IB Chemistry Review. Unit I. Topics 2
... C. Each magnesium atom loses two electrons and each chlorine atom gains one electron. D. Each magnesium atom gains one electron and each chlorine atom loses two electrons. 6. Which is the best description of ionic bonding? A. The electrostatic attraction between positively charged nuclei and an elec ...
... C. Each magnesium atom loses two electrons and each chlorine atom gains one electron. D. Each magnesium atom gains one electron and each chlorine atom loses two electrons. 6. Which is the best description of ionic bonding? A. The electrostatic attraction between positively charged nuclei and an elec ...
Topic 1 Review - Capital High School
... C. Each magnesium atom loses two electrons and each chlorine atom gains one electron. D. Each magnesium atom gains one electron and each chlorine atom loses two electrons. 6. Which is the best description of ionic bonding? A. The electrostatic attraction between positively charged nuclei and an elec ...
... C. Each magnesium atom loses two electrons and each chlorine atom gains one electron. D. Each magnesium atom gains one electron and each chlorine atom loses two electrons. 6. Which is the best description of ionic bonding? A. The electrostatic attraction between positively charged nuclei and an elec ...
Ch 4 Student
... • Limiting Reactant – reactant that is completely consumed and limits amount of product • Reactant in excess – reactant present in greater quantity than limiting reactant • Theoretical Yield – amount of product made based on consumption of all the limiting reactant • Actual Yield – amount of product ...
... • Limiting Reactant – reactant that is completely consumed and limits amount of product • Reactant in excess – reactant present in greater quantity than limiting reactant • Theoretical Yield – amount of product made based on consumption of all the limiting reactant • Actual Yield – amount of product ...
Reversible and irreversible reactions - Chemwiki
... In this case also some amount of gaseous hydrogen iodide will be left unreacted. This means that the products of certain reactions can be converted back to the reactants. These types of reactions are called reversible reactions. Thus, in reversible reactions the products can react with one another u ...
... In this case also some amount of gaseous hydrogen iodide will be left unreacted. This means that the products of certain reactions can be converted back to the reactants. These types of reactions are called reversible reactions. Thus, in reversible reactions the products can react with one another u ...
Exam practice answers
... The total enthalpy change is (+425 + 470 + 416 + 335) = +1646 kJ mol−1, which is the enthalpy change when four C−H bonds are broken in methane and, therefore, the enthalpy change when one C−H bond is broken is +1646/4 = 411.5 kJ mol−1. (c) ...
... The total enthalpy change is (+425 + 470 + 416 + 335) = +1646 kJ mol−1, which is the enthalpy change when four C−H bonds are broken in methane and, therefore, the enthalpy change when one C−H bond is broken is +1646/4 = 411.5 kJ mol−1. (c) ...
MID-TERM EXAM REVIEW! Unit 1 Convert the following: 1.) 2.02 x
... * 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 ...
Semester 1 Final Exam
... molecular formulas because they show the (A) bonding arrangement of each carbon atom. (B) geometric arrangement of the atoms. (C) number of atoms of each element present. (D) percentage composition of the compound. 31. How many carbons make up the “parent chain” in the following molecule? ...
... molecular formulas because they show the (A) bonding arrangement of each carbon atom. (B) geometric arrangement of the atoms. (C) number of atoms of each element present. (D) percentage composition of the compound. 31. How many carbons make up the “parent chain” in the following molecule? ...
Instructions for AP/IB 2 Chem Summer Assignment Note
... Note: Future AP/IB chemistry students are expected to learn the material in this packet before class starts in the fall. Most of this is a review of names, formulas and reactions that were learned in pre-AP/IB chemistry. Since this class is AP and IB chemistry combined, there will not be enough time ...
... Note: Future AP/IB chemistry students are expected to learn the material in this packet before class starts in the fall. Most of this is a review of names, formulas and reactions that were learned in pre-AP/IB chemistry. Since this class is AP and IB chemistry combined, there will not be enough time ...
