Results for "cobalt"

Cobalt-60 Calculation Factors

Preparation of Ammine Complexes of Cobalt(III)

Synthesis and Analysis of a Cobalt Amine Halide Complex

Dependant/ independent variables Independent- The variable being manipulated Dependant- The observed result of the independent variable being manipulated 3 Domains Prokaryotes, Eukaryotes, Archae 3 Types of Relationships Commensalism Parasitism Mutualism Scientific Hypothesis an idea that proposes a tentative explanation about a phenomenon or a narrow set of phenomena observed in the natural world. Difference between Archea/ Bacteria Archaea consists of three RNA whereas bacteria consists of single RNA. Quantitative/ Qualitative data Quantitative data is numbers-based, countable, or measurable Qualitative data is interpretation-based, descriptive, and related to language. Homeostasis Balance of the body Controlled Experiment In a controlled experiment, all extraneous variables are held constant so that they can't influence the results. Difference between Hydrophobic/ Hydrophilic Any substance that repels water Any substance that has an affinity for water Protons/ electrons/ neutron Protons- a subatomic particle with a positive electric charge Electrons- a negatively charged subatomic particle that can be either bound to an atom or free (not bound). Neutron- an uncharged atomic particle that has a mass nearly equal to that of the proton and is present in all known atomic nuclei except the hydrogen nucleus What a cation/ Anion Cations are ions that are positively charged. Anions are ions that are negatively charged. Isomers Chemical compounds that have identical chemical formulae but differ in properties and the arrangement of atoms in the molecule Picture of elements/ what's on valence electrons Valence electrons have negatively charged particles How many valence electrons are in shells 8 electrons What are examples of trace elements? zinc (Zn), copper (Cu), selenium (Se), chromium (Cr), cobalt (Co), iodine (I), manganese (Mn), and molybdenum (Mo). Different types of Bonds Covalent Bonds- one or more electrons shared between atoms Non-polar covalent: electrons are shared equally between nuclei Polar covalent- electrons shared equally between the nuclei Ionic Bonds- one or more electrons transformed from one to another Hydrogen Bonds- a weak bond between a partially positive hydrogen atom and a partially negative oxygen atom Cohesion/ Adhesion Cohesion- the attraction of molecules for other molecules of the same kind Adhesion- the sticking of molecules or surfaces to each other Radioactive Isotopes, Why are they used Radioisotopes are an essential part of medical diagnostic procedures. In combination with imaging devices that register the gamma rays emitted from within, they can be used for imaging to study the dynamic processes taking place in various parts of the body. Why is Water Important Water's role as a solvent helps cells transport and use substances like oxygen or nutrients. Properties of Water Water is polar Water is a solvent Water is less dense as a solid than a liquid What are reactions a process that converts one or more substances to another substance. .Why are trace elements important? function primarily as catalysts in enzyme systems What are Buffers Substances in the cells that help maintain a relatively stable pH What is the pH scale? a measure of how acidic/basic water is Find the molecular mass of something Atomic weight on the periodic table is equal to moles #/1m = x/ desired # moles Functional groups The shape of molecules directly affects their function Types of atoms, bonds A specific arrangement of atoms Difference between Hydraullisis/ Dehydration Dehydration- removes a water molecule from a new bond Hydrolysis- add a water molecule, breaking a bond Differentiate between Polymers/ Monomers A monomer is a molecule with low molecular weight that can combine with others of the same kind to form a chemical compound known as a polymer Different types of Proteins/ enzymes antibodies, contractile proteins, enzymes, hormonal proteins, structural proteins, storage proteins, and transport proteins Difference between plants and animals Plants are not mobile and animals are Cell membrane components Phospholipids, cholesterol, glycolipids, lipid bilayer, membrane proteins

