Finals Review Questions
|
|
|
- Hector Sharp
- 5 years ago
- Views:
Transcription
1 1. An example of a chemical change is (A) freezing of water. (B) burning a match. (C) boiling carbon tetrachloride. (D) dissolving alcohol in water. (E) stretching a rubber band 2. Which involves a chemical change? (A) powdering sugar (B) condensing steam (C) magnetizing an iron bar (D) separating cream from milk (E) exposing photographic film to light 3. The law of multiple proportions is based upon the idea that atoms of some elements may (A) have several isotopes. (B) exist in several physical forms. (C) have more than one atomic mass. (D) have both metallic and non metallic properties. (E) have more than one valence number. 4. Rutherford s alpha particle bombardment of gold foil helped develop our current model of the atom by (A) finding the mass of the electron. (B) showing the existence of the neutron. (C) showing that the electron carries a negative charge. (D) showing that the atom has a concentrated central charge. 5. Which set consists only of compounds? (A) Na, Ca, He (C) NaCl, CH 4, Br 2 (B) H 3 O +, Cl, I 3 (D) H 2 S, CuCl 2, KI 6. Which property would be most helpful in identifying a substance? (A) mass (C) volume (B) state (D) melting point 7. An insoluble solid has a mass of 20.0 g. It is placed in a graduated cylinder containing 40.0 ml of water. The final volume is read as 46.0 ml. What is the density of the solid? (A) g cm 3 (C) 2.30 g cm 3 (B) g cm 3 (D) 3.33 g cm 3 8. A solid, pure, orange substance was heated yielding a colorless gas and a green solid. What kind of material was heated? (A) an element (C) a mixture (B) a compound (D) a solution 9. Which unit represents l x 10 3 mol? (A) decimole (C) millimole (B) kilomole (D) micromole 10. The volume of one milliliter most nearly equals (A) 454 g (B) 1000 L (C) 1 mg (D) 1 in (E) 1 cm 3
2 11. A barometer is used to measure the (A) pressure of the air at 0 C only. (B) mass of a column of mercury. (C) temperature of the air at standard pressure. (D) density of mercury. (E) pressure of the air. 12. Which apparatus delivers ml of liquid most accurately? (A) 50 ml buret (B) 50 ml beaker (C) 50 ml test tube (D) 50 ml graduated cylinder 13. If atom A contains 18 protons and 22 neutrons, while atom B contains 20 protons and 20 neutrons, then atoms A and B are (A) isotopes. (B) both metallic. (C) both non metallic. (D) alike in number of'electrons. (E) different in number of electrons 14. The number of neutrons in an atom of the radioactive carbon isotope 14 6 C, is (A) 6 (B) 8 (C) 12 (D) 14 (E) Which particle consists of 13 protons, 14 neutrons, and 10 electrons? (A) neon atom (D) silicon atom (B) sodium atom (E) phosphide ion (C) aluminum ion 16. A hypothetical element X has three isotopes: 40 X, 41 X, and 42 X. Their abundances are 72.0%, 9.00%, and 19.0% respectively. What is the atomic mass of X? (A) 40.5 u (B) 40.8 u (C) 41.0 u (D) 41.5 u 17. A chlorine atom (Cl) differs from a chloride ion (Cl ) in that a chlorine atom (A) has a positive nucleus while the ion s nucleus is negative. (B) has a neutral nucleus while the ion s nucleus is positive. (C) contains one electron less than the ion. (D) contains one electron more than the ion. (E) contains one proton more in the nucleus 18. All positive ions differ from their corresponding atoms by having (A) larger diameters. (B) fewer electrons. (C) a charge of +1. (D) greater atomic masses. (E) stronger metallic properties 19. The correct formula for iron(iii) sulfate is (A) FeSO 4 (D) Fe 2 (SO 4 ) 3 (B) Fe(SO 4 ) 2 (E) Fe 3 (SO 4 ) 2 (C) Fe 2 SO 4
