Question 2!

“There are various methods of identifying elements.” There are two main methods like Electron Configurations and Spectroscopy. The Electron Configuration is an arrangement of electrons of an atom, a molecule, and other physical structure. The Spectroscopy is where an objects light turns into a component colors, using this makes it easier to infer physical properties of different objects. The different colors of an element on the periodic table makes us figure out what physical properties they have and to make out the element. The spectroscopy way is also very sensitive. The Electron Configuration helped them slove the different orders of the elements and the arrangement and electrons and also an example of that would be

1s which is Hydrogen but it also is like 1s2 2s2 which is Beryllium but it deals with the orbitals filling.

1s2 2s2 2p6 3s2 etc.

Nobelium which atomic number is 102 and weight is 259 its melting point is 827 degrees Celsius. Classified as a metal and group name is Actinide. This element was named after Alfred Nobel its electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 4f¹⁴ 5s² 5p⁶ 5d¹⁰ 5f¹⁴ 6s² 6p⁶ 7s² this element was founded by three different groups of scientist. First group is Nobel Institute of Physics in Stockholm, second was a Laboratory in Berkeley, California and then the third group was Joint Institute for Nuclear Research in Dubna, Russia.

Question 4

1st period
question 4



A ionic bond is a chemical bond. It occurs when one electron is lost. This makes a positive ion. When one is gained it makes a negative ion. It passes one on to the other. Molecules are made up of atoms in which they are joined together. The most straightforward molecules are made up of two atoms, such as, oxygen gas and nitrogen gas. An example would be bonding heat to a chemical, and letting it sit over time and becoming a crystal.

Question 3

Emily Jaska

3 Types of Bonds

Covalent Bond:

Covalent bonds share one or more electrons between atoms with opposite charges and it is a type of chemical bond. They all share together, and the bonds are best when the outer shell isn't fully filled.

Ionic Bond:

In ionic bonds atoms either share of transfer electrons. Sometimes one atom gains electrons and the other one loses some. Has low electronegativity and low number of electrons.

Hydrogen Bond:

Hydrogen bond is where the hydrogen and electronegative atom in two molecules are bonded together. Hydrogen bonding is usually stronger than most bonds.

Question #1

1. 1803 - John Dalton
2. 1830 - Michael Faraday
3. 1869 - Johannes Hittorf
4. 1879 - William Crookes
5. 1897 - J.J. Thompson
6. 1895 - William Conrad Roentgen
7. 1899 - Ernst Rutherford
8. 1908-1917 - Robert Millikan

1. John Dalton – Atomic Theory
2. Michael Faraday - Cathode – positive side. Anode – negative side
3. Johannes Hittorf - a shadow of an object was cast on the end of the tube toward the cathode.
4. William Crookes - Developed a better vacuum pump with a smaller gas pressure.
5. J.J. Thompson - Found that cathode rays could be deflected by an electric field.
6. William Conrad Roentgen - Found that x-rays could go through solid objects using cathode tubes.
7. Ernst Rutherford - Studied absorption of radioactivity.
8. Robert Millikan – Oil-drop experiment.

Question 3

Summer Dolezel
6th

Question 3- types of bonds





Ionic bonds- An ionic bond is a tie between two atoms that are caused by the forces between opposite charged ions in an ionic compound. When a negative ion meets a positive one, their opposite charges attract and attach the atoms together.











Covalent bonds- Covalent bonds are forces that hold atoms together. When the atoms share electrons, this forms the forces. This term is used to describe the bonds in compounds that share one or more pairs of electrons.











Polar Covalent- Polar Covalent bonds are relevent to a type of covalent bond. Mostly, the atoms spend more time by the Oxygen nucleus than the Hydrogen nucleus. All covalent bonds are polar somewhat unless the bond is between two atoms of the same element.













Hydrogen bonds- A hydrogen bond is between the hydrogen attached to an electronegative atom of one molecule and an electronegative atom of a different molecule. Hydrogen bonds keep water liquid over a wider range of temperature than is found for any other molecule its size.
The energy required to break multiple hydrogen bonds causes water to have a high heat of vaporization.


Useful Sites:

http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch8/valenceframe.html

http://www.green-planet-solar-energy.com/polar-covalent-bond.html

Kayly Adams

Question 3:

There are 3 main types of chemical bonds – ionic, covalent, and polar covalent
There’s also an “extra” that scientists must use sometimes – hydrogen bonds

· IONIC BONDS come from elements with low electronegativity – which means a low or absent number of electrons. And react best with elements with high electronegativity – many or full outer shells. Solids form lattice structures.
Example: sodium chloride (table salt), baking powder
· COVALENT BONDS have a complete sharing of electrons. Meaning they all switch and share together. This type of bond works best with elements that have only partially filled outer shells. Can be solid, liquid, or gas.
Examples: diamonds, carbon
· POLAR COVALENT BONDS (peptide bonds) are a mix of ionic and covalent. They bond best with elements that share electrons. The electrons in this bond spend most of their time around the atom. Atoms involved in polar covalent bonds differ from each other in their electronegativity.
Examples: water, amines
· HYDROGEN BONDS are just hydrogen combining with an electronegative element like nitrogen, oxygen, or fluorine. Opposites attract! (can also be a dihydrogen bond)
Examples: water, ammonia

Question 3

There are three different types of bonds Covalent, ionic, and metallic.

Chemical reactions are formed when 2 or more atoms are chemically bonded together. The result leaves a compound both chemical and physical from the parent atoms.

Ex. Sodium (metal) + chlorine (gas) makes table salt

Ionic bonding

During an ionic bond electrons are passed from atom to atom. while this is happening the atom will either lose or gain an electron, which this reaction will form an ion. The oppositely charged ions are drawn together by static electricity, which creates the ionic bond.

