a chemical reaction:
chemical reaction- a change in which one or more reactants change into one or more products, characterized by the breaking
of bonds in reactants and the formation of bonds in products:

• reactant- a substance present at the start of a reaction:
• product- a substance produced in a chemical reaction:

rust is a chemical change

burning is a chemical change

STATES OF MATTER (2.1 p.41)

By: Shannon Lamy

Three states of matter are...
1. Solid
2. Liquid
3. Gas

SOLIDS- form of matter that has a definite shape and volume.

• Doesn't form to shape of container
• Particles are tightly packed together (orderly)
• Difficult to squeeze into a smaller volume
• only expand slightly under heat

Particles of a solid are tightly packed together.

LIQUIDS- form of matter that has an indefinite shape, flows, yet has a fixed volume.

• Particles are in close contact with one another, but not orderly
• Particles free to flow
• Takes shape of container
• fixed volume
• Almost incompressible
• Expand slightly under heat

Particles of a liquid are in close contact, but can flow.

GASES- form of matter that takes both the shape and volume of its container.

• Takes the shape of its container
• ability to expand to volume of container
• Particles far apart
• easily compressible

Gas refers to a substance that exists in a gaseous state at room temperature, Vapor describes the gaseous state of a substance that is generally a liquid or solid at room temperature.

Particles of a gas are far apart.

PHYSICAL CHANGES (2.1 p.42)

By: Shannon Lamy


PHYSICAL CHANGE- some properties of a material change, but the composition of the material does not change.
EXAMPLE:

• Melting point
• Freezing point
• Boiling point

Physical changes can be classified as reversible or irreversible.

Reversible - can get original state of matter back
Examples:

• changes in states of matter

Irreversible - cannot get original state of matter back
Examples:

• Cutting
• Cracking
• Grinding

Distinguishing Elements and Compunds (2.3 p.48-49)

By: Becky Hyatt

• and element is the simplest form of matter that has a unique set of properties
• a compound is a substance that contains two or more elements chemically combined in a fixed proportion
• compounds can be broken down into simpler substances by chemical means, but elements cannot

Breaking Down Compounds:

• physical methods that are used to separate mixtures cannot be used to break a compound into simpler substances
• a chemical change is a change that produces matter with a different composition than the original matter
• there is no chemical process that will break down carbon into simpler substances because carbon is an element
• chemical change: Sugar ----- Carbon + Water
• chemical change: Water ----- Hydrogen + Oxygen

Properties of Compounds:

• the properties of compounds are different from those of their component elements
• Sugar is a sweet-tasting, white solid, but Carbon is a black, tasteless solid
• Hydrogen is a gas that burns in the presence of oxygen
• the product of this chemical change is water
• Sodium is a gray metal, Chlorine is a pale yellow-green gas, but Sodium Chloride is a white solid

Distinguishing Substances and Mixtures (2.3 p.50-51)

By: Becky Hyatt

• sometimes you can decide by considering whether there is more than one version of the material in question
• milk is a mixture because it can differ in the amount of fat
• gasoline is a mixture because it can be blended in different ways
• if the composition of a material is fixed, the material is a substance; if the composition of the material may vary, the material is a mixture

Conceptual Problem 2.2:

• When the a blue-green solid is heated, a colorless gas and a black solid form.
• All three materials are substances.
• Is it possible to classify these substances as elements or compounds?
• 1. Analyze- Identify the concepts
  • list the known facts and relevant concepts
• 2. Solve- Apply concepts to this situation
  • the blue-green solid must be a compound because of the change is the amount of substances
  • it isn't possible to know if the colorless gas of black solid are elements or compounds

Practice Problem:
Liquid A and Liquid B are clear liquids.
They are placed in open containers and allowed to evaporate.
When evaporation is complete, there is a white solid in container B, but no solid in container A.
From these results, what can you infer about the two liquids?

GROUP 2

Co-Editor: Zoey Killion

Mike Hanley
Caroline Rubino
Haley Conatser
Nate Lynch
James Payne
Olivia Richardson

Organizing the Elements: (page 155-156)

By: Mike Hanley

• By the year 1700, only 13 elements had been identified
• Chemists had assigned names to to some of the elements, but they were unable to isolate the elements from their compounds
• As scientific methods were beginning to be used to search for elements, to rate of their discovery had increased
• In the year 1829, J.W. Dobereiner published a classification system where the elements were grouped into triads, or a set of three elements with similar properties
• Chlorine, bromine, and iodine were placed next to each other in a triad because although they look very different, they have very similar chemical properties

external image s

Picture of chlorine, bromine, and iodine

• Dobereiner noticed a few patterns in his triads, but didn't really acknowledge them or consider them to be significantly important
• Unfortunately, not all of the elements were able to be placed in triads, so a different system of organization had to be made
• In 1869, a Russian chemist and teacher named Dmitri Mendeleev had published a greatly improved table of the elements
• Lothar Meyer also created a very similar version of the table of elements, but he didn't receive nearly as much credit as Mendeleev because his wasn't the first and wasn't explained as well as Dmitri's
• The type of organization Mendeleev chose was periodic, so he organized the elements based on a set of repeating properties
• Mendeleev was also able to predict the properties of some elements that hadn't even existed yet, such as gallium and germanium, and his predictions were correct
• These predictions he made and more proved that the periodic table he made was indeed an extremely useful and important resource, and was one of the most helpful tools for discoveries in chemistry

Mendeleev's Periodic Table (page 156)

By: Caroline Rubino

Mendeleev

• 1869 published a table of the elements
• Russian Chemist
• Won credit of creating the periodic table because.....