Chemical Reactions
... 2. Find the number of atoms for each element on the left side. Compare those against the number of the atoms of the same element on the right side. 3. Determine where to place coefficients in front of formulas so that the left side has the same number of atoms as the right side for EACH element in o ...
... 2. Find the number of atoms for each element on the left side. Compare those against the number of the atoms of the same element on the right side. 3. Determine where to place coefficients in front of formulas so that the left side has the same number of atoms as the right side for EACH element in o ...
The Bio-Organometallic Chemistry of Technetium and Rhenium
... Given its central position in the periodic table, it is not surprising that the chemistry of technetium, the most widely used element in diagnostic medicine, is so diverse. Compounds of technetium exist in oxidation states from -I to +VII consisting of ligands that are as simple as hydride (H-) to m ...
... Given its central position in the periodic table, it is not surprising that the chemistry of technetium, the most widely used element in diagnostic medicine, is so diverse. Compounds of technetium exist in oxidation states from -I to +VII consisting of ligands that are as simple as hydride (H-) to m ...
Chapter 4
... Check oxidation numbers to determine what is oxidized and what is reduced. Bromine goes from +5 in BrO3- to -1 in Br-. Thus, BrO3- is being reduced. Nitrogen goes from -2 in N2H4 to +2 in NO. Thus, N2H4 is being oxidized. So, the two unbalanced half reactions are: ...
... Check oxidation numbers to determine what is oxidized and what is reduced. Bromine goes from +5 in BrO3- to -1 in Br-. Thus, BrO3- is being reduced. Nitrogen goes from -2 in N2H4 to +2 in NO. Thus, N2H4 is being oxidized. So, the two unbalanced half reactions are: ...
Dr. Baxley`s Thermodynamics Worksheet
... you would look at how many bonds are formed vs how many break) b. Using ∆G°f, I get −1226 kJ. Using ∆H°f and S°f, then ∆G° = ∆H°–T∆S°, I get –1227 kJ 6. Since formation of a bond has − ∆H° and − ∆S°, breaking of bonds has + ∆H° and + ∆S°. Putting this into the equation ∆G° = ∆H° − T∆S°, you get sign ...
... you would look at how many bonds are formed vs how many break) b. Using ∆G°f, I get −1226 kJ. Using ∆H°f and S°f, then ∆G° = ∆H°–T∆S°, I get –1227 kJ 6. Since formation of a bond has − ∆H° and − ∆S°, breaking of bonds has + ∆H° and + ∆S°. Putting this into the equation ∆G° = ∆H° − T∆S°, you get sign ...
Atoms and Periodic Table Unit Name
... 29 - There are this many known quarks? 30 - The attraction that holds atoms close to each other 32 - Group of nitrogenous organic compounds that are essential parts of living cells. 33 - Atoms are arranged on The Periodic Table of the _____________. ...
... 29 - There are this many known quarks? 30 - The attraction that holds atoms close to each other 32 - Group of nitrogenous organic compounds that are essential parts of living cells. 33 - Atoms are arranged on The Periodic Table of the _____________. ...
PHYSICAL SETTING CHEMISTRY
... A separate answer sheet for Part A and Part B–1 has been provided to you. Follow the instructions from the proctor for completing the student information on your answer sheet. Record your answers to the Part A and Part B–1 multiple-choice questions on this separate answer sheet. Record your answers ...
... A separate answer sheet for Part A and Part B–1 has been provided to you. Follow the instructions from the proctor for completing the student information on your answer sheet. Record your answers to the Part A and Part B–1 multiple-choice questions on this separate answer sheet. Record your answers ...
Exam 2 Form N - TAMU Chemistry
... b) The number of electrons ejected from a metal surface irradiated with visible light does not depend on the color of the light as long as the light is above a certain, minimum energy . c) Electrons in atoms are found in s, p, d, or f orbitals. d) After an electron (in an atom) is excited to a highe ...