FACTS

- Ionic bonds come from a nonmetal and a metal.

-Ionic compounds conduct electricity.

-Will form crystals.

-Have a high melting point.

-Ionic compounds are solid.

Covalent bonding

Covalent bonding occurs when atoms share electrons, and when the use their electrons in similar ways. Covalent bonds usually occur when 2 nonmetals happen to bond. Instead of both atoms gaining electrons they share electrons, to complete their valance shells.

FACTS

-Electrons are shared.

-Occur by two nonmetals

-Covalent bonds are not strongly attracted to each other.

-Typically liquids or gasses.

Ex. Hydrogen bonding together to make H2

Metallic bonds

Metallic bonding is the bonding of 2 metals, that share electrons throughout each others metal atoms. Metallic bonding is based on the orbital theory ( s,p,d,f). Which basically shows the interaction of a delocalized electron and metal nuclei. The metals physical properties can usually be found by the molecular orbital theory.

FACTS

-Typically have high melting points.

-Most metals are examples of metallic bonding.

-Conduct electricity very well.

-Most metals only have one or two valence electrons.

Ex. Iron (Fe), lithium (Li), potassium (K)

www.visionlearning.com/library/module_viewer.php?mid=55

www.buzzle.com/articles/metallic-bonding.html

Question 1 by Charlotte Quaas

Democritus- stated that the material cause of all things that exist is the coming together of atoms and void. Atoms can never be destroyed and have many different shapes and can cluster together to form things that we can see, touch, taste, smell, etc. Different shapes and arrangements of atoms as well as positions can produce different things as well.

John Dalton- proposed the Atomic Theory in 1803. This theory stated that: all matter was composed of small indivisible particles called atoms, atoms of given elements possess unique characteristics and weight, and there are 3 types of atoms; simple, compound, and complex.

Dmitiri Mendeleev- is known for arranging the 63 known elements into a Periodic Table based on atomic mass. His first periodic table was created on the basis of organizing the elements in ascending order of atomic weight and grouping them by similarity of properties. Mendeleev gave space and variety from strict atomic weight order, which left space for new elements to be discovered. The original table has been modified and corrected several times over the years especially by Mosley. The non modified Periodic Table accommodated the discovery of isotopes, rare gases, etc.

J.J. Thompson- he was experimenting with electricity inside empty glass tubes as was investigating a very old puzzle known as "cathode rays". These experiments gave him the idea to make a bold proposal: that these mysterious rays are particles much smaller than atoms and also are parts of an atom these were called "corpuscles". This proposal turned out to be correct, the rays were made up of electrons.

Earnest Rutherford- whose work constituted a notable land mark in the history of the atom. How he did this was he developed Bacquerel's discovery of Radioactivity into proof that atoms of heavier elements actually disintegrate into different forms of radiation. He is also famous for using particles as atomic bullets and shot them at a thin piece of gold foil. He stated that the nucleus was very dense, small and positively charged. He assumed electrons were located outside of the nucleus.

H.G.J. Moseley- he studied the x-ray spectra of elements and created a truly scientific basis of the Periodic Table by arranging chemical elements in the order of their atomic numbers. During this time Rutherford and his team ( Niels Bohr, Moseley, and others) developed the first coherent theory of the structure of the atom. Their work demonstrated that each element has its own "finger print"; no element was the same. They discovered this by using spectroscopy which they did to nearly all of the elements.

Niels Bohr- he began to work on the problem of the atomic structure. Rutherford had recently said that the atom had a miniature nucleus surrounded by a cloud of electrons. There were some problems with this like: the electrons orbiting the nucleus would lose energy until the spiraled down into the center of the nucleus which would further collapse the atom. Bohr added the new idea of quanta to the model. If the atom absorbed energy the electron would move um a level from the nucleus, and vice versa. This model was a huge leap forward in making a theory fit the evidence gathered over the years.

Schrodinger- his great discovery was his wave equation, which came as a result of his dissatisfaction with the quantum condition in Bohr's orbit theory. he believed that the atomic spectra should be determined by some kind of problem. Schrodinger viewed electrons as continuous clouds which introduced wave mechanics as a mathematical model of the atom.

Question 3

The 3 types of bonds are - Covalent, Ionic, and Metallic.

IONIC- Ionic is the bonding between Metal, and non-metal ions. If a positive Ion meets a Negative, they both attract, (opposites attract). It is formed when one atom is transferred to another, because of the way the shells are. An example of a ionic bond would be common house hold salt. Ionic bonds are also very conductive.

COVALENT- In this type of bonding, unlike ionic, a pair of electrons are shared, one comes from each atom. These molecules usually have low melting points, along with low boiling points. This type of bond is usually used in the Lewis Dot Structure. H20 is a common example of a covalent bond. These atoms are also neutral in charge.

METALLIC - The electron sharing in this one is free sharing. Electrons move freely. These are also highly conductive, and have high boiling and melting points. These are also very conductive.
Iron + Carbon is an example of this type of bonding. The metal atoms in this don't lose electrons to form ions.



Sources:
http://www.historyoftheuniverse.com/ionicbon.html
http://www.buzzle.com/articles/metallic-bonding.html
http://www.youtube.com/watch?v=xTx_DWboEVs

Question 3

Covalent bonds:
These come from atoms sharing their valence electrons. Because they are not ionic, they obviously are not consisted of ions; they are consisted of molecules held together by forces called Van der Waal’s forces which are not strong. Just like how we know how gases are spread out, solids are compact, and liquids are the slightly spaced out substances with no shape, it is the same with covalent compounds and Van der Waal’s forces; the forces are not strong enough to create strong solids however, so the solids are soft. The compounds have low density because of how spread out the molecules are in the substances due to the weak forces. Low melting points and boiling points are a characteristic of these bonds because it is easy for energy to break Van der Waal’s forces. Electricity doesn’t travel well through these bonds because they don’t have as good electric potential as ionic bonds.