3 20. Which formula is incorrect? (A) BaHCO 3 (B) Ca(OH) 2 (C) Al 2 O 3 (D) K 2 SO 4 (E) ZnCO The compound not properly named is (A) Fe 2 O 3, iron(iii) oxide. (B) Pb 3 O 4, trilead tetraoxide. (C) CuCl 2, copper(ii) chloride. (D) Pb 3 (PO 4 ) 2, lead(iii) phosphate 22. What is the total number of oxygen atoms represented by the formula KAl(SO 4 ) 2 12H 2 O? (A) 9 (B) 16 (C) 20 (D) 48 (E) Using only these formulas, XY 2 X 2 Z QZ what formula would you expect for a compound of elements Q and Y? (A) QY (B) QY 2 (C) Q 2 Y (D) QY In the reaction 4Al + 3O 2 2Al 2 O 3 how many moles of aluminum oxide, Al 2 O 3, are produced from one mole of aluminum, Al? (A) 0.5 (B) 2 (C) 3 (D) Which expression is correctly balanced? (A) Na 2 O 2 + 2H 2 O 2NaOH + O 2 (B) 2Na 2 O 2 + 2H 2 O 4NaOH + 2O 2 (C) 4Na 2 O 2 + 3H 2 O 4NaOH + 2O 2 (D) 2Na 2 O 2 + 2H 2 O 4NaOH + O 2 (E) 3Na 2 O 2 + 2H 2 O 6NaOH + O Consider the unbalanced expression:? CH 3 CH 2 CHO(l) +? O 2 (g)? CO 2 (g) +? H 2 O(g) Which set of coefficients balances the equation? (A) 2, 8, 3, 6 (D) 1, 8, 3, 3 (B) 3, 8, 6, 6 (E) 1, 4, 3, 3 (C) 1, 4, 3, 2
4 27. Given the equation N 2 + 3H 2 2NH 3 Theoretically, the number of moles of ammonia produced from 2 mol of nitrogen is (A) 1 (B) 2 (C) 3 (D) 4 (E) One mole of substance X reacts with one mole of water and produces one mole of oxygen and two moles of hydrogen fluoride. What is the formula of substance X? X + H 2 O O 2 + 2HF (A) F 2 (B) OF 2 (C) O 2 F (D) HOF When basic copper(ii) carbonate, CuCO 3 Cu(OH) 2, is heated, it decomposes. What is the missing product in this equation? CuCO 3 Cu(OH) 2 2CuO + CO 2 +? (A) H 2 CO 3 (B) H 2 O (C) CuH 2 (D) H What is the net ionic equation for the reaction between solutions of sodium chloride, NaCl, and silver nitrate, AgNO 3? (A) Na + (aq) + NO 3 (aq) Na(s) + 1/2N 2 (g) + 3/2O 2 (g) (B) Ag + (aq) + Cl (aq) Ag(s) + 1/2Cl 2 (g) (C) Ag + (aq) + Cl (aq) Ag + (aq) + Cl (aq) (D) Ag + (aq) + Cl (aq) AgCl(s) 31. Which two ions do not participate in the reaction between solutions of silver nitrate, AgNO 3, and potassium chloride, KCl? (A) K + and Ag + (C) K + and Cl (B) K + and NO 3 (D) Ag + and Cl 32. A compound whose empirical formula is CH 2 has a molar mass of 28 g mol 1. What is the molecular formula? H 1.0 g mol 1 (A) CH 2 (B) C 2 H 4 (C) C 2 H 2 (D) CH 4
5 33. A substance with a molar mass of 92 g mol 1 consists of equal numbers of S and N atoms. What is the formula of the substance? N 14.0 g mol 1 S 32.1 g mol 1 (A) SN (B) S 2 N 2 (C) S 3 N 3 (D) S 4 N What is the mass of one mole of calcium nitrate, Ca(NO 3 ) 2? Ca 40. g mol 1 N 14. g mol 1 O 16. g mol 1 (A) 82 g (B) 102 g (C) 164 g (D) 204 g 35. What is the percentage by mass of carbon in oxalic acid, H 2 C 2 O 4? H 1.0 g mol 1 O 16.0 g mol 1 (A) 2.22% (B) 3.75% (C) 25.0% (D) 26.7% 36. How many molecules are in 11.0 g of carbon dioxide, CO 2? O 16.0 g mol 1 (A) 1.50 x (C) 4.40 x (B) 2.24 x (D) 5.60 x Calculate the mass of 12.0 x molecules of chlorine gas, Cl 2. Atomic Molar Mass Cl 35.5 g mol 1 (A) 35.5 g (B) 71.0 g (C) 142 g (D) 284 g
6 38. At STP, 4.48 L of hydrogen was prepared using the reaction: Approximately what mass of zinc was required? Zn + 2HCl ZnCl 2 + H 2 Zn 65 g mol 1 Atomic Molar Mass (A) 1.5 g (B) 2.0 g (C) 13.0 g (D) 36.5 g (E) 65.0 g 39. This potential energy diagram shows that the reaction A + B C is Energy! A + B x C Reaction Coordinate! (A) slow. (B) rapid. (D) endothermic. (E) at equilibrium. (C) exothermic. 40. Note the equation: 2Fe(s) + 3/2O 2 (g) Fe 2 O 3 (s) ΔH = 840 kj mol 1 Fe 2 O 3 If mol of iron reacts, how much heat is liberated? (A) 42.0 kj (B) 84.0 kj (D) 420 kj (E) 840 kj (C) 210 kj
