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