Covalent bonds share electrons. In the first electron shell of hydrogen, there is one valence electron; the first electron shell has space for two electrons, so an extra electron will be attracted to the atom.. Another hydrogen atom has the ability to combine with that atom so that their electrons will combine to fill up the electron shell, creating H2 – a covalent bond.

Ionic bonds:
In ionic bonds, electrons transfer between atoms. Electrostatic forces hold atoms together after they lose or gain electrons and their charges change, making the atoms attracted to each other.
When a sodium atom gives the electron it has in its outer shell to a chlorine atom, which has one open spot in its outer shell, the sodium gets a positive charge from losing an electron and the chlorine gets a negative charge when it gains the electron from the sodium atom. An ionic bond is made because opposites attract!

Ionic bonds are made up of metals and nonmetals because they attract to each other due to the fact that metals lose their electrons and nonmetals are the opposite. Ionic compounds conduct electricity well, most likely because of the presence of metal, and dissolve rapidly in water. Their bond has stronger forces than covalent bonds, so they can resist temperature a little better; therefore, they have a higher melting point. It’s tougher to break their bond and they make crystalline atoms.

Metallic bonding:
Metallic bonding happens between metals. Because, according to the Electron sea model/Electron gas theory, metallic bonds are not aimed at any specific direction, their bonds are weaker than covalent bonds.



The metals give up their valence electrons easily and electrons move around empty orbitals in the metals without restraint, like the liberated movement of sea water or gas (how it gets its name), because of the lower energy. Positive metal ion layers and electrons that are drawn to each other are what form the bond. Size and charge of the metal ions along with the number of valence electrons determine how strong the bond between two metals will be.

Metals are malleable and ductile because of the weak metallic bonds. The metals we can hold in our hands, such as lead – which is a very flexible metal, are perfect examples of these bonds.

Picture: http://www.geo.arizona.edu/xtal/nats101/s04-18.html

Question 1- Kallliieee(:

Democritus: The Greek philosophers wanted to explain the natural world; through observations, philosophers believed that a "primary matter" existed. It was because of this “primary matter”, changed in different ways that all other things were created. Democritus expanded the idea to state that matter was composed of small particles called "atoms" that couldn’t be divided more. These atoms were all composed of the same primary matter with the only differences between them being their size, shape and weight. These differences explained the differences in the properties of the matter around us. Democritus’ ideas were ignored for the next 2,000 years; however, they proved to be very useful in the further research of the atoms.

John Dalton: For nearly 2000 years science was unable to come up with experiments capable of testing Democritus’ ideas. During the 19th century, a huge amount of data on how substances react with each other was collected. From this data, some simple laws of chemical reactivity had been developed, including the law of conservation of matter. While others had similar theories, John Dalton is usually credited with developing the first atomic theory.

Dalton's theory:
Matter is composed of small particles called atoms.
All atoms of an element are identical, but are different from those of any other element.
During chemical reactions, atoms are neither created nor destroyed, but are simply rearranged.
Atoms always combine in whole number multiples of each other.

In addition to helping explain the laws of chemical reactivity, Dalton's theory also helped further the concept of atomic weights. He made symbols for some elements and a table, a big step in this time for the development of the atom.

Dmitri Mendeleev: Contributions of earlier 19th century scientists led to the accurate determination of atomic weights of elements and chemical formulas of compounds made from them. These determinations gave way for the first periodic table!! Whoop whoop! Dmitri Mendeleev tried to classify the elements in an exact way. He wanted this system to be numerical which meant, at this time, atomic weight. By putting them in order of increasing atomic weight, he found similar properities and lined them vertically with each other. He found some holes in the table where some elements should exist. He made predictions about this which helped in later discoveries


Henri Becquerel then Marie and Pierre Curie:
Henri Becquerel discovered that a sample of uranium was able to expose a photographic plate even when the sample and plate were separated by black paper (http://www.neoam.cc.ok.us/~rjones/Pages/online1014/chemistry/chapter_8/pages/history_of_atom.html).
He also discovered that the exposure of the plate did not depend on the chemical state of the uranium (what uranium compound was used) and that it must be due to some property of the uranium atom (http://www.neoam.cc.ok.us/~rjones/Pages/online1014/chemistry/chapter_8/pages/history_of_atom.html).

When Becquerel abandoned this work, it Pierre and Marie Curie picked up the slack and went on to discover other radioactive elements. Marie suggested that the uranium, and the new elements, were somehow dissolving over time and sending off radiation known as "radioactivity". For the first time it was thought that atoms might be composed of even smaller particles that could be further researched.

J.J. Thomson: At about the same time as radioactivity was being found, J.J. Thomson and others were performing experiments with cathode ray tubes. When a potential is placed between the cathode (the negatively charged plate) and the anode (the positively charged plate) a "ray" of electric current passes from one plate to the other. Thomson discovered the ray was composed of particles. (http://www.neoam.cc.ok.us/~rjones/Pages/online1014/chemistry/chapter_8/pages/history_of_atom.html)
In later experiments he predicted what metal was used to make the electrodes and what gas was used to filled the tube. Each time, the properties of the ray particles were the same. He concluded that negatively charged particles were subatomic particles which were part of every atom. He also concluded there were neutral and positive charges. Based on these conclusions Thomson proposed that an atom was composed of a ball of positive charges with "corpuscles" of negative charge inside it(http://www.neoam.cc.ok.us/~rjones/Pages/online1014/chemistry/chapter_8/pages/history_of_atom.html). The corpuscles were later known as electrons.

