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2015 Academic Challenge CHEMISTRY TEST – STATE
... E. All of these solutions have the same concentration of chloride ions. ...
... E. All of these solutions have the same concentration of chloride ions. ...
Chapter 4: Introduction to Earth Chemistry Section 1 Notes
... Elements rarely occur ____________ in Earth’s crust. They generally occur ____________ with other elements. compound a __________________________________________________________________________ The properties of a compound differ from the properties of the __________ that make up the compound. _____ ...
... Elements rarely occur ____________ in Earth’s crust. They generally occur ____________ with other elements. compound a __________________________________________________________________________ The properties of a compound differ from the properties of the __________ that make up the compound. _____ ...
lesson 5
... 9. How many minus charges does each fluorine atom gain? 10. How many minus charges does each fluorine atom now have? ...
... 9. How many minus charges does each fluorine atom gain? 10. How many minus charges does each fluorine atom now have? ...
halogen compounds organic chemistry
... (FeCl3, FeBr3, AlCl3) in the dark, at ordinary temperatures (310-320 K). The Lewis acid acts as a catalyst or a halogen carrier, as its function is to carry the chlorine to the aromatic hydrocarbon. In actual practice, iron filings in the presence of chlorine commonly used. The chlorine reacts with ...
... (FeCl3, FeBr3, AlCl3) in the dark, at ordinary temperatures (310-320 K). The Lewis acid acts as a catalyst or a halogen carrier, as its function is to carry the chlorine to the aromatic hydrocarbon. In actual practice, iron filings in the presence of chlorine commonly used. The chlorine reacts with ...
1 Q. If ΔrH is positive, what can you say about the reaction? 2 Q If
... How much heat would be released when 88 g of CO2 is produced? Where do we commonly see this reaction used? ...
... How much heat would be released when 88 g of CO2 is produced? Where do we commonly see this reaction used? ...
CHEMICAL EQUATIONS NAME PERIOD_______ DATE________
... reaction. In a chemical equation, the substances on the left side of the arrow are the starting substances. These substances are called ______________. The substances on the right side of the arrow are the substances that result from the reaction. These substances are called ____________________. Th ...
... reaction. In a chemical equation, the substances on the left side of the arrow are the starting substances. These substances are called ______________. The substances on the right side of the arrow are the substances that result from the reaction. These substances are called ____________________. Th ...
Lecture 24 (Slides) October 18
... • 1. Which of the following atoms and ions are paramagnetic (i.e. have unpaired electrons). Note: An even number of electrons does not indicate that all electrons are paired. (a) He atom, (b) F atom, (c) As atom, (d) F- ion (e) Al3+ ion and (f) Fe atom. • 2. Arrange the following in order of increas ...
... • 1. Which of the following atoms and ions are paramagnetic (i.e. have unpaired electrons). Note: An even number of electrons does not indicate that all electrons are paired. (a) He atom, (b) F atom, (c) As atom, (d) F- ion (e) Al3+ ion and (f) Fe atom. • 2. Arrange the following in order of increas ...
Microsoft Word
... Covalent Bonding Elements which are neither highly electropositive nor highly electronegative are less likely to form ionic compounds. Consider CH4, methane; carbon and hydrogen have similar electronegativities. It would be inappropriate to describe the bonds between carbon and hydrogen in methane a ...
... Covalent Bonding Elements which are neither highly electropositive nor highly electronegative are less likely to form ionic compounds. Consider CH4, methane; carbon and hydrogen have similar electronegativities. It would be inappropriate to describe the bonds between carbon and hydrogen in methane a ...
Chemistry I Honors – Semester Exam Review – Fall 2000
... d. fixed volume, low KE, particles can move past each other. 7. Compare and contrast a solution, colloid, and suspension. 8. Classify the following as element, compound, heterogeneous mixture, or solution. a. graphite (carbon) b. grape juice c. table salt (NaCl) d. pepper ...