1. was the first to publish his table
2. was able to better explain the tables usefulness

Lothar Meyer

• German Chemist
• published a nearly identical table to that of Mendeleev in the same year
• did not receive credit for the creation of the table

Picture of Lothar Meyer
Mendeleev Periodic Table

• He developed his table while working on a textbook for his students
• He needed a way to show the relationships between more that 60 elements
• Wrote the properties of each element on a seperate notecard so he could move the cards around until he found an orgainzation that worked
• Elements are arranged into groups based on a set of repeating properties

• Mendeleev arranged the elements in his periodic table in order of increasing atomic mass

• He left question marks between the entries on zinc and arsenic because he predicted that elements would be discovered to fill those spaces and he also predicted what their properties would be based on their locations in the table.

Mendeleev First Periodic Table of Elements

Metals (pg 158)

By: Haley Conatser

• The international Union of Pure and Applied Chemistry (IUPAC) is an organization that sets standards for chemistry
• The elements can be gouped into 3 broad classes based on their general properties
• These Classes are metals, nonmelts, and metalloids
• Across a period the elements become less metallic and more nonmetallic

Metals

• About 80% of elements are metals
• Metals are good conductors of heat and electric current
• All metals are soils at room temperature, except for mercury
• A freshly cut piece will have a high luster, or sheen
• Many are ductile meaning they can be drawn into a wire
• Most are malleable, which means they can be hammered into thin sheets

Nonmetals and Metalloids (pages 159-160)

By: Zoey Killion

Nonmetals-

• poor conductors of heat and electric current
• great variation in physical properties among nonmetals than among metals
• monst nonmetals are gases at room temperature, including the main components of air : nitrogen and oxygen
• a few are solids such as sulfur and phosphorus
• nonmetals are NOT metals (have properties that are opposite to those of metals)

Metalloids-

• generally has properties that are similar to those of metals and nonmetals
• under some conditions, a metalloid may behave like a metal but under others, it may behave like a nonmetal (controlled by changing conditions)
• example: pure silicon is a poor conductor of electric current but if a small amount of boron is mixed with silicon, the mixture is a good conductor of electric current, like most metals

Boron

Silicon

PUT TITLE HERE

By: Nate Lynch

By: James Payne

Electron Configuration (pg. 164)

-Properties of elements are mostly determined by the electrons

-Elements are sorted into:

1. Tranisition Metals

2. Inner Transition Metals

3. Noble/Inert Gases

4. Representative Elements

The First Four Noble Gases are:

Helium, Neon, Argon and Krypton.

Representative Elements

Groups 1A - 7A on the periodic table

These elements display a wide range of both physical and chemical properties

There is 1 liquid (Bromine), a few gases and mostly solids

It's group number is the number of electrons in the highest occupied energy level

Transition Elements (page 166)

By: Olivia Richardson

Transition Elements

• There are 2 groups in the Periodic Table, Groups A and B
• Group B are the transition elements
• Two types of transition elements are transition metals and inner transition metals.
• Group B is in the body of the Periodic Table
• Example of transition metals: copper, silver, gold, and iron
• In atoms of Transition Metals, the highest occupied s sub-level and a nearby d sub-level contain electrons
• Characterized by presence of electrons in d orbitals
• Inner transition metals and below main body
• In atoms an inner transition metals, the highest occupied s sub-level and a nearby f sub-level generally contain electrons
• Characterized by f orbitals that contain electrons
• Used to be none-earth elements

Silver is and example of a transition metal

Block of Elements

• With electron configurations and positions of elements in Periodic Table another pattern emerges
• In the diagram below, the Periodic Table is cut into different blocks according to highest occupied sub-level
• S block=elements in Groups 1A, 2A, and the noble gas helium
• P block= elements in Groups 3A, 4A, 5A, 6A, 7A, and 8A minus helium
• d block= transition metals
• f block= inner transition metals
• the diagram helps determine electron configurations of elements
• Each period corresponds to a principal energy level.

This periodic table divides it up into the different blocks.

Group 3

Co-Editor: Elizabeth Howard
Andrea Luongo
Dakota Pimentel
Dan McCormack
PJ Hamill

Trends in Atomic Size (page 170-171)

By: Andrea Luongo

• Atomic size can be recorded from the units that form when atoms of the same element are joined together.
• Atomic radius is one half of the distance between the nuclei of two atoms of the same element.
  • Used to estimate the size of atoms.
  • Measured in picometers because the distance betweeen two atoms is very small.
• Molecules- units of atoms of the same element.
  • Atoms in each molecule are identical.