Ernest Rutherford: Thomson had discovered that the atom was composed of positive and negative charges and that the mass was made up of these. If the negative and positive charges left empty space in the atom, particles that are shot at the atom might be able to pass through them. In 1909, with the help of Hans Geiger and Ernest Marsden, Rutherford worked on an experiment. The gold tin foil experiment. This later led to the discovery of the size of the atom and the nucleus.

Henry Moseley: When Henry Moseley tried to determine the frequency of an x-ray in an experiment, he found as a result a pattern he called the “Q” value. This led him to believe that there was a quanity that increased as he went from one element to the next. This value would later become known as the atomic number.

James Chadwick: Only two known elementary particles had been identified, the proton and the electron, until James Chadwick. Protons had a mass of 1 and a charge of +1, while electrons had no mass and a charge of -1. There was still a problem though, there was extra mass! The problem of the extra mass was solved in 1932 when Chadwick identified the neutron. While studying the radiation resulting from the combining of beryllium with alpha particles, Chadwick found a particle with about the same mass as a proton being let off. This was known as the neutron.

****when i cited words i couldnt re-word, since is was the actually experiment, i used the source at the very end instead of at the end of every single tiny thing.

Lindsey Kunze

Question # 3!!!!!

3 Types of bonds: Covalent, ionic, and metallic bonds

Covalent bond is a chemical bond that forms by sharing one or more electrons between atoms. Covalent bonds hold atoms together. Covalent bonds are the attraction and repulsive forces between atoms when they share electrons.
Characteristics:
low melting point
low boiling point
soluble in nonpolar solvents
most common in organic compounds
do not conduct electricity
Example
H2 and O2

Ionic bonds involves a metal and a nonmetal. In ionic bonds electrons are completely transferred and either lose or gain negatively charged electrons. The metal gives one or more electrons which causes a positively charged atom with a stable electron congiration. These electrons enter the nonmetal which causes it to form a negatively charged ion which has a stable configuration also. The attraction between the opposite charged ions causes them to come together and form a bond.
Characteristics
high melting points
conduct electricity
dissolve easily in water
well defined crystals
high boiling point
Example
NaCl

In metallic bonds, an atom achieves a stable configuration by sharing electrons of its outer shell with other atoms. Metallic bonds overcome elements in which the valence electrons are not tightly bounded with the nucleus, which mainly occurs in, metals. Each atom in a metal crystal all the electrons with its valence shell to all the other atoms.
Characteristics
thermal
conduct electricity
high melting point
high boiling point
strong
malleable
opaque
Example
Zn and Fe

Retest Question 2

Electron configuration and spectroscopy have facilitated the organization of the periodic table because it gives the table an order on which to follow. The electron configuration is a constant pattern that electrons fit into when forming new atoms, and spectroscopy deals with the light givin off by said electrons when they become excited. Because both of those things are unchangable variables, they can be used as a sense of order. The periodic table is constant because both electron configuration and spectroscopy are constant.

Americium was discovered in 1944 by Glenn. T. Seaborg. He discovered it by bombarding plutonium with neutrons. Am241 is commonly used as a part of home smoke detectors due to its radioactivity and the ability of radiation of radiation to be easily detected.

QUESTION #1 JORDAN YARBROUGH

QUESTION #1


JJ THOMSON- He used positive rays to discover a method to separate different kinds of atoms. He also discovered the electron. In 1897, he proved to other scientists that the atom was not invisible, but it in fact had electrons that you could see through a cathode ray. Later on he also discovered isotopes and improved mass spectrometry.


JAMES CHADWICK- In 1932, he, discovered the neutron. He inspired many other scientists to discover nuclear reactions. The discovery of this became well known because it


JOHN DALTON-. The modern atomic theory is something that Dalton spent a great deal of his life developing, and it is what we use today and in the future to come. His Experiments led to the discovery of the law of partial pressures and law of stoichiometry. He investigated in the gas laws and even made them better.


DMITRI MENDELEEV- He created the first periodic table and arranged them by atomic mass by using their properties/characteristics. He basically predicted unknown elements and put them into the periodic table without really knowing they were going to go there or whether there were elements to go there at all.


DEMOCRITUS- He believed that all matter consisted of tiny invisible particles. He theorized that atoms were never created but that they always existed, and they had different properties of matter. Basically, he didn’t discover anything, he just theorized almost precisely on the dot without any evidence whatsoever.


AMEDEO AVOGADRO- He is known for Avogadro’s number. What he came up with was the base for the molecular masses. He said the masses of the volume of gas had to do with their molecular weights.


RUTHERFORD- He theorized the atoms nucleus He also questioned the existence of the neuron and made a theory about that as well. Rutherford, along with some other scientists, discovered that the neutron was not the only particle inside the nucleus, which came to a result of a new atom structure. (Later to be changed again by Bohr.)


BOHR- He improved Rutherford’s structure of the atom. He realized what the electrons were good for and that they surrounded the nucleus at different levels but ONLY when energy is lost or gained.

Question 4 Cassidy Stigliano

Think about the types of bonds that we have discussed. We have disused the method used to determine the ratio of one element to another in an ionic bonded compound. We have not discussed how we determine covalent or metallic bonds. You are to discuss how we determine ionic bonds and then determine how we discover the bond and formation of the molecule. Make sure you use specific examples including experiments

Ionic bonds are determined by a metal and a nonmetal. The metal element loses the electrons and nonmetals gain the electrons. Ionic bonds have a high boiling point and a high melting point and they are brittle. An example of an ionic bond is Sodium Chloride which is salt. The discover of the ionic bond was Svante Arrhenius. The formation of the molecules in an ionic bond are the metals losing electrons and nonmetals gaining electrons.

