AP Chemistry Summer Assignment
|
|
- Jayson Wilkins
- 5 years ago
- Views:
Transcription
1 AP Chemistry Summer Assignment 1) Name this compound: Cr 3 (PO 4 ) 2 a) Chromium Diphosphate b) Trichromium Phosphate c) Chromium (II) Phosphate d) Chromium (II) Diphosphate 2) How many significant figures are there: a) 6 b) 3 c) 5 d) 2 3) The nucleus of an atom contains a) Electrons and neutrons b) Electrons and protons c) Protons and neutrons d) All three 4) What is the correct name for LiCl? a) lithium chloride b) Monolithium monochloride c) Dilithium Chloride d) Lithium dichloride 5. How many significant figures would there be for the answer to the calculation? 2.25 x (9.135 x 3.5) x (2 x 4.5) a) 1 b) 2 c) 3 d) 4 6. How much 10.0M of NaCl would you need to create a 50mL solution of 0.10M NaCl a) 5mL b) 10mL c) 2 ml d) 6mL 7. Convert 12 grams of oxygen gas (O 2 ) into moles using stoichiometry. A moles B moles C moles D moles 8. Find the answer using the right number of significant ml ml ml A B C D Round the following number to three significant grams A grams B grams C grams D grams 10. Density is expressed in a. Decantation b. Grams/mL c. Moles/Kilogram d. Cal/g*c 11. The general formula for a double replacement reaction is a. A + B à AB b. AB à A + B c. AB + C à CB + A d. AB + CD à AD + CB 12. The number has significant figures. a. 4 b. 6 c. 3 d. 7 e Equation: 4!"# $ 4!"# ' + 2# ' How many grams of # ' are produced from 138 g of!"# $? a) grams b) 40.3 grams c) 21.8 grams d) 4.8 grams
2 14. Write a chemical equation for the following circumstance: When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. a) 3,./ + 3"0, + 3"0./ b),./ ' + 2"0, + 2 "0./ c),./ + "0, + "0./ d),./ ', +./ 15. Which equation below is correctly balanced? e) # $ # ' f) "1 2 "# $ " ' # + 1 ' # g) 2.# + # ' 2.# ' h).3(#1) $ + 1./# 2.3(./# 2 ) $ + 1 ' # 16. What is the electron configuration for Iron? A: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 1 B: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5 C: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 D: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d Draw the Lewis structure of O 2. A: B: C: D: 18. What is the final volume from the dilution of 538.0mL of 2.573M H 2 SO 4 to 1.437M H 2 SO 4? A. 962mL B. 963mL C..964L D. 9.63L 19. Which ionic molecule is nonsoluble? A. NaO B. Ca(OH) 2 C. MgF 2 D. AgCl 20. What is the final volume of a gas if it is in a 5.6L sealed container with 1.48 atm at 25 o C and the pressure increased to 2.56 atm while the temperature also increases to 90 o C? A. 3.94L B L C..394L D. 1165mL 21. Which compound fully dissociates? A. HSO 4 B. HClO 2 C. HCl D. HNO Which compound has the smallest bond angle? A. CH 4 B. PCl 5 C. H 2 O D. PF What volume of 0.50 M HCl solution is needed to create 20 ml of 0.05 M HCl solution? a. 10 ml b. 5 ml c. 2 ml d. 1 ml 24. How many ml s of water are needed to satisfy the proposed situation above? a. 18 ml b. 13 ml c. 5 ml d. 2 ml 25. The following reaction is an example of what type of reaction? KBr (aq) + AgNO 3 (aq) à AgBr (s) + KNO 3 a. Single displacement b. Double displacement c. Synthesis d. Decomposition e. Combustion 26. How many moles of KNO 3 exist in 5 L of 0.2 M KNO 3 solution? a b. 1 c. 2.5 d. 10
3 27. How many moles of carbon are in 50.0g of carbon? (C s molar mass = g/mole) a b c d How many significant figures does 300 have? a. 0 b. 1 c. 2 d What is 25 C in Kelvin? a. 248 K b. 100 K c. 298 K d. 325 K 30. True or False: It is possible to have negative Kelvin. a. True b. False 31. What is the ph of a solution with a [H 3 O + ] = 5.61x10 8 M? a b c d What is the percentage of carbon in glucose? (C 6 H 12 O 6 ) a. 25% b. 40% c. 50% d. 72% 33. What is the electron configuration of nitrogen? a. 1s 2 2s 2 2p 3 b. 1s 1 2s 1 2p 3 3p 2 c. 1p 2 2p 2 2s 3 d. 1s 2 2s 2 2p What is the electron configuration of N 3? a. 1s 2 2s 2 2p 3 b. 1s 2 2s 2 2p 6 c. 1p 2 2p 2 2s 6 d. 1s 1 2s 1 2p 3 3p The number of valence electrons that an element has is based on its: A. Group number (vertical columns) B. Period (horizontal row) C. Mass 36. There are orbital types