7 41. The gaseous molecules that have the greatest average velocity at 150 C are represented by F 19.0 g mol 1 H 1.0 g mol 1 N 14.0 g mol 1 O 16.0 g mol 1 (A) O 2 (B) F 2 (C) H 2 (D) N 2 (E) H 2 O 42. The approximate number of molecules of hydrogen in 1.00 L of H 2 gas at STP is (A) 1.35 x (D) 2.69 x (B) 3.01 x (E) 5.38 x (C) 6.02 x A cylinder equipped with a movable piston contains 50.0 cm 3 of a gas. What is the new volume when the pressure is doubled at constant temperature? (A) 25.0 cm 3 (C) 75.0 cm 3 (B) 50.0 cm 3 (D) 100 cm 3
5. What is the name of the compound PbO? 6. What is the name of HCl(aq)?
1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole
Chemistry Final Exam Sample Items
Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons
5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]
![5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]](/thumbs/71/66177002.jpg "5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]")
1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?
8 Chemical Equations. Flames and sparks result when aluminum foil is dropped into liquid bromine.
8 Chemical Equations Flames and sparks result when aluminum foil is dropped into liquid bromine. Chapter Outline 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Types of Chemical
Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield
Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains
H Midterm Review. Page 1
Name: H Midterm Review 1. Which statement compares the masses of two subatomic particles? A) The mass of an electron is greater than the mass of a proton. B) The mass of an electron is greater than the
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is
5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons
1. Which substance can be decomposed by a chemical change? (A) beryllium (B) boron (C) methanol (D) magnesium 2. The particles in a crystalline solid are arranged (A) randomly and far apart (B) randomly
Test Booklet. Subject: SC, Grade: HS 2008 Grade High School Chemistry. Student name:
Test Booklet Subject: SC, Grade: HS 2008 Grade High School Chemistry Student name: Author: North Carolina District: North Carolina Released Tests Printed: Tuesday July 17, 2012 1 How many protons and electrons
REVIEW OF BASIC CHEMISTRY ANSWER KEY
REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F
How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?
1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams
Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.
Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the
Which of the following answers is correct and has the correct number of significant figures?
Avogadro s Number, N A = 6.022 10 23 1. [7 points] Carry out the following mathematical operation: 6.06 10 3 + 1.1 10 2 Which of the following answers is correct and has the correct number of significant
1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
(C) hydrogen chloride (D) perchloric acid REASON: (aq) tells us that it is a mixture of HCl with water. When HCl is mixed with water, it is an acid.
1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole
SCH4U Chemistry Review: Fundamentals
SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.
Silver nitrate solution is added to sodium dichromate solution
Chem. 110 50 Points Final Exam Part 1 Practice Write the chemical names or formulas for the following a H 2 SO 4 b NiNO 2 c Aluminum thiosulfate d Plumbic acetate e Ag 2 C 2 O 4 f P 2 O 5 g Cyanic acid
Unit 7: Stoichiometry Homework Packet (85 points)
Name: Period: By the end of the Unit 7, you should be able to: Chapter 12 1. Use stoichiometry to determine the amount of substance in a reaction 2. Determine the limiting reactant of a reaction 3. Determine
Part A Answer all questions in this part.
Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.
THE MOLE - PART 2. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
THE MOLE - PART 2 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which one of the following statements is a quantitative observation? a.
Name: Midterm Review Date:
Name: Midterm Review Date: 1. Which statement concerning elements is true? A) Different elements must have different numbers of isotopes. B) Different elements must have different numbers of neutrons.
Chemistry Final Review 2017
Chemistry Final Review 2017 Atomic/Molecular Structure and Periodic Trends 1. What is the atomic number trend on the periodic table? 2. On the following periodic table label metals, nonmetals, Alkali metals,
Advanced Chemistry Final Review
Advanced Chemistry Final Review 1. What are the products of complete combustion of hydrocarbons? Hydrocarbons are compounds made of carbon and oxygen. When they burn (combine with oxygen) they form carbon
Practice Multiple Choice
Practice Multiple Choice 1. A theory differs from a hypothesis in that a theory A. cannot be disproved C. always leads to the formation of a law B. represents an educated guess D. has been subjected to
Name Midterm Review Date
Name Midterm Review Date 1. In which process does a solid change directly into a vapor? A) sublimation B) deposition C) condensation D) solidification 2. What is the molecular formula of a compound that
Spring Semester Final Exam Study Guide
Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous
Red Hook Central High School. Honors CHEMISTRY. Midterm Examination. Thursday, January 25, :30 to 2:30 p.m., only. Notice...
Red Hook Central High School Honors CHEMISTRY Midterm Examination Thursday, January 25, 2018 11:30 to 2:30 p.m., only This is a test of your knowledge of chemistry. Use that knowledge to answer all questions
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
OPTIONAL PRACTICE PROBLEMS
OPTIONAL PRACTICE PROBLEMS 1 DIMENSIONAL ANALYSIS AND PROPERTIES OF MATTER (1) List the base (fundamental) SI units: (2) Fill in the following table: Object Weight, g Mass, g Piece of iron 50 g? Huge container
Student Name: Teacher: Date: District: NCGaston. Assessment: 9_12 Science Chemistry Exam 3. Description: Chemistry Mock Final Exam
Student Name: Teacher: Date: District: NCGaston Assessment: 9_12 Science Chemistry Exam 3 Description: Chemistry Mock Final Exam 2014-15 Form: 301 1. Shown below is a model of the structure of atom X.
Name: Date: 5. Which of the following formulas is not correct? A) ZnSO4 B) Ca(OH)2 C) NaS D) KF E) NH4Br. Page 1
Name: Date: 1. Which one of the following statements about atomic structure is false? A) The electrons occupy a very large volume compared to the nucleus. B) Almost all of the mass of the atom is concentrated
Chemical Reactions Unit
Name: Hour: Teacher: ROZEMA / Chemistry Chemical Reactions Unit 1 P a g e 2 P a g e 3 P a g e 4 P a g e 5 P a g e 6 P a g e Chemistry Balancing Equations Balance the following equations by inserting the
1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E
Hour Exam I Page 1 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E 2. Consider the measurements 9.74
9. The ratio of the volume of nitrogen to that of the ammonia in the reaction N2 + 3 H2 2 NH3 is 1) 1:2; 2) 1:3; 3) 3:2; 4) 2:3.
1. In a balanced chemical equation l) coefficients are equal; 2) atoms are conserved; 3) molecules are equal; 4) energy is always produced; 5) none of these. 2. Which of the following statements about
CST Review Part 2. Liquid. Gas. 2. How many protons and electrons do the following atoms have?
CST Review Part 2 1. In the phase diagram, correctly label the x-axis and the triple point write the names of all six phases transitions in the arrows provided. Liquid Pressure (ATM) Solid Gas 2. How many
UNIT 9 - STOICHIOMETRY
General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount
1. [7 points] How many significant figures should there be in the answer to the following problem?
![1. [7 points] How many significant figures should there be in the answer to the following problem?](/thumbs/89/97819589.jpg "1. [7 points] How many significant figures should there be in the answer to the following problem?")