Experiment:
1. You need to get a temperature probe.
2. Set up ring stand and bunsen burner.
3. Put water in a beaker.
4. Put NaCl (salt) in a test tube.
5. Put the test tube in the beaker.
6. Put the beaker on the ring clamp over the bunsen burner.
7. Find the melting point of the ionic compound.

Retest Blog-Question 3

Test Question 3---There are three divisions for the types of bonds that occur. Explain the three types of bonds and their characteristics. Then explain the reason for their characteristics by use of concepts such as ,metal, nonmetal, metalloid as well as forces of bonding (notice i did not give you the name for that). Make sure that you explain all the characteristicsand you give examples.



The three bonds that I know of are Ionic, Covalent, and Hydrogen Bonds.



Ionic- The characteristics for the Ionic Bonds: they are really hard, strong, and have a high melting point. They can be transparent through the spectrum, and can absorb easily. They also lose energy through electron exchange. Their outer shells are in the shape of a sphere and have a noble gas pattern. This bond takes place when you have 2 opposilty charged ions but they have to be a metal and a Non-metal. An example would be table salt or Sodium Chloride. Sodium and Chlorine form together to get salt. Through this process the Sodium loses an electron and the Chlorine gains one. Because of this it is known as a 1:1 ratio meaning that you get Sodium Chloride!



Covalent-The Characteristics for Covalent Bonds: these bonds have low polarity, low boiling point, and low melting point. Two non-metals are needed in order to form a covalent bond. It is also a neutral molecule and can be a solid, liquid or gas. It has a weak form of attraction between its molecule. Covalent bonding is the sharing of electrons. The elemenets dont have to have to same 2 atoms but they do need to have a close relationship of electronegativity.(Wikki) Electronegativity is the ability of an atom to attract electrons to itself (Wikki). An example of a covalent bond would be SO2. Sulphur Dioxide is a covalent bond because they are both non-metals.



Hydrogen-The characteristice for Covalent Bonds:The Hydrogen bond must have one hydrogen atom and one high electronegative atom from a different molecule. In order to form a hydrogen bond it will have gone through a covalent bond. The hydrogen bond will only have 5% to 10% of the strength of a Covalent bond. The Hydrogen bond is also what holds our DNA together. An example would be when hydrogen attaches to carbon, hydrogen bonding occurs when the carbon atom is bound to electronegative atom forming chloroform (CHCl3)!

Alexa Gee

Question Number Three!

The three types of bonds are ionic, covalent, and metallic.

Ionic Bonds
In this bond when and atom recieves or gives a valence electron. Ionic bonds have very high melting and boiling points, they conduct electricity, have crystals and dissolve in water. One of the atoms is a metal and one is a non-metal.
some examples are NaCl,MgO,and KBr.

Covalent Bonds
In this bond a pair of electrons are shared.Lewis Dot Stucture is used with this bond. Covalent bonds don't conduct electricity, have a low boiling and melting point. They are neutral in charge. They are hard. They don't disolve in water. Examples of covalent bonds are HCl, H2O

Metallic Bonds
In this type of bond they share free electrons. Not all metals can be used in metallic bonding. This bond holds stuff together. Most of the time this occurs in the outermost ring. Metallic bonds highly conduct electricity. They also conduct heat. They can be made into thin wires(ductile). It is very strong and hard. Examples of metallic bonds are copper,zinc and iron

Alex Warren

Question 3!
Let’s try this again!!

Ionic Bond
A chemical bond that uses a metal ion and a nonmetal ion, or sometimes a polyatomic, but must use two oppositely charged ions. The metal gives more electrons and forms a cation. The electrons go to the nonmetal and form an anion. A cation is positively charged and an anion is negatively charged. When these two come together they form an ionic bond.
Characteristics:
Dissolve quickly in water
Conduct electricity
High melting temperatures
Solids
Example:
NaCl

Covalent Bond
A chemical bond that shares valence electrons between atoms. These atoms do not have to be of the same element. The strength of the bond depends on the polyatomics.
Characteristics:
Low melting and boiling points
Solids, liquids gases
Do not dissolve in water
Do not conduct electricity
Example:
CO2

Polar Covalent Bond
A chemical bond that sharing electrons is unequal. The charges of some atoms are separated with some atoms being more charged than the other. The atom attracting electrons with another atom present is property called electronegativity.
Characteristics:
Share electrons unequally
Electronegativity has to be greater than .4
Strong forces
Partially negative and partially positive
Example:
H2O

There are three divisions for the types of bonds that occur. Explain the three types of bonds and their characteristics. Then explain the reason for their characteristics by use of concepts such as ,metal, nonmetal, metalloid as well as forces of bonding (notice i did not give you the name for that). Make sure that you explain all the characteristics
and you give examples.