... b) The number of electrons ejected from a metal surface irradiated with visible light does not depend on the color of the light as long as the light is above a certain, minimum energy . c) Electrons in atoms are found in s, p, d, or f orbitals. d) After an electron (in an atom) is excited to a highe ...
Terminology 1
... An ion is a charged species formed from a neutral atom or molecule when electrons are gained or lost as the result of a chemical change. Cation : an ion with a net positive charge Anion : an ion with a net negative charge Positive ions are called cations because they are attracted by the negative el ...
... An ion is a charged species formed from a neutral atom or molecule when electrons are gained or lost as the result of a chemical change. Cation : an ion with a net positive charge Anion : an ion with a net negative charge Positive ions are called cations because they are attracted by the negative el ...
Fall Final Review Honors
... 53. Rewrite and balance the following word equation using chemical formulas, physical states, and energy. – When solid sodium chlorate absorbs energy, it produces solid sodium chloride and oxygen gas. Predict the products and balance (54-57). Write N.R. if no reaction will occur. Include physical st ...
... 53. Rewrite and balance the following word equation using chemical formulas, physical states, and energy. – When solid sodium chlorate absorbs energy, it produces solid sodium chloride and oxygen gas. Predict the products and balance (54-57). Write N.R. if no reaction will occur. Include physical st ...
File
... 8. Acetylene gas (C2H2) and Calcium hydroxide are produced by adding water to calcium carbide (CaC 2). a) Write the balanced chemical equation. b) How many grams of acetylene are produced by adding excess water to 5.00 grams of calcium carbide? 9. Using the equation you balanced in the problem above ...
... 8. Acetylene gas (C2H2) and Calcium hydroxide are produced by adding water to calcium carbide (CaC 2). a) Write the balanced chemical equation. b) How many grams of acetylene are produced by adding excess water to 5.00 grams of calcium carbide? 9. Using the equation you balanced in the problem above ...
7th Chemistry Unit Test Study Guide Test Date: Friday, Nov. 16
... end up with in a chemical reaction and are found to the right of the arrow. _____________________ are the substances that you begin with in a chemical reaction and are found to the left of the arrow. What does the arrow mean in a chemical reaction? ...
... end up with in a chemical reaction and are found to the right of the arrow. _____________________ are the substances that you begin with in a chemical reaction and are found to the left of the arrow. What does the arrow mean in a chemical reaction? ...
Unit 4: Chemical Bonding Notes Chemical Bond—a mutual
... 1. Determine the total number of valence electrons in the atoms. 2. Arrange atoms to form a skeleton structure. If C is present, it is the central atom. Otherwise the least electronegative atom is ...
... 1. Determine the total number of valence electrons in the atoms. 2. Arrange atoms to form a skeleton structure. If C is present, it is the central atom. Otherwise the least electronegative atom is ...
In this experiment you will observe examples of the five basic types
... 1. What are some of the observable changes that are evidence that a chemical reaction has taken place? 2. How did the flaming splint behave when it was inserted into the tube with CO2 (g)? In what way was this different from the reaction of the H2(g) to the flaming splint? 3. In the reaction of magn ...
... 1. What are some of the observable changes that are evidence that a chemical reaction has taken place? 2. How did the flaming splint behave when it was inserted into the tube with CO2 (g)? In what way was this different from the reaction of the H2(g) to the flaming splint? 3. In the reaction of magn ...
Le Chatelier`s Principle Quiz Answer Key
... If the statement is true, write "true"on your answer sheet. If it is false, change the underlined word or words to make the statement true and write the corrected answer on your answer sheet. NH4Cl(s) + heat NH3(g) + HCl(g) 5. The above reaction is exothermic. 6. The production of ammonia from amm ...
... If the statement is true, write "true"on your answer sheet. If it is false, change the underlined word or words to make the statement true and write the corrected answer on your answer sheet. NH4Cl(s) + heat NH3(g) + HCl(g) 5. The above reaction is exothermic. 6. The production of ammonia from amm ...
Redox
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.