1 of 6 10/20/2009 3:54 AM Avogadro s Number = 6.022 10 23 1. [7 points] How many significant figures should there be in the answer to the following problem? (29.0025 + 0.2)/(6.1345 36.101) (a) 1 (b) 2
NATIONAL 5 CHEMISTRY
Farr High School NATIONAL 5 CHEMISTRY Unit 1 Chemical Changes and Structure Question Booklet 1 Rates of Reaction 1. Explain how the following would affect the rate of the reaction between 1.0 g of magnesium
1. How many protons, electrons, and neutrons are in one atom of the following isotopes (6 points)?
Chemistry 11 Department of Physical Sciences Kingsborough Community College City University of New York NAME Exam 1: Chapters 1-3 50 points 1. How many protons, electrons, and neutrons are in one atom
Chemical Reactions and Equations
Chemical Reactions and Equations 5-1 5.1 What is a Chemical Reaction? A chemical reaction is a chemical change. A chemical reaction occurs when one or more substances is converted into one or more new
Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change.
Chemical Reactions I. What is a chemical reaction? Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change. A. How can you
How did JJ Thomson conclude that the mobile charged particle in the atom had a ( ) charge.
Name Veritas Class Period Chemistry: Final Exam Practice Problems The final exam will focus on material covered in the spring semester. However, note that much of the material learned early in the year
1st Semester Review Worth 10% of Exam Score
1st Semester Review 2014-2015 Worth 10% of Exam Score Name: P: 1. Which of the following is the correct electron configuration for a neutral atom of oxygen in the ground state? A) 1s 2 2p 4 B) 1s 2 2s
2) Isotopes are atoms of the same element, which have the same number of but a different number.
AP Chemistry Semester 1 Exam Review Alternate Atomic Structure 1) Fill in the table: Name Per Isotope Symbol Atomic Mass Mass # Atomic # # of protons # of neutrons # of electrons Hydrogen-1 16 16 18 35.45
Chapter 01 Quiz Chang General Chemistry
Chapter 01 Quiz Chang General Chemistry 1. A bathroom-type scale is calibrated (marked off) in tenths of a kilogram from 1 to 200 kg and you can estimate to the nearest two-hundredths of a kilogram. How
AP Chemistry Summer Review Assignment
Name: Period: Chem I Teacher/year: AP Chemistry Summer Review Assignment Due on the FIRST DAY OF SCHOOL! A. Chemical Foundations 1. The beakers shown below have different precisions. a. Label the amount
MIDTERM REVIEW. UNIT 1: Mass/Measurement
MIDTERM REVIEW UNIT 1: Mass/Measurement Practice Problems 1. Circle the word/phrase that best fits the statement: A. [ PHYSICAL OR CHEMICAL] changes are changes in which the identity of the substance does
Semester 1 Review Chemistry
Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.
Practice I: Chemistry IGCSE
Practice I: Chemistry IGCSE cristian.obiol@gmail.com 1) Explain the following processes related to changes of states of matter. -Melting:... -Vaporization:... -Freezing:... -Condensation:... -Sublimation:...
Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield
Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains
Unit 5 Chemical Reactions Notes. Introduction: Chemical substances have physical and chemical properties
Unit 5 Chemical Reactions Notes Introduction: Chemical substances have physical and chemical properties Physical Properties 2 Types of Physical Properties Extensive Physical Properties Intensive Physical
Unit Two Worksheet WS DC U2
Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed
2. What is the charge of the nucleus in an atom of oxygen-17? (1) 0 (2) 2 (3) +8 (4) +17
60 Most Missed Chemistry Regents Exams Questions 1. In the wave-mechanical model, an orbital is a region of space in an atom where there is (1) a high probability of finding an electron (2) a high probability
California Standards Test (CST) Practice
California Standards Test (CST) Practice 1. Which element has properties most like those of magnesium? (a) calcium (b) potassium (c) cesium (d) sodium 5. Which pair of atoms will share electrons when a