Reactions of Transition Metal Complexes

cobalt

% cobalt

Ch 2 Chemical Compounds and Bondings Chemical bond: force of attraction between 2 atoms or 2 ions. There are 2 main types of chemical bonds: 1. Ionic bond: a bond between a metallic atom (metal) and a non-metallic atom (non-metal) in which there is a complete transfer of electrons from the metal to the non-metal. The compound which is formed is called an ionic compound. Ex.: NaCl , MgCl2, Al2O3 To write the formula of an ionic compound we use the criss-cross method (we down cross multiply the charges without the sign, only the numbers of the charges) Remark: if the charges are the same then they cancel each other in the formula so there will be one atom of the metal and one atom of the non-metal in the compound. Exercise: Write the formula of the compound which is formed between the following elements, and name each compound. a) Rb and S: b) Ca and Se: c) Al and Br: d) Na and N: - Draw a Bohr diagram to show the transfer of electrons (loss / gain) in an ionic compound. Example: Na2O (sodium oxide) Remark: The ionic bond is also described as an electrostatic force of attraction between a positive ion and a negative ion (eg: Na+ Cl- ). 2. Covalent bond: a bond between a non-metal and another non-metal in which there is a sharing of electrons between the non-metallic atoms. The compound that is formed is called a covalent or molecular compound. Molecule: 2 or more atoms (non-metallic) bonded together; the atoms can be of the same element such as O2 or of different elements such as HCl, CH4, H2O,….. We show the sharing of electrons between non-metallic atoms by using the Lewis diagram. In addition we can make intersecting circles for the atoms to show the sharing. Reminder: Lewis diagram of an atom shows only the valence electrons of that atom. Most of the atoms follow the octet rule (there are very few exceptions), that is each atom will have eight electrons in the valence shell (same as noble gases) except hydrogen will have 2 electrons after sharing (same as helium). Remark: 2 electrons that are not bonded to any other atom is called a lone pair (non-bonding pair) of electrons. Exercise: Draw lewis diagrams to show the sharing of electrons in each of the following compounds: 1. NF3 2. CH4 3. CO2 4. CCl4 5. CH2O Remark:In drawing Lewis structure, we show the bonds between the atoms and we also show all lone pairs (if present) on any atom. - Naming molecular compounds: 1: mono 2: di 3: tri 4: tetra 5: penta 6: hexa 7: hepta 8: octa 9: nona 10:deca Example: PCl5 : phosphorus pentachloride Remark: If the first element contains only one atom we don’t write mono before it; If the second element contains only one atom we have to write mono before it. Ex.: NO : nitrogen monoxide CO: carbon monoxide Exercise: Fill in the table below Name Chemical Formula diphosphorus pentoxide SO3 CO Aluminum sulfide Al2S3 SF6 Calcium oxide Lithium nitride Li3N Remark: If the compound contains a transition metal, then we have to mention the type of charge of the transition metal by inserting a roman numeral in brackets (I, II, III, IV ….) after the symbol of the transition metal. Example: Name the following compounds: - FeCl2 : Iron (II) chloride - Cu(NO3)2 : Copper (II) nitrate Remark: There are few transition metals that have only one type of charge such as zinc, nickel, and silver; in this case no roman numeral is required. Zinc : Zn+2 Silver: Ag+ Nickel: Ni+2 - ZnSO4 : zinc sulfate - AgNO3 : silver nitrate - CuSO4 : copper (II) sulfate - Co(NO3)3 : cobalt (III) nitrate Exercise: Write the formula of the following compounds. Calcium phosphate: Iron(III) hydroxide: Sodium hydroxide: Manganese(II) hydroxide: Barium sulfate: Zinc carbonate: Ammonium nitrate: Remark: We must enclose the polyatomic ion in brackets if the number after it is more than 1. Note: If the polyatomic ion that ends with the prefix –ate decreases by one oxygen atom then the prefix changes to -ite. If the prefix ending with – ite decreases by one oxygen atom then we precede the prefix by hypo, whereas if the prefix ending with – ate increases by one oxygen atom then we precede the prefix by per. Example: ClO3- is called chlorate; if we reduce one oxygen atom then the ion becomes ClO2- and is called chlorite, however if we increase by one oxygen atom then the ion becomes ClO4- and is called perchlorate; and if the chlorite is reduced by one oxygen atom then the ion becomes ClO- and is called hypochlorite. Exercise: Name the following compounds: K2SO3 : NaNO2 : Mg(ClO4)2 : LiBrO2 : - Comparison Table between ionic and covalent (molecular) compounds: property Ionic Compounds Covalent Compounds State (at room temperature) solids Solids, liquids or gases Melting point and boiling point Very high Usually low Involvement of electrons Loss and gain (transfer) of electrons Sharing of electrons Electric conductivity When dissolved in water (in solution) , electric conductivity is high

Cobalt mining

Section 1 Part 2: MV intro and Cobalt

Cobalt Essay Exam

Topic 2 - Cobalt-60 Therapy & Brachytherapy

Zn, Mn, Cobalt, iodine deficiency

cobalt coordination chemistry

Pre-lab 4 : Cobalt(II) Complexes & Le Chatlier’s Principle

Lab 11: Chrome cobalt clasp design

Lecture 6 - COBALT and analogy learning

PART 1: Iron, Zinc, Iodine, Copper, Cobalt, Fluorine, Selenium, Manganese, Sulfur

Geography - Cobalt Business Park

Al Aluminum  Ar Argon AsArsenic Ba Barium Be Beryllium Bi Bismuth B Boron Br Bromine Cd Cadmium Ca Calcium C Carbon Cs Cesium Cl Chlorine Cr Chromium Co Cobalt Cu Copper F Fluorine Au Gold He Helium H Hydrogen I Iodine Fe Iron Pb Lead Li Lithium Zn Zinc U Uranium Sn Tin Te Tellurium S Sulfur Sr Strontium Na Sodium Ag Silver Si Silicon Se Selenium Rb Rubidium Rn Radon K Potassium pu Plutonium Ra Radium Pt Platinum P Phosphorus O Oxygen N Nitrogen Ni Nickel Ne Neon Hg Mercury Mn Manganese Mg Magnesium