when writing electron configurations: A. 5 (S, P, D, F, G) B. 4 (S, P, D, F) C. 3 (S, P, D) 37. form when atoms gain or lose electrons: A. Ions B. Ionic compounds C. Covalent compounds 38. A 20 gram sample has a halflife of 15 years. How long does it take for half of the sample to remain? How long does it take for 5 grams to remain? A. 15 years, 25 years B. 25 years, 30 years C. 15 years, 30 years 39. An ionic compound: A. Consists of a metal + a nonmetal or a metal + a poly atomic ion B. Consists of two metals C. Consists of two nonmetals or a nonmetal + a poly atomic ion 40. A covalent compound: A. Consists of a metal + a nonmetal B. Consists of a poly atomic ion + a metal C. Consists of two nonmetals 41. Solubility refers to and the symbol for a soluble substance is : A. The ability of a substance to dissolve in water, aq B. The percentage of salt in a substance, s C. How acidic a substance is, a 42. bonds are primarily responsible for holding water molecules together in the liquid state: A. Hydrogen B. Oxygen C. Carbon 43. bonds are the strongest and closest together: A. Single B. Double C. Triple
4 44. A diatomic molecule is: A. A molecule with two atoms of the same element (N 2, O 2, F 2, Cl 2, Br 2, I 2, H 2 ) B. A molecule with two different elements of the same numerical charge (H +1 +F 1, Ca +2 +O +2, Al +3 +N 3 ) C. Not real 45. Which reaction is correctly balanced: A. 2Al Cl 2 1 à2alcl 3 B. 2Ca HBRà2CaBr 2 + 1H 2 C. 3CO + O 2 2 à2co Which of the following is an oxidation reaction? A. Ca e à Ca B. Ca à Ca e C. Ca e + Ca à Which of the following is a reduction reaction? A. Cl 2 + 2e à 2Cl B. 2Cl à Cl 2 + 2e C. 2Cl + 2e + Cl à What is the electron configuration of Al? a) 1s 2 2s 2 2p 6 3s 2 3p 6 b) 1s 2 2s 2 2p 6 3s 2 3p 1 c) 1s 2 2s 2 2p 6 3s 2 d) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d What is the molecular weight of CO 2? a g b g c g d g 50. What is the molecular weight of NaCl? a g b g c g d g 51. Which of the following is NOT Acetate? A: C 2 H 3 O 2 B: C 2 H 3 O 2 2 C: CH 3 COO D: all of the above 53. Which of the following bond angles are incorrect? a. linear 180 trigonal planar 120 tetrahedral 100 trigonal pyramidal 90 octahedral 90 b. linear 120 trigonal planar 180 tetrahedral trigonal pyramidal 120/90 octahedral 90 c. linear 180 trigonal planar 120 tetrahedral trigonal pyramidal 90/120 octahedral 90 D: linear 180 trigonal planar 120 tetrahedral 109 trigonal pyramidal 90/120 octahedral Equation: 4!"# $ 4!"# ' + 2# ' How many grams of # ' are produced from 138 g of!"# $? a grams b grams c grams d. 4.8 grams 55. Write a chemical equation for the following circumstance: When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. a. 3,./ + 3"0, + 3"0./ b.,./ ' + 2"0, + 2 "0./ c.,./ + "0, + "0./ d.,./ ', +./ 56. Which equation below is correctly balanced? a) # $ # ' b) "1 2 "# $ " ' # + 1 ' # c) 2.# + # ' 2.# ' d).3(#1) $ + 1./# 2.3(./# 2 ) $ + 1 ' # 57. What is the electron configuration for Titanium? a. 17 ' 27 ' ' ' 38 ' b. 17 ' 27 ' ' ' 4: ' c. 17 ' 27 ' ' ' 3: ;< d. 17 ' 27 ' ' ' 3: ' 52. What type of bond is the longest? A: single bonds B: double bonds C: triple bonds D: all the same length
5 58. Find the molarity: 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution. a. 1 M b. 10 M c. 5 M d. 8 M 59. Calculate the percent composition of silver in AgCl. a. 75.3% b. 97.3% c. 24.7% d. 45.8% 60. Which states of matter are significantly compressible? a. Solids only b. Solids & Liquids c. Liquids & Gases d. Gases only 61. Homogeneous mixtures are also known as a. Solids b. Solutions c. Compounds d. Substances 62. Gases and Liquids share the property of a. Definite shape b. Compressibility c. Indefinite shape d. Incompressibility 63. Which element is a metal? a) Carbon b) Phosphorus c) Krypton d) Yttrium 64. Which group consists of the alkali earth metals? a. 16 b. 18 c. 2 d Which element would have atoms with the same number of outer electrons as carbon atoms? a. Silicon b. Boron c. Nitrogen d. Neon 66. Name this compound: Cr 3 (PO 4 ) 2 a. Chromium Diphosphate b. Trichromium Phosphate c. Chromium (II) Phosphate