2. Identify each of the following samples of matter as heterogeneous or homogeneous.
EOC REVIEW #1 1. List the following in order from smallest to largest. (A) 1 dm 3 (B) 1 ml (C) 1 cl (D) 1 L (E) 1 dl 2. Convert the following. Express your answer in standard scientific notation. (A) 36
Indicators of chemical reactions
Indicators of chemical reactions Emission of light or heat Formation of a gas Formation of a precipitate Color change Emission of odor All chemical reactions: have two parts Reactants - the substances
Name: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
Regents Chemistry Practice Problems from Units 1-9 March 2018
1. Which is a pure substance? A) table salt B) bronze C) air D) soil 2. A tentative explanation of certain facts that provides the basis for further experimentation is a(n) A) observation B) hypothesis
Chemistry Term 2 Review 1) Using the diagram above, answer the following question: How many electrons are in the valence shell of this atom? A. 2 B.
Name: Date: Chemistry Term 2 Review 1) Using the diagram above, answer the following question: How many electrons are in the valence shell of this atom? A. 2 C. 6 E. 13 2) Which formula represents an ionic
Melting. Freezing. Triple Point. Sublimation. Deposition. Temperature. 2. How many protons and electrons do the following atoms have?
CST Review Part 2 1. In the phase diagram, correctly label the x-axis and the triple point write the names of all six phases transitions in the arrows provided. Melting Liquid Freezing Pressure (ATM) Solid
b. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
CHM 130: Final Exam Practice Problems
CHM 130: Final Exam Practice Problems 1. Complete the following table: Isotope Mass number # of protons # of neutrons # of electrons strontium-90 neon-19 iron-55 2. Consider Figures A-F below: A B C D
AP Chemistry. 9. Which of the following species CANNOT function as an oxidizing agent? (A) Cr 2 O 72 (B) MnO 4 (C) NO 3 (D) S (E) I
Name AP Chemistry AP Chemistry Exam Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on your scantron for each of the following. Use the following answers
Chapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
Balancing Equations Notes
. Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
Sample. Test Booklet. Subject: SC, Grade: HS MCAS 2007 HS Chemistry. - signup at to remove - Student name:
Test Booklet Subject: SC, Grade: HS Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Thursday February 14, 2013 1 Which of the following Lewis dot structures represents
Chemistry 12. Resource Exam B. Exam Booklet
Chemistry 12 Resource Exam B Exam Booklet Contents: 21 pages Examination: 2 hours 50 multiple-choice questions in the Exam Booklet Additional Time Permitted: 60 minutes Province of British Columbia PART
C. Perform the following calculations and Round into correct scientific notation.
Name Hour Honors Chemistry Final Exam Review 2018 - HERBERHOLZ *Due on the day of the exam! No photocopying or copying other classmate s review. Must be handwritten and show work for calculations. Chapter
Orchard School. New Document 1 Name: Class: Date: 129 minutes. Time: 126 marks. Marks: Comments: Page 1
New Document Name: Class: Date: Time: Marks: 29 minutes 26 marks Comments: Page Q. The ph scale is a measure of the acidity or alkalinity of a solution. (a) Solution Draw one line from each solution to
Chapter 8. Chemical Equations. Flames and sparks result when aluminum foil is dropped Into liquid bromine.
Chapter 8 Chemical Equations Flames and sparks result when aluminum foil is dropped Into liquid bromine. Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott
1. Dimensional Analysis: convert the following values a. 47,340 cm to m Unit 1: Chemistry Matters b. 40.64 km to m c. 58,700 ml to L 2. Calculate the number of significant figures a. 0.0210 b. 3.6056 c.
Physical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O
Balance the following chemical equations: (Some may already be balanced.) 1. H 2 + O 2 H 2 O 2. S 8 + O 2 SO 3 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C +
IB Chemistry Solutions Gasses and Energy
Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.
ACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
Questions for "Reaction Bingo" 1. The starting substances in a chemical reaction.
Chemical Reactions Bingo, April 2011 1 Questions for "Reaction Bingo" 1. The starting substances in a chemical reaction. 2. A single compound gets broken apart in this type of reaction. (one of the 5 types
Balancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS CHEMICAL REACTIONS Occurs when matter combines or breaks apart to produce new kinds of matter with different properties with a change in energy. EVIDENCE FOR
Set 1 Structure of the atoms & Chemical Equation Perfect Score F Matter is anything that. and has.