Ionic, Covalent, and Metallic Bonds are the three types of chemical bonds.
Ionic bonds come from elements with low electronegativity and they react with elements that have high electronegativity. There is a full transfer of electrons. One example is the reaction of sodium and chlorine. Sodium loses its valence electron to Chlorine, which results in a positively charged sodium ion and a negatively charged chlorine ion.
Ionic bonds form between metals and nonmetals.
When you name simple ionic compounds, the metal is always first, the nonmetal second..
Ionic compounds dissolve easily in water and other polar solvents.
In solution, ionic compounds easily conduct electricity.
Ionic compounds often form crystalline solids with high melting temperatures.
Covalent bonding is when two or more elements share electrons. Most of the time this happens when two nonmetals bond together. A good example of a covalent bond is what occurs between two hydrogen atoms. Each hydrogen atom will want to pick up a second electron which results in forming a covalent bond.
In a metallic bond an atom gets a more secure configuration by sharing the elctrons in its outer shell with many other atoms. Metallic bonds happen in elements where the valence electrons are not tightly bound with the nucleus, which are mostly metals.

Jessie Boswell question 1

Examine the history of the development of the atom. We have already discussed the
major players in the development of the atom. Pick out at least 8 major players who
helped aid in the development of the concept of the atom. Then explain each
experiment in a concise explanation. Then explain how each one aided in the
development of the next or how their concept assisted in the further development of the current quantum model of the atom.

Democritus, Dalton, Mendeleev, JJ Thomson, Rutherford, Moseley, Bohr, Chadwick,

Democritus-

Democritus was the type of person to look at the world with mechanistic type of views. Democritus had a theory that everything was made up of atoms and that they could never be destroyed and are always moving around. This is part of what helped Dalton create his theory.

Dalton-

He came up with Dalton’s atomic theory. This theory was partly right by him saying that atoms of the same element are alike in weight and other properties and that different atoms are different in weight and other properties. He was also right about compounds forming by the union or separation of definite numbers of atoms. The incorrect part was that all matter is composed of very small indivisible particles called atoms. Also, that atoms do not divide in chemical reactions; only whole atoms unite with other atoms, this was incorrect. Dalton helped with our quantum model by providing that every atom is different.

Mendeleev- organized the periodic table by the elements atomic weight and properties. Predicted where there was gaps in the periodic table that the element would be found and that it would be put in to the proper place without affecting the order of the table. Mendeleev was right and three elements were found in his lifetime. These elements are lifetimeógallium, scandium, and germanium. This helped with understanding the universe and how things are in the world. Mendeleev helped with Moseley to see that the PT needed to be arranged by atomic number.

JJ Thomson- Used Cathode rays to hypothesize that there were smaller particles contained inside of the atom. JJ was right and the particles inside are called electrons. These are negatively charged particles and are fundamental parts of the atom. The cathode rays are currents of electricity inside of glass tubes. Thomson finding electrons helped with the quantum model because it shows that there are electrons in the outer parts.

Rutherford- Used the gold foil experiment to shot that there are protons in the atom. This experiment used a particle emitter and shot the particles through a slit which then could pass through gold or bounce off of it and back onto the surrounding layer. Rutherford helped with the quantum model by showing that there is positive charged particles, which led to other people drawing the atom and leading up to the quantum atom.

Moseley-

Moseley provided a more accurate PT by arranging the elements by atomic number. Moseley showed that some of the elements did not have the correct atomic masses and that by ordering them by atomic number it helped solve the problem of missing elements. This helped the quantum model by showing how many electrons there truly are.

Bohr- Bohr corrected Rutherford by saying that electrons travel in different orbits around the nucleus. Bohr said that each ring going out could hold more than the inner rings. Bohr also said that these orbits determined the atom’s chemical properties. Bohr helped with the quantum model by showing that there are different electron energy levels and that electrons were in a certain level.

Chadwick-

Chadwick had been working with Rutherford and he thought that there was a neutral part to the atom because the atomic mass did not add up when you looked at the whole atom. Chadwick used a lot of experiments to show that point zero one percent of the neutron was bigger than the proton. The neutron helped to get the atomic mass to finally be equal, and this helped show where to put the neutron because neutrons do not bond with any other particles.

In 1897, J.J. Thomson discovered the electron through the use of his cathode ray experiment. He also concluded that they are a part of every atom.

In 1913, through one of his radioactive experiments, Frederick Soddy discovered the different types of atoms in different parts of the periodic table.

Margeret Todd made up the term isotopes for Soddy's discovery on atoms. This later led to the discovery of stable isotopes.

In 1913, Niels Bohr came up with the first model of the hydrogen atom. He also stated that electrons could jump from their individual spheres to others.

In 1938, chemist Otto Hahn, through his chemical experiments, discovered the element barium. This was later verified as the first example of nuclear fission.

In 1803, John Dalton used atoms in a theory to explain how different types of chemical reactions occurred. This caused him to be called the father of modern atom theory.

In 1789, Antoine Lavoisier created the law of conservation of mass and discovered that elements can't be broken down further.

In 1905, Albert Einstein was the first person to analyze Robert Brown's "Brownian Motion" using mathematics.


Sources:
http://en.wikipedia.org/wiki/Atom

Question #3

-There are 3 types of bonds: ionic, covalent, and metallic bonds.

Some of the Characteristics of Ionic Bonds are that they have high melting points, they can conduct electricity, they can dissolve easily in H2O, & they have well defined crystals.

"Examples: NaCl, CaCO3 (smallscalechemistry.com)."

Ionic bonding is a chemical bond that is transfering is's electrons from each atom to the other. They can either gain or lose electrons. When the ions become charged, they are then attracted to each other. The result of this attraction is the formation of a negative ion and a positive ion. A negative ion is called an Anion and a positive ion is called a Cation.

Example: sodium chloride

Ionic bonds occur between nonmetals & metals

Some of the Characteristics of Covalent Bonds are that they are neutral molecules, they are non conductors of electricity, and they have low boiling & melting points.