d. Chromium (II) Diphosphate 67. How many significant figures are there: a. 6 b. 3 c. 5 d The nucleus of an atom contains a. Electrons and neutrons b. Electrons and protons c. Protons and neutrons 69. What and where are the families on the periodic table? A: Alkali Metals col. 2, Alkaline Earth Metals col.1, Halogens col. 17, Noble Gases col. 18, Transition metals col. 316 B: Alkali Metals col. 2, Alkaline Earth Metals col.1, Halogens col. 17, Noble Gases col. 18, Transition metals col. 216 C: Alkali Metals col. 1, Alkaline Earth Metals col. 2, Halogens col. 17, Noble Gases col. 18, Transition metals col. 316 D: Alkali Metals col. 1, Alkaline Earth Metals col. 2, Halogens col. 17, Noble Gases col. 18, 70. Which Periodic table trend increases to the right and up? a. Electronegativity, Ionic Radii, Ionization Energy b. Metallic Ionic Radii, Ionization Energy c. Electronegativity, Ionization Energy, Nonmetallic d. Metallic, Atomic Radii, Electronegativity 71. What are the alkane prefixes for 15? a. Meth, Eth, Prop, But, Pentb. Meth, Prop, Pent, Hex, Heptc. Hex, Hept, Oct, Non, Decd. Pent, Hex, Hep, Oct, Non 72. What is the General Format of a Synthesis reaction? a. AB + CD à AD + CB b. element + element à compound c. compound à element + element d. A + BC à AC + B 73. WHAT IS THE OXIDATION STATE OF C IN CO 2? a. 4+ b. 2+ c. 2 d. 4
6 74. WHAT IS THE MOLE TO LITER RATIO? a. 1 mole = 22.2 liters b. 1 mole = 22.4 liters c. 1 mole = 24.2 liters d. 1 mole = 24.4 liters 75. What is the electron configuration of F? a) 1s 2 2s 2 2p 6 b) 1s 2 2s 2 2p 5 c) 1s 2 2s 2 2p 4 d) 1s 2 2s 2 2p What is the molecular weight of H 2 O? a g b g c g d g 77. How many Significant figures would there be for the answer to the calculation? 4.908* *2 a) 3 b) 2 c) 1 d) Equation: 4!"# $ 4!"# ' + 2# ' How many grams of # ' are produced from 138 g of!"# $? a grams b grams c grams d. 4.8 grams 79. Write a chemical equation for the following circumstance: When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. a. 3,./ + 3"0, + 3"0./ b.,./ ' + 2"0, + 2 "0./ c.,./ + "0, + "0./ d.,./ ', +./ 80. Which equation below is correctly balanced? a. # $ # ' b. "1 2 "# $ " ' # + 1 ' # c. 2.# + # ' 2.# ' d..3(#1) $ + 1./# 2.3(./# 2 ) $ + 1 ' # 81. What is the electron configuration for Titanium? a. 17 ' 27 ' ' ' 38 ' b. 17 ' 27 ' ' ' 4: ' c. 17 ' 27 ' ' ' 3: ;< d. 17 ' 27 ' ' ' 3: ' 82. Find the molarity: 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution. a. 1 M b. 10 M c. 5 M d. 8 M 83. Calculate the percent composition of silver in AgCl. a. 75.3% b. 97.3% c. 24.7% d. 45.8% 84. Which of the elements below has the highest electronegativity? a. Potassium b. Lithium c. Hydrogen d. Nitrogen 85. As you move up and to the right on the periodic table: a. Atomic radius increases and electronegativity decreases b. Atomic radius decreases and electronegativity increases c. Atomic radius increases and electronegativity increases d. Atomic radius decreases and electronegativity decreases 86. Choose ALL intermolecular forces that are in 1 ' #? a. Hydrogen bonding b. Hydrogen bonding, dipoledipole bonding c. Dispersion forces d. Hydrogen bonding, dipoledipole bonding, dispersion forces 87. What is the final volume from the dilution of 538.0mL of 2.573M H 2 SO 4 to 1.437M H 2 SO 4? A. 962mL B. 963mL C..964L D. 9.63L 88. Which ionic molecule is nonsoluble? A. NaO B. Ca(OH) 2 C. MgF 2 D. AgCl
7 89. What is the final volume of a gas if it is in a 5.6L sealed container with 1.48 atm at 25C and the pressure increased to 2.56 atm while the temperature also increases to 90C? A. 3.94L B L C..394L D. 1165mL 90. Which compound fully dissociates? A. HSO 4 B. HClO 2 C. HCl D. HNO Which compound has the smallest bond angle? A. CH 4 B. PCl 5 C. H 2 O D. PF In the ionic compound magnesium fluoride, what is the ratio of the two elements necessary so that each element obtains its octet from the transfer of electrons? a. 1 magnesium : 2 fluorine b. 3 magnesium : 1 fluorine c. 2 magnesium : 1 fluorine d. 1 magnesium : 1 fluorine 93. which is the Bronsted Base in the following equilibrium reaction? 