... d. fixed volume, low KE, particles can move past each other. 7. Compare and contrast a solution, colloid, and suspension. 8. Classify the following as element, compound, heterogeneous mixture, or solution. a. graphite (carbon) b. grape juice c. table salt (NaCl) d. pepper ...
stoichiometry - J. Seguin Science
... A can of butane lighter fluid contains 1.20 moles of butane calculate the number of moles of carbon dioxide given off when this butane is burned. ...
... A can of butane lighter fluid contains 1.20 moles of butane calculate the number of moles of carbon dioxide given off when this butane is burned. ...
Second Semester Final Review Guide
... 2. When more energy is released than absorbed, the reaction is (exothermic / endothermic). circle one 3. When more energy is absorbed than released, the reaction is (exothermic / endothermic). circle one 4. The energy of an endothermic reaction would be located on the (Left / Right) circle one side ...
... 2. When more energy is released than absorbed, the reaction is (exothermic / endothermic). circle one 3. When more energy is absorbed than released, the reaction is (exothermic / endothermic). circle one 4. The energy of an endothermic reaction would be located on the (Left / Right) circle one side ...
Methane - ARZELORIVAS IS
... Chloroform (CHCl3) and carbon tetrachloride (CCl4) react with hydrogen fluoride to form a mixture of chlorofluorocarbons, such as CHCl2F, CHClF2, CCl3F, CCl2F2, and CClF3, which are sold under trade names such as Freon and Genetron. The freons are inert gases with high densities, low boiling points, ...
... Chloroform (CHCl3) and carbon tetrachloride (CCl4) react with hydrogen fluoride to form a mixture of chlorofluorocarbons, such as CHCl2F, CHClF2, CCl3F, CCl2F2, and CClF3, which are sold under trade names such as Freon and Genetron. The freons are inert gases with high densities, low boiling points, ...
34.) Write out the set of four quantum numbers for the last electron
... * Tell predominant type of bonding in the following compounds (ionic, covalent, both): 53.) CO2 54.) Na2SO4 55.) MgBr2 56.) Ag2CO3 * Define and tell what types of substances exhibit these intermolecular forces: 57.) Hydrogen bonding 58.) Dipole-dipole 59.) London dispersion Unit 7 * Write formulas f ...
... * Tell predominant type of bonding in the following compounds (ionic, covalent, both): 53.) CO2 54.) Na2SO4 55.) MgBr2 56.) Ag2CO3 * Define and tell what types of substances exhibit these intermolecular forces: 57.) Hydrogen bonding 58.) Dipole-dipole 59.) London dispersion Unit 7 * Write formulas f ...
Determining Density through graphing
... In the first week, she studied daily for 15 minutes and her end of the week test scores were 60%. During the second week, she studied daily for 30 minutes and her end of the week test scores were 70%. During the third week, she studied for 45 minutes and her end of the week test scores were 80%. Fin ...
... In the first week, she studied daily for 15 minutes and her end of the week test scores were 60%. During the second week, she studied daily for 30 minutes and her end of the week test scores were 70%. During the third week, she studied for 45 minutes and her end of the week test scores were 80%. Fin ...
Semester Exam Review - Teach-n-Learn-Chem
... d. fixed volume, low KE, particles can move past each other. 7. Compare and contrast a solution, colloid, and suspension. 8. Classify the following as element, compound, heterogeneous mixture, or solution. a. graphite (carbon) b. grape juice c. table salt (NaCl) d. pepper ...
... d. fixed volume, low KE, particles can move past each other. 7. Compare and contrast a solution, colloid, and suspension. 8. Classify the following as element, compound, heterogeneous mixture, or solution. a. graphite (carbon) b. grape juice c. table salt (NaCl) d. pepper ...
Determining Density through graphing
... In the first week, she studied daily for 15 minutes and her end of the week test scores were 60%. During the second week, she studied daily for 30 minutes and her end of the week test scores were 70%. During the third week, she studied for 45 minutes and her end of the week test scores were 80%. Fin ...
... In the first week, she studied daily for 15 minutes and her end of the week test scores were 60%. During the second week, she studied daily for 30 minutes and her end of the week test scores were 70%. During the third week, she studied for 45 minutes and her end of the week test scores were 80%. Fin ...