Some Examples: Hydrogen, Carbon, Nitrogen, & Oxygen


-"Single covalent bond – one pair of electrons that are shared by 2 atoms.
Examples: H2, F2 & I2
-Double covalent bond- two pairs of shared electrons.
Examples: O2, CO2 & H2CO
-Triple covalent bonds- three pairs of shared electrons.
Examples: C2H2 & N2(visionlearning.com)."

When a nonmetal & another nonmetal bond, they form a covalent bond.


Some of the Characteristics of Metallic Bonds are that they are malleable solids, they have high melting and boiling points, and that they are insoluble in nonpolar solvents.

Examples: gold & copper(smallscalechemistry.com)."

"In Metallic Bonding the valence electrons of all the atoms of the certain substance are shared.

Metallic bonding occurs between a mix of metals in alloys(smallscalechemistry.com)."


References: http://www.smallscalechemistry.colostate.edu/PowerfulPictures/ChemicalBonding.pdf
http://www.visionlearning.com/library/module_viewer.php?mid=55

8 major players...

The development of the atom is an accomplishment that only few people have had the privilege of contributing to. It starts with English Chemist and Mathmatician John Dalton. Dalton was the first person to scientifically prove that matter consists of small descrete particles. This was known as the Atomic Theory. Michael Faraday then contributed to the development by setting up a pair of metal plates sealed into a small glass tube filled with a gas while metal plates were connected to a array of batteries. as pressure decreased, the gas seemed to glow. After later proving it was no know that whatever it was that produced the magnetic field; being atoms, were electronically charged. Demotocris was also a major player with the very first atomic theory that somehow had understanding of the present 21st century model of atom. Later scientists were able to build on this theory to gain the knoledge of today. That's when Ernest Rutherford, a very prestigious scientist that originated from Britain developed a basic concept of the atomic structure, making it easier for people without great scientific knowledge to understand and to better the understanding for other scientists and developers. Rutherford stated that atoms are made up of a nucleus at the center and a positive charge of electricity and negatively charged particles surrounding it, called electrons. German scientist J.J. Thompson discovered the electron in 1897 while working in his laboratory. In 1917 Robert Millikan performed an oil drop experiment involving the measurement the charge on an electron by using an oil-drop apparatus. A spray pump froma perfume bottle sprayed oil and water droplets into the sample. Conclusion was that the charge drop was always a multiple of 1.59 x 10 -19 Coulombs,proving the well know hypothesis that an electron was near 1000 times smaller than thatof the smallest atom. Also Niel Bohr made his fairly large contribution by developing the atomic model. The atomic model is an organized, process based, model to show the differences of atom configuration. Wrapping up most large developement, James Chadwick proved that nuetrons in the nucleous made up approximately half of the mass of an atom, existed. He also developed a series of Atomic Rules:
1.) The number of proton in the atom is equal to the atomic number, etc.

question #1

Examine the history of the development of the atom. We have already discussed themajor players in the development of the atom. Pick out at least 8 major players whohelped aid in the development of the concept of the atom. Then explain eachexperiment in a concise explanation. Then explain how each one aided in thedevelopment of the next or how their concept assisted in the further development of the current quantum model of the atom.

In 1803, John Dalton developed his Atomic Theory. According to Atomic Theory, matter is made up of indivisible atoms, all atoms of an element are identical, atoms are not created or destroyed, atoms of different elements have different weights and chemical properties, and atoms of different elements combine to form compounds. Dalton's theory had flaws, but it helped proceeding scientists understand atoms.

In 1830, Michael Faraday did an experiment that showed evidence of electrons through glowing in a magnetic field caused by electrical charges. Though electrons were not known of at the time, this experiment showed that something electrically charged existed.

In 1897, J.J. Thompson theorized that everything in the universe was made of small particles. He found that cathode rays could be deflected by an electric field, and that the rays were really particles. He also formed the Plum Pudding model of the atom, which showed electrons floating freely within the nucleus. Thompson concluded that there must also be positively charged particles, disproving the section of Dalton's theory that stated atoms were indivisible.

In 1911 Ernst Rutherford revised Thompson's atomic model in studies of the deflection of alpha particles as they were targeted at thin gold foil sheets. Most of the alpha particles penetrated straight through the sheets, but a few were deflected at small angles. This meant that the positive charge and mass of an atom were located in the center of the atom and only made up a little bit of the total volume. This center was named the nucleus.

In 1917, Thompsons theory that the atom was split in to smaller particles was further reasearched by Robert Millikan. By experimenting with an "oil-drop apparatus" that measured electron charge. He proved that the mass of electrons was 1000 times smaller that atoms.

In 1913, A. van Broek proposed that instead of being compared to the atomic weight, the postivive atomic charge should be equal to the atomic number, as is thought today.

In 1914, a scientist named H.G.J. Mosely formed a hypothesis that the nucleus emitting x-rays effected the rays frequencies. Through this hypothesis, he inferred that the positive charge in atoms was equal to the atomic number.

In 1932, James Chadwick proved the existence of particles in the atom that were not electronically or positively charged. These are called neutrons.

There 3 main types of divisions for bonding. There is ionic bonds, covalent bonds, and metallic bonds.
Ionic Bonds-
An ionic bond is a bond with an element with a positive and negative charge usually a metal and nonmetal. Anions are atoms with negative charges .Cations are atoms with positive charge . In ionic bonding the electrons are transferred from one atom to the other by either gaining or losing electrons; the purpose of the elements gaining or losing electrons is so that they can have a full octet like that of a noble gas. Group 1 to 3 will lose electrons and groups 5 to 7 will gain electrons. The oppositely charged atoms are attracted by electrostatic forces.
Covalent Bonds-
Covalent Bonds share electrons this type of bond can occur between two or more elements share electrons. A covalent bond occurs because the elements in the compound have similar tendencies for electrons usually to gain electrons. The most common thing for a covalent bond is when two nonmetals come together to bond because the nonmetals will want to gain electrons; therefore, the elements will share their electrons to fill the orbital.
Metallic bonds-
Metallic bonding is the attraction between certain electrons, called conduction electrons, and the metallic nuclei within the metals gatheraround the eletron cloud. Zinc and copper are good examples of a metallic bond.When Zinc and Copper are bonded brass is formed.because of the negative charge of the electron cloud pull the positive atoms causing them to form a metallic bond. The electronic cloud moves freely in a direction and when voltage is applied an electron current is formed where thermal energy is released allowing this to bond a good conductor of heat.