96. What is the VESPR Electron based bond shape of this molecule? a. Trigonal Pyramidal b. Linear c. TShaped d. Square Planar 97. What is the VESPR Electron based bond angle of this molecule? a. 180 b. 120 c d What are the bond pairs in the shape above? A. CH 3 COOH CH 3 COOH + H 2 O ß> H 3 O + + CH 3 COO B. H 2 O C. H 3 O + D. CH 3 COO 94. What is the Bronsted acid in the following equilibrium reaction? HCO 3 + H 2 O ß> OH + H 2 CO 3 A. H 2 O B. H 2 CO 3 C. HCO 3 D. OH 95. What is the oxidation number of Al in Al + I 2 à AlI 3? A. 0 B. 3 C. 3 D. 2 a. 5 bonds, 1 lone pair b. 6 bonds, 0 lone pairs c. 2 bonds, 3 lone pairs d. 4 bonds, 1 lone pair 99. How much 5.0 M of KF would you need to create a 50 ml solution of 0.20 M of KF? a ml b. 20mL c..10ml d..20ml 100. What is the molecular weight of CO? a g b. 30.0g c. 16.0g d g
8 101. What is the electron configuration of an O 2 ion? a) 1s 2 2s 2 2p 4 b) 1s 2 2s 2 2p 5 c) 1s 2 2s 2 2p 3 d) 1s 2 2s 2 2p A tshaped molecule has how many bonding pairs and lone pairs of electrons, respectively? a) 4 1 b) 3 2 c) 2 2 d) What is the electron configuration of a Cl ion? a) 1s 2 2s 2 2p 6 3s 2 3p 5 b) 1s 2 2s 2 2p 6 3s 2 3p 4 c) 1s 2 2s 2 2p 6 3s 2 3p 6 d) 1s 2 2s 2 2p 6 3s What is the molarity of 100 ml of a 0.10 M NaOH solution after being diluted with 50 ml of water? a) 0.66 M b) M c) 0.15 M d) M 105. What is the empirical for a Chromium Oxide that was found to contain 52 grams of Chromium and 32 grams of Oxygen? a) CrO 2 b) Cr 2 O c) CrO 3 d) Cr 2 O What is the oxidation number of Sulfur in the compound H 2 SO 4? a) 6+ b) 6 c) 2+ d) If the concentration of H + ions is greater than the concentration of OH ions the solution is: a) Basic b) Acidic c) Neutral d) It is impossible to tell from this given information Find the answer using the right number of significant ml ml ml a b c d Round the following number to three significant grams a grams b grams c grams d grams 111. Convert grams of sulfur into moles. a moles b moles c moles d moles 112. Find the answer using the right number of significant 9.40 g g g a g b. 14g c g d g 113. Round the following number to three significant a g b. 8.77g c. 8.87g d. 9.11g grams 108. Convert 12 grams of Oxygen gas (O 2 ) into moles. a moles b moles c moles d moles
9 114. What VSPER shape is the following image representing? a. Bent b. Tetrahedral c. Trigonal Planar d. Linear 115. What VSPER shape is the following image representing? a. Tetrahedral b. Trigonal Pyramidal c. Trigonal Planar d. Bent 116. Which of the following elements could be represented in the following image? 119. What is the final volume of a gas if it is in a 5.6L sealed container with 1.48 atm at 25 o C and the pressure increased to 2.56 atm while the temperature also increases to 90 o C? A L B L C..394 L D ml 120. Which compound fully dissociates? A. HSO 4 B. HClO 2 C. HCl D. HNO Which compound has the smallest bond angle? A. CH 4 B. PCl 5 C. H 2 O D. PF In the ionic compound magnesium fluoride, what is the ratio of the two elements necessary so that each element obtains its octet from the transfer of electrons? a. 1 magnesium : 2 fluorine b. 3 magnesium : 1 fluorine c. 2 magnesium : 1 fluorine d. 1 magnesium : 1 fluorine 123. what is the oxidation number of Al in Al + I 2 > AlI 3? A. 0 B. 3 C. 3 D. 2 a. H 2 O b. NH 3 c. BCl 3 d. BeCl What is the final volume from the dilution of 538.0mL of 2.573M H 2 SO 4 to 1.437M H 2 SO 4? A. 962 ml B. 963 ml C..964 L D L 118. Which ionic molecule is nonsoluble? A. NaO B. Ca(OH) 2 C. MgF 2 D. AgCl 124. Of the following, the smallest and lightest subatomic particle is the. A. neutron B. proton C. alpha particle D. electron 125. All atoms of a given element have the same. A. number of protons B. density C. mass D. number of electrons and neutrons 126. Which atom has the largest number of neutrons? A. phosphorus30 B. calcium40 C. potassium39 D. argon40
