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REACTION PREDICTION
... Reactants Products The arrow means “yields” or “produces” (s) = solid (g)= gas (l)= liquid (aq)= aqueous (dissolved in water) or = reversible reaction ...
... Reactants Products The arrow means “yields” or “produces” (s) = solid (g)= gas (l)= liquid (aq)= aqueous (dissolved in water) or = reversible reaction ...
TYPES OF SOLUTION CHEMICAL REACTIONS
... a. endpoint- the point (volume of standard) at which the unknown changes color b. equivalence point--# moles of standard solution = # moles of unknown solution. c. standardize- titration the unknown solution with the standard of known concentration. Exercise 14 A student carries out an experiment to ...
... a. endpoint- the point (volume of standard) at which the unknown changes color b. equivalence point--# moles of standard solution = # moles of unknown solution. c. standardize- titration the unknown solution with the standard of known concentration. Exercise 14 A student carries out an experiment to ...
CHEM_S1CourseReview_2011
... What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What rules must be obeyed to safely conduct an experiment? Why are significant figures important to chemists? What is the best method/graph to represent specific data? How ...
... What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What rules must be obeyed to safely conduct an experiment? Why are significant figures important to chemists? What is the best method/graph to represent specific data? How ...
Unit 4 - Calculations and Chemical Reactions
... reaction reactants (starting materials) are converted into products. Consider the reaction in which magnesium oxide reacts with carbon dioxide to form magnesium carbonate. We can represent the above “word description” by a “chemical equation”. Chemical equation: MgO + CO2 → MgCO3 Reactants Product W ...
... reaction reactants (starting materials) are converted into products. Consider the reaction in which magnesium oxide reacts with carbon dioxide to form magnesium carbonate. We can represent the above “word description” by a “chemical equation”. Chemical equation: MgO + CO2 → MgCO3 Reactants Product W ...
Chemical Reactions
... 1. Begin with atoms that appear in only one compound on the left and only one compound on the right. In the equation for the reaction of propane and oxygen, begin with either carbon or hydrogen 2. If an atom occurs as a free element—as for example, as Mg, Na, O2, or H2—balance this element last. 3. ...
... 1. Begin with atoms that appear in only one compound on the left and only one compound on the right. In the equation for the reaction of propane and oxygen, begin with either carbon or hydrogen 2. If an atom occurs as a free element—as for example, as Mg, Na, O2, or H2—balance this element last. 3. ...
Review for Final Exam - Short Answer and Problems
... A 28.2 g sample of a metal is heated to 95.2˚C and dropped in a calorimeter which contains 100.0 g of water at 25˚C. The final temperature in the calorimeter is 31.0˚C. Assuming no heat is lost to the surroundings or the calorimeter, calculate the specific heat of the metal. The specific heat of H2O ...
... A 28.2 g sample of a metal is heated to 95.2˚C and dropped in a calorimeter which contains 100.0 g of water at 25˚C. The final temperature in the calorimeter is 31.0˚C. Assuming no heat is lost to the surroundings or the calorimeter, calculate the specific heat of the metal. The specific heat of H2O ...
HW / Unit 2
... 5. Why do the elements show a decrease in size as one proceeds across a period? Why do the elements show an increase in size as one proceeds down a group? 6. Place the following atoms in order of increasing size: S, Rb, K, C, O, Al, P 7. What happens to the size of an atom when it loses an electron? ...
... 5. Why do the elements show a decrease in size as one proceeds across a period? Why do the elements show an increase in size as one proceeds down a group? 6. Place the following atoms in order of increasing size: S, Rb, K, C, O, Al, P 7. What happens to the size of an atom when it loses an electron? ...
key to sample questions test 2
... 2Na3PO4(aq) + 3 CaCl2(aq) 6 NaCl(aq) + Ca3(PO4)2(s) 2 PO4(aq) + 3 Ca(aq) Ca3(PO4)2(s) PO4(aq) + Ca(aq) CaPO4(s) 6 Na(aq) + 2PO4(aq) + 3Ca(aq) +6 Cl(aq) 6 Na(aq) + 6 Cl(aq) + Ca3(PO4)2(s) u. Which one of the following is an acid base reaction? 2 HCl + Mg H2 + MgCl2 HCl + KOH ...
