Stoichiometry Lab Report

The electrons on the outer shell are called valence electrons and are the ones who form chemical bonds with other

Thus, the six-membered ring is very stable. However, the individually small torsional effects can affect the shapes of molecules tremendously, and shapes affect

Observe and describe the effect of different wavelengths on speed of electrons emitted. 2. Observe and describe the effect of different levels of intensity on number of electrons emitted. 3. Select different elements of sodium, zinc, copper, platinum, and calcium.

Percentage of Oxygen in a Compound: Stoichiometry and Catalysis Jarling Perez Carl Eguez CHM1045L, U43 October 30,2015 Table of Contents: Introduction………………………………………………………………………………………3 Procedure…………………………………………………………………………………………4 Results.……………………………………………………………………………………………5 Discussion…………………………………………………………………………………………8 References…………………………………………………………………………………………9 Introduction: Stoichiometry refers to the quantitative relation between reactants and products during a chemical reactions. There are many ways in which this method can be used. For instance, if the initial reactant amount is given, this technique would help us determine the products formed or vice-versa.

These molecules were found to have a spheroidal geometry similar to that of Buckminster Fuller’s

bound much tighter and form more stable molecules than atoms of the ionic bond. The chemical formulas for covalent compounds are referred to as as molecular formulas because they exist as separate molecules. Another reason on why covalent is the best naming system is because the things in our daily lives such as oxygen, nitrogen gas, water vapor, and carbon dioxide are all made up of covalent compounds. Covalent compounds are common in the air we breathe, the gas we use to fuel our cars, the water we drink and even the food we eat. Without this bond we wouldn't have the things that help us carry on with our lives.

The atoms of the isotopes of Lithium behave almost exactly the same way when doing chemistry, since the atoms electrons only care about the charge of the nucleus. The arrangement of electrons in an atom is known as its electronic configuration. How does an electronic configuration look like? It is commonly believed that the electrons move around the nucleus randomly in a three-dimensional pattern defined by their energy level.

Lone Pairs ADI Lone pairs, the electrons that the central atom does not share during a covalent bond, can and will affect the shape of a molecule in various ways. During this lab, the goal was to answer the guiding question of, “How does the number of lone pairs affect the shape of the molecule?” Answering this question served to cement in those participating in the lab an understanding of the affect a central atom’s number of lone pairs will have on the shape of the molecule, and be able to identify a pattern of molecular shapes and their central atom’s lone pairs. We conducted this lab by first experimenting with 3-D molecular structures on a website, becoming familiar with the geometry of molecules and what exactly lone pairs were.

Atoms are the basic building blocks for everything we see in our lives today. Atoms combine, share, lose and gain electrons to become molecules. A molecule is a group of two or more atoms that are held and formed together by chemical bonds. Covalent bonds happens when there is both a strong enough attraction between atoms and room for electrons in the outer energy levels of the atoms, they share electrons. This process is what forms a covalent bond.

For instance, when N2 is formed, three pairs of electrons are shared, leading to the two particles having 8 valence electrons. When KBr is formed, the two elements also have 8 valence electrons. Furthermore, electrons in ionic bonds and covalent bonds are fixed, however, in metallic bonds, they are delocalized, which means electrons are able to flow freely. In the lattice of NaCl, electrons are restricted in specific space and it’s the same with oxygen compared with electrons in iron which are

Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have enough of or too much of one ingredient , which would be defined as limiting and excess reagent, respectively.

Atoms of chlorine bond together through covalent bonding, a process which involves ‘sharing’ the electrons found on the outer shells. All atoms ‘want’ to have a full outer shell so when two chlorine atoms bond together they both share one of their own electrons on their outer shell. By doing this, the shared electron effectively becomes the eighth electron on the other’s shell. By filling each other’s shell with a shared electron they form a stable structure, which in this case, is a molecule of chlorine. Consequently, chlorine has a simple molecular structure.

Then there are two letters which is the element symbol in the middle of the box, usually the element name is under the two letters. I need the very bottom of the box is the mass number, the mass number is the number of protons and neutrons in nucleus. Every element in the top row besides the hydrogen and helium element, has one orbital for its electrons. then the second row two orbitals, and the third row has three orbitals, and so on and so forth. There are only 7 rows and there is a maximum of 7 orbitals.

In atomic physics and quantum chemistry, the electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular

Here, Pauling's electronegativity conception was mostly useful; the degree of ionicity of the bond is anticipated by the electronegativity deviation between a pair of atoms Pauling's resonance theory proposed that some molecules "resonate" between different structures, rather than holding a single fixed structure He expressed that when the haemoglobin molecule gains or loses an