10 127. Which atom is being oxidized in the reaction? Mg + 2HCl à MgCl 2 + H 2 a) Mg b) HCl c) MgCl 2 d) H What is the correct formula for this chemical compound? Iron (II) hydroxide a. 2FeH 2 b. Fe(OH) 2 c. Fe 2 OH 2 d. Fe 2 H What is the strongest form of radiation? a. Alpha b. Beta c. Gamma d. Delta 130. The law of constant composition applies to. a. Solids b. compounds c. heterogeneous mixtures d. solutions 131. An element cannot. a. be a pure substance b. be part of a homogeneous mixture c. be part of a heterogeneous mixture d. be separated into other substances by chemical means 132. Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gases 4. compression of oxygen gas a. 1, 3 b. 2, 3, 4 c. 1, 4 d. 1, 3, 4
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
More informationSpring 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
More informationReview Multiple Choice Questions
Chapter 2 Matter and Changes Review Multiple Choice Questions 1. The random molecular motion of a substance is greatest when the substance is a. condensed b. a liquid c. frozen d. a gas 2. After elements
More informationSophomore AP Chem Practice Problems
Due on 8/17/18 Sophomore AP Chem Practice Problems Scientific notation and significant figures Determine the number of Significant Figures in the following numbers: 00034 2431. 8900 0.0094 Convert the
More informationGas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
More informationRegents 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
More informationb. 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
More informationUnit 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
More informationTA Wednesday, 3:20 PM Each student is responsible for following directions. Read this page carefully.
Name Chemistry 111 Section FINAL EXAM Total Points = TA Wednesday, 3:20 PM 200 Directions: December 12, 2007 1. Each student is responsible for following directions. Read this page carefully. 2. Write
More informationChemistry 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
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More information5. 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
More informationFinal 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
More informationVolume of water g g? 50.0 ml ?
MID-TERM EXAM REVIEW! KEY! Unit 1 Convert the following: 1.) 2.02 x 10 15 mg = g 2.02 x 10 15 mg 1 g = 2.02 x 10 12 g 1000 mg 2.) 1.29 x 10-7 m = cm 1.29 x 10-7 m 100 cm = 1.29 x 10-5 cm 1 m 3.) 13.5 dm
More informationBonding Mrs. Pugliese. Name March 02, 2011
Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest
More informationCh. 1: Introduction to Chemistry. Ch. 2: Matter and Change
Review Sheet for Chemistry First Semester Final Refer to your class notes, worksheets, and the textbook to complete this review sheet. Study early so that you will have time to ask questions about what
More informationChem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
More informationRegents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY
Name: Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Focus Questions for the Unit: How are compounds different... from elements?... from mixtures? What role do valence
More informationPhysical 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
More informationTopics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals a
Chemistry Final Exam Review and Practice Chapters Covered ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 13, 14, 15, 16, 19, 20 Topics to Expect: Periodic Table: s, p, d, f blocks Metal,
More informationAdvanced 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
More informationAnswer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide
Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10
More information(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
More informationCP Chemistry Semester 1 Final Test Review
Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega M 10 6 D. deka da 10 1 G. milli m 10 6 B. kilo k
More informationChemistry Mid-Term Exam Review Spring 2017
Unit 1 Measurement & Math Accuracy & Precision (recognizing given lab data) Density calculations Number of SFs in a measurement, Round answers to correct number of SFs Percent Error Unit conversions in
More informationPart 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.