... 2Na3PO4(aq) + 3 CaCl2(aq) 6 NaCl(aq) + Ca3(PO4)2(s) 2 PO4(aq) + 3 Ca(aq) Ca3(PO4)2(s) PO4(aq) + Ca(aq) CaPO4(s) 6 Na(aq) + 2PO4(aq) + 3Ca(aq) +6 Cl(aq) 6 Na(aq) + 6 Cl(aq) + Ca3(PO4)2(s) u. Which one of the following is an acid base reaction? 2 HCl + Mg H2 + MgCl2 HCl + KOH ...
Chapter 14…Kinetic Theory
... Arrhenius Theory Bronsted-Lowry Theory Lewis Theory Name the following: 15. HC2H3O2: 16. HF: 17. H2SO3: ...
... Arrhenius Theory Bronsted-Lowry Theory Lewis Theory Name the following: 15. HC2H3O2: 16. HF: 17. H2SO3: ...
Word and Skeleton Equations Practice (ws Fall 2010)
... 2. Solid sodium metal reacts with liquid water to form an aqueous solution of sodium hydroxide and hydrogen gas. 3. Solid potassium chlorate breaks down to form solid potassium chloride and oxygen gas. 4. Solid copper reacts with oxygen gas to form solid copper(II) oxide. 5. When aqueous solutions o ...
... 2. Solid sodium metal reacts with liquid water to form an aqueous solution of sodium hydroxide and hydrogen gas. 3. Solid potassium chlorate breaks down to form solid potassium chloride and oxygen gas. 4. Solid copper reacts with oxygen gas to form solid copper(II) oxide. 5. When aqueous solutions o ...
Chemical Reactions
... Fe + O2 → Fe2O3 How do you get Fe2 from Fe and O3 from O2? We do this by balancing equations. 4Fe + 3O2 → 2Fe2O3 You cannot make or destroy matter! It also helps to know if it is solid, liquid or gas. 4Fe(s) + 3O2(g)→ 2Fe2O3(s) ...
... Fe + O2 → Fe2O3 How do you get Fe2 from Fe and O3 from O2? We do this by balancing equations. 4Fe + 3O2 → 2Fe2O3 You cannot make or destroy matter! It also helps to know if it is solid, liquid or gas. 4Fe(s) + 3O2(g)→ 2Fe2O3(s) ...
Midterm Practice Exam Key
... ____________ in the oxidation number signifies reduction. 3. A ____________ reaction is one in which the aqueous (dissolved) ions combine to form a solid that is not readily soluble. 4. ____________ is the addition of a known amount of solution to determine the volume (or concentration) of another ...
... ____________ in the oxidation number signifies reduction. 3. A ____________ reaction is one in which the aqueous (dissolved) ions combine to form a solid that is not readily soluble. 4. ____________ is the addition of a known amount of solution to determine the volume (or concentration) of another ...
4.IonicCompounds - Gleneaglesunit1and2chemistry2012
... – The forces between the particles are strong. – There are no free-moving electrons present, unlike in metals. – There are charged particles present, but in solid state they are not free to move. – When an ionic compound melts, however, the particles are free to move and the compound will conduct el ...
... – The forces between the particles are strong. – There are no free-moving electrons present, unlike in metals. – There are charged particles present, but in solid state they are not free to move. – When an ionic compound melts, however, the particles are free to move and the compound will conduct el ...
Click here to Ch 06.2 Covalent Bonding_Lewis Structures
... **Remember, ALL elements EXCEPT Hydrogen and Boron want eight electrons around them, total. Hydrogen only wants two electrons. Boron only gets six electrons. ...
... **Remember, ALL elements EXCEPT Hydrogen and Boron want eight electrons around them, total. Hydrogen only wants two electrons. Boron only gets six electrons. ...
2002 Final Exam for Practice - Department of Chemistry | Oregon
... and your University ID Card. You may use a basic calculator (for example, TI-25X Solar or TI-30XA) if you wish. If you have notes or electronic devices with you, place them in a sealed backpack and place the backpack OUT OF SIGHT. Or place the notes directly on the table at the front of the room. Fi ...
... and your University ID Card. You may use a basic calculator (for example, TI-25X Solar or TI-30XA) if you wish. If you have notes or electronic devices with you, place them in a sealed backpack and place the backpack OUT OF SIGHT. Or place the notes directly on the table at the front of the room. Fi ...
2 - FacultyWeb
... Hydrogen Bonds • A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom In living cells, the electronegative partners of hydrogen are usually oxygen or nitrogen atoms • Hydrogen bonds are common between dipoles su ...
... Hydrogen Bonds • A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom In living cells, the electronegative partners of hydrogen are usually oxygen or nitrogen atoms • Hydrogen bonds are common between dipoles su ...
The Oxidation States of Tin
... 0.0797 g was torn into small pieces and placed in a flask with a stir bar. This was placed onto a hot plate in a hood. While in the hood, 1 mL of concentrated HCl and one drop of 0.1 M CuSO4 was added to the solution. This solution was heated jus under boiling and a watch glass was placed over the ...
... 0.0797 g was torn into small pieces and placed in a flask with a stir bar. This was placed onto a hot plate in a hood. While in the hood, 1 mL of concentrated HCl and one drop of 0.1 M CuSO4 was added to the solution. This solution was heated jus under boiling and a watch glass was placed over the ...
7.2 Balancing Equations
... Consider again the reaction between magnesium and oxygen to produce magnesium oxide. 2Mg + O2 2MgO The balanced equation tells you that two Mg atoms react with one O2 molecule to produce two MgO molecules. The coefficients in a balanced equation also tell you the mole ratio. The mole ratio is the ...
... Consider again the reaction between magnesium and oxygen to produce magnesium oxide. 2Mg + O2 2MgO The balanced equation tells you that two Mg atoms react with one O2 molecule to produce two MgO molecules. The coefficients in a balanced equation also tell you the mole ratio. The mole ratio is the ...
Advanced Chemistry Midterm
... 19. For the diatomic molecule Cl2, how many electron(s) does each chlorine atom share with the other chlorine atom so that each has an octet? a. 1 20. In the compound ammonia, d. the Lewis structure will have one unshared pair of electrons 21. What is the name of the compound whose formula is FeSO ...
... 19. For the diatomic molecule Cl2, how many electron(s) does each chlorine atom share with the other chlorine atom so that each has an octet? a. 1 20. In the compound ammonia, d. the Lewis structure will have one unshared pair of electrons 21. What is the name of the compound whose formula is FeSO ...
Chapter 4.1 and 4.2 - science-b
... all elements are composed of tiny indivisible particles called atoms. Dalton was wrong about the “indivisible” part, but the rest of this tenet is still fundamental to chemistry. ...
... all elements are composed of tiny indivisible particles called atoms. Dalton was wrong about the “indivisible” part, but the rest of this tenet is still fundamental to chemistry. ...
Chemical Reactions
... substance by using symbols to represent solid (s), liquid (l), gas (g) and aqueous (aq) ...
... substance by using symbols to represent solid (s), liquid (l), gas (g) and aqueous (aq) ...
Chemistry Midterm Review 2006
... 4. What kind of elements form ionic bonds? What kind of elements form covalent bonds? 5. Which of the following compounds contain ionic bonds? H2O, Na2O, CO2, CaS2, SO2, CaCO3. 6. Know the difference between a formula unit and a molecule. 7. What is the difference between a nonpolar covalent bond an ...
... 4. What kind of elements form ionic bonds? What kind of elements form covalent bonds? 5. Which of the following compounds contain ionic bonds? H2O, Na2O, CO2, CaS2, SO2, CaCO3. 6. Know the difference between a formula unit and a molecule. 7. What is the difference between a nonpolar covalent bond an ...
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.