Chapter 4 Student Notes
... Oxidation numbers (or oxidation states) help up keep track of electrons during chemical reactions. Oxidation numbers are assigned to atoms using specific rules: 1. For an atom in its elemental form, the oxidation number is always zero. 2. For any monatomic ion, the oxidation number equals the charge ...
... Oxidation numbers (or oxidation states) help up keep track of electrons during chemical reactions. Oxidation numbers are assigned to atoms using specific rules: 1. For an atom in its elemental form, the oxidation number is always zero. 2. For any monatomic ion, the oxidation number equals the charge ...
CHM 130 Final Exam Review Chapter 1 Scientific method Theory
... Naming covalent compounds Names of common acids Chapter 8 Writing chemical reactions from words Balancing chemical reactions Classifying chemical reactions o Combination o Decomposition o Combustion o Single replacement o Double replacement o Acid base neutralization Activity series Solubility rules ...
... Naming covalent compounds Names of common acids Chapter 8 Writing chemical reactions from words Balancing chemical reactions Classifying chemical reactions o Combination o Decomposition o Combustion o Single replacement o Double replacement o Acid base neutralization Activity series Solubility rules ...
CHM 130 Final Exam Review
... Polar vs nonpolar covalent bonds Metallic bonds Polar vs nonpolar molecules ...
... Polar vs nonpolar covalent bonds Metallic bonds Polar vs nonpolar molecules ...
Chem 1100 Chapter Three Study Guide Outline I. Molar Mass and
... a. SrH2 b. SrOH2 c. SrOH d. Sr(OH)2 22. What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest whole-number coefficients? _____ C3H8O (l) + _____ O2 (g) Æ ____ CO2 (g) + ____ H2O (l) a. 7 b. 9 c. 3 d. 5 23. What is the molar mass of aspartic acid, ...
... a. SrH2 b. SrOH2 c. SrOH d. Sr(OH)2 22. What is the stoichiometric coefficient for oxygen when the following equation is balanced using the lowest whole-number coefficients? _____ C3H8O (l) + _____ O2 (g) Æ ____ CO2 (g) + ____ H2O (l) a. 7 b. 9 c. 3 d. 5 23. What is the molar mass of aspartic acid, ...
Chemistry I Honors – Semester Exam Review – Fall 2000
... d. fixed volume, low KE, particles can move past each other. 7. Compare and contrast a solution, colloid, and suspension. 8. Classify the following as element, compound, heterogeneous mixture, or solution. a. graphite (carbon) b. grape juice c. table salt (NaCl) d. pepper ...
... d. fixed volume, low KE, particles can move past each other. 7. Compare and contrast a solution, colloid, and suspension. 8. Classify the following as element, compound, heterogeneous mixture, or solution. a. graphite (carbon) b. grape juice c. table salt (NaCl) d. pepper ...
SUMMER WORK AP Chemistry
... By examining these numbers, propose a relationship between the ground-state energy of hydrogen-like systems and the nuclear charge, Z. (c) Use the relationship you derive in part (b) to predict the ground-state energy of the C5+ ion. 18. Write the Lewis symbol for atoms of each of the following elem ...
... By examining these numbers, propose a relationship between the ground-state energy of hydrogen-like systems and the nuclear charge, Z. (c) Use the relationship you derive in part (b) to predict the ground-state energy of the C5+ ion. 18. Write the Lewis symbol for atoms of each of the following elem ...
4.1 PPT- Atomic Theory and Bonding
... Atoms gain and lose electrons in an attempt to be STABLE. The noble gases are stable because they have FULL outer shells of electrons. They don’t need to lose or gain any e-s. Atoms in each period want to have the same number of electrons in their outer shell (VALENCE ELECTRONS) as the noble gases ...
... Atoms gain and lose electrons in an attempt to be STABLE. The noble gases are stable because they have FULL outer shells of electrons. They don’t need to lose or gain any e-s. Atoms in each period want to have the same number of electrons in their outer shell (VALENCE ELECTRONS) as the noble gases ...
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.