• Distance between nuclei (an atomic radius)

Group Trends in Atomic Size: (page 171)

By: Andrea Luongo

• As the atomic number increases, the charge on the nucleus increases and the atom's energy levels also increases
• The positive charge brings electrons closer to the nucleus, allowing "shielding" for the electrons in the highest energy level. Since this affect is greater than the effect of increasing the nuclear charge, the atomic size increases.

Periodic Trends in Atomic Size: (page 171)

By Andrea Luongo

• Generally, the atomic size decreases across a left to right period.
• The atomic size also increases from top to bottom within a group.
• Elements gain one electron and one proton than the previous element in the period.
• All elements in the period also have the "shielding" effect (atomic size decreases when the nuclear charge pulls the electrons in the highest energy level closer to the nucleus).

• Dereasing atomic size by periods and increasing atomic size by groups.

Ionization of Energy pg 173-174

By: Dakota Pimentel

Quick bullets:

ionization energy- energy required to remove an electron from an atom is called

• electrons can move to higher energy levels when atoms absorb energy
• ionization energy is measured when an element is in it gaseous state
• the energy required to remove the first electron from an atom is called the first ionization energy
  • the cation produced has a 1+ charge
  • the second ionization energy is the energy required to remove an electron from an ion with a 1+ charge
    • the ion produced has a 2+ charge
  • the third ionization energy is the energy required to remove an electron from an ion with a 2+ charge
    • the ion produced has a 3+ charge
• ionization energy can help you predict what ions elements will form
• the first ionization energy decreases from top to bottom within a group
• the first ionization energy of representative elements tends to increase from left to right across a period
• ions are atoms or group of atom that has a positive or negative charge
• atoms are only neutral when the number of protons and electrons is the same
• the positive or negative charge is caused when electrons are either taken on or given away
• Ion: Names and symbols
  • a positively charged ion is called a cation and can be represented with a +
  • a negatively charged ion is called a anion and can be represented with a -

First Ionization Energy Versus Atomic Number:

external image m5f9.GIF

Ions Page (Page 172)

By: Dan McCormack

• Ion- is an atom or group of atoms that has a positive or negative charge
• an atom is electrically neutral because it has equal number of protons and electrons

• The net charge of an atom is zero because it has an equal amount of protons and electrons
• Positive and negative ions form when electrons are transfered between atoms
• If an ion has more electrons than protons then the ion is negative(-) also called a anion
• If an ion has more protons than electrons then the ion is positive(+) also called a cation
• When adding is an element is postitve or negative you just add a plus sign or minus sign but if it is more than one then you have to add the number ex.(Na1+)
• 
  

Trends in Electronegativity (Page 177)

By: Elizabeth Howard

· Electronegativity: The ability of an atom of an element to attract electrons when the atom is in a compound.
· Scientists use factors such as ionization energy to calculate values for electronegativity
· The data in table 1 is expressed in Paulings, named after Linus Pauling who worked on chemical bonds and was the first to define electronegativity
· In general, electronegativity values decrease from top to bottom within a group
· For representative elements, the values tend to increase from left to right across a period
· Metals at the far left of the periodic table have low values. Nonmetals at the far right have high values
· Electronegativity values among the transition metals are not as regular
· The least electronegativity element is cesium with a value of 0.7
· The most electronegativity element is fluorine with a value of 4.0
Table 1:

Summary of Trends (Page 178)

By: Elizabeth Howard

· Trends include atomic size, ionization energy, ionic size, and electronegativity in Groups 1A through 8A
· These trends can be explained by variation in atomic structure
· The increase in nuclear charge and an increase in shielding has a significant effect in trends

TRENDS IN ICONIC SIZE

By: PJ Hamill

When atoms gain or lose electrons, the atom becomes an ion. When an atom gains an electron, it becomes a negatively charged ion that we call an anion. Anions are larger in size than their parent atoms because they have one or more additional electrons, but without an additional proton in the nucleus to help moderate the size.When an atom loses an electron, it becomes a positively charged ion called a cation. Cations are smaller than their parent atoms because they have lost electrons (sometimes the entire outermost energy level) and the electrons that remain behind simply don't take up as much room.

Sizes of Atoms and Ions
Cations				Anions
Na 1.86	Na+ 0.95	Mg 1.60	Mg2+ 0.65	O 0.74	O2- 1.40	F 0.71	F- 1.36
K 2.27	K+ 1.33	Ca	Ca2+	S 1.03	S2- 1.84	Cl 0.99	Cl- 1.81

note that when comparing cations and anions, the anions are larger.




In this section it talks about the size of the elements and what happens to them when they undergo changes.
• Cations – smaller than the atoms in which they form
◦ a positively charged ion, esp. one that moves toward the cathode during electrolysis

• Anions – larger than the atoms in which they form.
◦ A negatively charged ion, especially the ion that migrates to an anode in electrolysis.




On a Periodic Table the size of the cations decrease as you go from left to right.
The same with the size of the anions because they also decrease on the table if you read it left to right.
If you were to look at the periodic table from top to bottom the size generally tends to increase.

Here are some diagrams that demonstraite some cations,
the most common cations, and certin size of cations.