STRUCTURE OF THE ATOMS 1. Matter is anything that. and has. 2. The particle theory of matter state that matter is.. 3. Type of particle Example 4. Property Solid Liquid Gas Diagrammatic representation
3 rd Nine Weeks Review
3 rd Nine Weeks Review Formula Writing & Naming What is the name of the compound with the chemical formula CrCl 3? A) chromium tetrachloride B) chromium trichloride C) chromium(ii) chloride D) chromium(iii)
Chapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
IONIC CHARGES. Chemistry 51 Review
IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from
Unit 8 Chemical Reactions- Funsheets
Part A- Balancing Equations and Types of Reactions Balance AND identify the following reactions: Unit 8 Chemical Reactions- Funsheets 1) Mg + Zn(NO 3) 2 Zn Mg(NO 3) 2 2) Ba + AgNO 3 Ag + Ba(NO 3) 2 3)
Chemical Reactions: An Introduction
Chemical Reactions: An Introduction Ions in Aqueous Solution Ionic Theory of Solutions Many ionic compounds dissociate into independent ions when dissolved in water H 2O NaCl(s) Na Cl These compounds that
4. Magnesium has three natural isotopes with the following masses and natural abundances:
Exercise #1. Determination of Weighted Average Mass 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. Suppose that a bag of pennies
Year 10 Science Chemistry Examination November 2011 Part A Multiple Choice
Year 10 Science Chemistry Examination November 2011 Part A Multiple Choice Answer these questions on the multiple choice answer sheet provided 2 Isotopes have been found as variations of atoms. Which of
CHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3
CHEMISTRY 123-02 Midterm #2 October 26, 2004 The total number of points in this exam is 100. The total exam time is 50 min. Good luck! PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point
TYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
2) Solve for protons neutrons and electrons for the bromide ION.
1) Write the formulas for the following a) Calcium nitride c)lithium hydroxide b) Iron (III) sulfide d) sulfuric acid 2) Solve for protons neutrons and electrons for the bromide ION. 3) Write the electron
Chemical Equations and Chemical Reactions
Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of
Lower Sixth Chemistry. Sample Entrance Examination
Lower Sixth Chemistry Sample Entrance Examination Time allowed: 60 minutes Name: Total : 60 Marks INSTRUCTIONS : Answer all questions Answers should be written in the spaces provided Dictionaries or reference
Unit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
CHEMICAL EQUATIONS WHAT BALANCING AN EQUATION MEANS
17 CHEMICAL EQUATIONS WHAT BALANCING AN EQUATION MEANS WHAT IS A CHEMICAL EQUATION? A chemical equation is a way of representing a chemical reaction in symbolic form. For example, when hydrochloric acid
NOTE: This practice exam contains more than questions than the real final.
NOTE: This practice exam contains more than questions than the real final. 1. The wavelength of light emitted from a green laser pointer is 5.32 10 2 nm. What is the wavelength in meters? 2. What is the
Name. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
4) Please indicate whether each of the following units are intensive or extensive. a) Density Intensive Extensive. b) Temperature Intensive Extensive
EXAM ONE Nomenclature Balancing Reactions Protons, Neutrons, Electrons Natural Abundance Solubility Rules Net Ionic Reactions Atom, Mole, Gram Conversions Empirical Formulas Solution Chemistry / Molarity
Lesson (1) Mole and chemical equation
Lesson (1) Mole and chemical equation 1 When oxygen gas reacts with magnesium, magnesium oxide is formed. Such Reactions are described by balanced equations known as "chemical equations" Δ 2Mg(s) + O2(g)
Chapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
4) Convert: a) 10 m = km b) 500 g = mg c) 250 ml = L
Data Analysis 1) Define: a) Accuracy b) Precision 2) The actual density of water is 1.00 g/ml Fred Wilma Barney Trial 1 1.12 g/ml 0.88 g/ml 1.00 g/ml Trial 2 1.13 g/ml 1.07 g/ml 1.01 g/ml Trial 3 1.11
Balancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting