(p. 522)
... 3. Disulfide bridges. These form between the side chains of two cysteine residues, and may hold distant parts of the chain close together. 4. Salt links. These form between oppositely-charged side chains, the charges being due to the COO¯ and -NH3+ groups. 5. Dispersion forces. Nonpolar side chains ...
... 3. Disulfide bridges. These form between the side chains of two cysteine residues, and may hold distant parts of the chain close together. 4. Salt links. These form between oppositely-charged side chains, the charges being due to the COO¯ and -NH3+ groups. 5. Dispersion forces. Nonpolar side chains ...
S3 Chemistry - eduBuzz.org
... State the location, charge and mass of each sub atomic particle Calculate the number of protons, neutrons and electrons in an atom Identify whether a species has an equal or unequal number of protons and electrons and use this to state whether it is an atom or ion. State the charge of an ion ...
... State the location, charge and mass of each sub atomic particle Calculate the number of protons, neutrons and electrons in an atom Identify whether a species has an equal or unequal number of protons and electrons and use this to state whether it is an atom or ion. State the charge of an ion ...
File
... (aq) aqueous solution (the substance is dissolved in water; example: NaCl(aq) is salt water) heat added to reactants (triangle appears above arrow) ...
... (aq) aqueous solution (the substance is dissolved in water; example: NaCl(aq) is salt water) heat added to reactants (triangle appears above arrow) ...
classification of chemical reactions
... Chemical change change in matter that produces new substances Example: rusting of iron burning of wood Physical change a change that does not produce a new substance a change in appearance or state Example: chopping wood ...
... Chemical change change in matter that produces new substances Example: rusting of iron burning of wood Physical change a change that does not produce a new substance a change in appearance or state Example: chopping wood ...
Stoichiometry - WordPress.com
... • It is rare that we will have the exact amount of each reactant for a reaction. • One or more reactants are in excess – ie there is more than what is needed. • The reactant that is completely used up is said to be the limiting reactant. • It is the limiting reactant that must be used in stoichiomet ...
... • It is rare that we will have the exact amount of each reactant for a reaction. • One or more reactants are in excess – ie there is more than what is needed. • The reactant that is completely used up is said to be the limiting reactant. • It is the limiting reactant that must be used in stoichiomet ...
Atomic Masses
... The relative numbers of reactants and products in a reaction are indicated by the coefficients in the balanced equation Writing and Balancing the Equation for a Chemical Reaction • Determine what reaction is occurring. What are the reactants, the products and the physical states involved? • Write th ...
... The relative numbers of reactants and products in a reaction are indicated by the coefficients in the balanced equation Writing and Balancing the Equation for a Chemical Reaction • Determine what reaction is occurring. What are the reactants, the products and the physical states involved? • Write th ...
File
... _____ 14. The activity series of metals can be used to predict products in double-replacement reactions. _____ 15. Carbon dioxide and water are the products of the combustion of hexane (C6H14). _____ 16. A nonmetal can replace another nonmetal from a compound in a single-replacement reaction. ...
... _____ 14. The activity series of metals can be used to predict products in double-replacement reactions. _____ 15. Carbon dioxide and water are the products of the combustion of hexane (C6H14). _____ 16. A nonmetal can replace another nonmetal from a compound in a single-replacement reaction. ...
CHAPTER 8
... temperature and pressure on solubility, Henry’s Law, Raoult’s law, vapor pressure curves, freezing-point depression/boiling-point elevation, osmotic pressure. 4. Chemical kinetics: rate of reactions, rates of consumption and formation, reaction orders, rate law constants, first-, second- and zero-or ...
... temperature and pressure on solubility, Henry’s Law, Raoult’s law, vapor pressure curves, freezing-point depression/boiling-point elevation, osmotic pressure. 4. Chemical kinetics: rate of reactions, rates of consumption and formation, reaction orders, rate law constants, first-, second- and zero-or ...
KEY Final Exam Review - Iowa State University
... a. What is the rate law for the reaction? k[BF3][NH3] seen by exp 1&2;4&5 b. What is the overall order of the reaction? 2 c. Calculate the Rate constant with proper units. Using exp 1 k=(0.2130)M/s/(0.250M)(0.250M)=3.41M-1s-1 could use any of the five to calculate this. kave=3.408M-1s-1 d. What is t ...
... a. What is the rate law for the reaction? k[BF3][NH3] seen by exp 1&2;4&5 b. What is the overall order of the reaction? 2 c. Calculate the Rate constant with proper units. Using exp 1 k=(0.2130)M/s/(0.250M)(0.250M)=3.41M-1s-1 could use any of the five to calculate this. kave=3.408M-1s-1 d. What is t ...
1 Chemical Reactions: Chemistry Word Equations • Write the names
... 2. Write the _______________________ equation. (Reactants on left, products on right, yield sign in between. If two or more reactants/products are involved, separate their formulas with plus signs. 3. Determine the number of ________________ of each element in the reactants and products. (Count poly ...
... 2. Write the _______________________ equation. (Reactants on left, products on right, yield sign in between. If two or more reactants/products are involved, separate their formulas with plus signs. 3. Determine the number of ________________ of each element in the reactants and products. (Count poly ...
CHEM_2nd_Semester_Final_R eview
... a. Al2O3 + Cl2 + C AlCl3 + CO c. P + O2 P2O5 b. C4H10 + O2 CO2 + H2O 7. What isotope is used to define one mole? 8. How many particles (atoms or molecules) are in one mole? 9. Find the molar mass for the following chemical formulas: d. ZnF2 f. NH4IO3 e. Al2(SO4)3 10. How many moles are in 4.37 ...
... a. Al2O3 + Cl2 + C AlCl3 + CO c. P + O2 P2O5 b. C4H10 + O2 CO2 + H2O 7. What isotope is used to define one mole? 8. How many particles (atoms or molecules) are in one mole? 9. Find the molar mass for the following chemical formulas: d. ZnF2 f. NH4IO3 e. Al2(SO4)3 10. How many moles are in 4.37 ...
Chemistry 2nd Semester Final Exam Review Chemical Bonds Give
... a. Al2O3 + Cl2 + C AlCl3 + CO c. P + O2 P2O5 b. C4H10 + O2 CO2 + H2O 7. What isotope is used to define one mole? 8. How many particles (atoms or molecules) are in one mole? 9. Find the molar mass for the following chemical formulas: d. ZnF2 f. NH4IO3 e. Al2(SO4)3 10. How many moles are in 4.37 ...
... a. Al2O3 + Cl2 + C AlCl3 + CO c. P + O2 P2O5 b. C4H10 + O2 CO2 + H2O 7. What isotope is used to define one mole? 8. How many particles (atoms or molecules) are in one mole? 9. Find the molar mass for the following chemical formulas: d. ZnF2 f. NH4IO3 e. Al2(SO4)3 10. How many moles are in 4.37 ...
2nd Semester Final Review
... a. Al2O3 + Cl2 + C AlCl3 + CO c. P + O2 P2O5 b. C4H10 + O2 CO2 + H2O 7. What isotope is used to define one mole? 8. How many particles (atoms or molecules) are in one mole? 9. Find the molar mass for the following chemical formulas: d. ZnF2 f. NH4IO3 e. Al2(SO4)3 10. How many moles are in 4.37 ...
... a. Al2O3 + Cl2 + C AlCl3 + CO c. P + O2 P2O5 b. C4H10 + O2 CO2 + H2O 7. What isotope is used to define one mole? 8. How many particles (atoms or molecules) are in one mole? 9. Find the molar mass for the following chemical formulas: d. ZnF2 f. NH4IO3 e. Al2(SO4)3 10. How many moles are in 4.37 ...
Le Chatelier`s Principle Quiz Answer Key
... 9. What factors alter the equilibrium position in chemical reactions? 10. Describe Le Chatelier's principle. 11. If more reactant is added to an equilibrium system, what happens to Keq (assume the temperature is not changed)? 12. How is changing the concentration of a reactant in a reaction related ...
... 9. What factors alter the equilibrium position in chemical reactions? 10. Describe Le Chatelier's principle. 11. If more reactant is added to an equilibrium system, what happens to Keq (assume the temperature is not changed)? 12. How is changing the concentration of a reactant in a reaction related ...
Rate of Reaction
... Rate of Reaction Rates of reactions are usually expressed in units of moles per liter per unit time. If we know the chemical equation for a reaction, its rate can be determined by following the change in concentration of any product or reactant that can be detected quantitatively. r = ∆ concentratio ...
... Rate of Reaction Rates of reactions are usually expressed in units of moles per liter per unit time. If we know the chemical equation for a reaction, its rate can be determined by following the change in concentration of any product or reactant that can be detected quantitatively. r = ∆ concentratio ...
General Chemistry - Review for final exam: (Make sure you bring
... 8. What is a heterogeneous mixture? 9. What are the 2 pure substances? 10. How are elements represented on the periodic table? 11. What does a chemical formula tell you about a compound? 12. Where do you find the reactants and products in a chemical equation? 13. How does the law of Conservation of ...
... 8. What is a heterogeneous mixture? 9. What are the 2 pure substances? 10. How are elements represented on the periodic table? 11. What does a chemical formula tell you about a compound? 12. Where do you find the reactants and products in a chemical equation? 13. How does the law of Conservation of ...
Catalyst Activity (in your notebook)
... each reactant and product Be sure to write the correct formula for each (crossing over for ionic compounds!) Balancing the equation when you are finished. ...
... each reactant and product Be sure to write the correct formula for each (crossing over for ionic compounds!) Balancing the equation when you are finished. ...