More informationMid-Term Review (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers?
Name Hour Mid-Term Review 2017-2018 (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers? a. 417.0 b. 0.0005 c. 500 000 d. 0.30034 e. 3.970 x 10 5 f. 200.10
More information1. 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.
More informationAn Incomplete Study Guide For The First Semester Exam
An Incomplete Study Guide For The First Semester Exam Dr Mandes 1. 2. Which term refers to the number of protons in an atom? a. atomic mass b. atomic number c. isotopic mass d. proton number A cation is
More informationChemistry Review. a) all of the b) a&b c) a,b&c d) a,b&d above
Chemistry Review 1. The elements whose symbols are P, C, and N are (a) potassium, cadmium, and nickel. (b) potassium, carbon, and nitrogen. (c) phosphorus, calcium, and neon. (d) phosphorus, carbon, and
More informationName: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW
Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More informationFinal Review Packet. When 100% correct, you will receive a
Final Review Packet When 100% correct, you will receive a 15-point bonus sticker to place on the final exam. Deadline: Wednesday, Feb. 8. NO EXCEPTIONS!!!!!! Note! The Final Exam will be worth two tests
More informationA) first electron shell D) are located in orbitals outside the nucleus A) 2-3 D) 18 A) K and Na C) a mixture C) Sb2O5
1. In a calcium atom in the ground state, the electrons that possess the least amount of energy are located in the A) first electron shell B) second electron shell C) third electron shell D) fourth electron
More informationCP Chemistry Midterm Topic List
CP Chemistry Midterm Topic List Converting SI Units (Kilo, Hecto, Deca, Base Unit, Deci, Centi, Milli) Scientific Notation Precision versus Accuracy Properties of Matter Classification of Matter (Element/Compound/Mixture)
More informationREVIEW 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
More informationUnit 1 Atomic Structure
Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:
More informationChemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
More informationGPISD Pre-AP Chemistry 1 st Semester Final Summative Assessment Blueprint
GPISD 201-2016 Pre-AP Chemistry 1 st Semester Final Summative Assessment Blueprint SE Description Number of Questions C.4A C.4D C.B C.C C.6D C.6E C.7A C.7B C.7C C.7E C.8A C.8B C.8C C.8D TOTAL: C.4(A) Differentiate
More informationFinal Exam Study Guide Honors Chemistry Semester Multiple Choice Questions
Final Exam Study Guide Honors Chemistry Semester 1 2017 60 Multiple Choice Questions Name: Students should be able to: Convert between metric units Convert between scientific notation and expanded (decimal)
More informationHonors Chemistry Semester 2 Final Exam MC Practice
Honors Chemistry Semester 2 Final Exam MC Practice Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1. What do the alkali metals all have in common?
More informationGeneral Chemistry First Semester Final Exam Study Guide 60 multiple choice questions
General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions 1. Define product. 2. Define reactant. 3. Label the products and reactants in the following chemical reactions: H 2
More informationChemistry 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,
More informationCHEMISTRY HONORS LEOCE Study Guide
BENCHMARK: N.1.1-1.2, N.1.6, N.3.1, N.3.3, N.3.4 CHEMISTRY HONORS CHEMISTRY AND SCIENTIFIC MEASUREMENT TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 1-3 ESSENTIAL QUESTION: How is measurement
More informationChemistry Final Exam Review
Chemistry Final Exam Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. All of the following are physical properties of matter EXCEPT.
More informationFunsheet 9.1 [VSEPR] Gu 2015
Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015
More informationSolid Gas Liquid Plasma
Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and
More informationPractice Examination #6 A. H :..
