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1 - shawnschmitt
... 20. What is the element with the largest atomic radius? smallest? largest = Fr, Smallest = F 21. When an electron in the excited state drops from n=4 to n=2, what color is the photon given off? blue light 22. How does an atom form a positive ion with a 3+ charge? anion with a 2- (two negative) charg ...
... 20. What is the element with the largest atomic radius? smallest? largest = Fr, Smallest = F 21. When an electron in the excited state drops from n=4 to n=2, what color is the photon given off? blue light 22. How does an atom form a positive ion with a 3+ charge? anion with a 2- (two negative) charg ...
Packet
... _____ 56. Equation obey the laws of conservation of mass if they’ve been properly ___. _____ 57. A solid product. _____ 58. A number within a formula representing the number of atoms of each element present in the formula. _____ 59. A solid compound dissolved in water. _____ 60. Elements that do not ...
... _____ 56. Equation obey the laws of conservation of mass if they’ve been properly ___. _____ 57. A solid product. _____ 58. A number within a formula representing the number of atoms of each element present in the formula. _____ 59. A solid compound dissolved in water. _____ 60. Elements that do not ...
Inorganic Chemistry 412 / 512
... Briefly describe the structure of black phosphorous (you do not need to sketch). [6 pts] Essentially this is the graphite structure, with non-planar sheets. P atoms form 6membered rings with chair-type conformations, each P has 3 single bonds within the sheet. There are no covalent interactions betw ...
... Briefly describe the structure of black phosphorous (you do not need to sketch). [6 pts] Essentially this is the graphite structure, with non-planar sheets. P atoms form 6membered rings with chair-type conformations, each P has 3 single bonds within the sheet. There are no covalent interactions betw ...
Chemistry: The Nature of Matter
... o 2nd shell has a little more energy and holds 8 electrons o 3rd shell has even more energy, etc. ____________________________________________________________ ____________________________________________________________ ____________________________________________________________ Electron config ...
... o 2nd shell has a little more energy and holds 8 electrons o 3rd shell has even more energy, etc. ____________________________________________________________ ____________________________________________________________ ____________________________________________________________ Electron config ...
CHM 101
... Bohr developed a model of the atom that looks like our planetary system. Explain what the model is and how he arrived at this design. ...
... Bohr developed a model of the atom that looks like our planetary system. Explain what the model is and how he arrived at this design. ...
6.1 Organizing the Periodic Table
... with more than one type of atom the electrons may not be shared equally • In general, elements on the right of the periodic table and at the top of groups have a greater attraction for electrons ...
... with more than one type of atom the electrons may not be shared equally • In general, elements on the right of the periodic table and at the top of groups have a greater attraction for electrons ...
Types of Chemical Reactions
... what type and how many reactants are present. We can use a generalized equation to represent each. In the generalized equation, the letters A and B represent positive ions (elements that lose electrons). The letters X and Y will represent negative ions (elements that gain electrons). In a synthesis ...
... what type and how many reactants are present. We can use a generalized equation to represent each. In the generalized equation, the letters A and B represent positive ions (elements that lose electrons). The letters X and Y will represent negative ions (elements that gain electrons). In a synthesis ...
Pre-AP Chemistry - Simple Rules for Electron Exchange Simple
... species loses and which species gains electrons. You will note that oxidation numbers (or “oxidation states” for groups of like atoms) are similar, but not identical to, formal ionic charges. Rule #1: The oxidation number for a pure or uncombined element is always 0. Rule #2: The oxidation state for ...
... species loses and which species gains electrons. You will note that oxidation numbers (or “oxidation states” for groups of like atoms) are similar, but not identical to, formal ionic charges. Rule #1: The oxidation number for a pure or uncombined element is always 0. Rule #2: The oxidation state for ...
Define:
... 86. Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant? 87. Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass numbe ...
... 86. Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant? 87. Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass numbe ...
Soluble salts
... 5.1 Exchange Reactions: Precipitation and Net Ionic Equations (p. 165) An __________________ is a compound whose aqueous solution conducts electricity. ____________ electrolytes are solutes that exist in solution predominantly in the form of hydrated (solvated) ions. A good example is sodium chlorid ...
... 5.1 Exchange Reactions: Precipitation and Net Ionic Equations (p. 165) An __________________ is a compound whose aqueous solution conducts electricity. ____________ electrolytes are solutes that exist in solution predominantly in the form of hydrated (solvated) ions. A good example is sodium chlorid ...
Solution
... 12.) Consider the unbalanced redox reaction below: Cr2O72- + I2 → Cr3+ + IO4What is the number of electrons transferred in the balanced equation under aqueous acidic conditions? A) 14 B) 17 C) 42 D) 4 E) 6 13.) Which of the following statements are true? A) pH of 0.01 M HCl > pH of 0.01 M KOH B) pH ...
... 12.) Consider the unbalanced redox reaction below: Cr2O72- + I2 → Cr3+ + IO4What is the number of electrons transferred in the balanced equation under aqueous acidic conditions? A) 14 B) 17 C) 42 D) 4 E) 6 13.) Which of the following statements are true? A) pH of 0.01 M HCl > pH of 0.01 M KOH B) pH ...