Question 4!

Svante Arrhenius discover the Ionic bond. Ionic bonds form when there are non-metals and metals bonding. To determine the ionic bonds you have to low electronagativity elements react with high electrongativity elements. When that happens it’s a complete transfer of electrons. An example is table salt, sodium chloride. Sodium makes one outer shell electron completely to chlorine which needs only on electron to fill its shell. This mixture between atoms is much like static electricity that is opposite chargers. Ionic bonds are hard and brittle and have a melting point at 500.C. Ionic bonds are solids at room temperature.

Wesley Barnhill question #4

You are to discuss how we determine ionic bonds and then determine how we discover the bond and formation of the molecule

"An ionic bond is a chemical bond between two ions with an electron and a proton. They are also known as electrovalent bonds." (answers.com -ionic-bond) These bonds were Discovered in 1897 by J.J. Thompson discovering that the most important part to to ionic bonding is the electron. (answers.com -chemical-bonding) This is important because an electron is either lost or gained in the process of bonding. An ionic bond is usually a non metal and a metal bonding, examples of the bond would be sodium chloride or also known as salt. Chemist John Dalton Came up with the theory that all known things are made of atoms and atoms are indestructible and indivisible, (iun) enabling another physicist by the name of Amedeo Avogadro to research the theory and describe the molecular model (which is the arrangement of the atoms within a molecule). His description of the molecule was eventually used by Stanislao Cannizzaro to figure out the atomic mass of elements was later became important in the discovery of ionic bonding. The name of the bonding product is the name of the metal then followed by the non metal . (Brighthub)

Videos:
http://www.youtube.com/watch?v=QqjcCvzWwww
http://www.youtube.com/watch?v=Ms_ehUVvKKk
References:
http://www.answers.com/topic/ionic-bond
http://www.iun.edu/~cpanhd/C101webnotes/composition/dalton.html
http://www.answers.com/topic/chemical-bonding
http://www.brighthub.com/education/homework-tips/articles/88778.aspx

Question 2 - Cory Wilson

Electron Configuration- Electron Configuration is a method that we use to better identify the elements of the periodic table. It uses orbitals labeled S,P,D, and F to locate different elements on the periodic table. Each element has its own electron configuration. Neils Bohr was the first to concieve of this method in 1923 but could not complete his theory. Later Pauli realized the problem, and finished Bohrs work.

Spectroscopy- Spectoscopy is another method for identifying the elements of the periodic table. There are many different types of spectroscopy, the type that we used in class was called infared spectroscopy. It uses a spectrum to identify the exact distance of the colors shown through the defracting gradient. This is also known as the elements molecular fingerprint because no two elements have the same spectrum.

Rutherfordium- This is a somewhat curious element because it was founded by two different groups of scientists using two different methods. In 1969 a man by the name of Albert Ghiorso, a New Zealand chemisist, first reported the production of Rutherfordium. In 1969, a team of scientists set out to confirm Ghiorso's discovery at the Lawrence Berkeley Laboratory in California. They didnt have the exact tools need to confirm Ghiorso's discovery so they used a slightly different method and got the same results.

Retest Blog

So since you did do some research, let’s save some time. You have a lot of things going on and I recognize that you are making the effort to rectify the situation. So you may choose any of the four original questions to do.

Make sure that you note which one you are choosing to do

Also remember it is not about quantity rather it’s about quality.

Give me your thoughts and understanding of the material. It helps me to understand what you understand in the material.

If you have to use a reference, make sure that you cite it.

Also do not use the author’s words- I want to hear your words!

Good Luck- the quicker you get it turned in, the quicker I can finalize your grades before I head to Houston!
___________________________________________________________

question 1

Examine the history of the development of the atom. We have already discussed the
major players in the development of the atom. Pick out at least 8 major players who
helped aid in the development of the concept of the atom. Then explain each
experiment in a concise explanation. Then explain how each one aided in the
development of the next or how their concept assisted in the further development of the current quantum model of the atom.

#2

There are various methods of identifying elements. We have discussed how electron
configurations can be used to identify elements as well as how to identify with
spectroscopy. We have also examined how the periodic table has been developed and
arranged through experimentation. Explain how all of these developments have verified
the construction and the arrangement of the periodic table. Then examine how scientist develop new elements. Pick one new element and explain how the scientist developed it and where it belongs on the periodic table of elements.

Test Question 3

There are three divisions for the types of bonds that occur. Explain the three types of bonds and their characteristics. Then explain the reason for their characteristics by use of concepts such as ,metal, nonmetal, metalloid as well as forces of bonding (notice i did not give you the name for that). Make sure that you explain all the characteristics
and you give examples.

#4

Think about the types of bonds that we have discussed. We have disused the method
used to determine the ratio of one element to another in an ionic bonded compound. We
have not discussed how we determine covalent or metallic bonds. You are to discuss
how we determine ionic bonds and then determine how we discover the bond and
formation of the molecule. Make sure you use specific examples including experiments.