Practice Examination #6 Name: Date:. Which kind of bond is formed when two atoms share electrons to form a molecule? A. ionic B. metallic C. electrovalent D. covalent 2. The distance between two adjacent
More informationChemistry Mid-Term Review: (HERBERHOLZ)
Name: Hour: Chemistry Mid-Term Review: 2017-2018 (HERBERHOLZ) This review is worth 5% extra credit to your mid-term exam. It is due the day you are scheduled to take your midterm. Your work must be hand
More informationName Pd SN Date Chemistry Review Packet- Spring 2014
Name Pd SN Date Chemistry Review Packet- Spring 2014 1.1.1 Draw pictures to illustrate the differing isotopes and ions of a given element. 1.1.1 Which atomic symbol represents an isotope of sulfur with
More informationChapter 6 and 7 Practice MC
Chapter 6 and 7 Practice MC MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Ammonium fluoride is considered which of the following? 1) A) molecular
More information4. Draw a concept map showing the classifications of matter. Give an example of each.
Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.
More informationChemistry Exam Review
Chemistry Exam Review This exam review was compiled using the NC Essential Standards. You need to answer each question. You will receive multiple grades for your work. If you study everything on the exam
More information1. Which response contains all the molecules below that violate the octet rule, and no others? SF 4, SiCl 4, H 2Te, AsF 5, BeI 2
Chem 1100 Pre-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which response contains all the molecules below that violate the octet rule, and no
More informationName: Unit 1: Nature of Science
Name: Unit 1: Nature of Science 1. Using the picture above, list lab safety rules that are being ignored. 2. What are the steps to the scientific method? 3. Convert the following into scientific notation:
More informationSemester 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.
More informationPRACTICE SAT CHEMISTRY SUBJECT TEST 1
PRACTICE SAT CHEMISTRY SUBJECT TEST 1 You are about to take the first of three practice SAT Chemistry Subject Tests. After answering questions 1 23, which constitute Part A, you ll be directed to answer
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationAP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
More informationCHM 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
More informationMultiple Choice Identify the choice that best completes the statement or answers the question.
Covalent Practice CP November 2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Bromine, atomic number 35, belongs to Group 17. How many electrons does
More informationMemorize: Understand: Know how to:
NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition
More informationExample: How many significant figures are in the measured number ml? (5)
Chem 143 Final Exam Study Guide 1.) Know significant figures. Example: How many significant figures are in the measured number 0.0012030 ml? (5) 2.) Know how to use dimensional analysis. Example: A pipe
More informationPeriod: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory?
Chemistry Name: Period: Chemistry Semester 1 Final Exam Review Packet 1. What is the difference between a hypothesis and a theory? 2. Distinguish between quantitative and qualitative observations. States
More informationREVIEW of Grade 11 Chemistry
REVIEW of Grade 11 Chemistry SCH4U_08-09 NAME: Section A: Review of Rules for Significant Digits All measurements have a certain degree of associated with them. All the accurately known digits and the
More informationThe ions/polyatomic ions, solubility rules, and activity series will need to be memorized.
AP Chemistry Summer Assignment 2012 The summer assignment is designed to help you practice: - writing chemical formulas, names, and chemical equations - reaction types - predicting reaction products -
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationChemistry 1-2E Semester I Study Guide
Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound
More informationUnit 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
More information2. Which is NOT considered matter? (A) air (B) lead (C) sugar (D) sunlight. 4. Which of the following is a metalloid? (A) Se (B) Sr (C) Si (D) Sn
Midterm Review Packet ANSWER KEY 01/26/2014 Multiple Choice Question 1. Which part of an atom is positively charged? (A) proton (B) neutron (C) electron (D) shells 2. Which is NOT considered matter? (A)
More informationCHAPTERS 4 & 25: Structure of the Atom and Nuclear Chemistry 6. Complete the table: Mass (amu) charge Proton 1 +1 Neutron 1 0 Electron 0-1
Name: Date: Period: CP CHEMISTRY SPRING FINAL REVIEW SHEET NOTE: Below are concepts that we have covered in class throughout the year. Questions are organized by chapter/concept to help you study. You
More informationCHM 1045 Qualifying Exam
CHM 1045 Qualifying Exam 1. Which of the following is the basic unit of volume in the metric system? A) liter B) kilogram C) meter D) centimeter E) gram 2. Which of the following is the largest unit? A)
More informationChem 42 Final Review Sheet Mr. J. Fassler Spring 2018
Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018 These problems are given to help you review concepts you may have forgotten. Old tests, quizzes and review sheets are also important in studying. Chapter
More informationFirst Semester Final Exam Study Guide
First Semester Final Exam Study Guide Name: Chemistry 1 2 3 4 5 6 7 60 multiple choice questions Chapter 1 1. Define matter and list five examples. Chapter 2 2. Define pure substance. 3. Define element.