Chemical reaction
... • Contain carbon atoms that are covalently bonded to other carbon atoms and to other elements : Typically hydrogen (H), nitrogen (N) and oxygen (O) ...
... • Contain carbon atoms that are covalently bonded to other carbon atoms and to other elements : Typically hydrogen (H), nitrogen (N) and oxygen (O) ...
9.2 Oxidation Numbers
... reading a chemical equation does not always tell us whether oxidation and reduction have occurred, so chemists have developed a numerical system to help identify a reaction as redox. For redox reactions, this system also shows us which element is oxidized, which is reduced, what the oxidizing agent ...
... reading a chemical equation does not always tell us whether oxidation and reduction have occurred, so chemists have developed a numerical system to help identify a reaction as redox. For redox reactions, this system also shows us which element is oxidized, which is reduced, what the oxidizing agent ...
Chemical reactions
... interact with the ions of another compound forming – A solid precipitate – A gas ...
... interact with the ions of another compound forming – A solid precipitate – A gas ...
Introduction to Chemistry
... Ionic- Two elements bond by transferring electrons to create ions that attract together (+ is attracted to - after an electron is transferred) ...
... Ionic- Two elements bond by transferring electrons to create ions that attract together (+ is attracted to - after an electron is transferred) ...
FINAL EXAM Review Sheet / Study Guide Honors Chemistry
... 2) Explain the difference between dissociation and dissolving. Use an example compound for each. ...
... 2) Explain the difference between dissociation and dissolving. Use an example compound for each. ...
2.4 Chemical Reactions and Enzymes
... Chemical reactions that release energy often occur on their own, or spontaneously. ...
... Chemical reactions that release energy often occur on their own, or spontaneously. ...
1. I can define valence electron and use the periodic
... 20. Determine if the follow molecules are held together by covalent or ionic bonds. a. H2O d. PO4 g. SO2 b. CO2 e. Mg Br2 h. KCl c. NaCl f. CaCO3 #6. I can identify how many atoms are in a compound by looking at its molecular formula. 21. List how many of each atom is present in each of the followin ...
... 20. Determine if the follow molecules are held together by covalent or ionic bonds. a. H2O d. PO4 g. SO2 b. CO2 e. Mg Br2 h. KCl c. NaCl f. CaCO3 #6. I can identify how many atoms are in a compound by looking at its molecular formula. 21. List how many of each atom is present in each of the followin ...
Earth`s Chemistry
... tightly together in fixed positions Solids have definite shape & volume Liquids = have definite volume but not shape Liquids take the shape of the container Particles tightly packed, but move freely in relation to each other Gases = No definite shape or volume ...
... tightly together in fixed positions Solids have definite shape & volume Liquids = have definite volume but not shape Liquids take the shape of the container Particles tightly packed, but move freely in relation to each other Gases = No definite shape or volume ...
Aqueous Reactions
... became ions. This is the result of a transfer of electrons. In the above reaction, an electron is transferred from a sodium atom to a chlorine atom. The sodium atoms now have ten electrons, instead of eleven. This means that the sodium has one more proton than electron and has a charge of +1. The c ...
... became ions. This is the result of a transfer of electrons. In the above reaction, an electron is transferred from a sodium atom to a chlorine atom. The sodium atoms now have ten electrons, instead of eleven. This means that the sodium has one more proton than electron and has a charge of +1. The c ...
Answer Key - La Quinta High School
... Answer Key Chapter 7: Standard Review Worksheet 1. All chemical reactions do produce some evidence that the reaction has occurred, but sometimes this evidence may not be visual and may not be very obvious. For example, when very dilute aqueous solutions of acids and bases are mixed, the neutralizati ...
... Answer Key Chapter 7: Standard Review Worksheet 1. All chemical reactions do produce some evidence that the reaction has occurred, but sometimes this evidence may not be visual and may not be very obvious. For example, when very dilute aqueous solutions of acids and bases are mixed, the neutralizati ...
2 - CronScience
... can predict the products if it is a binary compound (which means it is made up of only two elements) –It breaks apart into the elements: ...
... can predict the products if it is a binary compound (which means it is made up of only two elements) –It breaks apart into the elements: ...
Redox
![](https://commons.wikimedia.org/wiki/Special:FilePath/NaF.gif?width=300)
Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species. The term ""redox"" comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.Although oxidation reactions are commonly associated with the formation of oxides from oxygen molecules, these are only specific examples of a more general concept of reactions involving electron transfer.Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid–base reactions. Like acid–base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. The oxidation state of an atom is the fictitious charge that an atom would have if all bonds between atoms of different elements were 100% ionic. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as ""redox"" even though no electron transfer occurs (such as those involving covalent bonds).There are simple redox processes, such as the oxidation of carbon to yield carbon dioxide (CO2) or the reduction of carbon by hydrogen to yield methane (CH4), and more complex processes such as the oxidation of glucose (C6H12O6) in the human body through a series of complex electron transfer processes.