More informationCHM 151 Practice Final Exam
CM 151 Practice Final Exam 1. ow many significant figures are there in the result of 5.52 divided by 3.745? (a) 1 (b) 2 (c) 3 (d) 4 (e) 5 2. ow many significant figures are there in the answer when 9.021
More information1st 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
More informationScience 9 Midterm Study Guide
Science 9 Midterm Study Guide Name 1. What are the atomic mass units for protons, neutrons, and electrons? 2. What is the atomic number? 3. What is the mass number? 4. What particles are in equal numbers
More informationChemistry SOL Review Packet. beaker evaporating dish Erlenmeyer flask watch glass. volumetric flask graduated cylinder mortar & pestle crucible
Chemistry SOL Review Packet Name 1. Match the following lab equipment with its name: beaker evaporating dish Erlenmeyer flask watch glass volumetric flask graduated cylinder mortar & pestle crucible 2.
More information2. 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
More information(B) K2O potassium dioxide
PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium
More informationName: Period: AP Take Home Practice Test for Unit 0.5 Exam
Name: Period: AP Take Home Practice Test for Unit 0.5 Exam 1. Which of the following is a correctly balanced equation? a. Al 2(SO 4) 3 + 2 CaCl 2 2 CaSO 4 + 3 AlCl 3 b. Al 2(SO 4) 3 + 3 CaCl 2 3 CaSO 4
More information5. 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
More informationExam Review Questions - Multiple Choice
Exam Review Questions - Multiple Choice The following questions are for review. They are in no particular order. 1. An atom of iron 56 26Fe has... a) 26 protons, 26 electrons, 30 neutrons b) 30 protons,
More information1. 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
More informationAP Chemistry Summer Assignment
Name AP Chemistry Summer Assignment Welcome to AP chemistry! This summer assignment is intended to help you review the basic topics you learned in pre-ap chemistry that are crucial for your success in
More informationCP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega B.
Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega B. kilo D. deka E. deci G. milli H. micro C. hecto
More informationLab safety and equipment: Sig Figs and Metric Conversions. Matter. Chemistry Review
Lab safety and equipment: Chemistry Review Know: How to handle chemicals and laboratory equipment safely. Basic laboratory equipment Sig Figs and Metric Conversions Significant Figures How many significant
More informationICP Final Exam Review - Part 2
ICP Final Exam Review - Part 2 Modified True/False Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true. 1. A combustion reaction occurs
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More informationTest 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
More informationFirst Semester Final Exam Study Guide
First Semester Final Exam Study Guide Name: Chemistry 1 2 3 4 5 6 7 60 multiple choice questions Chapter 4 1. Explain the law of conservation of mass. 2. What mass of product is produced in the following
More informationChemistry 400: General Chemistry Sacramento City College HW#1: Review to Begin Chemistry 400. Review of Chapter 1
Chemistry 400: General Chemistry Sacramento City College HW#1: Review to Begin Chemistry 400 Review of Chapter 1 1) Identify a liquid. A) definite volume and definite shape B) definite volume and no definite
More informationBonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
More informationCHEM 1411 Fall 2017 SS Exam # 1 Name:
CHEM 1411 Fall 2017 SS Exam # 1 Name: 1. What is the physical state in which matter has no specific shape but does have a specific volume? A) gas B) solid C) liquid D) salts E) ice 2. A combination of
More informationAP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga
Name AP Chemistry Take Home Quiz Due Thursday, 1/9/2014 Bubble the correct answer on your scantron for each of the following. 1. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the
More informationChemistry 51 Chapter 5 OCTET RULE & IONS
OCTET RULE & IONS Most elements, except noble gases, combine to form compounds. Compounds are the result of the formation of chemical bonds between two or more different elements. In the formation of a
More informationChapter 2. The Components of Matter
Chapter 2. The Components of Matter 1 The Periodic Table (Section 2.6) 13 Al 26.981 Main Idea: 1. Groups: Old numbering system: New IUPAC numbering system: 2. Periods: 3. Know the names and properties
More informationChapter 1 Introduction to Chemistry 1. What is chemistry?
FIRST SEMESTER EXAM REVIEW Chapter 1 Introduction to Chemistry 1. What is chemistry? 2. Identify the independent and dependent variables using the graph above. IV: DV: 3. Write a hypothesis for this experiment.
More informationSCH4U 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.
More informationChemical Reactions Chapter 12 Study Guide (Unit 9)
Name: Hr: Understand and be able to explain all of the key concepts. Define and understand all of the survival words Memorize the names and symbols for these elements: (Ag, Al, Ar, As, Au, B, Ba, Be, Br,
More information